Question 1

Place the following in order of increasing bond length. NO2⁻ NO3⁻ NO

Accepted Answer

A)  NO 2⁻ 3⁻ 
B)  NO2⁻ 3⁻ 3⁻ 2⁻ 
D)  NO 3⁻ 2⁻ 
E)  NO3⁻ 2⁻ < NO 
A)  NO 2⁻ 3⁻ 
B)  NO2⁻ 3⁻ 3⁻ 2⁻ 
D)  NO 3⁻ 2⁻ 
E)  NO3⁻ 2⁻ < NO

Question 2

Identify the number of bonding pairs and lone pairs of electrons in water.

Accepted Answer

A)  1 bonding pair and 1 lone pair 
B)  1 bonding pair and 2 lone pairs 
C)  2 bonding pairs and 2 lone pairs 
D)  2 bonding pairs and 1 lone pair 
E)  3 bonding pairs and 2 lone pairs 
A)  1 bonding pair and 1 lone pair 
B)  1 bonding pair and 2 lone pairs 
C)  2 bonding pairs and 2 lone pairs 
D)  2 bonding pairs and 1 lone pair 
E)  3 bonding pairs and 2 lone pairs

Question 3

Choose the bond below that is the weakest.

Accepted Answer

A)  C≡O 
B)  N≡N 
C)  C-I 
D)  C=O 
E)  Na-Br 
A)  C≡O 
B)  N≡N 
C)  C-I 
D)  C=O 
E)  Na-Br

Question 4

Give the approximate bond angle for a molecule with an octahedral shape.

Accepted Answer

A)  109.5° 
B)  180° 
C)  120° 
D)  105° 
E)  90° 
A)  109.5° 
B)  180° 
C)  120° 
D)  105° 
E)  90°

Question 5

Describe the difference between a pure covalent bond and a polar covalent bond.

Accepted Answer

A pure covalent bond occurs when bonding

Question 6

Using periodic trends,place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl

Accepted Answer

A)  Sb-Cl > As-Cl > P-Cl 
B)  As-Cl > Sb-Cl > P-Cl 
C)  Sb-Cl > P-Cl > As-Cl 
D)  P-Cl > As-Cl > Sb-Cl 
E)  As-Cl > P-Cl > Sb-Cl 
A)  Sb-Cl > As-Cl > P-Cl 
B)  As-Cl > Sb-Cl > P-Cl 
C)  Sb-Cl > P-Cl > As-Cl 
D)  P-Cl > As-Cl > Sb-Cl 
E)  As-Cl > P-Cl > Sb-Cl

Question 7

Choose the best Lewis structure for NH4⁺.

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 8

Determine the electron geometry (eg)and molecular geometry (mg)of SiF4.

Accepted Answer

A)  eg = tetrahedral, mg = trigonal pyramidal 
B)  eg = octahedral, mg = square planar 
C)  eg = trigonal bipyramidal, mg = trigonal pyramidal 
D)  eg = tetrahedral, mg = bent 
E)  eg = tetrahedral, mg = tetrahedral 
A)  eg = tetrahedral, mg = trigonal pyramidal 
B)  eg = octahedral, mg = square planar 
C)  eg = trigonal bipyramidal, mg = trigonal pyramidal 
D)  eg = tetrahedral, mg = bent 
E)  eg = tetrahedral, mg = tetrahedral

Question 9

Choose the bond below that is most polar.

Accepted Answer

A)  C-N 
B)  C-F 
C)  C-O 
D)  C-C 
E)  F-F 
A)  C-N 
B)  C-F 
C)  C-O 
D)  C-C 
E)  F-F

Question 10

Determine the electron geometry (eg)and molecular geometry (mg)of CO2.

Accepted Answer

A)  eg = tetrahedral, mg = tetrahedral 
B)  eg = linear, mg = trigonal planar 
C)  eg = trigonal planar, mg = bent 
D)  eg = linear, mg = linear 
E)  eg = trigonal planar, mg = trigonal planar 
A)  eg = tetrahedral, mg = tetrahedral 
B)  eg = linear, mg = trigonal planar 
C)  eg = trigonal planar, mg = bent 
D)  eg = linear, mg = linear 
E)  eg = trigonal planar, mg = trigonal planar

Question 11

How many lone pairs are on the Cl atom in ClF2-?

