The document discusses how differences in electronegativity between bonding elements determine the type of bond formed. For instance, in H2, a covalent bond forms due to an electronegativity difference of 0, while in HF, an ionic bond forms with a difference of 3.04. It further describes the characteristics of ionic bonds as strong and difficult to break, compared to covalent bonds, which are held together by shared electrons and are relatively weaker.

1. Difference in Electronegativity Affects the Bond Type
Electronegativity differences between bonding elements is used to predict the bond type.
H2 – Electronegativity difference = 2.20 – 2.20 = 0 so a Covalent bond is formed.
HF – Electronegativity difference = 4.00 – 0.96 = 3.04 so an Ionic bond is formed
ELECTRONEGATIVITY DIFFERENCE
Ionic Bonds
• Held together by
electrical attraction
•Strong; hard to break
Covalent Bonds
• Held together by
shared electrons
• Not as strong