객관식
Which of the following is the correct Lewis structure for SCl2?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
객관식
Which of the following is the correct Lewis structure for OSF4, where sulfur (S) is the central atom and all atoms have a formal charge of zero?
A
S is bonded to one oxygen (O) atom with a single bond and four fluorine (F) atoms with single bonds, with one lone pair on the sulfur.
B
S is bonded to one oxygen (O) atom with a double bond and four fluorine (F) atoms with single bonds, with two lone pairs on the oxygen.
C
S is bonded to one oxygen (O) atom with a double bond and four fluorine (F) atoms with single bonds, with one lone pair on the sulfur.
D
S is bonded to one oxygen (O) atom with a single bond and four fluorine (F) atoms with double bonds, with no lone pairs on the oxygen.
검증된 단계별 안내1
Identify the central atom in the molecule. In OSF4, sulfur (S) is the central atom.
Determine the total number of valence electrons available. Oxygen (O) has 6 valence electrons, sulfur (S) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Calculate the total: 6 (O) + 6 (S) + 4 * 7 (F) = 40 valence electrons.
Arrange the atoms around the central sulfur atom. Connect sulfur to oxygen with a double bond and to each fluorine with a single bond. This uses 2 electrons for the S=O bond and 8 electrons for the S-F bonds (2 electrons per bond).
Distribute the remaining electrons to satisfy the octet rule. Place two lone pairs on the oxygen atom to complete its octet, using 4 electrons. Place one lone pair on the sulfur atom, using 2 electrons.
Verify the formal charges. Calculate the formal charge for each atom using the formula: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). Ensure all atoms have a formal charge of zero.
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