Question 1

Linus Pauling noticed that the energy of a polar bond is often greater than expected. He attributed the greater bond energy to

Accepted Answer

A)  a coulombic attraction between atoms with partially positive and negative charges. 
B)  the greater bond lengths of the heteronuclear bonds. 
C)  one of the many unexplainable phenomena that scientists encounter. 
D)  the ability of heteronuclear species to form double and triple bonds. 
E)  the greater number of valence electrons found in heteronuclear molecules. 
A)  a coulombic attraction between atoms with partially positive and negative charges. 
B)  the greater bond lengths of the heteronuclear bonds. 
C)  one of the many unexplainable phenomena that scientists encounter. 
D)  the ability of heteronuclear species to form double and triple bonds. 
E)  the greater number of valence electrons found in heteronuclear molecules.

Question 2

Use VSEPR theory to predict the molecular geometry of BrF5.

Accepted Answer

A)  tetrahedral 
B)  see-saw 
C)  trigonal-bipyramidal 
D)  square-pyramidal 
E)  octahedral 
A)  tetrahedral 
B)  see-saw 
C)  trigonal-bipyramidal 
D)  square-pyramidal 
E)  octahedral

Question 3

Place the following molecules in order from smallest to largest H−N−H bond angles: NH4+, NH3, and NH2-.

Accepted Answer

A)  NH4+ 3 2- 
B)  NH4+ 2- 3 
C)  NH2- 3 4+ 
D)  NH2- 4+ 3 
E)  NH3 2- 4+ 
A)  NH4+ 3 2- 
B)  NH4+ 2- 3 
C)  NH2- 3 4+ 
D)  NH2- 4+ 3 
E)  NH3 2- 4+

Question 4

One might expect PCl3 to have a trigonal planar molecular geometry since its central atom is surrounded by three outer atoms. However, PCl3 has a trigonal pyramidal geometry. Explain.

Accepted Answer

The shape of a molecule is dependent upo

Question 5

Using bond-energy data, what is ?rH for the following reaction? CH4(g) + 2Cl2(g) ? CCl4(g) + 2H2(g)
$$\begin{array} { l l } 
\text { Bond } & \text { Bond Energy } ( \mathrm { kJ } / \mathrm { mol } ) \
\mathrm { C } - \mathrm { H } & 413 \
\mathrm { H } - \mathrm { H } & 432 \
\mathrm { Cl } - \mathrm { Cl } & 242 \
\mathrm { C } - \mathrm { Cl } & 328
\end{array}$$

Accepted Answer

A)  -40 kJ/mol-rxn 
B)  -150 kJ/mol-rxn 
C)  40 kJ/mol-rxn 
D)  1415 kJ/mol-rxn 
E)  150 kJ/mol-rxn 
A)  -40 kJ/mol-rxn 
B)  -150 kJ/mol-rxn 
C)  40 kJ/mol-rxn 
D)  1415 kJ/mol-rxn 
E)  150 kJ/mol-rxn

Question 6

In molecules, as bond order increases,

Accepted Answer

A)  both bond length and bond energy increase. 
B)  both bond length and bond energy decrease. 
C)  bond length increases and bond energy is unchanged. 
D)  bond length is unchanged and bond energy increases. 
E)  bond length decreases and bond energy increases. 
A)  both bond length and bond energy increase. 
B)  both bond length and bond energy decrease. 
C)  bond length increases and bond energy is unchanged. 
D)  bond length is unchanged and bond energy increases. 
E)  bond length decreases and bond energy increases.

Question 7

The correct Lewis structure for Cl2CO is (the 2 Cl's and the O are bound to the C and not to each other):

Accepted Answer

A)    
B)    
C)    
D)    
E)  none of these 
A)    
B)    
C)    
D)    
E)  none of these

Question 8

Which of the following molecules is polar?

