Catalysts and Inorganic Compound Reactions
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| What are the two types of Catalyst? | Heterogenous and Homogenous.
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| What is a Heterogenous Catalyst: | A Catalyst which is in the a different phase to the reactants, usually a solid providing a surface for a reaction to occur.
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| What is a Homogenous Catalyst? | A Catalyst which is in the same phase as the reactants. They form reactive intermediates before being regenerated.
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| Give 3 Examples of Heterogenous Catalysts in industrial processes: | Iron in the Harbour Process. V2O5 (Vanadium Oxide) in the Contact process. Chromium Oxide (Cr2O3) in the production of Methanol via Synthesis Gas.
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| Explain the Contact Process and the role of its Catalyst: | 2SO2 + O2 <---> 2SO3
V2O5 + SO2 --> SO3 + V2O4
2 V2O4 + O2 ---> 2 V2O5
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| What is the Catalyst for the Harbour Process: | Fe
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| What is the Catalyst for the Contact Process: | V2O5
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| What is the Catalyst for production of Methanol? | Cr2O3
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| What are the 2+ ions which are covered in this unit: | Fe2+, Cu2+ and Co+ (Iron (II), Copper (II) and Cobalt (II))
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| What are the 3+ ions covered in this unit: | Fe3+, Cr3+ and Al3+ (Iron (III), Chromium (III) and Aluminium (III)).
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| Lewis Base: | An electron Pair Donor
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| Lewis Acid: | Electron Pair acceptor.
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| Which are stronger Acids, 2+ or 3+ ions: | The 3+ ions are stronger because they draw charge density from lone pairs towards themselves more and this leaves H atoms more delta positive than in 2+ ions.
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| Give as basic Formula of a M2+ ion in solution: | [M(H2O)6]2+
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| Give the basic formula of a M+ ion in solution: | [M(H2O)6]3+
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