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<note version="0.3" xmlns:link="http://beatniksoftware.com/tomboy/link" xmlns:size="http://beatniksoftware.com/tomboy/size" xmlns="http://beatniksoftware.com/tomboy">
<title>Chapter 11</title>
<text xml:space="preserve"><note-content version="0.1">Chapter 11
<size:huge>Intermolecular Forces, Liquids, and Solids</size:huge>
<size:large>States of Matter</size:large>
<list><list-item dir="ltr">fundamental different between states is the distance between them
</list-item><list-item dir="ltr">Condensed phases
<list><list-item dir="ltr">Solid and liquid states
</list-item></list></list-item><list-item dir="ltr">states depend on temperature
</list-item><list-item dir="ltr">pressure depends on two antagonistic entities
<list><list-item dir="ltr">the kinetic energy of the particles
<list><list-item dir="ltr">gas has highest motion thusly most pressure
</list-item></list></list-item><list-item dir="ltr">the strength of the attractions between the particles</list-item></list></list-item></list>
<size:large>Intermolecular Forces</size:large>
<list><list-item dir="ltr">attractions between molecules are not nearly as strong as the intermolecular attractions that hold compounds together
</list-item><list-item dir="ltr">they become closer when they get colder
</list-item><list-item dir="ltr">intermolecular attractions are always weaker than ionic and covalent bonds</list-item></list>
<size:large>London Dispersion Forces</size:large>
<list><list-item dir="ltr">When helium atoms cool down, it changes shape
<list><list-item dir="ltr">moves all of its protons to one side
</list-item><list-item dir="ltr">the protons are attracted to the electrons
</list-item><list-item dir="ltr">electrons do not revolve around the nuclceous
</list-item></list></list-item><list-item dir="ltr"><highlight>all atoms and molecules go through LDF</highlight>
</list-item><list-item dir="ltr">the weakest intermolecular attraction
</list-item><list-item dir="ltr">they are dipole - <link:internal>Chapter 6</link:internal>
</list-item><list-item dir="ltr">polarization
<list><list-item dir="ltr">tendency of an electron cloud to distort in this way [ppt]</list-item></list></list-item></list>
<size:large>Factors Affecting London Forces</size:large>
<list><list-item dir="ltr">shape of the molecule affects the strength of dispersion forces
<list><list-item dir="ltr">long, skinny molecules (like n-pentance then to have stronger dispersion forces than short, fat ones (like neopentance) - <link:internal>Chapter 2</link:internal>
</list-item><list-item dir="ltr">due to an increased surface are in n-pentane
</list-item><list-item dir="ltr">skinny chains have more surface area to give more force
</list-item></list></list-item><list-item dir="ltr">Increase with increased molecular weight
<list><list-item dir="ltr">the higher the molecular weight makes it harder to escape all the bonds (boiling point)
</list-item><list-item dir="ltr">larger atoms haver larger electron clouds which are easier to polarize</list-item></list></list-item></list>
<size:large>Dipole-Dipole Interations</size:large>
<list><list-item dir="ltr">molecules that have permanent dipoles are attracted to each other
<list><list-item dir="ltr">the postive end attracted to a negative end and vise versa
</list-item></list></list-item><list-item dir="ltr">the more polar the molecule, the higher is its boiling point
<list><list-item dir="ltr">the more polar, the more difficult they are to break, the higher boiling point
</list-item><list-item dir="ltr">electronegativity - <link:internal>Chapter 6</link:internal></list-item></list></list-item></list>
<size:large>Hydrogen Bonding</size:large>
<list><list-item dir="ltr">the dipole-dipole interactions experienced when H is bonded to N, O, or F are unusually strong
</list-item><list-item dir="ltr">H2O have a higher D-D attraction then HCl because of the Hydrogen Bonding
</list-item><list-item dir="ltr">H2O and NH3 are Hydrogen bonded because they both have a H and N, O, or F
</list-item><list-item dir="ltr">shape of snowflake depends on temperature
<list><list-item dir="ltr">the temperature depends how they bond
</list-item><list-item dir="ltr">geometry - <link:internal>Chapter 9</link:internal>
</list-item></list></list-item><list-item dir="ltr">a stronger D-D attraction</list-item></list>
<size:large>Ion-Dipole Interactions</size:large>
<list><list-item dir="ltr">NaCl dissociates in H20 very well because of the massive amount of O for Na and H for Cl fight for it
</list-item><list-item dir="ltr">strongest interaction
</list-item><list-item dir="ltr">ionic (<link:internal>Chapter 2</link:internal>)substance dissolving in polar substance</list-item></list>
<size:large>Difference between Diamond and Graphite?</size:large>
<list><list-item dir="ltr">Diamond is tetrahedral
<list><list-item dir="ltr">very strong bond
<list><list-item dir="ltr">covalent bond?
