Gain an understanding of terms related to basic chemistry Subject: Chemistry Date: Jan 24, 2014 Today’s Topic Intro to Chemistry Today’s Starter Question: In your own words, describe the term Chemistry Answer: The study of matter and it’s changes. Today’s Objectives: One: Gain an understanding of terms related to basic chemistry Two: Three: Receive an introduction to Chemistry Summary Notes: Next Page

Explain the formation and importance of ozone. Subject: Chemistry Date: Jan 27, 2014 Today’s Topic Intro to Chemistry Today’s Starter Question: Define substance Answer: A substance, also known as a chemical, is matter has a definite composition. Today’s Objectives: One: Explain the formation and importance of ozone. Describe the development of chlorofluorocarbons. Two: Three: Matter: anything that has mass and takes up space. Chemistry is the study of everything around us All the stuff in the universe is made from building blocks formed in the stars. Summary Notes: Next Page

Earth's atmosphere contains a layer of ozone that absorbs Chemistry Notes Continued These building blocks and everything Made from them Are called matter. Chemistry is the study of matter and the changes it undergoes. Ultraviolet light damages living organisms. Earth's atmosphere contains a layer of ozone that absorbs ultraviolet light and protects living organisms. The Exosphere: 500 km Thermosphere: between 85 km and 500 km Mesosphere: between 50 and 85 km Stratosphere: between 10 and 50 km Troposphere: from the ground up to 10 km Ozone is a substance in the atmosphere made up of oxygen. A substance, also known as a chemical, is matter has a definite composition. Summary Notes: Next Page

Chlorofluorocarbons, (CFCs) argues as coolant in refrigerators Chemistry Notes Continued Ozone is born when oxygen gas is exposed to ultraviolet radiation. And the mid-1980s, scientists detected in areas in the ozone layer over Antarctica. What do because I know zone hole? Chlorofluorocarbons, (CFCs) argues as coolant in refrigerators and propellant in aerosol cans. CFCs were considered safe because they are not toxic and don't react to other chemicals, CFCs were 1st detected in the atmosphere in the 1970s, and the concentration continued to increase through the 1990s. Was there a connection between ozone thinning and increasing CFCs in atmosphere? All of the stuff in the universe is made of a. Mixtures b. Matter c. O zone d. Mass Which of the following protects living organisms from harmful ultraviolet light? A. CFC B. Oxygen gas C. Exosphere D. Ozone Compare and contrast mass and weight Explain why chemists are interested in a submicroscopic description of matter. Summary Notes: Next Page

Identify the areas of emphasis the various branches of chemistry. Subject: Chemistry Date: Jan 28, 2014 Today’s Topic Intro to Chemistry Today’s Starter Question: Explain why chemists are interested in a submicroscopic description of matter. Answer: The structure, composition, and behavior of all matter can be described on this sub microscopic atomic level . Today’s Objectives: One: Identify the areas of emphasis the various branches of chemistry. Two: Technology: a practical application of scientific information. Three: Branches of chemistry involve the study of different kinds of matter. Matter has many different forms mass is a measurement that reflects the amount of matter. Weight is a measure of mass and the force of gravity on in object. Summary Notes: Next Page

Weight can change from place to place, but mass is constant. Chemistry Notes Continued Weight can change from place to place, but mass is constant. Much of matter and his behavior is macroscopic Meaning that it can be observed without a microscope. The structure, composition, and behavior of all matter can be described on this sub microscopic atomic level Chemistry explains events on the atomic level that causes macroscopic observations. A model is a verbal, visual, or mathematical explanation of experimental data A model is a verbal, visual, or mathematical explanation of experimental data Branches Area of emphasis Examples of emphasis Organic chemistry most carbon containing chemicals pharmaceuticals, plastics Inorganic chemistry in general, mattered at does not contain carbon minerals, Physical chemistry the behavior and changes a matter and the related energy changes reaction rates reaction mechanisms Analytical chemistry components and composition of substance food nutrients Biochemistry matter and processes of living organisms Metabolism fermentation Summary Notes: Next Page

pollution, biochemical cycles Industrial chemistry Chemistry Notes Continued Environmental chemistry matter and the environment pollution, biochemical cycles Industrial chemistry chemical processes in industry paints coatings Polymer chemistry polymers and plastics textile coating and plastic Theoretical chemistry chemical interactions any areas of emphasis Thermo chemistry It’s involved in chemical processes heat of reaction Summary Notes: Next Page

Scientists use scientific methods to systematically pose and test Subject: Chemistry Date: Jan 29, 2014 Today’s Topic Intro to Chemistry Today’s Starter Question: In your own words, describe the difference between a theory and a scientific law Answer: A theory is an explanation that has been repeatedly supported by many experiments. A scientific law is a relationship in nature that is supported by many experiments and no exceptions to these relationships are found. . Today’s Objectives: One: Gain an understanding of scientific inquiry and learn the systematic approach which is an organize method of solving a problem. Two: Three: Scientists use scientific methods to systematically pose and test solutions to questions and assess the results of the tests. The scientific method is a systematic approach used in scientific study, whether it is chemistry, physics, biology, or another science. It is an organized process used by scientists to do research, and provides methods for scientist to verify the work of others. Summary Notes: Next Page

A hypothesis is a tentative explanation for what has been observed. Chemistry Notes Continued The steps in a scientific method are repeated until a hypothesis is supported or discarded An observation is the act of gathering information. Qualitative data is obtained through observations that describe color, smell, shape or other physical characteristics that is related to the 5 senses A hypothesis is a tentative explanation for what has been observed. Quantitative data is obtained from numerical observations that describe how much, how little, how big or how fast. In experiment is a set of controlled observations that test the hypothesis. A variable is a quantity or condition that can have more than one value An independent variable is the variable you plan to change. The dependent variable is the variable of the changes in value in response to the change in the independent variable. A control is a standard for comparison in an experiment A conclusion is a judgment based on the information obtained from the experiment. Summary Notes: Next Page

Molina and Rowland's motto show how CFCs could destroy the ozone. Chemistry Notes Continued A hypothesis is never proven, only supported or discarded. A model can be used to make predictions. Molina and Rowland's motto show how CFCs could destroy the ozone. Ultraviolet radiation combines with oxygen. A theory is an explanation that has been repeatedly supported by many experiments. A theory takes a broad principle of nature that has been supported over time by repeated testing. Theory are successful if they can be used to make predictions that are true. A scientific law is a relationship in nature that is supported by many experiments and no exceptions to these relationships are found. Compare and contrast pure research, applied research, and technology Apply knowledge of laboratory safety synthetic: something that is human made and does not necessarily occur in nature. Summary Notes: Next Page

Applied research is research undertaken to solve a specific problem. Chemistry Notes Continued Some scientific investigations result into development of technology that can improve our lives and the world around us. Pure research is research to gain knowledge for the sake of knowledge itself. Applied research is research undertaken to solve a specific problem. Chance discovery occurred when scientists obtain results that are far different from what they expected You are responsible for your safety and the safety of others around you Applied research showed that CFCs and a few other chemicals react with the ozone many nations agreed in 1987 to the Montréal protocol, to phase out CFC use. From 1986 to 2000 CFCs in antarctica parts for Treo dropped from over 500 to less than 200. Scientists have learned the ozone thinning occurs over antarctica every spring. Chemists solve many real problems we face today such as: Ozone depletion Finding cures for disease Reducing the weight of cars Models are tools that scientists, including chemists use Summary Notes: Next Page

Scientific methods are systematic approaches to solving problems. Chemistry Notes Continued Macroscopic observations of matter replant the action of Atoms on a submicroscopic scale. There are several branches of chemistry including organic industry in organic chemistry physical chemistry analytical chemistry and biochemistry Scientific methods are systematic approaches to solving problems. Qualitative data describes an observation; Quantitative data use numbers. Independent variables are changed in an experiment Dependent variables change in response to the independent variable. A theory is a hypothesis that is supported by many experiments. Scientific methods can be use in pure research or in applied research. Some scientific discoveries are accidental, and some are the result of diligent research in response to a need. Laboratory safety is the responsibility of everyone in the laboratory. Many of the conveniences we enjoy today are technological applications of chemistry. Summary Notes: Next Page

A. Matter; mass B. Mass; manner C. Matter; weight Chemistry Test 1. ______ is anything that has_______ and takes up space. A. Matter; mass B. Mass; manner C. Matter; weight D. Weight; mass 2. Chemistry tries to explain_______ observations based on_________ observations. A. Macroscopic; submicroscopic B. Macroscopic; nuclear C. Atomic; submicroscopic D. Microscopic; macroscopic 3. Scientific methods are______ approaches to solving problems. A. Dependent B. Independent C. Hypothetical D. Systematic 4. What are accidental discoveries, like penicillin, called? A. Applied discoveries B. Chance discoveries C. Pure discoveries D. Newton's law 5. Quantitative data describes observations that are _____. A. Numerical B. Conditions C. Independent D. Hypothesis Summary Notes: Next Page

B. Exploratory C. Applied D. Model Chemistry Test 6. Which of the following is not an example of qualitative data? A. 1.35 kg B. Red flower C. Green car D. Orange flower 7. What kind of research is done for the sake of knowledge? A. Pure B. Exploratory C. Applied D. Model 8. Which of the following has a definite composition? A. Building block B. Variable C. Substance D. Mixture 9. What varies with change in gravitational force? A. Matter B. Weight C. Mass D. Composition 10. Which of the following would be an example of quantitative data? A. Blue socks B. Square peg C. 6 kg D. Loud noise Summary Notes: Next Page

B. Hypothetical method C. Theoretical method D. Scientific method Chemistry Test 11. Which of the following describes a systematic approach to solving problems? A. Pure research B. Hypothetical method C. Theoretical method D. Scientific method 12. Laboratory safety is the responsibility of everyone in the laboratory. A. Everyone in the Lab B. The science teacher only C. The Principal D. The students in the lab only 13 A control is a __________ for comparison in an experiment A. Independent variable B. Dependent variable C. Standard D. Response 14. Mass can change from place to place, but weight is constant. A. False B. True 15. Dependent variables change in response to the independent variable. A. False B. True Summary Notes: Next Page

