Chapter 1 -- Bonding and Isomerism

MULTIPLE CHOICE

	1.	What is the most electropositive element?
A)	Li	
B)	Be	
C)	B	
D)	C	
E)	N	

ANS:	A	TOP:	Valence, Bonding, and Lewis Structures	

	2.	Which of the following elements has three electrons in the valence (outer) shell?
A)	C	
B)	B	
C)	S	
D)	F	
E)	N	

ANS:	B	TOP:	Valence, Bonding, and Lewis Structures	

	3.	Which of the following would you expect to have ionic bonds?
A)	HBr	
B)	CO	
C)	ICl	
D)	CsF	
E)	NF3	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	4.	Which of the following would you expect to have polar covalent bonds?
A)	MgF2	
B)	N2	
C)	F2	
D)	NF3	
E)	NaF	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	5.	Which molecule has nonpolar covalent bonds?
A)	NO	
B)	N2	
C)	BCl3	
D)	HF	
E)	CCl4	

ANS:	B	TOP:	Valence, Bonding, and Lewis Structures	

	6.	The number of electrons in the valence shell of sulfur is:
A)	2	
B)	3	
C)	4	
D)	5	
E)	6	

ANS:	E	TOP:	Valence, Bonding, and Lewis Structures	

	7.	Which of the following elements is the most electronegative?
A)	O	
B)	S	
C)	Se	
D)	Te	
E)	Po	

ANS:	A	TOP:	Valence, Bonding, and Lewis Structures	

	8.	If the Cl–Cl bond length is 1.98Å and the C–C bond length is 1.54Å, what would you expect the bond length of Cl–C to be?
A)	0.74Å	
B)	1.54Å	
C)	1.76Å	
D)	1.98Å	
E)	3.52Å	

ANS:	C	TOP:	Valence, Bonding, and Lewis Structures	

	9.	Given the following electronegativity values, predict the most polar covalent bond below:

F	4.0	
Cl	3.0	
O	3.5	
C	2.5	
H	2.1	

A)	–F	
B)	C–Cl	
C)	C–O	
D)	C–H	
E)	C–C	

ANS:	A	TOP:	Valence, Bonding, and Lewis Structures	

	10.	The most electronegative elements in the periodic table are generally found
A)	toward the left in a horizontal row and toward the top in a column.	
B)	toward the right in a horizontal row and toward the top in a column.	
C)	toward the left in a horizontal row and toward the bottom in a column.	
D)	toward the right in a horizontal row and toward the bottom in a column.	
E)	distributed randomly throughout the table.	

ANS:	B	TOP:	Valence, Bonding, and Lewis Structures	

	11.	Which of the following Lewis Structures for ozone (O3) is incorrect?
A)	
	
B)	
	
C)	
	
D)	structures (A) and (B) are incorrect	
E)	none of the above structures are incorrect	

ANS:	C	TOP:	Valence, Bonding, and Lewis Structures	

	12.	Which of the following molecules are structural isomers?

A)	1, 2, and 4	
B)	1, 2, and 3	
C)	1, 3, and 4	
D)	2, 3, and 4	
E)	3 and 4	

ANS:	B	TOP:	Valence, Bonding, and Lewis Structures	

	13.	Which of the following abbreviated structural formulas is NOT an isomer of the others?
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	14.	The number of possible acyclic hydrocarbons with the molecular formula C4H6 is
A)	2	
B)	3	
C)	4	
D)	5	
E)	6	

ANS:	C	TOP:	Valence, Bonding, and Lewis Structures	

	15.	Which of the following structural formulas represents a structural isomer of CH3CH2CH2CH2CH3?
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	16.	Which of the following molecules are structural isomers?

A)	1, 2 and 3	
B)	1, 3 and 4	
C)	2, 3 and 5	
D)	1, 3 and 5	
E)	2 and 3	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	17.	Which of the following abbreviated structural formulas represents a structural isomer of CH3CH2CH2CH2CH3?
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	B	TOP:	Valence, Bonding, and Lewis Structures	

	18.	The structural formula for (CH3)2C(CH2CH3)2 is
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	19.	The structural formula  has the molecular formula:

A)	C7H16	
B)	C6H14	
C)	C7H14	
D)	C6H12	
E)	C7H10	

ANS:	E	TOP:	Valence, Bonding, and Lewis Structures	

	20.	Which of the following structural formulas does not have the molecular formula C6H14?
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	D	TOP:	Valence, Bonding, and Lewis Structures	

	21.	Which of the following structural formulas has the molecular formula C6H12?

	

