Download Chemical Reactions (Chapters 7 and 8) Vocab and Reading

Chemical Reactions (Chapters 7 and 8) Vocab and Reading Assignment
Please define these words (found in chapters 7 and 8) in your vocab notebook:
Law of Conservation of Mass
Product
chemical reaction
balancing a chemical equation coefficient
Precipitation reaction strong electrolyte
Molecular equation
Acid
chemical equation
strong acid
soluble solid
complete ionic equation
strong base
precipitate
insoluble (slightly soluble) solid
spectator ions net ionic equation
salt
oxidation-reduction reaction
Double-replacement reaction acid-base reaction
single-replacement reaction
Combustion reaction
base
precipitation
reactant
synthesis (combination) reaction
decomposition reaction
Chapter 7 reading questions (complete by December 17th)
1.
What types of evidence indicate that a chemical reaction has taken place (4 things)?
2. Write chemical equations for each of the following reactions:
a. Gaseous chlorine reacts with an aqueous solution of potassium bromide to form liquid
bromine and an aqueous solution of potassium chloride.
b. Solid aluminum reacts with solid iodine to produce solid aluminum iodide.
c. Solid magnesium reacts with an aqueous solution of hydrochloric acid to form an
aqueous solution of magnesium chloride and bubbles of hydrogen gas.
3. Balance each of the equations from question #2 (re-write each equation!).
4. What is the difference between a coefficient and a subscript in a chemical equation? Which can
be changed when balancing a chemical equation?
5. What is the difference between an aqueous solution and a liquid?
Chapter 8 reading questions (complete by January 10)
1.
What are the driving forces that indicate a chemical reaction is likely to occur?
2. Use the solubility rules in Table 8.1 or Figure 8.3 to predict which of the following will be soluble
in water:
a. Potassium nitrate
This assignment is DUE January 10th!!
b. Zinc hydroxide
c. Calcium carbonate
d. Ammonium chloride
3. Consider two separate beakers: one containing an aqueous solution of hydrochloric acid and
one containing an aqueous solution of lead (II) nitrate.
a. Draw a picture of each solution showing the ions present.
b. Draw a picture after the solutions are mixed showing what is present.
c. Predict the products for any reaction that occurs.
d. Write an equation for the reaction.
4. How does a molecular equation differ from a complete ionic equation?
5. What is a spectator ion and what happens to it in a net ionic equation?
6. Consider the following reaction: aqueous sodium sulfate is added to aqueous barium bromide
to form solid barium sulfate and aqueous sodium bromide.
a. Write the molecular equation.
b. Write the complete ionic equation
c. List the spectator ions.
d. Write the net ionic equation
7. What are the products in a reaction between an acid and a base? How can you tell that a
reaction has occurred?
8. What is an oxidation-reduction reaction? How can you identify this type of reaction?
9. What are the four driving forces in chemical reactions?
10. Classify the following unbalanced reaction equations as precipitation, acid-base, or oxidationreduction reactions.
a. Fe(s) + H2SO4(aq)
Fe3(SO4)2(aq) + H2(g)
b. HClO4(aq) + RbOH(aq)
RBClO4(aq) + H2O(l)
c. K2SO4(aq) + CaCl2(aq)
KCl(aq) + CaSO4(s)
d. Ni(s) + Cl2(g)
NiCl2(s)