Final Exam General Chemistry

Multiple Choice

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

____ 1. Which one of the following molecules will have the lowest boiling point?

a.	NH3
b.	CH3Cl
c.	CH4
d.	NH2Cl
e.	CHCl3

____ 2. Which functional group does not contain an oxygen atom?

a.	alcohol
b.	amine
c.	amide
d.	ester
e.	ether

____ 3. Use VSEPR theory to predict the molecular geometry of BCl₃.

a.	bent
b.	trigonal pyramidal
c.	trigonal planar
d.	tetrahedral
e.	t-shaped

____ 4. In general, atomic radii

a.	increase down a group and increase across a period.
b.	decrease down a group and remain constant across a period.
c.	increase down a group and decrease across a period.
d.	increase down a group and remain constant across a period.
e.	remain constant down a group and increase across a period.

____ 5. The functional group RCO₂R' is characteristic of an ________.

a.	ether
b.	ester
c.	amide
d.	aldehyde
e.	amine

____ 6. The balanced equation for the complete combustion of benzene, C₆H₆, is

a.	C6H6(ª) + 12 H2O ® 6 CO2(g) + 15 H2(g)
b.	C6H6(ª) ® 6 C(s) + 3 H2(g)
c.	2 C6H6(ª) + 9 O2(g) ® 12 CO (g) + 6 H2O(g)
d.	C6H6(ª) + O2(g) ® CO2(g) + H2O(g)
e.	2 C6H6(ª) + 15 O2(g) ® 12 CO2(g) + 6 H2O(g)

____ 7. Specific heat capacity is

a.	the quantity of heat required to melt 1.00 g of a substance.
b.	the mass of a substance 1.00 J of energy will heat by 1.00 K.
c.	the mass of a substance 1.00 cal of energy will heat by 1.00 K.
d.	the temperature change undergone when 1.00 g of a substance absorbs 1.00 cal.
e.	the quantity of heat needed to change 1.00 g of a substance by 1.00 K.

____ 8. The reaction of magnesium with elemental iodine, I₂, yields magnesium iodide. Write a balanced chemical equation for this reaction.

a.	2 Mg(s) + I2(s) ® 2 MgI(s)
b.	Mg(s) + 2 I(s) ® MgI2(s)
c.	4 Mg(s) + I2(s) ® 2 Mg2I(s)
d.	Mg(s) + 2 I2(s) ® MgI4(s)
e.	Mg(s) + I2(s) ® MgI2(s)

____ 9. What volume of O₂, measured at 27.2°C and 735 mm Hg, will be produced by the decomposition of 5.22 g KClO₃? (R = 0.08206 L·atm/mol·K)

2 KClO₃(s) ® 2 KCl(s) + 3 O₂(g)+

a.	0.0983 L
b.	1.09 L
c.	1.63 L
d.	199 L
e.	133 L

____ 10. How many protons, neutrons, and electrons are in a carbon-13 atom?

a.	6 protons, 6 neutrons, 1 electron
b.	6 protons, 7 neutrons, 6 electrons
c.	7 protons, 6 neutrons, 6 electrons
d.	7 protons, 6 neutrons, 7 electrons
e.	13 protons, 13 neutrons, 13 electrons

____ 11. When ethanol undergoes complete combustion, the products are carbon dioxide and water.

__ C₂H₅OH(ª) + __ O₂(g) ® __ CO₂(g) + __ H₂O(g)

What are the respective coefficients when the equation is balanced with the smallest whole numbers?

a.	2, 7, 4, 6
b.	1, 3, 2, 3
c.	2, 2, 1, 4
d.	1, 2, 3, 2
e.	2, 4, 6, 4

____ 12. Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)

a.	has two electrons per orbital, each with opposing spins.
b.	has two electrons per orbital, each with identical spins.
c.	only occurs for s and p-block elements.
d.	has a filled valence shell of electrons.
e.	has the maximum number of unpaired electrons, all with the same spin.

