1. © 2015 Pearson Education, Inc. Chapter 13 Lecture presentation Add image of chapter 13 cover page (pg. 1 of 28) here Phase Diagrams and Crystalline Solids Catherine E. MacGowan Armstrong Atlantic State University

2. © 2015 Pearson Education, Inc. Phase Diagrams Phase diagrams describe the different states and state changes that occur at various temperature/pressure conditions. Regions represent states. Lines represent state changes. The liquid/gas line is the vapor pressure curve. –On the line both phases exist simultaneously (i.e., in equilibrium with each other). Points –The critical point is the farthest point on the vapor pressure curve. – Triple point is the temperature/pressure condition in which all three states exist simultaneously. –For most substances, the freezing point increases as pressure increases.

3. © 2015 Pearson Education, Inc. Phase Diagram Navigation

4. © 2015 Pearson Education, Inc. Phase Diagrams of I 2 and CO 2

5. © 2015 Pearson Education, Inc. Practice Problem: Phase Diagrams

6. © 2015 Pearson Education, Inc. Crystalline Solids and Their Structure Crystalline solids are orderly geometric structures whose lattice points are occupied by atoms, ions, or molecules. Understanding of solid structure is often done using the technique of X-ray diffraction crystallography.

7. © 2015 Pearson Education, Inc. Diffraction from a Crystal When X-rays strike parallel planes of atoms or molecules in a crystal, constructive interference occurs if the difference in path length between beams reflected from adjacent planes is an integral number of wavelengths. Constructive interference “adds” to the amplitude of the electromagnetic wave whereas destructive interference “subtracts” from the wave’s amplitude. Bragg’s law allows scientists to determine the distance between layers of atoms or molecules in a crystal lattice. nλ = 2d sin θ

8. © 2015 Pearson Education, Inc. Practice Problem: Bragg’s Law

9. © 2015 Pearson Education, Inc. Crystal Lattice When allowed to cool slowly, the particles in a liquid will arrange themselves to give the maximum attractive forces. –Therefore, they minimize the energy. –The result will generally be a crystalline solid. The arrangement of the particles in a crystalline solid is called the crystal lattice. The smallest unit that shows the pattern of arrangement for all the particles is called the unit cell.

10. © 2015 Pearson Education, Inc. Unit Cells Unit cells are –three-dimensional; usually containing two or three layers of particles; –repeated over and over to give the macroscopic crystal structure of the solid. Starting anywhere within the crystal results in the same unit cell. Each particle in the unit cell is called a lattice point. Lattice planes are planes connecting equivalent points in unit cells throughout the lattice.

11. © 2015 Pearson Education, Inc. Cubic Crystalline Lattices

12. © 2015 Pearson Education, Inc. Unit Cells The number of other particles each particle is in contact with is called its coordination number. –For ions, it is the number of oppositely charged ions an ion is in contact with Higher coordination number means more interaction; therefore, stronger attractive forces hold the crystal together. The packing efficiency is the percentage of volume in the unit cell occupied by particles. –The higher the coordination number, the more efficiently the particles are packing together.

13. © 2015 Pearson Education, Inc. Cubic Unit Cells All 90 ° angles between corners of the unit cell The length of all the edges is equal. If the unit cell is made of spherical particles, –⅛ of each corner particle is within the cube; –½ of each particle on a face is within the cube; –¼ of each particle on an edge is within the cube.

14. © 2015 Pearson Education, Inc. Cubic Unit Cells: Simple Cubic Eight particles, one at each corner of a cube –⅛ of each particle lies in the unit cell. Each particle part of eight cells Total = one particle in each unit cell –8 corners × ⅛ –Edge of unit cell = twice the radius –Coordination number of 6

15. © 2015 Pearson Education, Inc. Cubic Unit Cells: Body-Centered Cubic Nine particles, one at each corner of a cube and one in center –⅛ of each corner particle lies in the unit cell. Two particles in each unit cell –8 corners × ⅛ –+ 1 center –Edge of unit cell = (4r) times the radius of the particle –Coordination number of 8

16. © 2015 Pearson Education, Inc. Body-Centered Cubic

17. © 2015 Pearson Education, Inc. Practice Problem: Unit Cell Volume, Edge Length, and Atomic Radius

18. © 2015 Pearson Education, Inc. Cubic Unit Cells: Face-Centered Cubic 14 particles, one at each corner of a cube and one on the center of each face –⅛ of each corner particle and ½ of face particle lie in the unit cell 4 particles in each unit cell –8 corners × ⅛ –+ 6 faces × ½ –Edge of unit cell = 2 2 times the radius of the particle –Coordination number of 12

19. © 2015 Pearson Education, Inc. Face-Centered Cubic

20. © 2015 Pearson Education, Inc. Practice Problem: Density of Crystal Structure

21. © 2015 Pearson Education, Inc. Closest-Packed Structures: First Layer With spheres, it is more efficient to offset each row in the gaps of the previous row than to line up rows and columns.

