Valence Electrons and Formal Charges

The video tutorial explains how to determine the formal charges for the SBr2 molecule. It begins with the Lewis structure and uses equations to calculate the formal charges for sulfur and bromine atoms. Sulfur, with 6 valence electrons, has a formal charge of zero after accounting for non-bonding and bonding electrons. Similarly, bromine, with 7 valence electrons, also has a formal charge of zero. The tutorial concludes that the SBr2 structure is valid as all formal charges are zero.

What is the first step in determining the formal charges for a molecule like SBr2?

• Determine the oxidation states

• Calculate the molecular weight

• Draw the Lewis structure

• Identify the molecular geometry

How many valence electrons does sulfur have in the SBr2 molecule?

• 6

• 4

• 8

• 2

What is the formal charge on sulfur in the SBr2 molecule?

• 0

• -1

• +2

• +1

In which group of the periodic table is bromine found?

• Group 17

• Group 6

• Group 16

• Group 7

How many non-bonding valence electrons does bromine have in SBr2?

• 8

• 2

• 6

• 4

What is the formal charge on each bromine atom in SBr2?

• +2

• 0

• -1

• +1

Why is the Lewis structure for SBr2 considered a good structure?

• All formal charges are zero

• It has the lowest energy configuration

• It maximizes the number of bonds

• It has the highest symmetry