Question #44348

Consider the following statements regarding the structural and electronic properties of methanol ($\ce{CH3OH}$) and silanol ($\ce{SiH3OH}$):

I. The $\ce{Si-O-H}$ bond angle in $\ce{SiH3OH}$ is larger than the $\ce{C-O-H}$ bond angle in $\ce{CH3OH}$ due to $\ce{p\pi-d\pi}$ back-bonding and the concentration of s-character in the $\ce{Si-O}$ bond as per Bent's rule. II. The $\ce{p\pi-d\pi}$ back-bonding in $\ce{SiH3OH}$ creates an electron density shift that opposes the primary $\ce{Si^{\delta+}-O^{\delta-}}$ sigma bond polarity, thereby reducing the overall bond dipole moment. III. $\ce{SiH3OH}$ is a stronger Brønsted acid than $\ce{CH3OH}$ because the $\ce{SiH3O-}$ conjugate base is stabilized by $\ce{p\pi-d\pi}$ delocalization, which effectively disperses the negative charge. IV. The Oxygen atom in $\ce{SiH3OH}$ is $sp$ hybridized, resulting in a linear $\ce{Si-O-H}$ geometry to maximize the overlap of both oxygen lone pairs with the vacant 3d orbitals of Silicon.

Determine the total number of CORRECT statements.