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AP Bonding Test & Atomic Structure Review

Total questions: 85

Worksheet time: 6hrs 57mins

Name
Class
Date
1.

As the number of bonds between two carbon atoms increases, which one of the following decreases?

a)

number of electrons between the carbon atoms

b)

bond energy

c)

bond length

d)

all of these

e)

None of these

2.

Which of the following atoms cannot exceed the octet rule in a molecule?

a)

N

b)

S

c)

P

d)

I

e)

All of these atoms can exceed the octet rule

3.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

4.

Is BCl3 polar or non-polar?

a)

Non-polar

b)

Polar

5.

Which of the following types of molecules always has a dipole moment (Polarity)?

a)

Linear molecules with two identical bonds.

b)

Tetrahedral molecules (four identical bonds equally spaced).

c)

Trigonal pyramid molecules (three identical bonds).

d)

Trigonal planar molecules (three identical bonds equally spaced).

e)

None has a dipole moment.

6.

Which of the following exhibits resonance?

a)

NH3

b)

PCl5

c)

H2O

d)

O3

e)

At least two of the molecules (A-D) exhibit resonance.

7.

Which ion is larger in each pair?

i) O2- or S2- ii) Fe2+ or Fe3+ iii) S2- or K+

a)

S2-, Fe2+, S2-

b)

S2-, Fe3+, S2-

c)

O2-, Fe3+, K+

d)

S2-, Fe2+, K+

e)

O2-, Fe2+, S2-

8.

A p (pi) bond is the result of the

a)

overlap of two s orbitals

b)

overlap of an s orbital and a p orbital

c)

overlap of two p orbitals along their axes

d)

sidewise overlap of two parallel p orbitals

e)

sidewise overlap of two s orbitals

9.

When a carbon atom, with no lone pairs, has sp2 hybridization, it has

a)

three single bonds

b)

three single bonds and one double bond

c)

two single bonds and a double bonds

d)

two double bond and two single bonds

e)

four single bonds

10.

What is the formal charge on the xenon atom in the following structure?

a)

-2

b)

-1

c)

0

d)

+1

11.

Consider the statements below about trigonal pyramidal molecular geometry:

I. Trigonal pyramidal molecular geometry has the same number of bonding domains as trigonal planar molecular geometry.

II. Trigonal pyramidal molecular geometry has the same number of total electron domains as tetrahedral molecular geometry.

III. Trigonal pyramidal molecular geometry has the same number of lone pair domains as bent molecular geometry (trigonal planar electron geometry)

IV. Trigonal pyramidal molecular geometry has all of the atoms in the same plane.

Which of the above statements are true?

a)

I, III, IV

b)

I, II, III

c)

III and IV

d)

III only

12.

Which of the following structures has two lone pairs around the central atom?

a)

BrF3

b)

XeF2

c)

BrF5

d)

IOF5

13.

Which statement(s) below can be used to explain why the bond angles in the following series of molecules (CCl4, NF3, and H2O) decrease steadily?


I. The electron domains around the central atom decreases as the bond angle decreases.

II. The terminal atoms have different electronegativity values, and thus, repel one another with different forces.

III. The electron densities associated with lone pairs are concentrated closer to the central atom than those of bonding pairs, causing a larger force of repulsion that pushes the terminal atoms closer together.

a)

I only

b)

II only

c)

III only

d)

I and III only

14.

Which of the following bonds has the longest bond length?

a)

N-O

b)

H-F

c)

H-Cl

d)

H-I

15.

What is the formal charge on the sulfur atom?

a)

-1

b)

0

c)

+1

d)

+2

16.

What is the formal charge on the nitrogen atom?

a)

-3

b)

-1

c)

0

d)

+1

17.

Which of the following groups contains no ionic compounds?

a)

HCN, NO2, Ca(NO3)2

b)

PCl5, LiBr, Zn(OH)2

c)

KOH, CCl4, SF4

d)

NaH, CaF2, NaNH2

e)

CH2O, H2S, NH3

18.

Which of the following bonds is least polar?

a)

C—O

b)

H—C

c)

S—Cl

d)

Br—Br

e)

They are all nonpolar.

19.

In which case is the bond polarity incorrect?

a)

d+H–Fd–

b)

d+K–Od–

c)

d+Mg–Hd–

d)

d+Cl–Id–

e)

d+Si–Sd–

20.

Which of the following bonds would be the most polar without being considered ionic?

a)

Mg-O

b)

C-O

c)

O-O

d)

Si-O

e)

N-O

21.

Which of the following statements is incorrect?

a)

Ionic bonding results from the transfer of electrons from one atom to another.

b)

Dipole moments result from the unequal distribution of electrons in a molecule.

c)

The electrons in a polar bond are found nearer to the more electronegative element.

d)

molecule with very polar bonds can be nonpolar.

e)

Linear molecules cannot have a net dipole moment.

22.

Which of the following molecules has no dipole moment?

a)

CO2

b)

NH3

c)

H2O

d)

all

e)

none

23.

Which of the following has the smallest radius?

a)

K+

b)

Cl–

c)

Rb+

d)

S2–

e)

Ar

24.

