Gen Chemistry Bonds, Properties Verified Test Bank Chapter 1

Organic Chemistry, 4e (Klein)

Chapter 1 A Review of General Chemistry: Electrons, Bonds, and Molecular Properties

1) Chemical reactions occur as a result of ________.

A) the attraction between opposite charges

B) the nucleus—nucleus interactions

C) the motion of electrons

D) like atoms interacting

E) combining two chemicals

Diff: 1

Learning Objective: 1.1 Compare and contrast organic and inorganic compounds

2) From the following, identify the item which does not contain organic compounds.

A) medicine

B) socks

C) a plant

D) a coin

E) a plastic cup

Diff: 1

Learning Objective: 1.1 Compare and contrast organic and inorganic compounds

3) What is the difference between inorganic and organic compounds?

A) organic compounds do not contain carbon

B) organic compounds contain carbon

C) organic compounds are without pesticides

D) inorganic compounds contain carbon

E) inorganic compounds are composed exclusively of transition metal elements

Diff: 1

Learning Objective: 1.1 Compare and contrast organic and inorganic compounds

4) Constitutional isomers do not differ in ________.

A) physical properties

B) atomic connectivity

C) molecular formula

D) name

E) constitution

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

5) What is the relationship between the following compounds?

A) isotopes

B) constitutional isomers

C) the same structure

D) composed of different elements

E) no relationship

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

6) What is the relationship between the following compounds?

A) resonance isomers

B) constitutional isomers

C) empirical isomers

D) isotopes

E) There is no relationship

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

7) Carbon is considered to be ________.

A) tetravalent

B) divalent

C) trivalent

D) monovalent

E) pentavalent

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

8) Which of the following compounds are constitutional isomers of each other?

A) I and II

B) III and IV

C) I, II and IV

D) II, III and IV

E) I, II, and III

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

9) Which of the following compounds are constitutional isomers of each other?

A) I and II

B) II and III

C) III and IV

D) I and IV

E) II and IV

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

10) Identify three constitutional isomers having the molecular formula C4H8BrCl.

A) I, II, and III

B) II, III, and IV

C) III, IV, and V

D) I, III, and V

E) II, III, and V

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

11) Identify three constitutional isomers having the molecular formula C4H8O.

A) I, II, and III

B) II, III, and IV

C) III, IV, and V

D) I, II, and IV

E) II, III, and V

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

12) What force is not considered in the formation of a covalent bond?

A) repulsion between two positively charged nuclei

B) force of attraction between positively charged nuclei and negatively charged electrons

C) repulsion between negatively charged electrons

D) repulsion between positively charged nuclei and negatively charged electrons

E) the distance between the atoms' nuclei

Diff: 1

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

13) What is the correct Lewis dot structure for the sulfur atom, S?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

14) What is the correct Lewis dot structure for the carbon atom, C?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

15) What is the correct Lewis structure for the molecule shown in the box below?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

16) What is the correct Lewis structure for the molecule shown in the box below?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

17) What is the correct Lewis structure for the molecule shown in the box below?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

18) Which of the following compounds has two lone pairs on the central atom?

A) CO2

B) SCl2

C) NF3

D) CS2

E) SO3

Diff: 2

Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair

19) What is the formal charge on oxygen in the following structure?

A) 2-

B) 1-

C) 2+

D) 1+

E) 0

Diff: 1

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

20) What is the formal charge on nitrogen in the following structure?

A) 2-

B) 1-

C) 2+

D) 1+

E) 0

Diff: 1

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

21) What is the formal charge on oxygen in the following structure?

A) 0

B) 1+

C) 2+

D) 1-

E) 2-

Diff: 1

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

22) What is the formal charge on oxygen in the following structure?

A) 2+

B) 2-

C) 1+

D) 1-

E) 0

Diff: 1

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

23) Which of the following structures have a formal charge of zero on the carbon atom?

A) I and III

B) II and III

C) III and IV

D) I and IV

E) II and IV

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

24) Which of the following structures have a 1- formal charge on the sulfur atom?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

25) Which of the following structures have a 1+ formal charge on the sulfur atom?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

26) What are the formal charges on boron and nitrogen in the following structure?

A) B = 1+, N = 1+

B) B = 1+, N = 1-

C) B = 1-, N = 1-

D) B = 1-, N = 1+

E) B = 1-, N = 0

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

27) What are the formal charges on boron and oxygen in the following structure?

A) B = 1-, O = 1-

B) B = 1-, O = 1+

C) B = 1+, O = 1+

D) B = 1+, O = 1-

E) B = 1-, O = 0

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

28) Which of the following structures have 1+ formal charge on the central atom?

A) I

B) II

C) III

D) III and V

E) IV and V

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

29) Which of the following structures have a formal charge on at least one atom?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

30) Which of the following structures have a 1— formal charge on the nitrogen atom?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

31) The bonding pattern of oxygen with a formal charge of 1— could be described as ________.

A) one lone pair of electrons and three single bonds

B) two lone pairs of electrons and two single bonds

C) three lone pairs of electrons, and one single bond

D) one lone pair of electrons, one single, and one double bond

E) zero lone pairs, and two single and one double bond

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

32) What is the correct Lewis structure for the molecule in the box, including the formal charge(s), if any?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

33) What is the correct Lewis structure for the molecule in the box, including the formal charge(s), if any?

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

34) What is the correct Lewis structure for the molecule in the box, including the formal charge(s), if any?

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

35) What is the correct Lewis structure for the molecule in the box, including the formal charge(s), if any?

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

36) What is the correct Lewis structure for the molecule in the box, including the formal charge(s), if any?

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

37) Which of the following bond-line structures are of the same compound?

