n - Wits Structural Chemistry

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Electronic Structure of IonsCation - remove electron/s from the valence orbitals withthe highest principal quantum number.i.e., the occupied orbital with the largest principalquantum number (n)Anion - add electron/s to empty or partially occupiedvalence orbitals with the lowest principal quantumnumber.i.e., the partially occupied or unoccupied orbital with thelowest principal quantum number (n)
ExampleWhat is the electron configurationfor sodium and that of its ion?Show this by means of an orbitalenergy diagram giving also thecondensed electron configuration.Periodic table: 11 Na – 11 e -Na: 1s 2 2s 2 2p 6 3sNa: [Ne] 3s11Na is a metal therefore forms a cationby loosing the highest energy electron.(Valence electron)i.e., the occupied orbital with the largestprincipal quantum number (n)↿↿⇂↿⇂2e - 6e -Valence electron↿↿↿ ⇂⇂⇂2e - 6e -2e -Na + : 1s 2 2s 2 2p 6Na + : [Ne]Na + and Ne are isoelectronic
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ExampleThe speed of a sound wave th
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All electromagnetic radiation (X-ra
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Classical Physics ~1800’sParticle
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Quantised Energy and PhotonsMax Pla
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ExampleWhat is the smallest increme
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If light shines on the surface of a
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Let w o = hυ oIf E < w o , i.e. if
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Some properties of light can only b
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Line spectra and the Bohr model of
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ExampleCalculate the wavelength in
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Bohr calculated, using classical eq
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- 1 / 16hcR H0- 1 / 9hcR H-¼hcR Hn
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0- 1 / 16hcR H- 1 / 9hcR Hn = ∞n
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- 1 / 16hcR H0- 1 / 9hcR H-¼hcR Hn
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(i)ExampleWhich quantum numbers are
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(i)ExampleWhich quantum numbers are
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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 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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