On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br

Question

Want to see more full solutions like this?

Answer 1

Textbook Question

Chapter 12, Problem 17QAP

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs.

msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br

Expert Solution

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Expert Solution

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

Predict the major products of the following organic reaction: + A ? Some important notes: • Draw the major product, or products, of the reaction in the drawing area below. • If there aren't any products, because no reaction will take place, check the box below the drawing area instead. • Be sure to use wedge and dash bonds when necessary, for example to distinguish between major products that are enantiomers. Explanation Check Click and drag to start drawing a structure. C © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cente

Polar solutes are most likely to dissolve into _____, and _____ are most likely to dissolve into nonpolar solvents. A. nonpolar solutes; polar solvents B. nonpolar solvents; polar solvents C. polar solvents; nonpolar solutes D. polar solutes; nonpolar solvents

Deducing the Peactants Can the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ? Δ If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. If your answer is no, check the box under the drawing area instead. Explanation Check Click and drag to start drawing a structure. © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center X

Answer 2

Textbook Question

Chapter 12, Problem 17QAP

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs.

msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br

Expert Solution

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Expert Solution

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Textbook Question

Chapter 12, Problem 17QAP

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs.

msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br

Expert Solution

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Expert Solution

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Textbook Question

Chapter 12, Problem 17QAP

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs.

msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br

Expert Solution

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Expert Solution

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Expert Solution

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.

Answer 8

Expert Solution

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

(a)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer 13

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.

Answer 14

Explanation of Solution

The given pair of bonds is H−F and H−Cl.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of fluorine is 4.0.

The difference in the electronegativity values for H−F bond is,

Difference in electronegativity for H−F bond=4.0−2.1=1.9

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.

Answer 15

Expert Solution

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Interpretation Introduction

(b)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer 20

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Answer 21

Explanation of Solution

The given pair of bonds is H−Cl and H−I.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of iodine is 2.5.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.

Answer 22

Expert Solution

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Answer 23

Expert Solution

Answer 24

Expert Solution

Answer 25

Expert Solution

Answer 26

Interpretation Introduction

(c)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer 27

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.

Answer 28

Explanation of Solution

The given pair of bonds is H−Cl and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of chlorine is 3.0.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Cl bond is,

Difference in electronegativity for H−Cl bond=3.0−2.1=0.9

The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.

The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.

Answer 29

Expert Solution

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.

Answer 30

Expert Solution

Answer 31

Expert Solution

Answer 32

Expert Solution

Answer 33

Interpretation Introduction

(d)

Interpretation:

On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.

Concept Introduction:

The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

Answer 34

Answer to Problem 17QAP

On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.

Answer 35

Explanation of Solution

The given pair of bonds is H−I and H−Br.

The electronegativity value of hydrogen is 2.1.

The electronegativity value of iodine is 2.5.

The electronegativity value of bromine is 2.8.

The difference in the electronegativity values for H−I bond is,

Difference in electronegativity for H−I bond=2.5−2.1=0.4

The difference in the electronegativity values for H−Br bond is,

Difference in electronegativity for H−Br bond=2.8−2.1=0.7

The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.

The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.