Questions: What are the angles (a) and (b) in the actual molecule of which this is a Lewis structure? Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. (a =) square degrees (b =) square degrees

What are the angles (a) and (b) in the actual molecule of which this is a Lewis structure? Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. (a =) square degrees (b =) square degrees
Transcript text: What are the angles $a$ and $b$ in the actual molecule of which this is a Lewis structure? Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. \[ \begin{aligned} a & =\square^{\circ} \\ b & =\square^{\circ} \end{aligned} \]
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Solution

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Solution Steps

Step 1: Identify the molecular geometry

The molecule in question is H₂C=N⁻. To determine the bond angles, we need to identify the molecular geometry around the central atoms (carbon and nitrogen).

Step 2: Determine the hybridization of the central atoms
  • The carbon atom is bonded to two hydrogen atoms and has a double bond with nitrogen, making it sp² hybridized.
  • The nitrogen atom has a double bond with carbon and a lone pair, making it sp² hybridized.
Step 3: Predict the bond angles based on hybridization
  • For sp² hybridized atoms, the ideal bond angle is approximately 120°.

Final Answer

  • Angle \( a \) (H-C-H) is approximately 120°.
  • Angle \( b \) (C-N) is approximately 120°.
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