QQuestionChemistry
QuestionChemistry
What is the correct Lewis structure for the sulfur atom?
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I will provide a step-by-step solution to draw the Lewis structure for a sulfur atom.
A sulfur atom has 6 electrons, so we need to follow these steps:
Step 2:
Draw a small dot for each electron around the nucleus, which represents the sulfur atom. We have 6 electrons, so there will be 3 pairs of electrons (2 electrons per pair) and 2 unpaired electrons. Situation after Step 1: • • • • • •
Step 3:
Connect the unpaired electrons with lines to form single covalent bonds. In this case, there are no other atoms to form bonds with, so just leave the unpaired electrons as they are. Situation after Step 2: • • • • • •
Step 4:
Place the remaining electrons (if any) as lone pairs on the central atom. In this case, all the electrons are already placed. Situation after Step 3: • • • • • •
Step 5:
Ensure that the central atom (sulfur in this case) has 8 electrons in its valence shell (either in bonds or as lone pairs). In this case, sulfur has 6 electrons in its valence shell.
Step 6:
If the central atom does not have 8 electrons, check for any nearby atoms to form additional bonds or move electrons around to satisfy the octet rule. However, since this is a single sulfur atom, there are no other atoms to form bonds with. Now, I will present the Lewis structure for the sulfur atom in a more visually appealing format: S: • • • There are 3 lone pairs of electrons around the sulfur atom, and there are no other atoms to share electrons with.
Final Answer
The Lewis structure for a sulfur atom is represented as S with 3 lone pairs of electrons around it.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students