Chapter 12 Chapter 5 Intermolecular Forces Physical States .
Chapter 12Chapter 5Intermolecular forcesPhysical States of MatterChapter 12Section 12.3Physical States of Matter¾Three phases of matter– solidDefinite shape and volumesolid– liquidDefinite volume, shape ofcontainer– gasShape and volume ofcontainerliquidgasCertain forces keep the molecules together in solids and liquids1
Chapter 5Chapter 12Physical States of MatterChapter 12Physical States of Matter¾ Physical state determined by the relative strength ofcohesive and disruptive forces¾ Cohesive forces¾Intramolecular forcesIntermolecular Forces¾ Ion-Ion forces (ionic compounds)¾ Ion-Dipole Forces¾ Solvation/HydrationS l ti /H d ti¾Intermolecular forces¾Disruptive forces2
Chapter 12Chapter 12Section 12.3Chapter 12Intermolecular ForcesIntermolecular ForcesDipole moment and boiling point¾ Dipole-dipole forces¾ For compounds of similar mass, the boiling pointincreases with increasing dipole moment¾ Exists between polar molecules¾ This is a fairly weak force except when one atomis hydrogenδ Cδ Oδ Cδ Oδ Cδ O3
Chapter 12Chapter 12Intermolecular Forces¾Chapter 12Intermolecular ForcesHydrogen bond¾Molecules capable of hydrogen bonding¾Effect of hydrogen bondingHydrogen bonding and boiling point A particularly strong type of dipole-dipole interaction It exist between an electronegative atom and a hydrogen atombonded to another electronegative atom.δ δ ¾It is an especially strongattractive force due to thesmall size and mass ofhydrogen and the highelectronegativity of oxygenHδ HOHδ Hδ Oδ Hδ δ δ Oδ Oδ Hδ Oδ Hδ Oδ Hδ Hδ HHδ HHδ Hδ δ Oδ δ Oδ HH4
Chapter 12Chapter 12Intermolecular ForcesChapter 12Intermolecular Forces¾¾ Which of the following molecules can formhydrogen bonding?Intermolecular ForcesDipole-induced dipole force¾ Exists between a non-polar compound and a polarcompound¾ Polarization: the process of inducing a dipole.¾ Polarizability: the ease with which the electron cloud ofan atom or a molecule can be distorted.CH3CH2OH, CH3CHO, and CH3COOH¾ Larger the molar mass, the greater the polarizability ofthe moleculesSymmetrical distributionof electron clouds¾Polarizability of atomsSymmetry is lostRank the following molecules in the order of increasingpolarizabilityCl2, Br2, and I25
Chapter 12Chapter 12Intermolecular Forces¾Induced dipole-induced dipole (Londondispersion forces)¾ Exists between non-polar molecules¾ Very weak attractive force resulting frommomentary (fleeting) distortions in electrondistributionsChapter 12Intermolecular Forces¾London Dispersion forces¾Why do LDF get stronger with increasing size?Intermolecular Forces¾London Dispersion forces¾ F2 , Cl2 , Br2 , I2¾ Which halogen should have the largestdispersion forces and why?¾ What is the impact?Symmetrical distributionof electron cloudAt a given instant of time,there is an unsymmetrical distributionof electron clouds6
Chapter 12Section 12.3Chapter 12Chapter 13Intermolecular ForcesSummary for intermolecular forces¾Relative ranking intermolecular forces .which is thestrongest force, which is the weakest force?3.1 Impact of IMF¾The relative strengths of IMF help explain .¾Physical states of matter¾B ili ttemperatureBoilingt¾Solubility (miscibility)7
Chapter 12Chapter 12Evaporation and CondensationChapter 12Evaporation and Vaporization¾ Evaporation or vaporization¾ Molecules escape the surface of a liquid¾ Vapor pressure¾ Condensation¾ Molecules strike and re-enter the surface of a liquid¾ What does equilibrium mean?Vapor Pressureδ vaporization¾ Vapor pressure dependson strengthtth off cohesiveh iforcesδ HOHOδ Oδ HHδ δ Hδ Oδ HHOHδ Oδ Hδ condensationHHδ HOHHOHH8
Chapter 12Chapter 12Vapor Pressure¾ Hydrogen bonds versus LDFPolarityVapor pressure(torr)P tPentane72Nonpolar414 thanol46Polar (hydrogen bonds)43.91-Propanol60Polar (hydrogen bonds)17.31-Butanol74Polar (hydrogen bonds)7.1Water18Vapor Pressure¾ Effect of TemperatureMolecularweight (μ)LiquidChapter 12Vapor PressurePolar (hydrogen bonds)17.5¾ Why does T affectvapor pressure?Temperature (oC)Vapor pressure ofwater (torr)04.62017.54055.360149.280355.5100760.0As T increases9
