Question

what are the geometry and hybridization around each carbon atom in benzene, c6h6
a. sp2, trigonal planar
b.sp,linear
c.sp3,tetrahedral
d. sp3, trigonal planar
question 2
1 pts
which of the following compounds is capable of hydrogen bonding?
a.hcl
b.h2s
c.nh3
d.hi

Explanation:

Step1: Analyze benzene's carbon - atom bonding

Each carbon in benzene has 3 sigma bonds and 1 pi bond. Hybridization is determined by the number of sigma - bonds and lone pairs. With 3 sigma - bonds, the hybridization is $sp^{2}$.

Step2: Determine the geometry

For $sp^{2}$ hybridized atoms, the electron - pair geometry and molecular geometry (when no lone pairs on the central atom) is trigonal planar. So, the geometry around each carbon in benzene is trigonal planar.

Step3: Analyze hydrogen - bonding conditions

Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (N, O, F) and there is another electronegative atom with a lone pair nearby. In $HCl$, $H_2S$, and $HI$, the electronegativities of $Cl$, $S$, and $I$ are not high enough compared to $N$, $O$, $F$ for strong hydrogen - bonding. In $NH_3$, hydrogen is bonded to nitrogen (a highly electronegative atom), and nitrogen has a lone pair, so it can form hydrogen bonds.

Answer:

Question 1: A. sp2, trigonal planar
Question 2: C. $NH_3$