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D-block

Posted: Sun Dec 01, 2019 8:22 pm
by curry 1E
In general, why do d-block elements behave differently than main-group elements?

Re: D-block

Posted: Sun Dec 01, 2019 9:04 pm
by Kimberly Koo 2I
The transition metals in the d-block are more electronegative than the metals in other groups.

Re: D-block

Posted: Sun Dec 01, 2019 9:09 pm
by Ryan Juncker 3D
Kimberly Koo 3C wrote: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.

Re: D-block

Posted: Sun Dec 01, 2019 10:19 pm
by 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.

Re: D-block

Posted: Sun Dec 01, 2019 10:24 pm
by 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.