Why is O2 enough to form a mole of Oxygen? [closed]








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I understand that this is the most basic knowledge of moles, however I'm still unsure - according to easy research, $\ce{O2}$ forms a mole of Oxygen. As a mole is $6.022\*10^{23}$, exactly what on the periodic table can we use to find out that it's 2 Oxygen in one mole? Wouldn't it be $6.022\*10^{23}$, instead of 2?




$\rm O\_2$ is the most common form of oxygen---the periodic table won't really tell you that. 


Avogadro's number tells you how many particles there are in a mole. 


There are $6.022\times 10^{23}$ O atoms in a mole of O atoms.


There are $6.022\times 10^{23}$ $\rm O\_2$ molecules in a mole of $\rm O\_2$. 


Since you have 2 oxygen atoms in one $\rm O\_2$ molecule, there are
$2\times 6.022\times 10^{23}$ O atoms in a mole of $\rm O\_2$. 


Do you see the difference?


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A 'mole' is not short for a 'molecule'.


The 'mole' is a specific quantity (number of objects) defined by Avogadro's constant $N\_A=6.022\times10^{23}mol^{-1}$. So a 'mole' of oxygen molecules has $6.022\times10^{23}$ molecules.


The '2' in $O\_2$ means there are two oxygen atoms in an oxygen molecule.


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