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TYPES OF SOLIDS

TYPES OF SOLIDS. Molecular Solids. Small covalent compounds (non-metals ), covalently bonded i.e. CO 2 , CH 4 , H 2 O weakest of all of the solids but range in strength due to intermolecular forces. Properties & Explanation. Property Odour , Soft, Low m.p . Explanation Weak bonds.

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TYPES OF SOLIDS

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  1. TYPES OF SOLIDS

  2. Molecular Solids • Small covalent compounds (non-metals), covalently bonded • i.e. CO2, CH4, H2O • weakest of all of the solids but range in strength due to intermolecular forces

  3. Properties & Explanation Property • Odour, Soft, Low m.p. Explanation • Weak bonds

  4. Property: • Solubility Explanation: • Mostly insoluble (non-polar), to soluble (polar) • likes dissolve likes: PC cpds can dissolve in polar water

  5. Property: • Conductivity Explanation: • Can't conduct in any state– no free charges

  6. Metallic Crystals • i.e. Na, Fe, Au • Metallic bonding • made up of nuclei surrounded by a "sea" of valence e- that move freely (more valence e-, stronger attraction)

  7. Properties & Explanation Property • High to very high m.p. hard (typically) Explanation • Strong attractive forces

  8. Property: • High lustre Explanation: • Moving e- reflect light Property: • Solubility Explanation: • Insoluble, no free charges

  9. Property: • Conductivity Explanation: • Free movement of e- make metals conductive in the solid and molten state  since can't dissolve, they do not conduct electricity in water

  10. Ionic Crystals • Metals bonded to non-metals • i.e. NaCl, Cu(NO3)2, Al2O3 • oppositely charged particles attracted to each other to make bonds

  11. Properties & Explanation Property: • no odour, High m.p. Explanation: • Strong attractive forces

  12. Property: • Brittle Explanation: • Striking the crystal causes atoms to vibrate, same charged atoms get closer, repel, split the crystal

  13. Property: • Solubility Explanation: • Soluble in water since charged particles (likes dissolve likes)

  14. Property: • Conductivity Explanation: • Can conduct in aqueous or molten state since charges are then free to move

  15. Covalent Network Crystals • C(s), SiC(s), SiO2(s) • large 3D covalently bonded molecules • strongest of all types of solids • most are hard and have very high melting points

  16. Diamond vs. Graphite Properties of Diamonds: • Very Hard, don’t conduct electricity Explanation: • Carbon is in large 3D network of tetrahedrals – very strong! • no lone e- (all e- in bonds)  can’t conduct electricity

  17. Diamond

  18. Properties of Graphite: • Soft, conducts electricity Explanation: • Flat layers of trigonal planar carbons attracted to each other through London forces  weak! • Since C needs 4 bonds and only has 3, 1 e- left on each C that is free to move and conduct electricity

  19. Graphite

  20. Quartz (SiO2)

  21. Bucky Balls • Invented by Buckminster Fuller • Medical field • Catalysts • Batteries

  22. Nanotubes • Strengthening composites • Conductivity in plastics • Flat screen TV displays • Cancer treatments – drugs delivered to cancerous cells by nanotubes or they are sent to a part of the body and heated by radio waves causing the cells to explode

  23. Examples • Classify each of the following compounds as a type of solid: a) C2H6 b) SiO2 c) Mg d) CaCl2

  24. 2) A solid compound is shiny, malleable, conductive in the sold state and hard. What type of solid is it?

  25. 3) A solid compound is soluble in water, conducts electricity in water, has a high melting point and is brittle. What type of solid is this?

  26. Homework  • P273 #2, 5-7 • P276 #3,6,7,9

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