A) I and II

B) II and III

C) III and IV

D) I and III

E) II and IV

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

38) Which of the following bond-line structures represent the same compound?

A) I and II

B) II and III

C) III and IV

D) I and III

E) II and IV

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

39) The electronegativity of elements on the periodic table tends to increase ________.

A) from left to right, top to bottom

B) from right to left, bottom to top

C) from left to right, bottom to top

D) from right to left, top to bottom

E) from upper right to lower left

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

40) Which of the following is the least electronegative element?

A) B

B) C

C) N

D) O

E) F

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

41) Which of the following is the most electronegative element?

A) B

B) C

C) N

D) O

E) H

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

42) Which of the following is the least electronegative element?

A) P

B) N

C) Na

D) Si

E) K

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

43) Which of the following is the most electronegative element?

A) P

B) N

C) S

D) O

E) F

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

44) What is the correct order of increasing electronegativity for Rb, F and O?

A) Rb < F < O

B) Rb < O < F

C) O < F < Rb

D) F < Rb < O

E) O < Rb < F

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

45) Which of the following series has the correct order of elements in increasing electronegativity?

A) C < N < B < Br

B) P < N < As < F

C) Li < B < N < F

D) Cl < Cs < C < Co

E) Be < B < Ba < Br

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

46) The Cl–Cl bond is best described as ________.

A) nonpolar covalent

B) polar covalent

C) ionic

D) coordinate covalent

E) None of these.

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

47) The C–Cl bond is best described as ________.

A) nonpolar covalent

B) polar covalent

C) ionic

D) coordinate covalent

E) None of these.

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

48) The bond between potassium and oxygen is best described as ________.

A) nonpolar covalent

B) polar covalent

C) ionic

D) coordinate covalent

E) None of these.

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

49) The bond between carbon and hydrogen is best described as ________.

A) nonpolar covalent

B) polar covalent

C) ionic

D) coordinate covalent

E) None of these.

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

50) Which of the following is the correct depiction of the dipole moment for a C–F bond?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

51) Which of the following illustrates the correct placement of partial charges for a P–Cl bond?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

52) Which of the following is the correct representation of partial charges at the indicated atoms?

A) I = δ+; II = δ+; III = δ+

B) I = δ—; II = δ—; III = δ—

C) I = δ+; II = δ+; III = δ—

D) I = δ—; II = δ—; III = δ+

E) I = δ+; II = δ—; III = δ+

Diff: 2

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

53) Which atom has the largest δ+ in the following compound?

A) N

B) O

C) Br

D) H

E) C

Diff: 2

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

54) Which of the following statements best describes the C–Cl bond in the following compound?

A) nonpolar; no dipole

B) polar; δ+ at carbon and δ— at chlorine

C) polar; δ— at carbon and δ+ at chlorine

D) polar; δ— at carbon and δ— at chlorine

E) ionic

Diff: 2

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

55) Which of the following compounds have both polar covalent and ionic bonds?

A) NH4Br

B) H2O2

C) HCN

D) H2S

E) CH4

Diff: 2

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

56) How many hydrogen atoms are connected to the indicated carbon atom?

A) one

B) two

C) three

D) four

E) none

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

57) How many hydrogen atoms are connected to the indicated carbon atom?

A) one

B) two

C) three

D) four

E) none

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

58) For NaOCH3, identify each bond as polar covalent, nonpolar covalent or ionic.

A) NaO = polar covalent; OC = polar covalent; CH = nonpolar covalent

B) NaO = ionic; OC = polar covalent; CH = nonpolar covalent

C) NaO = ionic; OC = ionic; CH = nonpolar covalent

D) NaO = polar covalent; OC = nonpolar covalent; CH = polar covalent

E) NaO = polar covalent; OC = nonpolar covalent; CH = nonpolar covalent

Diff: 2

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

59) For the following compound, identify the polar covalent bond(s) from the options provided.

A) I and II

B) II and III

C) I and III

D) I only

E) II only

Diff: 2

Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds

60) Orbitals with the same energy are called ________.

A) quantum orbitals

B) atomic orbitals

C) antibonding orbitals

D) bonding orbitals

E) degenerate orbitals

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

61) What is the letter designation for the following atomic orbital?

A) s

B) p

C) d

D) f

E) g

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

62) How many hydrogen atoms are connected to the indicated carbon atom?

A) one

B) two

C) three

D) four

E) none

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

63) In quantum mechanics a node (nodal surface or plane) is the ________.

A) location where ψ is negative

B) location where ψ is positive

C) location where ψ2 is positive

D) location where ψ2 is negative

E) location where ψ is zero

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

64) Which of the following principle states that "Each orbital can accommodate a maximum of two electrons with opposite spin"?

A) Aufbau principle

B) Pauli exclusion principle

C) Hund's Rule

D) Heizenberg Uncertainty principle

E) Le Chatelier's principle

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

65) Which of the following principle states "When orbitals of equal energy are available, every orbital gets one electron before any gets two electrons"?

A) Aufbau principle

B) Pauli exclusion principle

C) Hund's Rule

D) Heizenberg Uncertainty principle

E) Le Chatelier's principle

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

66) Which of the following represents the ground state electron configuration for a phosphorous atom?

A) 1s22s22p63s13p4

B) 1s22s22p63s23p4

C) 1s22s22p63s23p3

D) 1s22s22p63s23p2

E) 1s22s22p63s23p5

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

67) The atomic number for nitrogen is 7. Which of the following represents the ground state electron configuration for a nitrogen atom?

A) 1s22s12p4

B) 1s22p5

C) 2s22p5

D) 1s22s2 2p3

E) 1s22s23s3

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

68) Which element has the ground state electron configuration of 1s22s22p63s23p5?

