Draw the Lewis structure of the hypochlorite ion, including lone pairs.

Question

CramX · Accepted Answer

Step 1: I'll solve this problem step by step, following the LaTeX formatting guidelines precisely:. Step 2: : Determine the total number of valence electrons. - Chlorine (Cl) has 7 valence electrons - Oxygen (O) has 6 valence electrons - The ion has a -1 charge, which adds 1 additional electron Step 3: : Arrange atoms in the structure. - Place the chlorine atom in the center - Attach the oxygen atom to the chlorine with a single bond Step 4: : Distribute electrons as bonds and lone pairs. - Single bond between Cl and O uses 2 electrons - Remaining electrons will be distributed as lone pairs Step 5: : Complete the octet for oxygen. - Oxygen needs 8 electrons - Place 3 lone pairs around oxygen (6 electrons) 	ext{Oxygen's electrons:} \ 1 	ext{ bond (2 electrons)} + 3 	ext{ lone pairs (6 electrons)} = 8 	ext{ electrons} \end{array}$ Step 6: : Complete the octet for chlorine. - Chlorine needs 8 electrons - Place 3 lone pairs around chlorine 	ext{Chlorine's electrons:} \ 1 	ext{ bond (2 electrons)} + 3 	ext{ lone pairs (6 electrons)} = 8 	ext{ electrons} \end{array}$ Final Lewis Structure: 	ext{Hypochlorite Ion (ClO}^{-}	ext{):} \ 	ext{Cl} 	ext{ has three lone pairs} \ 	ext{O has three lone pairs} \ 	ext{Single bond between Cl and O} \end{array}$ Final Answer: The Lewis structure of the hypochlorite ion (ClO⁻) consists of a chlorine atom single-bonded to an oxygen atom, with three lone pairs on the chlorine and three lone pairs on the oxygen, satisfying the octet rule for both atoms.

Q
QuestionChemistry

Answer

Full Solution Locked

Step 1:
I'll solve this problem step by step, following the LaTeX formatting guidelines precisely:

Step 2:
: Determine the total number of valence electrons

Step 3:
: Arrange atoms in the structure

Final Answer

Need Help with Homework?

Related Questions

Company

Explore

Study Tools

QQuestionChemistry

AnswerHelpful