Final answer:
CH2O has a trigonal planar geometry with a bond angle of about 120 degrees and is a polar molecule due to the polar C=O bond.
Step-by-step explanation:
To answer the question regarding the compound CH2O, we start by drawing its Lewis structure, determining the VSEPR formula, assessing the electron pair geometry, establishing the molecular shape, looking at the bond angle, and evaluating the polarity of the molecule.
The Lewis structure for CH2O has carbon at the center with double bonds to oxygen and single bonds to each hydrogen. There are no lone pairs on carbon, giving it a VSEPR formula of AX3 where 'A' represents the central atom and 'X' represents surrounding atoms. The electron pair geometry is trigonal planar. Its molecular shape also remains trigonal planar due to the absence of lone pairs affecting the shape. The bond angles within this geometry are approximately 120 degrees. Concerning polarity, CH2O is a polar molecule because the C=O bond is polar and the overall geometry does not cancel out this polarity.