Shapes Of Orbitals

Question

Which of the following statements correctly describes the shape and orientation of the p_z orbital relative to the p_x and p_y orbitals?

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All three 2p orbitals (p_x, p_y, p_z) are degenerate (equal energy in the absence of an external field) and have identical dumbbell shapes—two lobes separated by a nodal plane through the nucleus. The p_z orbital has its lobes oriented along the z-axis with the nodal plane being the xy-plane. Similarly, p_x has lobes along the x-axis with the yz-plane as the nodal plane, and p_y has lobes along the y-axis with the xz-plane as the nodal plane. Option (A) is incorrect because p_z is also dumbbell-shaped, not spherically symmetric; only s orbitals are spherical. Option (C) is incorrect; all three p orbitals have the same size and energy—the magnetic quantum number labels orientation, not size. Option (D) is incorrect; each p orbital has exactly one nodal plane (its angular node), not two. The shape distinction between s, p, d, and f orbitals is a fundamental NCERT topic covered in detail in the atomic structure chapter. Plausibility check: l=1 for all p orbitals gives angular nodes = l = 1, confirming exactly one nodal plane per p orbital, consistent with the correct option.

Shapes Of Orbitals

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