2. Indicator 7-5 The Chemical Nature of Matter The student will demonstrate an understanding of the classifications and properties of matter and the changes that matter undergoes. (Physical Science) Standard 7-5.1 Recognize that matter is composed of extremely small particles called atoms. Standard 7-5.2 Classify matter as element, compound, or mixture on the basis of its composition.

4.  Atoms- All matter is composed of extremely small particles, too small to be seen with a classroom microscope.

5.  Elements - are pure substances that cannot be changed into simpler substances  Elements are composed of one kind of atom.  Examples:  O-Oxygen  H-Hydrogen  Cl-Chlorine  Na-Sodium  N-nitrogen  C-Carbon

6.  Compounds -are pure substances that are composed of two or more types of elements that are chemically combined. Examples  CO2- Carbon Dioxide  NaCl- Sodium Chloride  H2O- Water

7.  Mixtures- are composed of two or more different substances that retain their own individual properties and are combined physically (mixed together). Examples Trail Mix Munches Chips Snickers Lucky Charms

8.  homogeneous mixture, a mixture that is uniform throughout, the substances are evenly mixed and cannot be visibly distinguished. The particles of the substances are so small that they cannot be easily seen. Another name for a homogeneous mixture is a solution.  Example Kool-aide Tea

9.  heterogeneous mixture a mixture that is not uniform throughout, the component substances can be visibly distinguished.  Trail Mix  Oil and Water

10. It is essential for students to know that matter is composed of extremely small particles, too small to be seen with a classroom microscope, called atoms.  Atoms are the smallest part of an element that has the chemical properties of the element.  A single atom has mass and takes up space.

11.  Directions: Answer the questions using your notes. 1.What is the smallest particle which makes up any substance? 2. What makes up all substances on Earth? 3. Can atoms be seen with a classroom microscope? True or False?

13. It is essential to know that metals and nonmetals are two major groups of elements that have different physical properties.

14. Metals Non metals All the Elements in the Periodic Table are either a metal or non metal!

15. Luster Conductors Malleable Ductile High density

16.  Chrome is a Shiny Metal!!

17.  We use the element Copper (CU) for conducting electricity  The element Iron (Fe) is used to make pots and pans

18.  A blacksmith heats the metal to make it easier to hammer into different shapes

19. To this From this Raw Copper (Cu) Ore as dug from the Earth Copper Wire Found in most electrical appliances

20.  Cannon balls are small, but heavy.  Bowling balls, are small but heavy.

21.  Dull—Not shiny  Nonconductors—Heat and electricity do not move through them easily  Brittle—Break or shatter easily (solids) Na- Sodium C- Carbon Cl- Chlorine Gas

22. 1. List the physical properties of metals and non metals. Metals _________________ Non Metals _________________

23. 2. Describe the property of Luster in your own words using one picture from below.

24.  3. Look at the pictures. Write a summary of the physical properties of Nonmetals using one of the objects. Na- Sodium Cu-Copper WireCl- Chlorine Gas

25.  4. Using your periodic table, which of the following elements is ductile, malleable and has a high density. A. Cl – Chlorine B. Na – Sodium C. Ag- Gold D. C- Carbon

26.  5. Using your periodic table, which of the following elements is not a conductor and has a low density. F.Ag-Gold G.Cu-Copper H.Al-Aluminum I.O-Oxygen

27.  Answers 1. Metals Luster Conductors Malleable Ductile High density  2. You should have choose to write about the picture of the car and how shiny it is.  3. You should have choose to write about the Na- sodium or the Cl-chlorine gas and described the three physical properties of Non-Metals.  4. C. Ag- Gold- it is the only metal, the other choices are non metals.  5. I. O-Oxygen it is the only nonmetal, the other choices are metals. Non Metals Dull Nonconductors Brittle

29. It is essential to know how to use the periodic table to identify the basic organization of elements. TLWBAT: Recognize the organization of the elements by using the periodic table Exemplify elements that are metals and nonmetals given a periodic table Recognize the location of an element on the periodic table Recognize the location of groups of metals and nonmetals Recognize that families are columns of elements Identify an element using the organization of the periodic table (atomic number or symbol).

30.  Period – horizontal row on the periodic table is called a period. Periods go Side to side

31. Families go Up & Down  Families- also called groups, are vertical columns of elements on the periodic table

32.  Periodic tables have a square for each element. Each square contains 4 Bits of information on the element; atomic mass atomic number element symbol element name

33.  The elements are arranged in numerical order within the Periodic Table  On the periodic table there is a zigzag line on the right side of the table.  The line separates two sections of elements;  Metals  Nonmetals zigzag line__ __

34.  A horizontal row on the periodic table is called a period. Periods go Side to side

35.  Families, also called groups, are vertical columns of elements on the periodic table  Elements in the same family have similar properties. Families go Up & Down

36.  Metals A classification of elements located on the left side of the zigzag line on the periodic table.  Examples of metals are:  Sodium (Na),  Calcium (Ca)  Iron (Fe),  Aluminum (Al)  There are more elements are metals than nonmetals.

