Formal Charge and Valence Electrons

The video tutorial explains how to determine the formal charge on each atom in SF6 by examining its Lewis structure. It highlights that sulfur can have an expanded octet due to its position in period 3. The tutorial then details the calculation of formal charges for both fluorine and sulfur atoms, confirming that the most favorable Lewis structure for SF6 has a formal charge of zero for each atom.

What is the first step in determining the formal charge of an atom in a molecule?

• Determine the molecular weight of the compound.

• Look at the correct Lewis structure.

• Identify the number of protons in the atom.

• Count the number of neutrons in the atom.

Why is sulfur able to have more than eight electrons in its valence shell in SF6?

• Sulfur has a high electronegativity.

• Sulfur is in period 2, which allows expanded octets.

• Sulfur is in period 3, which allows expanded octets.

• Sulfur is a noble gas.

How many valence electrons does fluorine have?

• Eight

• Seven

• Six

• Five

What is the formal charge on a fluorine atom in SF6?

• +1

• -1

• 0

• +2

How many unbonded valence electrons does each fluorine atom have in SF6?

• Six

• Four

• Eight

• Two

What is the group number for sulfur in the periodic table?

• Group 17 or 7A

• Group 14 or 4A

• Group 15 or 5A

• Group 16 or 6A

How many total bonded valence electrons are around the sulfur atom in SF6?

• 8

• 14

• 10

• 12

What is the formal charge on the sulfur atom in SF6?

• +2

• 0

• -1

• +1

Why is it favorable for the formal charges in SF6 to be zero?

• It shows that the molecule is an ion.

• It means the molecule is highly reactive.

• It suggests the molecule is unstable.

• It indicates a stable and likely structure.

What does a formal charge of zero on all atoms in a molecule suggest?

• The molecule is unstable.

• The molecule is an ion.

• The molecule has the most favorable Lewis structure.

• The molecule is highly reactive.