Question 1

In PCl5, the Cl−P−Cl bond angle between an axial and an equatorial chlorine atom is ________ degrees.

Accepted Answer

Question 2

Use the bond energies provided to complete the following statement. ________ when all of the bonds in acetic acid (CH3COOH) are broken.
$$\begin{array}{l}
\begin{array} { l l } 
\text { Bond}&\text { Bond Energy } ( \mathrm { kJ } / \mathrm { mol } )\
\mathrm { C } - \mathrm { H } & 413 \
\mathrm { C } - \mathrm { O } & 358 \
\mathrm { O } - \mathrm { H } & 463 \
\mathrm { C } = \mathrm { O } & 745 \
\mathrm { C } - \mathrm { C } & 348 \
\mathrm { C } = \mathrm { C } & 614
\end{array}
\end{array}$$

Accepted Answer

A)  3153 kJ/mol of energy is consumed 
B)  3153 kJ/mol of energy is released 
C)  2805 kJ/mol of energy is released 
D)  2805 kJ/mol of energy is consumed 
E)  2766 kJ/mol of energy is consumed 
A)  3153 kJ/mol of energy is consumed 
B)  3153 kJ/mol of energy is released 
C)  2805 kJ/mol of energy is released 
D)  2805 kJ/mol of energy is consumed 
E)  2766 kJ/mol of energy is consumed

Question 3

Which of the following exhibits resonance?

Accepted Answer

A)  SCl4 
B)  H2O 
C)  SO2 
D)  BH3 
E)  none 
A)  SCl4 
B)  H2O 
C)  SO2 
D)  BH3 
E)  none

Question 4

Which of the following is a correct Lewis structure for oxygen?

Accepted Answer

A)    
B)    
C)    
D)    
E)  $: \mathrm { O } \equiv \mathrm { O } :$ 
A)    
B)    
C)    
D)    
E)  $: \mathrm { O } \equiv \mathrm { O } :$

Question 5

The molecule H2S has

Accepted Answer

A)  2 bonding pairs and 3 lone pairs 
B)  2 bonding pairs and 2 lone pairs 
C)  3 bonding pairs and 1 lone pair 
D)  3 bonding pairs and 3 lone pairs 
E)  none of these 
A)  2 bonding pairs and 3 lone pairs 
B)  2 bonding pairs and 2 lone pairs 
C)  3 bonding pairs and 1 lone pair 
D)  3 bonding pairs and 3 lone pairs 
E)  none of these

Question 6

Which of the following molecules or ions will have a Lewis structure most like that of phosphorus trichloride, PCl3?

Accepted Answer

A)  ClO3- 
B)  SO3 
C)  CO32- 
D)  BF3 
E)  Cl2CO 
A)  ClO3- 
B)  SO3 
C)  CO32- 
D)  BF3 
E)  Cl2CO

Question 7

Choose which central atom in the following molecules is most electronegative.

Accepted Answer

A)  PH3 
B)  CH4 
C)  H2S 
D)  H2O 
E)  NH3 
A)  PH3 
B)  CH4 
C)  H2S 
D)  H2O 
E)  NH3

Question 8

Which of the following molecules is nonpolar?

Accepted Answer

A)  sulfur dioxide, SO2 
B)  hydrogen fluoride, HF 
C)  phosphorus trifluoride, PF3 
D)  boron trifluoride, BF3 
E)  iodine trichloride, ICl3 
A)  sulfur dioxide, SO2 
B)  hydrogen fluoride, HF 
C)  phosphorus trifluoride, PF3 
D)  boron trifluoride, BF3 
E)  iodine trichloride, ICl3

Question 9

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

Accepted Answer

A)  isoelectronic 
B)  resonant structures 
C)  ionic 
D)  neutral 
E)  covalent 
A)  isoelectronic 
B)  resonant structures 
C)  ionic 
D)  neutral 
E)  covalent

Question 10

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

Accepted Answer

A)  B and C 
B)  S and O 
C)  N and F 
D)  Si and Cl 
E)  Mg and O 
A)  B and C 
B)  S and O 
C)  N and F 
D)  Si and Cl 
E)  Mg and O

Question 11

Use Lewis structures to predict the bond order for a sulfur-oxygen bond in SO32-?

Accepted Answer

A)  1 
B)  4/3 
C)  5/2 
D)  2 
E)  3/2 
A)  1 
B)  4/3 
C)  5/2 
D)  2 
E)  3/2

Question 12

How many different molecules have the molecular formula C6H14?

Accepted Answer

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

Question 13

What are the approximate H−N−H bond angles in NH4+?

Accepted Answer

A)  109.5° 
B)  120° 
C)  109.5° and 120° 
D)  90° 
E)  90° and 120° 
A)  109.5° 
B)  120° 
C)  109.5° and 120° 
D)  90° 
E)  90° and 120°

Question 14

What is the molecular geometry around carbon atom C1?

