Exam Review

1
Exam Review
2

• Which of the following elements is most commonly
  found as a negatively charged ion?
• Ne
• Li
• Al
• Cl

3

• Which molecule is nonpolar?
• H2O
• NH3
• CH4
• HF

4

• Which point could be the boiling point for the
  substance?

D
C
A
B
5

• Which molecule has trigonal pyramidal symmetry?
• H2O
• NH3
• CH4
• HF

6

• The empirical formula for a hydrocarbon that is
  20 hydrogen by weight is
• CH
• CH2
• CH3
• CH4

7

• What is the weight of sodium nitrate (MW 85.0)
  present in 100. mL of a 4.00M solution?
• 34.0 g
• 25.5 g
• 17.0 g
• 8.50 g

8

• Which does not exhibit hydrogen bonding?
• H2O
• NH3
• CH4
• HF

9

• 2 NO Br2 ? 2NO
• For the reaction above, the experimental rate law
  is
• Rate kNO2Br2
• Which statement is true regarding the reaction?
• The reaction is first order overall.
• The reaction is first order with respect to Br2.
• The reaction is first order with respect to NO.
• The reaction is second order overall.

10

• Which of the following is the most likely
  electron configuration for a sulfur atom in the
  ground state?
• 1s22s22p6
• 1s22s22p63s2
• 1s22s22p63s23p2
• 1s22s22p63s23p4

11

• Zn NO3- 10 H ? Zn2 NH4 3H2O
• Which of the following statements is true?
• The oxidation number of hydrogen changes from 1
  to 0.
• The oxidation number of hydrogen changes from 1
  to -1.
• The oxidation number of nitrogen changes from 5
  to -3.
• The oxidation number of nitrogen changes from 5
  to 3.

12

• How many grams of carbon are present in 271 g of
  glucose (C6H12O6)?
• 18.0 g
• 67.5 g
• 72.0 g
• 108 g

13

• Which compound has the highest melting point?
• NaCl
• LiF
• KI
• MgO

14

• What is the enthalpy change for the following
  reaction 2H2O2 S ? SO2 2H2O
• -500kJ
• -300kJ
• 200kJ
• 400kJ

Substance DHf (kJ/mol)
H2O2 -150
SO2 -300
H2O -250
S 0
15

• The reaction of elemental chlorine with ozone in
  the atmosphere occurs by a two-step process
• Cl O3 ? ClO O2
• ClO O ? Cl O2
• Which statement is true?
• Cl is a catalyst
• O3 is a catalyst
• ClO is a catalyst
• O2 is an intermediate

16

• Which is an impossible set of quantum numbers?
• 4, 0, 0, ½
• 4, 0, 1, ½
• 4, 1, 0, ½
• 4, 2, 1, ½

17

• A sample of water was electrolyzed to produce
  hydrogen and oxygen gas as shown below
• 2H2O ? 2H2 O2
• If 22.4L of hydrogen were produced at STP, how
  many grams of water were consumed in the
  reaction?
• 11.1 g
• 18.0 g
• 24.0 g
• 36.0 g

18

• How many mL of water must be added to 10mL of an
  HCl solution with a pH of 1 to produce a solution
  with a pH of 2?
• 10 mL
• 90 mL
• 100 mL
• 990 mL

19

• Which of the statements is NOT true regarding
  elemental nitrogen?
• It contains one sigma bond.
• It contains two pi bonds.
• It has a large dipole moment.
• It exists as a diatomic gas.

20

• A chemist creates a buffer solution by mixing
  equal volumes of 0.2M HOCl and 0.2M KOCl. Which
  of the following will occur when a small amount
  of KOH is added?
• HOCl increases
• OCl- increases
• H increases
• I only
• II only
• III only
• II and III

21

• C CO2 energy ? 2CO
• The above system is currently at equilibrium in a
  closed container. Which of the following changes
  to the system would serve to increase the number
  of moles of CO present at equilibrium?
• Raising the temperature
• Increasing the pressure
• Decreasing the amount of C
• I only
• II only
• III only
• All of the above

22

• 222Rn nuclide decays through the emission of two
  beta particles and two alpha particles. The
  resulting nuclide is
• 214Po
• 210Po
• 214Bi
• 210Bi

