Numford
Hybridisation

Hybridisation of BeCl₂

Be is sp hybridised (hybridization by the VSEPR count): 2 sigma bonds and no lone pairs give a linear shape, bond angle 180°.

ClBeCl
  • Be
  • Cl

BeCl₂Beryllium chloride

Linear

AB₂: 2 bond pairs, no lone pairs

i

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

  • Hybridisationsp
  • Bond angle180°
  • Polaritynon-polar

Why this shape

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

Lewis structure

16 valence electrons
i

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

BeClCl

Formal charges: none

Working

Why this hybridisation and shape

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

Class 11, Chapter 4 Chemical Bonding and Molecular Structure.

Questions

Hybridisation of BeCl2: quick answers

What is the hybridisation of BeCl2?

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.

What is the shape of BeCl2 and its bond angle?

Linear, with a bond angle of 180 degrees. 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°.

Is BeCl2 polar or non-polar?

Non-polar. The bond dipoles cancel in the symmetric linear shape, so BeCl₂ is non-polar.

Try any molecule