A) oxygen

B) fluorine

C) sulfur

D) chlorine

E) bromine

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

69) Which element has the ground state electron configuration of 1s22s22p63s23p4?

A) Cl

B) S

C) P

D) Al

E) N

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

70) What is the electronic configuration for the magnesium ion with a 2+ charge?

A) 1s22s22p63s2

B) 1s22s22p6

C) 1s22s22p4

D) 1s22s22p63s1

E) 1s22s22p63s22p2

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

71) Which element has the following electronic configuration?

A) boron

B) carbon

C) silicon

D) nitrogen

E) fluorine

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

72) Which element has the following electronic configuration?

A) boron

B) carbon

C) silicon

D) nitrogen

E) fluorine

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

73) The following ground state electron configuration violates ________.

A) the Aufbau principle

B) the Pauli Exclusion principle

C) Hund's Rule

D) Heisenberg's Uncertainty principle

E) None of these.

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

74) The following ground state electron configuration violates ________.

A) the Aufbau principle

B) the Pauli Exclusion principle

C) Hund's Rule

D) Heisenberg's Uncertainty principle

E) None of these.

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

75) The following ground state electron configuration violates ________.

A) the Aufbau principle

B) the Pauli Exclusion principle

C) Hund's Rule

D) Heisenberg's Uncertainty principle

E) None of these.

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

76) Ar, K+, and Cl— have equal numbers of electrons, and are considered isoelectronic. Select the correct ground state electron configuration for them.

A) 1s22s22p63s23p6

B) 1s22s22p63s6

C) 1s22s22p23s23p5

D) 1s22s22p63s13p64s1

E) 1s22s22p63s23p2

Diff: 2

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

77) Constructive interference of waves results in ________.

A) a wave with smaller amplitude

B) a wave with larger amplitude

C) cancellation of both waves

D) formation of a node

E) Both C and D

Diff: 1

Learning Objective: 1.8 Define a bond in terms of valence bond theory

78) Destructive interference of waves results in ________.

A) a wave with smaller amplitude

B) a wave with larger amplitude

C) cancellation of both waves

D) formation of a node

E) Both C and D

Diff: 1

Learning Objective: 1.8 Define a bond in terms of valence bond theory

79) All single bonds can be classified as ________.

A) nonpolar covalent

B) polar covalent

C) ionic

D) sigma bonds

E) pi bonds

Diff: 1

Learning Objective: 1.8 Define a bond in terms of valence bond theory

80) Which bonding type has circular symmetry with respect to the bond axis?

A) sigma bond

B) pi bond

C) delta bond

D) covalent bond

E) ionic bond

Diff: 2

Learning Objective: 1.8 Define a bond in terms of valence bond theory

81) Which best describes the difference between valence bond theory and molecular orbital (MO) theory?

A) valence bond theory requires the linear combination of atomic orbitals

B) MO theory requires the linear combination of atomic orbitals

C) valence bond theory considers only individual atomic orbitals

D) Both A and B

E) Both B and C

Diff: 2

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

82) How many molecular orbitals are formed when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?

A) 1

B) 2

C) 3

D) 4

E) 5

Diff: 2

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

83) Which molecular orbitals are formed when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?

A) two bonding molecular orbitals

B) only one bonding molecular orbital

C) one bonding molecular orbital and one antibonding molecular orbital

D) two antibonding molecular orbitals

E) only one antibonding orbital

Diff: 2

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

84) How are electrons distributed in the molecular orbitals when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?

A) two electrons in the bonding molecular orbital

B) one electron in the bonding molecular orbital, one electron in the non-bonding molecular orbital

C) one electron in the bonding molecular orbital, one electron in the antibonding molecular orbital

D) two electrons in the antibonding molecular orbital

E) two electrons in the non-bonding molecular orbital

Diff: 2

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

85) How many hydrogen atoms are connected to the indicated carbon atom?

A) one

B) two

C) three

D) four

E) none

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

86) How many hydrogen atoms are connected to the indicated carbon atom?

A) one

B) two

C) three

D) four

E) none

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

87) According to molecular orbital theory the highest energy molecular orbital that is occupied with an electron is referred to as ________.

A) degenerate

B) antibonding

C) the LCAO

D) the LUMO

E) the HOMO

Diff: 1

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

88) According to molecular orbital theory the lowest energy molecular orbital that is not occupied by an electron is referred to as ________.

A) degenerate

B) antibonding

C) the LCAO

D) the LUMO

E) the HOMO

Diff: 1

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

89) Identify the incorrect statement in regards to the overlap of 1s atomic orbitals of two hydrogen atoms resulting in constructive interference?

A) a sigma bonding molecular orbital is formed

B) the bonding molecular orbital formed is lower in energy than the 1s atomic orbital

C) the bonding molecular orbital formed has a node between the atoms

D) the bonding molecular orbital formed has circular symmetry

E) a maximum of two electrons may occupy the bonding molecular orbital

Diff: 3

Learning Objective: 1.9 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs

90) For the following chemical reaction, how many hydrogen atoms are added or lost?

A) one hydrogen atom added

B) two hydrogen atoms added

C) one hydrogen atom lost

D) two hydrogen atoms lost

E) no change in the number of hydrogen atoms

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

91) For the following chemical reaction, how many hydrogen atoms are added or lost?

A) one hydrogen atom added

B) two hydrogen atoms added

C) one hydrogen atom lost

D) two hydrogen atoms lost

E) no change in the number of hydrogen atoms

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

92) Interaction of the following two atomic orbitals in the orientation shown results in what kind of molecular orbital?

A) a sigma bonding molecular orbital is formed

B) a pi bonding molecular orbital is formed

C) a sigma antibonding molecular orbital is formed

D) a pi antibonding molecular orbital is formed

E) destructive interference occurs so no molecular orbital is formed

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

93) Interaction of the following two atomic orbitals results in what kind of molecular orbital, in the orientation shown?

