VIPSolutionsAct like a helpful tutor and exlain me : Give step-by-step solution with explanation and final answer: Where do formal charges need to be added? (+ or -)7 :0 I Cc VERN H H
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Act like a helpful tutor and exlain me :
Give step-by-step solution with explanation and final answer:
Where do formal charges need to be added? (+ or -)
7
:0
I
Cc
VERN
H H
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Asked by: Sagar
Created at: 2025-09-23 03:50:30
Asked by: Sagar
Created at: 2025-09-23 03:50:30
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# Step-by-Step Solution: Assigning Formal Charges
Let's determine where formal charges (positive or negative) should be added in the given molecule.
## 1. **Understanding the Structure**
The structure shown is for **formaldehyde hydrate** (methanediol), but the connectivity and bonding look like a resonance structure of formic acid or its conjugate base. Focus on the carbon center double-bonded to O, single bonded to OH, and two single bonds to H.
## 2. **Assigning Lone Pairs**
- The oxygen with a single bond to H has **2 lone pairs**.
- The carbon is making 4 bonds (2 to H, 1 to O, 1 to OH).
- The double-bonded oxygen has **2 lone pairs**.
## 3. **Count Valence Electrons for Each Atom:**
- **Carbon (C):** 4 valence electrons
- **Oxygen (O):** 6 valence electrons
- **Hydrogen (H):** 1 valence electron
## 4. **Calculate Formal Charge (FC)**
The formula is:
\[
\text{Formal Charge} = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{1}{2} \times \text{Bonding electrons}
\]
### **A. Double-Bonded Oxygen (top O)**
- Valence electrons = 6
- Non-bonding electrons = 4 (2 lone pairs)
- Bonding electrons = 4 (2 bonds to C)
\[
FC = 6 - 4 - \frac{1}{2}(4) = 6 - 4 - 2 = 0
\]
**No formal charge.**
### **B. Single-Bonded Oxygen (OH group)**
- Valence electrons = 6
- Non-bonding electrons = 4 (2 lone pairs)
- Bonding electrons = 4 (2 bonds: 1 to C, 1 to H)
\[
FC = 6 - 4 - \frac{1}{2}(4) = 6 - 4 - 2 = 0
\]
**No formal charge.**
### **C. Carbon (C)**
- Valence electrons = 4
- Non-bonding electrons = 0
- Bonding electrons = 8 (4 bonds)
\[
FC = 4 - 0 - \frac{1}{2}(8) = 4 - 0 - 4 = 0
\]
**No formal charge.**
### **D. Hydrogens**
- Valence electrons = 1
- Non-bonding electrons = 0
- Bonding electrons = 2 (each forms 1 bond)
\[
FC = 1 - 0 - \frac{1}{2}(2) = 1 - 1 = 0
\]
**No formal charge.**
---
## **Final Answer**
**There are no formal charges (+ or −) needed on any atom in this structure.**
- All atoms have a formal charge of zero.
---
### **Summary Table:**
| Atom | Formal Charge |
|-------|--------------|
| O (double bond) | 0 |
| O (single bond to H) | 0 |
| C | 0 |
| H | 0 |
**No formal charges need to be added to this structure.**
---
**If you have any further questions or want to see a case where formal charges do appear, just ask!**
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