Valence Electrons and Formal Charges in SeO2

Dr. B explains how to draw the Lewis structure for SeO2. Starting with the valence electrons, he places selenium in the center with oxygen atoms on either side. Initial electron distribution is adjusted to satisfy the octet rule. Formal charges are calculated to ensure the best structure, leading to the addition of a double bond to optimize the structure. The final structure has zero formal charges, indicating it is the most stable configuration.

How many valence electrons does Selenium have in the SeO2 molecule?

• 10

• 6

• 8

• 4

What is the total number of valence electrons in the SeO2 molecule?

• 12

• 16

• 18

• 20

Where is Selenium placed in the initial Lewis structure of SeO2?

• On the left

• Above the Oxygens

• On the right

• In the center

What adjustment is made to achieve the octet rule for Selenium in SeO2?

• Remove electrons from Oxygen

• Add a new Oxygen atom

• Add more electrons to Selenium

• Move electrons from outside to the center

What is the formal charge of Selenium in the initial structure of SeO2?

• +1

• +2

• 0

• -1

What is the formal charge of the Oxygen atom with 6 nonbonding electrons in the initial structure?

• +1

• 0

• -1

• -2

What change is made to the SeO2 structure to achieve zero formal charges?

• Add a single bond

• Add a double bond

• Remove a bond

• Add an extra electron

What is the formal charge of each atom in the revised SeO2 structure?

• +2

• -1

• 0

• +1

Why is the revised structure considered the best Lewis structure for SeO2?

• It has the most bonds

• It has zero formal charges

• It uses the least electrons

• It has the most electrons