Name: 
 

AP Chemistry Midterm Study Guide #2



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

 1. 

0.25 g is equivalent to
a.
250 kg.
c.
0.025 mg.
b.
250 mg.
d.
0.025 kg.
 

 2. 

The number of significant figures in the measurement 0.000 305 kg is
a.
2.
c.
6.
b.
3.
d.
7.
 

 3. 

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
 

 4. 

When 64.4 is divided by 2.00, the correct number of significant figures in the result is
a.
1.
c.
4.
b.
3.
d.
6.
 

 5. 

The dimensions of a rectangular solid are measured to be 1.27 cm, 1.3 cm, and 2.5 cm. The volume should be recorded as
a.
4.128 cm3.
c.
4.13 cm3.
b.
4.12 cm3.
d.
4.1 cm3.
 

 6. 

A compound is
a.
a pure substance that cannot be broken down into simpler, stable substances.
b.
a substance, made of two or more atoms that are chemically bonded, that can be broken down into simpler, stable substances.
c.
the smallest unit of matter that maintains its chemical identity.
d.
any substance, whether it is chemically bonded or not.
 

 7. 

Which of the following is not a physical change?
a.
grinding
c.
boiling
b.
cutting
d.
burning
 

 8. 

Which of the following is not a chemical change?
a.
rusting
c.
melting
b.
igniting
d.
burning
 

 9. 

A mixture is
a.
a combination of pure substances bonded chemically.
b.
any substance with a uniform composition.
c.
a blend of any two or more kinds of matter, as long as each maintains its own unique properties.
d.
any group of elements that are chemically bonded to one another.
 

 10. 

If a mixture is uniform in composition, it is said to be
a.
homogeneous.
c.
heterogeneous.
b.
chemically bonded.
d.
a compound.
 

 11. 

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a.
13.
c.
27.
b.
14.
d.
40.
 

 12. 

Chlorine has atomic number 17 and mass number 35. It has
a.
17 protons, 17 electrons, and 18 neutrons.
b.
35 protons, 35 electrons, and 17 neutrons.
c.
17 protons, 17 electrons, and 52 neutrons.
d.
18 protons, 18 electrons, and 17 neutrons.
 

 13. 

Phosphorus-33 (atomic number 15) contains
a.
33 protons.
c.
33 neutrons.
b.
18 neutrons.
d.
18 protons.
 

 14. 

Neon-22 contains 12 neutrons. It also contains
a.
12 protons.
c.
22 electrons.
b.
22 protons.
d.
10 protons.
 

 15. 

An element consists of two isotopes. The abundance of one isotope is 95.72% and its atomic mass is 114.9041 u. The atomic mass of the second isotope is 112.9043 u. What is the average atomic mass of the element?
a.
113.9 u
b.
113.0 u
c.
113.9 u
d.
114.8 u
e.
115.1 u
 

 16. 

Which of the following is a correct Lewis structure for the phosphate ion?

mc016-1.jpg
a.
1
b.
2
c.
3
d.
4
e.
5
 

 17. 

The central atom in IF2- is surrounded by
a.
no single bonds, 2 double bonds, and no lone pairs of electrons.
b.
no single bonds, 2 double bonds, and 2 lone pairs of electrons.
c.
1 single bond, 1 double bond, and 1 lone pair of electrons.
d.
2 single bonds, no double bonds, and 2 lone pairs of electrons.
e.
2 single bonds, no double bonds, and 3 lone pairs of electrons.
 

 18. 

Which of the following species will have a Lewis structure most like that of SF4?
a.
XeF4
b.
SO42-
c.
ICl4+
d.
PF4+
e.
IO4-
 

 19. 

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of the nitrite ion, NO2-.
a.
The electron-pair geometry is linear, the molecular geometry is linear.
b.
The electron-pair geometry is trigonal-planar, the molecular geometry is bent.
c.
The electron-pair geometry is trigonal-planar, the molecular geometry is linear.
d.
The electron-pair geometry is tetrahedral, the molecular geometry is bent.
e.
The electron-pair geometry is tetrahedral, the molecular geometry is linear.
 

 20. 

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of iodine trichloride, ICl3.
a.
The e--pair geometry is trigonal-planar, the molecular geometry is trigonal-planar.
b.
The e--pair geometry is tetrahedral, the molecular geometry is trigonal-pyramidal.
c.
The e--pair geometry is tetrahedral, the molecular geometry is trigonal-planar.
d.
The e--pair geometry is trigonal-bipyramidal, the molecular geometry is T-shaped.
e.
The e--pair geometry is trigonal-bipyramidal, the molecular geometry is trigonal-planar.
 

 21. 

Which of the following formulas is not correct?
a.
Al2(SO4)3
b.
NaClO3
c.
Ba2O3
d.
Mg(NO3)2
e.
KH2PO4
 

 22. 

What is the correct formula for an ionic compound that contains aluminum ions and carbonate ions?
a.
AlCO3
b.
Al(CO3)2
c.
Al(CO3)3
d.
Al2(CO3)3
e.
Al3(CO3)2
 

 23. 

