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AP Chemistry 2 Midterm Study Guide #3



Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 

A physical change occurs when a
A)
peach spoils.
C)
bracelet turns your wrist green.
B)
copper bowl tarnishes.
D)
glue gun melts a glue stick.
 

 2. 

The base unit for mass is the
A)
gram.
C)
meter.
B)
cubic centimeter.
D)
kilogram.
 

 3. 

Which of the following is an extensive property of matter?
A)
melting point
C)
volume
B)
boiling point
D)
density
 

 4. 

Which of the following is not a physical change?
A)
grinding
C)
boiling
B)
cutting
D)
burning
 

 5. 

The symbols for units of length in order from largest to smallest are
A)
m, cm, mm, km.
C)
km, mm, cm, m.
B)
mm, m, cm, km.
D)
km, m, cm, mm.
 

 6. 

What is the density of 37.72 g of material whose volume is 6.80 cm3?
A)
0.180 g/cm3
C)
30.9 g/cm3
B)
5.55 g/cm3
D)
256. g/cm3
 

 7. 

Which of these measurements has been expressed to three significant figures?
A)
0.052 g
C)
3.065 g
B)
0.202 g
D)
500 g
 

 8. 

How is the measurement 0.000 065 cm written in scientific notation?
A)
65 × 10–6 cm
C)
6.5 × 10–6 cm
B)
6.5 × 10–5 cm
D)
6.5 × 10–4 cm
 

 9. 

When 1.92 × 10–6 kg is divided by 6.8 × 102 mL, the quotient equals
A)
2.8 × 10–4 kg/mL.
C)
2.8 × 10–8 kg/mL.
B)
2.8 × 10–5 kg/mL.
D)
2.8 × 10–9 kg/mL.
 

 10. 

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
A)
13.
C)
27.
B)
14.
D)
40.
 

 11. 

Neon-22 contains 12 neutrons. It also contains
A)
12 protons.
C)
22 electrons.
B)
22 protons.
D)
10 protons.
 

 12. 

How many moles of atoms are in 50.15 g of mercury (atomic mass 200.59 amu)?
A)
0.1001 mol
C)
0.2500 mol
B)
0.1504 mol
D)
0.4000 mol
 

 13. 

The speed of an electromagnetic wave is equal to the product of its wavelength and its
A)
mass.
C)
velocity.
B)
color.
D)
frequency.
 

 14. 

What values can the angular momentum quantum number have when n = 2?
A)
mc014-1.jpg
C)
0, 1, 2
B)
mc014-2.jpg
D)
0, 1
 

 15. 

The p orbitals are shaped like
A)
electrons.
C)
dumbbells.
B)
circles.
D)
spheres.
 

 16. 

The statement that an electron occupies the lowest available energy orbital is
A)
Hund's rule.
C)
Bohr's law.
B)
the Aufbau principle.
D)
the Pauli exclusion principle.
 

 17. 

Two electrons in the 1s orbital must have different spin quantum numbers to satisfy
A)
quantum rule.
C)
the Pauli exclusion principle.
B)
the magnetic rule.
D)
the Aufbau principle.
 

 18. 

The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
A)
Mg (Z = 12).
C)
S (Z = 16).
B)
C (Z = 6).
D)
Si (Z = 14).
 

 19. 

What is the electron configuration for nitrogen, atomic number 7?
A)
1s2 2s2 2p3
C)
1s2 2s3 2p1
B)
1s2 2s3 2p2
D)
1s2 2s2 2p2 3s1
 

 20. 

The electron notation for aluminum (atomic number 13) is
A)
1s2 2s2 2p3 3s2 3p3 3d1.
C)
1s2 2s2 2p6 3s2 3p1.
B)
1s2 2s2 2p6 3s2 2d1.
D)
1s2 2s2 2p9.
 

 21. 

The energy required to remove an electron from an atom is the atom's
A)
electron affinity.
C)
electronegativity.
B)
electron energy.
D)
ionization energy.
 

 22. 

The element that has the greatest electronegativity is
A)
oxygen.
C)
chlorine.
B)
sodium.
D)
fluorine.
 

 23. 

In a row in the periodic table, as the atomic number increases, the atomic radius generally
A)
decreases.
C)
increases.
B)
remains constant.
D)
becomes immeasurable.
 

 24. 

Within a group of elements, as the atomic number increases, the atomic radius
A)
increases.
C)
decreases regularly.
B)
remains approximately constant.
D)
varies unpredictably.
 

 25. 

To draw a Lewis structure, one must know the
A)
number of valence electrons in each atom.
C)
bond length of each atom.
B)
atomic mass of each atom.
D)
ionization energy of each atom.
 

 26. 

According to VSEPR theory, the shape of an AB3 molecule is
A)
trigonal-planar.
C)
linear.
B)
tetrahedral.
D)
bent.
 

