This set of Class 11 Chemistry Chapter 2 Multiple Choice Questions & Answers (MCQs) focuses on “Quantum Mechanical Model of Atom”.
1. The principal quantum number describes ____
a) energy and size of the orbit
b) the shape of the orbital
c) spatial orientation of the orbital
d) the spin of the electron
View Answer
Explanation: Among the four quantum numbers, the principal quantum number describes the size and energy of the orbit. It is represented by the symbol “n”. For shells, K, L, M, N and O, n is given by 1, 2, 3, 4 and 5.
2. What is the shape the orbital, whose “l” is 1?
a) Spherical
b) Dumbbell
c) Double dumbbell
d) Complex
View Answer
Explanation: The azimuthal quantum number is given by “l”. When l = 0, 1, 2 and 3, they are s-orbital, p-orbital, d-orbital and f-orbital respectively. The shapes of s-orbital, p-orbital, d-orbital, and f-orbital are Spherical, Dumbbell, Double dumbbell and Complex respectively.
3. What is the magnetic quantum number of the orbital 2pz?
a) 1
b) ±1
c) -1
d) 0
View Answer
Explanation: The magnetic quantum of an orbital range from -( l – 1) to l – 1. Its symbol is given by m. For 2p orbital, there are 3 magnetic quantum numbers namely -1, 0 and 1. For 2pz orbital its 0, taken that z is the internuclear axis.
4. Total number of nodes for 3d orbital is ________
a) 3
b) 2
c) 1
d) 0
View Answer
Explanation: Total number of nodes include angular and radial nodes. Angular nodes and radial nodes are given by the formula n – l -1 and l respectively. So the total number of nodes are n – l -1 + l = n – 1. For 3d orbit, “n” is 3, so total number nodes is 3 – 1 = 2.
5. Which of the following set of quantum numbers is not valid?
a) n = 5, l = 2, m = 0, s = 1/2
b) n = 1, l = 2, m = 0, s = 1/2
c) n = 5, l = 3, m = 2, s = 1/2
d) n = 5, l = 2, m = 0, s = -1/2
View Answer
Explanation: The set of quantum number n = 1, l = 2, m = 0, s = 1/2, is not valid because the value of azimuthal quantum number should lie only in between 0 and n-1, where n is principal quantum number. So the above set of quantum numbers is not valid.
6. According to the Aufbau’s principle, which of the following orbital should be filled first?
a) 5d
b) 4p
c) 3p
d) 2s
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Explanation: As per the Aufbau’s principle, the orbital or subshell with the lowest energy should be filled first. The ascending order of orbital’s energy is given by 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 4f, 5d, 6p, 7s. So 2s orbital should be filled first.
7. No two electrons have the same set of all four quantum numbers.
a) True
b) False
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Explanation: Yes, no two electrons have the same set of all four quantum numbers. This is explained by Pauli’s exclusive principle. At most electrons can have all 3 quantum numbers the same as they are in the same orbital. But the spin quantum number’s values are different.
8. The below process of filling electrons in an orbital follows __________
a) Aufbau principle
b) Hund’s rule of maximum multiplicity
c) Pauli’s exclusive principle
d) Electronic configuration
View Answer
Explanation: According to Hund’s rule of maximum multiplicity, the pairing of electrons cannot be started until each of the orbitals is singly occupied. The reason behind this is that the half-filled or fully filled orbitals are much more stable comparatively.
9. How many electrons can exist with the principal quantum number’s value as 4?
a) 16
b) 4
c) 32
d) 12
View Answer
Explanation: The number of orbitals within an orbit is n2. But as each orbital can accommodate 2 electrons, the number of electrons that can exist with the “n” as the principal quantum number is 2n2. So here 2n2 = 2(4)2 = 2(16) = 32.
10. Write the values for l, n, and m for Ψ3,1,0?
a) 1, 3, 0
b) 3, 1, 0
c) 0, 3, 1
d) 1, 0, 3
View Answer
Explanation: The representation of the Schrodinger wave function is given by Ψn,l,m. Therefore by comparing Ψn,l,m and Ψ3,1,0 we get that n = 3, l = 1 and m = 0. Here n, l, and m are principal, azimuthal and magnetic quantum numbers respectively.
Sanfoundry Global Education & Learning Series – Chemistry – Class 11.
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