</list-item></list></list-item><list-item dir="ltr">overlapped so nicely it is strong
</list-item></list></list-item><list-item dir="ltr">Graphite
<list><list-item dir="ltr">covalent bonding very strong</list-item></list></list-item></list>
<size:large>Viscosity</size:large>
<list><list-item dir="ltr">resistance of a liquid to flow
</list-item><list-item dir="ltr">increases with stronger intermolecular forces
</list-item><list-item dir="ltr">decreases with higher temperature</list-item></list>
<size:large>Surface Tension</size:large>
<list><list-item dir="ltr">H2O has strong surface tension due to strong intermolecular forces</list-item></list>
<size:large>Phase Changes
</size:large>
<size:large>Vapor Pressure</size:large>
<list><list-item dir="ltr">at any temperature some molecules in a liquid have enough energy to escape
</list-item><list-item dir="ltr">as the temperature rises, the fraction of molecules that have that enough energy to escape increases
</list-item><list-item dir="ltr">at all points, liquid is trying to escape
</list-item><list-item dir="ltr">as more molecules try to escape, the more the pressure increases
</list-item><list-item dir="ltr">equilibrium
<list><list-item dir="ltr">point at which the escape and the pressure of atmospheric pressure is equal
</list-item></list></list-item><list-item dir="ltr">boiling point
<list><list-item dir="ltr">the temperature at which it's vapor pressure equals atmospheric pressure
</list-item><list-item dir="ltr">the less atmospheric pressure, the lower the boiling point
</list-item><list-item dir="ltr">point at which its at equilibrium
</list-item><list-item dir="ltr">normal boiling point = 760 torr
</list-item></list></list-item><list-item dir="ltr">vaporization
<list><list-item dir="ltr">past boiling point</list-item></list></list-item></list>
<size:large>Phase Diagrams</size:large>
<list><list-item dir="ltr">display the state of a substance at various pressures and temperatures and the places where equilibria exist between phases
</list-item><list-item dir="ltr">to get all three phases at once
<list><list-item dir="ltr">give it slightly about 0 C and drop the pressure to almost 0
<list><list-item dir="ltr">due to the strong van der Waals forces between water molecules
</list-item></list></list-item><list-item dir="ltr">triple point
</list-item></list></list-item><list-item dir="ltr">a lot of energy is used to phase change and not put into atmosphere as much</list-item></list>
<size:large>Heat of Fusion</size:large>
<list><list-item dir="ltr">energy required to melt a solid
</list-item><list-item dir="ltr">/\H sub f
</list-item><list-item dir="ltr">H20
<list><list-item dir="ltr"><highlight>6.01 KJ / mol = 6.01 KJ / 18 g</highlight></list-item></list></list-item></list>
<size:large>Heat of Vaporization</size:large>
<list><list-item dir="ltr">energy required to vaporize a liquid
</list-item><list-item dir="ltr">/\H sub {vap}
</list-item><list-item dir="ltr">H2O
<list><list-item dir="ltr">40.7 KJ / mol = 40.7 KJ / 18g</list-item></list></list-item></list>
<size:large>Phase Change Calculate</size:large>
<list><list-item dir="ltr">EX:
<list><list-item dir="ltr">[notebook]</list-item></list></list-item></list>
<size:large>Covalent-Network and Molecular Solids</size:large>
<list><list-item dir="ltr">graphite is an example of a molecular solid, ion which atoms are held together with van der Waals forces
<list><list-item dir="ltr">tend to be softer and have lower melting points</list-item></list></list-item></list>
<size:large>Solids</size:large>
<list><list-item dir="ltr">crystalline
<list><list-item dir="ltr">highly ordered arrangement
</list-item></list></list-item><list-item dir="ltr">amorphous
<list><list-item dir="ltr">no particular order in the arrangement of particles
</list-item></list></list-item><list-item dir="ltr">packing
<list><list-item dir="ltr">ions pack themselves so as to maximize the attractions and minimize repulsions between the ions
</list-item><list-item dir="ltr">must repeat / have pattern
<list><list-item dir="ltr">ABAB
<list><list-item dir="ltr">hexagonal close-packing (HCP)
</list-item></list></list-item><list-item dir="ltr">ACBA
<list><list-item dir="ltr">cubic close-packing (CCP)</list-item></list></list-item></list></list-item></list></list-item></list>
<size:large>Types of Bonding in Crystalline Solids</size:large>
<list><list-item dir="ltr">if you have covalent bonds, you always have covalent network
</list-item><list-item dir="ltr">if you have electrostatic attractions, you always have ionic network</list-item></list>
<size:large>Metallic Solids</size:large>
<list><list-item dir="ltr">metals are not covalently bonded
<list><list-item dir="ltr">but attractions between atoms are too strong to be van der Waals
</list-item></list></list-item><list-item dir="ltr">atoms share the electrons between all
<list><list-item dir="ltr">try to trow the electrons as far as possible</list-item></list></list-item></list>
<size:large>Crystalline Solids</size:large>
<list><list-item dir="ltr">perfect ruby
<list><list-item dir="ltr">Al2O3
</list-item></list></list-item><list-item dir="ltr">because of the ordered in a crystal, we can focus on the repeating pattern of arrangement (unit cell)</list-item></list>
</note-content></text>
<last-change-date>2010-08-03T02:01:20.6526090-04:00</last-change-date>
<last-metadata-change-date>2011-02-02T19:33:20.8650060-05:00</last-metadata-change-date>
<create-date>2010-09-02T16:35:30.9566150-04:00</create-date>
<cursor-position>42</cursor-position>
<width>424</width>
<height>589</height>
<x>0</x>
<y>0</y>
<tags>
<tag>system:notebook:CHEM 106</tag>
</tags>
<open-on-startup>False</open-on-startup>
</note>
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