1. Big Time Review
Kuberg

2. Independent vs. Dependent
Independent Variable – This is the number or item you have; the number you are measuring
Independent Variable – located on the x-axis
TIME IS INDEPENDENT
Dependent Variable – This is the number you need to find; the outcome
Dependent Variable – located on the y-axis
SPEED IS DEPENDENT

3. Physical Changes Texture Color Temperature Shape
Change of State (Boiling Point and Melting Point are significant factors in determining this change.)

4. Physical Properties Luster Malleability – Ability to bend
Ductility - Ability to be drawn into a thin wire
Density
Viscosity
Solubility
Mass
Volume 

5. Chemical Changes Change in Temperature Change in Color
Noticeable Odor (after reaction has begun)
Formation of a Precipitate
Formation of Bubbles

6. Indicators of chemical reactions
Emission of light or heat
Formation of a gas
Formation of a precipitate
Color change
Emission of odor

7. Chemistry

8. Atom Protons Neutrons Electrons Positively Charged Particles
Found in Nucleus
Equals Atomic Number
Neutrons
Neutral Charged Particles (No Charge)
Found in Nucleus
Electrons
Negatively Charged Particles
Found outside of Nucleus

9. Electron Shells Number of Protons = Number of Electrons
Electrons vary in the amount of energy they possess, and they occur at certain energy levels or electron shells.
Electron shells determine how an atom behaves when it encounters other atoms

10. Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons
C would like to
N would like to
O would like to
Gain 4 electrons
Gain 3 electrons
Gain 2 electrons

12. Electron Dot Structures
Symbols of atoms with dots to represent the valence-shell electrons
H He:
          
Li Be  B   C   N   O  : F  :Ne :
       
          
Na Mg  Al  Si  P S :Cl  :Ar :
       

13. Diatomic elements There are 8 elements that never want to be alone.
They form diatomic molecules.
H2 , N2 , O2 , F2 , Cl2 , Br2 , I2 , and At2
The –ogens and the –ines
1 + 7 pattern on the periodic table

14. Chemical Bonds

15. Types of Chemical Bonds
Ionic bonds – Metal and Non-Metal
Covalent bonds – Non-Metal
Metallic bonds - Metal

16. Ionic Bond
Between atoms of metals and nonmetals with very different electronegativity
Bond formed by transfer of electrons
Produce charged ions all states. Conductors and have high melting point.
Examples; NaCl, CaCl2, K2O

17. Formation of Ions from Metals
Ionic compounds result when metals react with nonmetals
Metals lose electrons to match the number of valence electrons of their nearest noble gas
Positive ions form when the number of electrons are less than the number of protons
Group 1 metals  ion 1+
Group 2 metals  ion 2+
Group 13 metals  ion 3+

18. Formation of Sodium Ion
Sodium atom Sodium ion
Na  – e  Na +
( = Ne)
11 p p+
11 e e-

19. Formation of Magnesium Ion
Magnesium atom Magnesium ion 
Mg  – 2e  Mg2+
(=Ne)
12 p p+
12 e e-

20. Covalent Bond
Between nonmetallic elements of similar electronegativity.
Formed by sharing electron pairs
Stable non-ionizing particles, they are not conductors at any state
Examples; O2, CO2, C2H6, H2O, SiC

21. 2. Covalent bonds- Two atoms share one or more pairs of outer-shell electrons.
Oxygen Atom
Oxygen Atom
Oxygen Molecule (O2)

22. Metallic Bond Formed between atoms of metallic elements
Electron cloud around atoms
Good conductors at all states, lustrous, shiny, very high melting points
Examples; Na, Fe, Al, Au, Co

23. Metals Form Alloys Metals do not combine with metals. They form
Alloys which is a solution of a metal in a metal.
Examples are steel, brass, bronze and pewter.

24. C2H4 + 3O2 -> 2CO2 + 2H2O This is a chemical equation.
C2H4 + 3O2 - These are the reactants.
2CO2 + 2H2O – These are the products.
C2H4 + 3O2 -> 2CO2 + 2H2O – The #s in red are the coefficients. These can be changed to balance the equation.
C2H4 + 3O2 -> 2CO2 + 2H2O - The #s in red are the subscripts. These balance the compound and cannot be changed.

