Questions: Give the electronic and molecular geometries for H2 S, SO3. Are either of them nonpolar?

Transcript text: 3. Give the electronic and molecular geometries for $\mathrm{H}_{2} \mathrm{~S}, \mathrm{SO}_{3}$. Are either of them nonpolar?

Solution

Solution Steps

Step 1: Determine the Electronic Geometry of $\mathrm{H}_2\mathrm{S}$

The electronic geometry is determined by the number of electron groups around the central atom. In $\mathrm{H}_2\mathrm{S}$, sulfur is the central atom with two hydrogen atoms bonded to it and two lone pairs of electrons. This results in a total of four electron groups.

The electronic geometry for four electron groups is tetrahedral.

Step 2: Determine the Molecular Geometry of $\mathrm{H}_2\mathrm{S}$

The molecular geometry considers only the arrangement of the atoms, not the lone pairs. With two bonded atoms and two lone pairs, the molecular geometry of $\mathrm{H}_2\mathrm{S}$ is bent.

Step 3: Determine the Polarity of $\mathrm{H}_2\mathrm{S}$

The bent shape and the difference in electronegativity between hydrogen and sulfur make $\mathrm{H}_2\mathrm{S}$ a polar molecule.

Step 4: Determine the Electronic Geometry of $\mathrm{SO}_3$

In $\mathrm{SO}_3$, sulfur is the central atom bonded to three oxygen atoms with no lone pairs. This results in three electron groups.

The electronic geometry for three electron groups is trigonal planar.

Step 5: Determine the Molecular Geometry of $\mathrm{SO}_3$

Since there are no lone pairs on the central atom, the molecular geometry is the same as the electronic geometry, which is trigonal planar.

Step 6: Determine the Polarity of $\mathrm{SO}_3$

The trigonal planar shape and the symmetrical distribution of the oxygen atoms around the sulfur atom make $\mathrm{SO}_3$ a nonpolar molecule.

Final Answer

$\mathrm{H}_2\mathrm{S}$:
- Electronic Geometry: Tetrahedral
- Molecular Geometry: Bent
- Polar: Yes
$\mathrm{SO}_3$:
- Electronic Geometry: Trigonal Planar
- Molecular Geometry: Trigonal Planar
- Polar: No

\[ \boxed{ \begin{array}{l} \text{H}_2\text{S}: \text{Tetrahedral, Bent, Polar} \\ \text{SO}_3: \text{Trigonal Planar, Trigonal Planar, Nonpolar} \end{array} } \]

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