Test Bank Organic Chemistry A Short Course, 13th Edition Harold Hart A+

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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