A) a sigma bonding molecular orbital is formed

B) a pi bonding molecular orbital is formed

C) a sigma antibonding molecular orbital is formed

D) a pi antibonding molecular orbital is formed

E) constructive interference occurs so no molecular orbital is formed

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

94) What is the hybridization of the oxygen atom in the following compound?

A) sp

B) sp2

C) sp3

D) sp3d

E) s2p

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

95) What is the hybridization of the carbon atom in CO2?

A) sp

B) sp2

C) sp3

D) sp3d

E) s2p

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

96) What is the hybridization of the nitrogen atom in the following compound?

A) sp

B) sp2

C) sp3

D) sp3d

E) s2p

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

97) What is the hybridization of the boron atom in the following compound?

A) sp

B) sp2

C) sp3

D) sp3d

E) s2p

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

98) What is the hybridization of the carbon (I) atom in the following compound?

A) sp

B) sp2

C) sp3

D) sp3d

E) sp3d2

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

99) What is the hybridization of the nitrogen atom in the following compound?

A) sp

B) sp2

C) sp3

D) sp4

E) s2p

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

100) The lone pair of electrons on the nitrogen atom in the following compound are located in which atomic orbital?

A) sp2

B) sp3

C) sp

D) s

E) p

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

101) Which of the following structures have carbon with sp2 hybridization?

A) I and II

B) III and IV

C) I and III

D) II and IV

E) I and IV

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

102) Which of the indicated carbon atoms are sp2 hybridized?

A) I and II

B) III and IV

C) II and III

D) I and III

E) II and IV

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

103) What is the correct hybridization for the indicated carbon atoms in the following compound?

A) I = sp3, II = sp2, III = sp

B) I = sp2, II = sp, III = sp2

C) I = sp, II = sp2, III = sp3

D) I = sp, II = sp2, III = sp

E) I = sp2, II = sp3, III = sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

104) How many s–sp2 sigma bonds are in the following compound?

A) 2

B) 3

C) 4

D) 5

E) 6

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

105) The C2–C3 bond in the following compound results from the overlap of which orbitals?

A) sp—sp2

B) sp—sp3

C) sp2—sp2

D) sp2—sp3

E) sp3—sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

106) The sigma bond in the C=C in the following compound results from the overlap of which orbitals?

A) sp—sp2

B) sp—sp3

C) sp2—sp2

D) sp2—sp3

E) sp3—sp2

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

107) The C–C sigma bond in ethyne (H–C≡C–H) results from the overlap of which orbitals?

A) sp—sp

B) sp—sp3

C) sp2—sp2

D) sp—s

E) p—p

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

108) How many pi bonds are present in the following compound?

A) one

B) two

C) three

D) four

E) five

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

109) How many pi bonds are present in the following compound?

A) two

B) three

C) four

D) five

E) six

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

110) The sigma bond that is part of C=N in the following compound results from the overlap of which orbitals?

A) sp2—sp2

B) sp—sp

C) sp2—sp3

D) sp3—sp3

E) sp3—sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

111) The bonds indicated by the arrow in the following compound results from the overlap of which orbitals?

A) sp2—sp2

B) sp3—sp3

C) p—p

D) Both A and B

E) Both A and C

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

112) Which orbitals are involved in the C–O sigma bond in acetone, shown below?

A) Csp2–Osp2

B) Csp3–Osp3

C) Csp–Osp

D) Cp–Op

E) Csp–Op

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

113) Which of the following best describes the orbitals involved in the formation of the C=O bond in acetone, shown below?

A) σ = Csp2 - Osp2 and π = Csp2 - Osp2

B) σ = Csp2 - Osp2 and π = Cp - Op

C) σ = Csp3 - Osp2 and π = Cp - Op

D) σ = Cp - Op and π = Csp2 - Osp2

E) σ = Csp - Osp and π = Cp - Op

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

114) The C–H bond in the methyl cation, CH3+, results from the overlap of which orbitals?

A) sp3—sp2

B) sp3—s

C) sp2—s

D) sp3—p

E) p—s

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

115) The lone pair of electrons in the methyl anion, :CH3–, resides in which orbital?

A) s2

B) p

C) sp

D) sp3

E) sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

116) What is the hybridization of the indicated atoms in the following compound?

A) I = sp ; II = sp2 ; III = sp3 ; IV = sp2

B) I = sp2 ; II = sp ; III = sp2 ; IV = sp3

C) I = sp3 ; II = sp2 ; III = sp ; IV = sp2

D) I = sp2 ; II = sp3 ; III = sp2 ; IV = sp

E) I = sp2 ; II = sp2 ; III = sp2 ; IV = sp3

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

117) The carbon and oxygen atoms in carbon monoxide are connected by which type of bond(s)?

A) a sigma (σ) bond

B) two sigma (σ) bonds

C) a pi (π) bond

D) two pi (π) bonds

E) both A and D

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

118) The N–H bond in the following compound is a ________ and is formed from the ________.

A) σ bond; sp2 — s orbital overlap

B) σ bond; sp3 — s orbital overlap

C) π bond; sp3 — s orbital overlap

D) π bond; sp2 — p orbital overlap

E) π bond; p — p orbital overlap

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

119) Identify the shortest bond in the following compound.

A) I

B) II

C) III

D) IV

E) I and III have the same length

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

120) Which of the following compounds has the shortest carbon—carbon bond?

A) I

B) II

C) III

D) IV

E) All the carbon bonds are equal in length

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

121) Which of the statements best describes the carbon-carbon bond length and strength for the following compounds.

