Formal Charges and Valence Electrons

The video tutorial explains how to calculate the formal charge of each element in the C2H4 molecule, also known as ethene or ethylene, using the Lewis structure and a specific equation. It demonstrates the calculation for hydrogen and carbon atoms, showing that all formal charges in the molecule are zero, indicating stability.

What is the purpose of using Lewis structures in the context of formal charges?

• To predict the color of the compound

• To determine the molecular weight

• To find the formal charge on each element

• To calculate the boiling point

How many valence electrons does a hydrogen atom have?

• Two

• Four

• Three

• One

What is the formal charge on a hydrogen atom in C2H4?

• 0

• -1

• +2

• +1

Which group on the periodic table does carbon belong to?

• Group 1

• Group 14

• Group 18

• Group 7

How many valence electrons does carbon have?

• Six

• Eight

• Four

• Two

What is the formal charge on a carbon atom in C2H4?

• +1

• -1

• 0

• +2

Why are all formal charges in C2H4 zero?

• Because it is an unstable molecule

• Because it has a high boiling point

• Because it is a stable molecule

• Because it is a colored compound

What does a formal charge of zero indicate about a molecule?

• It is highly reactive

• It is radioactive

• It is unstable

• It is stable

What is the significance of having identical formal charges on all atoms in a molecule?

• It shows varied electronegativity

• It suggests uniform stability

• It implies different reactivity

• It indicates a lack of symmetry

What is the common name for C2H4?

• Butane

• Propane

• Ethylene

• Methane