The Lewis structure for ClO3 (chlorate) involves representing the bonding and lone pairs of electrons in the molecule. To draw the Lewis structure, follow these steps:
- Count the total number of valence electrons: Chlorine (Cl) has 7 valence electrons, and each oxygen (O) has 6 valence electrons. Since there are three oxygen atoms, we have:
- 7 (for Cl) + 3 × 6 (for O) = 25 valence electrons.
- Determine the central atom: Chlorine is less electronegative than oxygen, so it will be the central atom.
- Connect the atoms: Place three oxygen atoms around the chlorine atom, forming single bonds. This uses up 6 of the 25 electrons.
- Add lone pairs to the oxygen atoms: Each oxygen needs 8 electrons to fulfill the octet rule. Adding three lone pairs to each oxygen will consume 18 more electrons, totaling 24. Now, place the remaining electron on the chlorine atom to form a double bond with one of the oxygen atoms, leading to resonance forms.
The final structures show one oxygen with a double bond to chlorine and two oxygens with single bonds. The chlorine will bear a positive charge, and one of the single-bonded oxygens will have a negative charge overall. The resonance and formal charges stabilize the structure.
This compound can be represented as depicted below:
Cl=O
|
O−
|
O−
In conclusion, the Lewis structure for ClO3 indicates a central chlorine atom formatively bonded to oxygen atoms, displaying aspects of resonance and charge distribution that are significant in understanding its chemical behavior.