To assess the accuracy of the statements comparing ionic and covalent bonds, let's evaluate each one:
A. Covalent bonds generally have less polarity than ionic bonds.
- This statement is true. Ionic bonds generally form between atoms with a large difference in electronegativity, which leads to polar character and the full transfer of electrons, while covalent bonds typically involve sharing electrons and usually have less polarity.
B. More electrons are transferred in the formation of covalent bonds compared to ionic bonds.
- This statement is false. In ionic bonds, there is complete transfer of one or more electrons from one atom to another, while in covalent bonds, electrons are shared (and not transferred), so typically one or two pairs of electrons are involved.
C. Elements in Group IA are more likely to form covalent bonds rather than ionic bonds with other atoms.
- This statement is false. Group IA elements (alkali metals) are more likely to form ionic bonds because they readily lose their one valence electron to achieve a stable electron configuration, forming cations. They typically do not form covalent bonds.
D. Atoms in covalent bonds have a greater difference in electronegativity than atoms in ionic bonds.
- This statement is false. In ionic bonds, there is a large difference in electronegativity (typically greater than 1.7), whereas covalent bonds usually have a smaller difference in electronegativity (usually less than 1.7).
In summary, the only accurate statement among the options is: A. Covalent bonds generally have less polarity than ionic bonds.
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