Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: o1ocups on February 22, 2009, 02:17:22 AM
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I know that a Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor. So in this case: CH3NH2(g)+HBr(g) :rarrow: CH3NH4Br(s), HBr is the Lewis acid and the other one is the base, right? But do they have to form a covalent bond at the end?
In this reaction: Al(NO3)3(s)+6H2O(l) :rarrow: Al(H2O)63+(aq)+NO3-(aq), can the reactants still be classified as Lewis acid and base?
I am just not sure if the electron pair donor and the electron pair acceptor have to form a covalent bond.
Thanks!!
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Someone can correct me if I am missing something.
The H forms a covalent bond with the N, but the Br itself is not covalently bonded as it became an ion. Since the CH3NH3 is now a positive ion the bromine likes to hang around unless they are in solution.
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But does the product of Lewis acid and base always contain a covalent bond (even if the bond doesn't include all the elements involved)?
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I have another related question: are all Brønsted-Lowry acids/bases Lewis acids/bases ?
All the examples of Lewis acids/bases that are given in my book have one single product that is the compound of the two reactants bonded by a covalent bond. Is that the standard form of Lewis acid/base reactions?
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But does the product of Lewis acid and base always contain a covalent bond (even if the bond doesn't include all the elements involved)?
In most of the examples I can think of I will say yes, but just because of that don't assume that it is only possible for it to form a covalent bond.
I have another related question: are all Brønsted-Lowry acids/bases Lewis acids/bases ?
All the examples of Lewis acids/bases that are given in my book have one single product that is the compound of the two reactants bonded by a covalent bond. Is that the standard form of Lewis acid/base reactions?
The since a Brønsted-Lowry acid/base involves the transfer of protons(H+) most if not all can be considered Lewis acids. Lewis took it one step further to explain the fact that not all acids or bases have an OH or a H.
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So Brønsted-Lowry acids/bases also form covalent bonds? I thought they are separate ions.
(for example NH3 +H2O ::equil:: NH4+ + OH-, do NH4+ and OH- form covalent bonds?)
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Al(NO3)3(s)+6H2O(l) ::equil:: Al(H2O)63+(aq)+NO3-(aq)
So in this reaction, is Al(NO3)3 the Lewis base since it's the electron-pair donor, and is H2O the Lewis acid because it's the electron-pair acceptor?
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Al(NO3)3(s)+6H2O(l) ::equil:: Al(H2O)63+(aq)+NO3-(aq)
So in this reaction, is Al(NO3)3 the Lewis base since it's the electron-pair donor, and is H2O the Lewis acid because it's the electron-pair acceptor?
Even if they are not stuck together at the product side?
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So Brønsted-Lowry acids/bases also form covalent bonds? I thought they are separate ions.
(for example NH3 +H2O ::equil:: NH4+ + OH-, do NH4+ and OH- form covalent bonds?)
The H itself forms a covalent bond. Any other bonds are usually ionic.