Describe the differences between the properties of first row transition metals and other transition metals.

First row transition metals have smaller atomic radii and higher electronegativities than other transition metals.

The first row transition metals (scandium, titanium, vanadium, chromium, manganese, iron, cobalt, and nickel) have smaller atomic radii and higher electronegativities than other transition metals. This is due to the increased nuclear charge in the first row, which attracts the electrons more strongly and results in a smaller atomic radius. The higher electronegativity also means that these elements are more likely to form covalent bonds.

In terms of their chemical properties, the first row transition metals have a greater tendency to form compounds with a +2 oxidation state, whereas the other transition metals can form a wider range of oxidation states. This is due to the smaller size of the first row transition metals, which makes it easier for them to lose two electrons and form a stable cation.

The first row transition metals also have lower melting and boiling points than other transition metals. This is due to the weaker metallic bonding in these elements, which is a result of their smaller size and higher electronegativity. The first row transition metals also tend to have lower densities than other transition metals, again due to their smaller size.

Overall, the first row transition metals have some distinct differences in their properties compared to other transition metals. These differences are largely due to their smaller size and higher electronegativity, which affect their atomic and chemical properties.