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Chemical Compounds

Lesson 7. Chemical Compounds. Lesson Outcome. B8: I am able to read and interpret chemical formulas for compounds of two elements, and give the IUPAC name and common names of compounds. B9: I am able to distinguish between ionic and molecular compounds.

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Chemical Compounds

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  1. Lesson 7 Chemical Compounds

  2. Lesson Outcome • B8: I am able to read and interpret chemical formulas for compounds of two elements, and give the IUPAC name and common names of compounds. • B9: I am able to distinguish between ionic and molecular compounds. • I am able to identify examples of combining ratios/numbers of atoms per molecule found in some common materials, and use information on ion charges to predict combining ratios in ionic compounds or two elements. • I am able to assemble and draw simple models of molecular and ionic compounds.

  3. Compounds • Elements combine to forms compounds. • There are two types of compounds: • Ionic Compounds • Molecular Compounds

  4. Ionic Compounds • Made up of a metal and non-metal • An element from both sides of the staircase • These elements give and take electrons to become a compound.

  5. Molecular Compounds • Made up of a non-metal and non-metal • Both elements are found on the right side of the stair case. • The elements share electrons to form a compound.

  6. Ionic or Molecular • NaCl • CO2 • MgO • NH3 • CH4 • FeCl2 • H2O • NaOH

  7. Chemical Formulas • Uses symbols and numbers to represent the number and type of each atom found in the compound. • Ex: H2O

  8. Practice Time! • What type and how many atoms?

  9. Diatomic Compounds • Di = 2 • These are compounds that have two of the same elements. • H O F Br I N Cl • H2 • O2 • F2 • Br2 • I2 • N2 • Cl2

  10. Naming Molecular Compounds • 1. Write the entire name of the first element. • 2. Change the ending on the name of the second element to “ide” • 3. Use a prefix to indicate the number of each type of atom in the formula • 1 = mono • 2= di • 3 = tri • 4= tetra • Note: the prefix mono is only used with the second element

  11. Practice • CO • CCl4 • SiO2 • SO2 • H2O • NH3 • CH4

  12. Practice • Phosphorous trihydride • Carbon tetrachloride • Nitrogen dioxide • Sulfur trioxide

  13. Naming Ionic Compounds • 1. Write the name of the metal in the compound first. • 2. Write the non-metal element second and change the ending to “ide” • 3. Subscripts indicate the ratio of ions in the compound: • Ex: CaCl2 = 1:2 ratio • Note: we do not use prefixes for ionic compounds

  14. Practice • NaCl • NaF • LiCl • ZnS • MgO • K2S • Na2O

  15. Making Ionic Formulas from a Name • 1. write the symbols for both elements. • 2. swap and drop the charges • 3. reduce

  16. Trends • What charges to metals always have? • What charges do non-metals always have?

  17. Practice • Sodium chloride • Potassium oxide • Magnesium nitride • Beryllium oxide • Cesium sulfide • Lithium bromide

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