Formal Charge and Electron Placement in I3-

The video tutorial explains how to calculate the formal charge for each iodine in the I3- Lewis structure. It begins by identifying the total valence electrons and the need to add extra electrons. The tutorial demonstrates calculating the formal charge for each iodine atom, emphasizing the importance of placing extra electrons on the central iodine to achieve a stable structure. It also explores the consequences of alternative electron placements, highlighting the optimal configuration for minimizing formal charges.

What is the total number of valence electrons in the I3- Lewis structure?

• 20

• 26

• 22

• 24

Where are the extra valence electrons initially placed in the I3- structure?

• On the central iodine

• On one of the outer iodines

• Not placed at all

• Distributed equally among all iodines

How many unbonded electrons does the central iodine have in the I3- structure?

• 4

• 2

• 6

• 8

What is the formal charge of the central iodine in the I3- structure?

• +1

• 0

• -1

• -2

What is the formal charge of the outer iodines in the I3- structure?

• +1

• 0

• -2

• -1

Why does the central iodine have a negative charge in the I3- structure?

• It is an ion

• It has more protons

• It has more electrons

• It is bonded to more atoms

What happens to the formal charge if extra electrons are placed on an outer iodine?

• It becomes +1

• It becomes 0

• It becomes -1

• It becomes -2

Why is placing extra electrons on the central iodine preferred?

• It balances the structure

• It is more symmetrical

• It maximizes formal charges

• It minimizes formal charges

What group is iodine in on the periodic table?

• Group 18

• Group 17

• Group 16

• Group 15

What is the main takeaway regarding electron placement in I3-?

• Place electrons on outer iodines

• Do not add extra electrons

• Distribute electrons equally

• Place electrons on central iodine