n - Wits Structural Chemistry

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Line spectra and the Bohr model of the atom Different gases under reduced pressure emit differentcolored light by electrical discharge when high voltageis applied.The light has only a few wavelengths and represented bya colored line in the spectrum.ie., a line spectrum not a continuous spectrum isobtainedNa vapor – street lightsDark areas!!Dark areas between lines!!
Line spectra and the Bohr model of the atomRydberg discovered that the lines in the H-atomspectrum could be predicted by an empirical equation:Where λ is the wavelength of the line in the H-atomspectrum, R H is the Rydberg constant (1.096776 x 10 7 m -1 ),and n 1 and n 2 are positive integers such that n 2 > n 1 .1λ= ⎛ 1 1R ⎜−H 2⎝ n n21 2⎞⎟⎠
Page 4 and 5: ExampleThe speed of a sound wave th
Page 6 and 7: All electromagnetic radiation (X-ra
Page 8 and 9: Classical Physics ~1800’sParticle
Page 10 and 11: Quantised Energy and PhotonsMax Pla
Page 12 and 13: ExampleWhat is the smallest increme
Page 14 and 15: If light shines on the surface of a
Page 16 and 17: Let w o = hυ oIf E < w o , i.e. if
Page 18 and 19: Some properties of light can only b
Page 22 and 23: ExampleCalculate the wavelength in
Page 24 and 25: Bohr calculated, using classical eq
Page 26 and 27: - 1 / 16hcR H0- 1 / 9hcR H-¼hcR Hn
Page 28 and 29: 0- 1 / 16hcR H- 1 / 9hcR Hn = ∞n
Page 30 and 31: - 1 / 16hcR H0- 1 / 9hcR H-¼hcR Hn
Page 32 and 33: (i)ExampleWhich quantum numbers are
Page 34 and 35: (i)ExampleWhich quantum numbers are
Page 36 and 37: ExampleWhat is the wavelength of th
Page 38 and 39: The Wave Behaviour of Matterde Brog
Page 40 and 41: Heisenberg Uncertainty PrincipleBec
Page 42 and 43: Quantum Mechanics and Atomic Orbita
Page 44 and 45: Quantum Mechanics and Atomic Orbita
Page 47 and 48: ExampleGive the values of n, l, and
Page 49 and 50: All s-orbitals are sphericalAs n in
Page 51 and 52: 0.529ÅElectron density× 4πr 2Dis
Page 53 and 54: 0.5Å3Å× 4πr 2
Page 55 and 56: As n increases, the number of nodes
Page 57 and 58: n = 3 (3 rd energy level of atom)
Page 59 and 60: Contour plots.m l = -1m l = 1 m l =
Page 61 and 62: d - orbitals
Page 63 and 64: In the H atom, allorbitals in a she
Page 65 and 66: s orbitals have Ψ 2 ≠ 0 at the n
Page 67 and 68: Effectivenuclear chargeActual nucle
Page 69 and 70: For multi-electronatoms (He, Li, Li
Page 71 and 72:
Electrons have a property called sp
Page 74 and 75:
Examples:Orbital diagramm s= ½m s=
Page 76 and 77:
Examples:m s= ½Have the same energ
Page 78 and 79:
Examples:Orbital diagram1s 2 2s 2 2
Page 80 and 81:
The periodic table reflects the ele
Page 82 and 83:
2e -Transition metals.(d - orbitlas
Page 84 and 85:
Anomalous Transition Metals.Copper
Page 86 and 87:
Pb: [Xe] 6s 2 4f 14 5d 10 6p 2Pb
Page 88 and 89:
Electronic Structure of IonsCation
Page 90 and 91:
ExampleWhat is the electron configu
Page 92 and 93:
Transition Metal Ions1 st and 2 nd
Page 94 and 95:
Answer (b)Fe: 1s 2 2s 2 2p 6 3s 23p
Page 96 and 97:
Anomalous Transition Metals.(Cu 2+
Page 98:
ExampleThe diagram shows the wavefu
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n - Wits Structural Chemistry

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