B. Applied research C. Variables D. Chance discovery Chemistry Test 16. What is the discovery of nylon an example of? A. Pure research B. Applied research C. Variables D. Chance discovery 17. ________ is/are anything that has mass and takes up space. A. Solids B. Building block C. Forces D. Matter 18. Which type of variables are controlled by the scientists? A. Independent B. Dependent C. Pure D. Response 19. Weight is a measure of________ and________. A. Force; gravity B. Mass; gravity C. Matter; mass D. Gravity; motion 20. Producing heat resistant plastics is an example of what kind of research? A. Independent B. Dependent defendant C. Pure D. Applied Summary Notes: Next Page

A. Matter; mass B. Mass; manner C. Matter; weight Chemistry Test 1. ______ is anything that has_______ and takes up space. A. Matter; mass B. Mass; manner C. Matter; weight D. Weight; mass 2. Chemistry tries to explain_______ observations based on_________ observations. A. Macroscopic; submicroscopic B. Macroscopic; nuclear C. Atomic; submicroscopic D. Microscopic; macroscopic 3. Scientific methods are______ approaches to solving problems. A. Dependent B. Independent C. Hypothetical D. Systematic 4. What are accidental discoveries, like penicillin, called? A. Applied discoveries B. Chance discoveries C. Pure discoveries D. Newton's law 5. Quantitative data describes observations that are _____. A. Numerical B. Conditions C. Independent D. Hypothesis Summary Notes: Next Page

B. Exploratory C. Applied D. Model Chemistry Test 6. Which of the following is not an example of qualitative data? A. 1.35 kg B. Red flower C. Green car D. Orange flower 7. What kind of research is done for the sake of knowledge? A. Pure B. Exploratory C. Applied D. Model 8. Which of the following has a definite composition? A. Building block B. Variable C. Substance D. Mixture 9. What varies with change in gravitational force? A. Matter B. Weight C. Mass D. Composition 10. Which of the following would be an example of quantitative data? A. Blue socks B. Square peg C. 6 kg D. Loud noise Summary Notes: Next Page

B. Hypothetical method C. Theoretical method D. Scientific method Chemistry Test 11. Which of the following describes a systematic approach to solving problems? A. Pure research B. Hypothetical method C. Theoretical method D. Scientific method 12. Laboratory safety is the responsibility of everyone in the laboratory. A. Everyone in the Lab B. The science teacher only C. The Principal D. The students in the lab only 13 A control is a __________ for comparison in an experiment A. Independent variable B. Dependent variable C. Standard D. Response 14. Mass can change from place to place, but weight is constant. A. False B. True 15. Dependent variables change in response to the independent variable. A. False B. True Summary Notes: Next Page

B. Applied research C. Variables D. Chance discovery Chemistry Test 16. What is the discovery of nylon an example of? A. Pure research B. Applied research C. Variables D. Chance discovery 17. ________ is/are anything that has mass and takes up space. A. Solids B. Building block C. Forces D. Matter 18. Which type of variables are controlled by the scientists? A. Independent B. Dependent C. Pure D. Response 19. Weight is a measure of________ and________. A. Force; gravity B. Mass; gravity C. Matter; mass D. Gravity; motion 20. Producing heat resistant plastics is an example of what kind of research? A. Independent B. Dependent defendant C. Pure D. Applied Summary Notes: Next Page

Why do you think we use the SI for the standards worldwide? Subject: Chemistry Date: Jan 30, 2014 Today’s Topic SI Units Today’s Starter Question: Why do you think we use the SI for the standards worldwide? Answer: To keep all research consistent all around the world. Today’s Objectives: One: Learn SI base units. Learn prefixes used with SI units Two: Learn how to recognize and determine significant digits Three: SI Based Units. Base quantity Base Unit Symbol Length meter m Mass kilogram kg Time second s Temperature kelvin K Amount of Substance mole mol Electric current ampere A Luminous candela cd Summary Notes: Next Page

Write the symbols for the following base quantities: Length, Subject: Chemistry Date: Jan 31, 2014 Today’s Topic SI Units Today’s Starter Question: Write the symbols for the following base quantities: Length, Mass, Time, Temperature, Amount of Substance,Electric Current Luminous Intensity. Answer: m, kg, s, K, mol, A, cd Today’s Objectives: “Continued:” Learn prefixes used with SI units One: Learn how to recognize and determine significant digits Two: Three: Prefixes Used with SI Units Prefix Symbol Multiplier Scientific Notation Example femto f 0.000000000000001 10 -15 femtosecond (fs) pico p 0.000000000001 10 -12 picometer (pm) nano n 0.000000001 10 -9 nanometer (nm) micro µ 0.000001 10 -6 microgram (µg) -3 milli m 0.001 10 milliamps (mA) centi c 0.01 10 -2 centimeter (cm) deci d 0.1 10 -1 deciliter (dL) kilo k 1000 10 3 kilometer (km) mega M 1,000,000 10 6 megagram (Mg) giga G 1,000,000,000 10 9 gigameter (Gm) tera T 1,000,000,000,000 10 12 terahertz (THz)

Student input: Atom e- Nucleus Protons p+ n Neutrons e- Electrons

H O 2 Student input: Covalent Bond Molecule of Water Protons Nucleus Neutrons e- e- The 1st energy level can hold 2 electrons H O 2 The second energy level can hold 8 electrons Electrons

Explain the characteristics of the neutron, proton and electron . Chemistry Feb 4, 2014 Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Explain the characteristics of the neutron, proton and electron . Answer: Neutrons and protons are located at the center of the atom which is called the nucleus. Protons are positively charged particles (P+). Electrons are negatively charged particles (E-) located on the outside of the nucleus. Electrons constantly move around the nucleus in energy levels. Today’s Objectives: One: Diagram the particles that make up an atom. Compare covalent and ionic bonds. An element is a pure substance that cannot be broken down into other substances By physical or chemical means. Elements are made of only one type of atom. Two: The periodic table of elements is organized into horizontal rows, called periods, and vertical columns called groups. Three: Atoms of the same element that have a different number of neutrons are called isotopes. Isotopes that give off radiation are called radioactive isotopes. A compound is a pure substance formed when two or more different elements combine. Compounds are always formed from a specific combination of elements in a fixed ratio. Compounds are physically and chemically different than the elements that comprise them. Compounds cannot be broken down into simpler compounds or elements by physical means, however, they can be broken down by chemical means. Summary Notes: Next Page

H O 2 Student input: Covalent Bond Molecule of Water Protons Nucleus Neutrons e- e- H O 2 Electrons

Ionic Bond: Student input: Chapter 6 + + Sodium atom + Chlorine atom Sodium ion + Chlorine ion Na + Cl NaCl

Electron Dot Diagrams for Some Group A Elements Chemical properties, such as reactivity, depend on an element’s electron configuration: When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react. The chemical properties of an element depend on the number of valence electrons. These atoms all have two valence electron These atoms all have four valence electron These atoms all have six valence electron These atoms all have one valence electron Example These atoms all have three valence electron These atoms all have five valence electron These atoms all have Seven valence electron Electron Dot Diagrams for Some Group A Elements Group 1A 2A 3A 4A 5A 6A 7A 8A These atoms all have eight valence electron He H F C N O Li Be B Ne Na Mg Al Si P Cl Ar S K Mg Ga Ge As Kr Se Br one electron in outer most shell two electron in outer most shell three electron in outer most shell four electron in outer most shell eight electron in outer most shell five electron in outer most shell six electron in outer most shell seven electron in outer most shell

Obtain a clear understanding of determining significant digits. Subject: Chemistry Date: Feb 6, 2014 Today’s Topic Scientific Notation Today’s Starter Question: Write the following numbers using scientific notation: 0.000000001, 0.000000000000001, 15,000,000, 19,000, 0.0000001, 1,000,000,000,000 Answer: -9 -15 7 4 -7 12 10 10 1.5 X 10 1.9 X 10 10 1.0 X 10 Today’s Objectives: One: Obtain a clear understanding of determining significant digits. Two: Three: Obtain a clear understanding of scientific notation Summary Notes: Next Page

Scientific Notation 0.000000001 243,500,000,000 - 9 11 1.0 X 10 2.435 X 10 0.0000000231 0.00030007 - 4 - 8 2.31 X 10 3.0007 X 10

and 30.01 is less precise than 30.001 Scientific Notation Precision 30.0 m is less precise than 30.01 and 30.01 is less precise than 30.001 5 X 10.3 = 51.5 The answer has to be 52 Because 5 is the least precise number in the equation

Distinguish between accuracy and precision. Subject: Date: Today’s Topic Scientific Notation Today’s Starter Question: Identify the significant digits in the following numbers: 0.089, 5.3098, 78.10001, 4.21, 3.1 Answer: 2, 5, 7, 3, 2 Today’s Objectives: One: Distinguish between accuracy and precision. Two: Determine the precision of measured quantities. Three: Measurements quantify our observation. A measurement is a comparison between an unknown quantity and a standard. The degree of exactness of a measurement is called its precision. The precision of a measurement is one half the smallest division of the instrument. Summary Notes: Next Page

Distinguish between accuracy and precision. Subject: Principles of Science Date: Sept. 28, 2011 Today’s Topic Scientific Notation Today’s Starter Question: Identify the significant digits in the following numbers: 0.089, 5.3098, 78.10001, 4.21, 3.1 Answer: 2, 5, 7, 3, 2 Today’s Objectives: “Continued” One: Distinguish between accuracy and precision. Two: Determine the precision of measured quantities. Three: A measure of 67.100 g is precise to the nearest thousandth of a gram. Accuracy describes how well the results of a measurement agree with the “real” value; that is the accepted value as measured by competent experimenters A common method for checking the accuracy of an instrument is called the two point calibration. Does the instrument read 0 when it should and secondly give a correct reading when it is measuring an accepted standard Summary Notes: Next Page