Choose the molecule with the strongest bond.

a)

CH4

b)

H2O

c)

NH3

d)

LiF

25.

As indicated by Lewis structures, which of the following would probably not exist as a stable molecule?

a)

C3H4

b)

CH2O

c)

CH3O

d)

C2H2

26.
a)

4, 2

b)

6, 3

c)

11, 5

d)

11, 2

e)

13, 0

27.

Which of the molecules obeys the octet rule?

a)

I

b)

II

c)

III

d)

IV

e)

V

28.

Which of these molecules show resonance?

a)

I, II

b)

II, IV

c)

II, V

d)

III, IV

e)

III, V

29.

How many of the molecules have no dipole moment: Br2, CH4, NH3, SO3 and CH3Cl ?

a)

1

b)

2

c)

3

d)

4

e)

They are all polar

30.

This molecule contains a carbon atom with trigonal planar geometry.

a)

CH3CHO

b)

CO2

c)

CH3Cl

d)

C2H6

e)

none of these

31.

This molecule shows the smallest number of lone pairs in its Lewis structure.

a)

CH3CHO

b)

CO2

c)

CH3Cl

d)

C2H6

32.

Which of the following molecules contains a double bond?

a)

CO2

b)

NH3

c)

H2O

d)

all

e)

none

33.

The Lewis structure for CHCl3 has nine lone electron pairs.

a)

True

b)

False

34.

As indicated by Lewis structures, which of the following species could probably not exist as a stable molecule?

a)

N2O4

b)

N2H2

c)

N2H4

d)

N2H6

35.

Which of the following has an incomplete octet in its Lewis structure?

a)

SO2

b)

ICl

c)

CO2

d)

F2

e)

NO

36.

In the cyanide ion (CN–), the nitrogen has a formal charge of

a)

-2

b)

-1

c)

0

d)

2

37.

How many resonance structures can be drawn for the molecule O3?

a)

1

b)

2

c)

3

d)

4

e)

5

38.

How many of the following molecules possess dipole moments?

BH3, CH4, PCl5, H2O, HF, H2

a)

1

b)

2

c)

3

d)

4

e)

5

39.

Which of the following statements are true?


I. The electrons in each molecule tend to orient themselves around the most electronegative element.


II. Each molecular drawing follows the localized electron model.


III. Both HF and CO2 are linear molecules and therefore polar.


IV. The bond angles of NH3 are slightly less than 109.5° because the lone pair compresses the angles between the bonding pairs.

a)

I, III, IV

b)

I, II, IV

c)

I, II, III

d)

II, IV

40.

Which ion is planar?

a)

NH4+

b)

CO32–

c)

SO32–

d)

ClO3–

41.

The bond angles about the carbon atom in the formaldehyde molecule, H2C=O, are about:

a)

120°

b)

60°

c)

109°

d)

180°

e)

90°

42.

SiH4

a)

pyramidal

b)

tetrahedral

c)

square planar

d)

octahedral

43.

ClO2

a)

pyramidal

b)

tetrahedral

c)

square planar

d)

octahedral

e)

none of these

44.

Atoms that are sp2 hybridized have how many unhybridized p orbitals that could form pi bond(s).

a)

0

b)

1

c)

2

d)

3

e)

4

45.

What hybridization is predicted for the nitrogen atom in the NO3– ion?

a)

sp2

b)

sp3

c)

dsp3

d)

sp

e)

none of these

46.

Which of the following does not contain at least one pi bond?

a)

H2CO

b)

CO2

c)

C2H4

d)

C2H6

e)

All of the above (A-D) contain at least one pi bond

47.

What is the hybridization of the carbon atom that is double-bonded to oxygen?

a)

sp

b)

sp2

c)

sp3

d)

dsp3

48.

What is the hybridization of the nitrogen atom?

a)

sp

b)

sp2

c)

sp3

d)

dsp3

49.

What is the hybridization of the oxygen atom?

a)

sp

b)

sp2

c)

sp3

d)

dsp3

50.

This molecule has __________ sigma and __________ pi bonds.

a)

4, 5

b)

6, 3

c)

11, 5

d)

13, 2

e)

13, 3

51.

The hybridization of the B in BH3 is sp3.

a)

True

b)

False

52.

Which of the following molecules contains the shortest C–C bond?

a)

C2H2

b)

C2H4

c)

C2H6

d)

C2Cl4

53.

Larger bond order means greater bond strength.

a)

True

b)

False

54.

As the bond order of a bond increases, the bond energy ______ and the bond length ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

55.

If a molecule demonstrates paramagnetism, then :


I. The substance must have unpaired electrons in it's valence shell.

II. The bond order is not a whole number.

III. It can be determined by drawing a Lewis structure.

IV. It must be an ion.

a)

I, II

b)

I, II, IV

c)

II, III

d)

I only

e)

All of the above are correct.

56.

Which of the following species is paramagnetic?

a)

C2

b)

O2

c)

F2

d)

Li2

e)

none of these

57.

