Acidic Environment d/p#2 (1 Viewer)

[babydoll_]

I was just wondering if anybody had any notes on this dot point... it can be found here....
In particular i need balanced equations for industrial and natural sources of sulfur dioxide

Thanks

 

[timmii]

-The more metallic an element, the more basic is its oxide.

-The more non-metallic an element, the more acidic is its oxide.
Some common acidic oxides are: CO2, NO2, N2O3, N2o5, SO2, SO3, P2O3, P2o5, Cl2O

The acidic nature of an oxide decreases down group 5. In group 6 oxygen is neutral but sulfur (SO2 and SO3) is acidic. In group 7 all oxides execpt F2O are acidic, and the oxides of chlorine (Cl2) and Cl207) dissolve in water to form strong perchloric acid (HCLO4) which acts as an oxidant.

-Aluminium forms amphoteric oxides (as do zinc, lead, tin)*

*not in syllabus - just a general note

 

[kini mini]

Someone's getting bored in the peaceful USyd forum

Sulphur dioxide is produced industrially in the smelting of iron ore when sulphur impurites react with the oxygen that is piped over the crushed ore. It's only produced naturally in volcanoes I think.

The equation is simply S + O2 ---> SO2 industrially I believe.

Check your textbook for more details, Thickett and others present what timmii said with a diagram as well and will give you more than we mere mortals can remember .