acids and bases

Moderators: Chem_Mod, Chem_Admin

Posts: 10
Joined: Fri Sep 25, 2015 3:00 am

acids and bases

Postby 504655187 » Tue Oct 27, 2015 1:03 am

I'm confused on the section of lewis acids and bases. how to we differentiate molecules as either acids or bases?

Posts: 37
Joined: Fri Sep 25, 2015 3:00 am

Re: acids and bases

Postby KarenaKaing_1D » Tue Oct 27, 2015 11:51 am

BASES donate a proton while ACIDS accept a proton
Last edited by KarenaKaing_1D on Sat Oct 31, 2015 11:16 am, edited 1 time in total.

Silvia Gomez 4K
Posts: 13
Joined: Fri Sep 25, 2015 3:00 am

Re: acids and bases

Postby Silvia Gomez 4K » Thu Oct 29, 2015 7:14 pm

A Lewis acid acts as the "acceptor" while the Lewis base acts as the "donator" when forming a coordinate covalent bond. The thing that is being "accepted" or "donated" is electrons because even though this type of reaction has a specific name, we are still dealing with the valence shell of the molecule and/or atoms and the whole purpose of this is to create a coordinate covalent bond instead of a simple covalent bond. So, let's take for example the acid and base reaction between Boron Trifluoride and Fluorine. When looking at the Lewis structure of each one, you can see that in the structure for Boron Trifluoride, Boron needs one pair of electrons to form it's octet. Fluorine alone has seven electrons and is more than willing to form a coordinate covalent bond in order to form it's octet. In this acid and base reaction, the "acceptor" is Boron Trifluoride because this molecule is the one that is gaining the pair of electrons from the "donor", Fluorine. The reactions forms tetrafluoroborate anion (negative because the formal charge for Boron in this newly formed structure is -1).

Return to “Bond Lengths & Energies”

Who is online

Users browsing this forum: No registered users and 1 guest