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AP CHEM UNIT 2 STUDY GUIDE

Total questions: 91

Worksheet time: 46mins

Name
Class
Date
1.
a)

It has the formula XZ2

b)

It does not dissolve in water

c)

It contains ionic bonds

d)

It contains covalent bonds

2.
a)

There is a partial negative charge on the H atom.

b)

Electrons are shared equally between the H and F atoms.

c)

The bond is extremely weak.

d)

The bond is highly polar.

3.
a)

The carbon-to-selenium bond is unstable.

b)

The carbon-to-selenium bond is nonpolar covalent.

c)

The compound has the empirical formula CSe.

d)

A molecule of the compound will have a partial negative charge on the carbon atom.

4.
a)

increasing strength of the bonds

b)

increasing electronegativity of the central atom

c)

increasing number of unshared pairs of electrons

d)

decreasing repulsion between hydrogen atoms

5.
a)

b)

c)

d)

6.
a)

CH4 < SiCl4 < SF4

b)

CH4 < SF4 < SiCl4


c)

SF4 < CH4 < SiCl4


d)

SiCl4 < SF4 < CH4


7.

Which of the following has the bonds arranged in order of decreasing polarity?


a)

H−F > N−F > F−F


b)

H−I > H−Br > H−F


c)

O−N > O−S > O−Te


d)

Sb−I > Sb−Te > Sb−Cl


8.

Which of the following complete Lewis diagrams represents a molecule containing a bond angle that is closest to 120°?

a)

b)

c)

d)

9.
a)

90*

b)

109.5*

c)

120*

d)

180*

10.
a)

180*

b)

120*

c)

105*

d)

90*

11.
a)

The leftmost C atom and all the atoms directly bonded to it lie in the same plane.


b)

Both C atoms and both O atoms lie in the same plane.


c)

The N−C−C bond angle is 180°.


d)

The geometry around the N atom is planar.


12.
a)

unequally shared and form nondirectional bonds


b)

unequally shared and form highly directional bonds


c)

equally shared and form nondirectional bonds


d)

equally shared and form highly directional bonds


13.
a)

The atoms form a bond with a bond length of 25pm.


b)

The atoms form a bond with a bond length of 75pm.


c)

The net force between the atoms is attractive at 25pm.


d)

The net force between the atoms is attractive at 75pm.


14.
a)

1 and 1.5

b)

1 and 2

c)

1.5 and 1.5

d)

2 and 2

15.
a)

C-Cl

b)

C-I

c)

C-H

d)

C-Br

16.
a)

Yes; it changes from sp to sp2.


b)

Yes; it changes from sp to sp3.


c)

Yes; it changes from sp2 to sp3.

d)


No; it does not change

17.
a)

the same because the molecular formulas are similar


b)

the same because C and S have similar electronegativity values


c)

different because the lone pair of electrons on the S atom make it the negative end of a dipole


d)

different because S has a greater number of electron domains (regions of electron density) surrounding it than C has


18.
a)

It conducts electricity because it is made of positive and negative ions.


b)

It conducts electricity because it is made of particles of different sizes.


c)

It does not conduct electricity because its ions cannot move freely within the solid.


d)

It does not conduct electricity because there are small spaces between the particles.


19.
a)

B2


b)

N2

c)

O2

d)

F2

20.
a)

B2

b)

N2

c)

O2


d)

F2

21.
a)

B2

b)

N2

c)

O2

d)

F2

22.
a)

b)

c)

d)

23.
a)


CS2, because the double bonds create an area of higher electron density around the Catom.

b)


PCl3, because the Clatoms draw electron density away from the Patom and the bond dipoles do not cancel one another.

c)


SF6, because it has the greatest number of polar bonds.

d)


CF4, because the large electronegativity difference between C and F results in very polar bonds.

24.
a)

The mass of F− ions is greater than that of O2− ions.


b)

The mass of Mg2+ ions is greater than that of Na+ ions.


c)

The difference between the electronegativity values of Mg and O is smaller than the difference between the values of Na and F.


d)

The charges of Mg2+ and O2− ions are greater than those of Na+ and F− ions.


25.
a)

Cu has two common oxidation states, but Ag has only one.


b)

Cu has a higher melting point than Au has, but Ag has a lower melting point than Au has.


c)

Cu atoms are smaller than Ag atoms, thus they interfere more with the displacement of atoms in the alloy.


d)

Cu atoms are less polarizable than are Au or Ag atoms, thus Cu has weaker interparticle forces.


26.

For which of the following molecules are reso­nance structures necessary to describe the bond­ing satisfac­torily?


a)

SO2


b)

CO2


c)

OF2

d)

PF3

27.
a)

BeCl2


b)

SO2

c)

N2

d)

F2

28.
a)

BeCl2


b)

SO2

c)

N2

d)

F2

29.

The geometry of the SO3 molecule is best de­scribed as


a)

trigonal planar


b)

trigonal pyramidal


c)

bent


d)

tetrahedral


30.

