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Ch10 z5e liq solids
- 1. Liquids and solids pp Chapter 10
- 6. + - + - + - + - + - + - + - + - + - + -
- 10. Fig 6-26, p.191 Predicting Polarity Tr 37
- 13. Hydrogen Bonding H H O + - + H H O + - +
- 14. Hydrogen bonding H H O H H O H H O H H O H H O H H O H H O
- 15. Boiling Points 0ºC 100 -100 -200 CH 4 SiH 4 GeH 4 SnH 4 PH 3 NH 3 SbH 3 AsH 3 H 2 O H 2 S H 2 Se H 2 Te HF HI HBr HCl
- 16. Water + - +
- 18. Example H H H H H H H H + - H H H H + - +
- 19. Figure 10.5 London Dispersion Forces
- 32. Cubic
- 35. Figure 10.9 Three Cubic Unit Cells & the Corresponding Lattices
- 37. Figure 10.12 Examples of Three Types of Crystalline Solids Atomic, Ionic and Molecular Solids
- 40. 10.4 Metallic bonding 1s 2s 2p 3s 3p 12+ 12+ 12+ 12+ 12+ 12+ Filled Molecular Orbitals Empty Molecular Orbitals Magnesium Atoms
- 41. Filled Molecular Orbitals Empty Molecular Orbitals The 1s, 2s, and 2p electrons are close to nucleus, so they are not able to move around. 1s 2s 2p 3s 3p 12+ 12+ 12+ 12+ 12+ 12+ Magnesium Atoms
- 42. Filled Molecular Orbitals Empty Molecular Orbitals 1s 2s 2p 3s 3p 12+ 12+ 12+ 12+ 12+ 12+ Magnesium Atoms The 3s and 3p orbitals overlap and form molecular orbitals.
- 43. Filled Molecular Orbitals Empty Molecular Orbitals 1s 2s 2p 3s 3p 12+ 12+ 12+ 12+ 12+ 12+ Magnesium Atoms Electrons in these energy levels can travel freely throughout the crystal.
- 44. Filled Molecular Orbitals Empty Molecular Orbitals 1s 2s 2p 3s 3p 12+ 12+ 12+ 12+ 12+ 12+ Magnesium Atoms This makes metals conductors Malleable because the bonds are flexible .
- 47. Malleable + + + + + + + + + + + +
- 59. Figure 10.24 The p Orbitals
- 60. Figure 10.22 p. 470 The Structures of Diamond and Graphite
- 67. Figure 10.30 Energy Level Diagrams for (a) an n-Type Semiconductor and (b) a p-Type Semiconductor
- 93. Figure 10.38 Vapor Pressure:Which is most volatile?
- 94. Temperature Effect Kinetic energy # of molecules T 1 Energy needed to overcome intermolecular forces
- 98. Figure 10.40 The Vapor Pressure of Water
- 101. Heating Curve for Water Ice Water and Ice Water Water and Steam Steam
- 102. Heating Curve for Water Heat of Fusion Heat of Vaporization Slope is Heat Capacity
- 103. Figure 10.42 Heating Curve for Water Bp plateau longer than Mp because takes almost 7x the energy to vaporize as melt. Slopes of other lines different because different states of water have different molar heat capacities
- 108. Solid Water Liquid Water Water Vapor Vapor
- 118. Phase Diagram for Water What happens to BP of water as pressure increases? To FP? BP increases, FP decreases What is the definition of triple point? The T and P at which all 3 states are in equilibrium
- 119. Temperature 1 Atm D D D Pressure D Solid Liquid Gas A A B B C C
- 120. Temperature Pressure Solid Liquid Gas Triple Point Critical Point
- 122. Phase Diagram for Carbon Note: There are 4 phases: Diamond, graphite, liquid, vapor. There are two “triple points”: Higher one is between Diamond, graphite & liquid Lower one is between graphite, liquid & vapor There can be different phases between solids if they have a different crystalline structure.