Accepted Answer

A)  0 
B)  1 
C)  2 
D)  3 
A)  0 
B)  1 
C)  2 
D)  3

Question 12

How many of the following elements can form compounds with an expanded octet?
I O Br Si

Accepted Answer

A)  2 
B)  0 
C)  3 
D)  1 
E)  4 
A)  2 
B)  0 
C)  3 
D)  1 
E)  4

Question 13

Give the number of valence electrons for ICl5.

Accepted Answer

A)  36 
B)  40 
C)  42 
D)  44 
E)  46 
A)  36 
B)  40 
C)  42 
D)  44 
E)  46

Question 14

Determine the electron geometry (eg)and molecular geometry (mg)of the underlined atom CH3OCH3.

Accepted Answer

A)  eg = tetrahedral, mg = tetrahedral 
B)  eg = linear, eg = linear 
C)  eg = tetrahedral, mg = bent 
D)  eg = trigonal bipyramidal, mg = tetrahedral 
E)  eg = octahedral, mg = square planar 
A)  eg = tetrahedral, mg = tetrahedral 
B)  eg = linear, eg = linear 
C)  eg = tetrahedral, mg = bent 
D)  eg = trigonal bipyramidal, mg = tetrahedral 
E)  eg = octahedral, mg = square planar

Question 15

Draw the Lewis structure for NO2⁻ including any valid resonance structures.Which of the following statements is TRUE?

Accepted Answer

A)  The nitrite ion contains one N-O single bond and one N   O double bond. 
B)  The nitrite ion contains two N-O bonds that are equivalent to 1   bonds. 
C)  The nitrite ion contains two N   O double bonds. 
D)  The nitrite ion contains two N-O single bonds. 
E)  None of the above are true. 
A)  The nitrite ion contains one N-O single bond and one N   O double bond. 
B)  The nitrite ion contains two N-O bonds that are equivalent to 1   bonds. 
C)  The nitrite ion contains two N   O double bonds. 
D)  The nitrite ion contains two N-O single bonds. 
E)  None of the above are true.

Question 16

Place the following in order of increasing dipole moment. I.BCl3 II.BIF2  III.BClF2

Accepted Answer

A)  I < II = III 
B)  II < III < I 
C)  I < II < III 
D)  II < I < III 
E)  I < III < II 
A)  I < II = III 
B)  II < III < I 
C)  I < II < III 
D)  II < I < III 
E)  I < III < II

Question 17

Give the number of valence electrons for SO2.

Accepted Answer

A)  16 
B)  18 
C)  20 
D)  22 
E)  12 
A)  16 
B)  18 
C)  20 
D)  22 
E)  12

Question 18

How are electron affinity and electronegativity different?

Accepted Answer

Electron affinity is the process of a si

Exam 6: Chemical Bonding I

Place the following in order of increasing bond length. NO2⁻ NO3⁻ NO

Identify the number of bonding pairs and lone pairs of electrons in water.

Choose the bond below that is the weakest.

Give the approximate bond angle for a molecule with an octahedral shape.

Describe the difference between a pure covalent bond and a polar covalent bond.

Using periodic trends,place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl

Choose the best Lewis structure for NH4⁺.

Determine the electron geometry (eg)and molecular geometry (mg)of SiF4.

Choose the bond below that is most polar.

Determine the electron geometry (eg)and molecular geometry (mg)of CO2.

How many lone pairs are on the Cl atom in ClF2-?

How many of the following elements can form compounds with an expanded octet? I O Br Si

Give the number of valence electrons for ICl5.

Determine the electron geometry (eg)and molecular geometry (mg)of the underlined atom CH3OCH3.

Draw the Lewis structure for NO2⁻ including any valid resonance structures.Which of the following statements is TRUE?

Place the following in order of increasing dipole moment. I.BCl3 II.BIF2 III.BClF2

Give the number of valence electrons for SO2.

How are electron affinity and electronegativity different?

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Place the following in order of increasing bond length. NO₂⁻ NO₃⁻ NO

Choose the best Lewis structure for NH₄⁺.

Determine the electron geometry (eg)and molecular geometry (mg)of SiF₄.

Determine the electron geometry (eg)and molecular geometry (mg)of CO₂.

How many lone pairs are on the Cl atom in ClF₂^-?

Give the number of valence electrons for ICl₅.

Determine the electron geometry (eg)and molecular geometry (mg)of the underlined atom CH₃OCH₃.

Draw the Lewis structure for NO₂⁻ including any valid resonance structures.Which of the following statements is TRUE?

Place the following in order of increasing dipole moment. I.BCl₃ II.BIF₂ III.BClF₂

Give the number of valence electrons for SO₂.