In your own words, explain the difference between multiplying Subject: Date: Today’s Topic Scientific Notation Today’s Starter Question: In your own words, explain the difference between multiplying and dividing using scientific notation Answer: The main difference is the fact that you will add the exponents when multiplying and you will subtract the exponent of the divisor from the exponent of the dividend when you divide Today’s Objectives: One: Obtain an understanding of how to multiply and divide using scientific notation. Multiply the values of M and add the exponents n. Multiply the units. Two: 3 11 Example: (4 X 10 kg) (5 X 10 m) = (4 X 5) X 10 kg.m 3 + 11 Three: = 20 X 10 kg.m 14 = 2.0 X 10 kg.m 15 Divide the value of M and subtract the exponent of the divisor from the exponent of the dividend. 6 Example: 8 X 10 m 2 X 10 m 3 8 2 = X 10 m 6 – (-3) 3 - 2 -3 2 9 = 4 X 10 m Summary Notes: Next Page

Practice Multiplying and Dividing using Scientific Notation Practice Multiplying and Dividing using Scientific Notation 4 9 (6 X 10 kg) (6 X 10 m) = (6 X 6) X 10 4 + 9 Kg.m = 36 X 10 13 Kg.m = 3.6 X 10 14 Kg.m

Practice Multiplying and Dividing using Scientific Notation Practice Multiplying and Dividing using Scientific Notation 8 4 9 X 10 m 9 8 - 4 4 - 2 = X 10 m 4 2 3 X 10 m 3 4 2 = 3 X 10 m

Work the following problem: (5 X 10 kg) (3 X 10 m) Multiplying and Divding Scientific Notation Subject: Date: Today’s Topic Today’s Starter Question: Work the following problem: (5 X 10 kg) (3 X 10 m) 4 5 Answer: = (5 X 3) X 10 kg.m 4 + 5 9 = 15 X 10 kg.m = 1.5 X 10 kg.m 10 Today’s Objectives: One: Gain an understanding of how to add and subtract using the scientific notation: Two: You can not add or subtract unlike terms. Three: Practice the problems on the following pages to secure a complete understanding of how to add and subtract using scientific notation. Summary Notes: Next Page

Practice Adding and Subtracting using Scientific Notation First Period Practice Adding and Subtracting using Scientific Notation 9 8 9 9.0 X 10 kg + 7.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal one digit to the left. This causes the exponent to rise by 1 9 Now, rewrite the equation like this 0.9 X 10 kg This is the correct answer. Make sure you line the decimals up 9 7.0 X 10 kg Now, simply add the bases and leave the exponents as is 7.9 X 10 9 kg

Practice Adding and Subtracting using Scientific Notation All Periods: Practice Adding and Subtracting using Scientific Notation 8 8 6 9.0 X 10 kg - 7.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal two digits to the left. This causes the exponent to rise by 2 8 Now, rewrite the equation like this 9.0 X 10 kg This is the correct answer. Make sure you line the decimals up 8 - 0.07 X 10 kg Now, simply subtract the bases and leave the exponents as is 8.93 X 10 8 kg

Work the following problem: 5.0 X 10 kg + 3.0 X 10 kg Multiplying and Divding Scientific Notation Subject: Date: Today’s Topic Today’s Starter Question: 5 4 Work the following problem: 5.0 X 10 kg + 3.0 X 10 kg Answer: = 5.0 5 X 10 kg + 0.3 X 5 10 kg This is the correct answer 5.3 X 10 5 kg Today’s Objectives: One: Learn how to convert related SI units: Two: Standard: A standard is an exact quantity that people agree to use to compare measurements. Three: Measurement: The dimensions, capacity, or amount of something. SI: The international system of units, which is used to keep research consistent around the world. Volume: The amount of space occupied by an object is called its volume. Mass: A measurement of quantity of matter in an object. Density; Is the mass per unit volume of a material. Summary Notes: Next Page

Currently, these two terms are not alike in regard Scientific Notation Problem # 3 9 7 9 9.0 X 10 kg + 5.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal two digits to the left. This causes the exponent to rise by 2 9 Now, rewrite the equation like this 0.09 X 10 kg This is the correct answer. Make sure you line the decimals up 9 +5.00 X 10 kg Now, simply add the bases and leave the exponents as is 5.09 X 10 9 kg

Currently, these two terms are not alike in regard Scientific Notation Problem # 4 7 7 4 4.0 X 10 kg - 7.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal three digits to the left. This causes the exponent to rise by 3 7 Now, rewrite the equation like this 4.000 X 10 kg This is the correct answer. Make sure you line the decimals up 7 - 0.007 X 10 kg Now, simply subtract the bases and leave the exponents as is 3.993 X 10 7 kg

A. Atoms B. Particles C. Molecules Chemistry Test 1 Matter is composed of small particles called ________. A. Atoms B. Particles C. Molecules D. ions 2. Atoms are made up of smaller particles called _______. A. pure compounds B. Ions C. pure substances D. neutrons, protons and electrons 3. A sub atomic particle that carries a negative charge. A. proton B. electron C. neutron D. molecule 4. A sub atomic particle that is located outside the nucleus . A. electron B. charge C. proton D. neutron 5. Elements on the periodic table that have the same number of electron in the outer shell are in the same _______ A. period B. level C. group D. class

Chemistry Test 6. An isotope is an atom that has a different number of _____________. A. proton vs. electrons B. Ions vs particles C. neutrons vs. protons D. molecules vs atoms 7. A carbon atom that has 8 neutrons is called a(n) __________ . A. pure molecule B. isotope C. ion D. model 8. The atomic number tells you the number of ___________ that’s in an atom. A. Protons or electrons B. variables C. charges D. ions 9. A(n) _____ is a pure substance formed when two or more different elements combine. A. charged particle B. isotope C. neutral particle D. compound 10. Compounds can be broken down chemically. A. true B. false Summary Notes: Next Page

Change the following numbers into Scientific Notation 11. 0.000000001 12. 0.000003001 13. 243,500, 000, 000 14. 19, 000, 100 15. 0.0000563

Write the number of significant digits 16. 0.000000001 17. 0.000003001 18. 243,500, 000, 000 19. 19, 000, 100 20. 0.0000563

Solve the following problems: 8 9 21. 5.0 X 10 kg + 3.0 X 10 kg 8 4 9 X 10 m 22. 4 2 3 X 10 m 23. 7 9 9.0 X 10 kg + 5.0 X 10 kg 7 5 24. 4.0 X 10 kg - 7.0 X 10 kg

Converting SI Units A conversion factor is a ratio that is equal to one and is used to change One unit to another. For Example, There are 1,000 mL in 1 L, so 1,000 mL = 1 L. If both sides of this equation are divided by 1 L, the equation becomes: 1,000 mL = 1 1L To convert units, you multiply by the appropriate conversion factor. For Example, To convert 1.255 L to mL, multiply 1.255 L by a conversion factor. Use the conversion factor with new units (mL) in the numerator (on top), and the old units (L) in the denominator (on bottom). 1,000 mL 1.255 L X = 1,255 mL 1L Do all conversions using this concept.

Converting SI Units Convert 1,567 centimeters to millimeters. 100 mm 1,567 cm = = 156,700 mm 1 cm Convert 520 kilometers to meters. Convert 55.012 kilograms to grams. Convert 1,000,000 micrometers to centimeters.

Converting SI Units How long in centimeters is a 3,075 mm rope? Identify known values and the unknown value. Identify the known values. The rope is 3,075 mm 1m = 100 cm = 1,000 mm Identify the unknown value. How long in centimeters (cm). Solve the problem. This is the equation you need to use: 100cm ? Cm =3,075 mm X 1000 mm Cancel units and multiply: 100cm 3,075 mm X = 307.5 cm 1000 mm

Name________________ Scientific Notation Quiz Period______ (5) Convert 1,567 centimeters to millimeters. 100 mm 1,567 cm = = 156,700 mm 1 cm (6) Convert 55.012 kilograms to grams. 1000 g 55.012 kg = = 55,012 g 1 kg 1 55.012 kg X 1000 g = 55,012 g . kg = 55,012 g 1 1 kg 1 kg

An Astronomical Unit is the standard measurement for the Multiplying and Divding Scientific Notation Subject: Date: Today’s Topic Today’s Starter Question: An Astronomical Unit is the standard measurement for the distance from Earth to the Sun (AU). The distance is about 150 billion (1.50 X 10 m ) 11 Answer: Calculate what 1 AU would equal in km 1 AU = 1.50 X 10 11 m 1,000 m = 1 km 1.50 X 10 11 m. km 8 1.0 km = 1.50 X 10 km 11 1.50 X 10 m X m 1,000 m 1.0 X 10 3 Today’s Objectives: One: Correctly answer 6 problems related to scientific notation and Converting from one SI unit to another Two: Three: Summary Notes: Next Page

Moles to Particles Calculate what 1 AU would equal in km. Subject: Chemistry Date: Feb 10, 2014 Today’s Topic Measuring Matter Today’s Starter Question: Calculate what 1 AU would equal in km. Answer: The distance is about 150 billion km. Today’s Objectives: One: Explain how a mole is used to indirectly count the number of particles of matter. Two: Moles to Particles Three: 23 6.02 X 10 Conversion Factor 1 Mole Ex. Number of molecules in 3.50 mol of sucrose. 23 6.02 X 10 3.50 mol of sucrose X = 2.11 X 10 24 Molecules of Sucr 1 Mole Summary Notes: Next Page

