Lewis structure of BeH2

Answer 1

It's quite hard to draw and does not follow normal bonding laws but:

H2>B<H2>BH2

The < represents a bond to one H bond above and one below.

There are two types of B - H bonds: where the terminal B-H bonds are standard B:H, and where the middle B-Hs involves 2 centre 3 electron bridging

Answer 2

The Lewis structure of BeH2 would show beryllium in the center with two hydrogen atoms bonded to it, each sharing a pair of electrons. Beryllium would have no lone pairs of electrons and would have a formal charge of 0.

Answer 3

H-Be-H. This is an exception to the octet rule as there are only four electrons around the beryllium atom.

On first principles you would expect BeH2 to be an exception as shown above, and recently gas phase molecular BeH2 has been confirmed to be a linear molecule. However solid BeH2 is normally encountered is amorphous white solid and has a polymeric structure with 3 centre 2 electron bonds, so called banana bonds. These break all the rules we use in drawing Lewis structures. Boron hydrides are similarly electron deficient and also can form these 3 centre banana bonds. This demonstrates that the electron deficient Be and B atoms in the hydrides are able to make use of the electrons that are around in order to get closer to the octet even though they can never achieve it.

Answer 4

H-Be-HMolecule Structure: Linear

Answer 5

The Lewis structure for Be2 is nonexistent. A bond between two Be atoms will not form according to molecular orbital theory.

Answer 6

..
h-se-h
..

Answer 7

See the link below.

Answer 8

H:Be:H

Answer 9

H-b(..)-b