chemistry : class11 Angular Nodes : Concept of subshells : Structure of Atom MCQ Questions and Answers
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Angular Nodes
MCQ questions and answers.
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MCQ Questions
1. An electron is described by the orbital 4d_{z^2}. How many angular nodes does its wavefunction possess?
A.
0
B.
1
C.
2
D.
3
Correct Answer:
2
Explanation:
The number of angular nodes in an orbital is equal to its azimuthal quantum number l. For a d orbital, l = 2, so 4d_{z^2} has two angular nodes.
2. Which set correctly gives the number of angular nodes in the orbitals 3s, 4p, 5d, and 6f, respectively?
A.
0, 1, 2, 3
B.
1, 2, 3, 4
C.
0, 2, 4, 6
D.
3, 4, 5, 6
Correct Answer:
0, 1, 2, 3
Explanation:
The subshells s, p, d, and f correspond to l values 0, 1, 2, and 3, respectively. Since angular nodes equal l, the numbers are 0, 1, 2, and 3.
3. An orbital in the n = 4 shell has exactly three angular nodes. Which subshell must contain this orbital?
A.
4s
B.
4p
C.
4d
D.
4f
Correct Answer:
4f
Explanation:
Three angular nodes require l = 3. In the n = 4 shell, l = 3 corresponds to the 4f subshell.
4. Which statement correctly compares the angular nodes of 3d_{xy} and 3d_{x^2-y^2} orbitals?
A.
The 3d_{xy} orbital has one more angular node than 3d_{x^2-y^2}
B.
The 3d_{x^2-y^2} orbital has one more angular node than 3d_{xy}
C.
Both orbitals have the same number of angular nodes, although their orientations differ
D.
Both orbitals have no angular nodes because they belong to the same shell
Correct Answer:
Both orbitals have the same number of angular nodes, although their orientations differ
Explanation:
Both orbitals belong to the d subshell, for which l = 2. Therefore, each has two angular nodes; their spatial orientations are different because of their different angular wavefunctions.
5. For a hydrogen-like orbital with quantum numbers n = 5 and l = 2, which statement about angular nodes is correct?
A.
It has two angular nodes and belongs to a d subshell
B.
It has three angular nodes and belongs to an f subshell
C.
It has five angular nodes because n = 5
D.
It has three angular nodes because n - l = 3
Correct Answer:
It has two angular nodes and belongs to a d subshell
Explanation:
The number of angular nodes depends only on l, not directly on n. With l = 2, the orbital has two angular nodes and is a 5d orbital.
6. Among the allowed subshells of the fourth shell, which subshell has the greatest number of angular nodes?
A.
4s
B.
4p
C.
4d
D.
4f
Correct Answer:
4f
Explanation:
For n = 4, the allowed values of l are 0, 1, 2, and 3. The largest l value is 3 for the 4f subshell, so it has the greatest number of angular nodes.
7. How many angular nodes are present in each individual orbital of the 3d subshell, regardless of whether it is d_{xy}, d_{xz}, d_{yz}, d_{x^2-y^2}, or d_{z^2}?
A.
0
B.
1
C.
2
D.
5
Correct Answer:
2
Explanation:
All orbitals in a d subshell have l = 2. Thus, every individual 3d orbital has two angular nodes, even though the orientations and shapes of their nodal surfaces differ.
8. An orbital has one angular node and its magnetic quantum number is m_l = 0. Which orbital is represented?
A.
2s
B.
2p_z
C.
3d_{z^2}
D.
3p_x
Correct Answer:
2p_z
Explanation:
One angular node means l = 1, identifying a p orbital. For l = 1 and m_l = 0, the real orbital conventionally represented is p_z. The 2p_z orbital therefore satisfies both conditions.
9. If an electron undergoes a transition from an orbital with l = 3 to one with l = 1, what is the change in the number of angular nodes?
A.
The number decreases by 1
B.
The number decreases by 2
C.
The number increases by 2
D.
The number remains unchanged
Correct Answer:
The number decreases by 2
Explanation:
Angular nodes equal l. The initial orbital has three angular nodes and the final orbital has one, so the number decreases by 3 - 1 = 2.
10. A subshell contains five orbitals, and every orbital in it has two angular nodes. Which combination identifies this subshell?
A.
l = 0, s subshell
B.
l = 1, p subshell
C.
l = 2, d subshell
D.
l = 3, f subshell
Correct Answer:
l = 2, d subshell
Explanation:
A subshell with l = 2 is a d subshell and contains 2l + 1 = 5 orbitals. Each of these orbitals has l = 2 angular nodes.
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