Question

what is the molecular geometry of so₂?
tetrahedral
linear
bent
trigonal pyramidal
question 9 (0.0862 points)
which molecule below has hydrogen bonding?
nh₃
h₂
ch₄
hcl

Explanation:

First Question (Molecular Geometry of \( \text{SO}_2 \)):

To determine the molecular geometry of \( \text{SO}_2 \), we use the VSEPR theory. The central sulfur atom has 6 valence electrons. It forms two double bonds with oxygen atoms and has one lone pair of electrons. The electron - pair geometry is trigonal planar (3 electron - dense regions: 2 bonding regions and 1 lone pair). The molecular geometry, which considers only the bonding regions, is bent (or angular) because the lone pair repels the bonding pairs, causing the bond angle to be less than 120°. Tetrahedral geometry has 4 bonding regions, linear has 2 bonding regions with no lone pairs, and trigonal pyramidal has 3 bonding regions and 1 lone pair (but in \( \text{SO}_2 \), the bonding is double bonds and the electron - pair arrangement is different from trigonal pyramidal).

Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (N, O, or F) and is attracted to another electronegative atom. In \( \text{NH}_3 \), the hydrogen atoms are bonded to nitrogen (a highly electronegative atom). The lone pair on the nitrogen atom can form hydrogen bonds with the hydrogen atoms of other \( \text{NH}_3 \) molecules. \( \text{H}_2 \) is a non - polar molecule with only H - H bonds, no electronegative atom to form hydrogen bonds. \( \text{CH}_4 \) has C - H bonds, and carbon is not electronegative enough to form hydrogen bonds. \( \text{HCl} \) has H - Cl bonds, and chlorine, while electronegative, does not form hydrogen bonds in the same way as N, O, or F (the H - Cl bond is polar, but the conditions for hydrogen bonding are not met as well as in \( \text{NH}_3 \)).

Answer:

C. bent

Second Question (Molecule with Hydrogen Bonding):