To accurately compare ionic and covalent bonds, let's evaluate each of the statements provided:
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Atoms in covalent bonds have a greater difference in electronegativity than atoms in ionic bonds.
- False. Ionic bonds typically form between atoms with a large difference in electronegativity (generally greater than 1.7), while covalent bonds form between atoms with a smaller difference in electronegativity.
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More electrons are transferred in the formation of covalent bonds compared to ionic bonds.
- False. In ionic bonding, electrons are transferred from one atom to another, often resulting in one atom gaining one or more electrons and another atom losing one or more electrons. In covalent bonding, atoms share electrons rather than transferring them.
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Covalent bonds generally have less polarity than ionic bonds.
- True. Ionic bonds are formed between ions with significant differences in electronegativity, leading to a complete transfer of electrons and resulting in highly polar bonds. Covalent bonds involve sharing electrons and can be polar or nonpolar depending on the electronegativity difference, but they generally exhibit less polarity compared to ionic bonds.
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Elements in Group IA are more likely to form covalent bonds rather than ionic bonds with other atoms.
- False. Elements in Group IA (alkali metals) tend to lose one electron easily and typically form ionic bonds when reacting with nonmetals, rather than forming covalent bonds.
Based on the analysis, the only accurate statement comparing ionic and covalent bonds is:
Covalent bonds generally have less polarity than ionic bonds.
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