无机化学英文ppt课件：chapter10.ppt

Chapter 10Liquids and SolidsSection 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved2Intramolecular Bonding“Within”the molecule.Molecules are formed by sharing electrons between the atoms.Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved3Intermolecular ForcesForces that occur between molecules.Dipoledipole forcesHydrogen bondingLondon dispersion forcesIntramolecular bonds are stronger than intermolecular forces.Section 10.1Intermolecular ForcesHydrogen Bonding in WaterBlue dotted lines are the intermolecular forces between the water molecules.Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved5Which are stronger,intramolecular bonds or intermolecular forces?How do you know?CONCEPT CHECK!CONCEPT CHECK!Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved6Phase ChangesWhen a substance changes from solid to liquid to gas,the molecules remain intact.The changes in state are due to changes in the forces among molecules rather than in those within the molecules.Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved7Schematic Representations of the Three States of MatterSection 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved8Phase ChangesSolid to LiquidAs energy is added,the motions of the molecules increase,and they eventually achieve the greater movement and disorder characteristic of a liquid.Liquid to GasAs more energy is added,the gaseous state is eventually reached,with the individual molecules far apart and interacting relatively little.Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved9Densities of the Three States of WaterSection 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved10Dipole-Dipole ForcesDipole moment molecules with polar bonds often behave in an electric field as if they had a center of positive charge and a center of negative charge.Molecules with dipole moments can attract each other electrostatically.They line up so that the positive and negative ends are close to each other.Only about 1%as strong as covalent or ionic bonds.Section 10.1Intermolecular ForcesDipole-Dipole ForcesCopyright Cengage Learning.All rights reserved11To play movie you must be in Slide Show ModePC Users:Please wait for content to load,then click to playMac Users:CLICK HERESection 10.1Intermolecular ForcesHydrogen BondingCopyright Cengage Learning.All rights reserved12Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved13Hydrogen BondingStrong dipole-dipole forces.Hydrogen is bound to a highly electronegative atom nitrogen,oxygen,or fluorine.That same hydrogen is then electrostatically attracted to a lone pair on the nitrogen,oxygen or fluorine on adjacent molecules.Section 10.1Intermolecular ForcesLondon Dispersion ForcesCopyright Cengage Learning.All rights reserved14Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved15London Dispersion ForcesInstantaneous dipole that occurs accidentally in a given atom induces a similar dipole in a neighboring atom.Significant in large atoms/molecules.Occurs in all molecules,including nonpolar ones.Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved16Melting and Boiling PointsIn general,the stronger the intermolecular forces,the higher the melting and boiling points.Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved17The Boiling Points of the Covalent Hydrides of the Elements in Groups 4A,5A,6A,and 7ASection 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved18Which molecule is capable of forming stronger intermolecular forces?N2 H2O Explain.CONCEPT CHECK!CONCEPT CHECK!Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved19Draw two Lewis structures for the formula C2H6O and compare the boiling points of the two molecules.CONCEPT CHECK!CONCEPT CHECK!Section 10.1Intermolecular ForcesCopyright Cengage Learning.All rights reserved20Which gas would behave more ideally at the same conditions of P and T?CO or N2 Why?CONCEPT CHECK!CONCEPT CHECK!Section 10.2The Liquid StateLiquidsLow compressibility,lack of rigidity,and high density compared with gases.Surface tension resistance of a liquid to an increase in its surface area:Liquids with large intermolecular forces tend to have high surface tensions.Copyright Cengage Learning.All rights reserved21Section 10.2The Liquid StateLiquidsCapillary action spontaneous rising of a liquid in a narrow tube:Cohesive forces intermolecular forces among the molecules of the liquid.Adhesive forces forces between the liquid molecules and their container.Copyright Cengage Learning.All rights reserved22Section 10.2The Liquid StateWhich force dominates alongside the glass tube cohesive or adhesive forces?cohesive forcesConvex Meniscus Formed by Nonpolar Liquid MercuryCopyright Cengage Learning.All rights reserved23Section 10.2The Liquid StateConcave Meniscus Formed by Polar WaterWhich force dominates alongside the glass tube cohesive or adhesive forces?adhesive forcesCopyright