Write electronic configuration of the element with atomic number 35. what will be the stable oxidation states of the element?

Explanation

Electronic configuration: `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)4s^(2)4p^(5)`.
Most stable oxidation state is -1 because it can accept one electron to achieve inert gas configuration `(1s^(2). . . .3d^(10)4s^(2)4p^(6))`. Again in excited state, it can also exhibit oxidation number +3 or +5 by forming covalent bond by using its 3 or 5 odd-electrons in its outermost shell.