![]() This reaction can be broken down into a few The product, NaCl, is much more stable than the reactants, Na and Cl 2. A great deal of heat is given off, indicatingĪ large decrease in the PE of the system. The link, below (which sometimes works and sometimesĭoesn't) shows this reaction taking place. An example of this is the reaction between Na Metals and non-metals interact to form ionic compounds. Lighter gray areas are the loosely held valence electrons, which areĮffectively shared by all of the metal atoms. "sea" of electrons which flow freely between the atoms. Instead, they are distributed throughout the metal and are completely delocalized. Metals share valence electrons, but these are Is a different sort of bonding than covalent bonding. Metals have relatively low ionizationĮnergies (easily removed electrons) but also low electron affinities (very Metallic bonding exists between metal atoms. The shared electrons are held betweenĬompounds represents actual numbers of atoms that are bonded to form molecules, They share valence electrons with other non-metals. Non-metals also have relatively high electron affinities, so they tend to Have fairly high ionization energies, meaning that it is relatively difficult There is no transfer of electrons, but a sharing There are no individual molecules ofĬovalent bonding takes place between non-metals. Indicates the ratio of sodium ions to chloride ions. Spheres, and the chloride ions, Cl -, by the yellow spheres. The sodium ions, Na +, are represented by the red In which each of the ions is surrounded by counter ions. On these anions and cations are stabilized by forming a crystal lattice, The chorine molecule gains electrons to form 2 Cl - ions. The sodium atom gives up an electron to form the Na + ion and The metal, sodium, and the non-metal, chlorine. An example of this is the reaction between The metal is oxidized and the non-metal is reduced. ![]() Transfer from the metal to the non-metal. Metals tend to lose electrons and non-metals tend to gainĮlectrons, so in reactions involving these two groups, there is electron Have relatively high Electron affinities and high Ionization energies. The most non-metallic element is fluorine. Non-metals are limited to the elements in the upper Metals) lose 1 and 2 valence electrons, respectively, because of their low Ionization Metals tend to lose electrons to attain Noble Gas electron configuration. Metallic elements are Cesium and Francium. Ionic bonds form between metals and non-metals. Of the PE and formation of more stable chemical species. This indicates an attractive forceīetween the charges and is a stabilizing factor. If the two charges have different signs, the PE will be negative. Like charges repel each other, so positive Or -,-) the PE will be a positive number. If the two charges have the same sign (+ class=GramE>,+ Product of two charges, Q 1 and Q 2 divided The PE can be calculated using Coulomb's Law, which is the At an atomic level, positive charges areĬarried by protons and negative charges are carried by electrons. The interaction of positive and negative charges. In large part, it is to lower the potential energy (PE) of
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