ch04---the-electronic-structure-of-atoms.ppt
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1、New Way Chemistry for Hong Kong A-Level Book 11Chapter 4The Electronic Structure of Atoms4.1The Electromagnetic Spectrum4.2 Deduction of Electronic Structure from Ionization Enthalpies4.3 The Wave-mechanical Model of the Atom4.4 Atomic OrbitalsNew Way Chemistry for Hong Kong A-Level Book 12The Elect
2、ronic Structure of AtomsNiels BohrBohrs Model of H atom Chapter 4 The electronic structure of atoms(SB p.90)New Way Chemistry for Hong Kong A-Level Book 13The Electronic Structure of AtomsNiels BohrBohrs Model of H atom Chapter 4 The electronic structure of atoms(SB p.90)New Way Chemistry for Hong K
3、ong A-Level Book 14 The Electromagnetic Spectrum4.1 The Electromagnetic Spectrum(SB p.91)New Way Chemistry for Hong Kong A-Level Book 15Continuous spectrum of white lightFig.4-5(a)4.1 The Electromagnetic Spectrum(SB p.92)New Way Chemistry for Hong Kong A-Level Book 16Line Spectrum of hydrogen4.1 The
4、 Electromagnetic Spectrum(SB p.93)Fig.4-5(b)New Way Chemistry for Hong Kong A-Level Book 17The Emission Spectrum of Atomic HydrogenUVVisibleIR4.1 The Electromagnetic Spectrum(SB p.93)New Way Chemistry for Hong Kong A-Level Book 18Interpretation of the Atomic Hydrogen Spectrum4.1 The Electromagnetic
5、Spectrum(SB p.94)New Way Chemistry for Hong Kong A-Level Book 19Interpretation of the Atomic Hydrogen Spectrum4.1 The Electromagnetic Spectrum(SB p.94)New Way Chemistry for Hong Kong A-Level Book 110Interpretation of the Atomic Hydrogen Spectrum4.1 The Electromagnetic Spectrum(SB p.94)New Way Chemis
6、try for Hong Kong A-Level Book 111Bohr proposed for a hydrogen atom:1.An electron in an atom can only exist in certain states characterized by definite energy levels (called quantum).2.Different orbits have different energy levels.An orbit with higher energy is further away from the nucleus.3.When a
7、n electron jumps from a higher energy level(of energy E1)to a lower energy level(of energy E2),the energy emitted is related to the frequency of light recorded in the emission spectrum by:E=E1-E2=h4.1 The Electromagnetic Spectrum(SB p.95)New Way Chemistry for Hong Kong A-Level Book 1124.1 The Electr
8、omagnetic Spectrum(SB p.96)How can we know the energy levels are getting closer and closer together?New Way Chemistry for Hong Kong A-Level Book 1134.1 The Electromagnetic Spectrum(SB p.97)E=E1-E2=hPlanck s constantFrequency of light emittedNew Way Chemistry for Hong Kong A-Level Book 114 Emission s
9、pectrum of hydrogenAbsorption spectrum of hydrogendark background(photographic plate)bright linesbright background(photographic plate)dark lines4.1 The Electromagnetic Spectrum(SB p.97)New Way Chemistry for Hong Kong A-Level Book 115Production of the Absorption SpectrumAbsorption spectrum of hydroge
10、n4.1 The Electromagnetic Spectrum(SB p.97)bright background(photographic plate)dark linesNew Way Chemistry for Hong Kong A-Level Book 116Convergence Limits and IonizationWhat line in the H spectrum corresponds to this electron transition(n=n=1)?Last line in the Lyman SeriesFor n=n=1:4.1 The Electrom
11、agnetic Spectrum(SB p.97)H(g)H+(g)+e-New Way Chemistry for Hong Kong A-Level Book 117The Uniqueness of Atomic Emission SpectraNo two elements have identical atomic spectraatomic spectra can be used to identify unknown elements.4.1 The Electromagnetic Spectrum(SB p.99)New Way Chemistry for Hong Kong
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