Question

Complete the Lewis dot structure for H₂CO (in which both H atoms are bonded to C). Complete the molecule by connecting carbon and oxygen with the appropriate bond. Include all lone pairs of electrons.

Answer 1

The Lewis dot structure for H₂CO involves a central carbon atom bonded to two hydrogen atoms and one oxygen atom. The structure includes lone pairs of electrons on the oxygen atom. The Lewis structure is O-C-H-H.

Step-by-step explanation:

The Lewis dot structure for H₂CO can be determined using the following steps:

1. Identify the central atom, which is carbon (C).
2. Determine the total number of valence electrons in the molecule. Carbon has 4 valence electrons, oxygen (O) has 6 valence electrons, and each hydrogen (H) has 1 valence electron, for a total of 12 valence electrons.
3. Place a single bond between carbon and each hydrogen atom, using 2 valence electrons.
4. Distribute the remaining 8 valence electrons as lone pairs around the oxygen atom, with 3 lone pairs in total.
5. If the central atom has fewer than 8 valence electrons, use a lone pair from an adjacent atom to form a double bond. In this case, one of the lone pairs from oxygen can form a double bond with carbon, resulting in the final Lewis structure for H₂CO.

The Lewis structure is:

O
|
C
| \
H H

This structure shows that carbon (C) is bonded to two hydrogen atoms (H) and one oxygen atom (O), with each atom having the appropriate number of valence electrons.