Which one of the following sets of quantum numbers represents the highest energy level in an atom?

• n = 4, l = 0, m = 0, s = +$\frac{1}{2}$

• n = 3, l = 1, m = 1, s = +$\frac{1}{2}$

• n = 3, l = 2, m = -2, s = +$\frac{1}{2}$

• n = 3, l = 0, m = 0, s = +$\frac{1}{2}$

The spin only magnetic moment of Fe²⁺ ion (in BM) is approximately

• 4

• 7

• 5

• 6

In an alkaline medium, glycine predominantly exists as/ in a/ an

• cation

• anion

• Zwitter ion

• covalent form

Which one of the followmg has no unpaired electrons?

• O${}_2^{-}$

• O${}_2^{+}$

• O${}_2^{2-}$

• O₂

The "spin only'' magnetic moment of Ni²⁺ in aqueous solution would be [At. no. of Ni = 28]

• $\sqrt{15}$ BM

• $\sqrt{2}$ BM

• $\sqrt{8}$ BM

• $\sqrt{6}$ BM

The correct set of four quantum numbers for the outermost electron of sodium (Z = 11) is

• 3, 1, 1, $\frac{1}{2}$

• 3, 2, 1, $\frac{1}{2}$

• 3, 0, 0, $\frac{1}{2}$

• 3, 1, 0, $\frac{1}{2}$

The statement that is not correct is

• Angular quantum number signifies the shape of the orbital

• Energies of stationary states in hydrogen like atoms is inversely proportional to the square of the principal quantum number

• Total number of nodes for 3s-orbital is three

• The radius of the first orbit of He is half that of the first orbit of hydrogen atom

198.

The two electrons have the following set of quantum numbers, P =3,2, -2 +1/2, Q =3,0,0 + 1/2. Which of the following statement is true?

• P and Q have same energy

• P has greater energy than Q

• P has lesser energy than Q

• P and Q represent same electron

Among the elements from atomic number 1 to 36, the number of elements which have an unpaired electron in their s subshell is

• 2

• 7

• 6

• 9

The energy of electron in the n^th Bohr orbit of H-atom is

• $-\frac{13.6}{{\mathrm{n}}^2} \mathrm{eV}$

• $-\frac{13.6}{\mathrm{n}} \mathrm{eV}$

• $-\frac{13.6}{\mathrm{n}4} \mathrm{eV}$

• $-\frac{13.6}{{\mathrm{n}}^3} \mathrm{eV}$