Consider the following statements :

(A) The principal quantum number 'n' is a positive integer with values of 'n' = 1, 2, 3, ...

(B) The azimuthal quantum number 'l' for a given 'n' (principal quantum number) can have values as 'l' = 0, 1, 2, ...... n

(C) Magnetic orbital quantum number 'm_l' for a particular 'l' (azimuthal quantum number) has (2l + 1) values.

(D) $\pm$ 1/2 are the two possible orientations of electron spin.

(E) For l = 5, there will be a total of 9 orbital

Which of the above statements are correct?

<p>(A) Principle quantum number n is a positive integer and it's possible values are n = 1, 2, 3 ........</p> <p>$\therefore$ A is correct.</p> <p>(B) Azimuthal quantum number 'l' for a given 'n' can have values as l = 0, 1, 2 ....... (n $-$ 1)</p> <p>$\therefore$ Statement B is wrong.</p> <p>(C) Magnetic orbital quantum number m_l for particular l has values from $-$ l to + 1 including zero means 2l + 1 values.</p> <p>$\therefore$ Statement C is correct.</p> <p>(D) $\pm \,\,{1 \over 2}$ are the two possible orientation of electron spin.</p> <p>$\therefore$ Statement D is correct.</p> <p>(E) For l = 5, there will be a total of 11 orbitals.</p> <p>$l$ = 0 $\Rightarrow$ 5 subshell</p> <p>$l$ = 1 $\Rightarrow$ p subshell</p> <p>$l$ = 2 $\Rightarrow$ d subshell</p> <p>$l$ = 3 $\Rightarrow$ f subshell</p> <p>$l$ = 4 $\Rightarrow$ g subshell</p> <p>$l$ = 5 $\Rightarrow$ h subshell</p> <p>We know,</p> <p>Number of orbital in any subshell = 2$l$ + 1.</p> <p>$\therefore$ For h subshell, number of orbitals = 2 $\times$ 5 + 1 = 11</p>