Multiple Choice
Draw the Lewis Dot Structure for the following cation:NH4+.
11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
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Determine the Lewis Dot Structure for the following ion:SCl42+.
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Verified step by step guidance1
Identify the central atom in the ion. In SCl4^2+, sulfur (S) is the central atom because it is less electronegative than chlorine (Cl) and can form multiple bonds.
Determine the total number of valence electrons available. Sulfur has 6 valence electrons, and each chlorine has 7 valence electrons. The ion has a 2+ charge, meaning 2 electrons are removed. Calculate the total: 6 + (4 * 7) - 2 = 32 valence electrons.
Place the sulfur atom in the center and arrange the four chlorine atoms around it. Connect each chlorine atom to the sulfur atom with a single bond, using 8 electrons (2 per bond).
Distribute the remaining electrons to complete the octets of the chlorine atoms. Each chlorine needs 6 more electrons to complete its octet, using 24 electrons in total (6 per chlorine).
Check the formal charges to ensure the structure is correct. Sulfur should have a formal charge of 0, and each chlorine should also have a formal charge of 0. Adjust if necessary to minimize formal charges while maintaining the 2+ charge of the ion.
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