Draw the Lewis structures of N2H4, N2H2, and N2.Draw the molecules by placing atoms on the grid and connecting them with bonds.
Include all lone pairs of electrons and hydrogen atoms.View Available Hint(s)
1 answer:
Answer:
The structures are shown below
Explanation:
To draw the Lewis structure, we must place the central atom with its valence electrons surrounded by the other atoms, with their valence electrons, then, using lines, we put the bonds (simple line for 1 pair sharing, a double line for 2 pairs sharing, and triple line for 3 pairs sharing).
For N₂H₄, the two nitrogens are bonded together and with two hydrogens, Nitrogen has 5 valence electrons, and hydrogen 1 valence electron, so, 3 bonds will be done by nitrogen, so there will one lone pair in the structure for each nitrogen, and none for hydrogen. The structure is shown below.
For the N₂H₂, the nitrogens are bonded together, sharing two pairs of electrons, and are each one is bonded to a hydrogen, sharing one pair of electrons. Both nitrogen, then, has one lone pair of electron. The structure is shown below.
For the N₂, the two nitrogens are sharing three pairs of electrons, and both have one lone pair of electron. The structure is shown below.
You might be interested in
Answer:
See explanation and image attached
Explanation:
Here attached are resonance forms of pyrrole and pyridine. The images were obtained from quora and researchgate respectively.
Now, we can see that in the resonance forms of pyrrole, the nitrogen atom in the heterocycle has a formal charge of +1. However, in the six membered pyridine hetrocycle, the nitrogen atom may have a formal charge of -1 or +1 as shown in the canonical structures attached. The structures in which nitrogen has a +1 formal charge in pyridine are comparable to structures obtained from pyrrole. These structures have less contribution to the structure of pyridine.
