The Lewis structures for acetone have to be drawn. Concept introduction: Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Question

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Answer 1

Question

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

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Answer 2

Question

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Answer 6

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer 7

Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

Count the number of valence electron pairs (bond pairs and lone pairs).

Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

If there are only two bond pair electrons, the molecule is linear.

If there are three bond pair electrons, the molecule is shaped like a trigonal planar.

If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.

Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

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Answer 15

Ch. 4.1 - Prob. 4.1P Ch. 4.2 - Prob. 4.2P Ch. 4.2 - Prob. 4.3P Ch. 4.3 - Prob. 4.4P Ch. 4.3 - Prob. 4.5P Ch. 4.4 - The BF3 molecule can also react with NH3 by...Ch. 4.5 - Prob. 4.7P Ch. 4.7 - Prob. 4.8P Ch. 4.7 - Add lone pairs where appropriate to the following...Ch. 4.7 - Prob. 4.10P

The Lewis structures for acetone have to be drawn. Concept introduction: Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Solution Summary: The author explains that Lewis structures represent the bonding between atoms of a molecule and the lone pairs of electrons.

Concept explainers

Videos

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Want to see the full answer?

Chapter 4 Solutions

The Lewis structures for acetone have to be drawn. Concept introduction: Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Solution Summary: The author explains that Lewis structures represent the bonding between atoms of a molecule and the lone pairs of electrons.

Concept explainers

Videos

Interpretation: The Lewis structures for acetone have to be drawn. Concept introduction: Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Interpretation: The polar bonds in the Lewis structures of acetone have to be determined. Concept introduction: Covalent bonds are formed by sharing of electrons between atoms. The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.

Want to see the full answer?

Chapter 4 Solutions

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.