Which of the period 4 orbitals below is a 3dyz orbital?

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BlackTom AI · Accepted Answer

Let’s examine what a 3d dyz orbital looks like and how it would appear in a set of period-4 orbitals. The d_yz orbital has its lobes oriented in the yz plane, meaning the regions of high electron density lie between the y and z axes, with a nodal surface that runs along the x-axis. Now evaluate each option:

Option a. orbital (e): This image shows a pattern where the lobes are aligned primarily along the x and z directions, not in the yz plane. Since the dyz orbital requires lobes oriented between y and z axes, this option does not match dyz.

Option b. orbital (b): Here the lobes are arranged in a way that places the high-density lobes between the y and z directions, consistent with the yz-plane orientation. The nodal plane would align along the x-axis, which corresponds to a dyz character.

Option c. orbital (d): This depiction appears to have lobes oriented between the x and z axes (xz direction), not between y and z. That makes it a different d orbital (likely dzx) rather than dyz.

Option d. orbital (c): The lobes are positioned between the x and y axes, i.e., in the xy plane. This orientation corresponds to a d_xy type, not d_yz.

Option e. orbital (a): The figure shows a doughnut-shaped lobe around the z-axis with lobes aligned along z as well, characteristic of dz^2, not dyz.

In summary, only option b displays the characteristic yz-oriented lobes of the d_yz orbital, while the others show orientations corresponding to d_xz, d_xy, d_x^2−y^2, or d_z^2. Therefore, orbital (b) is the 3d dyz orbital.

CHM1052 - MUM S2 2025 CHM1052 2022 practice exam 1

Which of the period 4 orbitals below is a 3dyz orbital?

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