Chemical bonding

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Chemical bonding

  1. 1. 3 Types Of Bonding Ginah Santiago Pd 5
  2. 2. Introduction to Bonding <ul><li>Chemical bonds are formed by the interaction of electron between atoms. </li></ul><ul><li>Atoms form chemical bonds to become stable. </li></ul>
  3. 3. Ionic Bonding <ul><li>An ionic bond forms when one or more electrons from a metal transfers to a non-metal. </li></ul>
  4. 4. Ionic Bonding (cont.) <ul><li>Physical Properties associated with an ionic bond : High melting and boiling points, Ionic solids don’t conduct electricity and become insulators, Molten (liquid) ionic compounds conduct electricity. </li></ul>
  5. 5. Ionic Bonding (cont.) <ul><li>The energy, called Lattice energy, is given off when oppositely charged ions in the gas phase group and come together to form an ionic solid. </li></ul>
  6. 6. Covalent Bonds <ul><li>The Octet Rule is when a cation and an anion become stable when they bond with each other. </li></ul>
  7. 7. Covalent Bonds (cont.) <ul><li>Single- Formed by mutual sharing of only one electron pair between two atoms. </li></ul><ul><li>Double- Formed by the mutual sharing of two electron pairs between two atoms. </li></ul><ul><li>Triple- Formed by the sharing of three electron pairs. </li></ul>
  8. 8. Sigma <ul><li>A Sigma – Single bond </li></ul><ul><li>A Sigma and A Pi- Double bond </li></ul><ul><li>A Sigma and 2 Pi- Triple bond </li></ul>
  9. 9. <ul><li>As bond length increases, bond dissociation energy increases, direct relation. </li></ul>
  10. 10. Metallic Bonds <ul><li>Chemical bond between atoms in a metallic element. Formed by valance electrons that are moving freely through the metal lattice. </li></ul>
  11. 11. Metallic Bond (cont.) <ul><li>Conductivity of Electricity- When a metal is a solid or liquid, its able to conduct electricity. The delocalized electrons in the metal have the freedom to move in the solid lattice. They act as a charge carriers in the conduction of electricity. </li></ul>
  12. 12. Metallic Bond (cont.) <ul><li>Melting Points- Metals have high melting and boiling points because of the great strength of metallic bonding. The strength depends on the number of electrons in delocalized sea of electrons and the packing arrangement of a metal atoms. </li></ul>
  13. 13. Metallic Bonds (cont.) <ul><li>Alloys- A mixture of two or more metals. If two metals like calcium and sodium combined they will be considered an alloy. </li></ul>

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