The common oxidation state of transition metals in the d-block is +2, as they often lose two electrons from their outermost shell.

Chromium (Cr) has the electron configuration [Ar] 3d5 4s1 due to stability of half-filled d-orbitals.

The presence of d-electrons allows transition metals to exhibit variable oxidation states.

Copper (Cu) is known for its excellent electrical conductivity.

Nickel (Ni) is commonly used in making various alloys due to its strength and corrosion resistance.

Neodymium (Nd) is a lanthanide element, while the others belong to different series.

Uranium is an f-block element as it is part of the actinides series.

Copper (Cu) is known for forming complex ions due to its ability to coordinate with ligands.

Platinum (Pt) is widely known for its catalytic properties in various chemical reactions.

Uranium is commonly used in the production of nuclear reactors due to its fissile properties.

Mn2+ has a d5 configuration as it loses two electrons from its 4s and 3d orbitals.

Transition metals are commonly used as catalysts in various chemical reactions.

Neodymium (Nd) is a member of the lanthanide series.

Transition metals generally have high density, not low density.

Neodymium (Nd) and Plutonium (Pu) are both f-block elements.

Lanthanum (La) and Cerium (Ce) are both f-block elements, belonging to the lanthanide series.

Iron (Fe) has the electron configuration [Ar] 3d6 4s2.

Tungsten (W) has the highest melting point among transition metals.

Cobalt commonly forms complex ions with a coordination number of 6, such as in [Co(NH3)6]3+.

Iron is used as a catalyst in the Haber process for ammonia synthesis.