3: 1s, 2s, 2px
6 electrons in total, 2 in each orbital
The maximum number of electrons in the 2p sublevel is 6. The p sublevel has three orbitals, each of which can take two electrons.
6
5 electrons in p orbitals in the outer shell. Cl has an electronic configuration of [Ne] 3s2, 3p5 In level 2 there a further 6 electrons in p orbitals making 11 electrons in total occupying p orbitals
6 electrons in total, 2 in each orbital
6 electrons in 3 orbitals of p-sublevel: px, py and pz
Multiply the orbitals in that sublevel by 2. The s sublevel has one orbital and can contain 2 electrons. The p sublevel has three orbitals and can contain 6 electrons. The d sublevel has five orbitals and can contain 10 electrons. The f sublevel has seven orbitals and can contain 14 electrons.
There are 5 d orbitals which hold 2 electrons each. Thus, 10 electrons are needed to completely fill them.
Each of the p orbitals can hold 2 electrons due to the Pauli exclusion principle. Because there are 3 p orbitals in a given subshell, the overall p subshell can hold 6 electrons.
In silver there are 2 electrons in 3s orbital, 6 electrons in 3p orbitals and 10 electrons in 3d orbitals. So there is a total of 18 electrons
Sulfur has two electrons in the 1s orbital, two electrons in the 2s orbital, and 6electrons in the 2 p orbitals. The electrons are part of the first and second energy levels, the electron core. The next energy level, the last one, is the outermost energy which comprises the valence shell.
6 degenerate orbitals allows for seven electrons, five of which are unpaired. ans is 6