I read this in a textbook -

Bi(V) is very unstable and is a good oxidizing agent

Why does it happen that way? Is it because in $\pu{+5}$ oxidation state $\ce{Bi}$ pulls in more electrons and hence gets reduced fast or there's a different concept?

Also then $\ce{BiCl5}$ should be more stable than $\ce{BiCl3}$ because it's getting the electrons that it needs, which is not true.

I read this in a textbook:

$\ce{Bi(V)}$ is very unstable and is a good oxidizing agent.

Why does it happen that way? Is it because in $\pu{+5}$ oxidation state $\ce{Bi}$ pulls in more electrons and hence gets reduced fast or there's a different concept?

Also then $\ce{BiCl5}$ should be more stable than $\ce{BiCl3}$ because it's getting the electrons that it needs, which is not true.

I read this in a textbook -

Bi(V) is very unstable and is a good oxidizing agent

Why does it happen that way? Is it because in +5 oxidation state Bi pulls in more electrons and hence gets reduced fast or there's a different concept?

Also then BiCl5 should be more stable than BiCl3 because it's getting the electrons that it needs, which is not true.

I read this in a textbook -

Bi(V) is very unstable and is a good oxidizing agent

Why does it happen that way? Is it because in $\pu{+5}$ oxidation state $\ce{Bi}$ pulls in more electrons and hence gets reduced fast or there's a different concept?

Also then $\ce{BiCl5}$ should be more stable than $\ce{BiCl3}$ because it's getting the electrons that it needs, which is not true.