What is the hybridization of the central atom in \(NH_3\)?
sp^3d
In \(NH_3\), the central atom is nitrogen. Nitrogen has 5 valence electrons and forms 3 single bonds with hydrogen atoms, leaving 1 lone pair. The steric number (number of bonded atoms + lone pairs) is: \[ 3 \, (\text{bonds}) + 1 \, (\text{lone pair}) = 4 \] A steric number of 4 corresponds to \(sp^3\) hybridization. Thus, the hybridization of nitrogen in \(NH_3\) is: \(\text{sp}^3\)
Given below are two statements:
Statement (II): Structure III is most stable, as the orbitals having the lone pairs are axial, where the $ \ell p - \beta p $ repulsion is minimum. In light of the above statements, choose the most appropriate answer from the options given below:
Consider the following statements:
Statement-I: The products formed when diborane burns in air are \({B}_2{O}_3\), \({H}_2\), and \({O}_2\).
Statement-II: Hybridization of boron atom in orthoboric acid is \(sp^2\). The correct answer is: