The outermost electron of boron experiences a lower effective nuclear charge than carbon because there is no additional number of shells and carbon has more protons and electrons than boron.
The effective nuclear charge is the amount of charge experienced by an electron taking into account any shielding effects from other electrons. This shielding effect occurs when electrons and shells come between the nucleus and the electron of interest, which causes the effective nuclear charge between the outermost electron and the nucleus to reduce. The more the intervening shells, the more the shielding effect.
However, both carbon and boron have the same number of shielding electrons, because no additional shells come in between. Hence, the main factor that increases the effective nuclear charge between boron and carbon is the increase in the number of protons and electrons.
Boron has an atomic number of 5, meaning that it has 5 electrons and 5 protons, while carbon has an atomic number of 6, so it has 6 electrons and 6 protons. Since opposite charges attract, more electrons and protons means there is an increase in the attraction between the nucleus and the outermost electrons in carbon than in boron; hence, a higher effective nuclear charge.
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