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

Write the line-angle formula for the organic compounds (a) propene; (b) heptan-1-ol;(c) chloroacetic acid; (d) hexanoic acid.

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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Write the line-angle formula for the organic compounds (a) propene; (b) heptan-1-ol;(c) chloroacetic acid; (d) hexanoic acid.

What kind of hybridization do you expect for each carbon atom in the following molecules? (a) Propane, CH3CH2CH3 (b) 2-Methylpropene, (c) But-l-en-3-yne, H2C=CHa€"Ca%ojCH (d) Acetic acid,

Name or write the condensed structural formula for the fol- lowing compounds: (a) trans-2-pentene (b) 2,5-dimethyl-4-octene (c) CH3 CH;CHCH,CH3 C=C `H. CH;CH2, H СООН H CH3 CH CH3 CH3 `CH2 (d)

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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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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