Question 1

Is it possible for a molecule to be nonpolar even though it contains polar bonds?
 Explain your answer and give an example.

Accepted Answer

Yes.The polarity of a molecule depends on the molecular geometry and whether or not all of the dipoles (polar bonds)cancel one another.If the molecular geometry causes all of the dipoles to cancel,the molecule will be nonpolar.An example is CF₄ where there are four polar bonds,but the dipoles sum to 0 making the molecule nonpolar.

Question 2

Choose the bond below that is the strongest.

Accepted Answer

A)  N=O 
B)  N-Br 
C)  N-O 
D)  N-C 
E)  N=N 
A)  N=O 
B)  N-Br 
C)  N-O 
D)  N-C 
E)  N=N A

Question 3

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 C

Question 4

Give the number of valence electrons for S I4.

Accepted Answer

A)  28 
B)  30 
C)  32 
D)  34 
A)  28 
B)  30 
C)  32 
D)  34

Question 5

Choose the best Lewis structure for BF3.

Accepted Answer

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

Question 6

Determine the electron geometry (eg)and molecular geometry (mg)of ICl2⁻.

Accepted Answer

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

Question 7

Choose the best Lewis structure for SF4.

Accepted Answer

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

Question 8

Draw the best Lewis structure for ClO⁻ and determine the formal charge on chlorine.

Accepted Answer

A)  -1 
B)  +1 
C)  0 
D)  +2 
E)  +3 
A)  -1 
B)  +1 
C)  0 
D)  +2 
E)  +3

Question 9

Place the following in order of decreasing X-A-X bond angle,where A represents the central atom and X represents the outer atoms in each molecule. CS2 CF4 SCl2

Accepted Answer

A)  CS2 > SCl2 > CF4 
B)  SCl2 > CF4 > CS2 
C)  CF4 > SCl2 > CS2 
D)  CS2 > CF4 > SCl2 
E)  CF4 > CS2 > SCl2 
A)  CS2 > SCl2 > CF4 
B)  SCl2 > CF4 > CS2 
C)  CF4 > SCl2 > CS2 
D)  CS2 > CF4 > SCl2 
E)  CF4 > CS2 > SCl2

Question 10

Determine the electron geometry,molecular geometry and polarity of HBrO2.

Accepted Answer

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

Question 11

The arsenic atom in AsCl3 would be expected to have a

Accepted Answer

A)  partial positive (δ+) charge. 
B)  partial negative (δ-) charge. 
C)  3+ charge. 
D)  3- charge. 
A)  partial positive (δ+) charge. 
B)  partial negative (δ-) charge. 
C)  3+ charge. 
D)  3- charge.

Question 12

How many lone pairs of electrons are on the P atom in P F3?

Accepted Answer

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

Question 13

Explain why oil and water do not mix.

Accepted Answer

Water molecules are

Question 14

Draw the Lewis structure for SO42⁻.How many equivalent resonance structures can be drawn?

Accepted Answer

A)  6 
B)  2 
C)  4 
D)  3 
E)  8 
A)  6 
B)  2 
C)  4 
D)  3 
E)  8

Question 15

Determine the electron geometry,molecular geometry and polarity of SF4.

Accepted Answer

A)  eg = trigonal bipyramidal, mg = trigonal bipyramidal, nonpolar 
B)  eg = tetrahedral, mg = tetrahedral, polar 
C)  eg = trigonal bipyramidal, mg = see-saw, polar 
D)  eg = octahedral, mg = trigonal bipyramidal, nonpolar 
E)  eg = octahedral, mg = octahedral, nonpolar 
A)  eg = trigonal bipyramidal, mg = trigonal bipyramidal, nonpolar 
B)  eg = tetrahedral, mg = tetrahedral, polar 
C)  eg = trigonal bipyramidal, mg = see-saw, polar 
D)  eg = octahedral, mg = trigonal bipyramidal, nonpolar 
E)  eg = octahedral, mg = octahedral, nonpolar

Question 16

Determine the electron geometry,molecular geometry and polarity of HCN.

Accepted Answer

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

Question 17

Using Lewis structures and formal charge,which of the following ions is most stable?
OCN⁻ ONC⁻ NOC⁻

Accepted Answer

A)  OCN⁻ 
B)  ONC⁻ 
C)  NOC⁻ 
D)  None of these ions are stable according to Lewis theory. 
E)  All of these compounds are equally stable according to Lewis theory. 
A)  OCN⁻ 
B)  ONC⁻ 
C)  NOC⁻ 
D)  None of these ions are stable according to Lewis theory. 
E)  All of these compounds are equally stable according to Lewis theory.

Question 18

Of the following elements,which has the lowest electronegativity?

Accepted Answer

A)  Mg 
B)  Cl 
C)  Ca 
D)  Br 
A)  Mg 
B)  Cl 
C)  Ca 
D)  Br

Question 19

Choose the best Lewis structure for PO43⁻.

Accepted Answer

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

Question 20

List the following compounds in decreasing electronegativity difference. Br2 H Br K Br

Accepted Answer

A)  K Br > Br2 > H Br 
B)  Br2 > H Br > K Br 
C)  H Br > K Br > Br2 
D)  K Br > H Br > Br2 
A)  K Br > Br2 > H Br 
B)  Br2 > H Br > K Br 
C)  H Br > K Br > Br2 
D)  K Br > H Br > Br2

Exam 6: Chemical Bonding I

Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

Choose the bond below that is the strongest.

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

Give the number of valence electrons for S I4.

Choose the best Lewis structure for BF3.

Determine the electron geometry (eg)and molecular geometry (mg)of ICl2⁻.

Choose the best Lewis structure for SF4.

Draw the best Lewis structure for ClO⁻ and determine the formal charge on chlorine.

Place the following in order of decreasing X-A-X bond angle,where A represents the central atom and X represents the outer atoms in each molecule. CS2 CF4 SCl2

Determine the electron geometry,molecular geometry and polarity of HBrO2.

The arsenic atom in AsCl3 would be expected to have a

How many lone pairs of electrons are on the P atom in P F3?

Explain why oil and water do not mix.

Draw the Lewis structure for SO42⁻.How many equivalent resonance structures can be drawn?

Determine the electron geometry,molecular geometry and polarity of SF4.

Determine the electron geometry,molecular geometry and polarity of HCN.

Using Lewis structures and formal charge,which of the following ions is most stable? OCN⁻ ONC⁻ NOC⁻

Of the following elements,which has the lowest electronegativity?

Choose the best Lewis structure for PO43⁻.

List the following compounds in decreasing electronegativity difference. Br2 H Br K Br

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

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

Give the number of valence electrons for S I₄.

Choose the best Lewis structure for BF₃.

Determine the electron geometry (eg)and molecular geometry (mg)of ICl₂⁻.

Choose the best Lewis structure for SF₄.

Place the following in order of decreasing X-A-X bond angle,where A represents the central atom and X represents the outer atoms in each molecule. CS₂ CF₄ SCl₂

Determine the electron geometry,molecular geometry and polarity of HBrO₂.

The arsenic atom in AsCl₃ would be expected to have a

How many lone pairs of electrons are on the P atom in P F₃?

Draw the Lewis structure for SO₄²⁻.How many equivalent resonance structures can be drawn?

Determine the electron geometry,molecular geometry and polarity of SF₄.

Choose the best Lewis structure for PO₄³⁻.

List the following compounds in decreasing electronegativity difference. Br₂ H Br K Br