It is the f sublevel. Uranium has the configuration [Rn] 5f3 6d1 7s2.
One electron occupies the highest energy sublevel of alkali metals. Alkali metals have one electron in their outermost energy level, making them highly reactive.
The maximum number of spins possible in a given sublevel is equal to the number of electrons that can occupy that sublevel, which is determined by the maximum number of electrons allowed in that sublevel based on the electron configuration rules (2 electrons per orbital). The total number of spins will be equal to twice the number of electrons in that sublevel.
The valence electrons in group 2 elements are found in the s sublevel. These elements are known as alkaline earth metals and have 2 valence electrons, which occupy the s sublevel of their outermost electron shell.
SPDF levels refer to the four sublevels in an electron shell: s, p, d, and f. These sublevels represent the different types of orbitals that electrons can occupy within an energy level. The s sublevel can hold up to 2 electrons, the p sublevel can hold up to 6 electrons, the d sublevel can hold up to 10 electrons, and the f sublevel can hold up to 14 electrons.
Hund's rule is the principle that within a sublevel, electrons prefer to occupy orbitals singly and with parallel spins before pairing up. This minimizes electron-electron repulsions and stabilizes the atom.
In uranium 238, the highest sublevel electron occupies is the 5f sublevel. Uranium has 92 electrons, so filling up the electron configuration involves reaching the 5f sublevel before completing the entire orbital diagram.
The highest sublevel that Promethium can have is 4f. It is possible for 14 electrons to be placed around Promethium, since the elements in this sublevel each have 7 orbitals.
The F-Sub level
One electron occupies the highest energy sublevel of alkali metals. Alkali metals have one electron in their outermost energy level, making them highly reactive.
The maximum number of spins possible in a given sublevel is equal to the number of electrons that can occupy that sublevel, which is determined by the maximum number of electrons allowed in that sublevel based on the electron configuration rules (2 electrons per orbital). The total number of spins will be equal to twice the number of electrons in that sublevel.
The maximum number of electrons in the 2p sublevel is 6. The p sublevel has three orbitals, each of which can take two electrons.
The elements in period 4 that have electrons in the 3d sublevel are elements 21 - 36. Refer to the Related Links for a printable periodic table that includes electron configurations.
The valence electrons in group 2 elements are found in the s sublevel. These elements are known as alkaline earth metals and have 2 valence electrons, which occupy the s sublevel of their outermost electron shell.
There are a total of six electrons that occupy the p orbital of a neutral silicon atom. The p sublevel can hold a maximum of six electrons, with each p orbital accommodating two electrons with opposite spins.
SPDF levels refer to the four sublevels in an electron shell: s, p, d, and f. These sublevels represent the different types of orbitals that electrons can occupy within an energy level. The s sublevel can hold up to 2 electrons, the p sublevel can hold up to 6 electrons, the d sublevel can hold up to 10 electrons, and the f sublevel can hold up to 14 electrons.
The f-suborbitals begin to be filled with the lanthanoids (atomic number 57-71). Each f-suborbital can hold a maximum of 14 electrons.
The alkali (Group 1) and alkaline earth (Group 2) metals occupy the s-block because their outermost electrons are in the s sublevel.