37.  Nonmetals A classification of elements located on the right side of the zigzag line on the periodic table.  Examples of nonmetals are: Chlorine (Cl) Oxygen (O) Sulfur (S) Iodine (I).

38. 1. Using your periodic table, answer the following the questions for the element Gold (Au) A.What is it’s atomic number? _________________ B.What is it’s symbol? ___________________ C.What is its atomic mass? ____________________ D.What Family is it in? ________________________ E.What Period is it in? ________________________

39. 2. Correctly label the Periodic table with the following information; Where is the Zig-Zag line located? What side are the Metals located on? What side are the Nonmetals located on?

40. 3. Give four bits of information about the following elements  Iron  Aluminum  Chlorine  Iodine

41. 4. Using your periodic table, list the metals located in groups # 2.

42. 5. Using your periodic table, list the non metals located in period # 3.

44. S

45. TLWBAT; Translate chemical symbols and chemical formulas of common substances listed above to show the component parts Recognize the chemical symbols and formulas of common substances Recall the components of a chemical.

46.  Chemical symbols  Chemical formulas  Subscripts

47.  It is essential to know that chemical symbols show the atoms of the elements composing a substance. Elements Symbol is found in the periodic table of elements.

48. Symbols are written with one, two, or three letters. The first letter is always capitalized. Each element has a different symbol. For Example: ElementSymbol SodiumNa ChlorineCL HydrogenH OxygenO CarbonC NitrogenN

49.  Elements are made up of one kind of atom and the symbol for each element is unique.  Compounds are composed of more than one element and their formulas have more than one type of symbol showing the different elements that compose the compound.

50. Compounds

51.  Chemical formulas are constructed from the symbols of the elements composing the substances. For instance: H 2 + O = H 2 O  In a chemical formula, the numbers as subscripts show how many of each kind of atom are in the compound. For instance: H 2 + O = H 2 O There are 2 hydrogen elements and 1 oxygen element

52.  The subscript is written to the lower right of the element symbol. H 2 O  If no subscript is written, only one atom of that element is part of the compound.  For example, in H 2 O, the number 2 is the subscript for hydrogen and means that there are 2 atoms of hydrogen in the compound of water; since there is no subscript for oxygen it is assumed to be one atom of oxygen.

53. 1. Chemical formulas are written in a certain way. What are the three basic rules for writing a chemical formula? 2. Describe the difference between an Element and a Compound. 3. Explain the manner in which a chemical formula is written: 4. Tell where you would write a subscript and what is the purpose of a subscript. 5. When a Chemical formula is written without the use of subscripts, what does this mean?

54.  7-5.7 Identify the reactants and products in chemical equations.

55.  Identify reactants and products in chemical equations  recall the characteristics of reactants and products in a chemical reaction  recognize the component parts of a chemical equation.

56.  It is essential for students to know that when a substance is broken apart or when substances are combined and at least one new substance is formed, a chemical reaction has occurred.

57.  Chemical reaction  Chemical equation

58.  Used to represent a chemical reaction that has occurred.  Contains the chemical names or the chemical formulas of the substances that are involved in the reaction.  An arrow is used to distinguish between the substances that are broken apart or combined from the substances that are formed in the reaction.  The arrow can be translated as “yields” or “makes.”

59.  Substances broken apart or combined in a chemical reaction. located on the left side of the arrow.

60.  New substances formed in a chemical reaction. Products are located on the right side of the arrow.

61.  Fill in your notes ReactantProduct Hydrogen gas + Oxygen gasYields/MakesWater 2H 2 + O 2  2H 2 O

62.  Identify the Reactants and the products in this reaction;  How many water molecules are present in this equation? ____________ O 2 + 2H 2 __________ 2H 2 O

63.  What is the purpose of the arrow in a Chemical Equation? A. To separate the elements B. To distinguish between the reactants and products C. To show where the energy is going D. To help the reader follow along

64.  Chemical equations are best described by which of the following statements? A.The way that elements form other compounds B.Elements that combine to form new substances C.Used to represent a chemical reaction that has occurred D.A way to understand a chemical

65.  Substances that are combined during a chemical reaction are called which of the following? A. Chemical Formula B. Chemical Equation C. Molecules of action D. Reactants

66.  Identify the correct order of the process of a chemical reaction. (Remember the arrows) A.ReactantYieldProduct X + X 2X B.Product YieldReactant 2xX + X C.Yield Reactant Product C X + X 2x D.Product YieldReactant 2xX + X

68.  The objective of this indicator is to explain how a balanced equation supports the law of conservation of matter; therefore the primary focus of assessment should be to construct a cause-and-effect model of how the number of atoms of elements on reactant side of the equation must equal the number of atoms of elements on the product side of the equation.

