I don't really understand the concept of organic oxidations.

[LogicX]

So let's say a hydrogen is replaced with an oxygen. Apparently this is an oxidation. But I just don't see any transfer of electrons going on. All the atoms still have the same number of valence electrons. Can someone give me an example of a simple organic oxidation and explain the electron transfer that is changing the oxidation states of the atoms? I can understand inorganic oxidations like Cr 3+ going to Cr 6+, I just can't wrap my mind around organic redox.

 

[chemisttree]

If you change the groups around a carbon with more electronegative ones, that is considered oxidation in the organic sense.

Consider the following ranking from lowest oxidation state to largest:

CH4<CH3O<CH2O2<CO2

CH3S<CH3O

CH2O2(geminal diol)<CH2O2(formic acid) The geminal diol has two C-O bonds and the acid has 3.

CH3Cl<CH3F

 

[Borek]

CH4<CH3O<CH2O2<CO2

LogicX: try to assign oxidation numbers to central carbon atoms.

 

[DrDu]

Borek has led you on the right track. Nevertheless I think your intuition is fine: The concept of oxidation states is much less usefull in organic chemistry and kind of formalistic.

 

[Point Conception]

For electron transfer in simple organic oxidation , look at the oxidation of glucose:
6O2 + C6H12O6 ----> 6CO2 + 6H2O

 

[chemisttree]

Yep! Total brain fart!

CH2(OH)2(geminal diol)<CH2O2(formic acid) The geminal diol has two C-O bonds and the acid has 3.

 

[Borek]

You better edit this formic acid

 

[chemisttree]

Geez! One of those days.

Consider the following ranking from lowest oxidation state to largest:

CH4<CH3OH<CH2O2<CO2

CH3SH<CH3OH

CH2(OH)2(geminal diol)<CH2O2(formic acid) The geminal diol has two C-O bonds and the acid has 3.

CH3Cl<CH3F

 

[Point Conception]

In organic chemistry one definition of oxidation - reduction is the removel or addition
of hydrogen. For example the oxidation of an alcohol to a ketone.

C3H7OH + O ---> C3H6O + H2O
2 propanol ----- > propanone