Intermolecular Forces and

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1 Intermolecular Forces and
Liquids and Solids Chapter 11

2 A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases Solid phase - ice Liquid phase - water 11.1

3 Intermolecular Forces
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) “Measure” of intermolecular force boiling point melting point DHvap DHfus DHsub Generally, intermolecular forces are much weaker than intramolecular forces. 11.2

4 Intermolecular Forces
Dipole-Dipole Forces Attractive forces between polar molecules Orientation of Polar Molecules in a Solid 11.2

5 Intermolecular Forces
Ion-Dipole Forces Attractive forces between an ion and a polar molecule Ion-Dipole Interaction 11.2

6 Intermolecular Forces
Dispersion Forces Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules ion-induced dipole interaction dipole-induced dipole interaction 11.2

7 Intermolecular Forces
Dispersion Forces Continued Polarizability is the ease with which the electron distribution in the atom or molecule can be distorted. Polarizability increases with: greater number of electrons more diffuse electron cloud Dispersion forces usually increase with molar mass. 11.2

8 What type(s) of intermolecular forces exist between each of the following molecules?
HBr HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules. CH4 CH4 is nonpolar: dispersion forces. S O SO2 SO2 is a polar molecule: dipole-dipole forces. There are also dispersion forces between SO2 molecules. 11.2

9 Intermolecular Forces
Hydrogen Bond The hydrogen bond is a special dipole-dipole interaction between they hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom. A H … B or A & B are N, O, or F 11.2

10 Why is the hydrogen bond considered a “special” dipole-dipole interaction?
Decreasing molar mass Decreasing boiling point 11.2

11 Strong intermolecular forces
Properties of Liquids Surface tension is the amount of energy required to stretch or increase the surface of a liquid by a unit area. Strong intermolecular forces High surface tension 11.3

12 Properties of Liquids Cohesion is the intermolecular attraction between like molecules Adhesion is an attraction between unlike molecules Adhesion Cohesion 11.3

13 Strong intermolecular forces
Properties of Liquids Viscosity is a measure of a fluid’s resistance to flow. Strong intermolecular forces High viscosity 11.3

14 Ice is less dense than water
Water is a Unique Substance Maximum Density 40C Density of Water Ice is less dense than water 11.3

15 Unit cells in 3 dimensions
A crystalline solid possesses rigid and long-range order. In a crystalline solid, atoms, molecules or ions occupy specific (predictable) positions. An amorphous solid does not possess a well-defined arrangement and long-range molecular order. A unit cell is the basic repeating structural unit of a crystalline solid. At lattice points: Atoms Molecules Ions lattice point Unit Cell Unit cells in 3 dimensions 11.4

16 11.4

17 11.4

18 11.4

19 11.4

20 Shared by 8 unit cells Shared by 2 unit cells 11.4

21 1 atom/unit cell 2 atoms/unit cell 4 atoms/unit cell (8 x 1/8 = 1) (8 x 1/8 + 1 = 2) (8 x 1/8 + 6 x 1/2 = 4) 11.4

22 11.4

23 4 atoms/unit cell in a face-centered cubic cell
When silver crystallizes, it forms face-centered cubic cells. The unit cell edge length is 409 pm. Calculate the density of silver. d = m V V = a3 = (409 pm)3 = 6.83 x cm3 4 atoms/unit cell in a face-centered cubic cell 107.9 g mole Ag x 1 mole Ag 6.022 x 1023 atoms x m = 4 Ag atoms = 7.17 x g d = m V 7.17 x g 6.83 x cm3 = = 10.5 g/cm3 11.4

24 11.5

25 Extra distance = BC + CD = 2d sinq = nl (Bragg Equation) 11.5

26 X rays of wavelength nm are diffracted from a crystal at an angle of Assuming that n = 1, what is the distance (in pm) between layers in the crystal? nl = 2d sin q n = 1 q = l = nm = 154 pm nl 2sinq = 1 x 154 pm 2 x sin14.17 d = = 77.0 pm 11.5

27 Types of Crystals Ionic Crystals
Lattice points occupied by cations and anions Held together by electrostatic attraction Hard, brittle, high melting point Poor conductor of heat and electricity CsCl ZnS CaF2 11.6

28 Types of Crystals Covalent Crystals Lattice points occupied by atoms
Held together by covalent bonds Hard, high melting point Poor conductor of heat and electricity carbon atoms diamond graphite 11.6

29 Types of Crystals Molecular Crystals
Lattice points occupied by molecules Held together by intermolecular forces Soft, low melting point Poor conductor of heat and electricity 11.6

30 Cross Section of a Metallic Crystal
Types of Crystals Metallic Crystals Lattice points occupied by metal atoms Held together by metallic bonds Soft to hard, low to high melting point Good conductors of heat and electricity Cross Section of a Metallic Crystal nucleus & inner shell e- mobile “sea” of e- 11.6

31 Types of Crystals 11.6

32 An amorphous solid does not possess a well-defined arrangement and long-range molecular order.
A glass is an optically transparent fusion product of inorganic materials that has cooled to a rigid state without crystallizing Crystalline quartz (SiO2) Non-crystalline quartz glass 11.7

33 Greatest Order Least T2 > T1 Evaporation Condensation 11.8

34 The equilibrium vapor pressure is the vapor pressure measured when a dynamic equilibrium exists between condensation and evaporation H2O (l) H2O (g) Rate of condensation evaporation = Dynamic Equilibrium 11.8

35 Before Evaporation At Equilibrium 11.8

36 Clausius-Clapeyron Equation
Molar heat of vaporization (DHvap) is the energy required to vaporize 1 mole of a liquid. ln P = - DHvap RT + C Clausius-Clapeyron Equation P = (equilibrium) vapor pressure T = temperature (K) R = gas constant (8.314 J/K•mol) 11.8

37 The boiling point is the temperature at which the (equilibrium) vapor pressure of a liquid is equal to the external pressure. The normal boiling point is the temperature at which a liquid boils when the external pressure is 1 atm. 11.8

38 The critical temperature (Tc) is the temperature above which the gas cannot be made to liquefy, no matter how great the applied pressure. The critical pressure (Pc) is the minimum pressure that must be applied to bring about liquefaction at the critical temperature. 11.8

39 H2O (s) H2O (l) The melting point of a solid or the freezing point of a liquid is the temperature at which the solid and liquid phases coexist in equilibrium Melting Freezing 11.8

40 Molar heat of fusion (DHfus) is the energy required to melt 1 mole of a solid substance.
11.8

41 11.8

42 H2O (s) H2O (g) Molar heat of sublimation (DHsub) is the energy required to sublime 1 mole of a solid. Sublimation Deposition DHsub = DHfus + DHvap ( Hess’s Law) 11.8

43 A phase diagram summarizes the conditions at which a substance exists as a solid, liquid, or gas.
Phase Diagram of Water 11.8

44 11.8