1. Draw the Lewis Structure
* Count valence electrons: H (1), Cl (7), O (6) x 3 = 26 valence electrons
* Central atom: Cl is the least electronegative atom and will be the central atom.
* Connect atoms: Connect Cl to each O atom and one O atom to the H atom.
* Complete octets: Place remaining electrons around the O atoms to complete their octets. The Cl atom will also have a complete octet.
The Lewis structure looks like this:
```
O
/ \
H - O - Cl - O
\
O
```
2. Determine the Electron Pair Geometry
* Count electron groups: Cl has 4 electron groups (3 single bonds and 1 double bond)
* Electron Pair Geometry: 4 electron groups result in a tetrahedral electron pair geometry.
3. Determine the Molecular Geometry
* Consider lone pairs: Cl has one lone pair.
* Molecular Geometry: The lone pair repels the bonding pairs, pushing them closer together. This results in a trigonal pyramidal molecular geometry.
Therefore, the molecular geometry of HClO3 is trigonal pyramidal.
