A metal ion with a net + 3 charge has five electrons in the 3d shell. Identify the metal.

Answer: the metal is Iron (Fe)

Explanation: The original electronic configuration of Fe is 1s2 2s2 2p6 3s2 3p6 3d6 4s2

Because it has no charge. The electronic configuration will change from the original because the metal has a charge of + 3, Fe is element number 26 on the periodic table b ut with the + 3 charge, the element number will change to 23 i. e 26 - (+3) = 23

The configuration for Fe3 + is 1s2 2s2 2p6 3s2 3p6 3d5, it automatically had 5 electron in 3d shell

Answer: The given metal is iron.

Explanation:

We are given:

The electrons in 3d-shell = 5

When the metal is present in a transition series (here it is present in first transition series), the removal of valence electron takes place from '4s' shell first and then from '3d' shell

Electronic configuration is defined as the representation of electrons around the nucleus of an atom.

Number of electrons in an atom is determined by the atomic number of that atom.

Inner shell electrons for the given element = 18

Total number of electrons in the ion = 18 + 5 = 23

We are given:

Charge on the ion = + 3

To calculate the number of electrons, we use the equation:

Number of electrons = Atomic number - charge

Atomic number = 23 + 3 = 26

The element having atomic number '26' is iron

Hence, the given metal is iron.