Let's analyze each statement to determine which one accurately compares ionic and covalent bonds:
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More electrons are transferred in the formation of covalent bonds compared to ionic bonds.
False - In ionic bonds, electrons are transferred from one atom to another (typically from metals to nonmetals), while in covalent bonds, electrons are shared between atoms. Generally, only a few electrons are involved in these processes, and covalent bonds do not involve the transfer of electrons. -
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 usually form between atoms with similar electronegativities (typically a difference of less than 1.7). -
Covalent bonds generally have less polarity than ionic bonds.
True - Ionic bonds are generally considered to be more polar because they result from the complete transfer of electrons, leading to the formation of charged ions. Covalent bonds, particularly those between similar atoms, have less polarity since the shared electrons are more evenly distributed. -
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) typically form ionic bonds with nonmetals, as they readily lose one electron to form positively charged ions.
Based on this analysis, the statement that accurately compares ionic and covalent bonds is:
Covalent bonds generally have less polarity than ionic bonds.