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Ionic bonds involve the transfer of valence electrons between cations and anions. This type of chemical bond usually forms between a metal and a non-metal. The difference in electronegativity values between the metal and non-metal determines the extent of the bond. Ionic bonds are also known as electrovalent bond. Ionic bonds don't just bond with metal ions and nonmetals ions, ionic bonding can also occur with polyatomic ions. Crystals are held together by ionic bonds. Ionic bonding typically occurs with metals and nonmetals.

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If a negative ion meets a positive one, their opposite charges attract strongly and glue the atoms together. This type of gluing is called an ionic bond. [1]

Common table salt is sodium chloride witch is an ionic bond. [2]

Ions in crystal lattices of purely ionic compounds are spherical. [3]

Electrons can flow directly through the ionic substance in a molten state. [4]

Atoms become more stable when their outer most energy level has 8 electrons. Pure ionic compounds usually are crystalline solids, liquids, or gases. Many ionic compounds are binary compounds. [5]

Definition

An ionic bond is the attraction between oppositely charged ions. [6] The ions are "bonded" together with an electrostatic attraction, the attraction of oppostiely charged ions. [7]In nature, metals and nonmetals are typically the only elements reacting into ionic compounds with the help of the ionic bonds. [8] An ionic compound is the result of an ionic bond. It is created when an atom loses electrons relatively easily, and then reacts with an atom that has a high attraction for electrons; valence electrons are then shared between the metal and nonmetal. [9] . When an ionic compund is being named, the metal is first and followed by the nonmetal. .[10]

The Invention of Ionic Bonds

Before G.N. Lewis’ theory of shared electrons pair bond was introduced, some believed that the bond s found in salts were explained by simple electrostatic forces between the positive and negative ions. At the time those ions were thought to be the basic molecular units of those compounds. G.N. Lewis continued to observe those thoughts about bonds after his theory was introduced. Lewis’ shared electron pair bond is known as the covalent bond, while the other type is the ionic bond. .[11]

The Creation of Ionic Bonds

Ionic bonds are made when an electron from the valence shell of one atom is transferred to the valence shell of another atom. Most atoms lose electrons to fill the outer energy level, so it can then contain eight electrons, by doing so the outside energy levels become more stable. [12] The atom that lost an electron becomes a positive ion, a cation, and the atom that gains the electron becomes a negative ion, an anion; the ions used are either monatomic or polyatomic. [13]. When the atoms combine to make the bond as stable as possible, it requires a lot of energy. The greater the charge of a positive ion, the greater the attraction to the negative ion., which leads to more energy being released when the ions come together. The energy used is ionization energy. When the energy is lost, the extra positive charge gathers the electrons and the electron cloud to contract even more. [14]

After the bond is made, electronegativity is used to find out what type of bond a bond is. [15] Electronegativity is a property that an atom shows when it is bonded to another atom; it shows how strong an atom attracts electrons to itself when bonded to another atom and its highest value is 4.0. By doing so, it is determined whether or not the atoms are evenly sharing atoms. If the electrons being "shared" are unevenly distributed, and there are differences are greater than 2.1, the bond formed is called an ionic bond. [16]

When the ionic bond takes place, anions are typically packed together with the ions scattered throughout it. [17]The ionic bond results in the same way as a covalent bond; both electrons are close to the nuclei, and the attractions combine the nuclei together[18]

Properties

The properties of ionic compounds is that the adjacent ions are arranged in a lattice structure. [19] They have higher melting and boiling points than covalent compounds and dissolve easily in water. [20] Ionic compounds are also brittle and are sometimes electricity conductors [21] Ionic compounds dissolve easily in water and other polar solvents. When in a solution, ionic compounds easily conduct electricity because they can move around more freely. [22] Ionic solids have electrons in fixed positions around the atoms, which make them poor electrical conductors. Ionic compounds tend to form crystalline solids with high melting temperatures. Ionic compounds are solid due to the intermolecular forces, forces between molecules. [23] Because of this, the charges on the ions are directly proportional to the strength of the ionic bonds and the sizes of the ions are inversely proportional to the strength of the ionic bonds. [24]

Bond Strength

Unlike other bonds, an ionic bond is very stable, because of the attractions between cations and anions.[25]It is considered by chemist to be the strongest bond, when there is not any water present. When water is present, the ionic bond is weak, such as in the biological system. [26] The bonds are so strong that large quantities of energy are needed to take these bonds apart. [27]

