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.
Determine the formal charge of nitrogen in the structure shown here:
SEE PIC
| 0 |
| +1 |
| −−1 |
| +2 |
![### Determining the Formal Charge of Nitrogen
In the given structure, we are asked to determine the formal charge of the nitrogen atom. The structure provided is as follows:
```
H
|
H - C - O - C ≡ N:
|
H
```
### Answer Choices:
- 0
- +1
- −1
- +2
### Explanation of the Structure:
The structure consists of a molecule with:
- A central carbon atom (C) bonded to three hydrogen atoms (H).
- An oxygen atom (O) bonded to the central carbon via a single bond and has two lone pairs of electrons.
- A carbon atom (C) triple-bonded to a nitrogen atom (N), where the nitrogen atom has one set of lone pair electrons.
To determine the formal charge on the nitrogen atom, we use the formula:
\[
\text{Formal Charge} = \text{Valence Electrons} - \left( \frac{\text{Bonding Electrons}}{2} + \text{Non-Bonding Electrons} \right)
\]
For nitrogen:
- Nitrogen has 5 valence electrons.
- In this structure, nitrogen forms 3 bonds (triple bond to carbon), so it shares 6 bonding electrons.
- It has 2 non-bonding electrons (one lone pair).
Applying the formula:
\[
\text{Formal Charge on N} = 5 - \left( \frac{6}{2} + 2 \right) = 5 - (3 + 2) = 5 - 5 = 0
\]
Thus, the formal charge of nitrogen in this structure is **0**.
### Test Your Understanding
Select the correct formal charge for the nitrogen atom in the structure shown:
- ⬤ 0
- ◯ +1
- ◯ −1
- ◯ +2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e9bc902-5aae-4660-a256-c76a2ed5e4a1%2F99fa9433-fada-4f29-a7a2-b60830540e9a%2Fnmq14c9_processed.png&w=3840&q=75)
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