a) Propane, CH 3 CH 2 CH 3 . Interpretation: The hybridization expected for each carbon atom in propane, CH 3 CH 2 CH 3 is to be stated. Concept introduction: Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp 3 hybridized state can form four single bonds. A carbon in sp 2 hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Question

C5H8 has two elements of unsaturation (right?), which may indicate the presence of either double bonds or triple bonds or rings. Show all the possible structures

Answer 1

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Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

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Answer 2

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Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

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Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

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Answer 4

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Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

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Answer 6

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Answer 7

Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 8

Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 9

Chapter 1.SE, Problem 36AP

Interpretation Introduction

a) Propane, CH₃CH₂CH₃.

Interpretation:

The hybridization expected for each carbon atom in propane, CH₃CH₂CH₃ is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 10

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 11

Interpretation Introduction

b) 2- Methyl propene.

Interpretation:

The hybridization expected for each carbon atom in 2- methyl propene is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 12

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 13

Interpretation Introduction

c) But-1-ene-3-yne.

Interpretation:

The hybridization expected for each carbon atom in but-1-ene-3-yne is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 14

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

Answer 15

Interpretation Introduction

d) Acetic acid.

Interpretation:

The hybridization expected for each carbon atom in acetic acid is to be stated.

Concept introduction:

Carbon uses hybridized orbitals for forming bonds with other atoms. A carbon in sp³ hybridized state can form four single bonds. A carbon in sp² hybridized state can form a double bond and two single bonds. A carbon in sp hybridized state can form a triple bond and a single bond or two double bonds with its neighboring atoms.

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Ch. 1.3 - Give the ground-state electron configuration for...Ch. 1.3 - How many electrons does each of the following...Ch. 1.4 - Prob. 3P Ch. 1.4 - Convert the following representation of ethane,...Ch. 1.4 - What are likely formulas for the following...Ch. 1.4 - Prob. 6P Ch. 1.4 - Prob. 7P Ch. 1.7 - Draw a line-bond structure for propane, CH3CH2CH3....Ch. 1.7 - Convert the following molecular model of hexane, a...Ch. 1.8 - Draw a line-bond structure for propene, CH3CH=CH2....

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