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Materials science

AP Chemistry Zumdahl 7E Chapter 10 Notes

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Chemistry
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Chemical bonding
Gases
Materials science
intermolecular forces
Chemical properties
Properties of water
Chemical bond
Molecular solid
Hydrogen bond
Vapor pressure
Enthalpy of vaporization
Boiling point

1 Chapter 10 - Liquids and Solids 10.1 Intermolecular Forces A. Dipole-Dipole Forces 1. Attraction between molecules with dipole moments a. Maximizes (+) ----- ( - ) interactions b. Minimizes (+) ----- ( + ) and (-) ----- ( - ) interactions 2. About 1% of strength of ionic bonds a. Unimportant in gas phase due to distance between molecules B. Hydrogen Bonding 1. Special dipole-dipole attraction a. Hydrogen covalently bonded to highly electronegative elements (N, O, F) has a higher than normal d+ charge 2. Bond strength is higher than other dipole-dipole attractions 3. Important in the bonding of molecules such as water and DNA C. London Dispersion Forces 1. Instantaneous dipoles a. Random movement of electrons can create a momentary

Crystalline_Solids

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Chemistry
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Chemistry
Physics
Crystallography
Materials science
Diffraction
Condensed matter physics
Optics
Ionic radius
Cubic crystal system
Pauling's rules
Coordination number
Powder diffraction

Crystalline Solids Crystal Lattice ? A 3D array of points where each point has an identical environment. Unit Cell ? The repeating unit (a unit cell is to a crystal, like a ?brick? is in a house). In a given crystal all unit cells are identical. CaF2 Unit Cell Large cation & Large anion r(Cation)/r(Anion) ~0.72 Small cation & Large anion r(Cation)/r(Anion) ~0.3 Cation Anion Anions and cations want to stay in contact with each other, but when the cation becomes much smaller than the anion, anion-anion contacts prevent this. The solution is to lower the coordination number Ionic radii and coordination number Radius Ratio Rules r(cation)/r(anion) Coordination Number Coordination Geometry ? 0.73 8 Cube ? 0.41 6 Octahedron ? 0.22 4 Tetrahedron ? 0.15 3 Trigonal Planar

Chapter 10

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Chemistry
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Chemistry
Thermodynamic properties
Chemical engineering
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Phase transitions
Enthalpy
Enthalpy of vaporization
Vapor pressure
Phase
Enthalpy of fusion
Dipole
Evaporation

Chapter 10 notes Claire Rafson 10.1-10.2 Intermolecular forces- occur b/w not in molecules. From solid to liquid to gas molecules remain in tact Forces: Dipole-dipole forces are forces that act between polar molecules Hydrogen bonding- strong form of dipole dipole with H and NOF London Dispersion- Present in all but ionic . noble gas and nonpolar and Polar. Big atom with a lot electrons LD can be stronger than dipole dipole Higher IMF = higher: surface tension, boiling/meltin point. Lower: vapor pressure Capillary action- polar liquids typically exhibit it 10.3- crystalline solids- highly regular arrangement of their components ionic and molecular amorphous solids- considerable disorder 10.5- Network atomic Solids- giant molecule Strong covalent bonds Silica- SiO2
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