The total number of lone pairs in NCl3 is

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

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

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

What is total number of lone pairs in the best Lewis structure for SOF4 that exceeds the octet rule (S is the central atom)?

A) 0 B) 2 C) 14 D) 16 E) 18 A) 0 B) 2 C) 14 D) 16 E) 18

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

Exam 9: Chemical Bonding I: Basic Concepts

Write a Lewis structure for the phosphate ion, PO₄^3-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for PO₄^3- that obey the octet rule.

(Essay)

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Question 101

The total number of lone pairs in NCl₃ is

(Multiple Choice)

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Question 102

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

(Multiple Choice)

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Question 103

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

(Multiple Choice)

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Question 104

Which of the bonds below would have the greatest polarity (i.e., highest percent ionic character)?

(Multiple Choice)

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Question 105

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

(Essay)

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Question 106

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

(Multiple Choice)

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Question 107

Write a Lewis structure for the chlorite ion, ClO₂^-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO₂^- that obey the octet rule.

(Essay)

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Question 108

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

(Multiple Choice)

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Question 109

For which of these species does the best Lewis structure have two or more equivalent resonance structures?

(Multiple Choice)

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Question 110

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25°C. BE(N $\equiv$ N)= 941.4 kJ/mol BE(H-H)= 436.4 kJ/mol BE(N-H)= 393 kJ/mol

(Multiple Choice)

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Question 111

What is total number of lone pairs in the best Lewis structure for SOF₄ that exceeds the octet rule (S is the central atom)?

(Multiple Choice)

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Question 112

The total number of valence electrons in the ion NH₄⁺ is

(Multiple Choice)

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Question 113

Dichloromethane, CH₂Cl₂, is an important solvent in synthetic chemistry.Write a Lewis structure for CH₂Cl₂.

(Essay)

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Question 114

Write a Lewis structure for the chlorate ion, ClO₃^-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO₃^- that obey the octet rule.

(Essay)

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Question 115

Which one of the following molecules has an atom with an expanded octet?

(Multiple Choice)

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Question 116

Use the Born-Haber cycle to calculate the standard enthalpy of formation ( $\Delta$ H $Use the Born-Haber cycle to calculate the standard enthalpy of formation ( \Delta H <sub> </sub> )for LiCl(s)given the following data: \Delta H(sublimation)Li = 155.2 kJ/mol I<sub>1</sub> (Li)= 520 kJ/mol Bond energy (Cl-Cl)= 242.7 kJ/mol EA (Cl)= 349 kJ/mol Lattice energy (LiCl(s))= 828 kJ/mol$ )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 117

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

(Multiple Choice)

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Question 118

Use the bond enthalpy data given to estimate the heat released when 25.0 g of acetylene gas, C₂H₂, burns in excess oxygen to yield carbon dioxide and water vapor at 25°C. BE(C-C)= 347 kJ/mol BE(C=C)= 812 kJ/mol BE(C=O in CO₂)= 799 kJ/mol BE(C-H)= 414 kJ/mol BE(O-H)= 460 kJ/mol BE(O=O)= 498.7 kJ/mol

(Multiple Choice)

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Question 119

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

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Question 120

Showing 101 - 120 of 137

Exam 9: Chemical Bonding I: Basic Concepts

Write a Lewis structure for the phosphate ion, PO43-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for PO43- that obey the octet rule.

The total number of lone pairs in NCl3 is

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

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

Which of the bonds below would have the greatest polarity (i.e., highest percent ionic character)?

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

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

Write a Lewis structure for the chlorite ion, ClO2-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO2- that obey the octet rule.

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

For which of these species does the best Lewis structure have two or more equivalent resonance structures?

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25°C. BE(N ≡\equiv≡ N)= 941.4 kJ/mol BE(H-H)= 436.4 kJ/mol BE(N-H)= 393 kJ/mol

What is total number of lone pairs in the best Lewis structure for SOF4 that exceeds the octet rule (S is the central atom)?

The total number of valence electrons in the ion NH4+ is

Dichloromethane, CH2Cl2, is an important solvent in synthetic chemistry.Write a Lewis structure for CH2Cl2.

Write a Lewis structure for the chlorate ion, ClO3-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO3- that obey the octet rule.

Which one of the following molecules has an atom with an expanded octet?

Use the Born-Haber cycle to calculate the standard enthalpy of formation ( Δ\DeltaΔ H )for LiCl(s)given the following data: Δ\DeltaΔ 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

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

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

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Write a Lewis structure for the phosphate ion, PO₄^3-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for PO₄^3- that obey the octet rule.

The total number of lone pairs in NCl₃ is

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

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

Write a Lewis structure for the chlorite ion, ClO₂^-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO₂^- that obey the octet rule.

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25°C. BE(N $\equiv$ N)= 941.4 kJ/mol BE(H-H)= 436.4 kJ/mol BE(N-H)= 393 kJ/mol

What is total number of lone pairs in the best Lewis structure for SOF₄ that exceeds the octet rule (S is the central atom)?

The total number of valence electrons in the ion NH₄⁺ is

Dichloromethane, CH₂Cl₂, is an important solvent in synthetic chemistry.Write a Lewis structure for CH₂Cl₂.

Write a Lewis structure for the chlorate ion, ClO₃^-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO₃^- that obey the octet rule.

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