25. Synthesis Reactions Mg3N2 (s) A + B ® AB Na (s) + Cl2 (g) ® NaCl (s)
Also called combination reactions
2 elements, or compounds combine to make one compound.
A + B ® AB
Na (s) + Cl2 (g) ® NaCl (s)
Ca (s) +O2 (g) ® CaO (s)
SO3 (s) + H2O (l) ® H2SO4 (s)
We can predict the products if they are two elements.
Mg (s) + N2 (g) ®
Mg3N2 (s)

26. Chemical Reactions

27. A simulation of the reaction: 2H2 + O2 ® 2H2O

28. Decomposition Reactions
decompose = fall apart
one compound (reactant) falls apart into two or more elements or compounds.
Usually requires energy
AB ® A + B
NaCl Na + Cl2
CaCO CaO + CO2

29. Decomposition Reactions
If the compound has more than two elements you must be given one of the products
The other product will be from the missing pieces
NiCO3 (aq)
H2CO3(aq) ®
CO2 (g)
+ Ni (s)
H2 (g)
+ CO2 (g)

30. Single Replacement A + BC ® AC + B
Also referred to as single displacement
One element replaces another
Reactants must be an element and a compound.
Products will be a different element and a different compound.
A + BC ® AC + B
2Na + SrCl2 ® Sr + 2NaCl
F2 + LiCl ® LiF + Cl2

31. Double Replacement AB + CD ® AD + CB ZnS + 2HCl ® ZnCl + H2S
Two things replace each other.
Reactants must be two ionic compounds or acids.
Usually in aqueous solution
AB + CD ® AD + CB
ZnS HCl ®
ZnCl + H2S
AgNO3 + NaCl ®
AgCl + NaNO3

32. Combustion
A reaction in which a compound (often carbon) reacts with oxygen
CH4 + O ® CO2 + H2O
C3H8 + O2 ® CO2 + H2O
C6H12O6 + O2 ® CO2 + H2O

33. The charcoal used in a grill is basically carbon
The charcoal used in a grill is basically carbon. The carbon reacts with oxygen to yield carbon dioxide. The chemical equation for this reaction is C + O2  CO2

34. How to recognize which type
Look at the reactants
Element(E), Compound(C)
E + E C
E + C
C + C
Acid + Base
Look at the Products
CO2 + H2O
Redox
Synthesis
Decomposition
Single replacement
Double replacement
Acid/Base reaction
Combustion

35. Examples Synthesis H2 + O2 ® H2O ® Decomposition AgNO3 + NaCl ®
Double replacement
Zn + H2SO4 ®
Single replacement
HgO ®
Decomposition
KBr +Cl2 ®
Single replacement
Mg(OH)2 + H2SO3 ®
Double replacement

36. Some Properties of Acids
Produce H+ (as H3O+) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule)
Taste sour
Corrode metals
Electrolytes
React with bases to form a salt and water
pH is less than 7
Turns blue litmus paper to red “Blue to Red A-CID”

37. Acid and Base

38. Some Properties of Bases
Produce OH- ions in water
Taste bitter, chalky
Are electrolytes
Feel soapy, slippery
React with acids to form salts and water
pH greater than 7
Turns red litmus paper to blue “Basic Blue”

39. Acid Nomenclature An easy way to remember which goes with which…
No Oxygen
w/Oxygen
An easy way to remember which goes with which…
“In the cafeteria, you ATE something ICky”

40. pH Scale

41. Law of Conservation of Mass
The Law of Conservation of Mass states that in any closed system the amount of mass will remain constant over time. This means that matter can neither be created nor destroyed.
In a chemical reaction, the mass of the reactants you start with will equal the mass of the products once the reaction is complete. Even when matter is transformed, the mass will remain constant.

42. Reaction Energy
All chemical reactions are accompanied by a change in energy. 
Exothermic - reactions that release energy to their surroundings (usually in the form of heat)
Endothermic - reactions that need to absorb heat from their surroundings to proceed.

43. Endothermic vs. Exothermic