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The image displays a multiple-choice question asking whether the given Lewis structures satisfy the octet rule.

### 1st Structure: Nitrogen (N), Oxygen (O), and Chlorine (Cl)
- **Lewis Structure:** \( N = O - Cl \) with lone pairs shown.
  - **Nitrogen (N)**: Has 5 valence electrons, needs 8.
  - **Oxygen (O)**: Has 6 valence electrons, needs 8.
  - **Chlorine (Cl)**: Has 7 valence electrons, needs 8.
- **Analysis**: 
  - Nitrogen has a double bond to oxygen and a single bond to chlorine, which gives nitrogen 7 electrons (1 short).
  - Chlorine satisfies the octet rule.
  - Oxygen satisfies the octet rule.
  
  **Answer**: "No, it has the right number of valence electrons but doesn't satisfy the octet rule." 
  - The problem atom is **N**.

### 2nd Structure: Dichloromethane (Cl-C-Cl) with Oxygen attached
- **Lewis Structure:** \( O \) single-bonded to \( C \), which is also single-bonded to two \( Cl \) atoms.
  - **Carbon (C)**: Has 4 valence electrons, needs 8.
  - **Oxygen (O)**: Has 6 valence electrons, needs 8.
  - **Chlorine (Cl)**: Each has 7 valence electrons, needs 8.
- **Analysis**:
  - Carbon has only 6 electrons (short of 8).
  - Oxygen and Chlorine satisfy the octet rule.

  **Answer**: "No, it has the right number of valence electrons but doesn't satisfy the octet rule."
  - The problem atom is **C**.

### 3rd Structure: Hydrogen Cyanide (HCN)
- **Lewis Structure:** \( H - C \equiv N \).
  - **Hydrogen (H)**: Has 1 valence electron, needs 2 (exception to the octet rule).
  - **Carbon (C)**: Has 4 valence electrons, needs 8.
  - **Nitrogen (N)**: Has 5 valence electrons, needs 8.
- **Analysis**:
  - Carbon has a triple bond with nitrogen and a single bond with hydrogen, satisfying the octet rule.
  - Nitrogen satisfies the octet rule.
  - Hydrogen satisfies its duet requirement.

  **Answer**: "Yes," because all atoms satisfy the octet rule (or duet rule for hydrogen).

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### Related Questions:
1. What is the significance of the octet rule in Lewis structures?
2. How do exceptions to the octet rule apply to molecules like HCN?
3. Can expanded octets occur in structures involving elements like chlorine or sulfur?
4. What are common violations of the octet rule seen in molecules?
5. How do resonance structures affect the octet rule in molecules like ozone (O3)?

**Tip**: Always count both lone pairs and bonds when assessing whether an atom satisfies the octet rule.

Deciding whether a Lewis structure satisfies the octet rule for N=O-Cl, O-C-Cl2, and H-C≡N.

Evaluate the Lewis structures of molecules such as N=O-Cl, O-C-Cl2, and H-C≡N to check if they satisfy the octet rule. Understand common exceptions and violations in molecular bonding.

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