TOC # _______ North Smithfield High School
REVIEW-Unit 3 (Ch. 6 & 7) Assessment
Name: __________________________________
Period: ____
Date: ___/___/___
ASSESSMENT OVERVIEW
Section 1: Key Terms – Match the definition of the key term to the correct definition.
Section 2: Knowledge of Content – Choose the most correct response to best answer the question (multiple
choice)
Section 3: Application of Content & Skill Mastery
• Compounds, Molecules & Bonding (Ch. 6)
• Chemical Reactions (Ch. 7-Sections 1 & 2)
• Types of Reactions (Ch. 7-Section 3)
• Rates of Reactions (Ch. 7-Section 4)
The following questions are meant to review your knowledge of the concepts and skills throughout the unit.
It is NOT an exhaustive review, meaning that beyond completion of the review, study of notes, practice, and
HW prior to the assessment will best prepare you for success.
Review Part 1: Key Terms-Use your notes and textbook to define the following key terms.
chemical bonds
chemical structure
compound
molecule
covalent bond
metallic bond
polyatomic ion
chemical formula
product
chemical equation
exothermic reaction endothermic reaction
synthesis reaction
decomposition reaction
combustion reaction
single-displacement reaction
double-displacement reaction
oxidation-reduction reaction
rate of reaction
collision theory
1.
2.
3.
4.
5.
6.
7.
ionic bond
reactant
How and why do atoms form chemical bonds?
When do chemical reactions take place?
What is a chemical equation?
What can a balanced equation tell you?
What is the role of energy in chemical reactions?
How does learning about reaction types help in understanding chemical reactions?
What kinds of things speed up a chemical reaction?
Review Part 3: Application of Content & Skill Mastery
1. Compare ionic and covalent compounds.
Ionic Compounds
Structure?
What happens to the valence
electrons during bonding?
Electrical conductivity?
State at room temperature?
Melting and boiling points?
Covalent Compounds
2. Explain why silver iodide, AgI, a compound used in photography, has a much higher melting point than
vanillin, C8H8O3, a sweet-smelling compound used in flavorings.
3. The periodic table can be divided into metals and nonmetals. Complete the following:
Metallic bonds form between ___________________ and __________________.
Ionic bonds form between ___________________ and __________________.
Covalent bonds form between ___________________ and __________________.
4. Determine if the following are likely to have ionic or covalent bonds. Explain.
a. strontium oxide, SrO
b. magnesium chloride, MgCl2
c. fluorine gas, F2
d. propanol, C3H7OH
5. Which of the following will conduct an electric current. Explain.
a. copper wiring
b. sugar, C12H22O11
c. potassium chloride, KCl, dissolved in water
6. Identify the products and reactants in the following word equation.
Isooctane and oxygen burn to form carbon dioxide and water.
7. Explain where the energy to cook food comes from when a gas stove burns natural gas, CH4, and oxygen, O2.
8. Describe three signs that a chemical reaction has taken place and give an example of each sign.
9. How does the energy of the reactants and products differ in an endothermic reaction? ...in an exothermic
reaction?
10. How can products and reactants have different amounts of energy without violating the law of conservation of
energy?
11. Why do we balance chemical equations? When is a chemical equation balanced?
12. How many atoms of each element are in the following compounds:
a. NaC2H3O2
b. (NH4)3PO4
c. 3H2O2
d. 2Ca3(PO4)2
13. Write balanced equations for the following:
a. N2 + H2 à NH3
b. KOH + HCl à KCl + H2O
c. Pb(NO3)2 + KI à KNO3 + PbI2
14. How are decomposition reactions related to synthesis reactions? Give an example of each to explain this.
15. How does a single displacement reaction differ from a double displacement reaction? Give an example of
each to explain this.
16. What are the products of a combustion reaction?
17. How does oxidation differ from reduction?
18. Classify the following types of reactions:
a. S8 + O2 à 8O2
b. 6Li + N2 à 2Li3N
c. AgNO3 + KBr à AgBr + KNO3
d. CaCO3 à CaO + CO2
e. Mg + Pb(NO3)2 à Pb + Mg(NO3)2
19. Describe three ways in which the rate of a reaction can be slowed down. Give an example of each.