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Lewis Structure of BERYLLIUM OXIDE

Jun 12,2026

Lewis Structure of BeO

BERYLLIUM OXIDE (BeO) is a metal oxide. Its Lewis structure consists of a central beryllium atom (Be) and an outer oxygen atom (O). The beryllium atom (Be) and the oxygen atom (O) are connected by a double bond, and the oxygen atom (O) has two lone pairs of electrons. The specific structural formula is as follows:

Lewis Structure of BERYLLIUM OXIDE

How to Draw the Lewis Structure of BeO

Step 1: Calculate the Total Number of Valence Electrons

In the BeO molecule, the outermost valence electrons of the beryllium atom (Be) and the oxygen atom (O) are 2 and 6 respectively. Therefore, the total number of valence electrons in BeO = 2 + 6 = 8.

Step 2: Determine the Central Atom

In the BeO molecule, the electronegativity of the Be atom is 1.57; the electronegativity of the O atom is 3.44. The electronegativity difference > 1.7, which means that the chemical bond between the Be and O atoms is an ionic bond. However, since the BeO molecule is insoluble in water but soluble in nonpolar solvents, and water is polar, this means that the chemical bond between the Be and O atoms is not an ionic bond but a covalent bond. Furthermore, the Be atom has relatively low electronegativity; therefore, the beryllium atom (Be) is the central atom.

Step 3: Labeling Electrons

We place the beryllium atom (Be) in the center. The oxygen atom (O) and the beryllium atom (Be) are connected by a single bond (one pair of electrons). The remaining three lone pairs of electrons are distributed on the oxygen atom. See the diagram below:

Lewis Structure Electron Marking of BeO

Step 4: Checking the Octet Rule

In the above steps, the oxygen atom has 8 electrons around it, satisfying the octet rule.

Step 5: Calculating Formal Charge

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

In the BeO molecule:

Formal charge of the beryllium atom (Be) = 2 - 0 - 2/2 = +1

Formal charge of the oxygen atom (O) = 6 - 6 - 2/2 = -1

Through the above calculation of formal charge, it can be seen that the formal charges of both the beryllium atom (Be) and the oxygen atom (O) are not zero. This indicates that the Lewis structure of the BeO molecule is unstable. To achieve a stable structure for each atom, a lone pair of electrons must be removed from the outermost oxygen atom. The 2s orbital on the Be atom changes from 2s2 to 2s12p1, forming two half-filled orbitals, which then hybridize with the O atom. This results in a double bond between the Be and O atoms. 

The Formation Process of the Stable Lewis Structure of BeO

At this point, the formal charge of the beryllium atom (Be) is 2 - 0 - 4/2 = 0; the formal charge of the oxygen atom (O) is 6 - 4 - 4/2 = 0. The Lewis structure of the BeO molecule is the most stable. It is important to note that in the Lewis structure of the BeO molecule, the chemical bond between the beryllium atom (Be) and the oxygen atom (O) is a covalent bond, not an ionic bond.

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  • What is beryllium oxide used for? Apr 10, 2024

    Beryllium oxide (BeO) is a white crystalline oxide. It is a well-known prototype refractory oxide with a wide range of applications ranging from optoelectronic devices to nuclear reactors.

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Jun 15,2026API

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  • BERYLLIUM OXIDE
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