Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. b. CO₃^2– c. ClO^– d. NO₂^–

Verified step by step guidance

1. Identify the total number of valence electrons for each molecule or ion. For CO_3^{2-}, sum the valence electrons of carbon, oxygen, and the extra electrons from the charge. Repeat for ClO^- and NO_2^-.
2. Draw a skeletal structure for each molecule or ion, connecting atoms with single bonds. Typically, the least electronegative atom is the central atom.
3. Distribute the remaining valence electrons as lone pairs to complete the octet for each atom, starting with the outer atoms. Adjust for any extra electrons due to negative charges.
4. If any atom lacks an octet, consider forming double or triple bonds by converting lone pairs from adjacent atoms into bonding pairs. Check for possible resonance structures by moving electrons to form equivalent structures.
5. Calculate the formal charge for each atom using the formula: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons). Adjust structures to minimize formal charges, ensuring the most stable configuration.