Multiple Choice
Determine the Lewis Dot Structure for the following ion:SCl42+.
10. Chemical Bonding
Lewis Dot Structures: Ions (Simplified)
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Determine the Lewis Dot Structure for the following ion:O22–.
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Verified step by step guidance1
Identify the total number of valence electrons available for the ion O₂²⁻. Each oxygen atom has 6 valence electrons, and the ion has an additional 2 electrons due to the 2- charge, giving a total of 14 valence electrons.
Determine the basic structure of the ion. Since there are two oxygen atoms, they will be connected by a bond. Start by placing a single bond between the two oxygen atoms.
Distribute the remaining valence electrons around the oxygen atoms to satisfy the octet rule. Each oxygen atom should have 8 electrons around it, including those in bonds.
Consider the possibility of multiple bonds if necessary to satisfy the octet rule for both oxygen atoms. If a single bond does not satisfy the octet rule, try a double bond.
Verify the formal charges on each atom to ensure the most stable structure. The formal charge is calculated using the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (Bonding Electrons/2). Adjust the structure if needed to minimize formal charges.
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