In this seciton, we will be contrasting the properties of transition elements with calcium.

Properties covered:
- melting point
- density
- atomic radius
- ionic radius
- first ionisation energy
- conductivity with calcium

Melting point of transition metals VS Calcium

Melting point of transition metals tends to be higher than calcium and other s-block metals due to the presence of delocalized electrons in the d and s orbitals. The greater number of delocalized electrons in transition elements as compared to calcium leads to stronger metallic bonds being formed. For example the valence shell of calcium ion has 4s2 configuration. However, the 3d54s1 electronic configuration for Chromium ( Cr) in the first series of transition metals is more stable and so produces stronger bonds than the 4s2 electronic configuration in calcium.

Therefore, more heat energy is required to break the metallic bonds in transition metals than calcium leading to higher melting points.

Atomic radii and density of transition metals VS Calcium
Densities of transition metals are much greater than densities of s-block metals like calcium. There is a gradual increase in the densities of transition metals from scandium (2.99g/cm^3) to copper (8.92g/cm^3). The greater densities of transition metals as compared to typical s-block metals s are due to their smaller atomic radii coupled with the greater atomic masses. For example, the density of calcium is 1.6g/cm^3.

As density is calculated by dividing the atomic mass of the metals by their atomic radii, transition metals consequently have higher densities than the s-block metals like calcium.

Ionic radius

First ionisation energy

The first ionisation energy is the energy required to remove the most loosely held electron from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+.All elements have a first ionisation energy

Conductivity of transition metals VS calcium

The delocalized electrons in a metal acts as as mobile charge carriers. Transition metals have electrons in at least the d orbital. While calcium only has electrons until the S orbital because of its electronic configuration(1s2 2s2 2p6 3s2 3p6 4s2 ).

As transition metals have more delocalized electons( mobile charge carriers) than calcium, they have a higher electrical conductivity than calcium.