The more stable base between B r − and I − has to be identified. Concept introduction: If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base. If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid. Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

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Answer 1

Question

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

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Answer 2

Question

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

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Answer 3

Question

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

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Answer 4

Question

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

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Answer 5

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

Answer 6

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

Answer 7

Chapter 2, Problem 10P

(a)

Interpretation Introduction

Interpretation:

The more stable base between Br− and I− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The more stable base between CH3O− and CH3S− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Size affecting the stability of the base: In order to determine the strength of the base, the size of an atom overrides electronegativity. As the atoms get larger and the stability of the anions increases even though the electronegativity of the atoms decreases. Stability of the bases increases going down the group. Stable bases are weak bases.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The more stable base between CH3CH2O- and CH3COO- has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Effect of electron delocalization: if a base has localized electrons, then the negative charge that results when the base’s conjugate acid loses a proton will belong to one atom.

A base with delocalized electron is more stable than a similar base with localized electrons.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The more stable base between H2C=C−H and HC≡C− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Hybridization: Electronegativity depends on the acidity of a species. Order of electronegativity of hybridization is sp> sp2 > sp3 so sp3 hybridized molecule is weak acid.

Answer 14

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

Answer 15

(e)

Interpretation Introduction

Interpretation:

The more stable base between FCH2CH2COO− and BrCH2CH2COO− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

Answer 16

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

Answer 17

(f)

Interpretation Introduction

Interpretation:

The more stable base between ClCH2CH2O− and ClCHCH2O− has to be identified.

Concept introduction:

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.

Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.

Effect of Inductive electron withdrawal on Acidity: Replacing a Hydrogen with an electronegative substituent pulls bonding electrons toward itself; increases the strength of the acid.

Answer 18

Expert Solution & Answer

Answer 19

Expert Solution & Answer

Answer 20

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Answer 21

Ch. 2.1 - Which of the following are not acids? CH3COOH CO2...Ch. 2.1 - Draw the products of the acidbase reaction when a....Ch. 2.1 - a.What is the conjugate acid of each of the...Ch. 2.2 - a. Which is a stronger acid, one with a pKa of 5.2...Ch. 2.2 - Prob. 5P Ch. 2.2 - Antacids are compounds that neutralize stomach...Ch. 2.2 - Are the following body fluids acidic or basic? a....Ch. 2.3 - Draw the conjugate acid of each of the following:...Ch. 2.3 - a. Write an equation showing CH3OH reacting as an...Ch. 2.3 - Prob. 10P

Solution Summary: The author explains that the more stable base between Br- and I€ has to be identified. Stability of the bases increases going down the group.

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Chapter 2 Solutions

Solution Summary: The author explains that the more stable base between Br- and I­€ has to be identified. Stability of the bases increases going down the group.

Concept explainers

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Chapter 2 Solutions

Solution Summary: The author explains that the more stable base between Br- and I€ has to be identified. Stability of the bases increases going down the group.