On the basis of molecular structure and bond polarity, which of the following compounds is most likely to have the greatest solubility in water?


a)

CH4


b)

CCl4

c)

NH3


d)

PH3

31.
a)

NaCl will have a lower boiling point than NaF because the coulombic attractions are weaker in NaCl than in NaF.


b)

NaCl will have a boiling point between that of NaF and MgO because the covalent character of the bonds in NaCl is intermediate between that of MgO and NaF.


c)

NaCl will have a higher boiling point than MgO because the ions are spaced farther apart in NaCl.


d)

NaCl will have a higher boiling point than MgO because the energy required to transfer electrons from the anion to the cation is larger in NaCl than in MgO.


32.

Which of the following Lewis electron-dot diagrams represents the molecule that contains the smallest bond angle?


a)

b)

c)

d)

33.
a)

H2O


b)

NH3

c)

BH3

d)

CH4

34.
a)

H2O

b)

NH3

c)

BH3

d)

CH4

35.
a)

H2O

b)

NH3

c)

BH3

d)

CH4

36.
a)

H2O

b)

NH3


c)

BH3

d)

CH4

37.

Which of the following has molecules with a pyramidal shape?


a)

NH3(g)


b)

BH3(g)


c)

H2S(g)


d)

HBr(g)


38.
a)

sp

b)

sp2


c)

sp3


d)

dsp2


39.
a)

Set A

b)

Set B

c)

Set C

d)

Set D

40.
a)


sp hybridized and 180°


b)


sp2 hybridized and 120°


c)


sp2 hybridized and 180°


d)


sp3 hybridized and 120*

41.
a)

sp


b)

sp2


c)

sp3


d)

dsp2


42.
a)

A

b)

B

c)

C

d)

D

43.
a)

b)

c)

d)

44.

Which of the following graphs correctly shows the relationship between potential energy and internuclear separation for two hydrogen atoms?


a)

b)

c)

d)

45.
a)

b)

c)

d)

46.

Which of the following substances has bonds with the greatest ionic character?


a)

CCl4

b)

CuCl2

c)

CaCl2

d)

NCl3

47.
a)


Cl2, PCl3,CaCl2

b)


Cl2, CaCl2,PCl3

c)


CaCl2, PCl3,Cl2

d)


CaCl2, Cl2,PCl3

48.

An atom of chlorine and an atom of which of the following elements will form a bond with the most ionic character?


a)

Germanium


b)

Carbon


c)

Copper

d)

Potassium

49.

Which of the following molecules has the largest dipole moment?


a)

b)

c)

d)

50.
a)

The solubility of MgF2 is less than that of NaF.


b)

The electronegativity of Mg is greater than that of Na

c)

The mass of the Mg cation is greater than that of the Na cation.


d)

The charge of the Mg cation is larger than that of the Na cation.


51.

The lattice energy of a salt is related to the energy required to separate the ions. For which of the following pairs of ions is the energy that is required to separate the ions largest? (Assume that the distance between the ions in each pair is equal to the sum of the ionic radii.)


a)

Na+(g) and Cl−(g)


b)

Cs+(g) and Br−(g)


c)

Mg2+(g) and O2−(g)


d)

Ca2+(g) and O2−(g)


52.
a)

In the C6H6 molecule, all the bonds between the carbon atoms have the same length.


b)

Because of variable bonding between its carbon atoms, C6H6 is a good conductor of electricity.


c)

The bonds between carbon atoms in C6H6 are unstable, and the compound decomposes quickly.

d)

The C6H6 molecule contains three single bonds between carbon atoms and three double bonds between carbon atoms.


53.

Which of the following Lewis diagrams best represents the bonding in the N2O molecule, considering formal charges?


a)

b)

c)

d)

54.
a)

The NO3− ion is not a polar species.


b)

The oxygen-to-nitrogen-to-oxygen bond angles are 90°.


c)

One of the bonds in NO3− is longer than the other two.


d)

One of the bonds in NO3− is shorter than the other two.


55.
a)

All the atoms in molecule 1 lie in one plane.


b)

All the molecules have the same empirical formula.


c)

The C-C-C bond angle in molecule 2 is close to 180°.


d)

The strongest carbon-to-carbon bond occurs in molecule 3.


56.

In the following diagrams, elements are represented by X and Z, which form molecular compounds with one another. Which diagram represents a molecule that has a bent molecular geometry?


a)

b)

c)

d)

57.
a)

CO2


b)

H2O


c)

C2H4


d)

PH3

58.
a)

CO2

b)

H2O


c)

C2H4

d)

PH3

59.
a)

CO2

b)

H2O

c)

C2H4

d)

PH3

60.

Which of the following molecules contains exactly three sigma (σ) bonds and two pi (π) bonds?


a)

C2H2

b)

CO2

c)

HCN

d)

SO3

61.

Which of the following molecules has an angular (bent) geometry that is commonly represented as a resonance hybrid of two or more electron-dot structures?


a)

CO2

b)

O3

c)

BeF2


d)

OF2


62.

Of the following molecules, which has the largest dipole moment?


a)

CO

b)

CO2

c)

HF

d)

F2


63.
a)

The attractive and repulsive forces are balanced, so the atoms will maintain an average internuclear distance x.


b)

There is a net repulsive force pushing the atoms apart, so the atoms will move further apart.

c)

There is a net attractive force pulling the atoms together, so the atoms will move closer together.

d)

It cannot be determined whether the forces between atoms are balanced, attractive, or repulsive, because the diagram shows only the potential energy

64.
a)

b)

c)

d)

65.

