Given below are two statements:
Statement I: The correct order of electronegativity of fluorine, oxygen and nitrogen is $$F > O > N$$.
Statement II: The oxidation state of oxygen in $$OF_2$$ is +2 and in $$Na_2O$$ is $$-2$$.
In the light of the above statements, choose the correct answer from the options given below

Statement I: The correct order of electronegativity of fluorine, oxygen and nitrogen is $$F > O > N$$.

Correct,

Electronegativity increases across a period in the periodic table from left to right. 

As nitrogen, oxygen, and fluorine all belong to the same period and follow this trend, fluorine is the most electronegative element, followed by oxygen, and then nitrogen (forming the exact order $$F > O > N$$.

Statement II: The oxidation state of oxygen in $$OF_2$$ is +2 and in $$Na_2O$$ is $$-2$$.

Correct,

For $$OF_2$$,

Since, fluorine is $$-1$$

$$x+\left(-1\right)\times\ 2=0$$

$$x=+2$$

For $$Na_2O$$,

Since, sodium is always $$+1$$

$$\left(+1\right)\times\ 2+x=0$$

$$x=-2$$

Therefore, Statement II is also correct.

Hence, it is Option A$$\longrightarrow\ $$ Both Statement I and Statement II are true.