Which of the following diatomic molecules has a bond order of 2?

a)

B2

b)

C2

c)

P2

d)

F2

e)

Li2

58.

Order the following from shortest to longest bond:

C2, B2, H2, N2

a)

H2, N2, C2, B2

b)

N2, C2, B2, H2

c)

C2, N2, H2, B2

d)

C2, B2, H2, N2

59.

Which of the following statements about the molecule BN is false?

a)

It is paramagnetic.

b)

Its bond order is 2.

c)

The total number of electrons is 12.

d)

It has two pi bonds

e)

All of these are true.

60.

Which of these statements about benzene (C6H6) is true?

a)

All carbon atoms in benzene are sp3 hybridized.

b)

Benzene contains only pi bonds between C atoms.

c)

The bond order of each C–C bond in benzene is 1.5.

d)

All C in Benzene have an electron geometry of tetrahedral because they form 4 bonds each.

61.

How many of the following molecules or ions are linear?


NH3 OF2 HCN CO2 NO2

a)

0

b)

1

c)

2

d)

3

e)

4

62.

According to VSEPR theory, which of the following species has a square planar molecular structure?

a)

TeBr4

b)

BrF3

c)

IF5

d)

XeF4

e)

SCl2

63.

NO3–

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

bent

e)

none of these

64.

SF4

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

bent

e)

none of these

65.

Atoms that are sp hybridized have how many unhybridized p orbitals that could form pi bond(s).

a)

0

b)

1

c)

2

d)

3

e)

4

66.

What is the total maximum number of atomic orbitals possible in an atom with the highest principal quantum number n = 3?

a)

3

b)

13

c)

14

d)

15

67.

The electronic configuration of an element QQ is: ...3s23p63d104s24p3. This means that the element QQ is...

a)

a d-block element

b)

a Group 13 element

c)

a Group 5 element

d)

a Group 15 element

68.

What is the electronic configuration of the N3- ion?

a)

1s22s22p3

b)

1s22s22p6

c)

1s22s22p63s23p2

d)

1s22s22p63s23p6

69.

All the following species have the same number of electrons except...

a)

F

b)

Ne

c)

Na+

d)

Al3+

70.

Which of the following elements does not have paired electrons in the p orbitals of its atom?

a)

Carbon

b)

Oxygen

c)

Aluminium

d)

Silicon

71.

How many unpaired electrons are found in one chromium atom in the ground state?

a)

3

b)

4

c)

5

d)

6

72.

States that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers.

a)

Heisenberg's Uncertainty Principle

b)

Aufbau Principle

c)

Pauli Exclusion Principle

d)

Hund's rule

73.

How many d orbitals have the value n = 2?

a)

0

b)

3

c)

5

d)

1

74.

How many electrons can be contained in all of the orbitals with n = 4?

a)

2

b)

8

c)

10

d)

18

e)

32

75.

Of the following elements, which has occupied d orbitals in its ground-state neutral atoms?

a)

Ba

b)

Ca

c)

Si

d)

P

e)

Cl

76.

Which of the following have 10 electrons in the d orbitals?

a)

Mn

b)

Fe

c)

Cu

d)

Zn

e)

Two of these do

77.

Which of the following atoms would have the largest second ionization energy?

a)

Mg

b)

Cl

c)

S

d)

Ca

e)

Na

78.

The first ionization energy of Mg is 735 kJ/mol. The second ionization energy is

a)

735 kJ/mol

b)

less than 735 kJ/mol

c)

greater than 735 kJ/mol

d)

More information is needed to answer this question.

e)

None of these.

79.

Which of the following is the highest energy orbital for a silicon atom?

a)

1s

b)

2s

c)

3s

d)

3p

e)

3d

80.

Select the correct electron configuration for Cu.

a)

[Ar]4s23d9

b)

[Ar]4s13d10

c)

[Ar]4s24p63d3

d)

[Ar]4s24d9

e)

[Ar]3d10

81.

Which of the following statements is true?

a)

The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer.

b)

The krypton 1s orbital is larger than the helium 1s orbital because krypton contains more electrons.

c)

The krypton 1s orbital is smaller than the helium 1s orbital because krypton's p and d orbitals crowd the s orbitals.

d)

The krypton 1s orbital and helium 1s orbital are the same size because both s orbitals can only have two electrons.

e)

The krypton 1s orbital is larger than the helium 1s orbital because krypton's ionization energy is lower, so it's easier to remove electrons.

82.

Which of the following atoms has the largest ionization energy?

a)

O

b)

Li

c)

Ne

d)

Be

e)

K

83.

The picture represents the photoelectric spectrum of an particular element in its ground state. Which subshell contains the most electrons?

a)

1s

b)

2p

c)

3s

d)

2s

e)

3p

84.

The picture represents the photoelectric spectrum of an particular element in its ground state. What element does these data represent?

a)

Beryllium

b)

Carbon

c)

Magnesium

d)

Aluminum

e)

Lithium

85.

States that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and that each of the single electrons must have the same spin.

a)

Heisenberg's Uncertainty Principle

b)

Aufbau Principle

c)

Pauli Exclusion Principle

d)

Hund's rule

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