Part II. There are 50 questions; each is worth 2 points. Choose the one alternative that best completes the statement or answers the question.
1)	Sodium belongs to the ________ group of the periodic table.	1) ______

	A)  noble gas
	B)  alkaline earth
	C)  alkali metal
	D)  halogen
	E)  super

2)

Which of the following elements is a good conductor of heat and electricity?

2) ______

	A)  oxygen
	B)  sulfur
	C)  fluorine
	D)  carbon
	E)  None of the above.

3)

Convert 0.0003002 to standard scientific notation.

3) ______

	A)  3002 × 10-7
	B)  3.002 × 104
	C)  3002 × 10-6
	D)  3.002 × 10-4
	E)  None of the above

4)

How many significant figures are there in the answer for the following problem? = ?

4) ______

	A)  one
	B)  two
	C)  three
	D)  four
	E)  five

5)

Which element indicated by letter in the following periodic table is a liquid at room temperature and a pressure of 1.0 atm?

5) ______

	A)  A
	B)  B
	C)  C
	D)  D
	E)  None of the above.

6)

To the correct number of significant figures, what is the temperature reading on the following Celsius thermometer?

6) ______

	A)  15.6°C
	B)  15.65°C
	C)  15°C
	D)  16°C
	E)  None of the above

7)

What is the chemical symbol for an atom that has 30 protons and 36 neutrons?

7) ______

	A)  Zn
	B)  Tb
	C)  Kr
	D)  N
	E)  None of the above.

8)

Pure water is an example of

8) ______

	A)  a homogeneous mixture.
	B)  a heterogeneous mixture.
	C)  a compound.
	D)  an element.
	E)  None of the above.

9)

In which of the following sets do all species have the same number of electrons?

9) ______

	A)  O2-, F-, Ne
	B)  Kr, Sr2+, Rb+
	C)  Br-, Kr, Rb+
	D)  C, N+, O2+
	E)  All of the above.

10)

The solid compound, Na2CO3, contains

10) ______

	A)  Na+ and CO32- ions.
	B)  Na2+2 ions and CO32-ions.
	C)  Na+, C6+, and O2- ions.
	D)  Na2CO3 molecules.
	E)  None of the above.

11)

The definitive distinction between ionic bonding and covalent bonding is that

11) ______

	A)  covalent bonding requires two nonmetals and ionic bonding requires a metal and a nonmetal.
	B)  ionic bonding requires two nonmetals and covalent bonding requires a metal and a nonmetal.
	C)  ionic bonding involves a transfer of electrons and covalent bonding involves a sharing of electrons.
	D)  ionic bonding involves a sharing of electrons and covalent bonding involves a transfer of electrons.
	E)  None of the above.

12)

Assume that the mixture of substances in drawing (1) undergoes a chemical reaction. Which of the drawings (2)-(4) represents a product mixture that is consistent with the law of mass conservation?

12) ______

	A)  drawing (2)
	B)  drawing (3)
	C)  drawing (4)
	D)  All of the above
	E)  None of the above

13)

Which one of the following statements about balanced equations is true? In a balanced reaction

13) ______

	A)  mass must be conserved.
	B)  atoms must be balanced on both sides of the reaction arrow.
	C)  protons must be balanced on both sides of the reaction arrow.
	D)  net charge must be balanced on both sides of the reaction arrow.
	E)  All are true

14)

What is the sum of the coefficients when the following equation is balanced using the lowest, whole numbered coefficients? ________ B2O3(s) + ________ HF(l) → ________ BF3(g) + ________ H2O(l)

14) ______

	A)  15
	B)  12
	C)  11
	D)  4
	E)  none of these

15)

What is the molar mass of hydrogen gas?

15) ______

	A)  2.00 g/mol
	B)  1.20 × 1023 g/mol
	C)  1.00 g/mol
	D)  6.02 × 1023 g/mol
	E)  None of the above.

16)

The following diagrams represent the reaction of A2 (shaded spheres) with B2 (unshaded spheres). Identify the limiting reactant and write a balanced equation for the reaction.

16) ______

	A)  B2 is the limiting reactant; A2 + 4 B2 → 2 AB4.
	B)  A2 is the limiting reactant; A2 + 4 B2 → 2 AB4.
	C)  A2 is the limiting reactant; A + 4 B → AB4.
	D)  B2 is the limiting reactant; A + 4 B → AB4.
	E)  None of the above.

17)

Which of the following statements is true concerning the formula of a compound?

17) ______

	A)  The empirical formula is the simplest whole numbered ratio of atoms in a compound.
	B)  The molecular formula is the true ratio of atoms in a compound.
	C)  The molecular formula and empirical formula can be identical.
	D)  The number of atoms in a molecular formula can be greater than the number of atoms in an empirical formula.
	E)  All of the above are true.

18)

Which one of the following is a molecular formula?

18) ______

	A)  P4O10
	B)  C2F6
	C)  H2S2O4
	D)  N2H4
	E)  All of the above.

