# CH3NH3+ Lewis structure

CH3NH3+ has one carbon atom, six hydrogen atoms, and one nitrogen atom.

In CH3NH3+ Lewis structure, there is a single bond between the carbon and nitrogen atom. Both carbon and nitrogen atoms are attached with two hydrogen atoms, and none of the atoms has a lone pair.

Also, there is a positive (+1) charge on the nitrogen atom.

Contents

## Steps

Here’s how you can easily draw the CH3NH3+ Lewis structure step by step:

#1 Draw a rough skeleton structure
#2 Mention lone pairs on the atoms
#3 If needed, mention formal charges on the atoms

Now, let’s take a closer look at each step mentioned above.

### #1 Draw a rough skeleton structure

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, hydrogen lies in group 1, and nitrogen lies in group 15.

Hence, carbon has four valence electrons, hydrogen has one valence electron, and nitrogen has five valence electrons.

Since CH3NH3+ has one carbon atom, six hydrogen atoms, and one nitrogen atom, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of six hydrogen atoms = 1 × 6 = 6
Valence electrons of one nitrogen atom = 5 × 1 = 5

Now the CH3NH3+ has a positive (+1) charge, so we have to subtract one electron.

So the total valence electrons = 4 + 6 + 5 – 1 = 14

• 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

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Now we have to choose the central atom from carbon and nitrogen. Place the least electronegative atom at the center.

Since carbon is less electronegative than nitrogen, assume that the central atom is carbon.

Therefore, place carbon in the center and hydrogen and nitrogen on either side.

• And finally, draw the rough sketch

### #2 Mention lone pairs on the atoms

Here, we have a total of 7 electron pairs. And seven bonds are already marked. So we do not have to mark any electron pair as a lone pair on the sketch.

### #3 If needed, mention formal charges on the atoms

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

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

For carbon atom, formal charge = 4 – 0 – ½ (8) = 0

For each hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For nitrogen atom, formal charge = 5 – 0 – ½ (8) = +1

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

In the above structure, you can see that the central atom (carbon) forms an octet. The outside atom (nitrogen) also forms an octet, and all hydrogens form a duet. Hence, the octet rule and duet rule are satisfied.

Therefore, this structure is the most stable Lewis structure of CH3NH3+.

And since the CH3NH3+ has a positive (+1) charge, mention that charge on the Lewis structure by drawing brackets as follows:

Next: SeI2 Lewis structure