Accepted Answer

A)  CS2 
B)  SO2 
C)  XeF2 
D)  XeF4 
E)  SO3 
A)  CS2 
B)  SO2 
C)  XeF2 
D)  XeF4 
E)  SO3

Question 9

What is the correct Lewis structure for SF4?

Accepted Answer

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

Question 10

Electronegativity is a measure of _____.

Accepted Answer

A)  the ability of a substance to conduct electricity 
B)  the charge on a polyatomic cation 
C)  the charge on a polyatomic anion 
D)  the ability of an atom in a molecule to attract electrons to itself 
E)  the oxidation number of an atom in a molecule or polyatomic anion 
A)  the ability of a substance to conduct electricity 
B)  the charge on a polyatomic cation 
C)  the charge on a polyatomic anion 
D)  the ability of an atom in a molecule to attract electrons to itself 
E)  the oxidation number of an atom in a molecule or polyatomic anion

Question 11

The central atom in N2O is a nitrogen atom. This nitrogen atom is surrounded by

Accepted Answer

A)  two single bonds and two lone pairs of electrons. 
B)  two single bonds and one lone pair of electrons. 
C)  one single bond, one double bond, and one lone pairs of electrons. 
D)  one single bond, one double bond, and one lone pair of electrons. 
E)  two double bonds and no lone pairs of electrons. 
A)  two single bonds and two lone pairs of electrons. 
B)  two single bonds and one lone pair of electrons. 
C)  one single bond, one double bond, and one lone pairs of electrons. 
D)  one single bond, one double bond, and one lone pair of electrons. 
E)  two double bonds and no lone pairs of electrons.

Question 12

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of boron tribromide, BBr3.

Accepted Answer

A)  The electron-pair geometry is trigonal-pyramidal, the molecular geometry is trigonal-pyramidal. 
B)  The electron-pair geometry is trigonal-planar, the molecular geometry is trigonal-planar. 
C)  The electron-pair geometry is trigonal-planar, the molecular geometry is bent. 
D)  The electron-pair geometry is tetrahedral, the molecular geometry is trigonal-pyramidal. 
E)  The electron-pair geometry is trigonal-pyramidal, the molecular geometry is t-shaped. 
A)  The electron-pair geometry is trigonal-pyramidal, the molecular geometry is trigonal-pyramidal. 
B)  The electron-pair geometry is trigonal-planar, the molecular geometry is trigonal-planar. 
C)  The electron-pair geometry is trigonal-planar, the molecular geometry is bent. 
D)  The electron-pair geometry is tetrahedral, the molecular geometry is trigonal-pyramidal. 
E)  The electron-pair geometry is trigonal-pyramidal, the molecular geometry is t-shaped.

Question 13

What is the formal charge on the O2 atom in the following Lewis structure?

Accepted Answer

A)  2 
B)  1 
C)  0 
D)  -1 
E)  -2 
A)  2 
B)  1 
C)  0 
D)  -1 
E)  -2

Question 14

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

Accepted Answer

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

Question 15

Determine the bond order of NO+?

Accepted Answer

A)  2 
B)  1.5 
C)  1 
D)  2.5 
E)  3 
A)  2 
B)  1.5 
C)  1 
D)  2.5 
E)  3

Question 16

What is the formal charge on the carbon atom in CO?

Accepted Answer

A)  +2 
B)  +1 
C)  0 
D)  -1 
E)  -2 
A)  +2 
B)  +1 
C)  0 
D)  -1 
E)  -2

Question 17

Which of the following is the correct Lewis structure for the sulfate ion?

Accepted Answer

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

Question 18

According to VSEPR theory, which of the following is the correct statement concerning the electron-pair geometry and the molecular geometry of sulfur dioxide?

