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

A) 738 kJ/mol B) 748 kJ/mol C) 758 kJ/mol D) 768 kJ/mol E) None of the above A) 738 kJ/mol B) 748 kJ/mol C) 758 kJ/mol D) 768 kJ/mol E) None of the above A

List all types of bonding present in the molecule S8. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

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

Calculate the energy change for the reaction K(g) + I(g) $\rarr$ K+(g) + I - (g) Given the following ionization energy (IE) and electron affinity (EA) values. $\begin{array}{cc} \text { IE } & \text { EA } \\ \text { K: } 419 \mathrm{~kJ} / \mathrm{mol} & 48 \mathrm{~kJ} / \mathrm{mol} \\ \text { I: } 1,010 \mathrm{~kJ} / \mathrm{mol} & 295 \mathrm{~kJ} / \mathrm{mol} \end{array}$

A) -124 kJ/mol B) -715 kJ/mol C) 715 kJ/mol D) 1429 kJ/mol E) None of these A) -124 kJ/mol B) -715 kJ/mol C) 715 kJ/mol D) 1429 kJ/mol E) None of these

Classify the Ca - Cl bond in CaCl2 as ionic, polar covalent, or nonpolar covalent.

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

Calculate the energy change for the reaction K(g) + Br(g) $\rarr$ K+(g) + Br- (g) Given the following ionization energy (IE) and electron affinity (EA) values. $\begin{array}{cc} \text { IE } & \text { EA } \\ \text { K: }: 419 \mathrm{~kJ} / \mathrm{mol} & 48 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Br}: 1140 \mathrm{~kJ} / \mathrm{mol} & 324 \mathrm{~kJ} / \mathrm{mol} \end{array}$

A) -1,092 kJ/mol B) -95 kJ/mol C) 95 kJ/mol D) 1,092 kJ/mol E) 1,187 kJ/mol A) -1,092 kJ/mol B) -95 kJ/mol C) 95 kJ/mol D) 1,092 kJ/mol E) 1,187 kJ/mol

Exam 9: Chemical Bonding I: Basic Concepts

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

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(Multiple Choice)

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Question 1

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Arrange the elements F, P, and Cl in order of increasing electronegativity.

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(Multiple Choice)

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Question 2

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

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

List all types of bonding present in the molecule S₈. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

(Multiple Choice)

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Question 4

Calculate the energy change for the reaction K(g) + I(g) $\rarr$ K⁺(g) + I ^- (g) Given the following ionization energy (IE) and electron affinity (EA) values. IE EA K: 419/ 48/ I: 1,010/ 295/

(Multiple Choice)

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Question 5

The Lewis structure reveals an unpaired electron (free radical) in which of the following species

(Multiple Choice)

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Question 6

Use the Born-Haber cycle to calculate the standard enthalpy of formation ( $\Delta{H}^{\circ}_f$ ) for LiCl(s) given the following data: $\Delta$ H(sublimation) Li = 155.2 kJ/mol I₁ (Li) = 520 kJ/mol Bond energy (Cl-Cl) = 242.7 kJ/mol EA (Cl) = 349 kJ/mol Lattice energy (LiCl(s)) = 828 kJ/mol

(Multiple Choice)

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Question 7

The Lewis dot symbol for the chloride ion is

(Multiple Choice)

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Question 8

The polarity of covalent bonds increases as the percent ionic character increases.

(True/False)

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Question 9

Which of the elements listed below would most likely form an ionic bond when bonded to oxygen

(Multiple Choice)

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Question 10

Which response includes all the molecules below that do not follow the octet rule (1) H₂S (2) BCl₃ (3) PH₃ (4) SF₄

(Multiple Choice)

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Question 11

Classify the Ca - Cl bond in CaCl₂ as ionic, polar covalent, or nonpolar covalent.

(Multiple Choice)

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Question 12

The Si - Cl bond has less ionic character than the C - Cl bond.

(True/False)

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Question 13

The Lewis structure reveals only single bonds in which of the following species

(Multiple Choice)

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Question 14

The Lewis structure for the nitrate ion, NO₃^-, showing all non-zero formal charges is shown here. This structure shows a violation of the octet rule.

