LSE_FM300
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In the chemistry text book for my course (OCR Salters B Chemical Ideas) it says (on page 193) that when you heat copper it looses electrons which, when combined with the other hand equation, leads to oxygen in the air gaining those electrons hence a reduction / oxidation reaction ---> Redox.

However, I was taught elsewhere that in order for an atom to loose electrons you need a really high amount of energy, something well beyond infra-red (heat) in terms of frequency, something closer to UV or gamma radiation.

So how can infra-red radiation cause copper to loose electrons, I thought it would simply cause the atoms to vibrate and the bonds to stretch ?

Thanks
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RickHendricks
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(Original post by LSE_FM300)
In the chemistry text book for my course (OCR Salters B Chemical Ideas) it says (on page 193) that when you heat copper it looses electrons which, when combined with the other hand equation, leads to oxygen in the air gaining those electrons hence a reduction / oxidation reaction ---> Redox.

However, I was taught elsewhere that in order for an atom to loose electrons you need a really high amount of energy, something well beyond infra-red (heat) in terms of frequency, something closer to UV or gamma radiation.

So how can infra-red radiation cause copper to loose electrons, I thought it would simply cause the atoms to vibrate and the bonds to stretch ?

Thanks
that's a physics thing.

In chemistry a redox reaction occurs due to higher reactivity of one of the species, which causes it to either gain or lose an electron.

the thing about copper losing electrons is the photoelectric effect.
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