Question

1. chemical name: hydrogen sulfide formula: h2s lewis electron - dot structure: perspective drawing with bond angles: standard electron geometry: molecular geometry: hybridization of central atom: is the molecule polar, nonpolar, or ion?

Explanation:

Step1: Determine valence - electrons

Sulfur has 6 valence electrons and each hydrogen has 1 valence electron. So, $H_2S$ has $6 + 2\times1=8$ valence electrons.

Step2: Draw Lewis structure

The sulfur atom is the central atom. Sulfur forms single bonds with two hydrogen atoms and has two lone - pairs of electrons.

Step3: Find electron - geometry

The central sulfur atom has 4 electron - groups (2 bonding pairs and 2 lone pairs). According to VSEPR theory, the electron - geometry is tetrahedral.

Step4: Determine molecular geometry

With 2 bonding pairs and 2 lone pairs around the central sulfur atom, the molecular geometry is bent.

Step5: Determine hybridization

Since there are 4 electron - groups around the central sulfur atom, the hybridization of the central sulfur atom is $sp^3$.

Step6: Determine polarity

The $H - S$ bonds are polar due to the electronegativity difference between hydrogen and sulfur. Also, the bent molecular shape means the bond dipoles do not cancel out. So, $H_2S$ is a polar molecule.

Answer:

Lewis electron - dot structure: S is the central atom with two single bonds to H atoms and two lone pairs of electrons on S.
Standard electron geometry: Tetrahedral
Molecular geometry: Bent
Hybridization of central atom: $sp^3$
Is the molecule polar, non - polar, or ion? Polar
(Note: A perspective drawing with bond angles would show a bent shape with bond angles slightly less than 109.5° due to the repulsion of lone pairs)