D-block

[curry 1E]

In general, why do d-block elements behave differently than main-group elements?

[Kimberly Koo 2I]

The transition metals in the d-block are more electronegative than the metals in other groups.

[Ryan Juncker 3D]

The transition metals in the d-block are more electronegative than the metals in other groups.

I'm not sure that this is necessarily true. While they do behave differently I believe that Fluorine and other elements nearing the top right of the periodic table (minus group 18) are more electronegative than d-block elements. As far as behavior in bonding, it is worth noting that the d-block elements can all expand their octets. While of course other elements can do this as well the expanded octet affects behavior.

[Jordan Ziegler 2J]

It's not that d-block elements are more electronegative. Because transition elements more easily form differing order cations, they are stronger Lewis acids and will form coordinate covalent bonds more easily.

[Hannah Lee 2F]

D-block elements can experience multiple oxidation states since they may have incomplete inner subshells that do not restrict valence e- to the outer shell. They are also a good source of e- due to their ability to form expanded octets, and they can form complexes via coordinate covalent bonds with ligands.