Questions: What are the angles (a) and (b) in the actual molecule of which this is a Lewis structure?

What are the angles (a) and (b) in the actual molecule of which this is a Lewis structure?
Transcript text: What are the angles $a$ and $b$ in the actual molecule of which this is a Lewis structure?
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Solution

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Solution Steps

Step 1: Identify the Molecular Geometry

The molecule in question is formaldehyde (CH2O). The central atom is carbon, which is bonded to two hydrogen atoms and one oxygen atom. The oxygen atom has two lone pairs of electrons.

Step 2: Determine the Electron Geometry

The electron geometry around the carbon atom is determined by the regions of electron density. There are three regions of electron density (two C-H bonds and one C=O double bond), which corresponds to a trigonal planar electron geometry.

Step 3: Determine the Ideal Bond Angles

In a trigonal planar geometry, the ideal bond angles are 120 degrees. This means that the angles around the carbon atom should ideally be 120 degrees.

Final Answer

  • Angle \( a \) (H-C-H): 120 degrees
  • Angle \( b \) (H-C=O): 120 degrees
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