1. Solids and Liquids
Chapter 14

2. Kinetic Molecular Theory
Solids-particles are highly ordered and packed closely together. They have slight vibrational movement. A solid maintains its shape regardless of the container.
Liquids-particles are more disordered and are spread further than in a solid. They more closely resemble solids than gases.

4. Phases Heat is added Heat is removed Endo Exo
Condensing-gas to liquid
Freezing-liquid to solid (0°C for water-freezing point)
Deposition-gas to solid (water vapor directly to ice)
Evaporation-liquid to gas (100°C for water-boiling point)
Melting-solid to liquid
Sublimation-solid to gas (dry ice directly to a gas)

5. It takes 7 times more energy to vaporize a mole of water than to melt a mole of water.

6. Phase Diagram of Water

7. One gram of ice has a greater volume than one gram of water.
liquid water
1.00g = 1.00g/mL
1.00mL
solid water
1.00g = 0.917g/mL
1.09mL

8. All phase changes are physical changes because a new substance is not created.

9. What keeps the molecules together?
Intramolecular forces (within the molecule)-holds the atoms of a molecule together
Ex: H bonds with O to make H2O
Intermolecular forces (between the molecules)-forces between molecules
Ex: H2O bonds are broken with other H2O molecules when making steam.

10. Intermolecular Forces
Hydrogen bonding-special type of strong dipole-dipole bond where H is bonded to a highly electronegative element Ex: H2S, HCl
Dipole-dipole attraction-polar molecules line up so the positive and negative poles attract (1% as strong as covalent or ionics)
London dispersion forces-forces that exist among noble gas atoms and nonpolar molecules (weakest force) Ex: H2, N2, I2

11. Intermolecular Forces: Hydrogen Bonding Forces
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12. Types of crystalline solids
Ionic-contains cations and anions, conduct electricity Ex: Salt (NaCl). Have high melting points.
Molecular-contains covalent bonds (molecules) Ex: Sugar (C12H22O11). Intermolecular forces are weak so they melt at low temperatures.
Atomic-1 element covalently bonded to itself Ex: Diamond (Carbon)

13. Structure of an Ionic Solid (NaCl)
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14. Molecular Solids Click in this box to enter notes.
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15. Comparison of a Molecular Compound and an Ionic Compound
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16. Metallic Solids Metals have strong, nondirectional bonding.
Electron sea model-metal atoms are located in a sea of valence electrons that are shared
Alloy-a substance that contains a mixture of elements and has metallic properties.

17. Alloys
Substitutional alloy-metal atoms are replaced by other metal atoms of similar size Ex: sterling silver (93% silver, 7% copper) Analogy: Substitute teacher
Interstitial alloy-some of the interstices (holes) among metal atoms are occupied by smaller atoms Ex: steel (carbon and iron) Analogy: Tutor

18. Electron Sea Model Click in this box to enter notes.
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