1st energy has 1 sublevel -- 1 orbital -- 2 electrons
2nd energy level has 2 sublevels -- 4 orbitals -- 8 e-
3rd energy level has 3 sublevels -- 9 orbitals -- 18 e-
4th energy level has 4 sublevels -- 16 orbitals -- 32 e-
Notice the pattern? number of orbitals = energy level squared
Number of electrons = 2x number of orbitals
1
describe the formation of this bond and the total number of electrons in theorbitals of each energy level.
There are three 2p orbitals and each can hold a maximum of two electrons with opposite spins, for a total of 6 electrons. This is true of the p sublevel in any energy level, except for the first energy level, which does not have a p sublevel.
The reason that orbitals of the same energy level degeneracy is due to similar molecular structure. The orbitals contains electrons that cancel each other out.
8 electrons. The second energy level (n=2) has 4 orbitals. One s orbital and three p orbitals. Each orbital can hold 2 electrons of opposite spin.
1
describe the formation of this bond and the total number of electrons in theorbitals of each energy level.
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 maximum number of electrons that can exist in 4f orbitals is 14.-pg. 110 Modern Chemistry table 2:)
There are three 2p orbitals and each can hold a maximum of two electrons with opposite spins, for a total of 6 electrons. This is true of the p sublevel in any energy level, except for the first energy level, which does not have a p sublevel.
1s orbital 3P, 5d, and 7f in discovered elements
The reason that orbitals of the same energy level degeneracy is due to similar molecular structure. The orbitals contains electrons that cancel each other out.
They can only have 1 S ORBITAL per energy level (1s, 2s, 3s...). Each S orbital consists of 2 electrons of opposite spin.
Any orbital can only contain a maximum of 2 electrons. The 5d energy level contains 5 orbitals - 5dxy 5dxz 5dyz 5d(x2-y2) and 5(dz2) each of which can contain a maximum of two electrons, so there are 10 total electrons in the set of 5 d orbitals.
10
8 electrons. The second energy level (n=2) has 4 orbitals. One s orbital and three p orbitals. Each orbital can hold 2 electrons of opposite spin.
s = 2 electrons p = 6 electrons d = 10 electrons f = 14 electrons Each single s orbital has two electrons in it. Each p orbital has two electrons in it and as there are three of these orbitals in a p subshell, the total electron number is six. d has five orbitals in its subshell, containing ten electrons (two in each orbital) when full, which form a dumbell-esque shape. f has seven orbitals each containing two electrons.