Draw the Lewis structure for CS
. Where are the electrons found? 2 in single bonds, 8 in double bonds, 6 in lone pairs 0 in single bonds, 8 in double bonds, 8 in lone pairs 8 in single bonds, 8 in double bonds, 0 in lone pairs 4 in single bonds, 4 in double bonds, 8 in lone pairs
The Correct Answer and Explanation is:
Correct answer:
0 in single bonds, 8 in double bonds, 8 in lone pairs
Explanation:
To draw the Lewis structure for carbon monosulfide (CS), we follow a structured approach:
Step 1: Count valence electrons
- Carbon (C) has 4 valence electrons
- Sulfur (S) has 6 valence electrons
- Total: 4 + 6 = 10 valence electrons
Step 2: Choose the central atom
Since there are only two atoms, we place carbon and sulfur next to each other. Carbon is typically the less electronegative atom, so it is placed on the left.
Step 3: Create a single bond
A single bond between C and S uses 2 electrons. That leaves 8 electrons.
Step 4: Complete the octets
Placing lone pairs on each atom to complete their octets with only a single bond will use more electrons than we have, and carbon will not have a full octet. So, we try using multiple bonds.
Step 5: Create a double bond
A double bond uses 4 electrons. With a double bond between carbon and sulfur, each atom can now have a full octet using lone pairs.
Structure:
:C=S:
This structure has:
- One double bond between carbon and sulfur (4 electrons per bond, total of 8 electrons)
- Two lone pairs on sulfur (4 electrons)
- Two lone pairs on carbon (4 electrons)
This accounts for all 10 valence electrons:
- 8 electrons in double bonds
- 8 electrons in lone pairs
- 0 electrons in single bonds
This structure is stable and satisfies the octet rule for both atoms. There is no need for single bonds, and the bonding pattern is similar to that found in carbon monoxide (CO) and other diatomic molecules with multiple bonds. The electrons are mainly found in the double bond and the lone pairs surrounding both atoms.
