This question is tricky because distance and location are not well defined within the electron cloud. So for the sake of explanation, let us assume that the question is "Which has a region maximum probability closest to the nucleus?"
I could not find an answer in print for the 4f vs 6s. However, I did find an answer comparing the 3d and 4s. I believe that an understanding of a comparison between the 3d and 4s can be extended to a comparison between the 4f and 6s.
The most probable distance of the 3d is less than the 4s. Therefore, we could extend this and say that most likely the 4f sublevel would have a distance of maximum probability closer than the 6s.
You did not ask why so I will not go into an explanation.
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The final electron in inner transition metals typically enters the 4f or 5f orbitals. These orbitals are part of the inner electron shells and are responsible for the unique chemical properties of inner transition metals.
Electrons are removed first from the 5d orbital than the 4f orbital in lanthanides because the 5d orbital has higher energy than the 4f orbital. In lanthanides, the energy difference between the 4f and 5d orbitals is small, making it more energetically favorable to remove electrons from the 5d orbital first before the 4f orbital.
I would think the s orbital, because it is closer to the nucleus, and because the outer energy level holds more energy than the inner ones.
4f orbital
The 4s orbital has the greatest shielding effect because it is the closest to the nucleus and experiences less shielding from inner electrons compared to the 4p, 4d, and 4f orbitals. This means that electrons in the 4s orbital are held less tightly by the nucleus and are more easily removed.
Yes, "4f" is a valid orbital shell designation in the electronic configuration of atoms. It represents the fourth energy level and the f subshell within that energy level.
There are 3 nodes present in a 4f orbital: one radial node and two angular nodes. This means that there are regions in the orbital where the probability of finding an electron is zero.
The 5s orbital has a lower energy level than the 4d or 4f orbitals in a rubidium atom, according to the aufbau principle. Electrons fill orbitals starting from the lowest energy level to the highest energy level. This is why the electron fills the 5s orbital before the 4d or 4f orbitals in a rubidium atom.
The energy sublevel being filled by the elements Ce to Lu is the 4f sublevel. These elements are part of the lanthanide series and have their outermost electrons entering the 4f orbital.
The 4f atomic orbitals have a more complex shape compared to s and p orbitals, characterized by their angular momentum and nodes. While they can extend into regions further from the nucleus, they do have some probability density near the nucleus. However, the likelihood of finding an electron in the 4f orbitals close to the nucleus is relatively low due to their higher energy and more complex structure. Overall, the 4f orbitals do not show a high probability of finding electrons near the nucleus compared to lower energy orbitals like 1s or 2s.
The electronic structure of neodymium (Nd) is [Xe] 4f4 6s2. This means it has 4 electrons in the 4f orbital and 2 electrons in the 6s orbital.
The maximum number of electrons that can exist in 4f orbitals is 14.-pg. 110 Modern Chemistry table 2:)
The element cerium has a single electron in the 4f orbital. Its electron configuration is [Xe] 4f1 5d1 6s2.