Draw plausible Lewis structures for the following species;...

Draw plausible Lewis structures for the following species; use expanded valence shells where necessary. (a) $\mathrm{Cl}_{2} \mathrm{O} ;$ (b) $\mathrm{PF}_{3} ;$ (c) $\mathrm{CO}_{3}^{2-} ;$ (d) $\mathrm{BrF}_{5}$.

Key Concepts

Formal Charges

Calculating formal charges involves comparing the number of electrons an atom ‘owns’ in the Lewis structure relative to its neutral state. Minimizing formal charges across the structure helps in identifying the most stable arrangement of electrons.

Valence Electrons

This concept involves counting the total number of electrons available for bonding by summing the valence electrons of all atoms involved, including adjustments for ionic charges. It forms the foundation for determining how electrons can be distributed among atoms in a molecule or ion.

Octet Rule and Expanded Octet

The octet rule is a guiding principle stating that atoms tend to form bonds until they are surrounded by eight electrons. For atoms in the third period or below, the possibility of an expanded octet exists, where atoms accommodate more than eight electrons by utilizing vacant d orbitals, thus influencing the structure of molecules with such atoms.

Bonding and Electron Pair Arrangement

This concept encompasses the assignment of electrons as bonding pairs or lone pairs around atoms. Determining how atoms share electrons through various bonds (single, double, triple) ensures that the resulting Lewis structure reflects the stable electron configuration of the molecule.

Resonance Structures

In cases where multiple valid electron arrangements exist, resonance structures are used to represent the delocalization of electrons. These multiple Lewis representations describe a molecule or ion, with the actual structure being a hybrid of the various resonance forms.

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