69.  Recall the law of conservation of matter;  Recognize whether or not a chemical equation is balanced or not  Identify the coefficient in a chemical equation  Summarize how the law of conservation of matter relates to a balanced equation.

70.  Coefficient  Law of conservation of matter  Balanced chemical equation

71.  It is essential to know that 1. the amount of matter does not change during a chemical reaction 2. the atoms are rearranged to form new substances.

72.  The law of conservation of matter states that matter can neither be created nor destroyed, but can be changed in form.

73.  Because matter is neither created nor destroyed, the total mass of the material(s) before the reaction is the same as the total mass of material(s) after the reaction.

74.  A balanced chemical equation has the same number of each kind of atom on the reactant side as on the product side.

75.  To determine whether a chemical equation is balanced, two numbers are considered: 1. the subscript and 2. the coefficient.

76.  A coefficient is the number that comes before the chemical formula and indicates the number of particles that participate in the reaction.

77.  In order to determine whether an equation is balanced multiply the number in front of the chemical formula in the equation (coefficient) by the number written below the symbol for the element(s) (subscript) in the formula.  If no coefficient is written, mulitiply by by one.

78.  For instance, for “2H 2 O” there are 4 hydrogen atoms and 2 oxygen atoms. 2 (coefficient) X 2 (subscript) =4 Hydrogen 2 (coefficient) X 1 (subscript) = 2 oxygen

79.  The number of each kind of atom on the left side of the arrow must equal the number of each kind of atom on the right side of the arrow then the equation is said to be balanced.

81.  7-5.9 Compare physical properties of matter (including melting or boiling point, density, and color) to the chemical property of reactivity with a certain substance (including the ability to burn or to rust).

82.  The objective of this indicator is to compare physical properties to chemical properties of matter and to determine the similarities and differences between physical and chemical properties of matter.

83.  Physical properties  Melting Point  Boiling Point  Density  Chemical properties  Rusting  Burning

84. It is essential to know that physical and chemical properties can be used to identify substances.

85.  Physical properties can be observed and measured without changing the kind of matter being studied.

86.  The following physical properties can be used to help identify a substance:  Melting Point  Boiling Point  Density  Color

87.  The temperature at which a solid changes to a liquid.  The temperature at which a pure substance melts is unchanging under constant conditions.

88. The melting point of a pure substance can be used as a physical property for identification. Example Ice melts to form liquid water at 0 0 C (32 o F).

89.  The temperature at which a liquid boils. During the process of boiling a substance changes from a liquid to a gas.  As long as the substance is boiling the temperature of the liquid remains constant (at the boiling point).

90.  Boiling point is unchanging under constant conditions for a given substance and therefore can be used as a physical property for identification of the substance.  Example: The boiling point for pure water at sea level is 100 o C or 212 o F.

91.  Density is a property that describes the relationship between the mass of a material and its volume.  Substances that are denser contain more matter in a given volume.

92.  The density of a substance will stay the same no matter how large or small the sample of the substance, and therefore, density can be used as a physical property for identification of the substance.

93.  Example lead is a heavy and dense metal. The density of lead is much greater than the density of the very light metal like aluminum.

94.  Color can be used to help identify a substance, along with other properties.  By itself color is not a significant identifier of a substance.  Transparency is the absence of color.

96.  A chemical property of one substance usually involves its ability to react (combine) or not react with another specific substance.

97.  Flammability is the ability of a substance to burn that involves reacting quickly with oxygen to produce light and heat.

98.  Rusting is -the ability of a substance to rust is a chemical property that involves a substance reacting slowly with oxygen.

99.  If a substance reacts with vinegar, it makes a new substance………………. If it does not react, you will have vinegar and that substance separate from one another.

100.  Example: Mixing the elements Copper (Cu) and Tin (Sn) to make Brass. A Chemical Change transforms one type of matter into another kind, which may have different properties.

101.  Example Taking a sheet of Paper and cutting it into small pieces. A Physical change is a change in which the identity of the substance does NOT change.

102. 1. List the three types of physical properties and describe each.

103. 2. Describe the difference between physical properties and chemical properties of substances.

104. 3. Summarize the two types of chemical properties.