The molecule that has greater dipole moment among SO 3 and SO 2 is to be identified. Concept introduction: The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom. The direction of the dipole moment is represented as follows: The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

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Answer 1

Question

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

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Answer 2

Question

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

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Answer 3

Question

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

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See solution

Answer 4

Question

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

Expert Solution & Answer

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Answer 5

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

Answer 6

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

Answer 7

Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

ΔEN=(electronegativity of B)−(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 10.1 - Write a Lewis structure for H2S; ; SOCl2. Ch. 10.1 - Prob. 10.1BFP Ch. 10.1 - Prob. 10.2AFP Ch. 10.1 - Prob. 10.2BFP Ch. 10.1 - Prob. 10.3AFP Ch. 10.1 - Prob. 10.3BFP Ch. 10.1 - Prob. 10.4AFP Ch. 10.1 - Prob. 10.4BFP Ch. 10.1 - Write a Lewis structure with minimal formal...Ch. 10.1 - Prob. 10.5BFP

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