Accepted Answer

A)  tetrahedral 
B)  trigonal planar 
C)  linear 
D)  trigonal pyramidal 
E)  bent 
A)  tetrahedral 
B)  trigonal planar 
C)  linear 
D)  trigonal pyramidal 
E)  bent

Question 15

What is the molecular geometry around an atom in a molecule or ion which is surrounded by zero lone pairs of electrons and four single bonds.

Accepted Answer

A)  tetrahedral 
B)  linear 
C)  bent 
D)  trigonal pyramidal 
E)  trigonal planar 
A)  tetrahedral 
B)  linear 
C)  bent 
D)  trigonal pyramidal 
E)  trigonal planar

Question 16

How many valence electrons are present in the Lewis formula for the chlorite ion, Cl2-?

Accepted Answer

A)  26 
B)  18 
C)  24 
D)  20 
E)  22 
A)  26 
B)  18 
C)  24 
D)  20 
E)  22

Question 17

According to VSEPR theory, which of the following is the correct molecular geometry around the carbon atom in formaldehyde?

Accepted Answer

A)  Linear 
B)  Bent 
C)  Trigonal-planar 
D)  Tetrahedral 
E)  Octahedral 
A)  Linear 
B)  Bent 
C)  Trigonal-planar 
D)  Tetrahedral 
E)  Octahedral

Question 18

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

Accepted Answer

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

Question 19

Which of the following molecules or ions does not have one or more resonance structures?

Accepted Answer

A)  O3 
B)  OCN- 
C)  SO2 
D)  H2CO 
E)  NO3- 
A)  O3 
B)  OCN- 
C)  SO2 
D)  H2CO 
E)  NO3-

Question 20

Three nonequivalent Lewis structures for carbonyl sulfide, SCO, are given below. Use the concepts of formal charge and electronegativity to choose the structure that is the best representation. 
  A   B   C

Accepted Answer

A)  Structure A, because all the formal charges equal 0 
B)  Structure B, because all the formal charges equal 0 
C)  Structure C, because all the formal charges equal 0. 
D)  Structure A, because the negative formal charge resides on the most electronegative atom 
E)  Structure C, because the negative formal charge resides on the most electronegative atom 
A)  Structure A, because all the formal charges equal 0 
B)  Structure B, because all the formal charges equal 0 
C)  Structure C, because all the formal charges equal 0. 
D)  Structure A, because the negative formal charge resides on the most electronegative atom 
E)  Structure C, because the negative formal charge resides on the most electronegative atom

Exam 9: Bonding and Molecular Structure

In PCl5, the Cl−P−Cl bond angle between an axial and an equatorial chlorine atom is ________ degrees.

Use the bond energies provided to complete the following statement. ________ when all of the bonds in acetic acid (CH3COOH) are broken. Bond Bond Energy (/) - 413 - 358 - 463 = 745 - 348 = 614

Which of the following exhibits resonance?

Which of the following is a correct Lewis structure for oxygen?

The molecule H2S has

Which of the following molecules or ions will have a Lewis structure most like that of phosphorus trichloride, PCl3?

Choose which central atom in the following molecules is most electronegative.

Which of the following molecules is nonpolar?

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

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

Use Lewis structures to predict the bond order for a sulfur-oxygen bond in SO32-?

How many different molecules have the molecular formula C6H14?

What are the approximate H−N−H bond angles in NH4+?

What is the molecular geometry around carbon atom C1?

What is the molecular geometry around an atom in a molecule or ion which is surrounded by zero lone pairs of electrons and four single bonds.

How many valence electrons are present in the Lewis formula for the chlorite ion, Cl2-?

According to VSEPR theory, which of the following is the correct molecular geometry around the carbon atom in formaldehyde?

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

Which of the following molecules or ions does not have one or more resonance structures?

Three nonequivalent Lewis structures for carbonyl sulfide, SCO, are given below. Use the concepts of formal charge and electronegativity to choose the structure that is the best representation. A B C

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

In PCl₅, the Cl−P−Cl bond angle between an axial and an equatorial chlorine atom is ________ degrees.

Use the bond energies provided to complete the following statement. ________ when all of the bonds in acetic acid (CH₃COOH) are broken. Bond Bond Energy (/) - 413 - 358 - 463 = 745 - 348 = 614

The molecule H₂S has

Which of the following molecules or ions will have a Lewis structure most like that of phosphorus trichloride, PCl₃?

Use Lewis structures to predict the bond order for a sulfur-oxygen bond in SO₃2-?

How many different molecules have the molecular formula C₆H₁₄?

What are the approximate H−N−H bond angles in NH₄⁺?

What is the molecular geometry around carbon atom C₁?

How many valence electrons are present in the Lewis formula for the chlorite ion, Cl₂^-?