Chemists use the mole to count atoms, molecules, ions, and formula units.: Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance. The mole is the SI base unit used to measure the amount of a Substance. 1 mole is the amount of atoms in 12 g of pure carbon-12, or 6.02 X 10 23 atoms. The number is called Avogadro”s number Summary Notes: Next Page

Conversion factors must be used. Moles to particle. 6.02 X 10 23 particles Conversion factor: 1 mol Number of molecules in 3.50 mol of sucrose 6.02 X 10 23 particles 3.50 mol sucrose X = 2.11 X 10 24 molecules 1 mol sucrose Summary Notes: Next Page

Use the inverse of Avogadro’s number as the conversion factor. Particles to moles Use the inverse of Avogadro’s number as the conversion factor. 1 mol Number of representative particles X 6.02 X 10 23 particles Number of molecules in 3.50 mol of sucrose 24 1 mol sucrose 2.11 X 10 molecules sucrose X = 3.50 mol sucrose 6.02 X 10 23 molecules Summary Notes: Next Page

1. How many moles are in 2.11 X 10 molecules of sucrose 24 1. How many moles are in 2.11 X 10 molecules of sucrose 2. How many particles are in 5 moles of CO2. 3 . What is the mass of 3 moles of C6H12oO6? 4 . What is the atomic number of carbon. 5 . What is the molar mass of 5 moles of H2O molecules. 6 . How many particles are in 5 moles of H2O molecules. Summary Notes: Next Page

How many particles are in 5 moles of CO2 6.02 X 10 Conversion Factor 1 Subject: Chemistry Date: Feb 11, 2014 Today’s Topic Measuring Matter Today’s Starter Question: How many particles are in 5 moles of CO2 23 6.02 X 10 Answer: Conversion Factor 1 Mole 23 6.02 X 10 5 mol of CO2 X = 3.01 X 10 24 Molecules of CO2 1 Mole Today’s Objectives: One: Become able to relate the mass of an atom to the mass of a mole of atoms Two: Convert between number of moles and the mass of an element. Three: Convert between number of moles and number of atoms of an element. Summary Notes: Next Page

A mole always contains the same number of particles; however, Moles of different substances have different masses. 1 mole of copper and 1 mole of carbon have different masses. Molar mass is the mass in grams of one mole of any pure substance. The molar mass of any element is numerically equivalent to its atomic mass and has the units g/mol. Mole to mass. Mass in grams number of moles X = mass 1 mole 63.546 g Cu Ex. 3.00 mol Cu X = 191g Cu 1 mole Cu 3.00 moles of copper has a mass of 191g. Summary Notes: Next Page

Convert mass to moles with the inverse molar mass conversion factor. Convert moles to atoms with Avogadro’s number as the conversion factor. Summary Notes: Next Page

Representative particle: an atom, molecule, formula unit, or ion. The molar mass of a compound can be calculated from its chemical Formula and can be used to convert from mass to moles of that Compound. Chemical formulas indicate the numbers and types of atoms Contained in one of the compound. One mole of CCl2F2 contains one mole of carbon atoms, two moles Of Cl atoms, and two moles of F atoms. The molar mass of a compound equals the molar mass of each element, multiplied by the moles of that element in the chemical Formula, added together. Summary Notes: Next Page

How many moles of NaCl are in 5.50 grams NaCl? 1 mole compound Subject: Chemistry Date: Feb 14, 2014 Today’s Topic Measuring Matter Today’s Starter Question: How many moles of NaCl are in 5.50 grams NaCl? 1 mole compound Answer: Conversion Factor grams compound 1 mol of NaCl 5.50 grams of NaCl X = 0.094 mols of NaCl 58.443 grams Today’s Objectives: One: Explain what is meant by the percent composition of a compound. Two: Determine the empirical and molecular formulas for a compound From mass percent and actual mass data. Three: Percent by mass: The ratio of the mass of each element to the total mass of the compound expressed as a percent A molecular formula of a compound is a whole-number multiple of its empirical formula. Summary Notes: Next Page

How many moles of NaCl are in 5.50 grams NaCl? 1 mole compound Subject: Chemistry Date: Feb 14, 2014 Today’s Topic Measuring Matter Today’s Starter Question: How many moles of NaCl are in 5.50 grams NaCl? 1 mole compound Answer: Conversion Factor grams compound 1 mol of NaCl 5.50 grams of NaCl X = 0.094 mols of NaCl 58.443 grams Today’s Objectives: One: Explain what is meant by the percent composition of a compound. Two: Determine the empirical and molecular formulas for a compound From mass percent and actual mass data. Three: Percent by mass: The ratio of the mass of each element to the total mass of the compound expressed as a percent A molecular formula of a compound is a whole-number multiple of its empirical formula. Summary Notes: Next Page

The molar mass of a compound demonstrates the law of conservation of mass. For elements, the conversion factor is the molar mass of the compound. The procedure is the same for compounds, except that you must first calculate the molar mass of the compound. The conversion factor is the inverse of the molar mass of the compound. 1 mole compound 5..50 g compound X = 0.0297 mol compound 185.0 g compound Summary Notes: Next Page

Convert mass to moles of compound with the inverse of molar mass. Convert moles to particles with Avogadro’s number. Summary Notes: Next Page

The percent by mass of any element in a compound can be found by Dividing the mass of the element by the mass of the compound and Multiplying by 100. Mass of element Percent by mass (element) = X 100 Mass of compound The percent by mass of each element in a compound is the percent Composition of a compound. Percent composition of a compound can also be determined from its Chemical formula. Mass of element in 1 mol of compound Percent by mass = X 100 Molar mass of compound Summary Notes: Next Page

The percent by mass of any element in a compound can be found by Dividing the mass of the element by the mass of the compound and Multiplying by 100. Mass of element Percent by mass (element) = X 100 Mass of compound The percent by mass of each element in a compound is the percent Composition of a compound. Percent composition of a compound can also be determined from its Chemical formula. Mass of element in 1 mol of compound Percent by mass = X 100 Molar mass of compound Summary Notes: Next Page

What is the percent composition of C, H and O atoms Subject: Chemistry Date: Feb 19, 2014 Today’s Topic Measuring Matter Today’s Starter Question: What is the percent composition of C, H and O atoms In one molecules of glucose, (C6 H12 O6) Answer: First, find the atomic mass for C, H, and O. C = 12g H = 1g O = 16g 6 X 12g 12 X 1g 6 X 16g = 72g = 12g = 96g = tot wt glucose 180g 72g 12g 96g X 100 = 40% C X 100 = 7% H X 100 = 53% O 180g 180g 180g Today’s Objectives: One: Determine the empirical and molecular formulas for a compound from mass percent and actual mass data. Two: Three: A molecular formula of a compound is a whole number multiple of its empirical formula Summary Notes: Next Page

The empirical formula for a compound is the smallest whole number mole ratio of the element You can calculate the empirical formula from percent by mass by Assuming you have 100.00g of the compound. Then, convert the mass of each element to moles Hematite = Fe2 O3 Magnetite = Fe3 O4 Which ore provides the greatest percent of iron per kilogram? Summary Notes: Next Page

The empirical formula may or may not be the same as the molecular formula. Molecular formula of hydrogen peroxide = H2 O2 H O Empirical formula of hydrogen peroxide Summary Notes: Next Page

Hematite = Fe2 O3 Magnetite = Fe3 O4 Subject: Chemistry Date: Feb 20, 2014 Today’s Topic Measuring Matter Today’s Starter Question: Which ore provides the greatest percent of iron per kilogram? Answer: Hematite = Fe2 O3 Magnetite = Fe3 O4 Today’s Objectives: One: Determine the empirical and molecular formulas for a compound from mass percent and actual mass data. Two: The molecular formula specifies the actual number of atoms of Each element in one molecule or formula unit of the substance. Three: Molecular formula is always a whole-number multiple of the Empirical formula.. Summary Notes: Next Page

Measuring Matter Test 2-21-2014 1. Find the molecular mass of 1 mole of hydrogen peroxide H2 O2 2. Number of molecules in 4.50 mol of sucrose. 3. What is the mass of 4.00 moles of copper. 4. How many moles of NaCl are in 8.50 grams NaCl? 5. What is the percent composition of C, H and O atoms In one molecules of glucose, (C6 H12 O6) Summary Notes: Next Page

HO Write the empirical formula for peroxide H2O2? Today’s Objectives: Subject: Chemistry Date: Feb 24, 2014 Today’s Topic Measuring Matter Today’s Starter Question: Write the empirical formula for peroxide H2O2? Answer: HO Today’s Objectives: One: Explain what a hydrate is and relate the name of the hydrate to its composition. Two: Determine the formula of a hydrate from laboratory data. Three: Crystal lattice: a three-dimensional geometric arrangement of particles. Hydrates are solid ionic compounds in which water molecules are Trapped. Summary Notes: Next Page

Express percent by mass in grams Find the number of composition Mass of component element Find the number of Moles of each element Mass of each element Molar mass Ratio of moles of elements Examine the mole ratio If all are Whole numbers If not all whole numbers Multiply by the smallest factor That will produce whole numbers Empirical Formula Write the empirical formula Summary Notes: Next Page

= n Determine the integer That relates the Empirical and Molecular formulas Experimental molar mass = n Mass of empirical formula Multiply the subscripts by n (empirical formula) n Write the molecular formula Molecular formula Summary Notes: Next Page

CH2O Write the empirical formula for glucose C6H12O6 Subject: Chemistry Date: Feb 25, 2014 Today’s Topic Measuring Matter Today’s Starter Question: Write the empirical formula for glucose C6H12O6 Answer: CH2O Today’s Objectives: One: When heated, water molecules are released from a hydrate leaving an anhydrous compound. Two: To determine the formula of a hydrate, find the number of Moles of water associated with 1 mole of hydrate. Three: Summary Notes: Next Page

A hydrate is a compound that has a specific number of water molecules bound to its atoms. The number of water molecules associated with each formula unit of the compound is written following a dot. Sodium carbonate decahydrate = Na2CO3. 10H2O Summary Notes: Next Page