____ 13. All of the following are examples of chemical change EXCEPT

a.	the condensation of steam.
b.	the rusting of iron.
c.	the combustion of propane gas.
d.	the tarnishing of silver.
e.	the decomposition of water to hydrogen gas and oxygen gas.

____ 14. At constant temperature, 10.0 L of N₂ at 0.983 atm is compressed to 2.88 L. What is the final pressure of N₂?

a.	0.283 atm
b.	0.293 atm
c.	2.98 atm
d.	3.41 atm
e.	28.3 atm

____ 15. How many moles are there in 5.00 g of AgNO₃?

a.	5.00 mol
b.	0.0294 mol
c.	8.49 mol
d.	0.00112 mol
e.	34.0 mol

____ 16. Nitrogen and oxygen form an extensive series of oxides with the general formula N_xO_y. What is the empirical formula for an oxide that contains 63.65% nitrogen?

a.	N2O
b.	NO
c.	NO2
d.	N2O3
e.	N2O5

____ 17. A rectangular box has dimensions of 20.0 cm ´ 15.0 cm ´ 8.00 cm. Calculate the volume of the box in liters.

a.	2.40 ´ 10^-3 L
b.	4.30 ´ 10^-3 L
c.	2.40 L
d.	43.0 L
e.	2.40 ´ 10^3 L

____ 18. Which equation represents the number of atoms in a face-centered cubic unit cell?

a.	# atoms = (8)
b.	# atoms = (8)
c.	# atoms = 1 + (8)
d.	# atoms =
e.	# atoms =

____ 19. What is the electron configuration for Fe²⁺?

a.	[Ar]3d^104s^2	d.	[Ar]3d^6
b.	[Ar]3d^5	e.	[Ar]4s^23d^5
c.	[Ar]3d^44s^2

____ 20. What is the correct Lewis structure for IF₃?

a.	1
b.	2
c.	3
d.	4
e.	2 and 4

____ 21. If 1.928 g KNO₃ is dissolved in enough water to make 250.0 mL of solution, what is the molarity of potassium nitrate?

a.	6.912 ´ 10^-4 M
b.	4.767 ´ 10^-3 M
c.	7.627 ´ 10^-2 M
d.	1.297 ´ 10^-1 M
e.	7.712 M

____ 22. In the unit cell below, element X is within the cell and element Y is at the corners. What is the formula for this compound?

a.	XY
b.	XY2
c.	XY4
d.	XY8
e.	X2Y

____ 23. What is the net ionic equation for the reaction below?

AgNO₃(aq) + KBr(aq) ® AgBr(s) + KNO₃(aq)

a.	K^+(aq) + NO3^-(aq) ® KNO3(s)
b.	AgNO3(aq) + KBr(aq) ® AgBr(s)
c.	K^+(aq) + NO3^-(aq) ® KNO3(aq)
d.	AgNO3(aq) + KBr(aq) ® AgBr(s) + KNO3(aq)
e.	Ag^+(aq) + Br^-(aq) ® AgBr(s)

____ 24. A 25.00 mL sample of NaOH is titrated with 15.23 mL of 0.2250 M HCl. What is the concentration of the NaOH solution?

a.	2.198 ´ 10^-3 M
b.	0.02872 M
c.	0.1371 M
d.	0.3693 M
e.	0.5223 M

____ 25. In order to form a set of sp³d hybrid orbitals, how many pure atomic orbitals must be mixed?

a.	one s, one p, and one d
b.	one s, three p, and one d
c.	two s, one p, and two d
d.	two s, six p, and two d
e.	none of the above

____ 26. Which of the following diagrams represent a p-orbital?

a.	(I) only
b.	(II) only
c.	(III) only
d.	(IV) only
e.	(I) and (II)

____ 27. Which of the following sets of quantum numbers refers to a 3d orbital?

a.	n = 3, ª = 1, mª = -1
b.	n = 3, ª = 2, mª = -1
c.	n = 2, ª = 3, mª = +3
d.	n = 3, ª = 3, mª = -3
e.	n = 2, ª = 2, mª = +3

