Add lone pairs where needed to give octets and determine the shape around each indicated atom. If no lone pairs need to be added, please check the box below.
HCOCH
Shape around the bold red C atom and blue O
To determine the shape around the bold red C atom and the blue O atom, we need to draw the Lewis structure of HCOCH and determine if any of the atoms need additional lone pairs to achieve an octet.
HCOCH:
H - C - O - C - H
First, we calculate the total number of valence electrons:
1 (H) + 4 (C) + 6 (O) + 1 (C) + 1 (H) = 13 valence electrons
Next, we arrange the atoms in a way that satisfies the octet rule:
H - C - O - C - H
Now, we need to check if any of the atoms require additional lone pairs to complete an octet.
The bold red C atom already has four bonds, so it does not need any additional lone pairs.
The blue O atom already has two bonds and two lone pairs, so it has an octet.
Therefore, no lone pairs need to be added to any atom in HCOCH.
The shape around the bold red C atom can be determined as trigonal planar, with a bond angle of approximately 120 degrees.
The shape around the blue O atom can be determined as bent or V-shaped, with a bond angle of less than 120 degrees.