23

• The freezing point of an aqueous potassium iodide
  solution is -3.72oC. What is the molal
  concentration of the KI? (kf 1.86 Kkg/mol)
• 0.500 molal
• 1.00 molal
• 1.50 molal
• 2.00 molal

24

• A sample of an ideal gas is placed in a sealed
  container at constant volume. If the temperature
  of the gas is increased from 40oC to 70oC, which
  of the following will NOT increase?
• The average speed of the molecules of gas
• The average kinetic energy of the molecules
• The density of the gas
• The pressure exerted by the gas

25

• If 52 g of Ba(NO3)2 (MW 260) are completely
  dissolved in 500 mL of water, what are the
  concentration of the barium and nitrate ions?
• Ba2 0.10M and NO3- 0.10M
• Ba2 0.10M and NO3- 0.20M
• Ba2 0.40M and NO3- 0.40M
• Ba2 0.40M and NO3- 0.80M

26

• An acid solution of unknown concentration is to
  be titrated with standardized sodium hydroxide
  that will be released from a buret. The buret
  should be rinsed with
• A neutral salt solution
• Room temp distilled water
• A sample of the unknown acid
• A sample of the hydroxide solution

27

• Each of the following compounds was added to
  distilled water. Which one produced a solution
  with a pH that was less than 7.
• SO2
• N2
• NaI
• MgO

28

• ___ Be2C ___H2O ? ___Be(OH)2 ___CH4
• When the equation above is balanced with the
  lowest whole-number coefficients, the coefficient
  for water will be
• 5
• 4
• 3
• 2

29

• All of the following statements concerning alkali
  metals are true EXCEPT
• They are strong oxidizing agents.
• They form ions with a 1 oxidation number.
• As the atomic number of the alkali metals
  increases, electronegativity decreases
• They form ions that are soluble in water.

30
Compound Ksp
FeS 6.3310-18
PbS 8.0310-28
MnS 1.0310-13

• A solution contains Fe2, Pb2, and Mn2 ions.
  Which of the following gives the order in which
  precipitates will form, from first to last, as
  Na2S is added to the solution?
• MnS, FeS, PbS
• MnS, PbS, FeS
• PbS, FeS, MnS
• FeS, PbS, MnS

31

• H2O(g) ? H2O(l)
• Which of the following is true of the spontaneous
  reaction above?
• DG is greater than zero.
• DH is less than zero.
• DS is greater than zero.
• II only
• III only
• I and II
• II and III

32

• All of the elements listed below are gases at
  room temperature. Which gas would be expected to
  show the greatest deviation from ideal behavior?
• Ne
• Ar
• Kr
• Xe

33

• What is the pH of a solution made by mixing 200mL
  of 0.20 M NH3 with 200mL of a 0.20M NH4Cl? (The
  Kb for ammonia is 1.810-5.)
• Between 9 and 10
• Between 8 and 9
• Between 5 and
• Between 4 and 5

34

• Which molecule does NOT exhibit sp3
  hybridization?
• H2O
• NH3
• HF
• CH4

35

• Which molecule exhibits hydrogen bonding?
• HF
• NH3
• HCl
• H2S

36

• A mixture of gases contains 5.0 moles of oxygen,
  12 moles of nitrogen and 4.0 moles of carbon
  dioxide. If the partial pressure due to carbon
  dioxide is 1.6 atm, what is the partial pressure
  due to oxygen.
• 1.3 moles
• 2.0 moles
• 4.8 moles
• 6.0 moles

37

• Which of the following represents the activation
  energy of the reaction?
• X
• Y
• XY
• X-Y

38

• A monoprotic acid was titrated with NaOH. For
  55.0mL of acid, 37.0mL of 0.450M NaOH was
  required to reach the equivalence point. Which of
  the following expressions is equal to the initial
  concentration of acid.

39

• Which element is the most electronegative?
• I
• Br
• Cl
• F

40

• A sparingly soluble metal hydroxide M(OH)2 has a
  molar solubility of S mol/L. Its Ksp value is
• S2
• 2S2
• 2S3
• 4S3

41

• Which of the following compounds provides an
  example of ionic and covalent bonding,
  respectively?
• HBr and NaCl
• NaCl and HBr
• NaCl and NaI
• NaI and NaCl