Answer
a. ionic
b. nonpolar covalent
c. polar covalent
d. ionic
e. polar covlent
f. nonpolar covalent
Work Step by Step
a. The electronegativity difference between chlorine (3.16) and rubidium (0.82) is 2.34. This difference is greater than the 1.6 difference necessary for the bond to be considered ionic.
b. Because the 2 atoms involved in this bond are both sulfur, the electronegativity difference is 0. This difference is indicative of a nonpolar bond.
c. The electronegativity difference between fluorine (3.98) and carbon (2.55) is 1.43. This difference is greater than the 0.4 difference necessary for the bond to be considered polar covalent but less than the 1.6 difference necessary for the bond to be considered ionic.
d. The electronegativity difference between sulfur (2.58) and barium (0.89) is 1.69. This difference is greater than the 1.6 difference necessary for the bond to be considered ionic.
e. The electronegativity difference between nitrogen (3.04) and phosphorus (2.19) is 0.85. This difference is greater than the 0.4 difference necessary for the bond to be considered polar covalent but less than the 1.6 difference necessary for the bond to be considered ionic.
f. The electronegativity difference between hydrogen (2.20) and boron (2.04) is 0.16. This difference is less than the 0.4 difference necessary for the bond to be considered polar covalent; therefore, it is nonpolar covalent.
