Answer
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Step 1:: Determine the total number of valence electrons in the molecule.
Hydrogen (H) has 1 valence electron, carbon (C) has 4, and nitrogen (N) has 5. The total number of valence electrons in HCN is therefore: \text{Total valence electrons} = 1 + 4 + 5 = 10 \ \text{valence electrons}
Step 2:: Draw a skeletal structure of the molecule.
The skeletal structure of HCN consists of a triple bond between carbon and nitrogen, with hydrogen attached to carbon: ```lua H - C - N ```
Step 3:: Place the remaining valence electrons as lone pairs on the more electronegative atoms.
In HCN, nitrogen is more electronegative than carbon. Therefore, we place the remaining valence electrons as lone pairs on nitrogen: ```lua H - C - N: : ```
Step 4:: Distribute the lone pairs to achieve an octet for each atom.
Carbon and nitrogen both have an octet in this structure. Therefore, we do not need to redistribute any lone pairs.
Step 5:: Check for formal charges.
In this structure, nitrogen has 5 valence electrons (5 from lone pairs) and carbon has 4 (4 from the triple bond). Hydrogen has 1 valence electron (from the single bond). The formal charges for each atom are: All atoms have a formal charge of 0, so the Lewis structure is valid.
Final Answer
The Lewis structure of HCN is: ```lua H - C - N: : ``` with no formal charges.
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