QQuestionChemistry
QuestionChemistry
"Draw the Lewis structure of the HOBr molecule (O is central).
a) How many shared pairs are in the molecule?
b) How many electron groups are around the central atom?
c) What is the predicted bond angle in the molecule?
d) What is the shape of this molecule?"
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Answer
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Step 1:I'll solve this Lewis structure problem step by step, following the LaTeX formatting guidelines precisely:
Step 2:: Determine the total number of valence electrons
Total valence electrons: $$1 + 6 + 7 = 14$$ electrons
- Hydrogen (H): 1 valence electron - Oxygen (O): 6 valence electrons - Bromine (Br): 7 valence electrons
Step 3:: Arrange atoms and connect with single bonds
\text{H} - \text{O} - \text{Br}
- Place O in the center - Connect H and Br to O with single bonds - Initial electron distribution:
Step 4:: Distribute remaining electrons as lone pairs
- Actual bond angle slightly less than $$109.5^{\circ}$$ due to lone pair repulsion
- Initial single bonds use 2 electrons - Distribute around O and Br to complete octets - Final Lewis structure shows: - O has two lone pairs - Br has three lone pairs - H has no lone pairs a) Shared Pairs: b) Electron Groups around Central Atom (O): c) Predicted Bond Angle: - With 4 electron groups (2 bonding, 2 lone pairs) - Electron group geometry: Tetrahedral d) Molecular Shape: - Bent molecular shape due to lone pairs on oxygen
Final Answer
a) Shared Pairs: 2 b) Electron Groups: 4 c) Bond Angle: \approx 109.5^{\circ} d) Molecular Shape: Bent
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