Boron and BBr3 Chemistry Concepts

Dr. B explains how to draw the Lewis structure for BBr3. Boron, with 3 valence electrons, is placed in the center, surrounded by three Bromines, each with 7 valence electrons, totaling 24 valence electrons. Initial bonds are formed, and the possibility of double bonds is considered. However, Boron is stable with 6 electrons, so formal charges are calculated to confirm the structure. All formal charges are zero, confirming the correct structure without double bonds.

How many valence electrons does Boron have?

• 8

• 7

• 5

• 3

What is the total number of valence electrons in BBr3?

• 27

• 18

• 21

• 24

Why is Boron placed in the center of the BBr3 molecule?

• It is the least electronegative

• It has the most valence electrons

• It is the most electronegative

• It has the highest atomic number

What is the electron deficiency of Boron in BBr3?

• 4 electrons

• 6 electrons

• 2 electrons

• 8 electrons

Why is a double bond not formed between Boron and Bromine in BBr3?

• Bromine is too electronegative

• Double bonds are unstable

• Boron cannot form double bonds

• There are not enough electrons

What is the formal charge on each Bromine atom in BBr3?

• +1

• 0

• -1

• +2

What is the formal charge on the Boron atom in BBr3?

• +1

• +2

• 0

• -1

What conclusion is drawn about the Lewis structure of BBr3?

• It requires double bonds

• It is incorrect

• It needs more electrons

• It is correct without double bonds

What is the significance of all formal charges being zero in BBr3?

• It indicates instability

• It confirms the structure is correct

• It shows an error in calculation

• It suggests a need for more bonds