Question

1. chemical name: chlorate anion

formula: clo₃⁻
lewis electron - dot structure (with resonance description):
perspective drawing of one resonance structure with bond angles:
standard electron geometry:
molecular geometry:
hybridization of central atom:
is the molecule polar, nonpolar, or ion?

Explanation:

Step1: Calculate valence - electrons

Chlorine (Cl) has 7 valence electrons, oxygen (O) has 6 valence electrons, and there is a - 1 charge. So the total number of valence electrons is \(7 + 3\times6+1=26\).

Step2: Draw Lewis structure

Place Cl in the center. Connect Cl to each O with a single - bond first, using 6 electrons. Then distribute the remaining 20 electrons as lone - pairs on the O atoms. Resonance occurs as the double - bond can be formed with any of the three O atoms.

Step3: Determine electron geometry

The central Cl atom has 4 electron - groups (3 bonding pairs and 1 lone - pair). So the standard electron geometry is tetrahedral.

Step4: Determine molecular geometry

With 3 bonding pairs and 1 lone - pair around the central Cl atom, the molecular geometry is trigonal pyramidal.

Step5: Determine hybridization

Since there are 4 electron - groups around the central Cl atom, the hybridization of the central Cl atom is \(sp^{3}\).

Step6: Determine polarity

The \(ClO_{3}^{-}\) is an ion.

Answer:

Lewis electron - dot structure: Cl is in the center, single - bonded to three O atoms. Resonance exists as the double - bond can be formed with any of the three O atoms.
Perspective drawing: Trigonal pyramidal shape with bond angles less than 109.5° due to the lone - pair repulsion.
Standard electron geometry: Tetrahedral
Molecular geometry: Trigonal pyramidal
Hybridization of central atom: \(sp^{3}\)
Is the molecule polar, nonpolar, or ion? Ion