Understanding the Lewis Structure of the Sulfate Ion

The video tutorial explains how to draw the Lewis structure of the sulfate ion (SO4 2-). It begins by calculating the total number of valence electrons, considering sulfur and oxygen atoms, and the ion's charge. The tutorial then discusses the ideal bonding arrangement to minimize formal charges, leading to the most stable Lewis structure. It also covers the concept of resonance structures, showing how different arrangements can exist with varying stability. The video concludes by identifying the most stable resonance form based on minimal formal charges.

How many valence electrons are present in the sulfate ion (SO4 2-)?

• 30

• 28

• 34

• 32

What is the ideal number of bonds sulfur should have in the sulfate ion to minimize formal charge?

• 5

• 6

• 4

• 7

What is the molecular geometry of the sulfate ion?

• Octahedral

• Tetrahedral

• Trigonal Planar

• Linear

What is the hybridization of the sulfur atom in the sulfate ion?

• sp3d

• sp3

• sp2

• sp

What happens to the formal charge of oxygen when it forms two bonds in the sulfate ion?

• It becomes +1

• It becomes -1

• It becomes neutral

• It becomes +2

How can resonance structures of the sulfate ion be generated?

• By removing oxygen atoms

• By moving lone pairs to form pi bonds

• By adding more electrons

• By changing the central atom

Which resonance structure of the sulfate ion is the most stable?

• The one with three negative charges on oxygen

• The one with sulfur having a formal charge of zero

• The one with maximum formal charges

• The one with sulfur having a +2 charge

Why is a neutral particle more stable than a charged particle?

• Because it has more bonds

• Because it is less reactive

• Because it has a higher energy level

• Because it has more electrons

What is the formal charge on sulfur in the most stable Lewis structure of sulfate?

• 0

• -1

• +1

• +2

What is the net charge of the sulfate ion?

• -1

• -2

• 0

• +1