Lewis Structures and Valence Electrons

This video tutorial explains how to draw the Lewis structure for the BRF2- ion. It begins by counting the valence electrons of bromine and fluorine, considering the extra electron due to the negative charge. Bromine, being less electronegative, is placed at the center with fluorine atoms on either side. The video demonstrates forming chemical bonds and completing the octet for each atom. It also discusses the concept of an expanded octet for bromine, allowing it to hold more than eight electrons. The tutorial concludes with finalizing the structure and indicating the ion's charge.

How many total valence electrons are present in the BrF2- ion?

• 23

• 20

• 21

• 22

Which atom is placed at the center of the Lewis structure for BrF2-?

• Oxygen

• Bromine

• Fluorine

• Hydrogen

How many valence electrons are used to form chemical bonds between bromine and fluorine in BrF2-?

• 4

• 8

• 2

• 6

What is the total number of valence electrons used after completing the octet for each atom in BrF2-?

• 16

• 18

• 22

• 20

What is the term used when bromine can hold more than 8 electrons in its valence shell?

• Octet rule

• Expanded octet

• Valence shell expansion

• Electron overflow

How many extra electrons are placed on bromine due to its expanded octet in BrF2-?

• 4

• 3

• 2

• 1

Why is it necessary to put brackets around the Lewis structure of BrF2-?

• To highlight the central atom

• To show it is an ion

• To indicate it is a molecule

• To emphasize the expanded octet

What charge is indicated on the BrF2- Lewis structure?

• Negative

• Double negative

• Neutral

• Positive

Which rule does fluorine strictly follow in the BrF2- Lewis structure?

• Octet rule

• Duet rule

• Triple bond rule

• Expanded octet

What is the significance of the negative sign in the BrF2- ion?

• It indicates a positive charge

• It signifies an extra electron

• It denotes a missing electron

• It shows an extra proton