# What is the Charge on Acetate ion (C2H3O2 or CH3COO)?

The Charge of Acetate ion (or C2H3O2 or CH3COO) is 1-.

But the question is how can you find the charge on Acetate ion (or C2H3O2 or CH3COO)?

Well there are 2 methods by which you can find the charge of Acetate ion (or C2H3O2 or CH3COO).

Lets dive right into these methods one by one.

You can also refer to the below video from which you will learn to find charge of any ion.

## Method 1: By looking at what it is bonded to

The charge of Acetate ion (or C2H3O2 or CH3COO) can be found out by looking at what it is bonded to.

So let’s take some examples of compounds that contain C2H3O2 (or CH3COO); like CH3COOH, CH3COONa, etc.

Example 1: CH3COOH
In CH3COOH, the CH3COO is bonded to Hydrogen (H).
You know that the ionic charge of H is 1+.
So you can easily say that the charge of CH3COO should be 1-, then only it will get canceled out.
Hence the charge of CH3COO in CH3COOH is 1-.

Example 2: CH3COONa
In CH3COONa, the CH3COO is bonded to Sodium (Na).
And again, you know that the ionic charge of Na is 1+.
So here also you can easily say that the charge of CH3COO should be 1-, then only it will get canceled out.
Hence the charge of CH3COO in CH3COONa is 1-.

As seen from the above examples,
The charge of CH3COO is 1-.

In this way, you can easily find the charge of CH3COO by looking at what it is bonded to.

## Method 2: By calculating the formal charge using lewis structure

In order to calculate the formal charge on CH3COO (Acetate ion), you should know the Lewis dot structure of CH3COO (Acetate ion).

Here is the lewis structure of CH3COO.

Now using the above lewis structure of CH3COO, you have to find the formal charge on each atom that is present in the CH3COO molecule.

For calculating the formal charge, you need to remember this formula;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

You can see the bonding and nonbonding electrons of CH3COO from the image given below.

So now let’s calculate the formal charge on each individual atom present in CH3COO.

Formal charge on Carbon atom:
Valence electrons = 4 (as it is in group 14 on periodic table) [1]
Nonbonding electrons = 0
Bonding electrons = 8

So according to the formula of formal charge, you will get;

Formal charge on Nitrogen = Valence electrons – Nonbonding electrons – (Bonding electrons)/2 = 4 – 0 – (8/2) = 0

So the formal charge on carbon atom is 0.

Formal charge on Hydrogen atom:
Valence electron = 1 (as it is in group 1 on periodic table) [2]
Nonbonding electrons = 0
Bonding electrons = 2

So according to the formula of formal charge, you will get;

Formal charge on Hydrogen = Valence electrons – Nonbonding electrons – (Bonding electrons)/2 = 1 – 0 – (2/2) = 0

So the formal charge on hydrogen atom is 0.

Formal charge on double bonded Oxygen atom:
Valence electron = 6 (as it is in group 16 on periodic table) [3]
Nonbonding electrons = 4
Bonding electrons = 4

So according to the formula of formal charge, you will get;

Formal charge on double bonded Oxygen = Valence electrons – Nonbonding electrons – (Bonding electrons)/2 = 6 – 4 – (4/2) = 0

So the formal charge on double bonded oxygen atom is 0.

Formal charge on single bonded Oxygen atom:
Valence electron = 6 (as it is in group 16 on periodic table)
Nonbonding electrons = 6
Bonding electrons = 2

So according to the formula of formal charge, you will get;

Formal charge on single bonded Oxygen = Valence electrons – Nonbonding electrons – (Bonding electrons)/2 = 6 – 6 – (2/2) = 1-

So the formal charge on single bonded oxygen atom is 1-.

Now let’s put all these charges on the lewis dot structure of NO3.

So there is overall 1- charge left on the entire molecule.

This indicates that the CH3COO (Acetate ion) has 1- charge.

I hope you have understood the above calculations of CH3COO (Acetate ion). But for your tests, you don’t need to remember the entire calculations. You should just try to remember that CH3COO has 1- charge.

Check out some other related topics for your practice.

Author
##### Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. With a desire to make learning accessible for everyone, he founded Knords Learning, an online learning platform that provides students with easily understandable explanations.