Understanding Lewis Structures: Xenon Difluoride

The video tutorial explains how to construct a Lewis diagram for xenon difluoride. It begins by calculating the total valence electrons for xenon and fluorine, followed by drawing the structure with single covalent bonds. The tutorial then allocates valence electrons to achieve a full octet for the fluorine atoms. Finally, it discusses the exception to the octet rule, where xenon has more than eight valence electrons, which is possible for elements in the third or higher period.

What is the first step in constructing a Lewis diagram for a molecule?

• Allocate electrons to achieve full octets

• Count the total number of valence electrons

• Draw single covalent bonds

• Identify the central atom

How many valence electrons does xenon have?

• 6

• 7

• 8

• 9

How many valence electrons are there in total for xenon difluoride?

• 20

• 22

• 26

• 24

Why is xenon chosen as the central atom in xenon difluoride?

• It has fewer valence electrons

• It is less electronegative than fluorine

• It is more electronegative than fluorine

• It is a metal

How many valence electrons are used in the initial single covalent bonds?

• 2

• 4

• 6

• 8

How many additional electrons are needed for each fluorine to achieve a full octet?

• 8

• 4

• 2

• 6

Where are the remaining valence electrons allocated after the terminal atoms?

• On the central atom

• On the terminal atoms

• They are not used

• In the bonds

How many valence electrons does xenon have in the final structure of xenon difluoride?

• 8

• 12

• 14

• 10

What is an exception to the octet rule demonstrated by xenon in xenon difluoride?

• It has fewer than 8 electrons

• It has exactly 8 electrons

• It has more than 8 electrons

• It forms ionic bonds

Which period elements can have more than 8 valence electrons?

• Third period or higher

• Only noble gases

• Second period

• First period