Aluminium should gain 5 electrons or lose 3 electrons. It will normally lose 3 electrons to form Al3+ ion, rather than gaining 5 electrons and forming Al5- ion.
Only three electrons.
Boron must give up 3 electrons in order to achieve a noble-gas electron configuration.
When ionised to have no electrons, the usual notation would be 1s0. However, this is almost never needed, as other information and context will usually imply or define that there are no electrons.
Mg
It depends on what element you start with.
The ionization energy of an element.
Shouldn't you do the homework yourself. Teach your teacher!
it has 2 because the first energy level has 1
It depends on the atom. List what element the atom is from.
The electron configuration for an element is the arrangement of electrons in the orbits (or shells) of a neutral atom. Shells closer to the nucleus have higher binding energy.For example, there are eleven electrons in a sodium atom (atomic number 11). Scientists have measured the quantities of energy needed to remove these electrons one by one from a sodium atom. It is quite easy to remove the the first electron. The next 8 are difficult to remove. Finally, it becomes really hard to remove the last two electrons, which are held very powerully because they are the closest to the nucleus.This is just a common representation of electron configuration.---Example : For an atom of oxygen, there are 8 protons and 8 electrons. The first 2 electrons are in the subshell designated 1s, which can contain 2 electrons. The next 2 are in the shell designated 2s, which can also contain 2 electrons. The final 4 are in the 2p shell, which can contain up to 6 electrons. So the configuration is written as :1s2 2s2 2p4
Carbon can support up to 4 bonds, or a total of 8 electrons.
A chemical reaction which combines atoms of more than one element, in a configuration that is not like any existing configuration. In some cases, the chirality (left-handed twist or right-handed twist) can be enough of a difference for it to be a new compound.