Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic. Concept Introduction: The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule. If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature. The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Question

Want to see the full answer?

Answer 1

Question

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Organic bases have lone pairs of electrons that are capable of accepting protons. Lone pair electrons in a neutral or negatively charged species, or pi electron pairs. Explain the latter case (pi electron pairs).

Describe the propyl anion.

Indicate the names of these compounds (if they exist). 0: HỌC—NH CH3CH2-CH2

Answer 2

Question

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 6

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 7

Chapter 10.7, Problem 56PP

(a)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for O-H and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 9

(b)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for Na-O and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 10

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 11

(c)

Interpretation Introduction

Interpretation:

Interpret the electronegativity difference for C-Br and determine whether the bond is non polar, polar or ionic.

Concept Introduction:

The large difference in the electronegativity between the atoms of the molecule results in polar nature of the molecule.

If the difference in electronegativity is lower or approaching to 0 then the molecule will have non polar nature.

The range of non-polar bond is 0 to 0.4 while for polar covalent bond the range is 0.4 to 1.8 and for ionic bond the range is 1.8 to 3.3.

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

Ch. 10.1 - Determine the total number of valence electrons...Ch. 10.1 - Determine the total number of valence electrons...Ch. 10.1 - Prob. 3PP Ch. 10.1 - If the available number of valence electrons for a...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.2 - Prob. 9PP Ch. 10.2 - When does a molecular compound have resonance?

Solution Summary: The author analyzes the electronegativity difference for O-H and determines whether the bond is non-polar, polar or ionic.

Want to see the full answer?

Chapter 10 Solutions