Question

A bond is rarely just ionic or covalent. Rather, bonds are described as having ionic character or covalent character. Discuss how differences in electronegativity contribute to this description.

a) Electronegativity is irrelevant to bond character
b) Higher electronegativity leads to more ionic character
c) Lower electronegativity leads to more covalent character
d) Electronegativity has no effect on bond properties

Answer 1

b) Higher electronegativity leads to more ionic character. The concept of ionic and covalent character in bonds is influenced by differences in electronegativity, which is the ability of an atom to attract electrons.

Step-by-step explanation:

b) Higher electronegativity leads to more ionic character. The concept of ionic and covalent character in bonds is influenced by differences in electronegativity, which is the ability of an atom to attract electrons. In a purely ionic bond, there is a significant difference in electronegativity between the atoms involved. One atom (usually a metal) has a much lower electronegativity, essentially donating electrons to the more electronegative atom (usually a nonmetal). This results in the formation of ions with opposite charges, and the bond is considered predominantly ionic. On the other hand, in a purely covalent bond, the atoms share electrons more equally. When there is a smaller electronegativity difference, the bond exhibits more covalent character. The degree of ionic or covalent character in a bond is often described on a continuum, with polar covalent bonds having intermediate characteristics. Therefore, option b, "Higher electronegativity leads to more ionic character," accurately reflects the relationship between electronegativity differences and bond character.