A silicon atom has 4 valence electrons. These electrons are paired up in the 3s and 3p orbitals. Therefore, a silicon atom does not have any unpaired electrons.
An atom of sulfur has 16 electrons. Since the electron configuration of sulfur is 2-8-6, there are two filled energy levels (1s and 2s/2p) with a total of 10 filled orbitals (2 in 1s, 8 in 2s/2p).
An atom of silicon has three electron shells or orbitals. These are the K, L, and M shells. The K shell can hold up to 2 electrons, the L shell can hold up to 8 electrons, and the M shell can hold up to 18 electrons.
There is one half-filled orbital in a chlorine atom. Chlorine has 17 electrons in its neutral state, distributed among 3s, 3p, and 3d orbitals. In the 3p subshell, there are three orbitals (px, py, pz), and if eight electrons are filled (as in the case of chlorine), one of these orbitals will contain only one electron, making it half-filled.
A phosphorus atom has 3s, 3p, and 3d orbitals for a total of 5 orbitals.
Three completely filled orbitals.
A silicon atom has 4 valence electrons. These electrons are paired up in the 3s and 3p orbitals. Therefore, a silicon atom does not have any unpaired electrons.
Sulfur has 4 half-filled orbitals, which are the three 3d orbitals and the 4s orbital. An orbital is considered half-filled when it contains one electron.
There are two completely filled orbitals in this atom: the 1s orbital with 2 electrons and the 2p orbitals with 6 electrons. The 2s orbital and 3s orbital are not completely filled.
In an arsenic atom, there are three half-filled orbitals. These are the 4s, 4p, and 4d orbitals. Each of these orbitals can hold a maximum of 2 electrons, so there are a total of 6 electrons in the half-filled orbitals of arsenic.
Selenium has four half-filled orbitals - the 4s, 4p_x, 4p_y, and 4p_z orbitals. This is because selenium has four electrons in its 4th energy level.
In a xenon atom, all five of its p orbitals are filled with electrons. Each p orbital can hold a maximum of 2 electrons, for a total of 10 electrons in the p orbitals of xenon.
A bromine atom has 7 half-filled orbitals: one in the 4s orbital, three in the 4p orbitals, and three in the 4d orbitals.
An atom of sulfur has 16 electrons. Since the electron configuration of sulfur is 2-8-6, there are two filled energy levels (1s and 2s/2p) with a total of 10 filled orbitals (2 in 1s, 8 in 2s/2p).
There are two orbitals that are completely filled in this atom: the 1s orbital with 2 electrons (1s2) and the 2s orbital with 2 electrons (2s2). The 2p orbital is not completely filled, as it should have a total of 6 electrons (2p6).
An atom of silicon has three electron shells or orbitals. These are the K, L, and M shells. The K shell can hold up to 2 electrons, the L shell can hold up to 8 electrons, and the M shell can hold up to 18 electrons.
In a cadmium atom, all 27 s orbitals are filled with electrons. Cadmium has 48 electrons, and the s sublevel can hold a total of 2 electrons per orbital, so 27 orbitals are needed to accommodate all the electrons.