Lewis structure of ClO-

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The Lewis structure of ClO^– contains a single bond between the chlorine atom and oxygen atom, and both the atoms have three lone pairs.

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

Steps

By using the following steps, you can easily draw the Lewis structure of ClO^–:

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… chlorine is a group 17 element and oxygen is a group 16 element. Hence, chlorine has seven valence electrons and oxygen has six valence electrons.

Now ClO^– has one chlorine atom and one oxygen atom.

So the total number of valence electrons = valence electrons of chlorine atom + valence electrons of oxygen atom

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

Therefore, the total number of valence electrons = 7 + 6 + 1 = 14

• Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for chlorine and oxygen as follows:

Electronegativity value of chlorine = 3.16
Electronegativity value of oxygen = 3.44

Obviously, chlorine is less electronegative than chlorine . Hence, assume that chlorine is the central atom.

So now, put chlorine and oxygen next to each other. And draw the rough skeleton structure for the Lewis structure of ClO^– something like this:

Also read: How to draw Lewis structure of Cl₂O (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond as follows:

Also read: How to draw Lewis structure of ClO₄^– (5 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 14 valence electrons. And in the above structure, we have already used two valence electrons. Hence, twelve valence electrons are remaining.

Two valence electrons represent one lone pair. So twelve valence electrons = six lone pairs.

Note that chlorine is 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.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atom is oxygen, so oxygen will get three lone pairs. And the central atom (chlorine) will also get three lone pairs.

So the Lewis structure of ClO^– looks something like this:

In the above structure, you can see that the octet is completed on the central atom (chlorine), and also on the outside atom. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of CBr₄ (4 steps)

#4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

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

Collect the data from the above structure and then, write it down below as follows:

• For chlorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

• For oxygen atom

Valence electrons = 6
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 6 – 6 – ½ (2) = -1

Mention the formal charges of atoms on the structure. So the Lewis structure of ClO^– looks something like this:

In the above structure, you can see that the formal charges of atoms are closer to zero. Therefore, this is the most stable Lewis structure of ClO^–.

And the horizontal line drawn in the above structure represents a pair of bonding valence electrons.

Now ClO^– is an ion having a negative (-1) charge, so draw brackets around the above Lewis structure and mention that charge on the top right corner. And then, the Lewis structure of ClO^– looks something like this:

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Related

• Lewis structure of Cl₂O
• Lewis structure of ClO₄^–
• Lewis structure of CBr₄
• Lewis structure of SeO₂
• Lewis structure of ICl₄^–

External links

• Lewis Structure for ClO- – The University of Maryland
• ClO- Lewis Structure in 6 Steps (With Images) – Pediabay
• How do we write the Lewis structure of the hypochlorite anion, ClO^–? – Socratic
• Formal charge of ClO- – Reddit
• Chemical Bonding: ClO- Lewis Structure – The Geoexchange
• Lewis Structure of ClO – CHEMISTRY COMMUNITY – Laurence Lavelle
• Lewis structure of ClO radical – Chemistry Stack Exchange
• ClO- Lewis Structure (Hypochlorite Ion) – Pinterest
• Clo- lewis structure, Characteristics:13 Facts You Should Know – Lamda Geeks
• ClO- lewis structure, molecular geometry, hybrid, polarity, acid-base – Topblogtenz
• ClO Lewis Structure, Geometry, Hybridization, and Polarity – Techiescientist
• Draw the Lewis structure of the hypochlorite ion, ClO – Homework.Study.com
• Lewis Structure Representation of Free Radicals Similar to ClO – ACS Publications
• Draw the Lewis structure for ClO – Brainly
• Draw the Lewis structure for the molecule ClO. Include all lone pairs of electrons – OneClass