1、Quantum Theory and the Electronic Structure of AtomsChapters 7 & 87.1 Light and Classic Quantum Theory 1. Classic theory of Light Different waves have different color, and different wavelength. Particles (Newton, 1680): an array of particles, emitted from light source, that move in space in one dime

2、nsional direction. forcespeedAcceleration speedExact position and speed can be determined at the same time. Wave (Huygens, 1690): an elastic vibrator, emitted from light source, that move in space in three dimensional direction. Kinetic energyWavelength (l)7.1 Light and Classic Quantum Theory Maxwel

3、l (1893) wrote an equation for light as a waveLight is an electromagnetic wave that spread in space.For a light in vacuum, u = c = 3.00 x 108 m/sFrequency n is the number of waves that pass in 1 s.u = l nabout 1.28 s from moon to Earth Wavelength l is the distance between two successive waves. Speed

4、 u is the distance of waves that pass in 1 s.Electromagnetic radiation is the emission and transmission of energy in the form of electromagnetic waves.Wavelength (l)a0 amplitude At a certain position (x), the wave change with t.At a certain time (t), the wave change with x.The energy intensityEnergy

5、 changescontinuously !Energy passed through a unit area per unit timePlancks Quantum Hypothesis (1901): For a single quantum, the smallest quantity of energy : E = h vPlanck constant h = 6.63 x 10-34 JsEnergy change is only by hv, 2hv, 3 hv, 4 hv . but never by 1.5 hv or 3.06 hvThen in 1918, he won

6、Nobel Prize in physics.2. Classic quantum theory of Light (Plank, 1900)Classical theory explains it well at low v, but very bad at high v. Energy is emitted or absorbed in discrete units (quantum). Black body radiation: curve E vs vExplains all results well.The Particle Nature of Light: Photoelectri

7、c Effect: hnvoltage currentV0(1) minimum frequency of light (v0)(2) v0 is dependent of metal. (3) The current light intensity.h v = p cParticlenatureWavenatureEinstein Photon Theory (1905)hn = KE + BEKE = hn - BEExplanation of the Photoelectric Effect:Light has both:Wave nature l, E = hvParticle nat

8、ure m, momentum p = mcEnergy E = mc2 7.2 Dual Nature of Electron 1. Hydrogen Emission line spectrum: Bohrs Planetary model Hg Li Cd Sr Ca Nae- can only have specific (quantized) energy valueslight is emitted as e- moves from one energy level to a lower energy levelBohrs Model of H Atom (1913)En = -R

9、H( )1n2n (principal quantum number) = 1,2,3,RH (Rydberg constant) = 2.18 x 10-18J = 13.6 eVEphoton = DE = Ef - Ei3. ifDE = RH( )1n21n2nf = 1ni = 2nf = 1ni = 3nf = 2ni = 3Ephoton = 2.18 x 10-18 J x (1/25 - 1/9)Ephoton = DE = 1.55 x 10-19 Jl = 6.63 x 10-34 (Js) x 3.00 x 108 (m/s)/1.55 x 10-19Jl = 1280

10、 nmCalculate the wavelength (in nm) of a photon emitted by a hydrogen atom when its electron drops from the n = 5 state to the n = 3 state.Ephoton = h c/ ll = h c / EphotonifDE = RH( )1n21n2Ephoton =De Broglie (1924) reasoned that e- is both particle and wave.2pr = nl l = h/muu = velocity of e- m =

11、mass of e-2. Dual nature of the Electron: Matter as wavesWhat is the de Broglie wavelength (in nm) associated with a 2.5 g Ping-Pong ball traveling at 15.6 m/s?l = 6.63 x 10-34 / (2.5 x 10-3 x 15.6)l = 1.7 x 10-32 m = 1.7 x 10-23 nmNobel Prize in 1929& 7. 3 Quantum Mechanical Description of Electron

12、s in Atoms Schrdinger Wave EquationBasis:Bohrs theory, good to explain the emission spectrum of H, but can not account for the spectrum of other elements.Dual nature of electron (m and l).In 1926, Schrodinger wrote an equation for electron in the atom. = E E = V + KETotal energy of the systemPotenti

13、al energykinetic energy (psi): wave function, or atomic orbital that describes the movement of electron in the atom in three dimensional space.: Hamiltonian Operator2: Laplacian Operator2Uncertainty principle (1927, W K Heisenberg): DX Dp h/4p It is impossible to determine precisely both the positio

14、n and momentum of a particle at the same time.1. Application of Schrdinger to Hydrogen Atom zxy(x,y,z)r = E (x,y,z) = E (x,y,z) hereAfter transferred into sphere coordinateGeneral solution for Hydrogen AtomSame as Bohrs result, ie. Only dependent of n;Angular partSpacial partn=1 l =0 ml=0E1s=-13.6 e

