why are metals easily oxidized and non metals not?
Answers
An easy example for a non-metal would be hydrogen.
If hydrogen reacts with a metal, like sodium, it forms sodium hydride by gaining electrons from sodium. The oxidation state of hydrogen changes from 0 to -1. That's a reduction.
If hydrogen reacts with non-metals which are more electronegative than itself…example chlorine, forming hydrogen chloride; here the oxidation state of hydrogen changes from 0 to +1. That's an oxidation.
For metals in the element state, they would normally lose electrons to react…therefore be oxidised to positive ions. However, if we are talking about metallic ions, then we can have a variety of reactions here…specially if we are looking at the transition metal cations.
For example, we have iron which can easily to be oxidised from the +2 to +3 oxidation state, and also reduced from +3 to +2
Answer:
There is a clear pattern in the chemistry of the main group metals: The main group metals are oxidized in all of their chemical reactions. These metals are oxidized when they react with nonmetal elements. ... When these elements react, the electrons are drawn toward the more electronegative oxygen atoms.
Explanation:
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