(True/False)

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Question 15

Which one of the following compounds utilizes both ionic and covalent bonding

(Multiple Choice)

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Question 16

A Lewis structure for SO₃ that obeys the octet rule, showing all non-zero formal charges, is shown here. How many resonance structures for SO₃ that obey the octet rule, are possible

(Multiple Choice)

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Question 17

Calculate the energy change for the reaction K(g) + Br(g) $\rarr$ K⁺(g) + Br^- (g) Given the following ionization energy (IE) and electron affinity (EA) values. IE EA K: :419/ 48/ :1140/ 324/

(Multiple Choice)

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Question 18

Shown here is a Lewis structure for the chlorate ion, ClO₃^-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s). What is the formal charge on Cl

(Multiple Choice)

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Question 19

A polar covalent bond would form in which one of the following pairs of atoms

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Question 20

Showing 1 - 20 of 136

Exam 9: Chemical Bonding I: Basic Concepts

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

Arrange the elements F, P, and Cl in order of increasing electronegativity.

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

List all types of bonding present in the molecule S8. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

Calculate the energy change for the reaction K(g) + I(g) →\rarr→ K+(g) + I - (g) Given the following ionization energy (IE) and electron affinity (EA) values. IE EA K: 419/ 48/ I: 1,010/ 295/

The Lewis structure reveals an unpaired electron (free radical) in which of the following species

The Lewis dot symbol for the chloride ion is

The polarity of covalent bonds increases as the percent ionic character increases.

Which of the elements listed below would most likely form an ionic bond when bonded to oxygen

Which response includes all the molecules below that do not follow the octet rule (1) H2S (2) BCl3 (3) PH3 (4) SF4

Classify the Ca - Cl bond in CaCl2 as ionic, polar covalent, or nonpolar covalent.

The Si - Cl bond has less ionic character than the C - Cl bond.

The Lewis structure reveals only single bonds in which of the following species

The Lewis structure for the nitrate ion, NO3-, showing all non-zero formal charges is shown here. This structure shows a violation of the octet rule.

Which one of the following compounds utilizes both ionic and covalent bonding

A Lewis structure for SO3 that obeys the octet rule, showing all non-zero formal charges, is shown here. How many resonance structures for SO3 that obey the octet rule, are possible

Calculate the energy change for the reaction K(g) + Br(g) →\rarr→ K+(g) + Br- (g) Given the following ionization energy (IE) and electron affinity (EA) values. IE EA K: :419/ 48/ :1140/ 324/

Shown here is a Lewis structure for the chlorate ion, ClO3-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s). What is the formal charge on Cl

A polar covalent bond would form in which one of the following pairs of atoms

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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

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

List all types of bonding present in the molecule S₈. I. ionic bond II. polar covalent bond III. nonpolar covalent bond

Calculate the energy change for the reaction K(g) + I(g) $\rarr$ K⁺(g) + I ^- (g) Given the following ionization energy (IE) and electron affinity (EA) values. IE EA K: 419/ 48/ I: 1,010/ 295/

Which response includes all the molecules below that do not follow the octet rule (1) H₂S (2) BCl₃ (3) PH₃ (4) SF₄

Classify the Ca - Cl bond in CaCl₂ as ionic, polar covalent, or nonpolar covalent.

The Lewis structure for the nitrate ion, NO₃^-, showing all non-zero formal charges is shown here. This structure shows a violation of the octet rule.

A Lewis structure for SO₃ that obeys the octet rule, showing all non-zero formal charges, is shown here. How many resonance structures for SO₃ that obey the octet rule, are possible

Calculate the energy change for the reaction K(g) + Br(g) $\rarr$ K⁺(g) + Br^- (g) Given the following ionization energy (IE) and electron affinity (EA) values. IE EA K: :419/ 48/ :1140/ 324/

Shown here is a Lewis structure for the chlorate ion, ClO₃^-, that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s). What is the formal charge on Cl