Calcium chloride dihydrate Tri- 3 NaC2H3O2 . 3H2O FORMULAS OF HyDRATES PREFIX MOLECULES H2O FORMULA NAME MONO- 1 (NH4)2C2O4.H2O AMMONIUM OXALATE MONOHYDRATE DI 2 CaCl2 . 2H2O Calcium chloride dihydrate Tri- 3 NaC2H3O2 . 3H2O Sodium acetate trihydrate Tetra- 4 FePO4 . 4H2O Iron(lll) phosphate tetrahydrate Penta- 5 CuSO4 . 5H2O Copper (ll) sulfate pentahydrate Hexa- 6 CoCl2 . 6H2O Cobalt (ll) chloride hexahydrate Hepta- 7 MgSO4 . 7H2O Magnesium sulfate heptahydrate Octa- 8 Ba(OH)2 . 8H2O Barium Hydroxide octahydrate Deca- 10 NaCO3 . 10H2O Sodium carbonate decahydrate Summary Notes: Next Page

Heat to drive off the water. Analyzing a hydrate: Weigh hydrate. Heat to drive off the water. Weigh the anhydrous compound. Subtract and convert the difference to moles. The ratio of moles of water to moles of anhydrous compound is the coefficient for water in the hydrate. Summary Notes: Next Page

Anhydrous forms of hydrates are often used to absorb water, Particularly during shipment of electronic and optical equipment. In chemistry labs, anhydrous forms of hydrate are used to remove Moisture from the air and keep other substances dry. Heat to drive off the water. Weigh the anhydrous compound. Subtract and convert the difference to moles. The ratio of moles of water to moles of anhydrous compound is the coefficient for water in the hydrate. Summary Notes: Next Page

Write the correct definition for volume: Subject: Date: Today’s Topic Measuring Volume Today’s Starter Question: Write the correct definition for volume: Answer: The amount of space occupied by an object is called its volume. Today’s Objectives: and Aim: Understand how to convert SI units. One: Learn how to measure volume and convert from one SI unit to another SI unit: Two: Volume: If you want to know the volume of a solid rectangle, such as a brick, you measure its length, width, and height and multiply the three numbers and their units. Three: (V = l X w X h) The volume would then be expressed in cubic centimeters, cm³ To find out how much a moving van can carry, your measurements probably would be in meters, and the volume would be expressed in cubic meters m³ because when you multiply you add your exponents. Summary Notes: Next Page

Measuring Liquid Volume In measuring a liquid volume, you are indicating the capacity of the container that holds that amount of liquid The most common units for expressing liquid volumes are liters and milliliters. A liter occupies the same volume as a cubic decimeter, dm³. A cubic decimeter is a cube that is 1 dm or 10 cm on each side: 1cm 1cm 1cm 1 cm X 1 cm X 1 cm = 1 cm³ = 1 mL 1 mL = 1 cm³ Suppose you wanted to convert a measurement in liters to cubic centimeters, you Use conversion factors to convert L to mL and then mL to cm³. 1,000 mL 1,500 cm³ 1.5 L X X = 1,500 cm³ 1 L 1 mL

Measuring Liquid Volume 1cm 1cm 1cm 1 cm X 1 cm X 1 cm = 1 cm³ = 1 mL 1 mL = 1 cm³ 1dm 1dm 1dm 1dm X 1dm X 1dm = 1dm³ 1dm³ = 1 L

Measuring Liquid Volume This is a cm³ space or volume capacity. Expressed like this: 1 cm X 1 cm X 1 cm = 1 cm³ = 1 mL 1 mL = 1 cm³ 1cm 1cm 1cm 1 mL of water from this container Will fill up this cm³ space: So this is the cm³ space And this is the mL of water 1 mL of water from this container:

Measuring Liquid Volume This is a dm³ space or volume capacity. Expressed like this: 1 dm X 1 dm X 1 dm = 1 dm³ = 1 L 1 L = 1 dm³ 1dm 1 L of water from this container Will fill up this dm³ space: 1dm 1dm So this is the dm³ space And this is the L of water 1 L of water from this container:

How many liters of water can a rectangular shaped pan that Subject: Date: Today’s Topic Measuring Volume Today’s Starter Question: How many liters of water can a rectangular shaped pan that measures 20 cm wide, 20 cm long and 20 cm high whole: Answer: 20 cm X 20 cm X 20 cm = 8000 cm³ 1 mL 8000 mL 1 L 8000 L 8000 cm³ X = X = = 8 L 1 cm³ 1 1000 mL 1000 Today’s Objectives: and Aim: Understand how to convert SI units One: Gain an understanding of how to measure matter. Two: Mass: Mass is the measurement of the quantity of matter in an object. Three: The mass and volume of an object can be used to find the density of the material the object is made of. Density: Is the mass per unit volume of a material. You find density by dividing an object’s mass by the object’s volume. For example: The density of an object having a mass of 10g and a volume of 2 cm³ is 5g / cm³ Summary Notes: Next Page

Measuring Matter Derived Units: The measurement unit for density, g / cm³ is a combination of SI units. A unit obtained by combining different SI units is called a derived unit. An SI unit multiplied by itself also is a derived unit Thus the liter, which is based on the cubic decimeter, is a derived unit. A meter cubed, expressed with an exponent -- m³ -- is a derived unit. Densities of Some Materials at 20º C Material Density g/cm³ Material Density g/cm³ Hydrogen 0.00009 Aluminum 2.7 Oxygen 0.0014 Iron 7.9 Water 1.0 Gold 19.3

Mini Lab Determine the density of different objects: One Example: Find a pencil that will fit in a 100mL graduated cylinder below the 90 mL mark. 2. Measure the mass of the pencil in grams. 3. Put 90mL of water (initial volume) into a 100mL graduated cylinder. 4. Lower the pencil, eraser first, into the cylinder. 5. Push the pencil down until it is just submerged. Hold it there and record the final volume to the nearest tenth of a milliliter (mL) Analysis: Determine the water displacement by the pencil by subtracting the initial volume from the final volume. Calculate the pencil’s density by dividing its mass by the volume of displaced. Is the density of the pencil greater than or less than the density of water? How do you Know?

Temperature Scale Formula and Equations 9/5 = 1.8, 9/4 = 2.25, 10/8 = 1.25 From To Equation Units Units Formula Fahrenheit Celsius C = (F – 32) / 1.8 Fahrenheit Kelvin K = F + 459.67) / 1.8 Fahrenheit Rankine Ra = F + 459.67 Fahrenheit Re’aumur Re = (F – 32) / 2.25 Celsius Fahrenheit F = C X 1.8 + 32 Celsius Kelvin K = C + 273.15 Celsius Rankine Ra = C + 32 + 459.67 Celsius Re’aumur Re = C X 0.8

Temperature Scale Formula and Equations 9/5 = 1.8, 9/4 = 2.25, 10/8 = 1.25 From To Equation Units Units Formula Kelvin Celsius C = K – 273.15 Kelvin Fahrenheit F = K X 1.8 - 459.67 Kelvin Rankine Ra = K X 1.8 Kelvin Re’aumur Re = (K – 273.15) X 0.8 Rankine Celsius C = (Ra – 32 – 459.67 / 1.8 Rankine Fahrenheit F = Ra – 459.67 Rankine Kelvin K = Ra / 1.8 Re’aumur Rankine Re = (Ra – 32 – 459.67) / 2.25

Temperature Scale Formula and Equations 9/5 = 1.8, 9/4 = 2.25, 10/8 = 1.25 From To Equation Re’aumur Celsius C = Re X 1.25 Re’aumur Fahrenheit F = Re X 2.25 + 32 Re’aumur Kelvin K = Re X 1.25 + 273.15 Re’aumur Rankine Ra = (Re X 2.25 + 32 + 459.67) ºC: Degrees Celsius (Centigrade), ºRe: Re’aumur, ºF: Degrees Fahrenheit, K: Kelvin, ºRa: Rankine Scale Factor ºC ºRe ºF K ºRa Boiling point of Water at 1 atmosphere 100 80 212 273.15 671.67 Freezing point of Water at 1 atmosphere 32 273.15 491.67

Convert 23.8 degrees Celsius to Fahrenheit Subject: Date: Today’s Topic Describing Motion Today’s Starter Question: Convert 23.8 degrees Celsius to Fahrenheit Answer: Use this equation: Fahrenheit = ( C X 1.8) + 32 (23.8 X 1.8) + 32 = 42.84 / + 32 74.84º Fahrenheit round up to 75º Today’s Objectives: and Aim: Understand how to convert SI units One: Learn how to distinguish between distance and displacement Review Vocabulary: Instantaneous: Occurring at a particular instant of time. Distance: Is how far an object has moved. Displacement: Is the distance and direction of an object’s change In position from the starting point. Speed: Is the distance an object travels per unit of time. Average Speed: Is the total distance traveled divided by the total time of travel Instantaneous Speed: Is the speed at a given point in time. Velocity: Includes the speed of an object and the direction of it’s motion. Summary Notes: Next Page

Convert 23.8 degrees Celsius to Fahrenheit Subject: Date: Today’s Topic Describing Motion Today’s Starter Question: Convert 23.8 degrees Celsius to Fahrenheit Answer: Use this equation: Fahrenheit = ( F – 32) / 1.8 (75 – 32) / 1.8 = 43 / 1.8 = 23.8º Celsius Today’s Objectives: and Aim: Understand how to convert SI units One: Learn how to distinguish between distance and displacement Review Vocabulary: Instantaneous: Occurring at a particular instant of time. Distance: Is how far an object has moved. Displacement: Is the distance and direction of an object’s change In position from the starting point. Speed: Is the distance an object travels per unit of time. Average Speed: Is the total distance traveled divided by the total time of travel Instantaneous Speed: Is the speed at a given point in time. Velocity: Includes the speed of an object and the direction of it’s motion. Summary Notes: Next Page