What is the correct formula for sodium acetate?
a.
Na2CH3O
b.
NaCH3CO2
c.
NaCH3O
d.
NaCH2O2
e.
NaCHO
 

 24. 

What is the correct formula for barium nitrate?
a.
Ba(NO3)2
b.
BNO2
c.
Ba(NO2)2
d.
BaN
e.
BaNO3
 

 25. 

All of the following are named correctly EXCEPT
a.
LiClO4; lithium perchlorate.
b.
CaHPO4; calcium hydrogen phosphide.
c.
NaCN; sodium cyanide.
d.
Mg(OH)2; magnesium hydroxide.
e.
CaSO3; calcium sulfite.
 

 26. 

Ammonia is prepared by reacting nitrogen and hydrogen gases at high temperature according to the unbalanced chemical equation below.

__ N2(g) + __ H2(g) ® __ NH3(g)

What are the respective coefficients when the equation is balanced with the smallest whole numbers?
a.
1, 1, 1
b.
1, 3, 1
c.
1, 3, 2
d.
2, 1, 2
e.
2, 3, 2
 

 27. 

If aqueous solutions of copper(II) nitrate and sodium carbonate are mixed, which insoluble compound will form?
a.
CuCO3
b.
Cu(NO3)2
c.
NaNO3
d.
Na2Cu
e.
Na2CO3
 

 28. 

What reaction occurs when aqueous solutions of sodium hydroxide and copper(II) bromide are mixed?
a.
Na+(aq) + OH-(aq) + Cu2+(aq) + 2Br-(aq) ® NaCu(s) + Br2OH(aq)
b.
Na+(aq) + OH-(aq) + CuBr2(s) ® NaBr2(aq) + CuOH(s)
c.
Na+(aq) + Br-(aq) ® NaBr(s)
d.
2Na+(aq) + Br2(aq) ® 2NaBr(s)
e.
2OH-(aq) + Cu2+(aq) ® Cu(OH)2(s)
 

 29. 

What net ionic reaction occurs when aqueous solutions of potassium carbonate and iron(III) bromide are mixed?
a.
CO32-(aq) + 2Fe+(aq) ® Fe2(CO3)(s)
b.
3CO32-(aq) + 2Fe3+(aq) ® Fe2(CO3)3(s)
c.
3CO32-(aq) + 6Fe+(aq) ® 3Fe2CO3(s)
d.
3K2CO3(aq) + 2Fe3+(aq) + 6Br-(aq) ® Fe2(CO3)3(s) + 6KBr(s)
e.
no reaction occurs
 

 30. 

Write a balanced net ionic equation for the reaction of aqueous solutions of lead(II) nitrate and potassium chloride.
a.
Pb(NO3)2(aq) + 2KCl(aq) ® PbCl2(s) + 2KNO3(aq)
b.
Pb2+(aq) + 2K+(aq) ® PbK2(s)
c.
Pb2+(aq) + 2Cl-(aq) ® PbCl2(s)
d.
NO3-(aq) + K+(aq) ® KNO3(s)
e.
no precipitation occurs.
 

 31. 

What is the mass in grams of 0.338 mol of glucose (C6H12O6)?
a.
0.00188 g
b.
0.0164 g
c.
1.88 g
d.
53.3 g
e.
60.9 g
 

 32. 

Which is a correct method for calculating the moles present in 132 grams of calcium carbonate?
a.
mc032-1.jpg
b.
mc032-2.jpg
c.
mc032-3.jpg
d.
mc032-4.jpg
e.
none of the above
 

 33. 

What is the percent composition of silicon nitride (Si3N4)?
a.
30.21% Si and 69.79% N
b.
42.92% Si and 57.08% N
c.
54.03% Si and 45.97% N
d.
60.06% Si and 39.94% N
e.
69.40% Si and 30.60% N
 

 34. 

What is the percent composition of iron(II) sulfate hexahydrate?
a.
4.2% Fe; 4.2% S; 41.6% O; 50.0% H
b.
16.7% Fe; 16.7%S; 66.6% O
c.
21.5% Fe; 12.3%S; 24.6% O; 41.6% H
d.
21.5% Fe; 12.3%S; 61.5% O; 4.7% H
e.
36.8% Fe; 21.1%S; 42.1% O
 

 35. 

Chalcopyrite is a mineral which contains 34.62% Cu, 30.43% Fe, and 34.95% S. What is the chemical formula for chalcopyrite?
a.
CuFeS
b.
CuFeS2
c.
CuFe2S
d.
Cu2FeS
e.
Cu2FeS2
 

 36. 

An oxide of nitrogen contains 63.1% oxygen and has a molar mass of 76.0 g/mol. What is the molecular formula for this compound?
a.
N2O
b.
NO
c.
NO2
d.
N2O3
e.
N2O5
 

 37. 

If 16.4 g of oxygen gas react with excess hydrogen, what mass of water is produced?

