Bond Order and Molecular Stability

The video tutorial explains how to determine the bond order of the cyanide ion (CN-). It begins with an introduction to bond order and the importance of a valid Lewis structure. The tutorial then demonstrates how to calculate the bond order by examining the shared electrons between carbon and nitrogen, resulting in a bond order of three for CN-. The video further discusses how a higher bond order correlates with shorter and stronger bonds, leading to a more stable molecule. Dr. B concludes by summarizing the key points about bond order and its implications for molecular stability.

What is the first step in finding the bond order for the cyanide ion?

• Draw a valid Lewis structure

• Determine the oxidation state

• Calculate the molecular weight

• Identify the hybridization

How many pairs of electrons are shared between carbon and nitrogen in CN-?

• One pair

• Two pairs

• Three pairs

• Four pairs

What is the bond order of CN-?

• 4

• 3

• 2

• 1

How does bond order affect bond length?

• Bond order does not affect bond length

• Higher bond order results in a longer bond

• Higher bond order results in a shorter bond

• Bond order and bond length are unrelated

Which bond is stronger: a triple bond or a double bond?

• All are equally strong

• Single bond

• Double bond

• Triple bond

What happens to molecular stability as bond order increases?

• Molecular stability decreases

• Molecular stability remains the same

• Molecular stability increases

• Molecular stability is unaffected

Why is a higher bond order associated with a stronger bond?

• Because it involves more atoms

• Because it involves more shared electrons

• Because it has a lower energy level

• Because it has a higher molecular weight