CHEMICAL BONDINGDOE-HDBK-1015/1-93Fundamentals of ChemistryCH-01Rev. 0Page 24Figure 6 Ionic Bond, Sodium ChlorideIn the case of H + Br , this is likely to take place because the exchange would satisfy the+-needs of both atoms. Although there is far more to consider than just the number of valenceelectrons, this is a good rule of thumb.If the atom needed two electrons and only picked up one, it would still actively seek out anadditional electron. The reaction of H + Te is far less likely to take place because the+ -2resulting molecule would still have an incomplete valence shell. Of course, the combining oftwo atoms, when both want to release or gain electrons, may take place (for example; H or2O ) but is less probable when other atoms are available.2Atoms are joined or bonded together through this interaction of their electrons. There areseveral types of chemical bonds that hold atoms together; three will be discussed, ionic,covalent, and metallic.Ionic BondsAn ionic bondis formed when one or more electrons is wholly transferred from one elementto another, and the elements are held together by the force of attraction due to the opposingcharges. An example of ionic bonding is shown in Figure 6(A) for sodium chloride (table salt).The sodium atom loses the one electron in its outer shell to the chlorine atom, which uses theelectron to fill its outer shell. When this occurs, the sodium atom is left with a +1 charge andthe chlorine atom a -1 charge. The ionic bond is formed as a result of the attraction of the twooppositely-charged particles. No single negatively-charged ion has a greater tendency to bondto a particular positively-charged ion than to any other ion.
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