Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
Choose the best lewis structure for NO3-
Answer Choices in the attached picture
![**Choose the best Lewis structure for NO₃⁻.**
1. The first diagram shows the nitrogen (N) atom at the center with one double-bonded oxygen (O) and two single-bonded oxygens, each carrying a negative formal charge. All atoms comply with the octet rule.
```
[::O::−N=O ↔ ::O::]
|
[::O::]
```
2. The second diagram displays the nitrogen (N) atom at the center double-bonded with two oxygens (O) and one single-bonded oxygen, which has a negative formal charge.
```
[O=N=O]
|
[O-]
```
3. The third diagram illustrates the nitrogen (N) atom at the center double-bonded with one oxygen (O) and single-bonded with two oxygens, both carrying negative formal charges.
```
[::O::−N=O ↔ ::O::]
|
[O-]
```
4. The fourth diagram presents the nitrogen (N) atom at the center single-bonded to three oxygens (O), and each oxygen exhibits a set of lone pairs completing the octet configuration. One of the bonds appears to be a resonance structure.
```
[O]−
/ \
N O]
| |
[O]− [O]
```
5. The fifth diagram displays the nitrogen (N) atom at the center double-bonded with one oxygen (O) and single-bonded with two oxygens, each carrying a negative formal charge.
```
[O=N=O]
|
[O-]
```
**Explanation:**
Each diagram is an attempt to represent the Lewis structure of the nitrate ion, NO₃⁻. The ideal structure typically considers resonance forms and formal charges to showcase the most stable configuration of electrons around the atoms involved.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bbf8297-dba5-4b47-a922-55444acdea37%2F6237bd98-548f-488c-9531-574d72791018%2Fgesv4_processed.png&w=3840&q=75)
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