22. © 2015 Pearson Education, Inc. Closest-Packed Structures: Second Layer The second-layer atoms can sit directly over the atoms in the first layer, which is called an AA pattern. Or the second layer can sit over the holes in the first layer, which called an AB pattern.

23. © 2015 Pearson Education, Inc. Hexagonal Closest-Packed Structures

24. © 2015 Pearson Education, Inc. Cubic Closest-Packed Structures

25. © 2015 Pearson Education, Inc. Classifying Crystalline Solids Crystalline solids are classified by the kinds of particles found. Some of the categories are subclassified by the kinds of attractive forces holding the particles together.

26. © 2015 Pearson Education, Inc. Classifying Crystalline Solids Molecular solids are solids whose composite particles are molecules. Ionic solids are solids whose composite particles are ions. Atomic solids are solids whose composite particles are atoms. –Nonbonding atomic solids are held together by dispersion forces. –Metallic atomic solids are held together by metallic bonds. –Network covalent atomic solids are held together by covalent bonds.

27. © 2015 Pearson Education, Inc. Molecular Solids The lattice sites are occupied by molecules. –CO 2, H 2 O, C 12 H 22 O 11 The molecules are held together by intermolecular attractive forces. –Dispersion forces, dipole–dipole attractions, and H bonds Because the attractive forces are weak, they tend to have low melting points. –Generally < 300 ° C

28. © 2015 Pearson Education, Inc. Ionic Solids Lattice sites are occupied by ions. They are held together by attractions between oppositely charged ions. –Nondirectional –Therefore, every cation attracts all anions around it, and vice versa. The coordination number represents the number of close cation–anion interactions in the crystal. –The higher the coordination number, the more stable the solid. Lowers the potential energy of the solid The coordination number depends on the relative sizes of the cations and anions that maintain charge balance. –Generally, anions are larger than cations. The number of anions that can surround the cation is limited by the size of the cation. The closer in size the ions are, the higher the coordination number.

29. © 2015 Pearson Education, Inc. Practice Problem: Classifying Crystalline Solids

30. © 2015 Pearson Education, Inc. Structure of Ionic Solids: Cesium Chloride Coordination number = 8 –⅛ of each Cl – (184 pm) inside the unit cell Whole Cs + (167 pm) inside the unit cell –Cubic hole = hole in simple cubic arrangement of Cl – ions Cs:Cl = 1:(8 × ⅛); therefore the formula is CsCl.

31. © 2015 Pearson Education, Inc. The Structure of Ionic Solids: Rock Salt Coordination number = 6 Cl – ions (181 pm) in a face-centered cubic arrangement. –⅛ of each corner Cl – inside the unit cell –½ of each face Cl – inside the unit cell Na + (97 pm) in holes between Cl – –Octahedral holes –1 in center of unit cell –1 whole particle in every octahedral hole –¼ of each edge Na + inside the unit cell Na:Cl = (¼ × 12) + 1:(⅛ × 8) + (½ × 6) = 4:4 = 1:1 –Therefore, the formula is NaCl.

32. © 2015 Pearson Education, Inc. The Structure of Ionic Solids: Zinc Blende Coordination number = 4 S 2– ions (184 pm) in a face- centered cubic arrangement –⅛ of each corner S 2– inside the unit cell –½ of each face S 2– inside the unit cell Each Zn 2+ (74 pm) in holes between S 2– –Tetrahedral holes –1 whole particle in ½ the holes Zn:S = (4 × 1):(⅛ × 8) + (½ × 6) = 4:4 = 1:1 –Therefore, the formula is ZnS.