- 124. Z5e Fig 10.52 Phase Diagram for CO 2 Solid/Liquid line has positive slope - Why? Density of solid carbon dioxide is greater than that of liquid.
Hinweis der Redaktion
- Z5e 10.1 p. 452
- Rf Z5e Ch10 early slide
- Z5e Fig 10.2 p. 453 Use this to predict relative boiling points.
- HRW Top are polar Bottom are non-polar
- Re Z5e ch 10 early slides
- Z5e Fig. 10.4 p. 454 Non-polar tetrahedral hydrides of Gp 4A show steady increase in b.p. w/molar mass But, for other gps, lightest member has unexpectedly high b.p. d/t H-bonding (polar X-H) AND because small size of 1st element in each group allows close approach of dipoles, further strengthening intermolecular forces.
- Z5e 453 rf Fig. 10.3
- Rf Z5e Ch10 early slides
- Z53 fig. 10.5 p. 455 Describes (a) instantaneous dipoles on atoms vs. (b) that on molecules
- As number of e- increase, greater chance of momentary dipole interactions. So, importance of London forces increases as size of atom increases.
- Z5e Section 10.2 p. 456
- Rf. Z5e fig. 10.6 p. 456
- SS look at Fig. 10.7 Z5e p. 456 for actual menisci of Hg and H2O
- Z5e 456
- Z5e 457
- Z5e 457-458
- Section 10.3 Z5e p. 458
- Z5e 10.3 An Introduction to Structures and Types of Solids
- Z5e 461-462.
- Aka Simple cubic (rf. Fig. 10.9 Z5e 459)
- Z5e459 Fig. 10.9. Three cubic unit cells and their corresponding lattices.
- Z5e 462 Fig. 10.12
- Z5e 462 -466
- Section 10.4 Z5e 463
- Hrw 181
- Z53 468 and fig. 10.21
- Z5e 468 Two Types of Alloys.
- Z5e Section 10.5 p. 470
- Rf. Fig. 10.22(a) Z5e 470
- Rf. Fig. 10.22(b) Z5e 470.
- Z5e 471 Fig. 10.24 - an extensive Pi-bonding network. Discuss Semiconductors Z5e p. 476; add figures
- Z5e 471. Fig. 10.24
- Z5e 470 Fig. 10.22.
- Z5e 476
- Z5e 476-477 & figs. 10.29 -10.31
- Energy level diagrams for (a) an n-type semiconductor and (b) a p-type semiconductor
- Section 10.6 Z5e 478
- Z5E 479
- Section 10.7 Z5e 479 Do Z5e SE 10.4 p. 483 Students copy Table 10.7 and I review!!!
- Section 10.8 Z5e 484
- Z5e Fig. 10.37 485 Rate of evaporation remains constant Rate of condensation increases as # molecules in vapor phase increase, until the two rates become equal
- Z5e 484
- Rf. Fig 10.38 Z5e 485
- Fig 10.38 Z5e 485 Ether is most volatile. In each case a little liquid remains floating at top.
- Rf. Fig 10.39 Z5e 486
- Fig 10.40 Z5e 487. (b) plot used in Lab 9 (Vapor Pressure and Enthalpy of Vaporization in H2O).
- Fig. 10.42 Z5e 490 Bp plateau longer than mp because almost 7x energy to vaporize vs. melt. Slopes of other lines are different because different states of water have different molar heat capacities.
- Merrill 435 SP
- Merrill 435 SP
- Rf. #87 Z5e 508 Ans. 1680 kJ (see solutions guide 247).
- Z5e 491-492
- Z5e 492.
- Section 10.9 Z5e 493
- Rf. HRW Tr 63
- Ask students what state exists for each letter
- Fig 10.47 Z5e 493 Be able to draw, given a set of data and to describe, including meaning of (-) slope.
- Fig. 10.52 Z5e 500 Be able to explain for test!!