 # 2-91 These are the first two ionization energy for lithium: Li(g) → Li + (g) + e - (g) Ionization energy = 523 kJ/mol Li + (g) → Li 2 + (g) + e - (g) Ionization energy = 7298 kJ/mol (a) Explain the large increase in ionization energy that occurs for the removal of the second electron. (b) The radius of Li is 78 pm (1 pm = 10-12 m) while that of a lithium atom, Li, is 152 pm. Exp lain why the radius of Li is so much smaller than the radius of Li. ### Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759 ### Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759

#### Solutions

Chapter
Section
Chapter 2, Problem 2.91P
Textbook Problem
57 views

## 2-91 These are the first two ionization energy for lithium: Li(g) → Li+(g) + e-(g) Ionization energy = 523 kJ/mol Li+(g) → Li2+(g) + e-(g) Ionization energy = 7298 kJ/mol(a) Explain the large increase in ionization energy that occurs for the removal of the second electron.(b) The radius of Li is 78 pm (1 pm = 10-12 m) while that of a lithium atom, Li, is 152 pm. Exp lain why the radius of Li is so much smaller than the radius of Li.

Expert Solution
Interpretation Introduction

(a)

Interpretation:

The large increase in ionization energy that occurs for the removal of the second electron should be explained.

Concept Introduction:

Ionization energy is defined as the energy needed to remove an electron from the outermost shell of an atom or an ion.

### Explanation of Solution

Given Information:

The first two ionization energy (IE) for lithium are given as follows:

Li (g)Li+(g) + e-(g)                                      IE = 523 KJ/mol Li (g)Li2+(g) + e-(g)                                                                            IE = 7298 KJ/mol

The large increase in ionization energy for the removal of the second electron i

Expert Solution
Interpretation Introduction

(b)

The reason for the smaller radius of Li+ as compared to Li should be explained.

### Want to see the full answer?

Check out a sample textbook solution.See solution

### Want to see this answer and more?

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

See solution 