The accurate comparison of ionic and covalent bonds from the provided statements is:
Covalent bonds generally have less polarity than ionic bonds.
Here's a brief explanation for each statement to clarify:
-
Atoms in covalent bonds have a greater difference in electronegativity than atoms in ionic bonds. - This statement is incorrect. Ionic bonds typically form between atoms with a large difference in electronegativity, often greater than 1.7, while covalent bonds usually form between atoms with similar electronegativities.
-
Covalent bonds generally have less polarity than ionic bonds. - This statement is correct. Ionic bonds are highly polar because of the complete transfer of electrons, while covalent bonds involve sharing of electrons, which can be nonpolar or polar depending on the difference in electronegativity.
-
More electrons are transferred in the formation of covalent bonds compared to ionic bonds. - This statement is incorrect. In ionic bonds, electrons are completely transferred from one atom to another, while in covalent bonds, electrons are shared but not transferred.
-
Elements in Group IA are more likely to form covalent bonds rather than ionic bonds with other atoms. - This statement is incorrect. Group IA elements (alkali metals) typically form ionic bonds by losing their single valence electron.
Therefore, the correct answer is the second statement.
1 answer