= = = Determine the speed of a car that moves 750 meters in 25 seconds Subject: Date: Today’s Topic Describing Motion Today’s Starter Question: Determine the speed of a car that moves 750 meters in 25 seconds Answer: Use this equation: speed ( in meters / seconds) = distance (in meters) 750 meters = = 30 m / s Time (in second) 25 seconds Today’s Objectives: and Aim: Understand how to convert SI units One: Explain the difference between speed and velocity. Interpret motion graphs. Summary Notes: Next Page

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript Al + O Al O 2 2 3 Aluminum Plus Oxygen Gas yields Aluminum Oxide To Balance: 2X 2X 2 Al 1.5 O + 2 Al O 2 2 3 3 1 2 2 3 4 6 2 3 Looks balanced, but you can’t have a half of an Atom. 4 6 So, multiply both sides by 2 Now, the equation is balanced

Explain the difference between a homogeneous mixture Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Explain the difference between a homogeneous mixture and a heterogeneous mixture Answer: When a mixture has a uniform composition throughout, it is called a homogeneous mixture. In a heterogeneous mixture, the components remain distinct, that is, you can tell what they are individually. Today’s Objectives: One: Describe the difference between acids and bases. Substances that release hydrogen (H+) ions in water are acids. Substances that release hydroxide (OH-) Ions in water are bases. The more hydrogen ions a substance releases in water, the more acidic the solution becomes. The more hydroxide ions a substance releases, the more basic the solution becomes Two: The pH scale is used to indicate strength of acids and bases. In other words, the concentration of H+ ions in solution. Three: . Pure water is neutral and has a pH of 7. Acidic solution have an abundance of H+ Ions and have a pH below 7. Basic solutions have more OH- than H+ and have a pH above 7. Buffers are mixtures that can react with acids or bases to keep the pH within a Particular range. In cells, buffers keep the pH in cells within the 6.5 to 7.5 pH range Summary Notes: Next Page Reactants Products

Which three elements are most abundant in the human body, Chemistry Feb. 26, 2014 Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Which three elements are most abundant in the human body, Also, list some other elements that are found in the human body Answer: Oxygen at 65%, Carbon at 18.5%, Hydrogen at 9.5%, Nitrogen at 3.3%, Calcium at 1.5%, Phosphorus 1%, and Others at 1.5%. Today’s Objectives: One: Learn how to balance a chemical equation. Two: In chemical equations, the number of atoms found in the reactants must equal the number of atoms in the product. Three: The coefficient is the number in front of the atom or molecule. Example: H O 1 oxygen 2 H O 2 2 2 oxygen 2 hydrogen . 4 hydrogen Summary Notes: Next Page Reactants Products

Explain the difference between an acid and a base. Chemistry Feb. 27, 2014 Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Explain the difference between an acid and a base. Answer: Substances that release hydrogen (H+) ions in water are acids. Substances that release hydroxide (OH-) Ions in water are bases. Today’s Objectives: One: Describe the role of carbon in living organisms. Organisms are made up of carbon-based molecules. Two: Scientists have devoted an entire branch of chemistry, called organic chemistry, to the study of organic compounds--- those compounds containing carbon. Three: Carbon compounds can be in the shape of straight chains, branched chains, And rings, together carbon compounds lead to the diversity of life on Earth. Macromolecules are large molecules that are formed by joining smaller organic molecules together, these large molecules are also called polymers. Polymers are molecules made from repeating units of identical or nearly identical Compounds, called monomers that are linked together by a series of covalent bonds. . Biological macromolecules are organized into four major categories: carbohydrates, Lipids, proteins, and nucleic acids. Summary Notes: Next Page Reactants Products

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript C H O + O C O + H O 6 12 6 2 2 2 Glucose Plus Oxygen Gas yields Carbon Dioxide Plus Water To Balance: C H O O H O 12 6 + O 6 6 C 6 6 2 2 2 + 6 6 12 2 2 1 2 1 8 12 12 12 6 6 6 12 18 18 18

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript Al + O Al O 2 2 3 Aluminum Plus Oxygen Gas yields Aluminum Oxide To Balance: 2X 2X 2 Al 1.5 O + 2 Al O 2 2 3 3 1 2 2 3 4 6 2 3 Looks balanced, but you can’t have a half of an Atom. 4 6 So, multiply both sides by 2 Now, the equation is balanced

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript C O + H C H + H O 2 2 4 2 C O 2 4 H H 2 H 2 C 4 O 2 + + 1 2 2 1 4 2 1 4 2 8 8 Now, the equation is balanced.

Balance chemical equations: Quiz 2-28-2014 Balance chemical equations: Without using your notes, balance the following chemical equations: C O + H C H + H O 2 2 4 2 Al + O Al O 2 2 3 C H O + O C O + H O 6 12 6 2 2 2

Name ______________ Period______________ Date Balance the following chemical equation to check for understanding. REMEMBER to Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. How to find the molecular and empirical formulas of a molecule. C H O 6 12 6 This is one molecule of glucose. The molecular mass of one molecule of glucose can be figured out by doing the following: One atom of carbon has a molecular mass of 12g / mol Therefore, there a 6 carbon atoms in one molecule of glucose which has a mass of 6 X 12 g / mol = 72 g of carbon One atom of hydrogen has a molecular mass of 1 g / mol Therefore, there a 12 carbon atoms in one molecule of glucose which has a mass of 6 X 1 g / mol = 12 g of hydrogen One atom of oxygen has a molecular mass of 16 g / mol Therefore, there a 6 oxygen atoms in one molecule of glucose which has a mass of 6 X 16 g / mol = 96 g of carbon

Name ______________ Period______________ Date Balance the following chemical equation to check for understanding. REMEMBER to Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. How to find the molecular and empirical formulas of a molecule. C H O 6 This is one molecule of glucose. 6 12 The empirical formula is . C H O 72 g / mol C 2 12 g /mol H 96 g / mol O To check your work 180 g /mol of glucose 180 g X .40 = 72 / 12 = 6 One mole of glucose is 40% carbon 180 g X .07 = 12 / 1 = 12 One mole of glucose is 7% Hydrogen One mole of glucose is 53% Oxygen 180 g X .53 = 95.4 / 16 = 6

Name__________________ Date_ ___ Period__________ Biochemistry Test The minimum amount of energy needed for reactants to form products in a chemical reaction is called _____________________. Colloid Activation Energy Heterogeneous Mixture Exothermic Distinct Solute Catalyst Solution Hydrogen Bond Solvent Substrate Two Homogeneous Mixture Endothermic Active Site Enzymes Polar Molecule Mixture Homogeneous B When the energy of the product is lower than the energy of the reactants, the chemical reaction is ________________. D When the energy of the product is higher than the energy of the reactants, the chemical reaction is _________________. N A ______________ is a substance that lowers the activation energy needed to start a chemical reaction. G Special protein called ____________ are the biological catalysts that speed up the rate of chemical reactions in biological processes. P K The reactants that bind to the enzyme are called _______________. O The specific location where a substrate binds on an enzyme is called the __________. Molecules that have an unequal distribution of charge are called _______________, meaning that they have oppositely charged regions. O A_____________ is a combination of two or more substances in which each substance retains its individual characteristics and properties. C In water, the electrostatic attraction is called a _______________. This bond is a weak interaction involving a hydrogen atom and a fluorine, oxygen, or nitrogen atom I When a mixture has a uniform composition throughout, it is called a _____________________. M S A solution is another name for a ________________________ mixture. L In a solution, there are __________ components, a solvent and a solute. J A __________ is a substance in which another substance is dissolved. F A __________ is a substance that is dissolved in the solvent. E In a heterogeneous mixture, the components remain ________, that is, you can tell what they are individually. H A _________ is a homogeneous mixture; a suspension is a heterogeneous mixture. A Blood is a heterogeneous mixture called a _________. 1

Which three elements are most abundant in the human body, Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Which three elements are most abundant in the human body, Also, list some other elements that are found in the human body Answer: Oxygen at 65%, Carbon at 18.5%, Hydrogen at 9.5%, Nitrogen at 3.3%, Calcium at 1.5%, Phosphorus 1%, and Others at 1.5%. Today’s Objectives: One: Learn how to balance a chemical equation. Two: In chemical equations, the number of atoms found in the reactants must equal the number of atoms in the product. Three: The coefficient is the number in front of the atom or molecule. Example: H O 1 oxygen 2 H O 2 2 2 oxygen 2 hydrogen . 4 hydrogen Summary Notes: Next Page Reactants Products

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript C H O + O C O + H O 6 12 6 2 2 2 Glucose Plus Oxygen Gas yields Carbon Dioxide Plus Water To Balance: C H O O H O 12 6 + O 6 6 C 6 6 2 2 2 + 6 6 12 2 2 1 2 1 8 12 12 12 6 6 6 12 18 18 18

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript Al + O Al O 2 2 3 Aluminum Plus Oxygen Gas yields Aluminum Oxide To Balance: 2X 2X 2 Al 1.5 O + 2 Al O 2 2 3 3 1 2 2 3 4 6 2 3 Looks balanced, but you can’t have a half of an Atom. 4 6 So, multiply both sides by 2 Now, the equation is balanced

How to balance a chemical equation: Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript C O + H C H + H O 2 2 4 2 C O 2 4 H H 2 H 2 C 4 O 2 + + 1 2 2 1 4 2 1 4 2 8 8 Now, the equation is balanced.

