CHEM 110 Lecture Notes - Lecture 13: Covalent Bond, Polarizability, Ammonia
28 Jun 2018
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CHEM 120: CHAPTER 11 LIQUIDS, SOLIDS, PHASE CHANGES:
Phase: physically distinct homogenous part of a system compromised of 1 physical state of matter (wave
functions from 110 on the macroscopic scale)
-Plasm as : (lightning) electron s are mobile, ionized nuclei at high
temp e r a t ur e s , abun da n t form of ma tt er
T = 2/3 NA/R(1/2mu 2) State is determined by interactions between particles
Entropy: measure of disorder within a system (gases can occupy microstates, move rotationally and
translationally so it has lots of disorder, gases > liquids > solids) increase T increase disorder
Enthalpy: stronger intermolecular forces larger enthalpy, attractive intermolecular forces cause the
particles to rearrange themselves going from gas – liquid – solid by enthalpy changes, type of IF
determines the magnitude of
Solids: large collection of particles, fixed shapes & volumes, less dense than water
Liquids: less viscosity than solids moderate flow and low compressibility (ice is most dense at 4)
Gas: variable shapes and volumes, high compressibility and high flow
Intermolecular Forces: small charges that are separated, what holds a liquid and solid together,
responsible for the existence of condensed states (relatively weak in comparison to bonding forces)
PE = q1q2/40r
The distance across which the PE is interaction is felt (SLIDE GRAPH)
-PE means you are forming a bond
Non-polar molecules that are close to each other will exhibit dispersion forces which will matter more
relevant the closer they are
-Long distan ce s Ionic dominates
-Short dista nc e s Dispersion dominates
-You can not go pas t 1/r 12 because they are too close, causing repulsion
Ion-Ion interactions: some of the strongest forces between molecules
-Non- directional; eac h ion inter act s equ ally strongly with all its neighbo ur s
(1/r)
-Calculate d as crystal lattice en er gy, wher e the ions form exten d e d repe atin g
units
-Opposit ely char ge d ions attrac t
PE = |Z A|ZB|/r
ZA & ZB magnitudes of the charges on the atoms (i.e. NA+ z = 1)
The attachment of H2O to solute particles Is called hydration (due to polar character of H2O)
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Document Summary
Chem 120: chapter 11 liquids, solids, phase changes: Phase: physically distinct homogenous part of a system compromised of 1 physical state of matter (wave functions from 110 on the macroscopic scale) T = 2/3 na/r(1/2mu 2) state is determined by interactions between particles. Entropy: measure of disorder within a system (gases can occupy microstates, move rotationally and translationally so it has lots of disorder, gases > liquids > solids) increase t increase disorder. Enthalpy: stronger intermolecular forces larger enthalpy, attractive intermolecular forces cause the particles to rearrange themselves going from gas liquid solid by enthalpy changes, type of if determines the magnitude of. Solids: large collection of particles, fixed shapes & volumes, less dense than water. Liquids: less viscosity than solids moderate flow and low compressibility (ice is most dense at 4) Gas: variable shapes and volumes, high compressibility and high flow.
