The correct statement comparing ionic and covalent bonds is:
Covalent bonds tend to be less polar than ionic bonds.
To elaborate:
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Covalent bonds tend to be less polar than ionic bonds: This is true because ionic bonds are formed between atoms with a large difference in electronegativity (typically 1.7 or greater), leading to a complete transfer of electrons. In contrast, covalent bonds involve atoms with smaller differences in electronegativity, resulting in shared electrons, which makes them generally less polar.
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Group IA elements are more likely to form covalent bonds than ionic bonds with other atoms: This statement is generally not true. Group IA elements (alkali metals) typically form ionic bonds with nonmetals because they readily lose their single valence electron.
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Covalent bonds have a greater difference in electronegativities between atoms than ionic bonds: This statement is incorrect. Ionic bonds are characterized by a significant difference in electronegativity, while covalent bonds are formed by smaller differences.
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More electrons are involved in forming covalent bonds than ionic bonds: This statement is misleading. Each covalent bond typically involves the sharing of two electrons, while ionic bonds usually involve the transfer of one or more electrons from one atom to another. However, the number of electrons involved depends on the specific compounds in question.
In summary, the first statement regarding polarity is the correct choice.
5 answers