Sodium has a single valence electron in its 3rd shell with two full core shells within that have the identical configuration to neon. This makes sodium keen to donate its single valence electron in order to regain the electron symmetry of neon, resulting in its 1+ ionic character when interacting with other non-metal atoms. Being larger than lithium or hydrogen, the lower electrostatic force from the nucleus and the greater core electron shielding cause sodium’s valence electron to be more weakly bound, and this makes sodium more reactive than lithium. Pure sodium metal reacts violently, sometimes explosively, when placed in water as it donates its valence electron to oxygen. The heat of this reaction ignites the hydrogen gas that is also produced, burning with a yellow flame.
As we saw in the case of neon, the 2nd shell orbitals are more like spherical tetrahedra, and the 3rd shell is a single electron in a spherical s-orbital. These orbitals represent phase-locked, resonant, coherent, harmonic, stationary waves.
Sodium will give up its valence electron readily in an ionic interaction in order to reach the stability of a full 2nd shell. This is the same electron configuration as the 2s22p6 noble gas configuration of neon — a multi-di-electron state with two concentric full shells. That is why sodium forms a 1+ ionic state.
When sodium and chlorine interact, sodium gives the electron it wants to lose to chlorine, which is keen to gain it. This forms both atoms into their ions and allows both to achieve full shell configurations. The ions can then stick to each other because of their opposite charges, forming sodium chloride (NaCl) crystals. This process is called ionic bonding.
Sodium chloride (NaCl) dissolves in water because the polar H2O molecules and the ions in the crystal attract each other. The water molecules can therefore tug ions off the crystal and still satisfy the ion’s desire to attract their opposite polarity. As each ion leaves the crystal, it becomes hydrated — surrounded by water molecules.
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