Question 1

Which of the following has the most valence electrons?

Accepted Answer

A) HF 
B) NS 
C) CNF1F1F1S1F1F1F10 
D) ArF 
E) ArFF1F1F1S1F1F1F10 
A) HF 
B) NS 
C) CNF1F1F1S1F1F1F10 
D) ArF 
E) ArFF1F1F1S1F1F1F10

Question 2

The measure of an atom's ability to attract electrons in a chemical bond is called ________

Accepted Answer

A) hybridization. 
B) ionization energy. 
C) electron affinity. 
D) electronegativity. 
E) ionic radius. 
A) hybridization. 
B) ionization energy. 
C) electron affinity. 
D) electronegativity. 
E) ionic radius.

Question 3

How many lone-pair electrons are on the central oxygen atom in the Lewis structure for dinitrogen pentoxide (N2O5)? A skeleton of the molecule is provided below.

Accepted Answer

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

Question 4

Nitrite (NO2F1F1F1S1F1F1F10) is an important nutrient in the eutrophic zone of the ocean. Which of the following is the correct set of resonance structures for this ion?

Accepted Answer

A) I 
B) II 
C) III 
D) IV 
A) I 
B) II 
C) III 
D) IV

Question 5

When sulfur-containing fuels are burned, sulfur trioxide (SO3) is formed in the atmosphere and contributes to acid rain (sulfur trioxide plus water produces sulfuric acid). How many resonance structures are there for SO3 when each atom satisfies the octet rule?

Accepted Answer

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

Question 6

Draw the Lewis structure for the oxalate anion, C2O42F1F1F1S1F1F1F10. Include all reasonable resonance structures.

Accepted Answer

Question 7

In which bond does the Cl atom have the highest electron density?

Accepted Answer

A) HF1F1F1S1F1F1F10Cl 
B) OF1F1F1S1F1F1F10Cl 
C) SF1F1F1S1F1F1F10Cl 
D) NF1F1F1S1F1F1F10Cl 
E) BrF1F1F1S1F1F1F10Cl 
A) HF1F1F1S1F1F1F10Cl 
B) OF1F1F1S1F1F1F10Cl 
C) SF1F1F1S1F1F1F10Cl 
D) NF1F1F1S1F1F1F10Cl 
E) BrF1F1F1S1F1F1F10Cl

Question 8

How many shared electron pairs are there in the Lewis structure of CNF1F1F1S1F1F1F10?

Accepted Answer

A) 3 
B) 6 
C) 4 
D) 2 
E) 10 
A) 3 
B) 6 
C) 4 
D) 2 
E) 10

Question 9

Which statements correctly describe a polar covalent bond?
I. Electrons are shared but not equally by the two atoms.
II. One atom has a small negative charge, and the other atom has a small positive charge.
III. The bond dipole is zero.
IV. One or more electrons are transferred from one atom to a second atom.

Accepted Answer

A) I and II only 
B) II and III only 
C) III and IV only 
D) I and III only 
E) I and IV only 
A) I and II only 
B) II and III only 
C) III and IV only 
D) I and III only 
E) I and IV only

Question 10

What is the formal charge of the nitrogen atom in hydrogen cyanide (HCN)?

Accepted Answer

A) (F1F1F1S1F1F1F101) 
B) 0 
C) 1 
D) 5 
E) 2 
A) (F1F1F1S1F1F1F101) 
B) 0 
C) 1 
D) 5 
E) 2

Question 11

Hydrogen isocyanide (HNC) and hydrogen cyanide (HCN) have the same elemental composition. Is one structure more stable than the other? Support your answer with the Lewis structures and formal charges assigned to each atom for these molecules.

Accepted Answer

@#IMG-DLM& The formal charges are zero u

Question 12

In which bond does the H atom have the highest electron density?

Accepted Answer

A) HF1F1F1S1F1F1F10Cl 
B) HF1F1F1S1F1F1F10Li 
C) HF1F1F1S1F1F1F10N 
D) HF1F1F1S1F1F1F10O 
E) HF1F1F1S1F1F1F10C 
A) HF1F1F1S1F1F1F10Cl 
B) HF1F1F1S1F1F1F10Li 
C) HF1F1F1S1F1F1F10N 
D) HF1F1F1S1F1F1F10O 
E) HF1F1F1S1F1F1F10C

Question 13

Which of the following properties is typically used to identify whether a bond is polar, nonpolar, or ionic?

Accepted Answer

A) electronegativity 
B) ionization energy 
C) atomic radius 
D) electron affinity 
E) atomic mass 
A) electronegativity 
B) ionization energy 
C) atomic radius 
D) electron affinity 
E) atomic mass

Question 14

Which of the following pairs of Lewis structures are not resonance structures of one another?

