What is the hybridization of the central atom in #NO_3^-#?
To get the answer to this question, you can take the approach of drawing the Lewis structure of
(For clarification, you need to calculate the number of electrons in
Now, to find hybridization, use the following table:
All we have to do now is count the number of bonds between atoms on the Lewis structure, and check the table. In the Lewis structure, you can see
If we refer to the table under "type of hybrid orbital," this is where the hybridization should be. For "number of bonds" =
I hope that helps!
P.S. If you still have trouble understanding how to draw the Lewis structure, just search up "Lewis structure no3-" on YouTube. There are great videos which explain it well. I am sorry if I didn't go in-depth enough.
The common Lewis representation gives a quaternized nitrogen, and thus a formal cationic centre. Two of the oxygen atoms have formal negative charges, whereas one is neutral, and thus a FORMAL negative charge is associated with the ion. And thus we gots.......
The oxygen-nitrogen-oxygen bond angle,