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1 hapter 12 Section 1 Kinetic Molecular Description of Liquids and Solids Noncovalent Forces Intermolecular interactions Electrostatic Forces Dispersion Forces -bonding DNA, RNA Mary J. Bojan hem 110 1
2 What s next? We now know about the structure of molecules. Lewis structures à shape, bonding information (hybrid orbitals) Organic molecules serve as examples Next: what are the PROPERTIES of these molecules? Properties of gases, liquids, and solutions (properties of solids in hem 112) We will always be connecting the properties to their structure! Mary J. Bojan hem 110 2
3 To understand properties, we want to connect what we see to what is happening on a molecular level. Start with states of matter Kinetic Molecular Theory is used to explain what is happening on a molecular level. Key postulate of this theory is that molecules have kinetic energy: they are in constant motion in all states. Mary J. Bojan hem 110 3
4 The state a substance is in at a particular temperature and pressure depends on two antagonistic entities: The kinetic energy of the particles The strength of the attractions between the particles gas à liquid à solid. Mary J. Bojan hem 110 4
5 If we know the relative strengths of these two interactions we could predict the state of a substance. gas: Kinetic energy >> intermolecular forces Liquid: Kinetic energy intermolecular forces Solid: Kinetic energy << intermolecular forces solid liquid gas! Kinetic Energy T eating: T é, KE é Mary J. Bojan hem 110 5
6 Intermolecular forces (non covalent interactions) are weaker than covalent bonds Strength of: chemical bonds intermolecular (IM) forces intermolecular attraction (weak) intramolecular Bond (strong) Relative strengths of intermolecular forces can be seen experimentally: higher boiling point (or melting point) È intermolecular interactions IM FORES: due to electrostatic attraction increase as intermolecular distances Mary J. Bojan hem 110 6
7 To predict the relative strength of InterMolecular (IM) Forces, start by understanding how IM Forces are connected to molecular properties (and structure). Strength of IM forces depends on: Q charge on ion µ dipole moment α Polarizability α - polarizability: ease with which electron clouds become distorted α increases as number of electrons increases α increases as size (MW) increases Mary J. Bojan hem 110 7
8 SUMMARY of TYPES OF INTERMOLEULAR FORES Ion-Ion ionic bond Depends on Q Depends on Dipole-Induced Dipole µ, α polar molecules in nonpolar solvents Ion-Dipole Q, µ Ions in aqueous solutions of electrolytes Dipole-Dipole µ Ion-Induced Dipole ions in nonpolar solvents Q, α Dispersion α induced-dipole induced-dipole ydrogen Bonding must have bonded to N,O,F directional dipole-dipole In general: IM Forces are due to ELETROSTATI attraction. Mary J. Bojan hem 110 8
9 Ion-Ion: IM Forces are due to ELETROSTATI attraction depends on ion charge Q and distance r Q + r Q Q1Q r 2 E! Q = charge r = distance between charges Opposite charges STRONG interaction alled: Mary J. Bojan hem 110 9
10 IM Forces are due to ELETROSTATI attraction Ion-Dipole Depends on ion charge Q, dipole moment, µ and r E! Qµ r 2 Example: salt dissolved in water. Ions: Na + and l Polar solvent; water Mary J. Bojan hem
11 IM Forces are due to ELETROSTATI ELETROSTATI attraction FORES Dipole-Dipole depends on µ and r! +!"! +!" E! µ µ r 1 2 3!"! +! +!" attraction repulsion Net effect averaged over time. l l l l l Example: Mary J. Bojan hem
12 DISPERSION FORES are the result of induced dipole interactions Ion Induced Dipole: depends on Q of ion, α and r Ease of electronic distortion is polarizability: α + +!"!+ Ion neutral molecule Induce dipole Mary J. Bojan hem
13 DISPERSION FORES are the result of induced dipole interactions Induced Dipole: depends on α and r London Dispersion forces = Induced dipoles - induced dipoles forces E "!! 1 r 6 2 Mary J. Bojan hem
14 London Dispersion Forces SUMMARY electrons are in constant motion instantaneous dipole moment forms when there are more electrons on one side of the molecule instantaneous dipole moment induces an instantaneous dipole moment in a neighboring molecule TEY MOVE IN SYN Mary J. Bojan hem
15 Dispersion interactions contribute to the intermolecular forces in ALL molecules. Ar interacts via LDF only Ar Ar l l l has LDF in addition to dipole dipole Mary J. Bojan hem
16 Dispersion Interactions depend on size, shape and polarizability SIZE: Ar BP = Xe BP = Size (number of electrons) is related to polarizability Mary J. Bojan hem
17 YDROARBONS 17 ALKANES ALKENES ALKYNES AROMATI 3 Mary J. Bojan hem 110 Dispersion Interactions depend on size, shape and polarizability
18 Dispersion Interactions depend on size, shape and polarizability Boiling Points of Alkanes Alkanes: hydrocarbons non polar LDF only Boiling Point Number of arbons As size of hydrocarbon increases boiling point (and melting point) increase. Mary J. Bojan hem
19 Dispersion Interactions depend on SAPE N-pentane BP = 36.2 isopentane BP = 28 Neopentane BP = 9.5 Mary J. Bojan hem
20 Boiling points increase as dispersion forces increase (mainly MW). We see this trend by plotting the boiling points of the molecular hydrides. Mary J. Bojan hem
21 ydrogen Bonding: IM force BUT directional like covalent bonds. The dipole-dipole interactions experienced when is bonded to N, O, or F (the most electronegative elements) are unusually strong. When hydrogen is bonded to N, O, F the hydrogen nucleus is exposed. Mary J. Bojan hem
22 bonds are: ydrogen Bonding ü strong as intermolecular forces go: ~ 4-25kJ/mole ü weak compared to covalent bonds, but are directional like covalent bonds. Water is especially interesting Mary J. Bojan hem
23 ow do you know which has the strongest Intermolecular (IM) forces? compare boiling point (BP) and melting (MP) higher BP (MP) means stronger IM forces If substances are similar, follow trends. Eg. inert gases, shape is the same IM forces increase as MW increases (as polarizability increases) If trends compete, need BP or MP Eg. 3 l 24.2 µ increases é 3 Br 3.6 size increases ê 3 I 42.4 (polarizability) BP follows trend in size: London Dispersion forces dominate here Mary J. Bojan hem
24 Q + Q r intermolecular Attraction (weak) intramolecular Bond (strong) Mary J. Bojan hem
25 Mary J. Bojan hem
26 l l l l l Mary J. Bojan hem
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