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.
![### Lewis Structure and Formal Charge
#### Question:
Draw the best Lewis structure for CO₂ and determine the formal charge on carbon.
#### Options:
- 0 (Radio button)
- +2 (Radio button)
- -1 (Radio button)
- +3 (Radio button)
- -4 (Radio button)
#### Explanation:
To solve this problem, follow these steps:
1. **Draw the Lewis Structure for CO₂:**
- Carbon (C) is the central atom and forms double bonds with each oxygen (O) atom.
- Each double bond consists of two pairs of electrons (4 electrons).
- Each oxygen atom will have two lone pairs of electrons remaining.
- The structure can be represented as: O=C=O.
2. **Calculate the Formal Charge:**
- Formal charge (FC) is calculated using the formula:
\[
\text{FC} = (\text{valence electrons}) - (\text{non-bonding electrons}) - \frac{(\text{bonding electrons})}{2}
\]
- For Carbon in CO₂:
- Valence electrons of Carbon: 4
- Non-bonding electrons on Carbon: 0
- Bonding electrons around Carbon: 8 (from the two double bonds)
\[
\text{FC} = 4 - 0 - \frac{8}{2} = 4 - 4 = 0
\]
Therefore, the formal charge on the carbon atom in the best Lewis structure of CO₂ is 0.
#### Answer:
Select the "0" radio button as the correct option for the formal charge on carbon in the best Lewis structure for CO₂.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc7df924-6a52-4175-b6ea-9e20e03510e5%2F7508a0f2-6720-4a77-adde-610b272608ef%2Fpsj3hz_processed.png&w=3840&q=75)
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