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Lewis Structure of Methanol

Jun 4,2026

Methanol (CH3OH) is a polar molecule. Its Lewis structure consists of a central carbon atom (C), three surrounding hydrogen atoms (H) and a hydroxyl (-OH) group. The hydroxyl (-OH) group acts as a single unit, with the atoms connected by single bonds. The carbon atom (C) is linked to the other three hydrogen atoms (H) via single bonds, and is also linked to the oxygen atom (O) of the hydroxyl (-OH) group via a single bond. Furthermore, the oxygen atom (O) possesses two pairs of lone pairs of electrons (see figure below).

Lewis Structure of Methanol

How to draw the Lewis structure of CH3OH?

tep 1: Calculate the total number of valence electrons

The total number of valence electrons in CH3OH is the sum of the valence electrons of one carbon atom (C), four hydrogen atoms (H) and one oxygen atom (O). According to the periodic table, the valence electrons of carbon (C), hydrogen (H) and oxygen (O) are 4, 1 and 6 respectively.

Thus, the total number of valence electrons in the CH3OH molecule = 1 (4) + 4 (1) + 1 (6) = 14

Step 2: Identifying the central atom

According to the rules of Lewis structures, the atom with the lower electronegativity is the central atom, and hydrogen atoms are always placed in the outermost layer. Therefore, in the CH3OH molecule, the hydroxyl (-OH) group is positioned as a whole in the outermost layer, the hydrogen atoms are also in the outermost layer, and the carbon atom (C) has a lower electronegativity than the oxygen atom (O). Consequently, the carbon atom (C) is the central atom.

Step 3: Label electron pairs and determine the molecular skeleton

We place the carbon atom (C) in the centre and connect three hydrogen atoms (H) and one hydroxyl (-OH) group to it via single bonds (i.e. a pair of electrons). The oxygen and hydrogen atoms in the hydroxyl (-OH) group are also connected by a pair of electrons (a single bond).

Step 4: Check whether the atoms satisfy the octet rule

In the above steps, we have used up a total of 10 valence electrons. There are 4 valence electrons remaining. It is known that a hydrogen atom requires only 2 valence electrons to achieve a stable structure, and the carbon atom already has 8 valence electrons in its outermost shell, satisfying the octet rule. However, the oxygen atom has only 4 valence electrons; therefore, the remaining 4 valence electrons are assigned to the oxygen atom (O).

Step 5: Calculating the formal charge

Formal charge = Valence electrons – Non-bonding electrons – (Bonding electrons)/2

In the CH3OH molecule:

The formal charge of the carbon atom (C) = 4-0-8/2 = 0;

The formal charge of the hydrogen atom (H) = 1 – 0 – 2/2 = 0;

The formal charge of the oxygen atom (O) = 6 – 4 – 4/2 = 0

From the above calculation of formal charges, it can be seen that the charges of the carbon atom (C), hydrogen atom (H) and oxygen atom (O) are all zero. This indicates that the Lewis structure of CH3OH described above is stable and requires no modification.

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