There are 6 unpaired electrons in Cr because it is an exception atom when doing electron configuration. Because of the extra stability with a full subshell, one of the two electrons in the 4s orbital will move up to the 3d orbital (which originally had only 4 unpaired) to make the 3d orbital full.
Now, there is one unpaired electron in the 4s orbital and 5 unpaired electrons in the 3d orbital, which adds up to 6 total.
An atom of antimony in its ground state has 3 unpaired electrons.
Iodine has one unpaired electron in its ground state.
3 electrons. This can be told from the periodic table. These electrons are in the 2p orbital.
Magnesium has five unpaired electrons and is therefor paramagnetic
Germanium has 0 unpaired electrons in its ground state, as it has a completely filled 4s and 4p orbitals, resulting in a full outer shell configuration.
Phosphorus has three unpaired electrons in its ground state.
An atom of antimony in its ground state has 3 unpaired electrons.
Iodine has one unpaired electron in its ground state.
3 electrons. This can be told from the periodic table. These electrons are in the 2p orbital.
There are 5 unpaired electrons in Fe^3+ in its ground state.
Magnesium has five unpaired electrons and is therefor paramagnetic
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.
Hund's Rule
There are 5 unpaired electrons in Fe^3+ in its ground state.
Germanium has 0 unpaired electrons in its ground state, as it has a completely filled 4s and 4p orbitals, resulting in a full outer shell configuration.
Two
There are three unpaired electrons in an atom of cobalt in its ground state. This can be determined by the electron configuration of cobalt, which is [Ar] 4s2 3d7. The 3d orbital has 5 electrons, so there are 3 unpaired electrons.