Moderators: Chem_Mod, Chem_Admin

Posts: 111
Joined: Fri Oct 02, 2020 12:17 am


Postby reva_bajjuri » Thu Dec 03, 2020 5:27 pm

could someone explain why cyanide cannot form two coordinate covalent bonds? prof. lavelle said that in the lecture from last week

Stuti Pradhan 2J
Posts: 159
Joined: Wed Sep 30, 2020 9:32 pm
Been upvoted: 5 times

Re: cyanide

Postby Stuti Pradhan 2J » Thu Dec 03, 2020 7:25 pm

Cyanide does have 2 lone pairs, but since it has a triple bond and is linear, the molecule cannot orient itself in a way the both lone pairs bond to the same transition metal.

To have a polydentate ligand, you need at least two lone pairs and at least one spacer between the two lone pairs. Cyanide does not have a spacer atom and it also has a triple bond which is very strong and not flexible, so it cannot bend or orient in any way to bond twice with one TM.

Hope this helps!

Maaria Abdel-Moneim 2G
Posts: 112
Joined: Wed Sep 30, 2020 10:09 pm

Re: cyanide

Postby Maaria Abdel-Moneim 2G » Thu Dec 03, 2020 8:55 pm

Because cyanide has a triple bond it cannot orient in a way where both lone pairs can bond to the transition metal. In order for something to be polydentate it has to be able to orient where each lone pair can bond easily.

Posts: 93
Joined: Wed Sep 30, 2020 9:55 pm

Re: cyanide

Postby Sara_Lim_2C » Thu Dec 03, 2020 9:07 pm

Cyanide doesn't have spacer atom(s) that allow the lone pairs on either side of the linear atom to bond to the transition metal. Because of that, only one of the lone pairs can bond to the transition metal.

Return to “Coordinate Covalent Bonds”

Who is online

Users browsing this forum: No registered users and 1 guest