Question

1. chemical name: selenium dioxide

formula: seo₂
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

Selenium has 6 valence electrons and each oxygen has 6 valence electrons. So total valence electrons = 6 (from Se)+2×6 (from O)=18.

Step2: Draw Lewis electron - dot structure

Se is the central atom. Connect Se to two O atoms with single bonds first. Then distribute the remaining electrons to satisfy the octet rule. The Lewis structure has Se with a lone pair and double - bonds to each O.

Step3: Find electron geometry

The central Se atom has 3 electron - groups (2 bonding and 1 lone pair). So the standard electron geometry is trigonal planar.

Step4: Determine molecular geometry

With 1 lone pair on the central Se atom, the molecular geometry is bent.

Step5: Find hybridization

Since Se has 3 electron - groups around it, the hybridization of the central Se atom is $sp^{2}$.

Step6: Determine polarity

The molecule is polar because the bent shape and the difference in electronegativity between Se and O result in a non - zero net dipole moment.

Answer:

Lewis electron - dot structure: Se with a lone pair and double - bonds to each O.
Perspective drawing with bond angles: Bent shape with bond angle less than 120°.
Standard electron geometry: Trigonal planar.
Molecular geometry: Bent.
Hybridization of central atom: $sp^{2}$.
Is the molecule polar, nonpolar, or ion? Polar.