Question

Which metal in the first series of transition metals exhibit +1 oxidation state most frequently and why?

Answer 1

Hint: Metals are those elements which lose electrons to attain a stable electronic configuration. They are good conductors of electricity as they readily lose electrons which can act as charge carriers.
Oxidation state defines the charge present on the metal when it is present in combined state.

Complete Step by step answer: For transition or D-block metals the value of Oxidation state can vary from +1 to +7.
Now in the question it is asked to determine the transition metal of the first series that exhibits +1 oxidation state most frequently.
The first series transition metals and its common oxidation states are given in the following table

Element Name and Symbol	Atomic Number	Most Common oxidation states	Electronic Configuration
Scandium(Sc)	21	+3	$[Ar]4s^23d^1$
Titanium(Ti)	22	+4	$[Ar]4s^23d^2$
Vanadium(V)	23	+2,+3,+4,+5	$[Ar]4s^23d^3$
Chromium(Cr)	24	+2,+3,+6	$[Ar]4s^13d^5$
Manganese(Mn)	25	+2,+3,+4,+6,+7	$[Ar]4s^23d^5$
Iron(Fe)	26	+2,+3	$[Ar]4s^23d^6$
Cobalt(Co)	27	+2,+3	$[Ar]4s^23d^7$
Nickel(Ni)	28	+2	$[Ar]4s^23d^8$
Copper(Cu)	29	+1,+2	$[Ar]4s^13d^{10}$
Zinc(Zn)	30	+2	$[Ar]4s^23d^{10}$

From the following table we can say that Copper(Cu) is the element with +1 oxidation state.
The electronic configuration of Copper(Cu) is $[Ar]4s^13d^{10}$. To achieve the most stable position it have lost one electron and got the status of plus one charge.

Note: It should be noted that Copper exists in +1 oxidation state as it loses one electron from 4s orbital to have fully filled 3d orbital which gives extra stability to $Cu^+$ ions. It must be kept in mind that the liberation of electrons takes place only from those orbitals having the highest energy level.