Given that the methyl group (ππ=2.3)Β is more electronegative than hydrogen (ππ=2.1), but the methyl group is a better electron-donating group, which of the following statements best explains this behavior?
1
The methyl group has a larger atomic radius compared to hydrogen, resulting in lower electron density around the carbon atom, thus promoting electron donation.
2
Despite the higher electronegativity of the methyl group, it has a higher degree of s-character in its hybrid orbitals, which stabilizes the lone pair and makes it an effective electron-pushing group.
3
The inductive effect of the methyl group, being a larger group, allows it to donate electron density more effectively than hydrogen, despite its higher electronegativity.
4
The hyperconjugation effect in methyl groups, which allows the overlap of Ο-bonds with adjacent empty orbitals, enhances its electron-donating ability compared to hydrogen.