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Chemistry Final
Review Topics
Chapter 1
Chemistry, theory, law,
Chapter 2
Mass, volume, mixture, compound, atom, element, period, group, reactant, product,
Chapter 3
Scientific notation, significant figures, milli, centi, kilo, density, weight, conversion factors
Chapter 4
Proton, neutron, electron, nucleus, atomic number, mass number, isotopes, atomic mass, amu,
Chapter 5
Electron configurations,
Chapter 6
Metals, nonmetals, metalloids, alkali metals, alkaline earth metals, transition metals, halogens, noble gases, electronegativity,
Chapter 7
Valence electrons, octet rule, ions (cation, anion), chemical formula, ionic bond,
Chapter 8
Molecule, covalent bond, polyatomic ions (use yellow periodic table),
Chapter 9
Writing formulas, naming compounds, balancing charges,
Chapter 10
The mole, Avogadro’s Number, molar mass, converting grams to moles (& mol to grams), % composition,
Chapter 11
Reactants, products, catalysts, skeleton equations, balancing chemical equations, coefficients, 5 rxn types (combination,
decomposition, single and double replacement, combustion), aqueous (aq), precipitate,
Chapter 12
Stoichiometry, mole ratios, limiting and excess reagents, yield (actual, theoretical, percent),
Chapter 19
Acids, bases, hydrogen and hydroxide ions, pH scale, titrations, neutralization rxns
Chapter 20
Oxidation and reduction, LEO the lion says GER, oxidation numbers,
Chemistry Final
Review Questions
1. Define the following terms, also write the unit that the quantity is normally measured in.
a. volume
b. mass
c. weight
d. density
2. Define the following terms and explain how the number of each is determined for an atom.
a. proton
b. electron
c. neutron
d. mass number
e. atomic number
3. Define the following terms and give an example of each
a. atoms
b. compound
c. ion
d. isotope
e. molecule
f. formula unit
g. mixture
4. Explain the difference between an ionic and a covalent bond
5. How can you determine if an element is a metal, nonmetal or metalloid
6. Draw a box around the significant digits in each measurement.
a. 5.01 g
d. 0.00450 L
g. 100.0 g
b. 0.34 g
e. 10.0 cm
h. 0.0100 mL
c. 0.00809 mL
f. 100 kg
i. 30.01 mm
7. Write the correct chemical formula for the following compounds
a. sodium fluoride
d. magnesium nitrate
g. sodium sulfate
b. potassium nitrate
e. copper(II) chloride
h. calcium chloride
c. carbon dioxide
f. aluminum sulfate
i. lithium iodide
8. Write the correct chemical name for each of the following compounds
a. KCl
d. N2O5
b. Sr(NO3)2
e. AlPO4
h. NH4NO3
c. Fe(NO3)2
f. NaIO3
i. CuSO4
g. PCl5
9. Calculate the molar mass of the compounds in problem 8 part a-d.
a. KCl
c. Fe(NO3)2
b. Sr(NO3)2
d. N2O5
10. Convert the following (use question #9 for the molar masses)
a. 10.5 grams of KCl to moles
c. 0.25 mol Sr(NO3)2 to grams
b. 0.58 grams of KCl to moles
d. 1.20 mol N2O5 to grams
11. Balance the following chemical equations; what is the name for the number that is placed in front of a chemical formula?
a.
Na +
b.
Al
H 2O CuCl2 +
NaOH +
H2
AlCl3
Cu
CaCO3 c.
MgCl2
+
d.
N2 +
H2 +
MgCO3
+
CaCl2
NH3
12. Calculate the percent composition of oxygen in the following compounds
a. H2SO4
b. K3PO4
13. The equation Mg(s)
14. The reaction 2Fe
2HCl(aq)
3Cl
MgCl (aq)
H (g) is an example of which type of reaction?
2FeCl is an example of which type of reaction?
15. Write a balanced equation representing the decomposition of lead(IV) oxide.
16. When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. Write a balanced
chemical equation for this reaction.
17. What are valence electrons?
18. Write the number of valance electrons in each atom.
a. Li
b. Mg
c. Al
d. C
e. N
f. O
g. Br
h. Ne
g. Br
h. Ne
19. Which of the atoms in question 18 has the highest electronegativity value? What is electronegativity?
20. Write the most common ion charge that each atom in question 18 will form.
a. Li
b. Mg
c. Al
d. C
e. N
f. O
21. Use the reaction, 2CO(g) + O2 (g) → 2CO2 (g) to answer the questions below.
a. What is the mole ratio of O2 to CO2?
b. What is the mole ratio of CO to CO2?
c. How many moles of CO2 would be formed by the complete reaction of 2 mol of CO?
d. How many moles of O2 would be required to form 4 mol CO2? Assume excess CO.
e. If 2 mol of CO reacted with 2 mol of O2, which would be the excess reactant?
f. How many moles of CO2 would be formed from the reaction in part e?
g. How many moles of CO2 would be produced from 2.4 mol of CO reacting with excess O2?
22. Aluminum reacts with sulfuric acid (H2SO4) to produce aluminum sulfate and hydrogen gas.
a. Write a balanced chemical equation for this reaction.
b. How many grams of Al2(SO4)3 would be formed if 250 g H2SO4 completely reacted with aluminum?
c. If the percent yield of the reaction in part b was 87.2%, what was the actual yield?
d. How much aluminum would be required to produce 10.56 grams of Al2(SO4)3?