Let's evaluate each statement to find the one that accurately compares ionic and covalent bonds:
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Atoms in covalent bonds have a greater difference in electronegativity than atoms in ionic bonds.
- This statement is false. Ionic bonds typically occur between atoms with a large difference in electronegativity, usually greater than 1.7. Covalent bonds occur when the difference is smaller (generally less than 1.7).
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More electrons are transferred in the formation of covalent bonds compared to ionic bonds.
- This statement is false. In ionic bonds, electrons are transferred from one atom to another (usually one atom loses one or more electrons, while another gains one or more), typically involving the transfer of whole electrons. In covalent bonds, electrons are shared between atoms; thus, the nature of "transfer" is different.
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Elements in Group IA are more likely to form covalent bonds rather than ionic bonds with other atoms.
- This statement is false. Group IA (alkali metals) typically form ionic bonds because they have one electron in their outermost shell, which they tend to lose easily to achieve a stable electron configuration, forming positive ions.
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Covalent bonds generally have less polarity than ionic bonds.
- This statement is true. Ionic bonds are formed between atoms with a significant difference in electronegativity, resulting in a strong dipole (high polarity). Covalent bonds can be polar or nonpolar, with nonpolar covalent bonds resulting in minimal or no polarity.
Based on this evaluation, the correct statement that accurately compares ionic and covalent bonds is:
Covalent bonds generally have less polarity than ionic bonds.
1 answer