Lewis Structures and Valence Electrons

Dr. B explains the process of constructing the Lewis structure for XeO4. Starting with the periodic table, he calculates the valence electrons for Xenon and oxygen, arranging them to form bonds. Initially, the structure seems correct, but formal charge calculations reveal it is not optimal. Adjustments are made by introducing double bonds, leading to a more stable structure with zero formal charges, confirming it as the best Lewis structure for XeO4.

How many valence electrons does Xenon have in the XeO4 molecule?

• 12

• 6

• 8

• 10

What is the total number of valence electrons in XeO4?

• 24

• 28

• 32

• 36

What is the initial step in drawing the Lewis structure for XeO4?

• Draw double bonds

• Calculate formal charges

• Place Xenon in the center

• Place Oxygen in the center

Why is it important to check formal charges in a Lewis structure?

• To verify the octet rule

• To confirm the structure's stability

• To ensure the structure is colorful

• To count the number of atoms

What formal charge does Xenon initially have in the first Lewis structure attempt?

• -1

• 0

• +2

• +4

What adjustment is made to the Lewis structure to improve formal charges?

• Add more electrons

• Introduce double bonds

• Remove an oxygen atom

• Change the central atom

How many double bonds are introduced in the revised Lewis structure of XeO4?

• 1

• 2

• 3

• 4

What is the formal charge on each oxygen atom in the final Lewis structure?

• +1

• 0

• -1

• +2

What indicates that the final Lewis structure is the best representation?

• All atoms have a formal charge of zero

• Xenon has a positive charge

• Oxygen atoms have a negative charge

• The structure is symmetrical

What was the main issue with the initial Lewis structure attempt?

• Wrong central atom

• Incorrect number of electrons

• Unbalanced formal charges

• Too many double bonds