Name ______________ Period______________ Date Balance the following chemical equation to check for understanding. REMEMBER to Identify the parts of a chemical reaction. To Balance, use the coefficient to make the atoms equal on both sides of the arrow. Multiply the coefficient by the subscript C O + H C H + H O 2 2 4 2

Balance the following chemical equation: Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Balance the following chemical equation: CO + H CH + H O Answer: 2 2 4 2 Today’s Objectives: One: C O 2 4 H H 2 H 2 C 4 O 2 + + Two: 1 2 2 1 4 2 1 Three: 4 2 8 8 . Summary Notes: Next Page Reactants Products

Balance the following chemical equation: Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Balance the following chemical equation: CO + H CH + H O Answer: 2 2 4 2 Today’s Objectives: One: C O 2 4 H H 2 H 2 C 4 O 2 + + Two: 1 2 2 1 4 2 1 Three: 4 2 8 8 . Summary Notes: Next Page Reactants Products

Balance the following chemical equation: Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Balance the following chemical equation: CO + H CH + H O Answer: 2 2 4 2 Biological macromolecules are organized into four major categories: carbohydrates, Lipids, proteins, and nucleic acids. Today’s Objectives: One: Summarize the four major families of biological macromolecules. Compounds composed of carbon, hydrogen, and oxygen in a ratio of one oxygen And two hydrogen atoms for each carbon atom are called carbohydrates. Two: A general formula for carbohydrates is written. ( CH O ) Three: 2 n This is a monosaccharide ( a simple sugar) with the subscript n ranging from three to seven. Two monosaccharides linked together forms a disaccharide. Glucose is a monosaccharide; Sucrose and lactose are both disaccharides. Glycogen is a polysaccharide that is an energy storage form of glucose that is found in the liver and skeleton muscles. A carbohydrate called cellulose provides structural support in plants. . Chitin is a nitrogen – containing polysaccharide that is the main component in the Hard outer shell of shrimp, lobsters, and some insects, as well as the wall of some fungi. Summary Notes: Next Page Reactants Products

Explain a Binary Compound (Type I) Chemistry March 3, 2014 Naming Simple Compounds Subject: Date: Today’s Topic Today’s Starter Question: Explain a Binary Compound (Type I) Answer: Binary Ionic Compounds (Type I) contain a positive ion (cation) always written first in the formula and a negative ion (anion). Today’s Objectives: One: Learn how to name Binary Ionic Compounds. (Type I) Two: In naming binary ionic compounds, the following rules apply: Three: 1. The cation is always named first and the anion is second. A monatomic (meaning “one-atom”) cation takes its name from the name of the element. + For example, Na is called sodium in the names of compounds containing this ion. . A monatomic anion is named by taking the root of the element name and adding -ide. - Thus the Cl ion is called chloride. Summary Notes: Next Page Reactants Products

Some common monatomic cations and anions follow: Ions Present Name + - Compound Ions Present Name + - NaCl Na Cl Sodium chloride + - K I Potassium iodide KI 2+ 2- Ca S Calcium Sulfide CaS 3- + Li3 N Li N Lithium nitride + - CsBr Cs Br Cesium Bromide 2+ 2- MgO Mg O Magnesium oxide Summary Notes: Next Page

Some common monatomic cations and anions follow: Name Anion Name + - Hydride H Hydrogen H + - Fluoride Li Lithium F + - Chloride Na Sodium Cl + - Bromide K Potassium Br + - Iodide Cs Cesium I 2+ 2- Oxide Be Beryllium O 2+ 2- Sulfide Mg Magnesium S 2+ 3- Nitride Ca Calcium N 2+ 3- Phosphide Ba Barium P 3+ Al Aluminum Summary Notes: Next Page

Given the name calcium chloride, we can write the formula as CaCl2. Formulas from Names: Given the name calcium chloride, we can write the formula as CaCl2. 2+ Because we know that calcium forms only Ca ions and that, - since chloride is Cl , two of these anions will be required to give a neutral compound. In the binary ionic compounds (Type I), the metal present forms Only a single type of cation. That is, sodium forms only Na , + 2+ Calcium forms only Ca , and so on. There are many metals that form more than one type of positive ion and thus form more than one type of ionic compound with a given anion. 2+ For example, the compound FeCl2 contains Fe ions. 3+ and, the compound FeCl3 contains Fe ions. Summary Notes: Next Page

In the case of the examples on the previous slide, the charge on Formulas from Names: In the case of the examples on the previous slide, the charge on the metal ion must be specified. The systematic names for these two iron compounds are iron(II) chloride and iron (III) chloride, respectively, the roman numeral indicates the charge of the cation. Another system for naming these ionic compounds that was used for metals that form only two ions. The ion with the higher charge has a name ending in –ic, and the one with the lower charge has a name ending in-ous 3+ 3+ For example, Fe is called the ferric ion, and Fe is called the ferrous ion. Summary Notes: Next Page

Common Type (II) cations: Systematic Name Systematic Name + Fe 3+ + Fe Iron (III) Ag Silver 2+ 2+ Fe Iron (II) Zn Zinc 2+ Cu Copper (II) 2+ Cd Cadmium + Cu Copper (I) Note that mercury (I) ions always occur bound together to form Hg2 3+ Co Cobalt (III) 2+ 2+ Co Cobalt (II) ions. 4+ Sn Tin (IV) Although these are transition Metals, they form only one type of ion, and Roman numeral is not used. 2+ Sn Tin (II) 4+ Pb Lead (IV) 2+ Hg Mercury (II) 2+ Hg2 Mercury (I) Summary Notes: Next Page

Given the following names, write the formula for each compound Chemistry March 3, 2014 Naming Simple Compounds Subject: Date: Today’s Topic Today’s Starter Question: Given the following names, write the formula for each compound a. Potassium iodide c. gallium bromide Answer: b. Calcium oxide + - a. KI Contains K and I 2+ 2- b. CaO Contains Ca and O 3+ - - 3+ c. GaBr3 Contains Ga and Br (must have 3Br to balance charge of Ga ) Today’s Objectives: One: Gain an understanding of how to name type II binary compounds. Two: View practice problems on next slide. Three: Summary Notes: Next Page Reactants Products

1. Given the systematic name for each of the following compounds a. CuCl b. HgO c. Fe2O3 2. Given the following systematic names, write the formula for each compound. a. Manganese (IV) oxide b. Lead (II) chloride 1. Formula Name Comments - + a. CuCl Copper (I) chloride Because the anion Cl , the cation must be Cu (for charge balance), which requires a Roman numeral I. b. HgO Mercury (II) oxide Because the anion O 2- , the cation must be Hg 2+ [mercury (II)] c. Fe2O3 Iron (III) oxide 2- 6 - The three O , ions carry a total charge of , so 6 + two Fe 3+ ions [iron (III)] are needed to give a charge. 2. Name Formula Comments 2- 4 - a. Manganese (IV) oxide MnO2 Two O ions (total charge ) are required by the 4+ Mn Ion [manganese (IV)] b. Lead (II) chloride PbCl2 - Two Cl 2+ ions are required by the Pb ion [lead (II)] for charge balance. Summary Notes: Next Page

1. Given the systematic name for each of the following compounds: a. CoBr2 b. CaCl2 c. Al2O3 2. Given the following systematic names, write the formula for each compound. a. Chromium (III) chloride b. Gallium iodide 1. Formula Name Comments - a. CoBr2 Cobalt (II) bromide Cobalt is a transition metal ; the compound name - must have a Roman numeral. The two Br ions 2+ must be balanced by a Co ions. b. CaCl2 Calcium Chloride Calcium, an alkaline earth metal, forms only the 2+ Ca ions. A Roman numeral is not necessary. c. Al2O3 Aluminum oxide 3+ Aluminum forms only the Al Ion. A Roman numeral is not necessary. Name Formula Comments 2. a. Chromium (III) chloride CrCl3 3+ Chromium (III) indicates that Cr is present - so 3 Cl ions are needed for charge balance. b. Gallium iodide GaI3 - Gallium always 3+ ions, so 3 I ions are required for charge balance. Summary Notes: Next Page

Summary Notes: Next Page 3- 2- - + Li N N F 2- - + 2+ 3+ Na Mg Al S Cl 2+ 2+ 2+ 2+ 2+ 2+ + 2+ Cr Mn Fe Co Cu 3+ - K 3+ 3+ 3+ 3+ 3+ Zn Ca Cr Mn Fe Co Cu Ga Br 2+ + 2+ + - Rb Sr Ag Cd I 2+ 2+ + Hg2 Ba 3+ Cs Hg Common Type I cations Common Type II cations Common monatomic anions Summary Notes: Next Page

Common polyatomic Ions Name ion Name - - 2+ NCS or SCN Thiocyanate Mercury (I) Hg2 2- + Carbonate CO3 NH4 Ammonium - - HCO3 Hydrogen Carbonate NO2 Nitrite Bicarbonate is a widely used common name - NO3 Nitrate - - ClO or OCl Hypochloride - SO3 Hydrogen sulfate ClO2 Chlorite Bisulfate is a widely used common name ClO3 Chlorate - OH Hydroxide ClO4 Perchlorate - CN Cyanide C2H3O2 Acetate 3- PO4 Phosphate MnO4 Permanganate 2- 2- HPO4 Hydrogen Phosphate Cr2O7 Dichromate 2- 2+ Dihydrogen Phosphate O2 Peroxide H2PO4 2- C2O4 Oxalate 2- S2O3 Thiosulfate Summary Notes: Next Page

Gain an understanding of orbitals So far the orbitals: Gain an understanding of orbitals 1S 2S 2P 2P 2P x y z The first orbital, the 1S orbital Electrons 1 & 2 Electrons 3 & 4 The 1S orbital will hold 2 electrons Electron 5 Electron 6 Electron 7 Electron 8 y x z Next, we move to the 2S orbital The third and fourth electrons will go in the 2S orbital Next, we have three 2P orbitals which will hold 2 electrons each along an X, y, and Z axis

Electric Charge Electric Current Electric Energy Learn about Electricity Electric Charge There are two types of electric charges, protons have positive electric charge and electrons have negative electric charge. Electric Current Electric charges move quickly from one place to another. The net movement of electric charges in a single direction is an electric current. Electric Energy Electrical energy is measured in units of kilowatt hours. Electric Energy (in kilowatt hours) = Electric Power (in kilowatt) X Time (in hours) E = P t

Electric Charge(Transferring Charge) Learn about Electricity Electric Charge(Transferring Charge) Electrons are bound more tightly to some atoms and molecules. Electrons are more tightly bound in the soles of your shoes than in a carpet. Electrons are transferred from the carpet to the soles of your shoes; therefore the sole of your shoes have an excess of electrons and has a negative charge and the carpet has a lost of electrons and has a positive charge. The accumulation of excess electric charge on an object is called: Static Electricity

Conservation of Charge Learn about Electricity Conservation of Charge According to the law of conservation of charge, charge can be transferred from object to object, but it can’t be created or destroyed Charges Exert Forces Unlike charges attract each other and like charges repel each other. As the amount of charge on either object increases, the electrical force also increases. The further apart the objects, the weaker the electrical force between them.

