Xenon Fluoride Structure and Properties

Dr. B explains how to draw the Lewis structure for XeF2. Starting with the calculation of valence electrons, he places Xenon at the center and Fluorines on the outside. He forms bonds and discusses the possibility of double bonds, considering Fluorine's electronegativity and Xenon's ability to hold more than 8 electrons. He then calculates formal charges to confirm the structure's validity, concluding that the formal charges are zero, making it the best structure for XeF2.

How many valence electrons does Xenon have?

• 8

• 7

• 9

• 6

What is the total number of valence electrons in XeF2?

• 22

• 20

• 26

• 24

Why is Xenon placed at the center of the XeF2 structure?

• It has the highest atomic number

• It forms the most bonds

• It is the most electronegative

• It is the least electronegative

How many valence electrons are left after initial bond formation in XeF2?

• 4

• 2

• 0

• 6

Why is a double bond not formed with Fluorine in XeF2?

• Fluorine prefers triple bonds

• Fluorine has no available orbitals

• Fluorine is too large

• Fluorine is very electronegative

How many nonbonding electrons does Fluorine have in the XeF2 structure?

• 7

• 4

• 5

• 6

What is the formal charge on Xenon in the XeF2 structure?

• 0

• -1

• +2

• +1

What is the best Lewis structure for XeF2 based on formal charges?

• Xenon has a negative charge

• Fluorine has a negative charge

• Xenon has a positive charge

• All formal charges are zero