Download CHM121 Exam I Review

California State Polytechnic University, Pomona
General Chemistry, CHM 121, Dr. Laurie S. Starkey
Exam I Review, Chapters 1–3
General Topics: significant figures, scientific notation, SI base unit & prefix, density, conversion
factors, periodic table (periods/groups), chemical formula, balancing equations, nomenclature,
molecular/formula weight, percent composition (mass percent), stoichiometry.
Be able to define the following terms: states of matter, element, compound, ionic vs. molecular
compounds, atom, atomic symbol, nucleus, electron, proton, atomic number, neutron, mass number,
nuclide, isotopes, atomic weight, metal, nonmetal, metalloid, ion, cation, anion, chemical reaction,
reactant, product, mole, Avogadro's number, empirical formula, limiting reactant/reagent, theoretical
yield, percent yield.
1. Complete the following conversion factors: 1 m = ______ cm
1 mL = _______ L
1 L = _______ mL
1 g = _______ kg
1 kg = _______ g
1. What is the mass number of carbon-13? What is the nuclide symbol for carbon-13?
2. How many neutrons does iodine-131 (131I) have?
3. How many electrons are in each of the following atoms?
Mn __________
Br–__________
potassium ion __________
Fe2+__________
copper (III) __________
4. What is the charge of the nucleus of a calcium atom? of a calcium ion?
5. What is the weight of a 165 pound person in grams? (1 lb = 0.4536 kg)
6. A procedure calls for 6.5 g thionyl chloride (SOCl2). SOCl2 is a liquid so you want to measure it
using a syringe. Its density is 1.631, according to an Aldrich catalog. How many mL are
required?
7. How many chlorine atoms are in 6.5 g thionyl chloride (SOCl2)?
8. What are the formulas for the following anions: nitrite? nitride? nitrate?
9. Which name is correct for Ca3(PO4)2? Explain what is wrong with each incorrect name.
a. calcium (II) phosphate
b. calcium (III) phosphate
c. tricalcium diphosphate
d. calcium (II) phosphite
e. calcium phosphite
f. calcium phosphate
10. The combustion of a 1.50 g sample yields 1.17 g H2O. What is the mass % of H in the sample?
11. What is the mass percent of carbon in the fuel octane (C8H18)?
12. Balance the following equation. When 5.00 g of Sn were combined with 5.00 g HNO3, an 82%
yield of SnO2 was obtained. How much SnO2 (in grams) was produced in that reaction?
_____Sn + _____HNO3
13. Fill in the missing blanks.
→
_____SnO2 + _____NO2
+ _____H2O
nuclide symbol
44
20
# of protons
# of electrons
# of neutrons
Ca2+
14. Provide the molecular formula and empirical formula for each of the following.
H
O
H
H
C
C
H
H
O
H
H
H
H
H
C
C
C
H
H
H
H
H
H
H
C
C
H
H
C
C
H
H
H
mol. form. _________
mol. form. _________
mol. form. _________
emp. form._________
emp. form._________
emp. form._________
15. Name or give formulas for each of the following compounds.
Formula
Name
Name
Formula
Zn3(PO4)2
______________________________
potassium sulfate
____________
NH4OH
______________________________
sulfuric acid
____________
calcium carbonate
____________
16. A compound contains 1.36 mol Li, 2.72 mol B and 4.76 mol O. What is its empirical formula?
17. Balance the following equation for the combustion of propane (BBQ fuel).
_____C3H6
+
_____O2
→
_____H2O
+ _____CO2
a. If 0.50 moles of each starting material were combined, what is the theoretical yield of carbon
dioxide (in grams)?
b. How many grams of oxygen are required to burn 20 pounds of propane (one tankful).
(1 kg = 2.2 lbs.)