To draw the Lewis structure for HClO3 (chloric acid), we start by determining the total number of valence electrons. Chlorine (Cl) has 7 valence electrons, each oxygen (O) has 6, and hydrogen (H) has 1. Therefore, the total count is:
- Cl: 7
- 3 × O: 3 × 6 = 18
- H: 1
Total = 7 + 18 + 1 = 26 valence electrons.
Next, we arrange the atoms with Cl as the central atom, bonded to three oxygens and one hydrogen. One of the O atoms is connected through a double bond to maximize the number of bonds and fulfill the octet rule for oxygen. This setup looks like:
- Cl is bonded to one -OH group and one O through a double bond, while the second O is bonded through a single bond.
After placing the bonds, we distribute the remaining electrons to satisfy the octets of all atoms. Based on this description, the Lewis structure can be represented visually with Cl in the center connected to three O atoms.
A) Electron Geometry:
The electron geometry of HClO3 is tetrahedral since there are four regions of electron density (three bonding pairs and one lone pair on the chlorine).
B) Molecular Geometry:
The molecular geometry is trigonal pyramidal. This is due to the presence of the lone pair on chlorine, which affects the arrangement of the bonding pairs.
C) Hybridization:
The hybridization of the central chlorine atom in HClO3 is sp3. This reflects the tetrahedral arrangement of electron pairs surrounding the chlorine atom.
D) Polarity:
HClO3 is a polar molecule. The difference in electronegativity between chlorine and oxygen, combined with the molecular geometry, creates a dipole moment, resulting in an uneven distribution of electron density.