Lewis Structures and Formal Charges

The video tutorial explains the Lewis structure of H3PO4, Phosphoric Acid. It begins by identifying the total valence electrons and arranging the atoms with Phosphorus at the center. The tutorial discusses the formation of OH groups and the use of valence electrons to achieve full outer shells for each atom. It emphasizes the importance of formal charges and demonstrates how to adjust them by forming a double bond between Phosphorus and Oxygen. The final structure is presented with optimal formal charges, making it the most plausible Lewis structure for H3PO4.

What is the total number of valence electrons in H3PO4?

• 28

• 30

• 32

• 34

Where are the hydrogen atoms typically attached in the structure of H3PO4?

• To the oxygen atoms forming OH groups

• To the sulfur atom

• To the phosphorus atom

• To the nitrogen atom

How many valence electrons are used to form chemical bonds in H3PO4?

• 24

• 32

• 40

• 14

What is the formal charge on phosphorus before adjusting the Lewis structure?

• +1

• 0

• -1

• +2

Which element in H3PO4 can have an expanded octet?

• Hydrogen

• Oxygen

• Phosphorus

• Nitrogen

What is the formal charge on the oxygen atom before forming a double bond with phosphorus?

• 0

• -1

• +1

• -2

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

• Adding more valence electrons

• Forming a double bond between oxygen and phosphorus

• Removing an oxygen atom

• Adding more hydrogen atoms

What is the most plausible Lewis structure for H3PO4 based on formal charges?

• One with no bonds

• One with a double bond between phosphorus and one oxygen

• One with all single bonds

• One with a triple bond between phosphorus and one oxygen