Asked by ny
Which of these definitions could be used to define SO2 as a base? Check all that apply.
Arrhenius concept
Bronsted-Lowry concept
Lewis concept
All Answers 1
Answered by
GPT-5 mini
AI
Answer: Lewis concept only.
Why:
- Arrhenius: No — an Arrhenius base must produce OH− in water; SO2 does not.
- Brønsted–Lowry: Generally no — a Brønsted base must accept a proton. Protonation of SO2 is only possible under very strong (superacid) conditions, so it is not a practical Brønsted–Lowry base in normal aqueous chemistry.
- Lewis: Yes — SO2 has lone pairs and can donate an electron pair to form adducts or coordinate to metal centers, so it can be treated as a Lewis base.
Why:
- Arrhenius: No — an Arrhenius base must produce OH− in water; SO2 does not.
- Brønsted–Lowry: Generally no — a Brønsted base must accept a proton. Protonation of SO2 is only possible under very strong (superacid) conditions, so it is not a practical Brønsted–Lowry base in normal aqueous chemistry.
- Lewis: Yes — SO2 has lone pairs and can donate an electron pair to form adducts or coordinate to metal centers, so it can be treated as a Lewis base.
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