Valence Electrons in XeCl4 Structure

The video tutorial explains the Lewis structure of XeCl4, starting with Xenon as the central atom surrounded by chlorine atoms. It discusses the total valence electrons available and how they are distributed to form chemical bonds and fill the octets of chlorine atoms. The tutorial highlights the issue of having extra valence electrons and resolves it by using Xenon's ability to have an expanded octet, accommodating more than eight electrons. The final structure is presented with all electrons accounted for, and the concept of expanded octets is emphasized.

Why is Xenon placed at the center of the XeCl4 Lewis structure?

• Because it is the most electronegative element.

• Because it is the least electronegative element.

• Because it has the highest atomic number.

• Because it forms the most bonds.

How many total valence electrons are there in the XeCl4 Lewis structure?

• 38

• 34

• 32

• 36

What is the initial step in distributing valence electrons in the XeCl4 structure?

• Distributing all electrons to Chlorine atoms first.

• Placing two electrons between each atom to form bonds.

• Leaving some electrons unpaired.

• Filling the octets of Xenon first.

What problem arises after initially distributing the valence electrons in XeCl4?

• There are not enough electrons to fill the octets.

• There are extra electrons left over.

• The electrons are not evenly distributed.

• The structure is unstable.

Why can Xenon hold more than eight valence electrons in its outer shell?

• Because it is below Period 2 and can have an expanded octet.

• Because it is highly reactive.

• Because it is a noble gas.

• Because it is in Period 1 of the periodic table.

How are the extra valence electrons accommodated in the XeCl4 structure?

• They are added to the Chlorine atoms.

• They are shared between all atoms.

• They are placed on the central Xenon atom.

• They are removed from the structure.

What is the final number of valence electrons around the Xenon atom in XeCl4?

• 14

• 10

• 8

• 12