Chemistry of Life.

Chemistry of Life

Section 1: The Atom _________ = smallest piece of _________ that still regains the property of the _____________ True or False: All matter is made up of atoms For example: Hydrogen is composed only of __________atoms, silver is only composed of _________atoms, etc Atoms are composed 3 of ___________particles: _________________ Atom matter element hydrogen silver Sub-atomic Proton Neutron Electron

Sub-atomic Particle Definition Location Charge Proton Particles with an electrical charge of +1 Nucleus= positively charged center of the atom Positive, + Neutron Neutral particles that do not have an electrical charge Nucleus Neutral, o Electron Particles with an electrical charge of -1 Electron Cloud Negative, -

Section 1: The Atom Are protons, neutrons, and electrons the smallest particles that can exist? __________ are not composed of smaller particles (one of the most basic types of particles) ___________ and __________ are made up of smaller particles called ___________ Electron Proton Neutron quark

Section 2: Mass of an Atom
_________ _________ Most of the __________ in an atom is contained in the ______________ _____________ and ____________ are far more massive than electrons Mass of an ____________ is so small, that it is not taken into account when measuring ___________ Atomic Mass mass nucleus proton neutron electrons atoms

Atomic mass unit (_______ )- __________________________________________ Equals about the mass of a _________ or ___________ AMU unit of measurement used for atomic particles Proton neutron

Wildcats Share Answer the following questions, by referencing to the front of your note packet. Does every element within the table have the same AMU? Does every element listed have the same atomic number? Why do you think these are all the same or different?

element Every __________ is different because they have a different number of ________ Number of __________ tells you what type of element you have Atomic number= the number of protons in an atom Atomic number of carbon= ___, therefore carbon has ____ protons Protons Protons 6 6

______________ = the sum of the number of __________ and _________in the nucleus of an atom Mass number= protons + neutrons Example Mass number of carbon=_____, therefore there must be ___ neutrons and ___ protons Number of neutrons= mass number- atomic number Mass number protons neutrons 12 6 6

Wildcats Share Solve the following within your groups.
If Boron has a mass number of 10, with 5 protons, then how many neutrons does it contain? The atomic number of Chlorine is 17, therefore how many protons does it contain? Magnesium has a mass number of 24, with 12 neutrons, what would the atomic number of magnesium be? 5 17 12

How do you name an element?
Naming Elements: ___________________ for elements can stand for several different things First letter(s) of the __________ _________ First letter(s) of the ___________ name for the element Example: ___________________________________ Some elements named for ________________ Other named for ____________ or___________ All these __________ are used world-wide, so everyone understands what the symbols mean Chemical Symbol Elements name Latin Ferris= Iron, argentum= silver Scientists places properties symbols

Isotopes ____________ Atoms of the ________ element that have different numbers of ___________ Examples: Carbon-___= most common form of carbon Carbon-___= carbon atoms with ___extra neutrons __________________ Because they have the same number of ______________, all isotopes of an ____________ have the same chemical properties. same neutrons 12 14 2 radioactive protons element

___________________ = weighted average mass of the mixture of its ___________ Example: Boron- ____ and Boron-____ ___ out of ___ boron atoms are Boron- 11 To find the average atomic mass: [4/5 (11 amu) + 1/5 (10 amu) amu] Average Atomic Mass isotopes 10 11 4 5

Section 3: The Periodic Table
In the late 1800’s,________________, a Russian chemist, searched for a way to organize the ___________ He Organized elements in order of ___________ atomic number Noticed a __________ _______________: elements are arranged by increasing atomic number and by changes in __________and __________ properties Dmitri Mendeleev elements increasing pattern Periodic Table physical chemical

________________________ What is the electron cloud? In a ___________ atom (no charge) the number of electrons _________ the number of ________ Electrons in the cloud have different amounts of ________ depending on which _______ they occupy Closer to the _________ the electron, the _______the energy of the electron Electrons fill the energy levels starting at the ________ levels (near the nucleus) then fill the ________ levels Electron Cloud Structure Neutral equals protons Energy level nucleus lower lower outer

electrons Elements with the same number of ___________ in their outer layer are in the same ________ and have similar ___________ _________ elements will contain ____ electrons in their ________________shell Outer most electrons=__________________ group properties Stable 8 Outer-most valence

Label the boxes within your diagrams.

