Draw the best Lewis structures for NO+, NO2-, NO2H, and NO3-. Based on the Lewis structures, list all of the the N-O bonds lengths in order of shortest (1) to longest (5).
N-O bond length in >>> 2
N-O double bond in NO2H >>> 1
N-O bond length in NO3- >>> 4
N-O bond length in NO2- >>> 3
N-O single bond in NO2H >>> 5
Does the order in N-O bond lengths predicted by Lewis agree with those computed in WebMO?
>>> what I answered was no, because in NO2H the bond lengths are the same
I've changed my answer for part one to
a) N-O bond length in >>> 4
b) N-O double bond in NO2H >>> 1
c) N-O bond length in NO3- >>> 2
d) N-O bond length in NO2- >>> 3
e) N-O single bond in NO2H >>> 5
To draw the Lewis structures for the given molecules, you need to determine the number of valence electrons for each atom. Here's how you can do it:
1. NO+:
- Nitrogen (N) is in Group 5 of the periodic table, so it has 5 valence electrons.
- Oxygen (O) is in Group 6 and has 6 valence electrons.
- Since there is a positive charge on NO+, subtract one electron from the total valence electrons: 5 + 6 - 1 = 10.
- Place the electrons around the atoms, starting with a single bond between N and O, and then distribute the remaining electrons as lone pairs:
O
|
N–O
2. NO2-:
- Nitrogen (N) still has 5 valence electrons.
- Oxygen (O) now has 6 valence electrons, but since there is a negative charge, add one electron to the total valence electrons: 5 + 6 + 1 = 12.
- Start with a single bond between N and one O atom. Distribute the remaining electrons as lone pairs and make sure all atoms have a full octet, except for the nitrogen atom, which can accept additional electrons:
O
|
N=O
- As there is one extra electron in this structure, place it as a lone pair on the nitrogen atom:
O
|
N=O:
|
:
3. NO2H:
- Nitrogen (N) still has 5 valence electrons.
- Oxygen (O) still has 6 valence electrons.
- Hydrogen (H) has 1 valence electron.
- Add up the valence electrons: 5 + 6 + 1 = 12.
- Start with a double bond between N and O, and distribute the remaining electrons as lone pairs:
O
||
N=O
- Since there are two hydrogens, connect them to the nitrogen atom with single bonds and distribute the remaining electrons:
O
||
N=O
| |
H H
4. NO3-:
- Nitrogen (N) has 5 valence electrons.
- Oxygen (O) has 6 valence electrons.
- Add up the valence electrons: 5 + (3 * 6) + 1 = 24.
- Start with a single bond between N and one O atom, then distribute the remaining electrons as lone pairs and make sure all atoms have a full octet:
O
|
N=O
- As there is a negative charge, add one electron as a lone pair on one of the oxygen atoms:
O
||O
N=O:
To determine the order of N-O bond lengths, observe the Lewis structures. The bond lengths can be ordered from shortest to longest as follows:
1. N-O double bond in NO2H
2. N-O bond length in NO+
3. N-O bond length in NO2-
4. N-O bond length in NO3-
5. N-O single bond in NO2H
However, it's important to note that the predictions of bond lengths based solely on Lewis structures might not always agree with those computed in software programs like WebMO. The actual bond lengths can be affected by factors such as resonance, bond polarity, and molecular geometry.