The observations that carbon tetrachloride ( CCl 4 ) is liquid and ammonia ( NH 3 ) is a gas at room temperature and pressure should be rationalized. Concept Introduction: Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out. Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each C − Cl bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound. Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each N − H bond. For this reason, ammonia is a polar covalent compound.

Question

Want to see the full answer?

Answer 1

Question

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 2

Question

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Answer 6

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Answer 7

Chapter 8, Problem 8.51PAE

Interpretation Introduction

Interpretation:

The observations that carbon tetrachloride $({CCl}_{4})$ is liquid and ammonia $({NH}_{3})$ is a gas at room temperature and pressure should be rationalized.

Concept Introduction:

Polar molecules have more boiling point due to partial ionic character between the ions. Net polarity is dependent on the structure of the molecule as, a molecule with atoms with electronegativity difference can be non-polar if all the dipole moments get cancelled out.

Carbon tetrachloride has a symmetrical tetrahedral structure in which the central carbon atom is attached to four chlorine atoms. Each $C - Cl$ bond has polarity, but the net polarity of the compound is cancelled due to the symmetrical structure of the compound. For this reason, carbon tetrachloride is a non-polar covalent compound.

Ammonia has a trigonal pyramidal structure in which the central nitrogen atom is attached to three hydrogen atoms. The molecule shows a net polarity, due to the polarity of each $N - H$ bond. For this reason, ammonia is a polar covalent compound.

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 8 - Prob. 1CO Ch. 8 - • describe the arrangement of atoms in the common...Ch. 8 - • use bind theory to describe bonding in solids.Ch. 8 - Prob. 4CO Ch. 8 - Prob. 5CO Ch. 8 - Prob. 6CO Ch. 8 - Prob. 7CO Ch. 8 - • explain the connection between intermolecular...Ch. 8 - Prob. 9CO Ch. 8 - Prob. 10CO

Solution Summary: The author explains that carbon tetrachloride is liquid and ammonia is a gas at room temperature and pressure.

Videos

Want to see the full answer?

Chapter 8 Solutions