____ 28. Which element has the electron configuration [Ar]3d⁷4s²?

a.	Cu
b.	Rh
c.	Ti
d.	Br
e.	Co

____ 29. The following reaction occurs spontaneously.

2 H⁺(aq) + Ca(s) ® Ca²⁺(aq) + H₂(g)

Write the balanced oxidation half-reaction.

a.	2 H^+(aq) + 2 e^- ® H2(g)
b.	2 H^+(aq) ® H2(g) + 2 e^-
c.	2 H^+(aq) + Ca(s) ® 2 e^-
d.	Ca(s) + 2 e^- ® Ca^2+(aq)
e.	Ca(s) ® Ca^2+(aq) + 2 e^-

____ 30. The following reaction occurs spontaneously,

3 Cu²⁺(aq) + 2 Fe(s) ® 2 Fe³⁺(aq) + 3 Cu(s)

Write the balanced reduction half-reaction.

a.	2 Fe(s) ® 2 Fe^3+(aq) + 6 e^-
b.	2 Fe(s) + 6 e^- ® 2 Fe^3+(aq)
c.	3 Cu^2+(aq) + 6 e^- ® 3 Cu(s)
d.	3 Cu^2+(aq) ® 3 Cu(s) + 6 e^-
e.	3 Cu^2+(aq) + 2 Fe(s) + 6 e^- ® 3Cu(s) + 2 Fe^3+(aq)

____ 31. Which two of the ions below have the same number of electrons?

a.
b.
c.
d.
e.	none of the above

____ 32. What is the correct symbol for iron?

a.	Fe
b.	I
c.	Ir
d.	Sn
e.	Pb

____ 33. Which of the following orbitals might have an m_ª equal to +2?

a.	s
b.	s and p
c.	p and d
d.	s and f
e.	d and f

____ 34. What element is in the third period in Group 5A?

a.	As
b.	Nb
c.	P
d.	In
e.	Tl

____ 35. Identify the ions in (NH₄)₂SO₄.

a.	N^3-, H^+, S^2-, and O^2-
b.	NH2^2+ and H2SO4
c.	NH4^+ and SO4^2-
d.	NH4^2+ and SO4^2-
e.	NH4^+ and SO4^-

____ 36. What is the name of the following compound?

a.	4,5-dihexane
b.	2,3-diethylhexane
c.	4,5-dimethane
d.	2,3-dimethylhexane
e.	4,5-dimethylhexane

____ 37. Which compound in the reaction below undergoes oxidation?

CH₄(g) + 2 O₂(g) ® CO₂(g) + 2 H₂O(g)

a.	CH4
b.	O2
c.	CO2
d.	H2O
e.	CH4 and CO2

____ 38. What is the charge on the lead ion in PbCl₂?

a.	-2
b.	-1
c.	+1
d.	+2
e.	+4

____ 39. Which one of the following substances will exhibit dipole-dipole intermolecular forces?

a.	Kr
b.	N2
c.	CO2
d.	CCl4
e.	CO

____ 40. Which of the following is a correct Lewis structure for N₂O?

a.	1
b.	2
c.	3
d.	4
e.	5

An antacid tablet weighing 0.853 g contained calcium carbonate as an active ingredient, in addition to an inert binder. When an acid solution weighing 56.519 g was added to the tablet, carbon dioxide gas was released, producing a fizz; the resulting solution weighed 57.152 g.

____ 41. Which of the following is the balanced equation for the above chemical reaction?

a.	Na2CO3 + H^+ è 2Na^+ + CO2 + H2O	c.	CaCO3 + 2HCl è CaCl + CO2 + H2O
b.	CaCO3 + 2H^+ è Ca^2+ + CO2 + H2O	d.	NaCO3 + H^+ è Na^+ + CO2 + H2O

____ 42. How many grams of calcium carbonate were in the tablet?

a.	0.853 g	c.	0.220 g
b.	0.633 g	d.	56.51 g

____ 43. How many moles of calcium carbonate were in the tablet?

a.	2.75 moles	c.	3.67 moles
b.	3.67 x 10^-3 moles	d.	2.20 x 10^-3 moles

____ 44. What volume of CO₂ was produced if the temperature was constant at 25 °C and the pressure of 1.00 atm?

a.	.00677 L	c.	53.8 mL
b.	2.75 mL	d.	27 mL

____ 45. What is the charge on carbonate?

a.	1	c.	-2
b.	2	d.	-1

Barium is a group IIA metal that reacts with water exothermically. The barium ion that is generated is used as an x-ray imaging agent. A 2.50 g of barium reacts completely with water at 21 °C and 748 mmHg.

