Where is an electron in a 3pz orbital most likely to be? If the nucleus is at the origin of the x, y, and z axes, where is there zero probability of finding it?
The Correct Answer and Explanation is:
Correct Answer:
An electron in a 3pz orbital is most likely to be found along the z-axis, above and below the nucleus. There is zero probability of finding the electron in the xy-plane, which is the nodal plane of the 3pz orbital.
Explanation:
Atomic orbitals describe the regions in an atom where there is a high probability of finding an electron. The 3pz orbital is one of the p orbitals in the third energy level. The “3” refers to the principal quantum number, indicating the energy level and average distance from the nucleus. The “p” tells us the orbital has a dumbbell shape, and the “z” subscript indicates its orientation along the z-axis.
P orbitals have one nodal plane that passes through the nucleus and separates the two lobes of the orbital. For the 3pz orbital, this nodal plane is the xy-plane. In this plane, the probability of finding the electron is exactly zero. This is because the wave function describing the orbital equals zero at the nodal plane, and the square of the wave function gives the probability density. When the wave function is zero, the probability density is also zero.
The regions where the electron is most likely to be found are the two lobes that lie above and below the nucleus along the z-axis. These lobes represent regions of high electron density. The exact distance from the nucleus where the electron is most likely to be found depends on the radial part of the wave function, which has three radial nodes for a 3p orbital. These nodes are spherical surfaces where the probability of finding the electron is also zero, but they do not affect the angular location of the electron, which is concentrated along the z-axis.
In summary, the electron in a 3pz orbital is most likely found along the z-axis, and it cannot be found in the xy-plane.
