Write the electron configurations of magnesium (z=12) and fluoride (z=9). Explain what electrons must be gained or lost from the atoms to form an electron configuration of a filled shell. Write the electron configuration of each ion too. Which noble gases have those electron configurations
Write the electron configurations of magnesium (z=12) and fluoride (z=9). Explain what electrons must be gained or lost from the atoms to form an electron configuration of a filled shell. Write the electron configuration of each ion too. Which noble gases have those electron configurations
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Write the electron configurations of magnesium (z=12) and fluoride (z=9). Explain what electrons must be gained or lost from the atoms to form an electron configuration of a filled shell. Write the electron configuration of each ion too. Which noble gases have those electron configurations?
Expert Solution
Step 1
Magnesium (z=12) electron configuration will be [Mg]= 1s22s22p63s2
Two electrons from 3s orbital must be a loss, to form an electron configuration of a filled shell.
After 2 electrons loss from 3s orbital, electron configuration will be
[Mg +2 ] = 1s22s22p6 (Neon noble gas electron configurations)
[Ne] = 1s22s22p6
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