A) the shortest and strongest bond is found in compound I

B) the shortest and strongest bond is found in compound II

C) the shortest and weakest bond is found in compound I

D) the shortest and weakest bond is found in compound II

E) the shortest bond is found in compound I and the weakest bond in compound II

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

122) Identify the longest C–C bond(s) in the following compound?

A) I

B) II

C) III

D) I and III

E) I and II

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

123) Rank the indicated C–C bonds in order of increasing bond length.

A) I < II < III

B) II < III < I

C) III < I< II

D) II < I< III

E) I < III< II

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

124) Identify the compound with the strongest carbon — nitrogen bond.

A) CH3CH2CH=NH

B) CH3CH2NH2

C) CH3CH2C≡N

D) (CH3)3N

E) The strength of the carbon-nitrogen bonds are the same

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

125) Identify the compound with the longest carbon — nitrogen bond.

A) CH3CH2CH=NH

B) CH3CH2NH2

C) CH3CH2C≡N

D) CH3CH=NCH3

E) The length of all the carbon-nitrogen bonds are the same

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

126) What is the molecular geometry of the central atom in the following compound?

A) tetrahedral

B) trigonal planar

C) trigonal pyramidal

D) square planar

E) linear

Diff: 1

Learning Objective: 1.11 Describe VSEPR theory

127) Which of the following compound(s) have trigonal planar molecular geometry?

A) I

B) II

C) III

D) IV

E) I and IV

Diff: 1

Learning Objective: 1.11 Describe VSEPR theory

128) Which of the following compound(s) have trigonal pyramidal molecular geometry?

A) I

B) II

C) III

D) IV

E) I and IV

Diff: 1

Learning Objective: 1.11 Describe VSEPR theory

129) Which of the following compound(s) have bent molecular geometry?

A) I

B) II

C) III

D) IV

E) I and IV

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

130) Which of the following compound(s) have trigonal planar molecular geometry?

A) I, II and III

B) II and III

C) III and V

D) V only

E) All of these

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

131) Which of the following compound(s) have a tetrahedral arrangement of electron pairs?

A) I, II and III

B) I, II, IV and V

C) III and IV and V

D) IV and V

E) All of these

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

132) Which of the following compounds have trigonal planar arrangement of electron pairs?

A) I, II and III

B) I, II, IV and V

C) III and IV and V

D) II and III

E) All of these

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

133) What is the molecular geometry at the central atom in in the molecule shown in the box?

A) trigonal planar

B) trigonal pyramidal

C) square planar

D) tetrahedral

E) None of these

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

134) What is the molecular geometry at the central atom in the molecule shown in the box?

A) trigonal planar

B) trigonal pyramidal

C) square planar

D) tetrahedral

E) bent

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

135) What is the molecular geometry at the nitrogen atom in the following compound?

A) trigonal planar

B) trigonal pyramidal

C) linear

D) tetrahedral

E) bent

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

136) Which compound does not have a linear molecular geometry?

A) CO2

B) H2O

C) BeCl2

D) HCN

E) C2H2

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

137) What is the approximate bond angle around the indicated carbon atom?

A) 60°

B) 90°

C) 109.5°

D) 120°

E) 180°

Diff: 1

Learning Objective: 1.11 Describe VSEPR theory

138) What is the approximate bond angle around the indicated carbon atom?

A) 60°

B) 90°

C) 109.5°

D) 120°

E) 180°

Diff: 1

Learning Objective: 1.11 Describe VSEPR theory

139) What is the approximate bond angle around the nitrogen atom?

A) 90°

B) 109.5°

C) 120°

D) 180°

E) 100°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

140) What is the approximate bond angle around the carbon atom in the following molecule?

A) 90°

B) 109.5°

C) 105°

D) 120°

E) 180°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

141) What is the hybridization and approximate bond angle around the carbon atom in the following molecule?

A) sp2, 120°

B) sp, 180°

C) sp3, 109.5°

D) sp3, 120°

E) sp, 120°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

142) What is the hybridization state and approximate bond angle around nitrogen in the following compound?

A) sp2, 109.5°

B) sp2, 107°

C) sp3, 109.5°

D) sp3, 107°

E) sp2, 120°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

143) What is the hybridization state and approximate bond angle around oxygen in the following compound?

A) sp, 109.5°

B) sp2, 109.5°

C) sp3, 109.5°

D) sp2, 120°

E) sp, 180°

Diff: 3

Learning Objective: 1.11 Describe VSEPR theory

144) What is the hybridization state and molecular geometry around the sulfur atom in the molecule shown in the box?

A) sp2, tetrahedral

B) sp2, trigonal planar

C) sp3, tetrahedral

D) sp3, trigonal pyramidal

E) sp2, trigonal pyramidal

Diff: 3

Learning Objective: 1.11 Describe VSEPR theory

145) What is the hybridization state and molecular geometry around the carbon atom in the molecule shown in the box?

A) sp, linear

B) sp2, trigonal planar

C) sp3, tetrahedral

D) sp3, trigonal pyramidal

E) sp2, trigonal pyramidal

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

146) Identify the hybridization state, molecular geometry and approximate bond angle for the species shown in box below.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, 120°

E) sp2, trigonal pyramidal, 180°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

147) Identify the hybridization state, molecular geometry and approximate bond angle for the species shown in box below.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, <109.5°

E) sp2, trigonal pyramidal, 180°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

148) Identify the hybridization state, molecular geometry and approximate bond angle around the sulfur atom for the following molecule.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, <109.5°

E) sp2, trigonal pyramidal, 180°

Diff: 3

Learning Objective: 1.11 Describe VSEPR theory

149) Identify the hybridization state, molecular geometry and approximate bond angle around the carbon atom for the molecule shown in box below.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, <109.5°

E) sp2, trigonal pyramidal, 180°

Diff: 3

Learning Objective: 1.11 Describe VSEPR theory

150) Following is the structure for Propranolol, an antihypertensive drug. Identify the hybridization state, molecular geometry and approximate bond angle at the nitrogen atom in Propranolol.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, ~109.5°

E) sp2, trigonal pyramidal, 180°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

151) Identify the hybridization state, molecular geometry and approximate bond angle at the indicated nitrogen atom in the following compound.

