Explanation Given: potassium and sulphur sodium and nitrogen aluminium and iodine gallium and oxygen An ion is formed when an atom loses or gain electron. The loss of electron forms a positive charge called cation and the gain of electron forms a negative charge called anion. Now we know that if there are eight electrons in the outermost orbit of an atom then it becomes stable like noble gases. So, atoms have a tendency to get eight electrons in its outermost orbit and becomes stable. In order to get eight electron, they either loses or gain electron thus forming ions. Ionic compounds are the combination of cation and anion. In order to form an ionic-bond we must neutralize the charges between the cation and anion. a. Potassium and Sulphur Here, the electronic configuration of potassium ( K ) is: K = 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 1 Now in order to get a stable configuration, it will lose one electron from its s − subshell forming K + ; K + = 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 Thus, the symbol for potassium ion is K + Again, the electronic configuration for sulphur ( S ) is S = 1 s 2 2 s 2 2 p 6 3 s 2 3 p 4 Now in order to attain a stable configuration it will gain two electrons in its p − subshell forming S 2 − ; S 2 − = 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 Thus, the symbol for sulphur ion is S 2 − Now, K + has + 1 charge and S 2 − has − 2 charge, so in order to neutralize we need two K + ion having + 1 charge each to combine to S 2 − having − 2 charge thus formed ionic compound is K 2 S b. Sodium and Nitrogen The electronic configuration of sodium ( N a ) is: N a = 1 s 2 2 s 2 2 p 6 3 s 1 In order to attain a stable configuration, it will lose one electron from its s − subshell forming N a + ; N a + = 1 s 2 2 s 2 2 p 6 Thus, the symbol for sodium ion is N a + Again, the electronic configuration for nitrogen ( N ) is N = 1 s 2 2 s 2 2 p 3 In order to get a stable configuration, it will gain three electrons in its p − subshell forming N 3 − ; N 3 − = 1 s 2 2 s 2 2 p 6 Thus, the symbol for nitrogen ion is N 3 − Now N a + has + 1 charge and N 3 − has − 3 charge, so in order to neutralize each other we need three N a + ion having + 1 charge each to combine with N 3 − having − 3 charge thus formed ionic compound is N a N 3 c...

General, Organic, and Biological Chemistry: Structures of Life (5th Edition)

5th Edition

ISBN: 9780321967466

Author: Karen C. Timberlake

Publisher: PEARSON

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Chapter 6.2, Problem 6.15QAP

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The symbols for the ions and the correct formula for the ionic compounds formed.

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Chapter 6.2, Problem 6.14QAP

Chapter 6.2, Problem 6.16QAP

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Chapter 6 Solutions

General, Organic, and Biological Chemistry: Structures of Life (5th Edition)

Ch. 6.1 - State the number of electrons that must be lost by...Ch. 6.1 - Prob. 6.2QAP Ch. 6.1 - State the number of electrons lost or gained when...Ch. 6.1 - State the number of electrons lost or gained when...Ch. 6.1 - Prob. 6.5QAP Ch. 6.1 - Prob. 6.6QAP Ch. 6.1 - Prob. 6.7QAP Ch. 6.1 - Prob. 6.8QAP Ch. 6.1 - Prob. 6.9QAP Ch. 6.1 - Prob. 6.10QAP

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The symbols for the ions and the correct formula for the ionic compounds formed.

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To determine: The symbols for the ions and the correct formula for the ionic compounds formed.

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Chapter 6 Solutions

To determine:

The symbols for the ions and the correct formula for the ionic compounds formed.