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Conductivity of Ionic vs Covalent Compounds in Lab 5.4

Learn about the conductivity of substances and the difference between ionic and covalent compounds. Discover why some solutions conduct while others do not. Understand the naming conventions for both types of compounds.

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Conductivity of Ionic vs Covalent Compounds in Lab 5.4

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  1. Lab 5.4 Ionic vs Covalent Compounds

  2. Conductivity • For a substance to conduct it must have: 1. Particles that are free to move 2. Charged Particles

  3. Conductivity of SolutionsSalt vs. Sugar Salt Sugar The particles must be charged. The particles must be neutral (not charged). Salt and Sugar both dissolve in water, forming clear solutions. During dissolving, the particles of the solid salt or sugar became free to move. So, while both have met that requirement of conductivity, only salt meets the 2nd requirement.

  4. Solutions that Conducted

  5. Solutions that Conduct • Ionic Compounds: • Composed of metal and nonmetal elements • Composed of charged particles called ions • Ion = an atom that has become charged

  6. Negative Ion Positive Ion Ionic bond: attraction between the oppositely charged ions In the solid salt, there are charged particles-the ions, but they are not free to move Dissolving Ions are free to move in the salt solution

  7. Dissolving an Ionic Compound • Watch the following animation: Dissolving an ionic compound Dissolving an ionic compound #2

  8. + + + + + - - - - - The ionic bond that once held the oppositely charged ions together is now broken. Na+ Cl- Water particles are not shown. Each ion is surrounded by many water particles, keeping them separate and no longer attracted to each other.

  9. Naming Ionic Compounds • Metal name goes 1st with no change. • Nonmetal name is changed to an “-ide” ending. • Sodium chloride, NOT sodium chlorine • Aluminum oxide, NOT aluminum oxygen

  10. Solutions that Don’t Conduct

  11. Solutions that do NOT conduct • Covalent Compounds: • Composed of only nonmetal elements. • Composed of neutral particles called molecules. • Molecule = group of atoms bonded together that acts as a single unit (particle)

  12. Molecules Ammonia (NH3) Water (H2O)

  13. Each individual molecule is “intact”; the atoms are still bonded as a group. The covalent bond between the nm atoms has not been broken. NH3

  14. Naming Covalent Compounds • Element listed first in the formula is named first with no change. • 2nd element is changed to “-ide” ending AND is preceded by a prefix. • Carbon dioxide, NOT carbon oxide. • Carbon tetrachloride, NOT carbon chloride.

  15. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

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