Which of the following statements accurately compares ionic and covalent bonds? (1 point)

Question

• Atoms in covalent bonds have a greater difference in electronegativity than atoms in ionic bonds.
• More electrons are transferred in the formation of covalent bonds compared to ionic bonds.
• Elements in Group IA are more likely to form covalent bonds rather than ionic bonds with other atoms.
• Covalent bonds generally have less polarity than ionic bonds.

Answer 1

The statement that accurately compares ionic and covalent bonds is:

• Covalent bonds generally have less polarity than ionic bonds.

This statement is true because ionic bonds typically form between atoms with a large difference in electronegativity, leading to a complete transfer of electrons and the formation of charged ions, which results in high polarity. Covalent bonds, on the other hand, usually involve the sharing of electrons between atoms that have similar electronegativities, leading to lower polarity.

The other statements are not accurate:

• Atoms in covalent bonds usually have a smaller difference in electronegativity compared to atoms in ionic bonds.
• In ionic bonds, electrons are transferred, while in covalent bonds, electrons are shared. Therefore, the statement about the number of electrons transferred is not correct.
• Elements in Group IA (alkali metals) typically form ionic bonds with nonmetals rather than covalent bonds.

Thus, the last statement about polarity is the only accurate comparison between ionic and covalent bonds.