In all p sublevels there are 3 sublevels, including 6p.
The atomic no of Boron is 5 , so two electrons in ist shell the last three electrons are divided in two sub energy levels two in lower level 's' and one in higher level 'p'
The element with 2 electrons in the 1s sub-level, 2 electrons in the 2s sub-level, and 2 electrons in the 2p sub-level is carbon (Atomic number: 6).
Sub level is also called orbital.It does not have any degenerate orbital.
The element with 2 electrons in the 4s sublevel is Calcium (Ca) with an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2.
2,8,1 or with sub-levels 1s22s22p63s1
The element cerium has a single electron in the 4f orbital. Its electron configuration is [Xe] 4f1 5d1 6s2.
The element with three unpaired electrons in the p sub level is phosphorus. It has a electron configuration of 1s2 2s2 2p6 3s2 3p3, with three unpaired electrons in the 3p sublevel.
The atomic no of Boron is 5 , so two electrons in ist shell the last three electrons are divided in two sub energy levels two in lower level 's' and one in higher level 'p'
The element with 2 electrons in the 1s sub-level, 2 electrons in the 2s sub-level, and 2 electrons in the 2p sub-level is carbon (Atomic number: 6).
Which sub level the electron is in.
Which sub level the electron is in.
Zinc
Hund's rule states that electrons pair up only after each orbital in a sub-level is singly occupied by electrons with the same spin. This minimizes electron-electron repulsion, leading to more stable electron configurations.
Sub level is also called orbital.It does not have any degenerate orbital.
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.
A break down of 2d1:2 = the quantum energy level or electron shell denoted as 'n'd = the sub-shell of the energy level (known as a degenerate level)1 = the number of electrons occupying the sub-shell.Through extensive research by scientists, no known element has a d sub-shell in the second (n=2) energy level. In fact, the d sub-shell does not appear until the fourth period (fourth row).The first d sub-shell is known to be in the third energy level (therefore the first energy level with this sub-shell is 3d, but not 2d).Transition metals are the elements known to fill the d sub-shells. The first transition metal in the periodic table is scandium (Sc) with the electron configuration of [Ar]4s23d1.The reasons for the formation of sub-shell of d is beyond my knowledge and the scope of basic chemistry.
there is a maximum of 6 electrons in the 'p'sublevel