Lewis structure

Lewis structure of BeCl₂

16 valence electrons. Two Be-Cl single bonds, with no lone pair on Be, so Be has only 4 electrons around it.

Molecule or ion

BeCl₂Beryllium chloride

Linear

AB₂: 2 bond pairs, no lone pairs

i

In the solid it forms chains; the linear molecule is the vapour.

16 valence electrons

i

Be has only four electrons around it, an incomplete octet.

Formal charges: none

Be has 2 valence electrons. It uses two in two single bonds to Cl, so none are left over.
Steric number = two sigma bonds + no lone pairs = 2, so Be is sp hybridised.
Two electron pairs point in opposite directions, along a line (linear electron geometry). With no lone pairs the atoms take the same shape: linear.
All the bond pairs repel each other equally, so the angle is the ideal 180°.
The bond dipoles cancel in the symmetric linear shape, so BeCl₂ is non-polar.

Working

How to draw it

Count the valence electrons: Be 2 + 2 × Cl 7 = 16 valence electrons, 8 pairs.
Put Be in the middle and join it to the two outer atoms with single bonds.
Give each outer atom lone pairs until it has an octet (H needs only two electrons), then put any electrons left over on the central atom.
Result: two Be-Cl single bonds, with no lone pair on Be, so Be has only 4 electrons around it.
Formal charge = valence electrons − lone pair electrons − number of bonds. Here: none.

Class 11, Chapter 4 Chemical Bonding and Molecular Structure.

Questions

How many valence electrons are in BeCl2?

Be 2 + 2 × Cl 7 = 16 valence electrons, 8 pairs.

What are the formal charges in the Lewis structure of BeCl2?

Every atom has a formal charge of zero.

How many lone pairs are in the Lewis structure of BeCl2?

6 in all, none on the central Be.