chemistry : class11 p-Subshell Characteristics : Concept of subshells : Structure of Atom MCQ Questions and Answers
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p-Subshell Characteristics
MCQ questions and answers.
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MCQ Questions
1. For a p-subshell in the third principal shell, which set of quantum numbers correctly represents all possible values of its magnetic quantum number?
A.
m_l = 0 only
B.
m_l = -1, 0, +1
C.
m_l = -2, -1, 0, +1, +2
D.
m_l = -3, -2, -1, 0, +1, +2, +3
Correct Answer:
m_l = -1, 0, +1
Explanation:
A p-subshell has azimuthal quantum number l = 1. Therefore, m_l can have the values -l through +l, giving -1, 0, and +1. These correspond to the three p orbitals.
2. How many angular nodes are present in every p orbital, irrespective of whether it is designated p_x, p_y, or p_z?
A.
Zero
B.
One
C.
Two
D.
Three
Correct Answer:
One
Explanation:
The number of angular nodes in an orbital equals its azimuthal quantum number l. For every p orbital, l = 1, so each has exactly one angular nodal plane.
3. A single p-subshell can accommodate a maximum of how many electrons, assuming the Pauli exclusion principle?
A.
2
B.
3
C.
6
D.
10
Correct Answer:
6
Explanation:
For a p-subshell, l = 1, so it contains 2l + 1 = 3 orbitals. Each orbital can hold two electrons with opposite spins, giving a maximum capacity of 3 × 2 = 6 electrons.
4. Which statement most accurately distinguishes the three orbitals within a p-subshell in the absence of an external field?
A.
They have different energies and identical orientations.
B.
They have identical energies but mutually perpendicular spatial orientations.
C.
They have different values of l but the same value of m_l.
D.
They have different principal quantum numbers but identical energies.
Correct Answer:
They have identical energies but mutually perpendicular spatial orientations.
Explanation:
The three p orbitals have the same n and l values and differ only in m_l, so they are degenerate in the absence of an external field. Their probability distributions are oriented along mutually perpendicular axes, conventionally labeled p_x, p_y, and p_z.
5. Which combination gives the number of orbitals and the maximum electron capacity of a p-subshell, respectively?
A.
2 orbitals and 4 electrons
B.
3 orbitals and 6 electrons
C.
4 orbitals and 8 electrons
D.
5 orbitals and 10 electrons
Correct Answer:
3 orbitals and 6 electrons
Explanation:
For a p-subshell, l = 1, so the number of orbitals is 2l + 1 = 3. Since each orbital accommodates two electrons, the maximum capacity is 6 electrons.
6. Which orbital description is impossible for an electron belonging to a p-subshell?
A.
3p_x
B.
4p_z
C.
2p_y
D.
1p_x
Correct Answer:
1p_x
Explanation:
A p-subshell requires l = 1, and for a given principal quantum number n, l can range only from 0 to n - 1. Thus, n = 1 permits only l = 0, so a 1p orbital cannot exist.
7. If an electron is specified as occupying a 4p subshell, which statement about its quantum numbers is necessarily correct?
A.
n = 4, l = 1, and m_l = -1, 0, or +1
B.
n = 4, l = 0, and m_l = 0
C.
n = 1, l = 4, and m_l = -4 through +4
D.
n = 4, l = 2, and m_l = -2, -1, 0, +1, or +2
Correct Answer:
n = 4, l = 1, and m_l = -1, 0, or +1
Explanation:
The number 4 identifies the principal shell, while p corresponds to l = 1. For l = 1, the allowed magnetic quantum numbers are -1, 0, and +1.
8. Which statement about the nodal structure of a p orbital is correct?
A.
It has one spherical radial node and no angular node.
B.
It has one angular nodal plane passing through the nucleus.
C.
It has two angular nodal planes perpendicular to each other.
D.
It has no node because its electron density is nonzero everywhere.
Correct Answer:
It has one angular nodal plane passing through the nucleus.
Explanation:
A p orbital has l = 1 and therefore one angular node. This node is a plane passing through the nucleus, separating the two opposite-lobed regions of the orbital.
9. When a p-subshell is completely filled, which electron arrangement within its three orbitals is consistent with both the Pauli exclusion principle and Hund's rule?
A.
One orbital contains six electrons and the other two are empty.
B.
Each orbital contains two electrons with paired opposite spins.
C.
Each orbital contains one electron, leaving three electrons unpaired.
D.
Two orbitals contain three electrons each and the third is empty.
Correct Answer:
Each orbital contains two electrons with paired opposite spins.
Explanation:
A p-subshell contains three degenerate orbitals, each with a capacity of two electrons. When fully occupied, all three orbitals contain electron pairs with opposite spins, satisfying the Pauli exclusion principle.
10. Which statement correctly compares the shapes and orientations of p_x, p_y, and p_z orbitals?
A.
They have different shapes because they possess different values of l.
B.
They are all spherically symmetric but differ in energy.
C.
They have the same two-lobed shape and differ in orientation along the x, y, and z axes.
D.
They have four lobes each, oriented in the xy, yz, and xz planes.
Correct Answer:
They have the same two-lobed shape and differ in orientation along the x, y, and z axes.
Explanation:
All p orbitals have l = 1 and therefore the same general dumbbell-like, two-lobed shape. Their distinction lies in spatial orientation: p_x, p_y, and p_z are aligned along the x-, y-, and z-axes, respectively.
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