   Chapter 14, Problem 134E

Chapter
Section
Textbook Problem

# Using your results from Exercise 133, place the species in each of the following groups in order of increasing base strength.a. OH−, SH−, SeH−b. NH3, PH3c. NH3, HONH2

(a)

Interpretation Introduction

Interpretation: Using the results from the exercise 133 , the species in the given groups are to be placed in the order of increasing base strength.

Concept introduction: A species that does not easily release the H+ ions is considered to be less acidic as compared to the one that does.

The bond energy is inversely proportional to the bond length. The longer the bond, the more easily it breaks.

To determine: The correct order of increasing base strength.

Explanation

Explanation

The bond energy value for OH is 467kJ/mol .

The bond energy value for HS is 363kJ/mol .

The bond energy value for HSe is 276kJ/mol .

The correct increasing order according to bond energy value is,

OH>SH>SeH

The bond length is inversely proportional to bond energy

(b)

Interpretation Introduction

Interpretation: Using the results from the exercise 133 , the species in the given groups are to be placed in the order of increasing base strength.

Concept introduction: A species that does not easily release the H+ ions is considered to be less acidic as compared to the one that does.

The bond energy is inversely proportional to the bond length. The longer the bond, the more easily it breaks.

To determine: The correct order of increasing base strength.

(c)

Interpretation Introduction

Interpretation: Using the results from the exercise 133 , the species in the given groups are to be placed in the order of increasing base strength.

Concept introduction: A species that does not easily release the H+ ions is considered to be less acidic as compared to the one that does.

The bond energy is inversely proportional to the bond length. The longer the bond, the more easily it breaks.

To determine: The correct order of increasing base strength.

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