chapter 2

11th Standard

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Chemistry

Time : 00:01:00 Hrs
Total Marks : 1
    14 x 2 = 28
  1. How many orbitals are possible for n =4?

  2. How many radial nodes for 2s, 4p, 5d and 4f orbitals exhibit? How many angular nodes

  3. Which quantum number reveal information about the shape, energy, orientation and size of orbitals?

  4. What are the defects of Rutherford's model?

  5. What is the charge and mass of an electron?

  6. How many neutrons and protons are there in the Following nuclei?
    \(_{ 6 }^{ 13 }{ C }\),\(_{ 2 }^{ 18 }{ O }\).\(_{ 12}^{ 24}{ Mg }\),\(_{26 }^{ 56}{ Fe }\),\(_{ 88}^{ 38}{ Sr }\)

  7. Draw the shapes (boundary surfaces) for the following orbitals.
    (i) 2px
    (ii) 3dz
    (iii) 3dx2y2

  8. How many unpaired electrons are present in the ground state of
    (i) Cr3+ (Z = 24) (ii) Ne (Z = 10)

  9. What is meant by electronic configuration? Write the electronic configuration of N (Z = 7).

  10. Write a note about J.J. Thomson's atomic model.

  11. Explain about the significance of de Broglie equation.

  12. Write the equation to calculate the energy of nth orbit.

  13. What are degenerate orbitals?

  14. State Hund's rule of maximum multiplicity

  15. 23 x 3 = 69
  16. What are quantum numbers?

  17. Using s, p, d notations, describe the orbital with the following quantum numbers.
    (i) n =1 ,l = 0 ,(ii) n = 3, l= 1 (iii)n = 4, l= 2 (iv) n =4 , l = 3

  18. Which one among the following salts is more stable? Ferrous and ferric salts

  19. State and explain pauli's exclusion principle

  20. Explain briefly the time independent schrodinger wave equation?

  21. (i) State (n + 1) rule.
    (ii) Arrange the orbials in the increasing order of energies based on (a) principal quantum number and (b) (n + 1) rule.

  22. Write the electronic configurations of the following ions:
    (a) H- (b) Na+ (c) O2- (d) F-

  23. What are the atomic numbers of elements whose outermost electrons are represented by
    (a) 3s2 (b) 2p3 (c) 3p5

  24. If the K.E of electron is 2.5 \(\times\)10-24 J, then calculate its de-Broglie wavelength.

  25. What is Zeeman effect?

  26. What is Stark effect?

  27. Which of the following are isoelectronic species? Na+, K+, Mg2+, Ca2+, S2-, Ar.

  28. Write the Schrodinger wave equation

  29. State Heisenberg's uncertainty principle and give its mathematical expression

  30. What are the significance of \(\Psi \) and \(\Psi ^{ 2 }\)

  31. Bring out the main points of difference between orbit and orbital.

  32. What are the conclusions of Rutherford's α-rays scattering experiment?

  33. What are the limitations of Bohr's atom model?

  34. Write a note about principal quantum number.

  35. Using Aufbau principle, write the ground state electronic configuration of following atoms.
    (i) Boron (Z = 5)
    (ii) Neon (Z = 10)
    (iii) Aluminium (Z = 13)
    (iv) Chlorine (Z = 17)
    (v) Calcium (Z = 20)
    (vi) Rubidium (Z = 37)

  36. From the following sets of quantum numbers, state which are possible. Explain why the others are not possible.
    \(n=1,l=1,m_l=0,m_s=+\frac{1}{2}\)

  37. State Hund's rule of maximum multiplicity.

  38. Describe the Autbau principle

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