객관식
Draw the Lewis Dot Structure for the following cation:NH4+.
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
객관식
Determine the Lewis Dot Structure for the following ion: SCl42+.
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검증된 단계별 안내1
Step 1: Determine the total number of valence electrons for the SCl4 ion with a 2+ charge. Sulfur (S) has 6 valence electrons, each chlorine (Cl) has 7 valence electrons, and there are 4 chlorine atoms. Since the ion has a 2+ charge, subtract 2 electrons from the total count. So, total valence electrons = 6 + (4 × 7) - 2.
Step 2: Draw the skeletal structure with sulfur as the central atom bonded to four chlorine atoms. Connect each chlorine atom to sulfur with a single bond initially.
Step 3: Distribute the remaining valence electrons as lone pairs around the chlorine atoms to complete their octets. Each chlorine should have three lone pairs (6 electrons) after bonding.
Step 4: Place any leftover electrons on the central sulfur atom. Since sulfur can expand its octet, it can accommodate more than 8 electrons if needed.
Step 5: Check the formal charges on each atom to ensure the overall charge of the ion is +2. Adjust bonding (single or double bonds) if necessary to minimize formal charges and achieve the correct charge on the ion.
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