2H2(g) + O2(g) mc037-1.jpg 2H2O(g)
a.
9.23 g
b.
18.5 g
c.
20.4 g
d.
23.9 g
e.
36.9 g
 

 38. 

Which method is correct for determining the mass of carbon dioxide that can be made by the combustion of 3.219 grams of ethanol with excess oxygen?

C2H5OH(l) + 3O2(g) ® 2CO2(g) + 3H2O(l)
a.
mc038-1.jpg
b.
mc038-2.jpg
c.
mc038-3.jpg
d.
mc038-4.jpg
e.
mc038-5.jpg
 

 39. 

Sodium metal and water react to form sodium hydroxide and hydrogen gas. What mass of Na will react with excess water to produce 15 g NaOH?

2Na(s) + 2H2O(l) ® H2(g) + 2NaOH(aq)
a.
4.3 g
b.
5.4 g
c.
8.6 g
d.
11 g
e.
26 g
 

 40. 

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
 

 41. 

Which of the following does not increase the rate of dissolving a solid in water?
a.
raising the temperature of the water
b.
stirring the solution
c.
using larger pieces of solid
d.
crushing the solid
 

 42. 

What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution?
a.
0.0132 M
c.
0.459 M
b.
0.0253 M
d.
1.363 M
 

 43. 

What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution? (molar mass of NaCl = 58.44 g/mol)
a.
0.535 M
c.
8.56 M
b.
2.14 M
d.
31.3 M
 

 44. 

What is the mass of solute in 225 mL of 5.91 ´ 10-2 M KIO3?
a.
0.0133 g
b.
0.0562 g
c.
0.263 g
d.
1.51 g
e.
2.85 g
 

 45. 

If 5.00 mL of 0.314 M KOH is diluted to exactly 125 mL with water, what is the concentration of the resulting solution?
a.
5.02 ´ 10-4 M
b.
1.26 ´ 10-2 M
c.
0.127 M
d.
0.281 M
e.
7.85 M
 

 46. 

For a neutron (mass = 1.675 ´ 10-27 kg) moving with a velocity of 5.2 ´ 103 m/s, what is the de Broglie wavelength?
a.
7.6 ´ 10-11 m
b.
4.5 ´ 10-9 m
c.
2.1 ´ 10-6 m
d.
486 m
e.
1.3 ´ 1010 m
 

 47. 

What type of orbital is designated n = 4, l = 3, ml = -3?
a.
4s
b.
4p
c.
4d
d.
4f
e.
none
 

 48. 

All of the following sets of quantum numbers are allowed EXCEPT
a.
n = 5, l = 3, ml = +2
b.
n = 3, l = 2, ml = -1
c.
n = 3, l = 0, ml = 0
d.
n = 4, l = 4, ml = -2
e.
n = 5, l = 3, ml = +3
 

 49. 

Which element has the following electron configuration?

mc049-1.jpg
a.
P
b.
S
c.
O
d.
N
e.
F
 

 50. 

Place the following atoms in order of increasing atomic radii: Ca, Mg, P, and Cl.
a.
Cl < P < Mg < Ca
b.
Mg < P < Cl < Ca
c.
Ca < Mg < P < Cl
d.
P < Cl < Mg < Ca
e.
Ca < Cl < P < Mg
 

 51. 

A balloon is filled with oxygen gas to a volume of 1.75 L at 36ºC. The balloon is then heated to 72ºC. What is the volume of the heated balloon?
a.
0.875 L
b.
1.57 L
c.
1.95 L
d.
3.50 L
e.
4.11 L
 

 52. 

A 10.0 L flask contains 14.1 grams of an unknown gas. If the pressure in the flask is 2.3 atm at 65ºC, which of the following is a possible identity of the gas?
a.
NH3
b.
CO
c.
O2
d.
CO2
e.
CS2
 

 53. 

If 5.00 L of propane is burned in 21.0 L of oxygen, what volume of carbon dioxide is produced? Assume that the temperature of the reactants and products is 25ºC and the pressure of the system remains constant at 1.0 atm.

C3H8(g) + 5O2(g) ® 3CO2(g) + 4H2O(l)
a.
12.6 L
b.
15.0 L
c.
21.0 L
d.
25.6 L
e.
26.0 L
 

 54. 

Water can be decomposed by electrolysis to hydrogen gas and oxygen gas. What mass of water must decompose to yield 24.0 L of oxygen gas at 1.00 atm and 25ºC?

2H2O(l) ® 2H2(g) + O2(g)
a.
11.1 g
b.
17.7 g
c.
23.6 g
d.
35.3 g
e.
70.7 g
 

 55. 

A 10.0 L flask is used to collect 0.500 moles of N2 and 0.180 moles of O2 over water at 30ºC. What is the pressure in the flask? (vapor pressure H2O(l) = 31.8 mm Hg)
a.
-30.1 atm
b.
1.15 atm
c.
1.48 atm
d.
1.69 atm
e.
1.73 atm
 



 
Check Your Work     Start Over