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Draw the Lewis Dot Structure for the radical hydroxide, OH.
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10. Chemical Bonding
Lewis Dot Structures: Exceptions (Simplified)
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Determine the Lewis Dot Structure for the following compound:SOCl2
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Identify the central atom in the compound SOCl2. Sulfur (S) is typically the central atom because it can form multiple bonds and has a lower electronegativity compared to oxygen (O) and chlorine (Cl).
Determine the total number of valence electrons available. Sulfur has 6 valence electrons, oxygen has 6, and each chlorine has 7. Therefore, the total is 6 (S) + 6 (O) + 7 (Cl) + 7 (Cl) = 26 valence electrons.
Arrange the atoms around the central sulfur atom. Typically, oxygen will form a double bond with sulfur, and each chlorine will form a single bond with sulfur.
Distribute the remaining valence electrons to satisfy the octet rule for each atom. Start by placing electrons around the outer atoms (O and Cl) to complete their octets, then place any remaining electrons on the central atom (S).
Check the formal charges to ensure the most stable structure. The formal charge is calculated as: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). Adjust the structure if necessary to minimize formal charges across the molecule.
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