How Electron Configuration Accounts for Ion Formation

How Electron Configuration Accounts for Ion FormationConsider negatron configuration as it applies to the bimonthly table and explain in detail how this accounts for the formation of ions.Elements argon arranged in the biweekly table (see figure 1) concord to their electronic configuration, which describes the numerate and arrangement of electrons in an atom, helping to make comprehend of the chemistry of an element. The notion of Electron configuration was first highlighted with the Bohr model, in which the electron fonts were orbits at a headstrong distance from the nucleus of an atom, and it is still common to speak of atomic structures in terms of sticks and sub-shells. An electron shell is the set of atomic orbitals which share the same prinicpal quantum number n (Krauskopf 1995) the number out front the letter in the oribital label. Orbitals are filled in the order of increasing n+1, where two orbitals permit the same treasure of n+1, they are filled in order of i ncreasing n (reference.com). This gives the following order for make full the orbitals1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7pIf we look at this in relation to the periodic table we tail end see that beginning with Hydrogen (which has one electron) going across to Helium having two. These two electrons have no filled up the first shell, called 1s. The next shell, 2s, is filled by Lithium and Beryllium. Moving across to the 2p sub shell (1p does not exist) B, C, N, O, F, Ne. Each whole (one row in the table) shell holds 8 electrons (with the S sub-shell safekeeping 2 electrons, and the p sub-shell holding 6). So the second shell, looking at one row of the periodic table, is Li and Be (2s), and B, C, N, O, F, and Ne (2p). The elements of group 2 of the perdioic table have an electron configuration of Ens2 (where E is an idle gas configuration, taken from reference.com). Those elements grouped together in the periodic table have notable similarities in their chemi cal properties (Drever 1997).Electrons fill readiness levels according to the Aufbau principle the principle that the electron configurations of atoms build up according to a set of rules. The three rules are thatElectrons go into the orbital at the lowest available energy levelEach orbital can only contain at most two electrons (with blow spins)Where there are two or much orbitals at the same energy, they fill singly before the electrons pair up.Figure 1 Periodic Table of ElementsValence electrons are the electrons contained in the outmost shell (commonly called the valence shell) of an atom, and are important in determining the chemical properties of an element (Krauskopf 1995). As a result of this, elements with the same number of valence electrons are grouped together in the period table. As a general rule, the fewer electrons an atom holds, the less stable it becomes and the more likely it is to react. Conversely the more complete the valence shell is the more inert an at om is and the less likely it is to chemically react. Elements in the same group of the periodic table have similar properties because they have the same outer electron configuration.There are trends in properties down a group because of the shielding effect of the increasing number of inner full shells (Drever 1997). Electrons are able to move from one energy level to another by emission or absorption of a quantum of energy, in the form of a photon (reference.com). It is this gain or leaving of energy that can trigger an electron to move to another shell or even rest period free from the atom and its valence shell. When an electron absorbs/gains more photons, then it moves to a more outer shell depending on the amount of energy the electron contains and has gained due to absorption. When an election releases/loses photons, then it moves to a more inner shell depending on the amount of energy the electron contains and has lost.If we use fluorine as an example, we can see that the f ull electron configuration of Fluorine is 1s2s2p5 (F is 5th from the left in p-block, one tail Neon so has 5 2p electrons). The valence electrons are 2s2p5 as there are two shells and these electrons are in the outer one. The key point is that atoms like to have a whole shell of 8 electrons, as this makes them more stable. As we can see from figure 1, Fluorine has only 7 electrons (7th from the well(p) on the second row). It really wants to gain an electron (to be like Neon) in order to have 8, and complete its shell. Fluorine is, therefore, very reactive and steals and electron off anything it can find. When it does this it gains an electron and becomes a damaging ion F (1s2s2p6). The reverse of this is Sodium (1s2s2p3s1), where 3s1 are the valence electrons. It really wants to loose this one extra electron to become 1s2s2p8 like Neon. It looses an electron and becomes a positive ion (Na+).REFERENCESBaird, C. (1995) Environmental Geochemistry. USA W.H. Freeman and CompanyDrever , J.I. (1997) The Geochemistry of earthy Waters. London Prentice-HallKrauskopf, K.B, Bird D.K. (1995) Introduction to Geochemistry. USA McGraw-HillHoward A.G. (1998) Aquatic Environmental Chemistry. Oxford Science PublicationsGarrels, R. M., and J. C.Christ. (1965). Solutions, minerals, and equilibria. San Francisco Freeman, Cooper.Web Resouceswww.reference.com