Question 1

BeF42- is called the fluoberyllate ion.The formal charge on the beryllium atom in this ion is

Accepted Answer

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

Question 2

Write the Lewis dot symbol for the chloride ion.

Accepted Answer

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

Question 3

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 B

Question 4

Arrange the elements C, O, and H in order of increasing electronegativity

Accepted Answer

A) C < O < H 
B) H < C < O 
C) C < H < O 
D) O < C < H E H < O < C 
A) C < O < H 
B) H < C < O 
C) C < H < O 
D) O < C < H E H < O < C

Question 5

What type of bonding is present in the molecule NH2NH2 (ionic, covalent, or both)?

Accepted Answer

Question 6

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

Accepted Answer

A) NCl3 
B) BaCl2 
C) CO 
D) SO2 
E) SF4 
A) NCl3 
B) BaCl2 
C) CO 
D) SO2 
E) SF4

Question 7

Use bond energies to estimate the enthalpy of formation of HBr(g). BE(H-H)= 436 kJ/mol
BE(Br-Br)= 192 kJ/mol
BE(H-Br)= 366 kJ/mol

Accepted Answer

A) +262 kJ/mol 
B) +104 kJ/mol 
C) +52 kJ/mol 
D) -52 kJ/mol 
E) -104 kJ/mol 
A) +262 kJ/mol 
B) +104 kJ/mol 
C) +52 kJ/mol 
D) -52 kJ/mol 
E) -104 kJ/mol

Question 8

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

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 9

Complete this statement: Coulomb's law states that the magnitude of the force of interaction between two charged bodies is

Accepted Answer

A) directly proportional to the product of the charges on the bodies and directly proportional to the distance separating them. 
B) directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance separating them. 
C) inversely proportional to the product of the charges on the bodies, and directly proportional to the square of the distance separating them. 
D) directly proportional to the sum of the charges on the bodies, and inversely proportional to the square of the distance separating them. 
A) directly proportional to the product of the charges on the bodies and directly proportional to the distance separating them. 
B) directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance separating them. 
C) inversely proportional to the product of the charges on the bodies, and directly proportional to the square of the distance separating them. 
D) directly proportional to the sum of the charges on the bodies, and inversely proportional to the square of the distance separating them.

Question 10

Write a Lewis structure for SO3 that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

Accepted Answer

Question 11

Assuming the octet rule is obeyed, how many covalent bonds will an oxygen 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 12

Use the Born-Haber cycle to calculate the lattice energy of MgO (s)given the following data: $\Delta$H(sublimation)Mg = 130 kJ/mol
I1 (Mg)= 738.1 kJ/mol
I2 (Mg)= 1450 kJ/mol
Bond energy (O=O)= 498.7 kJ/mol
EA (O)= 141 kJ/mol
EA (O-)= -780 kJ/mol
$\Delta$H    
(MgO(s))= -601.8 kJ/mol

Accepted Answer

A) 2200 kJ/mol 
B) 2800 kJ/mol 
C) 3200 kJ/mol 
D) 3800 kJ/mol 
E) 4100 kJ/mol 
A) 2200 kJ/mol 
B) 2800 kJ/mol 
C) 3200 kJ/mol 
D) 3800 kJ/mol 
E) 4100 kJ/mol

Question 13

The number of resonance structures for the nitrate ion that satisfy the octet rule is

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) None of these 
A) 1 
B) 2 
C) 3 
D) 4 
E) None of these

Question 14

List all types of bonding present in the molecule SO3  I.ionic bond
II.polar covalent bond
III.nonpolar covalent bond

Accepted Answer

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

Question 15

Arrange the following bonds in order of increasing ionic character

Accepted Answer

A) B - C < C - N < C - O < C - C 
B) C - C < B - C < C - N < C - O 
C) C - C < C - N < B - C < C - O 
D) C - O < C - N < B - C < C - C 
E) C - N < C - C < B - C < C - O 
A) B - C < C - N < C - O < C - C 
B) C - C < B - C < C - N < C - O 
C) C - C < C - N < B - C < C - O 
D) C - O < C - N < B - C < C - C 
E) C - N < C - C < B - C < C - O

Question 16

Of the species NO2, NO, and N2, only NO2 is an exception to the octet rule.

Accepted Answer

A) True 
 B)False

Question 17

The Lewis dot symbol for the S 2- ion is

Accepted Answer

A)      
B)      2- 
C) S2- 
D) -     - 2- 
E)      - 
A)      
B)      2- 
C) S2- 
D) -     - 2- 
E)      -

Question 18

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 19

A molecule with two resonance structures is shifting quickly back and forth from one structure to the other

Accepted Answer

A) True 
 B)False

Question 20

Arrange the following bonds in order of increasing ionic character

Accepted Answer

A) C - F < O - F < H - F < Na - F 
B) C - F < H - F < O - F < Na - F 
C) O - F < C - F < H - F < Na - F 
D) H - F < C - F < O - F < Na - F 
E) Na - F < H - F < C - F < O - F 
A) C - F < O - F < H - F < Na - F 
B) C - F < H - F < O - F < Na - F 
C) O - F < C - F < H - F < Na - F 
D) H - F < C - F < O - F < Na - F 
E) Na - F < H - F < C - F < O - F

Exam 9: Chemical Bonding I: Basic Concepts

BeF42- is called the fluoberyllate ion.The formal charge on the beryllium atom in this ion is

Write the Lewis dot symbol for the chloride ion.

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

Arrange the elements C, O, and H in order of increasing electronegativity

What type of bonding is present in the molecule NH2NH2 (ionic, covalent, or both)?

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

Use bond energies to estimate the enthalpy of formation of HBr(g). BE(H-H)= 436 kJ/mol BE(Br-Br)= 192 kJ/mol BE(H-Br)= 366 kJ/mol

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

Complete this statement: Coulomb's law states that the magnitude of the force of interaction between two charged bodies is

Write a Lewis structure for SO3 that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

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

Use the Born-Haber cycle to calculate the lattice energy of MgO (s)given the following data: Δ\DeltaΔ H(sublimation)Mg = 130 kJ/mol I1 (Mg)= 738.1 kJ/mol I2 (Mg)= 1450 kJ/mol Bond energy (O=O)= 498.7 kJ/mol EA (O)= 141 kJ/mol EA (O-)= -780 kJ/mol Δ\DeltaΔ H (MgO(s))= -601.8 kJ/mol

The number of resonance structures for the nitrate ion that satisfy the octet rule is

List all types of bonding present in the molecule SO3 I.ionic bond II.polar covalent bond III.nonpolar covalent bond

Arrange the following bonds in order of increasing ionic character

Of the species NO2, NO, and N2, only NO2 is an exception to the octet rule.

The Lewis dot symbol for the S 2- ion is

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

A molecule with two resonance structures is shifting quickly back and forth from one structure to the other

Arrange the following bonds in order of increasing ionic character

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

BeF₄^2- is called the fluoberyllate ion.The formal charge on the beryllium atom in this ion is

What type of bonding is present in the molecule NH₂NH₂ (ionic, covalent, or both)?

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

Write a Lewis structure for SO₃ that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

List all types of bonding present in the molecule SO₃ I.ionic bond II.polar covalent bond III.nonpolar covalent bond

Of the species NO₂, NO, and N₂, only NO₂ is an exception to the octet rule.

The Lewis dot symbol for the S^2- ion is