Identify the orbital with the following quantum members-
(i) n = 1, l = 0 (ii) n = 2, l = 1, m = 0

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Solution

Principal quantum number, $n = 1$
Azimuthal quantum number, $l = 0$
$l 0123 . . . . . .$
$s p d f . . . . . .$

(i) $n = 1$
$l = 0$
Orbital is $1 s$

(ii) $n = 2$
$l = 1$
$m = 0$
Orbital is $2 p$

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Q. Describe the orbital with following quantum numbers:

(i) n = 3, l = 2 (i i) n = 4, l = 3

Using s, p, d notations, describe the orbital with the following quantum numbers.
(a) n = 1, l = 0; (b) n = 3; l =1 (c) n = 4; l = 2; (d) n = 4; l =3.

Q. In a multi-electron atom, which of the following orbitals, described by the three quantum numbers, will have the same energy in the absence of magnetic field and electric field?
(i)

n = 1, l = 0, m = 0

(ii)

n = 2, l = 0, m = 0

(iii)

n = 3, l = 1, m = 1

(iv)

n = 3, l = 2, m = 1

(v)

n = 3, l = 2, m = 0

Q. From the following sets of quantum number, sets which are possible?

(i) n = 1 l = 0 m = 0 s = + \frac{1}{2} (i i) n = 3 l = 1 m = 0 s = - \frac{1}{2} (i i i) n = 2 l = 1 m = + 2 s = + \frac{1}{2} (i v) n = 3 l = 2 m = + 2 s = - \frac{1}{2} (v) n = 3 l = 3 m = + 1 s = + \frac{1}{2}

Q. The electrons are identified by quantum number n and l. Place them in increasing order of energy:
(i) n = 4, l = 1
(ii) n = 4, l = 0
(iii) n = 3, l = 2
(iv) n = 3, l = 1

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Identify the orbital with the following quantum members-(i) n = 1, l = 0 (ii) n = 2, l = 1, m = 0

Principal quantum number, n=1Azimuthal quantum number, l=0l0123......spdf......(i) n=1l=0Orbital is 1s(ii) n=2l=1m=0Orbital is 2p

Identify the orbital with the following quantum members-
(i) n = 1, l = 0 (ii) n = 2, l = 1, m = 0

Principal quantum number, $n = 1$
Azimuthal quantum number, $l = 0$
$l 0123 . . . . . .$
$s p d f . . . . . .$

(i) $n = 1$
$l = 0$
Orbital is $1 s$

(ii) $n = 2$
$l = 1$
$m = 0$
Orbital is $2 p$