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1. There will be total 20  MCQ in this test.
2. Please keep a pen and paper ready for rough work but keep your books away.
3. The test will consist of only objective type multiple choice questions requiring students to mouse-click their correct choice of the options against the related question number.
4. No negative marking for incorrect choice.
5. Please click on “Finish the Test” when you want to exit.
6. All the best – Happy Studying.

1. Which electronic configuration  violate the Pauli’s exclusion principle?

 A

 B

 C

 D

Question 1 of 20

2. The ground state electron configuration of Fe is:

 A

 B

 C

 D

Question 2 of 20

3. What is the ground-state electronic configuration of Si?

  1s² 2s² 2p⁶ 3s¹ 3p³

 1s² 2s² 2p⁶ 3s² 3p²

 1s² 2s² 2p⁷ 3s¹ 3p²

 1s² 2s² 2p⁶ 3s³ 3p¹

Question 3 of 20

4. If there are three electrons in p-subshell, which one of the following is the correct electronic configuration for these electrons?

  px⁰ py¹ pz²

 px² py⁰ pz¹

 px² py¹ pz⁰

 px¹ py¹ pz¹

Question 4 of 20

5. Which one of the following electronic configurations depict an oxygen atom?

 1s²2s²2p²

 1s²2s²2p⁴

  1s²2s²2p²3s²

 1s²2s²2p¹

Question 5 of 20

6. Which electronic configuration represents a violation of Hund’s rule for an atom in its ground state?

 A

 B

 C

 D

Question 6 of 20

7. The shape of a 2s orbital resembles:

  An ellipse

 Double spherical

 A hockey stick

 Double dumbbell

Question 7 of 20

8. Which quantum numbers must be the same for the orbitals so that they are designated to be degenerate in a one-electron system (like hydrogen)?

  m only

 l and m

  n and m

  n and l only

Question 8 of 20

9. Which of the following sets of orbitals is arranged in order of increasing energy?

  4s < 3d < 4p < 5s < 4d

 3d < 4s < 4p < 5s < 4d

 4s < 3d < 4p < 5s < 4d

 3d < 4s < 4p < 4d < 5s

Question 9 of 20

10. How many unpaired electrons are there in Ni²⁺ ( Z = 28)?

 2

 4

 8

Question 10 of 20

11. Which of the following is a possible electronic configuration?

  1s² 2s² 2p⁶ 3s² 3p⁸ 3d⁷

 1s² 2s² 2p⁶ 3s² 3d¹²

 1s² 2s³ 2p⁶

 1s² 2s² 2p⁶ 3s² 3p⁴

Question 11 of 20

12. The Pauli exclusion principle states that:

  Both the position of an electron and its momentum cannot be known simultaneously very accurately.

 The wavelength and mass of a subatomic particle are related by I = h/m v

 The wavelength of a photon of light times its frequency is equal to the speed of light.

 No two electrons in the same atom can have the same set of four quantum numbers.

Question 12 of 20

13. The shape of the p_x orbital is:

  Dumb-bell

 Octahedral

 Double Dumb-bell

 Spherical

Question 13 of 20

14. Which of the following would be diamagnetic?

  K

 O

 Ne

 Al

Question 14 of 20

15. Which electron configuration denotes an atom in its ground state?

 A

 B

 C

 D

Question 15 of 20

16. The shape of a 3p orbital resembles:

  Double spherical

 A circle

 Dumbbell

 A sphere

Question 16 of 20

17. Why is the electronic configuration of Cr – [Ar] 4s¹ 3d⁵ and not [Ar] 4s² 3d⁴ as predicted by Aufbau Principle?

  Because the 3d orbital is full with 5 electrons

 Because the 4s orbital can hold only one electron

 Because the 4s and 3d orbitals are then half-filled

 Because the 4s orbital is half-filled

Question 17 of 20

18. Which of the following electronic configurations is possible?

 1s² 2s² 2p¹⁰ 3s² 3d²

 1s² 2s² 2p⁵ 3s² 3p² 3d¹

 1s² 2s² 2p⁶ 3s² 3p²

 1s² 2s² 2p⁶ 3s² 3p² 3d¹⁰

Question 18 of 20

19. Which of the following electronic configurations is impossible?

 1s² 2s² 2p⁶ 3s² 3p² 4s²

 1s² 2s² 2p⁶ 3s² 3p⁶4s²3d¹

 2s² 2p⁶ 3s² 3p²

 1s² 2s² 2p⁶

Question 19 of 20

20. As atomic orbitals are filled according to the Aufbau principle, the 6s orbitals are filled immediately after which of the following orbitals?

  7s

 5p

 4f

 5d

Question 20 of 20

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