Lecture 7.3- Metallic Bonds


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Section 7.3 lecture for Honors & Prep Chemistry

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Lecture 7.3- Metallic Bonds

  1. 1. Bellwork- Determine Formula <ul><li>What is the formula of the compound formed between the following ions. </li></ul><ul><ul><ul><li>Calcium ion and bromide ion </li></ul></ul></ul><ul><ul><ul><li>Potassium ion and sulfide ion </li></ul></ul></ul><ul><ul><ul><li>Aluminum ion and selenide ion </li></ul></ul></ul>
  2. 2. Lecture 7.3 – Metallic Bonds <ul><li>Ionic bonds are formed between a metal cation and a non-metal anion. </li></ul>Metallic bonds are formed between two or more metal cations.
  3. 3. <ul><li>The attraction of these free electrons to the metal cations is called a metallic bond. </li></ul>Sea of Valence Electrons Model <ul><li>Metal atoms release their valence electrons into a sea of valence electrons shared by all of the metal atoms. </li></ul>
  4. 4. Atomic View of Metallic Bonding A Group 2 metal Each atom releases its two valence electrons into a pool of electrons to be shared by all of the metal atoms.  
  5. 5. <ul><ul><ul><li>Metals are ductile—they can be drawn into wires. </li></ul></ul></ul>
  6. 6. <ul><ul><ul><li>A force can change the shape of a metal. A force can shatter an ionic crystal. </li></ul></ul></ul>
  7. 7. <ul><ul><li>See how metallic bonding explains some physical properties of metals. </li></ul></ul>
  8. 8. <ul><li>Metals are good electrical conductors because the valence electrons are free to travel. </li></ul>
  9. 9. Atomic View of Metallic Bonding <ul><li>Bonding in metals is not rigid. </li></ul><ul><li>The same ability to reorganize explains why metals can be pulled into long, thin wires. </li></ul><ul><li>As a metal is struck by a hammer, the atoms slide through the electron sea to </li></ul>new positions while continuing to maintain their connections to each other.
  10. 10. <ul><ul><ul><li>Metal atoms are arranged in very compact and orderly patterns. </li></ul></ul></ul>
  11. 11. <ul><ul><ul><li>These tomatoes have a closed-packed arrangement. Similar arrangements can be found in the crystalline structure of metals. </li></ul></ul></ul>
  12. 12. <ul><ul><ul><li>Alloys are mixtures composed of two or more elements, at least one of which is a metal. </li></ul></ul></ul><ul><ul><ul><ul><li>Alloys are important because their properties are often superior to those of their component elements. </li></ul></ul></ul></ul>
  13. 13. <ul><ul><ul><li>Bicycle frames are often made of titanium alloys that contain aluminum and vanadium. </li></ul></ul></ul>
  14. 14. <ul><ul><ul><li>The most important alloys today are steels. </li></ul></ul></ul><ul><ul><ul><li>Steels have a wide range of useful properties, such as corrosion resistance, ductility, hardness, and toughness. </li></ul></ul></ul>
  15. 15. <ul><ul><li>1. The valence electrons of metals can be modeled as </li></ul></ul><ul><ul><ul><li>a body-centered cube. </li></ul></ul></ul><ul><ul><ul><li>octets of electrons. </li></ul></ul></ul><ul><ul><ul><li>a rigid array of electrons. </li></ul></ul></ul><ul><ul><ul><li>a sea of electrons. </li></ul></ul></ul>7.3 Section Quiz.
  16. 16. <ul><ul><li>2. In most metals, the atoms are </li></ul></ul><ul><ul><ul><li>free to move from one part of the metal to another. </li></ul></ul></ul><ul><ul><ul><li>arranged in a compact and orderly pattern. </li></ul></ul></ul><ul><ul><ul><li>placed at irregular locations. </li></ul></ul></ul><ul><ul><ul><li>randomly distributed. </li></ul></ul></ul>7.3 Section Quiz.
  17. 17. <ul><ul><li>3. Alloys are important because they </li></ul></ul><ul><ul><ul><li>are pure substances. </li></ul></ul></ul><ul><ul><ul><li>are the ores from which metals can be refined. </li></ul></ul></ul><ul><ul><ul><li>can have properties superior to those of their components. </li></ul></ul></ul><ul><ul><ul><li>are produced by the combustion of metals. </li></ul></ul></ul>7.3 Section Quiz.