33. © 2015 Pearson Education, Inc. The Structure of Ionic Solids: Fluorite Coordination number = 4 Ca 2+ ions (99 pm) in a face-centered cubic arrangement –⅛ of each corner Ca 2+ inside the unit cell –½ of each face Ca 2+ inside the unit cell Each F – (133 pm) in holes between Ca 2+ –Tetrahedral holes –1 whole particle in all the holes Ca:F = (⅛ × 8) + (½ × 6):(8 × 1) = 4:8 = 1:2 –Therefore, the formula is CaF 2. –Fluorite structure common for 1:2 ratio Usually get the antifluorite structure when the cation:anion ratio is 2:1. –The anions occupy the lattice sites and the cations occupy the tetrahedral holes.

34. © 2015 Pearson Education, Inc. Metallic Atomic Solids Solid held together by metallic bonds –Strength varies with sizes and charges of cations. Coulombic attractions Melting point varies. Mostly closest-packed arrangements of the lattice points –Cations

35. © 2015 Pearson Education, Inc. Network Covalent Nonbonding Atomic Solids Noble gases in solid form Solid held together by weak dispersion forces –Very low melting Tend to arrange atoms in closest-packed (cP) structure –Either hexagonal cP or cubic cP –Maximizes attractive forces and minimizes energy

36. © 2015 Pearson Education, Inc. Network Covalent Solids Atoms attach to their nearest neighbors by covalent bonds. Because of the directionality of the covalent bonds, these do not tend to form closest- packed arrangements in the crystal. Because of the strength of the covalent bonds, these have very high melting points. –Generally > 1000 ° C Dimensionality of the network affects other physical properties.

37. © 2015 Pearson Education, Inc. The Graphite Structure: A Two-Dimensional Network In graphite, the carbon atoms in a sheet are covalently bonded together. –Forming six-member flat rings fused together Similar to benzene Bond length = 142 pm –sp 2 Each C has three sigma bonds and one pi bond. –Trigonal-planar geometry –Each sheet a giant molecule The sheets are then stacked and held together by dispersion forces. –Sheets are 341 pm apart.

38. © 2015 Pearson Education, Inc. Properties of Graphite Hexagonal crystals High melting point, ~3800 ° C –Need to overcome some covalent bonding Slippery feel –Because there are only dispersion forces holding the sheets together, they can slide past each other. Glide planes –Lubricants Electrical conductor –Parallel to sheets Thermal insulator Chemically very nonreactive

39. © 2015 Pearson Education, Inc. The Diamond Structure: A Three-Dimensional Network Each of the carbon atoms in a diamond has four covalent bonds to surrounding atoms. –sp 3 –Tetrahedral geometry This effectively makes each crystal one giant molecule held together by covalent bonds. –You can follow a path of covalent bonds from any atom to every other atom.

40. © 2015 Pearson Education, Inc. Properties of Diamond Very high melting point, ~3800 °C –Need to overcome some covalent bonds Very rigid –Due to the directionality of the covalent bonds Very hard –Due to the strong covalent bonds holding the atoms in position –Used as abrasives Electrical insulator Thermal conductor –Best known Chemically very nonreactive

41. © 2015 Pearson Education, Inc. Buckminsterfullerene: Buckyball A form of carbon occurs as soccer-ball-shaped clusters of 60 carbon atoms (C60). –The atoms form five- and six-membered carbon rings wrapped into a 20-sided icosahedral structure. The compound is named buckminsterfullerene. –After R. Buckminster Fuller, a twentieth-century engineer and architect who advocated the construction of buildings using a structurally strong geodesic dome shape that he patented Other carbon clusters have been identified similar to C60 that contain from 36 to over 100 carbon atoms. –As a class, these carbon clusters are called fullerenes and nicknamed buckyballs. Properties: –At room temperature, fullerenes are black solids. –The individual clusters are held to one another by dispersion forces. –Fullerenes are somewhat soluble in nonpolar solvents. –Some fullerenes are colored when in solution.

42. © 2015 Pearson Education, Inc. Nanotubes

43. © 2015 Pearson Education, Inc. Silicates and Quartz Silicates: ~90% of Earth’s crust Extended arrays of Si—O –Sometimes with Al substituted for Si— aluminosilicates Glass is the amorphous form. Quartz: SiO 2 in pure form –Impurities add color. Three-dimensional array of Si covalently bonded to 4 O – Tetrahedral Melts at ~1600 ° C Very hard