The stability of a solid depends upon the heat of formation of the compound. Concept introduction: Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path. The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes. Process Energy M ( s ) = M ( g ) Heat of Sublimation (+)S M ( g ) = M + ( g ) Ionization Energy (+)I 1 2 X 2 ( g ) = X ( g ) Heat of dissociation (+) 1 2 D X ( g ) = X − ( g ) Electron Affinity (-)E.A. M + ( g ) + X − ( g ) = M X ( s ) Lattice Energy (-)U M ( s ) + 1 2 X 2 ( g ) = M X ( s ) Heat of Formation (-) Δ H f The algebraic sum of the energy terms should be equal to the heat of formation ( Δ H f ) of MX. As heat is actually involved in the reaction, Δ H f will be negative. So, ( − ) Δ H f = ( + ) S + ( + ) I + ( + ) 1 2 D − E . A . − U The lattice energy can be calculated as- U = S + I + 1 2 D − E . A . + Δ H f . Given: i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole. ii) The 1 s t Ionisation energy (I.E.1) of Cs (g) to C s + ( g ) = (+) 375.7kJ/mole. iii) The 2 n d ionisation energy (I. E. 2) of Cs (g) to C s 2 + ( g ) = (+) 2422 kJ/mole. iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole. v) Bond dissociation energy of F 2 ( g ) toF(g) is (+)158kJ/mole. vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole. vii) The lattice energy ( U 1 ) of C s F 2 ( s ) is (+) 2347 kJ/mole. To determine: i) The overall energy change in kilo Joules per mole for the formation of C s F 2 ( s ) . ii) The energy absorb or release in the process. iii) The compound is more likely to form CsF (s) or C s F 2 ( s ) .

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Answer 1

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Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

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Answer 2

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

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Answer 3

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

Expert Solution & Answer

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Answer 4

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

Answer 6

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

Answer 7

Chapter 6, Problem 6.81SP

Interpretation Introduction

Interpretation:

The stability of a solid depends upon the heat of formation of the compound.

Concept introduction:

Born-Haber Cycle: It is a thermodynamic cycle correlating the heat of formation of a compound with other thermochemical quantities; among these are included the energy terms involved in a various processes which may be carried on successively to form the same substance in a different path.
The construction of Born-Haber cycle may be illustrated with the reference to formation of an alkali halide (MX) from the elemental state. We consider the stepwise formation as represented by the following processes.

Process Energy

M(s)=M(g) Heat of Sublimation (+)S

M(g)=M+(g) Ionization Energy (+)I
12X2(g)=X(g) Heat of dissociation (+) 12D
X(g)=X−(g) Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s) Lattice Energy (-)U
M(s)+12X2(g)=MX(s) Heat of Formation (-) ΔHf

The algebraic sum of the energy terms should be equal to the heat of formation ( ΔHf ) of MX. As heat is actually involved in the reaction, ΔHf will be negative. So, (−)ΔHf=(+)S+(+)I+(+)12D−E.A.−U

The lattice energy can be calculated as-
U=S+I+12D−E.A.+ΔHf.

Given:

i) The electron affinity (E.A.) of F (g) = (-) 328 kJ/mole.
ii) The 1^s^t Ionisation energy (I.E.1) of Cs (g) to Cs+(g) = (+) 375.7kJ/mole.
iii) The 2ⁿ^d ionisation energy (I. E. 2) of Cs (g) to Cs2+(g) = (+) 2422 kJ/mole.
iv) Heat of sublimation (S) of Cs(s) to Cs (g) is (+) 76.1 kJ/mole.
v) Bond dissociation energy of F2(g) toF(g) is (+)158kJ/mole.
vi) The lattice energy (U) of CsF (s) is (+) 740kJ/mole.
vii) The lattice energy ( U1 ) of CsF2(s) is (+) 2347 kJ/mole.

To determine:

i) The overall energy change in kilo Joules per mole for the formation of CsF2(s).
ii) The energy absorb or release in the process.
iii) The compound is more likely to form CsF (s) or CsF2(s).

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 6 - Prob. 6.1P Ch. 6 - APPLY 6.2 Which of the following sets of ions are...Ch. 6 - Prob. 6.3P Ch. 6 - Conceptual APPLY 6.4 Which of the following...Ch. 6 - Prob. 6.5P Ch. 6 - Prob. 6.6A Ch. 6 - Prob. 6.7P Ch. 6 - Conceptual APPLY 6.8 The figure on the right...Ch. 6 - Prob. 6.9P Ch. 6 - Conceptual APPLY 6.10 Which of the indicated three...

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Chapter 6 Solutions

Process	Energy
M(s)=M(g)	Heat of Sublimation (+)S
M(g)=M+(g)	Ionization Energy (+)I
12X2(g)=X(g)	Heat of dissociation (+) 12D
X(g)=X−(g)	Electron Affinity (-)E.A.
M+(g)+X−(g)=MX(s)	Lattice Energy (-)U
M(s)+12X2(g)=MX(s)	Heat of Formation (-) ΔHf