Transcribed image text: The Lewis structure of nitrous acid (HNO2) is shown below. =a. What is the formal charge for each atom in this structure? H N O (1) O (2)
The correct answer and explanation is:
Formal Charges in the Lewis Structure of Nitrous Acid (HNO₂)
To determine the formal charges on each atom in HNO₂, we use the formula: Formal Charge=Valence Electrons−Nonbonding Electrons−Bonding Electrons2\text{Formal Charge} = \text{Valence Electrons} – \text{Nonbonding Electrons} – \frac{\text{Bonding Electrons}}{2}
Step 1: Draw the Lewis Structure of HNO₂
- Hydrogen (H) has 1 valence electron and forms one single bond with oxygen.
- Nitrogen (N) has 5 valence electrons and forms one single bond with oxygen and one double bond with another oxygen.
- Oxygen (O1, single bonded to H and N) has 6 valence electrons.
- Oxygen (O2, double bonded to N) has 6 valence electrons.
The correct Lewis structure follows the octet rule and minimizes formal charges.
Step 2: Calculate the Formal Charges
- Hydrogen (H)
- Valence electrons: 1
- Nonbonding electrons: 0
- Bonding electrons: 2
- Formal Charge: 1 – 0 – (2/2) = 0
- Nitrogen (N)
- Valence electrons: 5
- Nonbonding electrons: 0
- Bonding electrons: 8 (2 single + 1 double bond)
- Formal Charge: 5 – 0 – (8/2) = 5 – 4 = +1
- Oxygen (O1) – Single bonded to H and N
- Valence electrons: 6
- Nonbonding electrons: 6
- Bonding electrons: 2
- Formal Charge: 6 – 6 – (2/2) = 6 – 6 – 1 = -1
- Oxygen (O2) – Double bonded to N
- Valence electrons: 6
- Nonbonding electrons: 4
- Bonding electrons: 4
- Formal Charge: 6 – 4 – (4/2) = 6 – 4 – 2 = 0
Final Formal Charges:
- H = 0
- N = +1
- O1 (Single bonded to H and N) = -1
- O2 (Double bonded to N) = 0
Thus, the overall charge of HNO₂ is neutral because the sum of formal charges equals zero.
Now, I’ll generate an image of the correct Lewis structure.
Here is the Lewis structure of nitrous acid (HNO₂) with formal charges labeled. Let me know if you need any modifications or further explanations!
