With the exception of BeH
2, your counting of valence electrons is way off. It would help if you can explain how you are counting them. Remember, only the outer shell is involved in bonding.
I will give you an example, SF
6.
Sulfur has 6 valence electrons.
Fluorine has 7.
There are 6 bonds at the S centre. If you draw a Lewis dot and cross diagram (see below, try it), you will see that each of these 6 electrons shares with a F atom, and each F atom shares on of its electrons with S, to form a covalent bond. In SF
6, each F atom had 7 electrons and shares one more from S to give a total of 8 - so the F atoms satisfy the octet rule. However, S had 6 electrons and shares one more from each of the 6 F atoms to give a total of 12 - the S atom does not satisfy the octet rule.
Have a go yourself with the compounds in the list you posted.