Accepted Answer

A)  The electron-pair geometry is trigonal planar, and the molecular geometry is trigonal planar. 
B)  The electron-pair geometry is trigonal-planar, and the molecular geometry is bent. 
C)  The electron-pair geometry is tetrahedral, and the molecular geometry is bent. 
D)  The electron-pair geometry is tetrahedral, and the molecular geometry is linear. 
E)  The electron-pair geometry is trigonal bipyramidal, and the molecular geometry is linear. 
A)  The electron-pair geometry is trigonal planar, and the molecular geometry is trigonal planar. 
B)  The electron-pair geometry is trigonal-planar, and the molecular geometry is bent. 
C)  The electron-pair geometry is tetrahedral, and the molecular geometry is bent. 
D)  The electron-pair geometry is tetrahedral, and the molecular geometry is linear. 
E)  The electron-pair geometry is trigonal bipyramidal, and the molecular geometry is linear.

Question 19

Use VSEPR theory to predict the molecular geometry around the nitrogen atom in nitrite ion, NO2-.

Accepted Answer

A)  trigonal-planar 
B)  tetrahedral 
C)  trigonal-pyramidal 
D)  T-shaped 
E)  bent 
A)  trigonal-planar 
B)  tetrahedral 
C)  trigonal-pyramidal 
D)  T-shaped 
E)  bent

Question 20

Which of the following elements is able to form a molecular structure that exceeds the octet rule?

Accepted Answer

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

Exam 9: Bonding and Molecular Structure

Linus Pauling noticed that the energy of a polar bond is often greater than expected. He attributed the greater bond energy to

Use VSEPR theory to predict the molecular geometry of BrF5.

Place the following molecules in order from smallest to largest H−N−H bond angles: NH4+, NH3, and NH2-.

One might expect PCl3 to have a trigonal planar molecular geometry since its central atom is surrounded by three outer atoms. However, PCl3 has a trigonal pyramidal geometry. Explain.

Using bond-energy data, what is ?rH for the following reaction? CH4(g) + 2Cl2(g) ? CCl4(g) + 2H2(g) Bond Bond Energy (/) - 413 - 432 - 242 - 328

In molecules, as bond order increases,

The correct Lewis structure for Cl2CO is (the 2 Cl's and the O are bound to the C and not to each other):

Which of the following molecules is polar?

What is the correct Lewis structure for SF4?

Electronegativity is a measure of _____.

The central atom in N2O is a nitrogen atom. This nitrogen atom is surrounded by

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of boron tribromide, BBr3.

What is the formal charge on the O2 atom in the following Lewis structure?

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

Determine the bond order of NO+?

What is the formal charge on the carbon atom in CO?

Which of the following is the correct Lewis structure for the sulfate ion?

According to VSEPR theory, which of the following is the correct statement concerning the electron-pair geometry and the molecular geometry of sulfur dioxide?

Use VSEPR theory to predict the molecular geometry around the nitrogen atom in nitrite ion, NO2-.

Which of the following elements is able to form a molecular structure that exceeds the octet rule?

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

Use VSEPR theory to predict the molecular geometry of BrF₅.

Place the following molecules in order from smallest to largest H−N−H bond angles: NH₄⁺, NH₃, and NH₂^-.

One might expect PCl₃ to have a trigonal planar molecular geometry since its central atom is surrounded by three outer atoms. However, PCl₃ has a trigonal pyramidal geometry. Explain.

Using bond-energy data, what is ?_rH for the following reaction? CH₄(g) + 2Cl₂(g) ? CCl₄(g) + 2H₂(g) Bond Bond Energy (/) - 413 - 432 - 242 - 328

The correct Lewis structure for Cl₂CO is (the 2 Cl's and the O are bound to the C and not to each other):

What is the correct Lewis structure for SF₄?

The central atom in N₂O is a nitrogen atom. This nitrogen atom is surrounded by

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of boron tribromide, BBr₃.

What is the formal charge on the O₂ atom in the following Lewis structure?

Use VSEPR theory to predict the molecular geometry around the nitrogen atom in nitrite ion, NO₂^-.