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Transcript
Chapter 13 – Electrons in Atoms 13.1 13.2 13.3 Models of the Atom Electron Arrangement in Atoms Physics and the Quantum Mechanical Model 13.1 Models of the Atom The Evolution of Atomic Models Dalton Thomson Gold-foil Bohr Plum pudding Rutherford Solid, indivisible Planetary Quantum Mechanical Probability 13.2 Electron Arrangement in Atoms Electron Configurations Fortunately, we can “predict” where these electrons are most likely to be found and represent these locations with simple notation by following some simple rules: Aufbau Principle Electrons fill lowest energy levels first. Pauli Exclusion Principle Only two electrons can be in an orbital at once. Hund’s Rule Each orbital must have at least one electron in it before getting a second. Example: O, Atomic # 8 – 1s22s22p4 Configuration vs. Notation Examples: 13.3 Physics and the Quantum Mechanical Model Light and Atomic Spectra To fully understand quantum mechanics you must understand the nature of light and waves. 13.3 Physics and the Quantum Mechanical Model (cont.) Light and Atomic Spectra (cont.) Light is an electromagnetic wave that when passed through a prism separates into a spectrum of colors: 13.3 Physics and the Quantum Mechanical Model (cont.) Light and Atomic Spectra (cont.) Atoms/elements emit light when the electrons are excited (first absorb then emit energy in the form of light) at specific frequencies. Chapter 13 Assignment CPQ 1 pg. 386 #27,28,29,30,31,33
