Chem 210 final review

Chem 210 final review - Chem 210 Final review Exam notes...

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Chem 210 Final review Exam notes Test o Change in entropy, free energy o Standard entropy o Calc ∆H, ∆S with given ∆G CHP 12 Nature of electronic band structure o How it is different in metals, semiconductors and insulators o Use molecular orbital principles Examples of metals, semiconductors, and insulators o Metals Alloys themoelectrics o Semiconductors Optoelectronics photovoltaics o Insulators ceramics Elements in periodic table that are natural semiconductors o Types of simple compounds with semiconducting properties How “doping” materials with controlled amounts of impurity atoms can result in semiconducting properties o Distinguish btwn p-type and n-type semiconductors Define term superconductivity o Examples of superconducting materials including superconducting ceramic oxides Superconducting transition temp, T c o Explain why it is an important property of superconducting materials Meissner effect Materials for optics o How some semiconductor devices are used as light emitting diodes and their importance Difference btwn Polymers and Biomaterials What is meant by the terms polymer and monomer o Examples o How certain types of polymers react to changes in temp How a polymer is formed from monomers o Via addition polymerization
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o Via condensation polymerization Process of cross-linking in polymers o How it affects polymer properties Temp o Solubility of solid solutes in liquid solvents increases with increasing temp o Opposite is true with gases Ways of expressing concentration o Mass percentage, ppm, ppb o All methods involve quantifying amount of solute per amount of solvent/solution o Amounts/measures are masses, moles, or liters o Qualitatively solutions are dilute/concentrated o Mass % of component = (mass of component in solution)/(total mass of solution) *100 o CHP 13 PART 1 Energy changes in solutions o 3 processes affect the energetics of the process (H solution ) Separation of solute particles (requires energy = positive) ∆H1 Uniform to scatter Separation of solvent particles (requires energy = positive) ∆H2 Non-uniform to scatter Formation of solute-solvent interactions (releases energy b/c attracting molecules = is the energy greater or less than the other two number will depend on if it’s positive or negative; greater = warmer) Add the strengths together Look at diagram pg 5 Look at problem example pg 6 why do endothermic processes occur? o Enthalpy is a part of the picture Ex: mash potatoes and peas for entropy Less work to mix them More work to separate them Disappearing doesn’t mean dissolving o Disappear = not in solution, do not mix with solvent (a reaction) o Dissolution = physical change; you can get back the original solute by evaporating solvent (called re-crystallization) 3 types of solutions o saturated not stable rate of dissolving and something else becomes the same
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This note was uploaded on 03/17/2011 for the course CHEM 210 taught by Professor Hirzy during the Spring '10 term at American.

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Chem 210 final review - Chem 210 Final review Exam notes...

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