 27. 

According to VSEPR theory, the structure of the ammonia molecule, NH3, is
A)
trigonal-planar.
C)
trigonal-pyramidal.
B)
bent.
D)
tetrahedral.
 

 28. 

Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.
A)
tetrahedral
C)
bent
B)
linear
D)
trigonal-planar
 

 29. 

The hybridized orbitals responsible for the bent shape of the water molecule are
A)
1s2 2s2.
C)
sp3.
B)
ps1.
D)
2s2 sp2.
 

 30. 

What is the formula for zinc fluoride?
A)
ZnF
C)
Zn2F
B)
ZnF2
D)
Zn2F3
 

 31. 

Name the compound SO3.
A)
sulfur trioxide
C)
selenium trioxide
B)
silver trioxide
D)
sodium trioxide
 

 32. 

What is the oxidation number of hydrogen in KH?
A)
–1
C)
+1
B)
0
D)
+2
 

 33. 

What is the oxidation number of sulfur in H2SO4?
A)
–2
C)
+4
B)
0
D)
+6
 

 34. 

What is the formula mass of (NH4)2SO4?
A)
114.09 amu
C)
128.06 amu
B)
118.34 amu
D)
132.16 amu
 

 35. 

How many oxygen atoms are there in 0.500 mol of CO2?
A)
6.02 mc035-2.jpg 1023
C)
15.9994
B)
3.01 mc035-3.jpg 1023
D)
11.0
 

 36. 

What is the percentage composition of CF4?
A)
20% C, 80% F
C)
16.8% C, 83.2% F
B)
13.6% C, 86.4% F
D)
81% C, 19% F
 

 37. 

What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen?
A)
KClO2
C)
K2Cl2O3
B)
KClO3
D)
K2Cl2O5
 

 38. 

A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?
A)
N2O5
C)
NO3
B)
N4O10
D)
N2O4
 

 39. 

The complete balanced equation for the reaction between zinc hydroxide and acetic acid is
A)
ZnOH + CH3COOH ZnCH3COO + H2O.
B)
Zn(OH)2 + CH3COOH Zn + 2CO2 +3H2O.
C)
Zn(OH)2 + 2CH3COOH Zn(CH3COO)2 + 2H2O.
D)
Zn(OH)2 + 2CH3COOH Zn(CH3COO)2 + H2 + O2.
 

 40. 

The equation A + X AX is the general equation for a(n)
A)
combustion reaction.
C)
synthesis reaction.
B)
ionic reaction.
D)
double-displacement reaction.
 

 41. 

Oxides of active metals, such as CaO, react with water to produce
A)
metal carbonates.
C)
acids.
B)
metal hydrides.
D)
metal hydroxides.
 

 42. 

When a metal chlorate is heated, it decomposes to yield a metal chloride and
A)
a metal oxide.
C)
hydrogen.
B)
a metal hydroxide.
D)
oxygen.
 

 43. 

Predict the product of the reaction represented by the following equation:
MgO + CO2
A)
MgCO3
C)
MgC + O3
B)
Mg + CO3
D)
MgCO2 + O
 

 44. 

What is the balanced equation when aluminum reacts with copper(II) sulfate?
A)
Al + Cu2S Al2S + Cu
B)
2Al + 3CuSO4 Al2(SO4)3 + 3Cu
C)
Al + CuSO4 AlSO4 + Cu
D)
2Al + Cu2SO4 Al2SO4 + 2Cu
 

 45. 

In the equation 2KClO3 2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely?
A)
1.0 mol
C)
3.0 mol
B)
2.5 mol
D)
4.5 mol
 

 46. 

For the reaction represented by the equation CH4 + 2O2 CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 100. g of methane?
A)
6.23 mol
C)
12.5 mol
B)
10.8 mol
D)
25 mol
 

 47. 

For the reaction represented by the equation SO3 + H2O H2SO4, how many grams of sulfuric acid can be produced from 200. g of sulfur trioxide and 100. g of water?
A)
100. g
C)
245 g
B)
200. g
D)
285 g
 

 48. 

If the percentage yield is equal to 100%, then
A)
the actual yield is greater than the theoretical yield.
C)
the actual yield is less than the theoretical yield.
B)
the actual yield is equal to the theoretical yield.
D)
there was no limiting reactant.
 

 49. 

For the reaction represented by the equation SO3 + H2O H2SO4, calculate the percentage yield if 500. g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid.
A)
82.7%
C)
91.2%
B)
88.3%
D)
93.9%
 

 50. 

The replacement of bromine by chlorine in a salt is an example of a single-displacement reaction by
A)
halogens.
C)
water.
B)
sodium.
D)
electrolysis.
 



 
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