Of the following compounds, which is the most ionic?


a)

SiCl4


b)

BrCl


c)

PCl3


d)

CaCl2

66.

Which of the following Lewis electron-dot diagrams represents the molecule that is the most polar?


a)

b)

c)

d)

67.

NH3 reacts with BF3 to form a single species. Which of the following structural diagrams is the most likely representation of the product of the reaction?


a)

b)

c)

d)

68.

Which of the following molecules contains polar covalent bonds but is a nonpolar molecule?


a)

CH3Cl


b)

CH2Cl2

c)

NH3


d)

CCl4

69.

Which of the following molecules is nonpolar but has polar covalent bonds?


a)

H2O2


b)

H2O

c)

CCl4

d)

CH2Cl2


70.

Of the following single bonds, which is the LEAST polar?


a)

N—H


b)

H—F


c)

O—F


d)

I—F


71.

Which of the following arranges the molecules N2, O2, and F2 in order of their bond enthalpies, from least to greatest?


a)

F2 < O2 < N2


b)

O2 < N2 < F2


c)

N2 < O2 < F2


d)

N2 < F2 < O2


72.

Of the following diagrams, which best represents the structure of solid KF?

a)

b)

c)

d)

73.

Steel is an alloy consisting of Fe with a small amount of C. Elemental Cr can be added to steel to make the steel less likely to rust; Cr atoms react with oxygen in the air to form a nonreactive layer of chromium oxide on the surface of the steel, preventing the oxidation of underlying Fe atoms. A sample of steel-chromium alloy contains 15 percent Cr by mass. Which of the following diagrams best shows a particle-level view of a surface section and an interior section of the alloy represented below at the left? (The atomic radii of the atoms involved are given in the table below at the right.)


a)

b)

c)

d)

74.

Which of the following diagrams best illustrates how a displacement in an ionic crystal results in cleavage and brittleness?


a)

b)

c)

d)

75.

Which of the following diagrams best depicts an alloy of Ni and B?


a)

b)

c)

d)

76.

Pi (π) bonding occurs in each of the following species EXCEPT


a)

CO2


b)

CN–


c)

C6H6


d)

CH4


77.
a)

b)

c)

d)

78.
a)

H2<CI2<HCI

b)

H2<HCI<CI2

c)

CI2<HCI<H2

d)

CI2

79.

Resonance is most commonly used to describe the bonding in molecules of which of the following?


a)

CO2


b)

O3

c)

H2O

d)

SF6


80.

Which of the following molecules has the shortest bond length?


a)

N2


b)

O2


c)

Cl2

d)

I2

81.

Steel is an alloy containing Fe atoms and C atoms. Which of the following diagrams best represents the particle-level structure of steel?

Responses


a)

b)

c)

d)

82.
a)

Luster


b)

Brittleness

c)

High melting point


d)

Solubility in water


83.

The BF3 molecule is nonpolar, whereas the NF3 molecule is polar. Which of the following statements accounts for the difference in polarity of the two molecules?

Responses


a)

In NF3, each F is joined to N with multiple bonds, whereas in BF3 , each F is joined to B with single bonds.

b)

N — F bonds are polar, whereas B — F bonds are nonpolar.


c)

NF3 is an ionic compound, whereas BF3 is a molecular compound.


d)

Unlike BF3, NF3 has a nonplanar geometry due to an unshared pair of electrons on the N atom.

84.

The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom?

a)

H2S

b)

NH3

c)

HCN

d)

CO2

85.
a)

Elemental carbon is harder than elemental iron.


b)

The additional carbon atoms within the alloy make the high-carbon steel less dense.


c)

The additional carbon atoms within the alloy increase the thermal conductivity of the high-carbon steel.

d)

The additional carbon atoms within the alloy make it more difficult for the iron atoms to slide past one another.

86.
a)

I and II only


b)

I and III only


c)

II and III only


d)

I, II, and III


87.

Which of the following is a nonpolar molecule that contains polar bonds?


a)

CHF3


b)

CO2

c)

HCl

d)

NH3


88.

Which of the molecules represented below contains carbon with sp2 hybridization?


a)

CH2Cl2

b)

C2H6

c)

C2H2Cl2


d)

C2H4Cl2


89.

Which of the following best helps to explain why the value of ΔH° for the dissolving of CaF2 in water is positive?


a)

CaF2(s) is insoluble in water.


b)

CaF2(s) dissolves in water to form CaF2(aq) particles.


c)

Ca2+ ions have very strong ion-ion interactions with F- ions in the crystal lattice.


d)

Ca2+ ions have very strong ion-dipole interactions with water molecules in the solution.

90.

Which of the following has a zero dipole mo­ment?


a)

HCN


b)

SO2

c)

NO2


d)

PF5

91.

Which of the following species is NOT planar?

a)

CO32-

b)

NO3-

c)

ClF3


d)

PCl3


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