Cengage Learning.All rights reserved24Section 10.2The Liquid StateLiquidsViscosity measure of a liquids resistance to flow:Liquids with large intermolecular forces or molecular complexity tend to be highly viscous.Copyright Cengage Learning.All rights reserved25Section 10.3An Introduction to Structures and Types of SolidsSolidsAmorphous Solids:Disorder in the structuresGlassCrystalline Solids:Ordered StructuresUnit CellsCopyright Cengage Learning.All rights reserved26Section 10.3An Introduction to Structures and Types of SolidsThree Cubic Unit Cells and the Corresponding LatticesCopyright Cengage Learning.All rights reserved27Section 10.3An Introduction to Structures and Types of SolidsBragg EquationUsed to determine the interatomic spacings.n=integer =wavelength of the X raysd=distance between the atoms =angle of incidence and reflectionCopyright Cengage Learning.All rights reserved28Section 10.3An Introduction to Structures and Types of SolidsBragg EquationCopyright Cengage Learning.All rights reserved29Section 10.3An Introduction to Structures and Types of SolidsTypes of Crystalline SolidsIonic Solids ions at the points of the lattice that describes the structure of the solid.Molecular Solids discrete covalently bonded molecules at each of its lattice points.Atomic Solids atoms at the lattice points that describe the structure of the solid.Copyright Cengage Learning.All rights reserved30Section 10.3An Introduction to Structures and Types of SolidsExamples of Three Types of Crystalline SolidsCopyright Cengage Learning.All rights reserved31Section 10.3An Introduction to Structures and Types of SolidsClassification of SolidsCopyright Cengage Learning.All rights reserved32Section 10.4Structure and Bonding in MetalsClosest Packing ModelClosest Packing:Assumes that metal atoms are uniform,hard spheres.Spheres are packed in layers.Copyright Cengage Learning.All rights reserved33Section 10.4Structure and Bonding in MetalsThe Closest Packing Arrangement of Uniform Spheresabab packing the 2nd layer is like the 1st but it is displaced so that each sphere in the 2nd layer occupies a dimple in the 1st layer.The spheres in the 3rd layer occupy dimples in the 2nd layer so that the spheres in the 3rd layer lie directly over those in the 1st layer.Copyright Cengage Learning.All rights reserved34Section 10.4Structure and Bonding in MetalsThe Closest Packing Arrangement of Uniform Spheresabca packing the spheres in the 3rd layer occupy dimples in the 2nd layer so that no spheres in the 3rd layer lie above any in the 1st layer.The 4th layer is like the 1st.Copyright Cengage Learning.All rights reserved35Section 10.4Structure and Bonding in MetalsHexagonal Closest PackingCopyright Cengage Learning.All rights reserved36Section 10.4Structure and Bonding in MetalsCubic Closest PackingCopyright Cengage Learning.All rights reserved37Section 10.4Structure and Bonding in MetalsThe Indicated Sphere Has 12 Nearest NeighborsEach sphere in both ccp and hcp has 12 equivalent nearest neighbors.Copyright Cengage Learning.All rights reserved38Section 10.4Structure and Bonding in MetalsThe Net Number of Spheres in a Face-Centered Cubic Unit CellCopyright Cengage Learning.All rights reserved39Section 10.4Structure and Bonding in MetalsDetermine the number of metal atoms in a unit cell if the packing is:a)Simple cubicb)Cubic closest packinga)1 metal atomb)4 metal atomsCopyright Cengage Learning.All rights reserved40CONCEPT CHECK!CONCEPT CHECK!Section 10.4Structure and Bonding in MetalsA metal crystallizes in a face-centered cubic structure.Determine the relationship between the radius of the metal atom and the length of an edge of the unit cell.Copyright Cengage Learning.All rights reserved41CONCEPT CHECK!CONCEPT CHECK!Section 10.4Structure and Bonding in MetalsSilver metal crystallizes in a cubic closest packed structure.The face centered cubic unit cell edge is 409 pm.Calculate the density of the silver metal.Density=10.5 g/cm3Copyright Cengage Learning.All rights reserved42CONCEPT CHECK!CONCEPT CHECK!Section 10.4Structure and Bonding in MetalsBonding Models for MetalsElectron Sea ModelBand Model(MO Model)Copyright Cengage Learning.All rights reserved43Section 10.4Structure and Bonding in MetalsThe Electron Sea ModelA regular array of cations in a“sea”of mobile valence electrons.Section 10.4Structure and Bonding in MetalsBand or Molecular Orbital(MO)ModelElectrons are assumed to travel around the metal crystal in molecular orbitals formed from the valence atomic orbitals of the metal atoms.Copyright Cengage Learning.All rights reserved45Section 10.4Structure and Bonding in MetalsMolecular Orbital Energy Levels Produced When Various Numbers of Atomic Orbitals InteractCopyright Cengage Learning.All rights reserved46Section 10.4Structure and Bonding in MetalsThe Band Model for MagnesiumVirtual continuum of levels,called bands.Copyright Cengage Learning.All