QQuestionChemistry
QuestionChemistry
For OCl^2, provide the Lewis dot structure, shape, polarity of bonds, and whether it is a polar molecule or not.
A. Lewis dot structure, bent, polar bonds, polar molecule
B. Lewis dot structure, bent, nonpolar bonds, nonpolar molecule
C. Lewis dot structure, linear, polar bonds, polar molecule
D. Lewis dot structure, linear, nonpolar bonds, nonpolar molecule
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Answer
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Step 1:I'll solve this step by step using the specified LaTeX formatting guidelines:
Step 2:: Determine the number of valence electrons
- Total valence electrons: $$12 + 14 = 26$$ electrons
- Chlorine (Cl): 7 \times 2 = 14 valence electrons
Step 3:: Draw the Lewis dot structure
- Central oxygen atom with two chlorine atoms - Arrange electrons to satisfy octet rule - Two single bonds between O and Cl atoms - Remaining electrons as lone pairs on oxygen
Step 4:: Determine molecular geometry
- Bond angle will be less than $$109.5^\circ$$ due to lone pair repulsion
- Central oxygen has two bonding pairs and two lone pairs - This results in a BENT molecular geometry
Step 5:: Analyze bond polarity
- Oxygen is more electronegative than chlorine - O-Cl bonds will be polar - Unequal electron distribution creates polar bonds
Step 6:: Determine overall molecular polarity
- Bent geometry - Asymmetric distribution of polar bonds - Lone pairs on oxygen contribute to molecular polarity
Final Answer
Lewis dot structure, bent, polar bonds, polar molecule Key reasoning: - Bent geometry due to lone pairs - Polar O-Cl bonds - Asymmetric structure leads to net molecular polarity
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