19)

The reaction of HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l) is best classified as a(n)

19) ______

	A)  acid-base neutralization reaction.
	B)  single replacement reaction.
	C)  precipitation reaction.
	D)  oxidation-reduction reaction.
	E)  All of the above.

20)

The reaction of Na3PO4(aq) + 3 AgNO3(aq) → Ag3PO4(s) + 3 NaNO3(aq) is best classified as a(n)

20) ______

	A)  oxidation-reduction reaction.
	B)  acid-base neutralization reaction.
	C)  single replacement reaction.
	D)  precipitation reaction.
	E)  None of the above.

21)

Write a balanced net ionic equation for the reaction of Pb(NO3)2(aq) with NaI(aq).

21) ______

	A)  Pb(NO3)2(aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq)
	B)  Pb2+(aq) + 2 I-(aq) → PbI2(s)
	C)  Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2 I-(aq) → PbI2(s) + 2 Na+(aq) + 2 NO3-(aq)
	D)  Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2 I-(aq) → Pb2+(aq) + 2 I-(aq) + 2 Na+(aq) + 2 NO3-(aq)
	E)  None of the above.

22)

What is the molar concentration of sodium ions in a 0.150 M sodium sulfate solution?

22) ______

	A)  0.150 M
	B)  0.300 M
	C)  0.450 M
	D)  0.075 M
	E)  None of the above.

23)

Which pair of reactants will produce a precipitate when mixed together?

23) ______

	A)  HCl(aq) and Na2CO3(aq)
	B)  HCl(aq) and NaOH(aq)
	C)  HCl(aq) and Na2S(aq)
	D)  HCl(aq) and Ca(NO3)2(aq)
	E)  None of the above.

24)

The greater the energy of a photon, the

24) ______

	A)  longer the wavelength and the higher the frequency.
	B)  shorter the wavelength and the lower the frequency.
	C)  shorter the wavelength and the higher the frequency.
	D)  longer the wavelength and the lower the frequency.
	E)  None of the above are correct.

25)

According to the Heisenberg uncertainty principle,

25) ______

	A)  the position and momentum of a particle can be measured precisely, but not at the same time.
	B)  the position of a particle cannot be measured precisely.
	C)  neither the position nor the momentum of a particle can be measured precisely.
	D)  the momentum of a particle cannot be measured precisely.
	E)  None of the above are correct.

26)

Which of the following represent electron configurations that violate the Pauli exclusion principle? (A) [Ne]3s13p5 (B) [Kr]4d125s25p3 (C) [Ar]3d104s24p2

26) ______

	A)  only (A)
	B)  only (B)
	C)  (B) and (C)
	D)  (A) and (B)
	E)  (A) and (B) and (C)

27)

For an electron in a given atom, the greater the value of n, the

27) ______

	A)  smaller the average distance from the nucleus and the lower the orbital energy.
	B)  larger the average distance from the nucleus and the higher the orbital energy.
	C)  smaller the average distance from the nucleus and the higher the orbital energy.
	D)  larger the average distance from the nucleus and the lower the orbital energy.
	E)  None of the above are correct.

28)

For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l?

28) ______

	A)  n = 4 and l = 0
	B)  n = 4 and l = 2
	C)  n = 4 and l = 1
	D)  n = 4 and l = 3
	E)  None of the above.

29)

What is the oxidation number of the sulfur atom in H2SO4?

29) ______

	A)  +6
	B)  +2
	C)  -2
	D)  +4
	E)  None of the above.

30)

Using the following portion of the activity series for oxidation half reactions K(s) → K+(aq) + e- Al(s) → Al3+(aq) + 3e- Fe(s) → Fe2+(aq) + 2e- Sn(s) → Sn2+(aq) + 2e- determine which pairs of reactions will occur.

30) ______

	A)  K(s) with Al3+(aq) and Fe(s) with Al3+(aq)
	B)  Al(s) with Fe2+(aq) and Sn(s) with K+(aq)
	C)  Fe(s) with Sn2+(aq) and Al(s) with Sn2+(aq)
	D)  Fe(s) with Al(s) and Al3+(aq) with Sn2+(aq)
	E)  None of the above

31)

For a multielectron atom, a 3p orbital is higher in energy than a 3s orbital because

31) ______

	A)  there are more p orbitals than s orbitals in a given shell.
	B)  a 3p orbital has more nodal surfaces than a 3s orbital.
	C)  other electrons more effectively shield electrons in the 3s orbital from the nucleus.
	D)  other electrons more effectively shield electrons in the 3p orbital from the nucleus.
	E)  None of the above.

32)

What is the ground-state electron configuration of Zn?

32) ______

	A)  [Ar]4s24p63d4
	B)  [Ar]3d10
	C)  [Ar]4s23d8
	D)  [Ar]4s23d10
	E)  None of the above.

33)

Of the following, which element has the highest first ionization energy?

33) ______

	A)  beryllium
	B)  lithium
	C)  boron
	D)  nitrogen
	E)  fluorine

34)

Which ionic compound would be expected to have the greatestest lattice energy?

34) ______

	A)  NaCl
	B)  MgO
	C)  AlF3
	D)  Al2O3
	E)  They are all about the same.

