Question

what is the hybridization of the indicated atoms? i ii n≡ n nh oh o i ii a. sp² sp² b. sp² sp³ c. sp sp² d. sp sp³ a b c d

Explanation:

Step1: Analyze atom I

Atom I is a nitrogen in a triple - bond ($N\equiv C$). A triple - bonded atom has two regions of electron density (the triple bond and a lone pair or another bond). According to the VSEPR theory, the hybridization of an atom with two regions of electron density is sp.

Step2: Analyze atom II

Atom II is a nitrogen in a single - bonded environment ($-NH -$). This nitrogen has four regions of electron density (three single bonds and one lone pair). According to the VSEPR theory, the hybridization of an atom with four regions of electron density is $sp^{3}$.

Answer:

D. sp, $sp^{3}$