D-block

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curry 1E
Posts: 55
Joined: Wed Sep 18, 2019 12:15 am

D-block

Postby curry 1E » Sun Dec 01, 2019 8:22 pm

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

Kimberly Koo 2I
Posts: 99
Joined: Sat Aug 17, 2019 12:17 am

Re: D-block

Postby Kimberly Koo 2I » Sun Dec 01, 2019 9:04 pm

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

Ryan Juncker 3D
Posts: 51
Joined: Wed Sep 18, 2019 12:18 am

Re: D-block

Postby Ryan Juncker 3D » Sun Dec 01, 2019 9:09 pm

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.

Jordan Ziegler 2J
Posts: 59
Joined: Sat Aug 17, 2019 12:15 am

Re: D-block

Postby Jordan Ziegler 2J » Sun Dec 01, 2019 10:19 pm

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
Posts: 117
Joined: Thu Jul 11, 2019 12:15 am

Re: D-block

Postby Hannah Lee 2F » Sun Dec 01, 2019 10:24 pm

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.


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