QQuestionAnatomy and Physiology
QuestionAnatomy and Physiology
Draw the Lewis structure of SF₂ showing all lone pairs.
What is the hybridization of the central atom?
- sp
- sp²
- sp³
- sp³d
- sp³d²
An SF₂ molecule is
- polar.
- nonpolar.
Identify the molecular geometry of SF₂.
- trigonal bipyramidal
- bent
- tetrahedral
- square planar
- square pyramidal
- trigonal pyramidal
- T-shaped
- linear
- trigonal planar
- see-saw
- octahedral
What is the approximate bond angle in SF₂?
- 90 degrees
- 105 degrees
- 120 degrees
- 180 degrees
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Answer
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Step 1: Draw the Lewis structure of SF₂
To draw the Lewis structure of SF₂, we first need to determine the total number of valence electrons. A sulfur atom (S) has 6 valence electrons, and each fluorine atom (F) has 7 valence electrons. Since there are two fluorine atoms, the total number of valence electrons is: \text{Total valence electrons} = 6\ (\text{S}) + 2 \times 7\ (\text{F}) = 20 Now, let's distribute these electrons around the atoms. Sulfur is the central atom, and it shares one electron with each fluorine atom, forming two single bonds. This uses up 4 of the valence electrons. The remaining 16 electrons will be placed as lone pairs on the fluorine atoms and the sulfur atom to complete their octets: \chemfig{S(-[:150]F)(-[:210]F)}
Step 2: Determine the hybridization of the central atom
The hybridization of the central atom can be determined by counting the number of electron domains (σ bonds and lone pairs) around it. In this case, sulfur has two σ bonds and one lone pair, resulting in a total of 3 electron domains. The hybridization of the central atom is sp²: \text{Hybridization} = \boxed{\text{sp}^2}
Final Answer
1. Lewis structure: \chemfig{S(-[:150]F)(-[:210]F)} 2. Hybridization: sp² 3. Polarity: nonpolar 4. Molecular geometry: bent 5. Approximate bond angle: 105 degrees
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