A)	2 and 3	
B)	1 and 4	
C)	1, 4, and 5	
D)	1 and 2	
E)	4 and 5	

ANS:	C	TOP:	Valence, Bonding, and Lewis Structures	

	22.	The structural formula for (CH3CH2)2CHCH2CH(CH3)2 is
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	B	TOP:	Valence, Bonding, and Lewis Structures	

	23.	The structural formula  has the molecular formula:

A)	C7H16	
B)	C6H14	
C)	C7H14	
D)	C6H12	
E)	C7H10	

ANS:	E	TOP:	Valence, Bonding, and Lewis Structures	

	24.	The structural formula  has the molecular formula:

A)	C10H16	
B)	C9H16	
C)	C11H22	
D)	C9H14	
E)	C10H18	

ANS:	E	TOP:	Valence, Bonding, and Lewis Structures	

	25.	For carbon monoxide, , C has a formal charge of:

A)	+1	
B)	–1	
C)	0	
D)	–2	
E)	+2	

ANS:	B	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	26.	For carbon monoxide, , O has a formal charge of:

A)	+1	
B)	–1	
C)	0	
D)	–2	
E)	+2	

ANS:	A	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	27.	What is the formal charge of N in HNO3, as seen below?

A)	+1	
B)	+2	
C)	0	
D)	–1	
E)	–2	

ANS:	A	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	28.	The formal charges in the perchlorate ion are:

A)	–1 on each O and +3 on the Cl.	
B)	0 on each O and –1 on the Cl.	
C)	–1 on each O and +4 on the Cl.	
D)	–1/4 on each O and 0 on the Cl.	
E)	+1 on each O and –1 on the Cl.	

ANS:	A	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	29.	Which of the following structures is a resonance structure of :

A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	C	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	30.	The formal charges in the complex  are:

A)	0 on each H, +1 on N, and –1 on B.	
B)	+1 on each H, +1 on N, and –1 on B.	
C)	0 on each H, –1 on N, and +1 on B.	
D)	0 on each H, 0 on N, and 0 on B.	
E)	–1 on each H, +3 on N, and +3 on B.	

ANS:	A	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	31.	The curved arrows in the resonance structure for the acetate ion shown below indicate the following alternative resonance structure for the acetate ion:

A)	
	D)	
	
B)	
	E)	
	
C)	

ANS:	C	TOP:	Formal Charge, Resonance, and Curved-Arrow Formalism

	32.	What is the percent s character in an sp2 hybridized orbital?
A)	25%	
B)	33%	
C)	50%	
D)	67%	
E)	75%	

ANS:	B	TOP:	Electronic Structure and Molecular Geometry

	33.	The maximum number of electrons that a molecular orbital can contain is:
A)	1	
B)	2	
C)	3	
D)	4	
E)	5	

ANS:	B	TOP:	Electronic Structure and Molecular Geometry

	34.	The approximate H–C–H bond angle in methane is:
A)	60°	
B)	90°	
C)	109.5°	
D)	120°	
E)	180°	

ANS:	C	TOP:	Electronic Structure and Molecular Geometry

	35.	The Lewis structure of methane is

The shape of the methane can be described as a
A)	square planar	
B)	trigonal planar	
C)	trigonal pyramidal	
D)	tetrahedral	
E)	square pyramidal	

ANS:	D	TOP:	Electronic Structure and Molecular Geometry

	36.	Which of the following molecules can be classified as an amide?
A)	
	
B)	
	
C)	
	
D)	
	
E)	Answers A and D	

ANS:	B	TOP:	Classification of Organic Compounds	

	37.	Which of the following molecules contain the same functional group?

CH3OH 	CH3OCH3	CH3CH2OH	CH3CH(OH)CH3	
1	2	3	4	

A)	1, 2 and 3	
B)	1, 3 and 4	
C)	1 and 2	
D)	2 and 4	
E)	3 and 4	

ANS:	B	TOP:	Classification of Organic Compounds	

	38.	Which of the following molecules is acyclic?
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	B	TOP:	Classification of Organic Compounds	

	39.	Which of the following molecules is heterocyclic?
A)	
	
B)	
	
C)	
	
D)	
	
E)	

ANS:	A	TOP:	Classification of Organic Compounds	

	40.	Which of the following molecules contain the same functional group? 

A)	2 and 3	
B)	1, 2 and 4	
C)	2 and 4	
D)	1 and 2	
E)	1 and 4	

ANS:	E	TOP:	Classification of Organic Compounds