Download South Pasadena · AP Chemistry

Station 1 
Chapter 1 (Matter) & 2 (Measurements)
1. a. What is the density of an 84.7 g sample of an unknown substance if
the sample occupies 4906 mL?
b. What volume would be occupied by 7.75 g of the same substance?
2. How many significant figures are there in each of the following
measured values?
a. 6.002 cm
b. 0.0020 m
c. 10.0500 g
d. 7000 kg
e. 7000. kg
3. Round 2.6765 to two significant figures.
4. Write the following numbers in scientific notation.
a. 560000
b. 33400
c. 0.0004120
8. A student measures the mass of a beaker filled with corn oil. The mass
reading averages 215.6 g. The mass of the beaker is 110.4 g.
a. What is the mass of the corn oil?
b. What is the density of the corn oil if its volume is 114cm3?
Station 2 
Chapter 3 (Atoms)
1. Describe one conclusion made by each of the following scientists that
led to the development of the current atomic theory:
a. Thomson
b. Rutherford
c. Bohr
2. Compare and contrast the three types of subatomic particles in terms
of location in the atom, mass, and relative charge.
3. Define each of the following:
a. atomic number
b. mass number
d. average atomic mass e. mole
g. molar mass
h. isotope
c. ion
f. Avogadro’s number
4. Determine the number of protons, electrons, and neutrons in each of
the following isotopes:
a. sodium – 23
b. calcium – 40
c. Cu
d. Ag
5. Write the nuclear symbol (chemical configuration) and hyphen notation
for each of the following isotopes:
a. mass number of 28 and atomic number of 14
b. 26 protons and 30 neutrons
c. 56 electrons and 82 neutrons
Station 3___________________________________________
1. Complete the table below:
Number of
valence e
H2O
CO2
BF3
SiF4
Lewis Diagram
Molecular Geometry
Molecular Polarity
Station 4 
 Chapter 4(Electrons in Atoms)&5(Periodic Law)
1. What is the octet rule?
2. Write the noble-gas notation, electron dot diagram, quantum numbers,
and the orbital notation for the following elements:
a. carbon
b. neon
c. sulfur
3. Identify the elements having the following electron configurations:
a. 1s22s22p63s23p3
b. [Ar]4s1
c. contains four electrons in its third and outer main energy level
d. contains one set of paired and three unpaired electrons in its
fourth and outer main energy level
4. Distinguish between the ground state and an excited state of an atom.
5. Who established atomic numbers as the basis for organizing the
periodic table?
6. State the general period and group trends among main group
elements with respect to each of the following properties:
a. atomic radii
b. first ionization energy
c. electronegativity
7. Circle the atom with the LARGER radius.
a. Na Cl
b. Ne Xe
8. Circle the atom with the HIGHER first ionization energy.
a. Li Cs
b. Ba As
Station 5 
Chapter 7 (Formulas and Compounds)& Light
1.
a.
b.
c.
d.
e.
f.
g.
h.
Write formulas for the compounds formed between the following:
aluminum and bromine
sodium and oxygen
magnesium and iodine
Pb2+ and O2Sn2+ and IFe3+ and S2Cu2+ and NO3NH4+ and SO42-
2. Name the following compounds:
a. P2O4
b. MgS
c. CO
3.
a.
b.
c.
d.
e.
f.
g.
h.
d. K2S
e. CuBr
f. FeCl2
Write formulas for each of the following compounds:
barium sulfide
sodium hydroxide
lead(II) nitrate
potassium permanganate
iron(II) sulfate
diphosphorous trioxide
disulfur dichloride
carbon diselenide
4. What is the energy of a quantum of light with a frequency of 4.31 X 1014 sec-1 or Hz?
5. A certain violet light has a wavelength of 413 X 10-9 m. What is the frequency of the light?
6.
7.
239
93Np
→
239 Pu
94
226
88Ra
→
4
2He
+ _____
+ ____
Station 6
Chapter 7 (Formulas and Compounds)
1. Determine the percentage by mass of water in the hydrate CuSO 4·5H2O.
2. What is the mass in grams of each of the following samples?
a. 1.000 mol NaCl
b. 2.000 mol H2O
c. 3.500 mol Ca(OH)2
d. 0.625 mol Ba(NO3)2
3. How many molecules of aspirin, C9H8O4, are there in a 100.0mg tablet of asprin?
i.
Calculate the percentage composition of (NH4)2CO3.
Station 7
Chapter 7 (Formulas and Compounds)
1. A compound is found to contain 36.48% Na, 25.41% S, and 38.11% O. Find its empirical
formula.
2. Find the empirical formula of a compound that contains 53.70% iron and 46.30% sulfur.
3. Analysis of a compound indicates that it contains 1.04g K, 0.70 g Cr, and 0.86 g O. Find its
empirical formula.
4. If 4.04 g of N combine with 11.46 g O to produce a compound with a formula mass of 108.0
amu, what is the molecular formula of this compound?
5. The molar mass of a compound is 93 g/mol. Analysis of a sample of the compound
indicates that it contains 0.606 g N and 1.390 g O. Find its molecular formula.
6. Write the quantum numbers, orbital notation, and e- configuration for oxygen.
7. Calculate the average atomic mass for copper if there are two naturally occurring isotopes:
Cu-63 with a mass of 62.9296 amu (69.17%) and Cu-65 with a mass of 64.9278 amu