____ 46. Which of the following is the chemical reaction?

a.	Ba + 2H2O à Ba(OH)2 + H2	c.	Ba + 2H2O à Ba + H2
b.	Ba + H2O à CO2 + H2O	d.	Ba + 2H2O à Ba+ + H2 + O2

____ 47. What is the number of total electrons in elemental barium?

a.	56	c.	58
b.	54	d.	138

____ 48. What is the number of valence electrons in elemental barium?

a.	1	c.	3
b.	2	d.	4

____ 49. What does the exothermic reaction mean?

a.	consumes energy	c.	consumes heat
b.	generates energy	d.	generates light

____ 50. What volume of hydrogen gas is produce?

a.	44 mL	c.	440 mL
b.	69 mL	d.	.0469 L

Acetic acid is an organic acid found in vinegar. In the lab a student reacts a 200.0 mL sample of acetic acid with 0.125 M solution of NaOH for a compete neutralization process.

____ 51. Which of the following functional groups does acetic acid have?

a.	amine	c.	alcohol
b.	carboxylic acid	d.	ester

____ 52. What best describes the acetic acid molecule?

a.	Polar	c.	ionic
b.	non polar	d.	element

____ 53. What is the balanced acid base reaction for sodium hydroxide and acetic acid?

a.	Na2OH + 2HCl à H2O + 2NaCl	c.	Na2OH + CH3COOH à H2O + CH3COONa2
b.	NaOH + HCl à H2O + NaCl	d.	NaOH + CH3COOH à H2O + CH3COONa

____ 54. What is the molarity of acetic acid if it required 100.0 mL of NaOH to reach the end point of a titration?

a.	0.0313 M	c.	0.0625M
b.	0.012 M	d.	6.00 M

____ 55. When the student correctly set-up the experiment she placed the NaOH into which type of glassware?`

a.	Buret	c.	Erlenmeyer
b.	Beaker	d.	test tube

A molecular compound is 60.4 % Xe, 22.1 % O, and 17.5 % F by mass and has a molecular weight of 217.3 g/mol. The compound has five sigma bonds and three pi bonds.

____ 56. What is the empirical formula?

a.	XeFO	c.	XeF3O2
b.	XeF2O2	d.	XeF2O3

____ 57. What is the molecular formula?

a.	XeFO	c.	XeF3O2
b.	XeF2O2	d.	XeF2O3

____ 58. What is the hybride orbitals used to by Xe to make 5 sigma bonds?

a.	sp^3	c.	spd
b.	sp^3d	d.	sp^3d^2

____ 59. The pi bonds are between what two atoms?

a.	Xe and F	c.	Xe and O
b.	F and O	d.	none of the above

____ 60. What is the most electronegative atom in this compound?

a.	F	c.	Xe
b.	O

Final Exam General Chemistry

Answer Section

MULTIPLE CHOICE

1. C

2. B

3. C

4. C

5. B

6. E

7. E

8. E

9. C

10. B

11. B

12. E

13. A

14. D

15. B

16. A

17. C

18. D

19. D

20. C

21. C

22. A

23. E

24. C

25. B

26. B

27. B

28. E

29. E

30. C

31. B

32. A

33. E

34. C

35. C

36. D

37. A

38. D

39. E

40. B

41. B

42. C

43. D

44. C

45. C

46. A

47. A

48. B

49. B

50. C

51. B

52. A

53. D

54. C

55. C

56. D

57. D

58. B

59. C

60. A