15、V(Z is atomic number, and for H, Z=1)n=2 l =0 ml=0n=2 l =1 ml=0n=2 l =1 ml=-1n=2 l =1 ml=+1E* = -3.4 eV r distance from the nucleusY2ElectrondensityBut the probability to find e in space (DV) is P= Y2 DV, highest at r = 0.529 90 % of electron density foundl = 0n=1n=2n=3ml = -1ml = 1ml = 0ml = -2ml =

16、 -1ml = 0ml = 1ml = 27.6n: Principal quantum numbern = 1, 2, 3, 4, .distance of e- from the nucleus, and determination of energyHere n, l, m are called as the quantum numberl: angular momentum quantum numberl = 0, 1, 2, 3, n-1n = 1, l = 0n = 2, l = 0 , 1n = 3, l = 0, 1, 2Shape of the “volume” of spa

17、ce that the e- occupies l = 0 1 2 3Orbital s p d fml : magnetic quantum numberml = -l, ., 0, . +lif l = 1 (p orbital), ml = -1, 0, 1if l = 2 (d orbital), ml = -2, -1, 0, 1, 2orientation of the orbital in spaceEnergy of orbitals in a single electron atomEnergy only depends on principal quantum number

18、 nEn = -RH( )1n2n=1n=2n=3Ground stateexcited state2. Application of Schrdinger to Many-electron atomszxy(xi,yi,zi)ri = E rjrij(xj,yj,zj)For the ith electron, the average net potential is spherically approximated as:shielding constanti = Ei i Effective charge of the nucleusGeneral solutionEnergy of o

19、rbitals in a multi-electron atomEnergy depends on n and ln=1 l = 0n=2 l = 0n=2 l = 1n=3 l = 0n=3 l = 1n=3 l = 2Order of orbitals (filling) in multi-electron atom1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s3. The Building-Up Principle of electrons in the orbitals:1. Electrons occupy first the lowest energy or

20、bitals available.2. Each orbital accommodates only two electrons, and these two electrons must have opposing spins.Pauli exclusion principlespin quantum number ms= + or - To descript one electron completely, Four quantum numbers of n, l, ml and ms are needed.3. In the degenerate orbitals (same n and

21、 l), the electrons occupy the orbitals as many as possible with same spins. N (Z=7)1s2s2p(Z=7) N 1s2 2s2 2p3Electron configurationHunds ruleWhat is the electron configuration of Mg?Mg 12 electrons1s 2s 2p 3s 3p 4s 1s2 2s22p6 3s22 + 2 + 6 + 2 = 12 electronsAbbreviated as Ne3s2Ne 1s22s22p6What are the

22、 possible quantum numbers for the last (outermost) electron in Cl?Cl 17 electrons1s 2s 2p 3s 3p 4s 1s2 2s22p6 3s23p52 + 2 + 6 + 2 + 5 = 17 electronsLast electron added to 3p orbitaln = 3l = 1ml = -1, 0, or +1ms = or -Noble gas coreFe 26 electrons1s 2s 2p 3s 3p 4s 3d 1s2 2s22p6 3s23p6 4s23d6Abbreviat

23、ed as Ar4s23d6Ar 1s22s22p63s23p6What is the electron configuration of Fe?What is the electron configuration of Mo?Mo 42 electrons1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p1s2 2s22p6 3s23p6 4s23d104p6 5s24d4Abbreviated as Kr5s24d4Kr5s14d5Half-filled and fully-filled subshell are more stable. (p3, d5, f7)(p6, d

24、10, f14)One e- choiceOutermost subshell being filled with electrons& 7. 4 Periodic Relationships Among the ElementsIonization energy is the minimum energy (kJ/mol) required to remove an electron from a gaseous atom in its ground state.I1 + X (g) X+(g) + e-I2 + X+ (g) X2+(g) + e-I3 + X2+ (g) X3+(g) +

25、 e-I1 first ionization energyI2 second ionization energyI3 third ionization energyI1 I2 I3General Trend in First Ionization Energies8.4Increasing First Ionization EnergyIncreasing First Ionization EnergyElectron Configurations of Cations and AnionsNa Ne3s1Na+ NeCa Ar4s2Ca2+ ArAl Ne3s23p1Al3+ NeAtoms

26、 lose electrons so that cation has a noble-gas outer electron configuration.H 1s1H- 1s2 or HeF 1s22s22p5F- 1s22s22p6 or NeO 1s22s22p4O2- 1s22s22p6 or NeN 1s22s22p3N3- 1s22s22p6 or NeAtoms gain electrons so that anion has a noble-gas outer electron configuration.Electron Configurations of Cations of Transition MetalsWhen a cation is formed from an atom of a transition metal, e