QQuestionChemistry
QuestionChemistry
Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of ClO^3−. If multiple resonance structures exist, use one that does not involve an expanded valence.
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Step 1:: Draw the Lewis structure for ClO^3−, starting with the central atom (Cl).
Place three O atoms around the Cl atom, ensuring each O atom has a single bond with the Cl atom.
Step 2:: Add remaining valence electrons to complete the octet for each O atom.
O has 6 valence electrons, so add 3 electrons to each O atom (6 in total, since one electron is used in the single bond with Cl).
Step 3:: Add the remaining valence electrons to the central atom (Cl).
Cl has 7 valence electrons, so add the remaining 4 electrons to Cl.
Step 4:: Calculate the formal charge for each atom.
For each atom, subtract the number of valence electrons from the group number, add the number of bonds, and subtract the lone pair electrons. - For each O atom: (6 - 6) + 2 - 4 = - 2 - For the Cl atom: (7 - 7) + 6 - 0 = + 6 - 1 (for the - 1 charge on the ion) = + 5
Step 5:: The Lewis structure for ClO^3− with the given conditions is:
Cl—O—O | O
Step 6:: The formal charge for the central atom (Cl) is + 5.
Final Answer
The Lewis structure for ClO^3− is: Cl—O—O | O The formal charge for the central atom (Cl) is + 5.
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