Ionic compounds are a prevalent chemical compound, but a unique form. You will learn about their formation and structure in this video lesson and see examples of ion-formed compounds.
Each atom is unique in that it consists of a certain number of protons, neutrons and electron. The number of protons and electrons for an atom is usually the same. Moreover, while the number of protons will never change for any atom, because that would mean you have an entirely different element of electrons sometimes changes. When associate degree atom gains or loses an electron, we tend to get ion. Since electrons themselves have a net charge, adding or removing electrons from associate degree atom changes the charge of the atom. This is as a result of the amount of electrons is not any longer in balance with the number of protons that have an electric charge.
When we say ions, it is true that opposites attract. The alternative negative and positive charges of the ions hold along in ionic bonds, forming ionic compounds that are simply what they sound like: compounds made from ions. The loss or gain from one atom matches the loss or gain of the opposite, thus one atom primarily 'donates' associate degree electron to the opposite atom it pairs up with.
Table salt is example of an ionic compound. Atomic number 11 and Cl ions move to make common salt, or NaCl. The atomic number 11 atom during this compound loses Associate in electron to become Na+, whereas the Cl atom gains Associate in electron to become Cl-. Together, they kind a neutral compound because of the ions balance one another out. This is often true for all ionic compounds - the positive and negative charges should be in balance.
Ions generally pack into extraordinarily regular crystalline structures, in a meeting that minimizes the lattice energy (maximizing attractions and minimizing repulsions). The lattice energy is that the summation of the interaction of all sites with all alternative sites. For polarizable spherical ions, solely the costs and distances are needed to see the electricity interaction energy. For any explicit ideal crystal structure, all distances are geometrically associated with the littlest intern clear distance.
Ionic bonding may end up from a chemical reaction reaction once atoms of a part (usually metal), whose ionization energy is low, provide a number of their leptons to attain a stable electron configuration. In doing therefore, cations are fashioned. AN atom of another part (usually nonmetal) with larger lepton affinity accepts the electron(s) to realize a stable electron configuration, and once accretive electron(s) an atom becomes an ion. Typically, the stable lepton configuration is one among the noble gases for components within the s-block and therefore the p-block, and explicit stable lepton configurations for d-block and f-block components. The static attraction between the Associate in ions and cations results in the formation of a solid with a crystallographic lattice within which the ions are stacked in an alternating fashion. In such a lattice, it is typically impracticable to differentiate separate molecular units, so the compounds fashioned are not molecular in nature. However, the ions themselves are often complicated and type molecular ions just like the acetate ion or the ammonium ion.
For example, common table salt is an example of an ionic compound. Sodium and chlorine ions come together to form sodium chloride, or NaCl. The sodium atom in this compound loses an electron to become Na+, while the chlorine atom gains an electron to become Cl-. These ions are then attracted to each other in a 1:1 ratio to form sodium chloride (NaCl).
Na + Cl → Na+ + Cl− → NaCl
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