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i) Give the ionic half equation for the formation of fluoride ions from fluorine gas.
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The answer in the mark scheme is:
F2 + 2e- > 2Fe-
Just wondering if you could do :
F2 > F + 2e-
As in it doesn't accept electrons, it gives them out to form positive ions ?
------------------------------
The answer in the mark scheme is:
F2 + 2e- > 2Fe-
Just wondering if you could do :
F2 > F + 2e-
As in it doesn't accept electrons, it gives them out to form positive ions ?
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#3
The fluoride ion is F- by definition, hence in order to become that from F2, you need to add two electrons (one to each fluorine atom) in order to become F-.
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#6
(Original post by Tulian)
i) Give the ionic half equation for the formation of fluoride ions from fluorine gas.
------------------------------
The answer in the mark scheme is:
F2 + 2e- > 2Fe-
Just wondering if you could do :
F2 > F + 2e-
As in it doesn't accept electrons, it gives them out to form positive ions ?
i) Give the ionic half equation for the formation of fluoride ions from fluorine gas.
------------------------------
The answer in the mark scheme is:
F2 + 2e- > 2Fe-
Just wondering if you could do :
F2 > F + 2e-
As in it doesn't accept electrons, it gives them out to form positive ions ?
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reply
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#7
(Original post by Asad_2015)
The oxidation state of Florine is always -1, therefore it will always gain an electron. Hence you equation is wrong. Plus what you did is not balanced either, Florine is diatomic :s
The oxidation state of Florine is always -1, therefore it will always gain an electron. Hence you equation is wrong. Plus what you did is not balanced either, Florine is diatomic :s
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#8
(Original post by alow)
What's the oxidation state of Fluorine in this compound: F2?
What's the oxidation state of Fluorine in this compound: F2?
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