Bonding Practice Problems

Name:

Multiple Choice

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

For an atom of a main group element, the number of valence electrons is equal to

a.	its number of core electrons.
b.	the principle quantum number of its outer shell.
c.	its period number.
d.	its group number.
e.	eight minus its group number.

Which combination of atoms is most likely to produce a compound with ionic bonds?

a.	Al and F
b.	P and H
c.	C and O
d.	Si and O
e.	S and Br

Which of the following statements are CORRECT?

1.	Ionic bonds form when one or more valence electrons are transferred from one atom to another.
2.	Covalent bonds involve sharing of electrons between atoms.
3.	Ionic bond formation is always exothermic; covalent bond formation is always endothermic.

a.	1 only
b.	2 only
c.	3 only
d.	1 and 2
e.	1, 2, and 3

Which of the following compounds is expected to have the strongest ionic bonds?

a.	RbF
b.	NaF
c.	NaI
d.	CsBr
e.	CsI

Which of the following molecules or ions are isoelectronic: SO₂, CO₂, NO₂^-, ClO₂^-?

a.	SO₂ and CO₂
b.	SO₂ and NO₂^-
c.	CO₂ and ClO₂^-
d.	NO₂^- and ClO₂^-
e.	SO₂, NO₂^-, and ClO₂^-

If two or more species have the same number of electrons resulting in similar Lewis structures, they are said to be ____.

a.	neutral
b.	resonant structures
c.	symmetric
d.	isoelectronic
e.	covalent

Which of the following species will have a Lewis structure most like that of the hydronium ion, H₃O⁺?

a.	NO₃^-
b.	NH₃
c.	SO₃
d.	CO₃^2-
e.	H₂CO

Which of the following is a correct Lewis structure for ozone, O₃?

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

Which of the following is a correct Lewis structure for the phosphate ion?

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

10.

Which of the following are resonance structures for the formate ion, HCO₂^-?

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

11.

Which of the following elements is most likely to form a molecular structure that disobeys the octet rule?

a.	B
b.	C
c.	N
d.	O
e.	F

12.

When both of the electrons in a molecular bond originate from the same atom, the bond is called a(n)

a.	double bond.
b.	coordinate covalent bond.
c.	pi bond.
d.	sigma bond.
e.	ionic bond.

13.

The central atom in XeF₄ is surrounded by

a.	3 single bonds, 1 double bond, and no lone pairs of electrons.
b.	2 single bonds, 2 double bonds, and no lone pairs of electrons.
c.	3 single bonds, 1 double bond, and 1 lone pair of electrons.
d.	4 single bonds, no double bonds, and no lone pairs of electrons.
e.	4 single bonds, no double bonds, and 2 lone pairs of electrons.

14.

Use VSEPR theory to predict the molecular geometry of H₃O⁺.

a.	trigonal-pyramidal
b.	trigonal-planar
c.	bent
d.	T-shaped
e.	linear

15.

Use VSEPR theory to predict the molecular geometry of CS₂.

a.	linear
b.	bent
c.	trigonal-planar
d.	tetrahedral
e.	octahedral

16.

Use VSEPR theory to predict the molecular geometry of IF₅.

a.	tetrahedral
b.	see-saw
c.	trigonal-bipyramidal
d.	square-pyramidal
e.	octahedral

17.

Use VSEPR theory to predict the molecular geometry of CO₃^2-.

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

18.

What are the Cl-P-Cl bond angles in PCl₃?

a.	109.5°
b.	120°
c.	109.5° and 120°
d.	90° and 120°
e.	90° and 180°

19.

What is the bond angle in N₂O?

a.	90°
b.	107°
c.	109.5°
d.	120°
e.	180°

20.

Place the following molecules in order from smallest to largest bond angles: NH₄⁺, NH₃, and NH₂^-.

a.	NH₄⁺ < NH₃ < NH₂^-
b.	NH₄⁺ < NH₂^- < NH₃
c.	NH₂^- < NH₃ < NH₄⁺
d.	NH₂^- < NH₄⁺ < NH₃
e.	NH₃ < NH₂^- < NH₄⁺

21.

What is the formal charge on each atom in a hypobromite ion, OBr^-?

a.	O = -2, Br = -1
b.	O = -2, Br = +1
c.	O = -1, Br = +1
d.	O = -1, Br = 0
e.	O = 0, Br = -1

22.

One resonance structure for thiocyanate ion is drawn below. What is the formal charge on each atom?

a.	S = 0, C = -1, N = 0
b.	S = 0, C = 0, N = -1
c.	S = -1, C = 0, N = 0
d.	S = 0, C = +2, N = -3
e.	S = -2, C = +4, N = -3

23.

