Why oxides are easier to reduce

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Cancel Notify me. Aryan 13 Points. Oxygen is more electronegative than sulphur and will quickly accept electrons and get reduced easily. Bonds formed in oxides are weaker than bonds in sulphides hence oxide bonds are easy to break. Other Related Questions on Physical Chemistry. How does a oxidation reaction involves gain of Electronegative Element and loss of Electropositive Please make me understand this problem not able to View all Questions ».

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And why is copper an exception? The concentrated ore must be converted into a form which is suitable for reduction.

Usually the sulphide ore is converted to oxide before reduction. Oxides are easier to reduce. Thus isolation of metals from concentrated ore involves two major steps viz. Coal is still abundant on our planet. Try to pull that with a sulfide! In the unlikely case if it will, you'll have to deal with the byproduct.

Copper is less active, so instead of going via oxide, we have a chance to go straight to the metal in one step. Would be stupid not to use it. Then there is aluminum which is not reduced like that, but then again, we don't convert it from sulfide to oxide either, primarily because we don't have much sulfide around. Should it be otherwise, it isn't immediately clear would we choose to convert it or not.

Sign up to join this community. The best answers are voted up and rise to the top. Stack Overflow for Teams — Collaborate and share knowledge with a private group. Create a free Team What is Teams? Learn more. Why are the sulfide ores generally converted to an oxide and then reduced? Asked 3 years, 4 months ago. Active 6 months ago. Viewed 5k times.