Chapter 10 Modern Atomic Theory and the Periodic Table

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n = 1 1s orbital spherical shapethe electron does not move around on thesurface of sphere, the surface encloses a spacewhere there is a 90% probability that theelectron may be foundhow many electrons can fit into a 1s orbital?spin a property of electroneach electron can only spin in two directionsrepresentation of the spin ↑ or ↓two electrons with the same spin cannot occupythe same orbitalPauli exclusion principle – an atomic orbitalcan hold a maximum of two electrons whichmust have opposite spinsn = 1 energy level contains one type of orbital(1s) that hold a maximum of 2 electronsn = 2 2s spherical shapehold a maximum of two electrons2p – 2p x , 2p y , 2p z8
each p orbital has two lobes and can hold amaximum of two electronsthe total number of electrons that can reside inall three p orbitals is 6n = 3n = 2 energy level contains two types oforbitals (a 2s and three 2p) that hold amaximum of 8 electrons3s3p – 3p x , 3p y , 3p z3d – 3d xz , 3d xy , 3d yz , 3d z 2, 3d x 2 –y 2n = 3 energy level contains three types oforbitals (a 3s, three 3p, five 3d) that hold amaximum of 18 electrons9
Page 2 and 3: 10.1 A brief history10.1 A brief hi
Page 4 and 5: 10.3 The Bohr atomat high temperatu
Page 6 and 7: 1924 de Broglie all objects have wa
Page 12 and 13: valence electrons - the electrons u
Page 14 and 15: the valence electron configurations
Page 16: groups of elements show similar che

Chapter 10 Modern Atomic Theory and the Periodic Table

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