the answer is 3
There are three 4p orbitals in an atom. Each orbital can hold up to 2 electrons with opposite spins.
A bromine atom has 7 half-filled orbitals: one in the 4s orbital, three in the 4p orbitals, and three in the 4d orbitals.
Arsenic has three electrons occupying the three 4p orbitals in its valence shell. Hund's first rule tells us that they will each occupy separate orbitals before they start to pair up. So there are three half-filled orbitals in an arsenic atom.
The valence electrons in a bromine atom are located in the 4s and 4p atomic orbitals. Bromine has 7 valence electrons, with two in the 4s orbital and five in the 4p orbitals.
There are three 4p orbitals: 4px, 4py, and 4pz. Each orbital can hold a maximum of two electrons.
The last orbital to fill in a bromine atom is the 4p orbital. Bromine has a total of 35 electrons, with the electron configuration of [Ar] 4s2 3d10 4p5. The 4p orbital can hold a maximum of 6 electrons.
The central atom in BrCl3 is bromine (Br). The bromine atom in BrCl3 adopts sp3d hybridization, which involves the mixing of one 4s, three 4p, and one 4d atomic orbitals to form five sp3d hybrid orbitals.
Twelve: 6 electrons in 2p6 and 6 electrons in 3p6. No electrons in 4p orbital in ground state, so 4p0, only 4s1 is occupied (4th period, group 1)
zero - after the 4s orbitals are filled at Calcium, the 3d orbitals start to fill - not until Gallium do the 4p orbitals start to fill.
The hybridization of the central atom (Cl) in ClF5 is sp3d2. This means that the 3d, 4s, and three 4p orbitals of chlorine hybridize to form six equivalent sp3d2 orbitals, allowing for the five bonding pairs of electrons in the molecule.
apparently 8. according to another website. :)
All p sublevels contain three orbitals, including the 4p sublevel.