Problem: Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2? A) That would give positive formal charges bo the chlorine atoms and a negative formal charge to the beryllium atom.B) There aren't enough electrons. C) That would result in more than eight electrons around beryllium. D) That would result in more than eight electrons around each chlorine atom. E) That would result in the formal charges not adding up to zero.

FREE Expert Solution

For BeCl2Be (E.N. 1.5) is less electronegative than Cl (E.N. 3.0) → Be is the central atom


          Group             Valence Electrons

Be        2A                   1 × 2 e2 e

Cl         7A                   2 × 7 e14 e

         Total: 16 valence e


  • halogen → form only one bond when not a central atom; preferred to form an octet.

The Lewis structure for BeCl2 is:

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Problem Details

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2

A) That would give positive formal charges bo the chlorine atoms and a negative formal charge to the beryllium atom.

B) There aren't enough electrons. 

C) That would result in more than eight electrons around beryllium. 

D) That would result in more than eight electrons around each chlorine atom. 

E) That would result in the formal charges not adding up to zero.

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