Bromine and Fluorine Bonding Concepts

The video tutorial explains how to draw the Lewis structure for BrF2. Bromine and Fluorine's valence electrons are calculated, resulting in an odd number, indicating an unpaired electron. Bromine is placed in the center with Fluorines on either side, forming bonds and completing octets. Bromine, being in period 3, can hold more than eight electrons, allowing for the placement of the remaining electron. The formal charges are checked, confirming the structure's validity.

How many valence electrons does Bromine contribute in the BrF2 molecule?

• 6

• 7

• 5

• 8

What is the total number of valence electrons in BrF2?

• 18

• 19

• 20

• 21

Why is one electron unpaired in the Lewis structure of BrF2?

• Due to the high electronegativity of Bromine

• Because of an odd number of valence electrons

• Due to the presence of a lone pair on Fluorine

• Because of an even number of valence electrons

How many electrons are used to form chemical bonds between Bromine and Fluorine in BrF2?

• 4

• 2

• 6

• 8

What is the significance of Bromine being in period 3 of the periodic table?

• It forms ionic bonds with Fluorine

• It has a higher electronegativity than Fluorine

• It can hold more than 8 valence electrons

• It can only hold 8 valence electrons

What is the formal charge on each atom in the BrF2 molecule?

• +2

• 0

• -1

• +1