rights reserved47Section 10.4Structure and Bonding in MetalsMetal AlloysSubstitutional Alloy some of the host metal atoms are replaced by other metal atoms of similar size.Interstitial Alloy some of the holes in the closest packed metal structure are occupied by small atoms.Copyright Cengage Learning.All rights reserved48Section 10.4Structure and Bonding in MetalsTwo Types of AlloysBrass is a substitutional alloy.Steel is an interstitial alloy.Copyright Cengage Learning.All rights reserved49Section 10.5Carbon and Silicon:Network Atomic SolidsNetwork SolidsCopyright Cengage Learning.All rights reserved50Section 10.5Carbon and Silicon:Network Atomic SolidsThe Structures of Diamond and GraphiteCopyright Cengage Learning.All rights reserved51Section 10.5Carbon and Silicon:Network Atomic SolidsPartial Representation of the Molecular Orbital Energies in a)Diamond b)a Typical MetalCopyright Cengage Learning.All rights reserved52Section 10.5Carbon and Silicon:Network Atomic SolidsThe p Orbitals and Pi-system in GraphiteCopyright Cengage Learning.All rights reserved53Section 10.5Carbon and Silicon:Network Atomic SolidsCeramicsTypically made from clays(which contain silicates)and hardened by firing at high temperatures.Nonmetallic materials that are strong,brittle,and resistant to heat and attack by chemicals.Copyright Cengage Learning.All rights reserved54Section 10.5Carbon and Silicon:Network Atomic SolidsSemiconductorsn-type semiconductor substance whose conductivity is increased by doping it with atoms having more valence electrons than the atoms in the host crystal.p-type semiconductor substance whose conductivity is increased by doping it with atoms having fewer valence electrons than the atoms of the host crystal.Copyright Cengage Learning.All rights reserved55Section 10.5Carbon and Silicon:Network Atomic SolidsEnergy Level Diagrams for (a)an n-type Semiconductor (b)a p-type SemiconductorCopyright Cengage Learning.All rights reserved56Section 10.5Carbon and Silicon:Network Atomic SolidsSilicon Crystal Doped with(a)Arsenic and(b)BoronSection 10.6Molecular SolidsCopyright Cengage Learning.All rights reserved58Section 10.7Ionic SolidsCopyright Cengage Learning.All rights reserved59Section 10.7Ionic SolidsIonic SolidsIonic solids are stable,high melting substances held together by the strong electrostatic forces that exist between oppositely charged ions.Copyright Cengage Learning.All rights reserved60Section 10.7Ionic SolidsThree Types of Holes in Closest Packed Structures1)Trigonal holes are formed by three spheres in the same layer.Copyright Cengage Learning.All rights reserved61Section 10.7Ionic SolidsThree Types of Holes in Closest Packed Structures2)Tetrahedral holes are formed when a sphere sits in the dimple of three spheres in an adjacent layer.Copyright Cengage Learning.All rights reserved62Section 10.7Ionic SolidsThree Types of Holes in Closest Packed Structures3)Octahedral holes are formed between two sets of three spheres in adjoining layers of the closest packed structures.Copyright Cengage Learning.All rights reserved63Section 10.7Ionic SolidsFor spheres of a given diameter,the holes increase in size in the order:trigonal tetrahedral octahedralCopyright Cengage Learning.All rights reserved64Section 10.7Ionic SolidsTypes and Properties of SolidsCopyright Cengage Learning.All rights reserved65Section 10.8Vapor Pressure and Changes of StateBehavior of a Liquid in a Closed Container a)Initially b)at EquilibriumCopyright Cengage Learning.All rights reserved66Section 10.8Vapor Pressure and Changes of StateThe Rates of Condensation and EvaporationCopyright Cengage Learning.All rights reserved67Section 10.8Vapor Pressure and Changes of StateVapor PressurePressure of the vapor present at equilibrium.The system is at equilibrium when no net change occurs in the amount of liquid or vapor because the two opposite processes exactly balance each other.Copyright Cengage Learning.All rights reserved68Section 10.8Vapor Pressure and Changes of StateWhat is the vapor pressure of water at 100C?How do you know?1 atmCopyright Cengage Learning.All rights reserved69Section 10.8Vapor Pressure and Changes of StateVapor PressureCopyright Cengage Learning.All rights reserved70Section 10.8Vapor Pressure and Changes of StateVapor PressureLiquids in which the intermolecular forces are large have relatively low vapor pressures.Vapor pressure increases significantly with temperature.Copyright Cengage Learning.All rights reserved71Section 10.8Vapor Pressure and Changes of StateVapor Pressure vs.TemperatureCopyright Cengage Learning.All rights reserved72Section 10.8Vapor Pressure and Changes of StateClausiusClapeyron EquationPvap=vapor pressureHvap=enthalpy of vaporizationR=8.3145 J/KmolT=temperature(in kelvin)Copyright Cengage Learning.All rights reserved73Section 10.8Vapor Pressure and Changes of StateThe vapor pressure of water at 25C is 23.8