Chem 16 2nd LE Notes

Chem 16 Notes
UPD
Should only be a supplement to discussions

Table of Contents*
[A] Lecture
[1] Thermodynamics
[2]Energy
[3]Enthalpy
[4]Hess's Law
[5]Determining Enthalpy
[6]Heat Capacity
[7]Calorimetry
[8] Entropy
[9] Gibb's Free Energy
[10] Waves
[11] Quantum Theory
[12] Quantum Numbers
[13] Electron Configuration
[14] Periodic Table
[15] Periodic Trends
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[16] Chemical Bonding
[17] Formal Charge
[18] Resonance Structure
[19] Bonds
[20] VSEPR
[22] Valence Bond Theory
[22] Molecular Orbital Theory
[B]Lab
[1] Corrosion
[2] Oxidation Reduction Reactions
[3] Calorimetry
[4] Qualitative Analysis
[5] Flame Test
[6] Molecular Model
*(Ctrl + F the roman numeral to skip to that part. Ex: [B.3])

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[A.1] Thermodynamics
Thermodynamics
 “thermo” = heat
 “dynamics” = movement
 It has 3 parts
 system
 the object being observed
 surroundings
 everything not part of the system
 boundary
 the division between system and surrounding
 Universe
 the sum of the 3 parts
 Internal Energy
 energy found within the universe
 sum of all Potential Energy (PE), Kinetic Energy (KE), and energy is general
 Δ E=E final−E init= E product−E reactant

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[A.2]Energy
Energy
 capacity for heat and/or work
 heat
 symbolized by q
 movement of energy due to the difference in temperature
 when a system is “cold”, it means it has a higher temperature and the heat is leaving the system
 When a system is “hot”, it means the surrounding has a higher temperature and the heat is entering the system
 work
 symbolized by w
 can done by or to the system
 When work is done by the system, there is a release of energy
 When work is done to the system, there is an absorption of energy
 Δ E=q+w
 sign depends on change
 +q = endo
 -q = exo
Properties of Energy
 1st Law
 energy is constant
 Δ E univ=Δ E sys+Δ E surr =0
 SI unit is Joules (J)
[(kg)(m)2 ]
1
s2

 1 cal = 4.184 J
 Capital Letter(Cal) = kilo (kilocal)
 State function
 doesn't care on process, just