ClO- Lewis structure

ClO^– (hypochlorite) has one chlorine atom and one oxygen atom.

In the ClO^– Lewis structure, there is a single bond between the chlorine and oxygen atom, and on both chlorine and oxygen atoms, there are three lone pairs.

Also, there is a negative (-1) charge on the oxygen atom.

Alternative method: Lewis structure of ClO^–

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, chlorine lies in group 17, and oxygen lies in group 16.

Hence, chlorine has seven valence electrons and oxygen has six valence electrons.

Since ClO^– has one chlorine atom and one oxygen atom, so…

Valence electrons of one chlorine atom = 7 × 1 = 7
Valence electrons of one oxygen atom = 6 × 1 = 6

Now the ClO^– has a negative (-1) charge, so we have to add one more electron.

So the total valence electrons = 7 + 6 + 1 = 14

Learn how to find: Chlorine valence electrons and Oxygen valence electrons

• Second, find the total electron pairs

We have a total of 14 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 14 ÷ 2 = 7

• Third, determine the central atom

We have to place the least electronegative atom at the center.

Since chlorine is less electronegative than oxygen, assume that the central atom is chlorine.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 7 electron pairs. And one Cl — O bond is already marked. So we have to only mark the remaining six electron pairs as lone pairs on the sketch.

Also remember that chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell. And oxygen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atom is oxygen.

So for each atom, there are three lone pairs.

Mark the lone pairs on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

For oxygen atom, formal charge = 6 – 6 – ½ (2) = -1

Here, the oxygen atom has a charge, so mark it on the sketch as follows:

Final structure

The final structure of ClO^– consists of a chlorine atom connected to an oxygen atom through a single covalent bond. In this arrangement, both the chlorine and the oxygen atoms satisfy the octet rule by maintaining three lone pairs each alongside their shared bonding pair. This setup is the most stable because it results in a formal charge of 0 on the chlorine atom and -1 on the oxygen atom, which is the most electronegative element, representing the most energetically favorable distribution for the ion. Consequently, this specific electronic distribution serves as the definitive and most accurate Lewis representation of the hypochlorite ion.

To complete the representation, draw square brackets around the entire Lewis structure and place a “-” or “-1” sign as a superscript outside the upper right bracket. This notation signifies that the negative charge is a property of the whole ion.

Next: NOCl Lewis structure

External video

• ClO- Lewis Structure – How to Draw the Lewis Structure for ClO- – YouTube • Wayne Breslyn

External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/ClO-lewis-structure.html
• https://techiescientist.com/clo-lewis-structure/
• https://socratic.org/questions/57f93c5f7c01492217dba649
• https://lambdageeks.com/clo-lewis-structure/
• https://topblogtenz.com/hypochlorite-ion-clo-lewis-structure-molecular-geometry-hybridization-polarity-acid-base/