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Structure of Atom Class 11 MCQs Questions with Answers
Multiple Choice Type Questions
Question 1.
Rutherford’s experiment which established the nuclear model of the atom used a beam of
(a) β-particles which impinged on a metal foil and got absorbed
(b) γ-rays, which impinged on a metal foil and got absorbed
(c) helium atoms which impinged on a metal foil and got reflected
(d) helium nuclei which impinged on a metal foil and got scattered.
Answer
Answer: (d) helium nuclei which impinged on a metal foil and got scattered.
Question 2.
How many moles of electrons weigh one kilogram?
(a) 6.022 × 1023
(b) \(\frac {1}{9.108}\) × 1031
(c) \(\frac {6022}{9.108}\) × 1054
(d) \(\frac {1}{9.108 ×6.022}\) × 108
Answer
Answer: (d) \(\frac {1}{9.108 ×6.022}\) × 108
Question 3.
The wavelength associated #vith a golf ball weighing 200 g and moving at a speed of 5 m/h is of the order
(a) 10-10 m
(b) 10-20 m
(c) 10-30 m
(d) 10-40 m
Answer
Answer: (c) 10-30 m
Question 4.
The number of nodal planes in px orbital is
(a) one
(b) two
(c) three.
(d) zero
Answer
Answer: (a) one
Question 5.
The electronic configuration of an element is 1s² 2s² 2p6 3s² 3p6 3d5 4s1. It represents
(a) excited state
(b) cationic states
(c) ground state
(d) anionic state
Answer
Answer: (c) ground state
Question 6.
Azimuthal quantum number determines the
(a) size
(b) spin
(c) orientation
(d) angular momentum of orbitals
Answer
Answer: (d) angular momentum of orbitals
Question 7.
The electronic configuration of Cu2+ ion is
(a) [Ar] 4s1 3d8
(b) [Ar] 4s² 3d10 4p1
(c) [Ar] 4s1 3d10
(d) [Ar] 3d9
Answer
Answer: (d) [Ar] 3d9
Question 8.
The total number of orbitals in a shell having principal quantum n is
(a) 2n
(b) n²
(c) 2n²
(d) (n + 1)
Answer
Answer: (b) n²
Question 9.
The ion iso-electronic with CO is
(a) O–2
(b) N+2
(c) CN–
(d) O+2
Answer
Answer: (c) CN–
Question 10.
The line spectrum of hydrogen obtained in the visible region of light corresponds to
(a) Lyman series
(b) Balmer series
(c) Paschen series
(d) Brackett series
Answer
Answer: (b) Balmer series
Question 11.
If the nitrogen atom had electronic configuration 1s², it would have energy lower than that of the normal ground state configuration 1s² 2s² 2p³, because the electrons would be closer to the nucleus. Yet, 1s² is not observed because it isolates.
(a) Heisenberg’s Uncertainty Principle
(b) Hund’s rule
(c) Pauli Exclusion Principle
(d) Bohr postulate of stationary orbits
Answer
Answer: (c) Pauli Exclusion Principle
Question 12.
The quantum numbers + 1/2 and – 1/2 for the electron spin represent
(a) rotation of the electron in clockwise and anticlockwise direction respectively
(b) rotation of the electron in anticlockwise and clockwise direction respectively
(c) magnetic moment of the electron pointing up and down respectively
(d) two quantum mechanical spin states which have no classified analogue
Answer
Answer: (d) two quantum mechanical spin states which have no classified analogue
Question 13.
The energy of electron in the first Bohr orbit of H atom is 13.6 eV. The possible energy value (s) of the excited state(s) for electron in Bohr orbitals of hydrogen is (are)
(a) – 3.4 eV
(b) -4.2eV
(c) – 6.8 eV
(d) + 6.8 eV
Answer
Answer: (a) – 3.4 eV
Question 14.
The last entering electron in an element has quantum number n = 3, l = 2, m = + 2 and s = + 1 /2. The atomic number of the element will be
(a) 13
(b) 21
(c) 29
(d) 39
Answer
Answer: (c) 29
Question 15.
What is the wavelength of light. Given energy = 2.91 × 10-19], h = 6.36 × 10-34 Js, c = 3.0 × 108 m/s?
(a) 6.56 nm
(b) 656 nm
(c) 0.656 nm
(d) 65.6 nm
Answer
Answer: (b) 656 nm
Question 16.
Bohr atomic model can explain
(a) the spectrum of hydrogen atom only
(b) spectrum of an atom or ion containing one electron only
(c) the spectrum of hydrogen molecule
(d) the solar spectrum
Answer
Answer: (b) spectrum of an atom or ion containing one electron only
Question 17.
Magnetic quantum number specifies
(a) orbital size
(b) orbital shape
(c) orbital orientation
(d) nuclear stability
Answer
Answer: (c) orbital orientation
Question 18.
Which of the following set of quantum numbers belong to highest energy?
(a) n = 4, l = 0, m = 0, s = + \(\frac {1}{2}\)
(b) n = 3, l = 0, m = 0, s = + \(\frac {1}{2}\)
(c) n = 2, l = 1, m = 1, s = + \(\frac {1}{2}\)
(d) n = 3, l = 2, m = 1, s = + \(\frac {1}{2}\)
Answer
Answer: (d) n = 3, l = 2, m = 1, s = + \(\frac {1}{2}\)
Question 19.
