Draw the Lewis structure of HCN and then choose the appropriate formal charges for each of the atoms. H-C=N Click to edit molecule A) H = 0, C = 0, N = 0 B) H=0, C = -1, N = +1 C) H = 0, C = 0, N = -1 D) H = 0, C = 0, N = +1 E) H=+1, C = 0, N = -1

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**Educational Resource: Understanding Lewis Structures and Formal Charges**

---

**Activity: Drawing the Lewis Structure of HCN**

**Task:**
1. Draw the Lewis structure of HCN.
2. Choose the appropriate formal charges for each of the atoms in the molecule.

**Diagram:**

The diagram provided shows the Lewis structure of Hydrogen Cyanide (HCN):

```
H — C ≡ N
```
In this Lewis structure:
- Hydrogen (H) forms a single bond with Carbon (C).
- Carbon (C) forms a triple bond with Nitrogen (N).

**Options:**

You are provided with several options to select the correct formal charges for the atoms in HCN:

A) H = 0, C = 0, N = 0

B) H = 0, C = -1, N = +1

C) H = 0, C = 0, N = -1

D) H = 0, C = 0, N = +1

E) H = +1, C = 0, N = -1

---

**Instructions:**

Review the Lewis structure and consider the rules for calculating formal charges. Determine the correct set of formal charges for Hydrogen (H), Carbon (C), and Nitrogen (N) in the HCN molecule.

_Tap here or pull up for additional resources_

---

**Note:**
- Formal charge is calculated as follows:
\[ \text{Formal Charge} = (\text{Number of Valence Electrons}) - (\text{Number of Non-Bonding Electrons}) - \frac{(\text{Number of Bonding Electrons})}{2} \]
Transcribed Image Text:**Educational Resource: Understanding Lewis Structures and Formal Charges** --- **Activity: Drawing the Lewis Structure of HCN** **Task:** 1. Draw the Lewis structure of HCN. 2. Choose the appropriate formal charges for each of the atoms in the molecule. **Diagram:** The diagram provided shows the Lewis structure of Hydrogen Cyanide (HCN): ``` H — C ≡ N ``` In this Lewis structure: - Hydrogen (H) forms a single bond with Carbon (C). - Carbon (C) forms a triple bond with Nitrogen (N). **Options:** You are provided with several options to select the correct formal charges for the atoms in HCN: A) H = 0, C = 0, N = 0 B) H = 0, C = -1, N = +1 C) H = 0, C = 0, N = -1 D) H = 0, C = 0, N = +1 E) H = +1, C = 0, N = -1 --- **Instructions:** Review the Lewis structure and consider the rules for calculating formal charges. Determine the correct set of formal charges for Hydrogen (H), Carbon (C), and Nitrogen (N) in the HCN molecule. _Tap here or pull up for additional resources_ --- **Note:** - Formal charge is calculated as follows: \[ \text{Formal Charge} = (\text{Number of Valence Electrons}) - (\text{Number of Non-Bonding Electrons}) - \frac{(\text{Number of Bonding Electrons})}{2} \]
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