Answer:
Explanation:
When we want to decipher the chemical behavior of atoms, we consider the electrons in such an elements. Electrons are negatively charged particles and they are the reasons why chemical reactions proceeds. In nuclear reactions, the nucleons which are the protons and neutrons takes center stage.
For chemical bonds to form, atoms would want to mimic the configuration of the noble gases by either gaining or losing electrons. Some atoms also would share their electrons in order to have a more stable configuration.
Chemical bonds are formed using the valence or outermost shell electrons. The valence shell electrons have relatively low ionization energy compared to those of the inner orbitals.
For an atom with atomic number 12, its electronic configuration would be 2,8,2 with the sublevel notation written as 1S²2S²2P⁶3S²
This atom has 2 valence electrons in its valence shell.
The closest group 8 element to atom with atomic number of 12 is neon. Neon has an atomic number of 10 and its configuration is given as 2,8.
For our atom to be like Ne, it must be ready to lose two of the valence electrons.
Atom-12 would prefer to form an ionic bond because of its high electropositivity i.e ability to lose electrons.
