Question

What are transition elements? Write the names and electronic configuration of the elements of the first transition series. Transition metals and their maximum compounds are paramagnetic. Explain.

Hint:

The presence of unpaired electrons in transition metals’ d-orbitals makes them paramagnetic.

Answer 1

Step 1: Definition of Transition Elements.
Transition elements are the elements found in the d-block of the periodic table. They are characterized by having partially filled d-orbitals in at least one of their oxidation states. These elements tend to form colored compounds, exhibit variable oxidation states, and are often good conductors of electricity.
Step 2: Electronic Configuration of the First Transition Series.
The elements of the first transition series are from Scandium (Sc) to Zinc (Zn). Their electronic configurations are as follows: - Scandium (Sc): [Ar] 3d\(^1\) 4s\(^2\) - Titanium (Ti): [Ar] 3d\(^2\) 4s\(^2\) - Vanadium (V): [Ar] 3d\(^3\) 4s\(^2\) - Chromium (Cr): [Ar] 3d\(^5\) 4s\(^1\) - Manganese (Mn): [Ar] 3d\(^5\) 4s\(^2\) - Iron (Fe): [Ar] 3d\(^6\) 4s\(^2\) - Cobalt (Co): [Ar] 3d\(^7\) 4s\(^2\) - Nickel (Ni): [Ar] 3d\(^8\) 4s\(^2\) - Copper (Cu): [Ar] 3d\(^9\) 4s\(^1\) - Zinc (Zn): [Ar] 3d\(^1\) 4s\(^2\)
Step 3: Paramagnetism of Transition Metals.
Transition metals are often paramagnetic because they have unpaired electrons in their d-orbitals, which make them attracted to an external magnetic field. The paramagnetism in transition metals is due to the presence of these unpaired electrons in the metal's electronic configuration. The number of unpaired electrons determines the strength of the paramagnetism.