35)

Which chemical process is associated with the lattice energy for sodium chloride?

35) ______

	A)  NaCl(s) + H2O(l) → Na+(aq) + Cl-(aq)
	B)  NaCl(g) → Na+(g) + Cl-(g)
	C)  Na(s) + 1/2 Cl2(g) → NaCl(s)
	D)  NaCl(s) → Na+(g) + Cl-(g)
	E)  None of the above.

36)

Which electrostatic forces hold atoms together in a molecule?

36) ______

	A)  electron-nucleus forces
	B)  nucleus-nucleus forces
	C)  electron-electron forces
	D)  all three forces

37)

How many electrons are in the valence shell of I in IF4-?

37) ______

	A)  8
	B)  14
	C)  10
	D)  12
	E)  None of the above.

38)

Which orbital hybridization is associated with an octahedral charge cloud arrangement?

38) ______

	A)  sp3d
	B)  sp2
	C)  sp3d2
	D)  sp
	E)  sp3

39)

Use the following MO diagram for Be2, Be2+, and Be2-. (Be sure to put the 1s electrons in the diagram) Based on this diagram,

39) ______

	A)  Be2 is more stable than either Be2+ or Be2-.
	B)  Be2+ and Be2- are both more stable than Be2.
	C)  Be2+ is more stable than Be2, and Be2 is more stable than Be2-.
	D)  Be2- is more stable than Be2, and Be2 is more stable than Be2+.
	E)  Not enough informstion to tell.

40)

A process is carried out at constant pressure. Given that ΔE is positive and ΔH is negative,

40) ______

	A)  the system loses heat and expands during the process.
	B)  the system absorbs heat and expands during the process.
	C)  the system absorbs heat and contracts during the process.
	D)  the system loses heat and contracts during the process.
	E)  None of the above.

41)

Which combination always results in a process being spontaneous?

41) ______

	A)  ΔH is positive and ΔS is positive.
	B)  ΔH is negative and ΔS is positive.
	C)  ΔH is negative and ΔS is negative.
	D)  ΔH is positive and ΔS is negative.
	E)  All of these can be spontaneous.

42)

If a process with a negative value of ΔS is spontaneous at constant temperature and pressure,

42) ______

	A)  ΔG is negative and ΔH is negative.
	B)  ΔG is positive and ΔH may be positive or negative.
	C)  ΔG is negative and ΔH is positive.
	D)  ΔG is negative and ΔH may be positive or negative.
	E)  None of the above.

43)

An approximation of absolute zero was made from an extrapolation of

43) ______

	A)  V vs. 1/T
	B)  P vs. 1/V
	C)  V vs. T
	D)  n vs. V
	E)  None of the above.

44)

If the number of moles of gas is doubled at constant temperature and volume, the pressure of the gas

44) ______

	A)  remains the same.
	B)  is doubled.
	C)  is halved.
	D)  is quadrupled.
	E)  Not enough information.

45)

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains CH4, flask B contains CO2, flask C contains N2. Which flask contains the largest number of moles?

45) ______

	A)  flask A
	B)  flask B
	C)  flask C
	D)  All flasks contain the same number of moles.
	E)  Not enough information.

Assume that you have a sample of gas in a cylinder with a moveable piston, as shown in diagram (1). The initial pressure, number of moles, and temperature of the gas are noted on the diagram.
46)	Which diagram (2)-(4) most closely represents the result of doubling the pressure and temperature while keeping the number of moles of gas constant?	46) ______

	A)  diagram (2)
	B)  diagram (3)
	C)  diagram (4)
	D)  both diagrams (2) and (4)
	E)  diagrams (2), (3) and (4)

47)

Which diagram (2)-(4) most closely represents the result of doubling the pressure and doubling the temperature and the number of moles of gas?

47) ______

	A)  diagram (2)
	B)  diagram (3)
	C)  diagram (4)
	D)  both diagrams (2) and (4)
	E)  None of the above

48)

Assume that you have a sample of gas in a cylinder with a moveable piston, as shown in diagram (1). The initial pressure, number of moles, and temperature of the gas are noted on the diagram. Which diagram (2)-(4) most closely represents the result of doubling the pressure and number of moles of gas while increasing the temperature?

48) ______

	A)  diagram (2)
	B)  diagram (3)
	C)  diagram (4)
	D)  diagrams (3) and (4)
	E)  diagrams (2), (3) and (4)

In the diagram below, nitrogen molecules are represented by unshaded spheres, oxygen molecules by gray spheres, and chlorine molecules by black spheres.
49)	If the total pressure in the container is 900 mm Hg, what is the partial pressure of oxygen?	49) ______

	A)  180 mm Hg
	B)  270 mm Hg
	C)  450 mm Hg
	D)  90 mm Hg
	E)  None of the above.

50)

Three bulbs, two of which contain different gases and one of which is empty, are connected as shown in drawing (a). Which drawing (b) - (d) best represents the system after the stopcocks are opened and the system is allowed to come to equilibrium?

50) ______

	A)  drawing (b)
	B)  drawing (c)
	C)  drawing (d)