Which is the correct statement?As the s-character of a hybrid orbital decreases(I) The bond angle decreases(II) The bond strength increases(III) The bond length increases(IV) Size of orbitals increases(A) (I), (III) and (IV)(B) (II), (III) and (IV)(C) (I) and (II)(D) All are correct

The correct statement is:

(B) (II), (III), and (IV)

Explanation:

(I) The bond angle is not directly affected by the s-character of a hybrid orbital. It primarily depends on the number of lone pairs and bonding pairs around the central atom, as well as the repulsion between these electron pairs. Therefore, statement (I) is incorrect.

(II) The bond strength increases as the s-character of a hybrid orbital increases because the s-orbital is closer to the nucleus and has better overlap with other orbitals, leading to stronger bonding. So, statement (II) is correct.

(III) The bond length decreases as the s-character of a hybrid orbital increases because the s-orbital is smaller and closer to the nucleus, resulting in shorter bond lengths. So, statement (III) is correct.

(IV) The size of orbitals does not necessarily increase or decrease with changes in s-character. It depends on the specific hybridization and the involvement of different types of orbitals. Therefore, statement (IV) is not necessarily correct.

Therefore, the correct statements are (II), (III), and (IV), making option (B) the correct choice.