References

  1. ↑ (2009). Ionic Bond. Retrieved February 6, 2009, from http://www.historyoftheuniverse.com/ionicbon.html
  2. ↑ (2009). Ionic Bond. Retrieved February 6, 2009, from http://www.historyoftheuniverse.com/ionicbon.html
  3. ↑ (2009).Ionic bond: Facts, Discussion Forum, and Encyclopedia Article. Retrieved February 6, 2009, from http://www.absoluteastronomy.com/topics/Ionic_bond
  4. ↑ (2009).Ionic bond: Facts, Discussion Forum, and Encyclopedia Article. Retrieved February 6, 2009, from http://www.absoluteastronomy.com/topics/Ionic_bond
  5. ↑ Ionic Bonds. Retrieved February 5, 2009 from http://www.promotega.org/UGA06004/ionic_bonds.html
  6. ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company. pg.360
  7. ↑ Ionic and Covalent Bonds. Retrieved February 5, 2009 from http://www.western.edu/faculty/jryter/chem101/Unit5/page3.htm
  8. ↑ Capri, A. (1999). Retrieved February 5, 2009 from http://web.jjay.cuny.edu/~acarpi/NSC/5-bonds.htm
  9. ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company. pg.360, 369
  10. ↑ Clark, J. (2000). Ionic (electrovalent) Bonding. Retrieved February 5, 2009, from http://www.chemguide.co.uk/atoms/bonding/ionic.html
  11. ↑ Lower, S. (2007). Chemical Bonds: covalent or ionic or what?. Retrieved February 5, 2009, from http://www.chem1.com/acad/webtut/bonding/polcov.html
  12. ↑ Lower, S. (2007). Chemical Bonds: covalent or ionic or what?. Retrieved February 5, 2009, from http://www.chem1.com/acad/webtut/bonding/polcov.html
  13. ↑ Molecular Bonding. Retrieved February 5, 2009 from http://library.thinkquest.org/10429/high/bonding/bonding.htm
  14. ↑ Sibert, G. Note son Ionic Bonding. Retrieved February 5, 2009 from http://www.files.chem.vt.edu/RVGS/ACT/notes/Notes-Chapter_10.html
  15. ↑ Lower, S. (2007). Chemical Bonds: covalent or ionic or what?. Retrieved February 5, 2009, from http://www.chem1.com/acad/webtut/bonding/polcov.html
  16. ↑ Damelin, D. (2007). Ionic and Covalent Bonds Overview. Retrieved February 5, 2009, from http://chemsite.lsrhs.net/ChemicalBonds/electronegativity.html
  17. ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company. pg.369
  18. ↑ Lower, S. (2007). Chemical Bonds: covalent or ionic or what?. Retrieved February 5, 2009, from http://www.chem1.com/acad/webtut/bonding/polcov.html
  19. ↑ Clark, J. (2000). Ionic (electrovalent) Bonding. Retrieved February 5, 2009, from http://www.chemguide.co.uk/atoms/bonding/ionic.html
  20. ↑ Ionic Bonds. Retrieved February 5, 2009 from http://www.promotega.org/UGA06004/ionic_bonds.html
  21. ↑ Ionic and Covalent Bonds. Retrieved February 5, 2009 from http://www.western.edu/faculty/jryter/chem101/Unit5/page3.htm
  22. ↑ Intermolecular Forces of Attraction. Retrieved February 5, 2009, from http://www.library.thinkquest.org/C006669/data/Chem/bonding/inter.html
  23. ↑ Carpi, A. (2003).Chemical Bonding. Retrieved February 5, 2009 from http://www.visionlearning.com/library/module_viewer.php?mid=55
  24. ↑ Intermolecular Forces of Attraction. Retrieved February 5, 2009, from http://www.library.thinkquest.org/C006669/data/Chem/bonding/inter.html
  25. ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company. pg.360, 369
  26. ↑ Chemical Bonds. Retrieved February 5, 2009 from http://www.biology.lsu.edu/introbio/tutorial/CHEM-TUTORIAL/chemtutorial/Bonds.html
  27. ↑ Zumdahl, S.S., Zumdahl, S. L., DeCoste, D. J. (2006). World of Chemistry. Houghton Mifflin Company. pg.369


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