Draw the Lewis structure for the CH2O molecule

/ Exams & Certification / By


Draw the Lewis structure for the CH2O molecule: Based on this structure_ the number of polar bonds and non-polar bonds is 01) 3 polar bonds and no non-polar bonds 2) 2 polar bonds and non ~polar bond polar bonds and 2 non-polar bonds no polar bonds and 3 non-polar bonds 2 polar bonds and 2 non- polar bonds

The Correct Answer and Explanation is:

To determine the number of polar and non-polar bonds in the CH2O molecule (formaldehyde), we must first look at its Lewis structure and analyze the bonds.

Step 1: Draw the Lewis Structure of CH2O

  1. Count Valence Electrons:
    • Carbon (C): 4 valence electrons
    • Hydrogen (H): 2 × 1 = 2 valence electrons
    • Oxygen (O): 6 valence electrons
    Total valence electrons = 4 + 2 + 6 = 12 electrons.
  2. Place the Atoms:
    • Carbon is the central atom because it is less electronegative than oxygen and can form multiple bonds.
    • Oxygen is double-bonded to carbon, and each hydrogen is single-bonded to carbon.
  3. Distribute Electrons:
    • Carbon will form two single bonds with two hydrogens and one double bond with oxygen.
    • Oxygen will use 4 of its valence electrons to form the double bond with carbon and will have two lone pairs.
    The structure looks like this: mathematicaCopyEdit H | H-C=O In this structure:
    • Carbon (C) has 4 electrons: two single bonds to hydrogen and one double bond to oxygen.
    • Oxygen (O) has 6 electrons: 4 are involved in the double bond with carbon, and the remaining 2 are lone pairs.

Step 2: Analyze the Bond Polarity

Now, let’s look at the polarity of the bonds:

  1. Carbon-Hydrogen Bonds (C-H):
    • The C-H bond is non-polar because carbon and hydrogen have very similar electronegativities.
  2. Carbon-Oxygen Bond (C=O):
    • The C=O bond is polar because oxygen is more electronegative than carbon, creating a dipole where oxygen has a partial negative charge (δ-) and carbon has a partial positive charge (δ+).

Step 3: Conclusion

In the CH2O molecule:

  • There are 2 non-polar bonds (C-H).
  • There is 1 polar bond (C=O).

Thus, the correct answer is:

  • 2 polar bonds and 1 non-polar bond.

This means the molecule contains both polar and non-polar bonds, and the number of polar bonds is greater than the non-polar ones.

The overall polarity of the molecule is determined by the fact that the C=O bond introduces a dipole, making the CH2O molecule polar overall. However, this question only focuses on the individual bond types.

Related Posts

Scroll to Top