Question 1

Which of the following solids would have the highest melting point?

Accepted Answer

A) NaI 
B) NaF 
C) MgO 
D) MgCl2 
E) KF 
A) NaI 
B) NaF 
C) MgO 
D) MgCl2 
E) KF

Question 2

Which one of the following is most likely to be an ionic compound?

Accepted Answer

A) ClF3 
B) FeCl3 
C) NH3 
D) PF3 
E) SO3 
A) ClF3 
B) FeCl3 
C) NH3 
D) PF3 
E) SO3

Question 3

The number of lone electron pairs in the NO2- ion is ___.

Accepted Answer

A) 4 
B) 5 
C) 6 
D) 7 
E) 8 
A) 4 
B) 5 
C) 6 
D) 7 
E) 8

Question 4

A charge of 2+ is most likely to occur for an ion formed from an atom whose electron configuration is 1s22s22p63s23p4.

Accepted Answer

A) True 
 B)False

Question 5

In the best Lewis structure for the fulminate ion, CNO-, what is the formal charge on the central nitrogen atom?

Accepted Answer

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

Question 6

Which of the following Lewis structures is incorrect?

Accepted Answer

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

Question 7

Use the Born-Haber cycle to calculate the lattice energy of NaBr(s)given the
following data:
$\Delta$H(sublimation)Na = 109 kJ/mol
I1 (Na)= 496 kJ/mol
Bond energy (Br-Br)= 192 kJ/mol
EA (Br)= 324 kJ/mol
$\Delta$Hf (NaBr(s))= -361 kJ/mol

Accepted Answer

The answer of Use the Born-Haber cycle to calculate the...

Question 8

Write a Lewis structure for SO3 that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for SO3 that obey the octet rule.

Accepted Answer

@#IMG-DLM& Total number of res

Question 9

The electron dot structure for AsCl3 shows

Accepted Answer

A) a total of 84 electron dots. 
B) three single bonds and 10 lone pairs. 
C) two single bonds, one double bond, and 9 lone pairs. 
D) one single bond, two double bonds, and 8 lone pairs. 
E) three single bonds and one lone pair. 
A) a total of 84 electron dots. 
B) three single bonds and 10 lone pairs. 
C) two single bonds, one double bond, and 9 lone pairs. 
D) one single bond, two double bonds, and 8 lone pairs. 
E) three single bonds and one lone pair.

Question 10

Classify the O - H bond in CH3OH as ionic, polar covalent, or nonpolar covalent.

Accepted Answer

A) ionic 
B) polar covalent 
C) nonpolar covalent 
A) ionic 
B) polar covalent 
C) nonpolar covalent

Question 11

What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule?

Accepted Answer

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

Question 12

Write the Lewis dot symbol for the chloride ion.

Accepted Answer

The answer of Write the Lewis dot symbol for the...

Question 13

The azide ion, N3-, is very reactive although it is isoelectronic with the very stable CO2 molecule. This reactivity is reasonable inasmuch as

Accepted Answer

A) a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero. 
B) there is no valid Lewis structure possible for the azide ion. 
C) there are resonance structures for azide ion but not for carbon dioxide. 
D) nitrogen cannot form multiple bonds. 
E) charged species always decompose in solution. 
A) a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero. 
B) there is no valid Lewis structure possible for the azide ion. 
C) there are resonance structures for azide ion but not for carbon dioxide. 
D) nitrogen cannot form multiple bonds. 
E) charged species always decompose in solution.

Question 14

Estimate the enthalpy change for the reaction 2CO + O2$\rarr$ 2CO2 given the following bond energies. BE(C$\equiv$O)= 1074 kJ/mol
BE(O=O)= 499 kJ/mol
BE(C=O)= 802 kJ/mol

Accepted Answer

A) +2380 kJ/mol 
B) +744 kJ/mol 
C) +1949 kJ/mol 
D) -561 kJ/mol 
E) -744 kJ/mol 
A) +2380 kJ/mol 
B) +744 kJ/mol 
C) +1949 kJ/mol 
D) -561 kJ/mol 
E) -744 kJ/mol

Question 15

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero?

Accepted Answer

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

Question 16

Calculate the energy required for the gas phase process represented by
Na(g)+ Br(g)$\rarr$ Na+(g)+ Br - (g)
Given: Ionization energy (Na)= 496 kJ/mol
Electron affinity (Br)= 324 kJ/mol
Electron affinity (Na)= 53 kJ/mol

Accepted Answer

The answer of Calculate the energy required for the gas...

Question 17

Nitrous oxide, N2O, is sometimes called "laughing gas". What is the formal charge on the central nitrogen atom in the best Lewis structure for nitrous oxide? (The atom connectivity is N-N-O.)

Accepted Answer

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

Question 18

Classify the C - Cl bond in CCl4 as ionic, polar covalent, or nonpolar covalent.

Accepted Answer

A) ionic 
B) polar covalent 
C) nonpolar covalent 
A) ionic 
B) polar covalent 
C) nonpolar covalent

Which of the following solids would have the highest melting point?

Which one of the following is most likely to be an ionic compound?

The number of lone electron pairs in the NO₂^- ion is ___.

A charge of 2+ is most likely to occur for an ion formed from an atom whose electron configuration is 1s²2s²2p⁶3s²3p⁴.

In the best Lewis structure for the fulminate ion, CNO^-, what is the formal charge on the central nitrogen atom?

Which of the following Lewis structures is incorrect?