A) sp2, bent, 109°

B) sp2, bent, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, ~109.5°

E) sp2, trigonal pyramidal, 120°

Diff: 3

Learning Objective: 1.11 Describe VSEPR theory

152) Tryptophan is an essential amino acid that is important in the synthesis of the neurotransmitter serotonin. Identify the hybridization state, molecular geometry and approximate bond angle at the indicated carbon atom.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, trigonal pyramidal, ~109.5°

E) sp2, trigonal pyramidal, 180°

Diff: 3

Learning Objective: 1.11 Describe VSEPR theory

153) Which of the following covalent bonds has the largest dipole moment?

A) C–C

B) C–H

C) C–O

D) N–H

E) H–F

Diff: 1

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

154) Which of the following compounds has no dipole moment?

A) CH4

B) NH3

C) HF

D) HCl

E) HBr

Diff: 1

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

155) Which of the following compounds has polar covalent bonds?

A) NH3

B) Na2O

C) H2

D) KF

E) CH4

Diff: 1

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

156) Which of the following compounds have a net dipole moment?

A) CBr4

B) CO2

C) CH4

D) H2O

E) C2H4

Diff: 2

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

157) Which of the following compounds does not have a dipole moment?

A) HCl

B) NCl3

C) CO

D) BF3

E) H2O

Diff: 2

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

158) Which of the following compounds has a net dipole moment of zero?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

159) Identify the following compound(s) having a dipole moment?

A) II

B) III

C) II and III

D) I, II and III

E) II, III and IV

Diff: 2

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

160) Rank the following compounds in order of decreasing dipole moment.

A) I > II > III

B) II > III > I

C) I > III > II

D) III > II > I

E) II > I > III

Diff: 3

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

161) Rank the following compounds in order of decreasing dipole moment.

A) I > II > III

B) II >III > I

C) I > III > II

D) III > I > II

E) II > I > III

Diff: 2

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

162) For the following transformation, how many hydrogen atoms are added or lost?

A) one hydrogen atom added

B) two hydrogen atoms added

C) one hydrogen atom lost

D) two hydrogen atoms lost

E) no change in the number of hydrogen atoms

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

163) For the following equation, how many hydrogen atoms are added or lost?

A) one hydrogen atom added

B) two hydrogen atoms added

C) one hydrogen atom lost

D) two hydrogen atoms lost

E) no change in the number of hydrogen atoms

Diff: 1

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

164) For the following equation, how many hydrogen atoms are added or lost?

A) one hydrogen atom added

B) two hydrogen atoms added

C) one hydrogen atom lost

D) two hydrogen atoms lost

E) no change in the number of hydrogen atoms

Diff: 2

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

165) Which of the intermolecular forces listed below is generally considered the strongest?

A) London dispersion forces

B) fleeting dipole-dipole interactions

C) dipole-dipole interactions

D) hydrogen bonding

E) the vital force

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

166) Which intermolecular force is generally considered the weakest?

A) ion-dipole interactions

B) London dispersion forces

C) dipole-dipole interactions

D) hydrogen bonding

E) covalent bonding

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

167) What is the strongest intermolecular force possible between molecules of the following structure?

A) ion-dipole interactions

B) London dispersion forces

C) dipole-dipole interactions

D) hydrogen bonding

E) covalent bonding

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

168) What is the strongest intermolecular force possible between molecules of the following structure?

A) ion-dipole interactions

B) London dispersion forces

C) dipole-dipole interactions

D) hydrogen bonding

E) covalent bonding

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

169) Which of the following statements best explains the observation that hydrogen fluoride has the highest boiling point of all the hydrogen halides?

A) The fluorine in HF is the smallest atom for all of the halogens.

B) Fluorine is the most electronegative of the atoms.

C) Hydrogen fluoride can participate in hydrogen bonding.

D) HF is very reactive and can react and dissolve glass.

E) HF is a weak acid, and doesn't completely dissociate.

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

170) Identify the following compound(s) having the greatest London dispersion forces between like molecules?

A) I

B) II

C) III

D) IV

E) II and III

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

171) Identify the following compound(s) having the highest boiling point?

A) I

B) II

C) III

D) IV

E) II and IV

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

172) Identify the following compound(s) having the lowest boiling point?

A) I

B) II

C) III

D) IV

E) II and IV

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

173) Which of the following compounds have the lowest boiling point?

A) CH3Cl

B) CH2Cl2

C) CH4

D) CHCl3

E) CCl4

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

174) Identify the following compound(s) having the lowest boiling point?

A) I

B) II

C) III

D) IV

E) I and IV

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

175) Rank the following compounds in order of decreasing boiling point.

A) III > I > IV > II

B) II > I > IV > III

C) III > I > II > IV

D) IV > II > I > III

E) I > III > II > IV

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

176) Rank the following compounds in order of decreasing boiling point.

A) III > I > IV > II

B) II > IV > I > III

C) III > I > II > IV

D) IV > II > I > III

E) I > III > II > IV

Diff: 3

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

177) Rank the following compounds in order of decreasing boiling point.

A) III > I > IV > II

B) II > IV > III > I

C) III > I > II > IV

D) IV > II > I > III

E) I > III > II > IV

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

178) For the following equation, how many hydrogen atoms are added or lost?

