Atomic orbitals quantum numbers and shapes of s p d orbitals - Question Bank

1. The azimuthal quantum number 'l' determines the number of angular nodes and also:
A) The energy of the orbital
B) The number of subshells
C) The shape of the orbital
D) The spin of the electron
2. How many unpaired electrons are present in a nitrogen atom's ground state configuration (considering only valence orbitals)?
A) 0
B) 1
C) 2
D) 3
3. For an orbital with n=4 and l=1, what is the total number of nodes?
A) 1
B) 2
C) 3
D) 4
4. The shape of the dz^2 orbital is best described as:
A) Dumbbell with lobes along the z-axis
B) Spherical with a torus in the xy plane
C) Two cones along the z-axis
D) Cloverleaf in the xy plane
5. Which of the following sets of quantum numbers is NOT allowed for an electron in an atom?
A) n=1, l=0, ml=0, ms=+1/2
B) n=2, l=1, ml=-1, ms=-1/2
C) n=3, l=2, ml=3, ms=+1/2
D) n=4, l=3, ml=0, ms=-1/2
6. The quantum numbers for the 2p_z orbital are:
A) n=2, l=1, ml=0, ms=±1/2
B) n=2, l=1, ml=1, ms=±1/2
C) n=2, l=2, ml=0, ms=±1/2
D) n=2, l=0, ml=0, ms=±1/2
7. How many nodal surfaces does a 2s orbital have?
A) 0
B) 1
C) 2
D) 3
8. The shape of the dxy orbital is characterized by lobes in which plane?
A) xz plane
B) yz plane
C) xy plane
D) xz and yz planes
9. Which quantum number dictates the number of subshells within a principal energy level?
A) n
B) l
C) ml
D) ms
10. How many electrons can be placed in the 3d subshell?
A) 2
B) 6
C) 10
D) 14
11. The shape of a 4f orbital is:
A) Spherical
B) Dumbbell
C) Double dumbbell
D) Complex and multi-lobed
12. A 3d orbital has l = 2. How many possible values of ml are there?
A) 1
B) 3
C) 5
D) 7
13. What is the term used for the region of space around the nucleus where the probability of finding an electron is maximum?
A) Node
B) Orbit
C) Orbital
D) Nucleus
14. The probability density function |ψ|^2 represents:
A) The exact position of an electron
B) The energy of an electron
C) The probability of finding an electron in a unit volume at a given point
D) The angular momentum of an electron
15. Which quantum number is not derived from the solution of the Schrödinger equation for the hydrogen atom?
A) n
B) l
C) ml
D) ms
16. The set of quantum numbers (n, l, ml, ms) uniquely defines:
A) An energy level
B) A subshell
C) An atomic orbital
D) An electron shell
17. Which of the following orbitals has the highest energy in a multi-electron atom?
A) 2s
B) 2p
C) 3s
D) 3p
18. For multi-electron atoms, the energy of an electron depends on both 'n' and 'l'. Which statement is generally true?
A) Energy increases with 'l' for a given 'n'
B) Energy decreases with 'l' for a given 'n'
C) Energy is independent of 'l'
D) Energy is independent of 'n'
19. Which quantum number is related to the energy of the electron in a hydrogen atom?
A) n
B) l
C) ml
D) ms
20. The shape of a 3s orbital compared to a 2s orbital is:
A) Smaller and less diffuse
B) Larger and more diffuse
C) Same shape, different orientation
D) Different shape, same size
21. How many angular nodes does a d orbital have?
A) 0
B) 1
C) 2
D) 3
22. The number of angular nodes in an orbital is equal to the value of:
A) n
B) l
C) ml
D) ms
23. What is the total number of nodes in a 3p orbital?
A) 1
B) 2
C) 3
D) 4
24. The formula for the number of radial nodes in an orbital is (n - l - 1). For a 2p orbital, how many radial nodes are there?
A) 0
B) 1
C) 2
D) 3
25. What is the number of radial nodes in a 3s orbital?
A) 0
B) 1
C) 2
D) 3
26. A node in an atomic orbital is a region where:
A) The probability of finding an electron is maximum
B) The probability of finding an electron is zero
C) The electron energy is highest
D) The electron spin is zero
27. The number of orbitals in a subshell is given by 2l + 1. For a d subshell (l=2), how many orbitals are there?
A) 3
B) 5
C) 7
D) 9
28. What is the maximum number of electrons that can be accommodated in the n=2 energy level?
A) 2
B) 4
C) 8
D) 18
29. How many electrons can a single orbital hold according to the Pauli Exclusion Principle?
A) 1
B) 2
C) 3
D) Unlimited
30. The subshells present in the n=3 energy level are:
A) s, p
B) s, p, d
C) p, d, f
D) s only
31. For n=3, what are the possible values of 'l'?
A) 0, 1
B) 0, 1, 2
C) 1, 2
D) 0, 1, 2, 3
32. What is the total number of orbitals in the n=3 energy level?
A) 3
B) 5
C) 7
D) 9
33. The shape of the d orbitals is generally described as:
A) Spherical
B) Dumbbell
C) Double dumbbell
D) Complex
34. Which d orbital has lobes lying between the x and y axes in the xy plane?
A) dxy
B) dxz
C) dyz
D) dz^2
35. The five d orbitals have different spatial orientations. Which d orbital is oriented along the z-axis and also has lobes in the xy plane?
A) dz^2
B) dxz
C) dyz
D) dxy
36. How many d orbitals are there in a d subshell?
A) 1
B) 3
C) 5
D) 7
37. How many nodal planes are present in a p orbital?
A) 0
B) 1
C) 2
D) 3
38. What is the shape of a p orbital?
A) Spherical
B) Dumbbell
C) Double dumbbell
D) Cloverleaf
39. The three p orbitals (px, py, pz) are oriented along which axes?
A) x, y, z axes
B) x and y axes only
C) y and z axes only
D) x and z axes only
40. How many orientations are possible for a p orbital in space?
A) 1
B) 2
C) 3
D) 5
41. What is the shape of an s orbital?
A) Dumbbell
B) Spherical
C) Double dumbbell
D) Complex
42. An orbital with l = 2 is designated as:
A) p orbital
B) d orbital
C) f orbital
D) g orbital
43. An orbital with l = 1 is designated as:
A) s orbital
B) p orbital
C) d orbital
D) f orbital
44. An orbital with l = 0 is designated as:
A) p orbital
B) d orbital
C) f orbital
D) s orbital
45. For l = 1, what are the possible values for the magnetic quantum number (ml)?
A) 0
B) -1, 0, +1
C) -2, -1, 0, +1, +2
D) +1
46. If n = 2, what are the possible values for 'l'?
A) 0, 1
B) 0, 1, 2
C) 1, 2
D) 0
47. What does the spin quantum number (ms) represent?
A) The energy level of the electron
B) The shape of the electron cloud
C) The intrinsic angular momentum of an electron
D) The number of subshells in an energy level
48. For a given principal quantum number 'n', what are the possible values of the azimuthal quantum number 'l'?
A) 0, 1, 2, ..., n
B) 0, 1, 2, ..., n-1
C) 1, 2, 3, ..., n
D) -l, 0, +l
49. The magnetic quantum number (ml) determines:
A) The energy of the electron
B) The size of the orbital
C) The spatial orientation of the orbital
D) The spin of the electron
50. Which quantum number describes the shape of an atomic orbital?
A) Principal quantum number (n)
B) Azimuthal or angular momentum quantum number (l)
C) Magnetic quantum number (ml)
D) Spin quantum number (ms)
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