12 are paired, 3 are unpaired
To figure this out make a Bohr diagram! :)
Phosphorus typically borrows three electrons to achieve a full outer shell of eight electrons. This allows phosphorus to reach a stable electron configuration similar to the noble gas neon.
the electron configuration of phosphorous is 1s2, 2s2, 2p6, 3s2, 3p3. Your welcome! -Bri .C.
Noble gases, like helium, neon, and argon, have no unpaired electrons in their ground state electron configuration. This means that all of their electrons are paired up in orbitals.
Phosphorus has 3 unpaired electrons in its outermost shell.
The elements that have 5 electrons in the dot diagram means that they have 5 valence electrons. These elements are found in group 5A. Elements include, nitrogen, phosphorus, arsenic, antimony, and bismuth.
This is a chemical element. You can find the how many electron in a single atom by using a periodic table.
There are 5 electrons in the outermost electron shell of a phosphorus atom. Phosphorus has an electron configuration of 2, 8, 5.
A phosphorus atom has one nonbonding pair of electrons.
5
5 electrons where two electrons are paired and three are unpaired
There are 5 electrons in the outermost electron shell of a phosphorus atom. Phosphorus has the electron configuration 2-8-5, so it has 5 electrons in its outermost shell.
The total electron number for phosphorus is 15 because phosphorus has 15 electrons.
Phosphorus in is 3rd period. So it has 3 electron shells.
Phosphorus needs to gain three electrons to achieve a stable electron configuration.
Phosphorus has 5 valence electron. It forms anion by gaining 3 electrons.
The answer is 1. This is because the only atom with lone paires is phosphorus and it only has 1.
Phosphorus has five valence electrons.