A) one hydrogen atom added

B) two hydrogen atoms added

C) one hydrogen atom lost

D) two hydrogen atoms lost

E) no change in the number of hydrogen atoms

Diff: 2

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

179) Identify the following compound(s) expected to be the most soluble in water?

A) I

B) II

C) III

D) IV

E) II and IV

Diff: 1

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

180) Identify the following compound(s) expected to be the most soluble in butane, CH3CH2CH2CH3?

A) I

B) II

C) III

D) IV

E) II and III

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

181) For soap molecules to remove and dissolve oil in water, what molecular features are needed?

A) one end of the molecule must be polar

B) the compound must contain oxygen atoms

C) one end of the molecule must be nonpolar

D) Both A and C

E) All A, B and C

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

182) Amino acids are the building blocks of proteins. Which statement best describes the physical properties of the following amino acid?

A) high melting point and low solubility in water

B) large dipole moment and no hydrogen bonding

C) high melting point and large dipole moment

D) low solubility in water and small dipole moment

E) small dipole moment and hydrophobic

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

183) Which statement best describes the physical properties of the following sugar?

A) high melting point and high solubility in water

B) large dipole moment and no hydrogen bonding

C) low melting point and large dipole moment

D) low solubility in water and large dipole moment

E) small dipole moment and hydrophobic

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

184) Naproxen, sold under the trade name Aleve, has the following structure. What is the molecular formula for naproxen?

A) C13H15O3

B) C14H14O3

C) C12H16O3

D) C14H16O3

E) C14H18O3

Diff: 2

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

185) AZT, used in the treatment of AIDS, has the following structure. What is the molecular formula for AZT?

A) C9H14N5O4

B) C9H9N5O4

C) C9H12N5O4

D) C10H13N5O4

E) C11H12N5O4

Diff: 2

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

186) Capsaicin, found in peppers, has the following structure. What is the molecular formula for capsaicin?

A) C18H27NO3

B) C17H25NO3

C) C18H30NO3

D) C19H27NO3

E) C18H24NO3

Diff: 2

Learning Objective: 1.6 Demonstrate how to read and draw bond-line structures through converting other styles of molecular representation into bond-line structures and vice versa

187) Of the following examples, which would be considered organic compounds?

A) I and II

B) II and III

C) III and IV

D) I and III

E) II and IV

Diff: 1

Learning Objective: 1.1 Compare and contrast organic and inorganic compounds

188) Constitutional isomers differ in ________.

A) physical properties

B) atomic connectivity

C) molecular formula

D) A and B

E) B and C

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

189) What is the relationship between the following compounds?

A) isotopes

B) constitutional isomers

C) the same structure

D) composed of different elements

E) no relationship

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

190) What is the relationship between the following compounds?

A) resonance isomers

B) constitutional isomers

C) empirical isomers

D) isotopes

E) There is no relationship

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

191) Which of the following compounds are constitutional isomers?

A) I and II

B) I and III

C) I, II and IV

D) II, III and IV

E) I, II, and III

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

192) Which of the following compounds are constitutional isomers of each other?

A) I and II

B) II and III

C) III and IV

D) I and IV

E) II and IV

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

193) Identify three constitutional isomers having the molecular formula C4H8BrCl.

A) I, II, and III

B) II, III, and IV

C) III, IV, and IV

D) I, III, and V

E) II, III, and V

Diff: 1

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

194) Identify three constitutional isomers having the molecular formula C4H8O.

A) I, II, and III

B) II, III, and IV

C) III, IV, and IV

D) I, II, and IV

E) II, III, and V

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

195) Which of the following represent identical molecules?

A) I and II

B) II and III

C) III and IV

D) IV and V

E) II and IV

Diff: 2

Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula

196) What are the formal charges on the atoms indicated for the following structure?

A) I = 0; II = 1+; III = 2+

B) I = 1-; II = 0; III = 1+

C) I = 1+; II = 1-; III = 2+

D) I = 1-; II = 1+; III = 1-

E) I = 0; II = 1-; III = 2+

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

197) What are the formal charges on fluorine and nitrogen in the following structure?

A) F = 1+, N = 1+

B) F = 0, N = 1-

C) F = 1-, N = 1-

D) F = 0, N = 1+

E) F = 1+, N = 1-

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

198) Which of the following have a 1+ formal charge on the central atom?

A) I

B) II

C) III

D) III and V

E) IV and V

Diff: 2

Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated

199) Which of the following principle states "The lowest energy orbital is filled first"?

A) Aufbau principle

B) Pauli exclusion principle

C) Hund's Rule

D) Heizenberg Uncertainty principle

E) Le Chatelier's principle

Diff: 1

Learning Objective: 1.7 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons

200) Which of the indicated carbon atoms in the following compound are sp2 hybridized?

A) I and II

B) III and IV

C) II and III

D) I and III

E) II and IV

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

201) What is the hybridization for each of the indicated carbon atoms in the following compound?

A) I = sp3, II = sp2, III = sp

B) I = sp2, II = sp, III = sp2

C) I = sp, II = sp2, III = sp3

D) I = sp, II = sp2, III = sp

E) I = sp2, II = sp3, III = sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

202) How many s–sp2 sigma bonds are in the following compound?

A) 2

B) 3

C) 4

D) 5

E) 6

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

203) The C2–C3 bond in the following compound results from the overlap of which orbitals?

A) sp—sp2

B) sp—sp3

C) sp2—sp2

D) sp2—sp3

E) sp3—sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

204) The sigma bond that is part of C=C in the following compound results from the overlap of which orbitals?

A) sp—sp2

B) sp—sp3

C) sp2—sp2

D) sp2—sp3

E) sp3—sp2

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

205) How many pi bonds are present in the following compound?

