Question 1

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 2

Write a Lewis structure for the phosphate ion, PO43-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

Accepted Answer

Question 3

The total number of lone pairs in NCl3 is

Accepted Answer

A) 6 
B) 8 
C) 9 
D) 10 
E) 13 
A) 6 
B) 8 
C) 9 
D) 10 
E) 13

Question 4

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 5

Which one of these polar covalent bonds would have the greatest percent ionic character?

Accepted Answer

A) H -Br 
B) H - Cl 
C) H - F 
D) H- I 
A) H -Br 
B) H - Cl 
C) H - F 
D) H- I

Question 6

Each of the three resonance structures of NO3- has how many lone pairs of electrons?

Accepted Answer

A) 7 
B) 8 
C) 9 
D) 10 
E) 13 
A) 7 
B) 8 
C) 9 
D) 10 
E) 13

Question 7

Which of the atoms listed below is the most electronegative?

Accepted Answer

A) Li 
B) Cs 
C) P 
D) As 
E) Ge 
A) Li 
B) Cs 
C) P 
D) As 
E) Ge

Question 8

The Lewis dot symbol for the S 2- ion is

Accepted Answer

A)  ( ) 
B)  (  2-) 
C) (S2-) 
D) (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
  F1F1F1S1F1F1F10 2-) 
E)  (  F1F1F1S1F1F1F10) 
A)  ( ) 
B)  (  2-) 
C) (S2-) 
D) (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
  F1F1F1S1F1F1F10 2-) 
E)  (  F1F1F1S1F1F1F10)

Question 9

Which one of the following is most likely to be a covalent compound?

Accepted Answer

A) Rb2O 
B) BaO 
C) SrO 
D) SeO2 
E) MnO2 
A) Rb2O 
B) BaO 
C) SrO 
D) SeO2 
E) MnO2

Question 10

Use bond energies to estimate the enthalpy change for the reaction of one mole ofCH4 with chlorine gas to give CH3Cl and hydrogen chloride. BE(C-H)= 414 kJ/mol
BE(C-Cl)= 326 kJ/mol
BE(H-Cl)= 432 kJ/mol
BE(Cl-Cl)= 243 kJ/mol

Accepted Answer

A) -101 kJ/mol 
B) -106 kJ/mol 
C) +331 kJ/mol 
D) +106 kJ/mol 
E) +101 kJ/mol 
A) -101 kJ/mol 
B) -106 kJ/mol 
C) +331 kJ/mol 
D) +106 kJ/mol 
E) +101 kJ/mol

Question 11

Consider the hypothetical element Y with electron-dot formula   Give the formula for the simplest compound this element forms with chlorine.

Accepted Answer

The answer of Consider the hypothetical element Y with electron-dot...

Question 12

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 13

The formal charge on the sulfur atom in the resonance structure of sulfur dioxide which has one single bond and one double bond is

Accepted Answer

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

Question 14

Write the Lewis structure for the product that forms when boron trifluoride combines with ammonia.

Accepted Answer

The answer of Write the Lewis structure for the product...

Question 15

Write a Lewis structure for the nitrate ion, NO3-, showing all non-zero formal charges.

Accepted Answer

Question 16

The bond in which of the following pairs of atoms would be the least polar (i.e., lowest percent ionic character)?

Accepted Answer

A) C - Cl 
B) C - C 
C) C - H 
D) O - C 
E) N - C 
A) C - Cl 
B) C - C 
C) C - H 
D) O - C 
E) N - C

Question 17

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 18

What type of chemical bond holds the atoms together within a water molecule?

Accepted Answer

A) Ionic bond 
B) Nonpolar covalent bond 
C) Polar covalent bond 
D) Coordinate covalent bond 
A) Ionic bond 
B) Nonpolar covalent bond 
C) Polar covalent bond 
D) Coordinate covalent bond

Question 19

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 20

The covalent bond with the greatest polarity would form in which of the atom pairs below?

Accepted Answer

A) Br - Br 
B) S - O 
C) C - P 
D) C - O 
E) B - O 
A) Br - Br 
B) S - O 
C) C - P 
D) C - O 
E) B - O

Exam 9: Chemical Bonding I: Basic Concepts

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

Write a Lewis structure for the phosphate ion, PO43-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

The total number of lone pairs in NCl3 is

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

Which one of these polar covalent bonds would have the greatest percent ionic character?

Each of the three resonance structures of NO3- has how many lone pairs of electrons?

Which of the atoms listed below is the most electronegative?

The Lewis dot symbol for the S 2- ion is

Which one of the following is most likely to be a covalent compound?

Use bond energies to estimate the enthalpy change for the reaction of one mole ofCH4 with chlorine gas to give CH3Cl and hydrogen chloride. BE(C-H)= 414 kJ/mol BE(C-Cl)= 326 kJ/mol BE(H-Cl)= 432 kJ/mol BE(Cl-Cl)= 243 kJ/mol

Consider the hypothetical element Y with electron-dot formula Give the formula for the simplest compound this element forms with chlorine.

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

The formal charge on the sulfur atom in the resonance structure of sulfur dioxide which has one single bond and one double bond is

Write the Lewis structure for the product that forms when boron trifluoride combines with ammonia.

Write a Lewis structure for the nitrate ion, NO3-, showing all non-zero formal charges.

The bond in which of the following pairs of atoms would be the least polar (i.e., lowest percent ionic character)?

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

What type of chemical bond holds the atoms together within a water molecule?

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

The covalent bond with the greatest polarity would form in which of the atom pairs below?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

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

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Write a Lewis structure for the phosphate ion, PO₄^3-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

The total number of lone pairs in NCl₃ is

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

Each of the three resonance structures of NO₃^- has how many lone pairs of electrons?

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

Use bond energies to estimate the enthalpy change for the reaction of one mole ofCH₄ with chlorine gas to give CH₃Cl and hydrogen chloride. BE(C-H)= 414 kJ/mol BE(C-Cl)= 326 kJ/mol BE(H-Cl)= 432 kJ/mol BE(Cl-Cl)= 243 kJ/mol

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

Write a Lewis structure for the nitrate ion, NO₃^-, showing all non-zero formal charges.