Valence Electrons and Lewis Structures

This video tutorial explains how to draw the Lewis structure for SO2Cl2. It begins by counting the valence electrons for sulfur, oxygen, and chlorine, totaling 32. The initial structure is constructed with sulfur in the center, surrounded by oxygen and chlorine atoms. The video then checks the formal charges, finding that adjustments are needed to achieve the most stable structure. By forming a double bond with oxygen, the formal charges are optimized to zero, resulting in the best Lewis structure. The video concludes by noting sulfur's exception to the octet rule.

How many total valence electrons are there in SO2Cl2?

• 28

• 30

• 34

• 32

Which atom is placed at the center of the SO2Cl2 Lewis structure?

• Hydrogen

• Sulfur

• Chlorine

• Oxygen

What is the first step in forming chemical bonds in the SO2Cl2 Lewis structure?

• Putting valence electrons between atoms

• Arranging atoms in a straight line

• Placing all electrons on sulfur

• Removing electrons from chlorine

How many valence electrons are used before completing the octets in SO2Cl2?

• 30

• 34

• 28

• 32

What is the formal charge on the chlorine atoms in the initial Lewis structure?

• 0

• +2

• +1

• -1

What adjustment is made to achieve zero formal charges on all atoms in SO2Cl2?

• Adding more electrons to sulfur

• Changing the central atom

• Forming a double bond with oxygen

• Removing electrons from chlorine

What is the formal charge on sulfur after adjusting the Lewis structure?

• -1

• +2

• 0

• +1

How many valence electrons does sulfur have in the final Lewis structure?

• 14

• 10

• 12

• 8

Which rule does sulfur violate in the final Lewis structure of SO2Cl2?

• Duet rule

• Pauli exclusion principle

• Hund's rule

• Octet rule

Why is it acceptable for sulfur to have more than eight valence electrons?

• It is a noble gas

• It is highly electronegative

• It is an exception to the octet rule

• It forms ionic bonds