why AL attend ms gets 3+ charge when it loses three electrons
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An isolated aluminum atom has three electrons outside a closed shell. That is, the valence electrons include two 3s electrons and one 3p electron all outside a filled n=2 shell. Those three electrons in the n=3 subshell of s- and p-orbitals fill approximately the same physical space and are more or less equally energetic. So they are approximately equally easy to remove from the aluminum atom. Nature tends to strongly prefer either filled, half-filled, or empty shells rather than “oddly” filled shells. So aluminum atoms, when interacting with other atoms to form a solid, can lose one 3p electron (leaving a filled 3s orbital) creating an Al+ ion, or one 3s and one 3p electron (leaving a half-filled 3s orbital) creating an Al++ ion, or can lose all three of its n=3 shell electrons to form an Al+++ ion. Which it does depends on what it is interacting with. As with everything else, whatever lowers the energy the most is what nature chooses.
When Aluminum metal is formed, for example, all three of the valence electrons are delocalized creating an crystalline arrangement of Al+++ ions with three electrons per aluminum atom migrating among the ions. That makes metallic aluminum a good electrical conductor as well as a good thermal conductor. When the compound aluminum oxide (Al2O3) is formed, again each of the two aluminum atoms loses its three electrons to then complete the 2p orbitals of each of the three oxygen atoms - that is, six electrons are transferred from the two aluminums to the three oxygens to form the Al(2)O(3) molecule. In other aluminum compounds, one or two or three of those electrons are exchanged with the other atoms of the compound depending on what they are - and the specific configurations depend on which minimizes the total energy of the collection of atoms.