Chapter 12Chapter 12Chapter 12Boiling and Boiling Point¾ What happens to vapor pressure as temperaturerises?Boiling Point¾Boiling PointCompare propanol, butane and acetone (58 - 60amu). What IMF are possible?¾Another comparison¾ StandardSt d d or normall bboilingili pointi tpropanolbutaneacetonepropaneoctaneC17-ane10
Chapter 12Chapter 13Chapter 13Boiling Point¾ Why does water have a high boiling point?SolubilityMiscibility¾ Solubility¾ A nice sounding but technically WRONG answer:¾ Miscibility“Water has high boiling point because the bonds in waterrequire a lot of energy to break. Therefore, a hightemperature is needed to break the bonds and producethe gas.”¾ Compounds with IMF of similar strength tend to besoluble¾ “like (IMF) dissolves like (IMF)”11
Chapter 13Solubility*Expressed in mol alcohol/100g solvent at 20 C.Can you explain the data shown above?12
Summary for intermolecular forces Chapter 12 Section 12.3 Intermolecular Forces ¾Relative ranking intermolecular forces .which is the strongest force, which is the weakest force? Chapter 12 3.1 Impact of IMF ¾The relative strengths of IMF help explain . ¾Physical states of matter
AP Chemistry Chapter 11. Intermolecular Forces, Liquids, and Solids - 1 - Chapter 11. Intermolecular Forces, Liquids, and Solids 11.2 Intermolecular Forces Intermolecular forces are much weaker than ionic or covalent bonds (e.g., 16 kJ/mol versus 431 kJ/mol for HCl). Melting o
Mar 06, 2007 · intermolecular forces. Volatility-The more volatile, the weaker the intermolecular forces. Vapor pressure-The higher the vapor pressure, the weaker the intermolecular forces. The melting point/boiling point is higher in substances that have stronger intermolecular forces. Other physical properties include viscosity.File Size: 556KB
Intermolecular Forces 1. Evidence for Intermolecular Forces 2. Phase Diagrams (briefly) 3. Liquid-Vapor Equilibrium 1. Kinetic theory 2. Gas escape as a way to measure liquid intermolecular forces 4. Boiling points related liquid Intermolecular Forces 1. Dipole-dipole 2. Dispersion 3. H-b
intermolecular forces. Intermolecular Force (IMF): between molecules. This is the force that holds molecules together. It is a form of “stickiness” between molecules. Examples of intermolecular forces are London dispersion forces (LDF), dipole-dipole forces (DDF), and hydrogen bridging forces (HBF).File Size: 832KB
Forces Jacob Israelachvili ch 3,4 L6 Interaction forces- II Binnig, Quate, Gerber (reader) Intermolecular & Surface Forces Jacob Israelachvili ch 4,5 L5 Interaction forces-III Intermolecular & Surface Forces Jacob Israelachvili ch 5,6 Interaction forces-IV Intermolecular & Surface Forces Jacob Israelachvili ch 6,7 L7 F-Z, F-d curves – I
The surface of proteins seem to have evolved to avoid . Nanotechnology requires to produce particles with a finite size. 6 Intermolecular forces and crystal growth Adjustable parameters e.g.: pH, concentration of precipitant, ionic strength, . (see J. Israelachvili, Intermolecular and surface forces). 15 Intermolecular interactions partial .
Intermolecular Forces 11.2 Intermolecular forces are attractive forces between molecules. Intramolecular forces hold atoms together in a molecule. Intermolecular vs Intramolecular 41 kJ to vaporize 1 mole of water (inter) 930 kJ to break all O-H bonds in 1 mole of water (intra) Generally,
ANATOMI LUTUT Lutut adalah salah satu sendi terbesar dan paling kompleks dalam tubuh. Sendi ini juga yang paling rentan karena menanggung beban berat dan beban tekanan sekaligus memberikan gerakan yang fleksibel. Ketika berjalan, lutut menopang 1,5 kali berat badan kita, naik tangga sekitar 3–4 kali berat badan kita dan jongkok sekitar 8 kali. Lutut bergabung dengan tulang femur di atasnya .
