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1st Year Chemistry Chapter 03 Atomic Structure MCQs Quiz Test

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If you are looking MCQs for 1st year Chapter Three "Atomic Structure" MCQs Question Answers with solutions you are here on right website. On this Page you will learn Chapter Three objective type solved Questions with solutions. All of these chapter wise first Year Chemistry question answers are helpful for upcoming exams and tests preparations. These MCQs are also helpful for entry tests.

Chemistry MCQs Chapter Three
First Year Chemistry Chapter Three Atomic Structure MCQs Quiz Test



You will learn in this Chapter:

  • Discovery of Electrons
  • Properties of Cathodes
  • Discovery of protons and their properties
  • Discovery of Neutrons and their properties
  • Measurement of e/m value and Measurement of Charge on electron
  • Rutherford’s atomic model
  • Planck’s Quantum Theory
  • Bohr’s Atomic Model/Defects
  • Spectrum
  • X-Rays and Atomic number
  • Wave-Particle Nature of Matter
  • Heisenberg’s Uncertainty principle
  • Quantum Numbers
  • Electronic Distribution


Q.1: Isotopes differ in?
  1. Properties with respect to their mass number
  2. Properties with respect to their proton number
  3. Isotopes don’t differ as they have same number of electrons and protons
  4. All of the above
A
Q.2: Isotopes are?
  1. Chemically similar
  2. Physically dissimilar
  3. Chemically dissimilar
  4. Both a and b
D
Q.3: Ionization energy depends upon?
  1. Atomic/ionic radii
  2. Proton to electron ratio
  3. Shielding effect
  4. All of the above
D
Q.4: 2nd ionization energy of Mg is higher than the first because?
  1. Metallic character of Mg+1 is less than that of Mg
  2. Nuclear pull for Mg+1electron is more than that for the Mg atom
  3. Size of Mg+1 is greater than Mg+2
  4. Both a and b
B
Q.5: With the increasing atomic number, ionization energy increases along a period because?
  1. No change in shielding effect along a period
  2. Nuclear pull increases with the increase in the number of protons
  3. Atomic/ionic size decreases along a period
  4. All of the above
D
Q.6: The correct set of four quantum numbers for the valence electron of rubidium (Z = 37) is?
  1. n = 5, 1 = 0, m = 0 and s = +1/2
  2. n = 5, 1 = 1, m = 1 and s = +1/2
  3. n = 5, 1 = 1, m = 0 and s = +1/2
  4. n = 6, 1 = 0, m = 0 and s = +1/2
A
Q.7: The electron configuration of K(19) is?
  1. 1s3 2s3 2p5 3s3 3p5
  2. 1s2 2s2 2p6 3s2 2p5 4s2
  3. 1s2 2s2 2p6 3s2 3p6 4s1
  4. None of the above
C
Q.8: The number of d-electrons in Fe+2 (Z=26) is not equal to?
  1. p electrons in Ne (Z = 10)
  2. d electrons in Fe (Z = 26)
  3. s electrons in Mg (Z = 12)
  4. p electrons in Ar (Z = 17)
C
Q.9: The electronic configuration of an element is 1s2 2s2 2p3. This represents a/an?
  1. Ground state
  2. Hybridized state
  3. Excited-state
  4. Molecular state
A
Q.10: In which of the following, all have the same number of electrons?
  1. Cl–, Br– and I–
  2. H–, H and H+
  3. F–, Ne and Na+
  4. Li+, Na+ and K+
C
Q.11: Identify the correct order of increasing energy?
  1. 1s < 2s < 3s
  2. 2s > 3s > 1s
  3. 1s > 2s > 3s
  4. None of the above
A
Q.12: The shapes of s orbitals is circular and their size?
  1. Increase with the increase in principal quantum number
  2. Decrease with the increase in principal quantum number
  3. Remains the same with the change in principal quantum number
  4. None of the above
A
Q.13: The place between the two orbitals is called?
  1. Free zone
  2. Nodal surface
  3. Neutral zone
  4. Resonance area
B
Q.14: Shapes of p orbitals?
  1. Circular
  2. Dumb-bell
  3. Elliptical
  4. Complex
B
Q.15: The correct number of degenerate orbitals?
  1. s = 2, p = 6, d = 10, f = 14
  2. s = 3, p = 1, d = 5, f = 7
  3. s = 1, p = 3, d = 5, f = 7
  4. s = 1, p = 3, d = 7, f = 5
C
Q.16: The ion that is iso-electronic with CI atom is?
  1. CN–
  2. O+2
  3. N+2
  4. O–2
D
Q.17: Which of the following particles would on losing an electron has its outermost p-orbital as half-filled?
  1. Nitrogen atom
  2. O+ ion
  3. P-1 ion
  4. S+1 ion
C
Q.18: The ionic specie having more electrons than neutrons is?
  1. Mg+2
  2. O2–
  3. Na+
  4. F-1
B
Q.19: Which pair of electrons of elements will have the same chemical properties?
  1. 2, 24
  2. 2, 4
  3. 13, 22
  4. 3, 11
D
Q.20: An orbital which is spherically symmetrical is?
  1. p-orbital
  2. s-orbital
  3. d-orbital
  4. f-orbital
B
Q.21: The value of e/m for the electron is?
  1. 1.7588 x 1011 kg C-1
  2. 1.7588 x 10-11 Ckg-1
  3. 1.7588 x 1011 kg C-1
  4. 1.7588 x 1011 Ckg-1
D
Q.22: A nodal plane in an orbital is the plane where the electron density is?
  1. Maximum
  2. -ve
  3. Zero
  4. +ve
C
Q.23: How many times the mass of neutrons is greater than the mass of an electron?
  1. 1480
  2. 2000
  3. 1840
  4. 1200
C
Q.24: The mass of an oxygen atom is?
  1. 2.657 x 10-23g
  2. 2.657 x 1023
  3. 16g
  4. 32g
A
Q.25: The mass of a neutron is?
  1. Same as that of proton
  2. A little bit smaller than that of proton
  3. Slightly more than that of proton
  4. Slightly less than that of proton
C
Q.26: The smallest charge of electricity which has been measured on any particle is?
  1. Charge on the positive ray of He gas
  2. Charge on particles
  3. Charge on any droplet in Millikan Experiment
  4. Charge on an electron
D
Q.27: Which of the following has highest ionization energy value?
  1. Li
  2. Be
  3. H
  4. He
D
Q.28: Greater shielding effect corresponds to ionization energy value?
  1. Greater
  2. Lesser
  3. Remain the same
  4. No effect
B
Q.29: The mass of a proton is?
  1. 9.1 x 10-10 g
  2. 9.1 x 10-18 g
  3. 1.672 x 10-27 kg
  4. 9.1 x 10-31 kg
C
Q.30: Which group shows the abnormal behavior in trend of ionization energy in periods?
  1. Group I-A
  2. Group III-A
  3. Group-VI-A
  4. Both b and c
B
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