Q1-1:  State the definition for REACTANT.

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Q1-2:  State the definition for PRODUCT.

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A1-2: A substance that forms in a chemical reaction. (Note: usually found on the RIGHT side of a chemical equation.)

Q1-3:  State the definition for CHEMICAL ENERGY.

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Q1-4:  State the definition for EXOTHERMIC REACTION.

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Q1-5:  State the definition for ENDOTHERMIC REACTION.

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Q1-6:  List three signs that could indicate that a chemical reaction is taking place.

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Q1-7:  List four forms of energy that may be absorbed or released during a chemical reaction.

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Q1-8:  In the following equation, what are the reactants and what are the products?
                  CH₄   +    2O₂     -------à   CO₂    +      2H₂O

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A1-8: a) reactants:  CH₄   +    2O₂    [methane & oxygen]; b)products: CO₂    +      2H₂O [carbon dioxide & water]

Q2-1: What is a CHEMICAL EQUATION?

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Q2-2: What is a COEFFICIENT?

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Q2-3:  What is a SUBSCRIPT?

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Q2-4:  Balance the following chemical equation   ---- a)

H₂O        à        H₂           +         O_{2
water    (yields)      hydrogen         +        oxygen}

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A2-4:
                  2 H₂O        à      2 H₂           +         O₂
 

Q2-4: Balance the following chemical equation   ---- b)
KOH        +       HCl              à            KCl           +     H₂O
_{potassium hydroxide  +  hydrochloric acid    (yields)        
                                                                               potassium chloride   +   water}

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A2-4:
 2 KOH     +    2 HCl        à     2 KCl      +   2 H₂O 

Q2-4:  Balance the following chemical equation   ---- c)
NaHCO₃         à      H₂O       +      CO₂           +    Na₂CO_{3
sodium bicarbonate    (yields)  water   +    carbon dioxide  +   sodium carbonate
(baking soda)}

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A2-4:
     2 NaHCO₃      à      H₂O    +     CO₂     +    Na₂CO₃

Q2-4:  Balance the following chemical equation   -----   d)

FeS        +    HCl          à        H₂S               +         FeCl_{2  
iron sulfide  +  hydrochloric acid   (yields)  hydrogen sulfide   +   iron chloride}

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A2-4:
       FeS     +    2 HCl        à       H₂S      +    FeCl₂  
 

Q2-5: Balance the following chemical equation   ---- e)

Mg          +             O₂          à           MgO
_{magnesium    +           oxygen       (yields)         magnesium oxide}

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A2-4:
        2 Mg       +    O₂        à      2 MgO 

Q2-4: Balance the following chemical equation   ---- f)

K            +       H₂O      à           KOH                 +      H_{2
potassium       +   water     (yields)   potassium hydroxide    +        hydrogen}

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A2-4:
         2 K    +    2  H₂O      à      2  KOH     +     H₂ 

Q2-4: Balance the following chemical equation   ----  g) 

CuCl₂          +       Al        à            AlCl₃             +     Cu
_{copper chloride     +   aluminum   (yields)    aluminum chloride   +   copper}

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A2-4:
        3 CuCl₂    +     2 Al      à    2 AlCl₃     +   3 Cu

Q2-4: Balance the following chemical equation   ----  h)

CH₄          +       O₂       à          CO₂             +     H₂O
_{methane        +      oxygen    (yields)      carbon dioxide    +      water}

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A2-4:
       CH₄     +     2 O₂       à      CO₂        +    2 H₂O 

Q2-4:Balance the following chemical equation   ----   i) 

CO₂          +       H₂O        à         C₆H₁₂O₆      +          O_{2
carbon dioxide   +    water     (yields)         sugar              +                oxygen}

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A2-4:
    6 CO₂      +     6 H₂O       à    C₆H₁₂O₆     +   6 O₂ 

Q2-4: Balance the following chemical equation   ----  j)   

   Fe          +       O₂        à        Fe₂O_{3
  iron             +      oxygen      (yields)       iron oxide}

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A2-4:
          4 Fe       +    3 O₂       à      2 Fe₂O₃ 

Q2-4: Balance the following chemical equation   ----   k)  

   N₂          +       H₂        à        NH_{3            
nitrogen         +    hydrogen     (yields)      ammonia}

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A2-4:
             N₂      +    3 H₂       à    2 NH₃              

Q2-4: Balance the following chemical equation   ----  l)   

 Cu₂O          +       C        à        Cu         +     CO_{2
copper oxide     +    carbon     (yields)    copper      +   carbon dioxide}

