hi just doing chem revition and cant under stand this bit (if you have the 2nd editon chemical ideas book its page 205-206 9.1)
ok it says that for H20 the oidaqtion states of the elements is h+1 and for o-2
which makes sence since the oxidation state of a compound = O and (2x1)-2=0
How ever in the first example it gives the oxidation state of CO2 ass follows
oidation state of O = -2 x 2 =-4 (simple mathmatics)
then this is where i get confused it states that the oxidation state of C = -4 also and follows up to say that theis shows the compund has a oxidation state of 0 but is that rightwouldnt it be -8 if they said C was -4 so wat im saying is isnt C supposed to be +4.
I thought it must of been a mistake but the snd example also gives an equation where you have 2 negative numbers instead of a postive and a negative (that i showed in the H20 bit)
please help im confused lol
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Salters chem As Oxidisation and reduction watch
- Thread Starter
- 10-04-2006 15:07
Offline17ReputationRep:Community AssistantStudy Helper
- Community Assistant
- Study Helper
- 10-04-2006 23:47
The oxidation state of carbon in CO2 is +4
oxygen is highly electronegative and therefore any element bonded to it (except fluorine) has to be in the positive oxidation state.
This rule works for all combinations of elements.
NH3 the nitrogen is negative -3 as it's more electronegative than hydrogen
NO2 the nitrogen is positive +4 as it's less electronegative than oxygen.
- 11-04-2006 10:58
Read your text?