1s2, 2s2, 2p6, 3s2, 3p6
(gain 3e) 3p^6
1s2 2s2 2p6 3s2 3p6
2,8,4
Phosphorus ion (PĀ³ā») typically gains three electrons to achieve a stable electron configuration. As a result, it carries a charge of -3 and has a full outer electron shell.
nickel's outside electron shell is not full.
The actual configuration is [Ar] 4s^1 3d^10. Copper is anomalous. The atom is more stable with a full 3d shell and a partially filled 4s shell than it would be if it had a full 4s shell and a partially filled 3d shell.
The key to "happiness" for an atom is a full outer electron shell. (The outer electron shell is called the valence shell.) There are two conditions that cause a shell not to be full. Either it has only an electron or two (or three) in the outer electron shell or it's short an electron or two in that outer shell. The direct answer to the question is that if an element is chemically active, its outer electron shell is incomplete or is not full.
In the Group 1 and Group 2 elements, these metals want to loan out electrons to achieve what is called inert gas electron configuration, which is a full outer electron shell or valence shell. Because of their electron configurations as elemental metals, they are in a big hurry to do this (they are very reactive). In the ion, the metal has already loaned an electron (in the case of the Group 1 metals) or two electrons (in the case of the Group 2 metals). As an ion, the metal is "happy" because it has already reacted and loaned out the electron or electrons that will allow it to achieve inert gas electron configuration.
Phosphorus ion (PĀ³ā») typically gains three electrons to achieve a stable electron configuration. As a result, it carries a charge of -3 and has a full outer electron shell.
Where there are 8 electrons in the outer shell so a full shell. Elements are reactive when they need to lose or gain an electron. The noble gases are unreactive as they have a full outer shell.
The correct short electron configuration of silver is [Kr]4d105s1. The reason this happens is because 4d9 is less stable than the energy it takes to keep a pair of electrons in the 5S shell. Meaning because it is a lower energy state to maintain a full D shell than to maintain a full S shell. So the electron configuration tends toward a full D shell rather than a full S shell.
nickel's outside electron shell is not full.
The full electron configuration for sulfur atom is 1s2.2s2.2p6.3s2.3p4.
the outer electron shell has 7 electrons. its full configuration is 2.8.7
The actual configuration is [Ar] 4s^1 3d^10. Copper is anomalous. The atom is more stable with a full 3d shell and a partially filled 4s shell than it would be if it had a full 4s shell and a partially filled 3d shell.
Lithium does not have a '0' charge. Its electron configuration is 2,1. This means there is one valence electron in its outer shell. Losing this electron will make Lithium have a full shell (2 only) which all atoms try to achieve, therefore Li has a +1 charge because it loses an electron to gain noble gas configuration.
Atoms in Group 1, also known as alkali metals, typically have one less electron than a full outer orbit. These elements have one electron in their outermost shell, making them highly reactive and likely to lose that electron to achieve a more stable, full outer shell configuration.
The key to "happiness" for an atom is a full outer electron shell. (The outer electron shell is called the valence shell.) There are two conditions that cause a shell not to be full. Either it has only an electron or two (or three) in the outer electron shell or it's short an electron or two in that outer shell. The direct answer to the question is that if an element is chemically active, its outer electron shell is incomplete or is not full.
Phosphorus, like all atoms, tries to achieve a full electron shell. For Phosphorus to achieve its full shell and obtain an electron configuration that is isoelectronic with Argon, it must gain 3 electrons. Therefore, Phosphorus forms a -3 anion.
1s22s22p63s23p4