A) one

B) two

C) three

D) four

E) five

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

206) How many pi bonds are present in the following compound?

A) two

B) three

C) four

D) five

E) six

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

207) How many sigma bonds are present in the following compound?

A) 20

B) 22

C) 24

D) 25

E) 27

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

208) The sigma bond that is part of C=N in the following compound results from the overlap of which orbitals?

A) sp2—sp2

B) sp—sp

C) sp2—sp3

D) sp3—sp3

E) sp3—sp2

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

209) The bonds indicated by the arrow in the following compound results from the overlap of which orbitals?

A) sp2—sp2

B) sp3—sp3

C) p—p

D) Both A and B

E) Both A and C

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

210) Which orbitals are involved in the C–O sigma bond in acetone, shown below?

A) Csp2–Osp2

B) Csp3–Osp3

C) Csp–Osp

D) Cp–Op

E) Csp–Op

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

211) Which of the following best describes the orbitals involved in the formation of the C=O bond in acetone, shown below?

A) σ = Csp2 - Osp2 and π = Csp2 - Osp2

B) σ = Csp2 - Osp2 and π = Cp - Op

C) σ = Csp3 - Osp2 and π = Cp - Op

D) σ = Cp - Op and π = Csp2 - Osp2

E) σ = Csp - Osp and π = Cp - Op

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

212) Identify the shortest bond in the following compound.

A) I

B) II

C) III

D) IV

E) I and III are of equal length

Diff: 1

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

213) Identify the longest C–C bond(s) in the following compound?

A) I

B) II

C) III

D) IV

E) II and IV are of equal length

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

214) Identify the longest C–C bond(s) in the following compound?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

215) Identify the longest C–C bond(s) in the following compound?

A) I

B) II

C) III

D) IV

E) V

Diff: 3

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

216) Rank the indicated C–C bonds in increasing order of bond length.

A) I < II < III < IV

B) II < IV < III < I

C) III < I < IV < II

D) III < I < II < IV

E) IV < II < I < III

Diff: 3

Learning Objective: 1.10 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed

217) Following is the structure for Propranolol, an antihypertensive drug. Identify the hybridization state, molecular geometry and approximate bond angle at the indicated oxygen atom in Propranolol.

A) sp2, tetrahedral, 109°

B) sp2, bent, 120°

C) sp3, tetrahedral, 109.5°

D) sp3, bent, ~109.5°

E) sp2, bent, 180°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

218) Following is the structure for Propranolol, an antihypertensive drug. Identify the hybridization state, molecular geometry and approximate bond angle at the nitrogen atom in Propranolol.

A) sp2, tetrahedral, 109°

B) sp2, trigonal planar, 120°

C) sp3, tetrahedral, ~109.5°

D) sp3, trigonal pyramidal, ~109.5°

E) sp2, trigonal pyramidal, 180°

Diff: 2

Learning Objective: 1.11 Describe VSEPR theory

219) Rank the following compounds in order of decreasing dipole moment.

A) I > II > III

B) II >III > I

C) I > III > II

D) III > I > II

E) II > I > III

Diff: 2

Learning Objective: 1.12 Describe how dipole moment is used in calculating the ionic character of a bond

220) What is the strongest intermolecular force possible between molecules of the following structure?

A) ion-dipole interactions

B) London dispersion forces

C) dipole-dipole interactions

D) hydrogen bonding

E) covalent bonding

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

221) What is the strongest intermolecular force possible between molecules of the following structure?

A) ion-dipole interactions

B) London dispersion forces

C) dipole-dipole interactions

D) hydrogen bonding

E) covalent bonding

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

222) Which of the following compounds has the greatest London dispersion forces between like molecules?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

223) Which of the following compounds is expected to have the highest boiling point?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

224) Which of the following compounds is expected to have the lowest boiling point?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

225) Identify the following compound expected to have the lowest boiling point?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

226) Rank the following compounds in decreasing order of boiling point.

A) III > I > IV > II

B) II > I > IV > III

C) III > I > II > IV

D) IV > II > I > III

E) I > III > II > IV

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

227) Rank the following compounds in decreasing order of boiling point.

A) III > I > IV > II

B) II > IV > I > III

C) III > I > II > IV

D) IV > II > I > III

E) I > III > II > IV

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

228) Rank the following compounds in decreasing order of boiling point.

A) III > I > IV > II

B) II > IV > III > I

C) III > IV > I > II

D) IV > II > I > III

E) I > III > II > IV

Diff: 2

Learning Objective: 1.13 Describe the basic nature of all intermolecular forces

229) Identify the following compound expected to be the most soluble in water?

A) I

B) II

C) III

D) IV

E) V

Diff: 1

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

230) Identify the following compound expected to be the most soluble in butane, CH3CH2CH2CH3?

A) I

B) II

C) III

D) IV

E) V

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

231) Amino acids are the building blocks of proteins. Which statement best describes the physical properties of the following amino acid?

A) high melting point and low solubility in water

B) large dipole moment and no hydrogen bonding

C) high melting point and large dipole moment

D) low solubility in water and small dipole moment

E) small dipole moment and hydrophobic

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

232) Which statement best describes the physical properties of the following sugar?

A) high melting point and high solubility in water

B) large dipole moment and no hydrogen bonding

C) low melting point and large dipole moment

D) low solubility in water and large dipole moment

E) small dipole moment and hydrophobic

Diff: 2

Learning Objective: 1.14 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility

© (2021) John Wiley & Sons, Inc. All rights reserved. Instructors who are authorized users of this course are permitted to download these materials and use them in connection with the course. Except as permitted herein or by law, no part of these materials should be reproduced, stored in a retrieval system, or transmitted, in any form or by any means, electronic, mechanical, photocopying, recording or otherwise.