lewis acid or lewis base? then draw the product.
H3C^+ :NH3 ---->
I'm assuming H3C is the acid and :NH3 is the base? As for drawing out the product I don't know what to do.
Are you sure that it is H3C?
H3C+ yes that's what the problem says
Lewis acids are electron pair acceptors (CH3+), and Lewis bases are electron pair donors (NH4).
thank you. but when the question asks me to draw out the product am I drawing two structures or one?
for instance would i draw something like this? the diagonal lines are suppose to be straight lines.
H-C-H
/
H-N-H
/
H
You forgot an H at the top of the C, but yes.
oh i did. thank you for your responses!
it's wrong you have to put the lone pairs and the charge somewhere you do something with both.
In the given reaction, H3C^+ is a Lewis acid and :NH3 is a Lewis base.
To understand the reaction and draw the product, we need to know that a Lewis acid is a species that accepts an electron pair, while a Lewis base is a species that donates an electron pair.
In this case, the Lewis acid H3C^+ accepts the electron pair from the Lewis base :NH3.
To draw the product, we need to show the transfer of the electron pair from :NH3 to H3C^+.
First, let's focus on the Lewis acid, H3C^+. It is a positively charged species because it has lost one electron.
Second, let's consider the Lewis base, :NH3. It contains a lone pair of electrons that can be donated to the Lewis acid.
When the lone pair from :NH3 donates to H3C^+, the reaction forms a new bond. The H3C^+ gains an additional electron, neutralizing the positive charge, and forming a new bond with the nitrogen atom from :NH3.
So, the product can be represented as:
H3C^+ + :NH3 --> H3C-NH3
In this product, the nitrogen atom becomes positively charged due to the formation of the bond with the carbon atom.