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.

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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.

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1. This experiment is more about understanding the colligative properties of a solution rather than the determination of the molar mass of a solid. a. Define colligative properties. b. Which of the following solutes has the greatest effect on the colligative properties for a given mass of pure water? Explain. (i) 0.01 mol of CaCl2 (ii) 0.01 mol of KNO3 (iii) 0.01 mol of CO(NH2)2 (an electrolyte) (an electrolyte) (a nonelectrolyte)

5. b. For Trials 2 and 3, the molar mass of the solute was 151 g/mol and 143 g/mol respectively. a. What is the average molar mass of the solute ? b. What are the standard deviation and the relative standard deviation (%RSD) for the molar mass of the solute ?

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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.

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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

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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

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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

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Answer 13

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Answer 14

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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.

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