Wildcats Share Use the color pencils at your desk to color the sulfur atom below. Nucleus = blue Electrons= green Circle the electrons That are found within The valence shell. What is the atomic mass of sulfur? What is the number of protons and neutrons?

Organizing the Periodic Table ________ (families)= __________columns in the periodic table Numbered __________ Elements in each group have __________ properties Example: group ______(copper, silver, and gold) are all shiny and good conductors of electricity and heat What is responsible for these similar properties? ______________________ Groups vertical 1-18 similar 11 Structure of the atoms

Row __________ on the Table Notice: row one only has _________ and _________ Hydrogen= ____ electron, helium= ____electrons Since the first shell can only hold ____ electrons, helium has a _____ outer shell and is happy Row ____ starts over with__________, which has _____ electrons… End of each row is an ___________ that has _____ valence electrons Helium Hydrogen 1 2 2 full 2 Lithium 3 element 8

________ Group, _________ Properties Example: group 17, the _________ All have ___ outer electrons All will undergo __________reactions in the same way All have the ability to form ____________ with elements readily with elements in group ____ ____________ : a substance formed by the chemical combination of 2 or more elements Elements in group ____ all have ___ valence electron same similar halogens 7 Chemical compounds 1 compounds 1 1

For Example: Na (________) and Cl (_________) bond easily to form table salt (_________) Group ____ have __ valence electrons which make them unreactive Group 17 Group 1 NaCl 8 18

Regions _____________on the Periodic Table _________ = horizontal rows of elements on the periodic table that increase by one __________ and one __________ as you go from _________to __________ _____________________________________ Periods proton electron left right Metals, metalloids, and nonmetals

Section 4: Bonding __________ _________: tells what elements a compound contains and the exact number of the atoms of each element in the compound Example- What is the chemical symbols and chemical formulas for the following? Chemical Formula Sodium Chloride + → Sodium Chloride Na Cl NaCl 2Hydrogen Oxygen + → Water H2 O H2 O

Section 4: Bonding What does the H2 mean? The “little” 2 is a __________ A subscript written after the ____________, tells you how many _______ of that element are in a unit of the compound If a symbol has no __________, then the unit only contains ___ atom of that element So how many atoms of each element were involved within the compound of NaCl? So how many atoms of each element were involved within the compound of H2O? subscript symbol atoms subscript 1 1 atom 1 atom of O 2 atoms of H

Section 4: Bonding _________ _________ Chemical stability
Occurs when the __________ ________ level has a maximum number of _________ Outer energy levels of _________ and _________ are stable with ___ electrons All other _________ are stable or “happy” with ___ electrons So why are Nobel gases always “happy” or considered unique? __________________________________________ Chemical stability Outermost energy electrons Helium Hydrogen 2 elements 8 They contain 8 electrons in their outermost energy level/shell

Section 4: Bonding ________ _______- getting their fill Outer levels
So how does Hydrogen or any other element without a full outer energy level become stable? ______ with partially stable outer energy levels can _____________ electrons _____________electrons they do this by ___________ within other atoms with partially complete _______ ________ ________ As a result of this combination they become _______ Which makes them atoms gain lose share Combining Outer energy level stable

Section 4: Bonding electrons ________ - lose or gain ________ to become _________ An atom that has ________ or _______ an electron is called an ______ _________ - is a _________ particle because of having lost or gained an electron, which causes it to have __________ or _________ electrons than protons atoms stable Gained lost ion ion charged more fewer

Section 4: Bonding This means:
These ____________ __________ between oppositely charged particles, such as _________, that hold _____________ together The protons and electrons are not balanced Electric forces ions compounds

Section 4: Bonding Force of attraction between the opposite charges of the ions in an ionic compound Ionic bond= _________________________________ __________________________________________ ___________ of 1 or more ________________ takes place Large amount of ____________________________ Usually formed by combining ______________________________________ Example: group _______________________ Ionic compounds= ___________________________________________ Transfer electrons Energy is released Metals and nonmetals 1 and group 17 Crystalline solids with high melting points

