객관식
Which of the following Lewis dot structures for CO\(_2\) (carbon dioxide) is reasonable for a neutral molecule?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
객관식
Which of the following statements correctly describes the Lewis dot structure of the neutral compound SF_2?
A
Sulfur is the central atom with two double bonds to fluorine atoms and no lone pairs on sulfur.
B
Sulfur is the central atom with one single bond and one double bond to fluorine atoms and one lone pair on sulfur.
C
Sulfur is the central atom with two single bonds to fluorine atoms and two lone pairs on sulfur.
D
Fluorine is the central atom with single bonds to two sulfur atoms.
검증된 단계별 안내1
Step 1: Identify the total number of valence electrons in the molecule SF_2. Sulfur (S) is in group 16 and has 6 valence electrons, and each fluorine (F) atom is in group 17 with 7 valence electrons. Calculate the total by adding these together: \(6 + 2 \times 7\).
Step 2: Determine the central atom. Generally, the less electronegative atom is the central atom. Between sulfur and fluorine, sulfur is less electronegative, so sulfur will be the central atom.
Step 3: Draw single bonds between the central sulfur atom and each fluorine atom. Each single bond represents 2 electrons shared between atoms.
Step 4: Distribute the remaining valence electrons to satisfy the octet rule. Start by completing the octets of the fluorine atoms (each fluorine needs 8 electrons total, including bonding electrons). Then place any leftover electrons as lone pairs on the sulfur atom.
Step 5: Check the formal charges and the octet rule for all atoms. Ensure that sulfur has a complete octet and that the structure has no unnecessary charges. This will confirm that sulfur has two single bonds to fluorine atoms and two lone pairs on sulfur.