Predict which of the following compounds will have the most polar covalent bond(s).

a.	HF
b.	CBr₄
c.	H₂S
d.	NCl₃
e.	HI

24.

Which one of the following molecules has a dipole moment?

a.	CI₄
b.	PF₅
c.	NCl₃
d.	SO₃
e.	O₂

25.

In molecules, as bond order increases,

a.	both bond length and bond energy increase.
b.	both bond length and bond energy decrease.
c.	bond length increases and bond energy is unchanged.
d.	bond length is unchanged and bond energy increases.
e.	bond length decreases and bond energy increases.

26.

How many sigma (s) bonds and pi (p) bonds are in the following molecule?

a.	five s and two p
b.	five s and three p
c.	five s and five p
d.	seven s and two p
e.	seven s and three p

27.

How many sigma (s) bonds and pi (p) bonds are in acetic acid?

a.	six s and one p
b.	six s and two p
c.	seven s and one p
d.	eight s and zero p
e.	eight s and one p

28.

To form a set of sp³d² hybrid atomic orbitals, what set of pure atomic orbitals must be mixed?

a.	one s, one p, and one d
b.	one s, three p, and one d
c.	one s, three p, and two d
d.	two s, six p, and two d
e.	two s, six p, and four d

29.

What is the maximum number of hybridized orbitals formed by an oxygen atom?

a.	2
b.	3
c.	4
d.	5
e.	6

30.

What is the hybridization of the carbon atom in carbon disulfide?

a.	sp
b.	sp²
c.	sp³
d.	sp³d
e.	sp³d²

31.

What is the hybridization of the sulfur atom in SO₂?

a.	sp
b.	sp²
c.	sp³
d.	sp³d
e.	sp³d²

32.

What is the hybridization of the sulfur atom in SF₄?

a.	sp
b.	sp²
c.	sp³
d.	sp³d
e.	sp³d²

33.

What is the hybridization of the central atom in a molecule with a square-planar molecular geometry?

a.	sp
b.	sp²
c.	sp³
d.	sp³d
e.	sp³d²

34.

What is the hybridization of the central atom in a molecule with a trigonal-planar geometry?

a.	sp
b.	sp²
c.	sp³
d.	sp³d
e.	sp³d²

35.

In which of the following molecules and ions does the central carbon atom have sp hybridization: Cl₂CO, CH₂Br₂, CO₂, and OCN^-?

a.	Cl₂CO only
b.	Cl₂CO and CH₂Br₂
c.	CH₂Br₂ and CO₂
d.	CH₂Br₂ and OCN^-
e.	CO₂ and OCN^-

36.

What is the molecular geometry around a central atom that is sp³ hybridized and has one lone electron-pair?

a.	bent
b.	linear
c.	trigonal-planar
d.	trigonal-pyramidal
e.	trigonal-bipyramidal

37.

What is the molecular geometry around a central atom that is sp² hybridized, has three sigma bonds, and has one pi bond?

a.	trigonal-planar
b.	trigonal-pyramidal
c.	trigonal-bipyramidal
d.	linear
e.	tetrahedral

38.

What is the molecular geometry around a central atom that is sp³d hybridized and has three sigma bonds and two lone electron-pairs?

a.	linear
b.	trigonal-pyramidal
c.	trigonal-planar
d.	tetrahedral
e.	T-shaped

39.

What is the molecular geometry around a central atom that has four sigma bonds and has no lone electron-pairs?

a.	square-pyramidal
b.	tetrahedral
c.	trigonal-planar
d.	square-planar
e.	see-saw

40.

Which of the following characteristics apply to PCl₃?

1.	nonpolar molecule
2.	polar bonds
3.	trigonal-pyramidal molecular geometry
4.	sp² hybridized

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

41.

Which of the underlined atoms (C₁, C₂, N, and O) are sp² hybridized?

a.	C₁ and C₂
b.	C₁, N, and O
c.	N and O
d.	O and C₂
e.	O only

42.

Which of the following statements are CORRECT?

1.	A paramagnetic substance is attracted to a magnetic field.
2.	Atoms with one or more unpaired electrons are paramagnetic.
3.	Electron spin is quantized.

a.	1 only
b.	2 only
c.	3 only
d.	1 and 2
e.	1, 2, and 3

43.

Which of the following statements are CORRECT?

1.	Substances that retain their magnetism after they are withdrawn from a magnetic field are called ferromagnetic.
2.	A diamagnetic substance is slightly repelled by a magnetic field.
3.	An atom with an even number of electrons is diamagnetic.

a.	1 only
b.	2 only
c.	3 only
d.	1 and 2
e.	1, 2, and 3

44.

Which of the following atoms is paramagnetic?

a.	Se
b.	Cd
c.	Ar
d.	He
e.	Ca