Section 4: Bonding Covalent bond= _________________________________________________________________ Covalent compounds= ___________________________________________ Molecule= ________________________________________ The attraction that forms between atoms when they share electrons liquids or gases at room temperature neutral particle that forms as a result of electron sharing

Section 5: Chemical Reactions
________________________________ always involve the ________________ of ____________ in reactants and the formation of new ___________ in the products ____________________= are the _____________ or _________________ that enter into a chemical reaction ____________________= are the ______________ or ________________ that are formed after the chemical reaction has occurred CO2 + H2O → H2CO3 Chemical Reactions bonds breaking bonds reactants elements compounds elements products compounds Reactants products

Chemical reactions that _____________ ___ often occur all of the time however, chemical reactions that __________________ will not happen unless a source of _____________ is available Not all chemical reactions happen automatically, most often they require ____________ the energy that is needed to get a reaction started is referred to as the ____________________ ___________ release energy require energy energy energy activation energy

______________ a substance that ______________ up the rate of a reaction __________________ are ______________ that act as biological _____________ cells use enzymes to _____________ up chemical reactions that take place within the cell this occurs by ________________ the activation energy that is needed catalyst speeds Enzyme proteins catalyst speed lowering

Chemical Properties Mixture _________-a combination of substances in which the individual ___________ retain their own __________. Example: _________- a mixture in which one or more substances (________) are distributed ________ in another substance (________) components properties Chocolate chip cookies, sugar and sand, m & m’s and skittles Solution solute solvent evenly Kool-Aid, lemonade, Gatorade, sugars and mineral ions in water

Chemical Properties The more solute that is dissolved in a given amount of solvent, the ________ the solution’s ____________ (strength) Organisms can’t live unless the _________ of dissolved substances stays within a _________, _______ ______ Organisms have many __________ to keep the concentration of __________ and ions within this range greater concentration concentration specific Narrow range mechanisms molecules

Chemical Properties Chemical reactions in organisms can depend on the ____ of the ___________. ____- a _________ of how _______ or ______ a solutions is. A scale with values ranging from ___ to ___ is used to measure pH. ______- substance with a pH _______ 7 and that forms _________ ions in water ______- substances with a pH _______ 7 and that forms _________ ions (OH-) environment pH pH measure acidic basic 14 below Acids hydrogen bases above hydroxide

Elements Important to Life
Water is necessary for many of life’s _________ and _______ ________ Water is a ______ ______ These molecules occur when there is an ________ sharing of electrons which results is each molecule having a ________ end and a ________ end processes Material transport Polar molecule unequal negative positive

Water molecules attract each other, as well as _____ and other ______ ________, because of this water can dissolve many ______ ________ and many other _________ _______ _________ _____-weak, chemical bond formed by the attraction of __________ charged hydrogen atoms to other _________ charged atoms ions Polar molecules Ionic compounds Polar molecules Hydrogen bonds positively negatively

Because of its ________ water has the unique property of being able to ______ up thin tubes. This property is important within ______ Water resists ________ in ____________ This property helps cells _________ an optimum environment polarity creep plants changes temperature maintain

_________- the net __________ of particles from an area of _______ concentration to an area of _______ concentration Diffusion is a ______ process because it relies on the _________ molecular motion of ______ Three key factors ____________, ____________, and _________ affect the rate of diffusion Diffusion movement higher lower slow random atoms concentration temperature pressure

The more ___________ the substances, the more rapidly ________ occurs Increasing ___________ and ________ increase particle motion and increase diffusion _________ _________-result of diffusion where there is __________ movement of particles but no overall change in ___________ concentrated diffusion temperature pressure Dynamic equilibrium continuous concentration

The difference in _____________ of a substance across space is called a __________ _________ Because ions and molecules diffuse from an area of _______ concentration to an area of ______ concentration they are said to move ______ the gradient Diffusion is one of the ________ by which cells move __________ in and out of the cell concentration Concentration gradient higher lower with methods substances

Fill in the diagram to show diffusion and dynamic equilibrium

Chemistry of Life.

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