Question

Using the table of electron negativities, subtract the larger from the smaller for each of these bonds. If the difference is 2.0 or greater, it is ionic. If it's 0.5 or less, it's nonpolar. If it's between 0.5 and 2.0, it's polar covalent.

A) O-Se
B) Be-Cl
C) Br-Cl
D) Na-O

Answer 1

To determine the bond type, subtract the lesser electronegativity value from the greater one for each atom pair. Bonds with a difference of 2.0 or more are ionic, 0.5 or less are nonpolar covalent, and between 0.5 and 2.0 are polar covalent.

Step-by-step explanation:

The question involves determining the type of bonding (ionic, nonpolar covalent, or polar covalent) between two atoms based on the difference in their electronegativities. To categorize each bond: Subtract the electronegativity of the less electronegative atom from that of the more electronegative atom. If the difference is 2.0 or greater, the bond is ionic. If the difference is 0.5 or less, the bond is nonpolar covalent. If the difference is between 0.5 and 2.0, the bond is polar covalent.

Without the specific electronegativity values for the pairs mentioned (O-Se, Be-Cl, Br-Cl, Na-O), we refer to a general table of electronegativities to determine the type of bond. Typically, a bond between a metal (like Na) and a nonmetal (like O) would be ionic, and bonds between nonmetals (like O and Se, or Br and Cl) would be either nonpolar or polar covalent depending on the electronegativity difference.