CBSE Class 11 Chemistry Structure of Atom Worksheet Set 06

Practice Worksheets for Class 11 Chemistry: Chapter 02 Structure of Atom

Explore reliable practice materials for Chapter 02 Structure of Atom tailored for Class 11 learners. Utilizing these Chemistry worksheets ensures thorough preparation and strengthens problem-solving speed for upcoming school assessments.

Practice Chapter 02 Structure of Atom Worksheets for Class 11 Chemistry

Access the complete worksheet PDF for Chapter 02 Structure of Atom below. Regular practice with these targeted questions builds familiarity with standard exam patterns and helps secure higher marks in final Chemistry evaluations.

STRUCTURE OF ATOM
 
1. Ca lculate the energy of each of the photons which
i) correspond to light of frequency 3x 1015 Hz
ii) have wavelength of 0.50 A0
 
2. Ca lculate the energy and radius of the first orbit of He+ ion.
 
3. Ca lculate the wavelength of the photon that is emitted when an electron in Bohr’s orbit n=2 returns to the orbit n=1 in the hydrogen atom.
 
4. Ca lculate the de Broglie wavelength of a bullet of mass 2.2 x 10-3 Kg fired with a velocity of 300 m/s.
 
5. Ca lculate the speed of an electron if its de Broglie wavelength is twice its displacement in one second.
 
6. Ca lculate the uncertainty in the velocity of a cricket ball if the mass is 200 g. Uncertainty in the position is 1pm.
 
7. An electron beam from an accelerator is with kinetic energy 1.6 x 10-17J. What is its de Broglie wavelength?
 
8. A photon of wavelength 4 × 10–7 m strikes on metal surface, the work function of the metal being 2.13 eV. Calculate
(i) the energy of the photon (eV)
(ii) the kinetic energy of the emission, and
(iii) The velocity of the photoelectron (1 eV= 1.6020 × 10–19J).
 
9. Sh ow that the wavelength related to a 250g object moving with a speed of 100 m/s is too short to be observed.
 
10. i. State Heisenberg’s uncertainty principle.
ii. A table tennis ball has mass 10g and a speed of 90m/s. If speed can be measured with an accuracy of 4% what will be the uncertainty in the speed and position?
 
11. Tw o particles A and B are in motion. If the momentum of A is half of that of B and if the wavelength of A is 4.5 x 102 nm, what is the wavelength of B?
 
12. W hat is meant by “ Energy of an electron in a hydrogen atom is quantized”
 
13. i. Explain the dual nature of light.
ii. When would the wavelength associated with an electron be equal to the wavelength associated with a proton?
 
14. Ele ctrons are emitted with zero velocity from a metal surface when it is exposed to radiation of wavelength 6800Ao.Calculate the threshold frequency and work function of the metal.
 
15. W hy is the electronic energy of hydrogen negative?
 
16. De fine
i. Photoelectric effect
ii. Black body radiation
 
17. Di fferentiate
i. Absorption and emission spectrum
ii. Orbit and orbital
 
18. W hy is the concept of orbit replaced by the concept of orbital?
 
19. Dr aw the shapes (boundary surfaces) of the following orbitals.
(i) 2py (ii) 3dz2 (iii) 3dx2 – y2
 
 
20. i) What do you understand by quantum numbers? What is their significance?
ii) Describe the orbital: a) n=2, l=0 b) n=6, l = 4 c) n= 2, l =3
 
21. i) State (n+l) rule.
ii) Give reason: In the building up of atoms, 4s is filled before 3d
 
22. Ho w many electrons are possible in a) 4p b) 5pz c) n= 3, l= 2 d) n= 4, l=2, s= + ½
 
23. W hy are half filled and completely filled orbitals more stable?
 
24. W ith the help of Pauli’s exclusion principle and the concept of atomic numbers for orbitals, show that an M shell cannot accommodate more than 18 electrons.
 
25. Lis t the quantum numbers of a) unpaired electron in F , b) valence electrons in P , Ca
 
26. W hat are the possible values of l and m for a) n=3 b) n=2
 
27. (a) How many electrons in an atom may have the following quantum number?
 
(i) n = 4 ms = +1/2 (ii) n = 3 , l = 0
 
(b) What are the atomic numbers of elements whose outermost electrons are represented by
 
(i) 3s1 (ii) 2p3 (iii) 3d6
 
28. Ba sed on Bohr Bury rules arrange the following orbitals in the increasing order of energy.
(i) 5f , 4d , 7s , 7p (ii) 5p , 4d , 5d , 4f , 6s
 
29. Di scuss the similarities and differences (two each) between a 1s and a 2s orbital.
 
30. i . Which is more stable a) Mn2+ or Mn3+ b) Fe2+ or Fe3+? Give reason.
ii. Which rule is disobeyed while writing electronic configuration of carbon as 1s2 ,2s2 ,2px2? State the rule and write the correct configuration.
 
iii. Electronic configuration in Copper is [Ar] 4s1, 3d10 and not [Ar] 4s2, 3d9.Why?
 
iv. Among the following pairs of orbitals which orbital will experience the larger effective nuclear charge? (i) 2s and 3s, (ii) 4d and 4f, (iii) 3d and 3p.


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Chapter 02 Structure of Atom Practice Sheet and Solutions for Class 11 Chemistry

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