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Chapter 6

Chapter 6. Chemical Bonds. Show second one. http://science.howstuffworks.com/periodic-table-videos-playlist.htm. Ionic Bonds Sec. 6.1. When elements react they tend to transfer electrons to become stable Ex. Na and Cl

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Chapter 6

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  1. Chapter 6 Chemical Bonds

  2. Show second one http://science.howstuffworks.com/periodic-table-videos-playlist.htm

  3. Ionic Bonds Sec. 6.1 • When elements react they tend to transfer electrons to become stable • Ex. Na and Cl • When ions form the charge changes from neutral because of a change in the number of protons or electrons. • Ex. Na+ and Cl-

  4. 1 2 3 4 5 6 7 Lose e- Gain/ Lose e- Gain e-

  5. Anion • Negative charge • Have the ending –ide • Ex. Cl- becomes chloride

  6. Cation • Positive charge • The name is the same as the element • Ex. Na+ is sodium

  7. Ionic Compounds • Shows the ratio of the atoms in the compound • Ex. NaCl • Ex. MgCl2 (2 Cl atoms needed)

  8. Properties of Ionic Compounds • Strong attraction of ions • High melting point • Not malleable

  9. Ionic Compounds • The name of the compound must distinguish it from other compounds of the same elements • The formula describes the ratio of the elements that make up the compound

  10. Naming Binary Compounds • They follow a predictable pattern of the cation followed by the anion • Remember: the anion will end in –ide • Ex. Figure 16 Common Anions

  11. Practice with compounds • Write the chemical formulas for the following compounds using their valence electrons to assist you… • Li and N K and P H and F • Al and P C and S Al and Br • C and Sn B and N Rb and Se • Answers • Li3N K3P HF • Al3P3(AlP) C2S4(CS2) AlBr3 • C4Sn4 (CSn) B3N3 (BN) Rb2Se

  12. Naming the compounds from previous slide • Li and N K and P H and F • Al and P C and S Al and Br • C and Sn Ba and C Rb and Se • Lithium nitride Potassium phosphide • Hydrogen fluoride Aluminum phosphide • Carbon sulfide Carbon Tinide • Aluminum Bromide Boron Nitride • Rubidium selenide

  13. Multiple Ions • The transition metals form more than one type of ion • Ex. Cu (I) with a 1+ charge and Cu (II) with a 2+ charge • The other elements have positive charges that are equal to their group number

  14. Polyatomic Ions • Many ions • Positive or negatively charged • Figure 19

  15. Writing Formulas for Ionic Compounds • Determine the ratio of elements needed in the compound by using the charges given. • Ex. Na has a 1+ charge and S has a 2- charge = Na2S • Practice Page 174

  16. Covalent Bonding 6.2 • Sharing electrons (Co) means to share • Ex. Hydrogen • Single bond between the elements H-H • H2 describes a molecule of Hydrogen • Many nonmetals exist as diatomic molecules • Ex. Cl2

  17. Multiple Covalent Bonding • Sharing multiple pairs of electrons • Ex. N2 has a triple bond Page 167

  18. Polar or Nonpolar Molecule? • If it has only two atoms, it is polar • If there are more than two atoms, the type of atoms and the shape determine whether the molecule is polar or nonpolar • H2O is polar because it has a bent shape • Polar attractions are greater than nonpolar

  19. Naming Molecular Compounds6.3 • The most metallic element appears first in the name • The name of the second will end in –ide • Ex. N2O4 – dinitrogen tetraoxide • NO2 – nitrogen dioxide • Prefixes for naming compounds is figure 20

  20. Metallic Bonds 6.4 • Metals become cations with a pool of shared electrons surrounding it • The attraction between the cation and the surrounding electrons is the metallic bond

  21. Properties of Metal • The ability to conduct and malleability are two properties of metal that are explained by the structure of the electrons around the metal • Figure 22 - malleability

  22. Alloys • Mixture of metals • Copper – when mixed with tin will produce bronze, and when mixed with zinc will produce brass • Steel – a mixture of iron and small amounts of carbon

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