×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide
Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide

Solved: Use Lewis symbols to determine the formula for the

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro ISBN: 9780321809247 1

Solution for problem 42E Chapter 9

Chemistry: A Molecular Approach | 3rd Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Chemistry: A Molecular Approach | 3rd Edition

4 5 1 288 Reviews
29
4
Problem 42E

Use Lewis symbols to determine the formula for the compound that forms between each pair of elements:

a. Ca and N

b. Mg and I

c. Ca and S

d. Cs and F

Step-by-Step Solution:

Solution 42 E Step 1 of 4 Couple a) Calcium (Ca) belongs to II A group, thus it has two electrons in its outer shell Nitrogen (N) belongs to V A group thus it has five electrons in its outer shell. Because of the Nitrogen’s high electronegativity respect to Calcium, Nitrogen can gain two electrons from Calcium. In order to reach their stability, Calcium can give two electrons to Nitrogen, but Nitrogen needs only three electrons to complete its outer shell. So we have to think in a different way respect to other times. If we look to the picture above, we can see that Calcium has two unpaired electrons, while Nitrogen has three unpaired electrons. So the better is to consider that the atoms mix together in a reverse ratio respect to their unpaired electrons. In this case, since the ratio between the Calcium’s unpaired electrons and Nitrogen unpaired electrons is 2:3, we need to combine Ca end N in a 3:2 ratio, thus obtaining the formula Ca O . 3 2 Calcium turns to be a positive, bivalent, ion (because every atom of Calcium loses two electrons) Nitrogen becomes a negative, trivalent ion (because every atom of Nitrogen acquires two electrons). Thus the Lewis formula for the final compound is the one we see as a product of the reaction below Step 2 of 4 Couple b) Magnesium (Mg) belongs to II A group, thus it has two electrons in its outer shell Iodine (I) belongs to VII A group thus it has seven electrons in its outer shell. Because of the Iodine’s high electronegativity respect to Magnesium, Iodine can gain one electron from Magnesium. Unfortunately, when an atom of Iodine acquires an electron, it completes its outer shell. Magnesium, instead, when it loses a single electron doesn’t reach its stability because another electron still remains in the outer shell. That means that Magnesium needs to give its other electron to another Iodine atom. Thus Magnesium and Iodine combine together in a 1:2 ratio. The final formula will be MgI . 2 Magnesium turns to be a positive, bivalent, ion (because every atom of Magnesium loses two electrons), Iodine becomes a negative, monovalent ion (because it acquires one electron). Thus, the Lewis structure of the ionic compound is the one that form at the end of the reaction below as follows:

Step 3 of 4

Chapter 9, Problem 42E is Solved
Step 4 of 4

Textbook: Chemistry: A Molecular Approach
Edition: 3
Author: Nivaldo J. Tro
ISBN: 9780321809247

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

Solved: Use Lewis symbols to determine the formula for the

×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide
Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide
×
Reset your password