Electric Fields Learn about Electricity An electric field surrounds every electric charge, and exert The force that causes other electric charges to be attracted or repelled. This is an example of how an electric field will make a positive charge move + -

Conductor Insulator Learn about Electricity A material in which electrons are able to move easily is a conductor. The best electrical conductors are metals Insulator A material in which electrons are not able to move easily is an insulator. Electrons are held tightly to atoms in insulators. Good insulators are plastics, wood rubber, and glass.

Charging by Contact Charging by Induction Learn about Electricity The process of transferring charge by touching or rubbing. Charging by Induction The rearrangement of electrons on a neutral object caused by nearby charged objects.

Lightning Thunder Learn about Electricity Lighting is a large static discharge . A static discharge is a transfer of charge between two objects because of a buildup of static electricity. Thunder The electrical energy in a lightning bolt rips electrons off atoms in the atmosphere and produces great amounts of heat . The heat causes air in the bolt’s path to expand rapidly producing sound waves that you here as thunder.

Electric Current Voltage Difference Electric Circuit Resistance Learn about Electricity Electric Current The net movement of electric charge in a single direction. Voltage Difference Related to the force that causes electric charge to flow. Measured in volts Electric Circuit A closed path that electric current follows. Resistance The tendency for a material to oppose the flow of electrons

V V R I I R Ohm’s Law so = = Learn about Electricity The relationship between voltage difference, current and Resistance in a circuit. The current in a circuit equals the voltage difference divided by the resistance. Voltage difference (in volts) current (in amperes) = resistance (in ohms V V R I so = = I R

Magnetism Magnetic Field Magnetic Poles Learn about magnetism Refers to the properties and interactions of magnets. Magnetic Field A magnet is surrounded by a magnetic field. A magnetic field exerts a force on other magnets and objects made of magnetic materials. Magnetic Poles The regions at the ends of a bar magnet is where the magnetic force is strongest. All magnets have a north pole and a south pole.

Magnetic Field Direction Learn about magnetism How Magnets Interact Two north poles or two south poles repels each other. Magnetic Field Direction When a compass is brought near a bar magnet, the compass needle rotates until it is lined up with the magnetic field lines. The north pole of a compass points in the Direction of the magnetic field. This direction is always away from a north magnetic pole and toward a south magnetic pole

The north pole of a compass points north. Learn about magnetism Earth’s Magnetic Field The north pole of a compass points north. The direction of a magnetic Is always away from the North pole toward the south pole. N North geographic pole Toward S Magnetic South N This is way the compass Needle points North W E Away From When it lines up with the Magnetic field. S N Magnetic North S South geographic pole

What makes these elements magnetic? Learn about magnetism Magnetic Materials Only a few metals, such as iron, cobalt, or nickel are attracted to magnets or can be made into permanent magnets. What makes these elements magnetic? Every atom has electrons; electrons have magnetic Properties. In most elements, the magnetic properties Cancels out. In iron, cobalt and nickel, these properties do not cancel out. Each atom in these elements behaves like a small magnet and has its own magnetic field.

Magnetic Domains (a model for Magnetism) Learn about magnetism Magnetic Domains (a model for Magnetism) In iron, cobalt, nickel and some other magnetic materials, the magnetic field created by each atom exerts a force on the other nearby atoms. Because of these factors, large groups of atoms align their magnetic poles so that almost all like poles point in the same direction. The groups of atoms with aligned magnetic poles are called Magnetic Domains. Because the magnetic poles of individual atoms in a domain are aligned, the domain itself behaves like a magnet with a north pole and a south pole.

Permanent Magnets Can a pole be Isolated Learn about magnetism A permanent magnet can be made by placing a magnetic Material, such as iron, in a strong magnetic field. The strong magnetic field causes the magnetic domains In the material to line up. Can a pole be Isolated Because every magnet is made of many aligned smaller magnets, even the smallest pieces have both a north pole and a south pole

Electric Current and Magnetism Learn about magnetism Electric Current and Magnetism Oersted hypothesized that the electric current must produce a magnetic field around the wire, and the direction of the field changes with the direction of the current Moving charges and magnetic Fields The direction of the magnetic field around the wire reverses when the direction of the current in the wire reverses. As the current in the wire increases, the strength of the magnetic field increases.

Moving charges and magnetic Fields Learn about magnetism Electromagnets An electromagnet is a temporary magnet made by wrapping a wire coil carrying a curren around an iron core. Moving charges and magnetic Fields The direction of the magnetic field around the wire reverses when the direction of the current in the wire reverses. As the current in the wire increases, the strength of the magnetic field increases.

Using Electromagnets to Make Sound Learn about magnetism Solenoid A single wire wrapped into a cylindrical wire coil. The field inside the solenoid with an iron core can be a 1000 time greater than the field inside the solenoid without The iron core. Using Electromagnets to Make Sound The CD player produces a voltage that changes according to the musical information on the CD. The CD player produces a voltage that changes according to the musical information on the CD. The varying electric Current causes both the strength and direction of the magnetic field in the electromagnet to change

Continued) Learn about magnetism The electromagnet is surrounded by a permanent fixed magnet. The changing direction of the magnetic field in the electromagnet causes the electromagnet to be attracted or repelled by the permanent magnet. This makes the electromagnet move back and forth, causing the speaker cone the vibrate and reproduce the sound that was recorded on the CD.

Making an Electromagnet Rotate Learn about magnetism Making an Electromagnet Rotate The force exerted on an electromagnet by another magnet can be used to make the electromagnet rotate. - + N S - + Permanent Magnet Permanent Magnet Unlike poles attract each other Unlike poles attract each other Electric Current in Like poles repel each other Like poles repel each other Electric Current out

Producing Electric Current Learn about magnetism Producing Electric Current Moving a loop of wire through a magnetic field causes an electric current to flow in the wire. Also, moving a magnet through a loop of wire produces a current. The magnet and wire loop must be moving relative to each other for an electric current to be produced. Electromagnetic Induction The generation of a current by changing magnetic field. If the current in a wire changes with time, the changing magnetic field around the wire can also induce a current In a nearby coil.

Using Nuclear Energy Nuclear Reactor Learn about Nuclear Energy Energy is released when the nucleus of an atom breaks apart. In this process, called nuclear fission, an extremely small Amount of mass is converted into an enormous amount of energy. Nuclear Reactor A nuclear reactor uses the energy from controlled nuclear reactions to generate electricity. They contain a fuel that can be made to undergo nuclear fission; they contain control rods that are used to control the nuclear reactions .

Nuclear Reactor Cont’d Learn about Nuclear Energy Nuclear Reactor Cont’d They have a cooling system that keeps the reactor from Being damaged by the heat produced. The actual fission of the radioactive fuel occurs in a relatively small part of the reactor known as the core . Nuclear Fuel Only certain elements have nuclei that can undergo fission. Natrutally occuring uranium contains an isotope, U-235, Whose nucleus can split apart. The fuel that is in a nuclear reactor is usually uranium dioxide. In a reactor, the uranium usually is enriched so That it contains three percent to five percent U-235.

Reactor Core Learn about Nuclear Energy Contains uranium dioxide fuel in the form of tiny pellets. The pellets are about the size of a pencil eraser and are place end to end in a tube forming a fuel rod. The tubes are then bundled and covered with a metal alloy. The core of a typical reactor contains about a hundred thousand kilograms of uranium in hundreds of fuel rods. For every kg of uranium that undergoes fission in the core, One gram of matter is converted into energy. The energy released by this gram of matter is equivalent to the energy released by burning 3 million kg of coal. .

Nuclear Fission Learn about Nuclear Energy When a U-235 nucleus absorbs a neutron, it splits into two smaller nuclei and two or three other additional Neutrons. These neutrons strike other U-235 nuclei causing them to release two or three more nuetrons each when they split.. This process is called a nuclear chain reaction .

Define the following terms 1) Lysosomes 2) Subject: Date: Today’s Topic Structures and Organelles Define the following terms 1) Lysosomes 2) Mitochondria, 3) Vacuole 4) and Golgi Apparatus, Today’s Starter Question: A vesicle that contains digestive enzymes for the Breakdown of excess or worn-out cellular substances. A membrane – bound organelle that makes energy available to the rest of the cell. A membrane bound vesicle for the temporary storage of materials. A flattened stack of tubular membranes that modifies protein and packages them for distribution outside the cell Answer: Today’s Objectives: Explain the process of diffusion, facilitated diffusion, and active transport. One: Two: Cellular transport moves substances within the cell and moves substances into and out of the cell Substances dissolved in water move constantly in random motion called Brownian motion. This random motion causes diffusion, which is the net movement of particle from an area where there are many particle of the substance to an area where there are fewer particles of the substance. The amount of substance in a particular area is called concentration. When there is no further change in concentration, but continuous movement continues, the condition is called dynamic equilibrium. A form of transport called facilitated diffusion uses transport protein to move other ions and small Molecules across the plasma membrane Summary Notes: Next Page