Q
QuestionChemistry

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}

Step 3:
: Determine the polarity and molecular geometry of SF₂

Since sulfur and fluorine have similar electronegativity values, the dipole moments of the two S-F bonds cancel each other out, making the SF₂ molecule nonpolar: \text{Polarity} = \boxed{\text{nonpolar}} The molecular geometry of SF₂ can be determined by considering the number of electron domains around the central atom. With 3 electron domains, the molecular geometry is bent: \text{Molecular geometry} = \boxed{\text{bent}}

Step 4:
: Calculate the approximate bond angle in SF₂

The ideal bond angle for a bent molecular geometry with sp² hybridization is 120 degrees. However, the lone pair on the sulfur atom occupies more space than the bonding electrons, causing the bond angle to be slightly smaller. The approximate bond angle in SF₂ is: \text{Bond angle} \approx \boxed{105\ degree}

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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Q
QuestionChemistry

Answer

Full Solution Locked

Step 1:
: Draw the Lewis structure of SF₂

Step 2:
: Determine the hybridization of the central atom

Step 3:
: Determine the polarity and molecular geometry of SF₂

Step 4:
: Calculate the approximate bond angle in SF₂

Final Answer

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QQuestionChemistry

AnswerHelpful

Full Solution Locked

Step 1:: Draw the Lewis structure of SF₂

Step 2:: Determine the hybridization of the central atom

Step 3:: Determine the polarity and molecular geometry of SF₂

Step 4:: Calculate the approximate bond angle in SF₂

Final Answer

Need Help with Homework?

Related Questions

Q
QuestionChemistry

Answer

Step 1:
: Draw the Lewis structure of SF₂

Step 2:
: Determine the hybridization of the central atom

Step 3:
: Determine the polarity and molecular geometry of SF₂

Step 4:
: Calculate the approximate bond angle in SF₂