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A2-4:
     2 Cu₂O      +     C        à   4 Cu      +    CO₂ 

Q3-1: Define the term SYNTHESIS REACTION and give an example.   
    a) Definition:
    b) Example:

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A3-1:  a) Two or more substances combine to form a new substance. b) N₂    +  3 H₂    à   2 NH₃ 

Q3-2: Define the term DECOMPOSITION REACTION and give an example.
    a) Definition:
    b) Example:

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A3-2:  a) When a single compound is broken down to form two or more simpler substances; b) 2 H₂O   à    2 H₂    +   O₂

Q3-3: Define the term COMBUSTION REACTION and give an example.  
    a) Definition:
    b) Example:

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A3-3: a) The oxidation reaction of an organic compound, in which heat is released; b) CH₄    +   2 O₂    à  CO₂    +   2 H₂O

Q3-4: Define the term SINGLE-DISPLACEMENT REACTION and give an example.         a) Definition:
                             b) Example:

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A3-4: a) Where one element or radical takes the place of another element or radical in a compound; b) 2 Cu₂O  +  C        à  4 Cu   +  CO₂

Q3-5: Define the term ELECTROLYSIS.

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A3-5: The breaking down of water into hydrogen and oxygen by passing electric current through water.

Q3-6: Define the term DOUBLE-DISPLACEMENT REACTION and give an example.       a) Definition:
                           b) Example:

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A3-6: a) A reaction in which two compounds exchange ions; b)  FeS   +   2 HCl          à   H₂S   +   FeCl₂

Q3-7: What is a FREE RADICAL?

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A3-7: An atom or a group of atoms that has one unpaired electron. (Hydrogen is often a free radical because it only has one electron available for bonding.)

Q3-8: Define the term REDOX REACTION and give an example.
    a) Definition:
    b) Example:

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A3-8: a) This is an oxidation-reduction reaction in which one species is oxidized (loses electrons) and another is reduced (gains electrons); b) iron rusting to produce iron oxide

Q4-1: List four factors that affect the rate of a reaction.
a)                               b)                      c)                              d)

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A4-1: temperature, surface area, concentration, pressure

Q4-2: Define the term CATALYST.

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A4-2: A substance that changes the rate of a chemical reaction without being consumed or changed significantly.

Q4-3: Define the term ENZYME.

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A4-3: A type of protein that speeds up metabolic reactions in plants and animals without being permanently changed or destroyed.

Q4-4: Define the term SUBSTRATE.

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A4-4: The reactant in reactions catalyzed by enzymes.

Q4-5: Substances that slow reactions are called ____________________.

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A4-5: inhibitors

Q4-6: When you open a soda bottle, what change occurs that allows the dissolved carbon dioxide in the soda to come out of solution?

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A4-6: You have changed the pressure. As long as the cap is on the bottle, the carbon dioxide dissolved in the water is spread out evenly throughout the bottle due to the pressure in side the bottle. Opening the bottle allows the gas to escape from a high pressure environment inside the bottle to a lower pressure area outside the bottle.

Q4-7: Define the term CHEMICAL EQUILIBRIUM.

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A4-7: A state of balance in which the rate of a forward reaction equals the rate of the reverse reaction and the concentrations of products and reactants remain unchanged.

Q4-8: What is Le Chatelier’s principle?

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A4-8: If a change is made to a system in chemical equilibrium, the equilibrium shifts to oppose the change until an new equilibrium is reached.

Q4-9: Compare a catalyst and an inhibitor.

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A4-9: A catalyst speeds up a reaction, an inhibitor slows it down.

Q4-10: The Haber process uses Le Chatelier’s principle to produce more ammonia. What two things do they have to do to the reaction to get more ammonia as a product?

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A4-10: high pressure and low temperature

Q5-1: Chemical reactions occur when substances undergo __________ changes to form new substances.

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A5-1: chemical

Q5-2: Chemical reactions involve changes in __________.

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A5-2: energy

Q5-3: A chemical equation uses __________ to represent a chemical reaction

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A5-3: symbols

Q5-4: . A balanced equation tells you the _______ ______, or proportion of ________ and ________, in a chemical reaction.

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A5-4: mole ratio ..... reactants ... products

Q5-5: List four types of chemical reactions.

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A5-5: synthesis, decomposition, single-replacement, double-displacement

Q5-6: Free-radical reactions and redox reactions can be understood as changes in the number of __________ that atoms have.

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A5-6: electrons

Q5-7: Anything that increases _________ between particles will increase the rate of a reaction.

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A5-7: contact

Q5-8: Process that go in both directions may result in ______________.

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A5-8: chemical equilibrium