Ground state electronic configuration of nitrogen is represented as
Answer
Answer: (a)
Question 20.
The orbital diagram in which Aufbau principle is violated is
Answer
Answer: (b)
Fill in the Blanks
Question 1.
Wave functions of electrons in atoms and molecules are called ……………….
Answer
Answer: Orbitals
Question 2.
The 2px, 2px 2z orbitals of atoms have identical shapes but differ in their ………………
Answer
Answer: Orientation
Question 3.
Cathode rays produce ……………… when they strike against the surface of a hard metal like Tungstun.
Answer
Answer: X-rays
Question 4.
Cathode rays produce ……………….. on striking ZnS screen.
Answer
Answer: flourescence
Question 5.
For n = 3, the values of l are ………………..
Answer
Answer: 0, 1, 2
Question 6.
The probability of finding the electron at any point around the nucleus is found from the values of ……………….
Answer
Answer: ψ²
Question 7.
The values of n, l and m for the last electron of atom with electronic configuration 2, 8, 3 are ………………..
Answer
Answer: 3, 1, -1 (or + 1 or 0)
Question 8.
The outermost electronic configuration of Cr is ……………….
Answer
Answer: 3d54s1
Question 9.
The light radiations with discrete quantities of energy are called …………………
Answer
Answer: photons
Question 10.
\(\frac {h}{λ}\) is the angular momentum of the electron in the ………………. orbit of He+.
Answer
Answer: 2nd
True or False Statements
Question 1.
The nucleus of an atom contains electrons and protons.
Answer
Answer: False
Question 2.
2H is more reactive than 1H.
Answer
Answer: False
Question 3.
The energy of the electron in 3d orbital is less than that in 4s orbital.
Answer
Answer: False
Question 4.
F– has more electrons than Na+.
Answer
Answer: False
Question 5.
Three electrons in p-orbital remains unpaired.
Answer
Answer: True
Question 6.
For a given value of l, the shape of orbital is independent of the value of n.
Answer
Answer: True
Question 7.
Cu+ is less stable than Cu2+.
Answer
Answer: True
Question 8.
2nd orbital is larger in size than Is orbital.
Answer
Answer: True
Question 9.
The energy of an electron in 3d orbital is less than that in the 4s orbital in the hydrogen atom.
Answer
Answer: True
Question 10.
Angular momentum of electron in a shell is quantized, was derived by Bohr.
Answer
Answer: False
Question 11.
For s-orbitals, orbital angular momentum is zero.
Answer
Answer: True
Question 12.
The angular momentum of a moving electron is an integral multiple of h/2π.
Answer
Answer: True
Question 13.
Bohr’s atom consists of circular orbits.
Answer
Answer: True
Question 14.
Two electrons can have the same values for n, l and m but should have different values of s.
Answer
Answer: True
Question 15.
The maximum number of electrons which can be accommodated in an orbital is 2n².
Answer
Answer: False
Match type Questions
| Column I | Column II |
| 1. Discovery of neutrons was done by. | 1. R.A. Millikan |
| 2. Degenrate orbitals are first singly occupied. | 2. Balmer Series |
| 3. Orbitals are filled in order of increasing energy. | 3. Max Planck |
| 4. An orbital can have maximum two electrons. | 4. Chadwick |
| 5. Position and momentum of a small particle cannot be measured simultaneously with absolute accuracy. | 5. Hund’s rule |
| 6. The angular momentum of a moving electron in an orbit is quantised. | 6. Thomson |
| 7. An atom is like a watermelon of positive charge in which electrons are embedded like the seeds. | 7. Aufbau principle |
| 8. The energy of each photon is directly proportional to the frequency. | 8. Pauli Exclusion principle |
| 9. When an electron jumps from 4th orbit to 2nd orbit, it gives rise to | 9. Heisenburg’s uncertainty principle |
| 10. The charge on an electron was found by oil drop exp. = 1.60 × 10-19 coulombs | 10. Bohr’s model of atom |
Answer
Answer:
| Column I | Column II |
| 1. Discovery of neutrons was done by. | 4. Chadwick |
| 2. Degenrate orbitals are first singly occupied. | 5. Hund’s rule |
| 3. Orbitals are filled in order of increasing energy. | 7. Aufbau principle |
| 4. An orbital can have maximum two electrons. | 8. Pauli Exclusion principle |
| 5. Position and momentum of a small particle cannot be measured simultaneously with absolute accuracy. | 9. Heisenburg’s uncertainty principle |
| 6. The angular momentum of a moving electron in an orbit is quantised. | 10. Bohr’s model of atom |
| 7. An atom is like a watermelon of positive charge in which electrons are embedded like the seeds. | 6. Thomson |
| 8. The energy of each photon is directly proportional to the frequency. | 3. Max Planck |
| 9. When an electron jumps from 4th orbit to 2nd orbit, it gives rise to | 2. Balmer Series |
| 10. The charge on an electron was found by oil drop exp. = 1.60 × 10-19 coulombs | 1. R.A. Millikan |
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