Use the Born-Haber cycle to calculate the lattice energy of NaBr(s)given the following data: $\Delta$ H(sublimation)Na = 109 kJ/mol I₁ (Na)= 496 kJ/mol Bond energy (Br-Br)= 192 kJ/mol EA (Br)= 324 kJ/mol $\Delta$ H_f (NaBr(s))= -361 kJ/mol

Write a Lewis structure for SO₃ that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for SO₃ that obey the octet rule.

The electron dot structure for AsCl₃ shows

Classify the O - H bond in CH₃OH as ionic, polar covalent, or nonpolar covalent.

What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule?

Write the Lewis dot symbol for the chloride ion.

The azide ion, N₃^-, is very reactive although it is isoelectronic with the very stable CO₂ molecule. This reactivity is reasonable inasmuch as

Estimate the enthalpy change for the reaction 2CO + O₂ $\rarr$ 2CO₂ given the following bond energies. BE(C $\equiv$ O)= 1074 kJ/mol BE(O=O)= 499 kJ/mol BE(C=O)= 802 kJ/mol

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero?

Calculate the energy required for the gas phase process represented by Na(g)+ Br(g) $\rarr$ Na⁺(g)+ Br^-(g) Given: Ionization energy (Na)= 496 kJ/mol Electron affinity (Br)= 324 kJ/mol Electron affinity (Na)= 53 kJ/mol

Nitrous oxide, N₂O, is sometimes called "laughing gas". What is the formal charge on the central nitrogen atom in the best Lewis structure for nitrous oxide? (The atom connectivity is N-N-O.)

Classify the C - Cl bond in CCl₄ as ionic, polar covalent, or nonpolar covalent.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 9: Chemical Bonding I: the Covalent Bond

Which of the following solids would have the highest melting point?

Which one of the following is most likely to be an ionic compound?

The number of lone electron pairs in the NO2- ion is ___.

A charge of 2+ is most likely to occur for an ion formed from an atom whose electron configuration is 1s22s22p63s23p4.

In the best Lewis structure for the fulminate ion, CNO-, what is the formal charge on the central nitrogen atom?

Which of the following Lewis structures is incorrect?

Use the Born-Haber cycle to calculate the lattice energy of NaBr(s)given the following data: Δ\DeltaΔ H(sublimation)Na = 109 kJ/mol I1 (Na)= 496 kJ/mol Bond energy (Br-Br)= 192 kJ/mol EA (Br)= 324 kJ/mol Δ\DeltaΔ Hf (NaBr(s))= -361 kJ/mol

Write a Lewis structure for SO3 that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for SO3 that obey the octet rule.

The electron dot structure for AsCl3 shows

Classify the O - H bond in CH3OH as ionic, polar covalent, or nonpolar covalent.

What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule?

Write the Lewis dot symbol for the chloride ion.

The azide ion, N3-, is very reactive although it is isoelectronic with the very stable CO2 molecule. This reactivity is reasonable inasmuch as

Estimate the enthalpy change for the reaction 2CO + O2 →\rarr→ 2CO2 given the following bond energies. BE(C ≡\equiv≡ O)= 1074 kJ/mol BE(O=O)= 499 kJ/mol BE(C=O)= 802 kJ/mol

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero?

Calculate the energy required for the gas phase process represented by Na(g)+ Br(g) →\rarr→ Na+(g)+ Br - (g) Given: Ionization energy (Na)= 496 kJ/mol Electron affinity (Br)= 324 kJ/mol Electron affinity (Na)= 53 kJ/mol

Nitrous oxide, N2O, is sometimes called "laughing gas". What is the formal charge on the central nitrogen atom in the best Lewis structure for nitrous oxide? (The atom connectivity is N-N-O.)

Classify the C - Cl bond in CCl4 as ionic, polar covalent, or nonpolar covalent.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

The number of lone electron pairs in the NO₂^- ion is ___.

A charge of 2+ is most likely to occur for an ion formed from an atom whose electron configuration is 1s²2s²2p⁶3s²3p⁴.

In the best Lewis structure for the fulminate ion, CNO^-, what is the formal charge on the central nitrogen atom?

Use the Born-Haber cycle to calculate the lattice energy of NaBr(s)given the following data: $\Delta$ H(sublimation)Na = 109 kJ/mol I₁ (Na)= 496 kJ/mol Bond energy (Br-Br)= 192 kJ/mol EA (Br)= 324 kJ/mol $\Delta$ H_f (NaBr(s))= -361 kJ/mol

Write a Lewis structure for SO₃ that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for SO₃ that obey the octet rule.

The electron dot structure for AsCl₃ shows

Classify the O - H bond in CH₃OH as ionic, polar covalent, or nonpolar covalent.

The azide ion, N₃^-, is very reactive although it is isoelectronic with the very stable CO₂ molecule. This reactivity is reasonable inasmuch as

Estimate the enthalpy change for the reaction 2CO + O₂ $\rarr$ 2CO₂ given the following bond energies. BE(C $\equiv$ O)= 1074 kJ/mol BE(O=O)= 499 kJ/mol BE(C=O)= 802 kJ/mol

Calculate the energy required for the gas phase process represented by Na(g)+ Br(g) $\rarr$ Na⁺(g)+ Br^-(g) Given: Ionization energy (Na)= 496 kJ/mol Electron affinity (Br)= 324 kJ/mol Electron affinity (Na)= 53 kJ/mol

Nitrous oxide, N₂O, is sometimes called "laughing gas". What is the formal charge on the central nitrogen atom in the best Lewis structure for nitrous oxide? (The atom connectivity is N-N-O.)

Classify the C - Cl bond in CCl₄ as ionic, polar covalent, or nonpolar covalent.