Accepted Answer

A) I 
B) II 
C) III 
D) IV 
E) All pairs are resonance structures. 
A) I 
B) II 
C) III 
D) IV 
E) All pairs are resonance structures.

Question 15

Which of the following bonds is the strongest?

Accepted Answer

A) CF1F1F1S1F1F1F10O 
B) C   O 
C) O   O 
D) C   O 
A) CF1F1F1S1F1F1F10O 
B) C   O 
C) O   O 
D) C   O

Question 16

Which of the following bonds is the weakest?

Accepted Answer

A) CF1F1F1S1F1F1F10O 
B) C   O 
C) O   O 
D) C   O 
A) CF1F1F1S1F1F1F10O 
B) C   O 
C) O   O 
D) C   O

Which of the following has the most valence electrons?

The measure of an atom's ability to attract electrons in a chemical bond is called ________

How many lone-pair electrons are on the central oxygen atom in the Lewis structure for dinitrogen pentoxide (N₂O₅)? A skeleton of the molecule is provided below.

Nitrite (NO₂^) is an important nutrient in the eutrophic zone of the ocean. Which of the following is the correct set of resonance structures for this ion?

When sulfur-containing fuels are burned, sulfur trioxide (SO₃) is formed in the atmosphere and contributes to acid rain (sulfur trioxide plus water produces sulfuric acid). How many resonance structures are there for SO₃ when each atom satisfies the octet rule?

Draw the Lewis structure for the oxalate anion, C₂O₄²^. Include all reasonable resonance structures.

In which bond does the Cl atom have the highest electron density?

How many shared electron pairs are there in the Lewis structure of CN^?

What is the formal charge of the nitrogen atom in hydrogen cyanide (HCN)?

Hydrogen isocyanide (HNC) and hydrogen cyanide (HCN) have the same elemental composition. Is one structure more stable than the other? Support your answer with the Lewis structures and formal charges assigned to each atom for these molecules.

In which bond does the H atom have the highest electron density?

Which of the following properties is typically used to identify whether a bond is polar, nonpolar, or ionic?

Which of the following pairs of Lewis structures are not resonance structures of one another?

Which of the following bonds is the strongest?

Which of the following bonds is the weakest?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Exam 8: Chemical Bonds: What Makes a Gas a Greenhouse Gas

Which of the following has the most valence electrons?

The measure of an atom's ability to attract electrons in a chemical bond is called ________

How many lone-pair electrons are on the central oxygen atom in the Lewis structure for dinitrogen pentoxide (N2O5)? A skeleton of the molecule is provided below.

Nitrite (NO2) is an important nutrient in the eutrophic zone of the ocean. Which of the following is the correct set of resonance structures for this ion?

When sulfur-containing fuels are burned, sulfur trioxide (SO3) is formed in the atmosphere and contributes to acid rain (sulfur trioxide plus water produces sulfuric acid). How many resonance structures are there for SO3 when each atom satisfies the octet rule?

Draw the Lewis structure for the oxalate anion, C2O42. Include all reasonable resonance structures.

In which bond does the Cl atom have the highest electron density?

How many shared electron pairs are there in the Lewis structure of CN?

What is the formal charge of the nitrogen atom in hydrogen cyanide (HCN)?

Hydrogen isocyanide (HNC) and hydrogen cyanide (HCN) have the same elemental composition. Is one structure more stable than the other? Support your answer with the Lewis structures and formal charges assigned to each atom for these molecules.

In which bond does the H atom have the highest electron density?

Which of the following properties is typically used to identify whether a bond is polar, nonpolar, or ionic?

Which of the following pairs of Lewis structures are not resonance structures of one another?

Which of the following bonds is the strongest?

Which of the following bonds is the weakest?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

How many lone-pair electrons are on the central oxygen atom in the Lewis structure for dinitrogen pentoxide (N₂O₅)? A skeleton of the molecule is provided below.

Nitrite (NO₂^) is an important nutrient in the eutrophic zone of the ocean. Which of the following is the correct set of resonance structures for this ion?

When sulfur-containing fuels are burned, sulfur trioxide (SO₃) is formed in the atmosphere and contributes to acid rain (sulfur trioxide plus water produces sulfuric acid). How many resonance structures are there for SO₃ when each atom satisfies the octet rule?

Draw the Lewis structure for the oxalate anion, C₂O₄²^. Include all reasonable resonance structures.

How many shared electron pairs are there in the Lewis structure of CN^?