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# scan-11 - Dr Pustam October 4 2009 Chem 127 — Fall 2009...

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Unformatted text preview: Dr. Pustam October 4*, 2009. Chem 127 — Fall 2009. Cha 0 tline Although the concepts you need to understand are emphasized here, you need to READ THE ENTIRE CHAPTER! 1. The nature of light (Section 7.1) — (a) the wave nature of light — know the properties of a wave such as frequency and wavelength and the mathematical relationship between the two (9» X v = c). Be able to do calculations with this equation (eg. sample problem 7.1). Know the relative orders of the different regions of the electromagnetic spectrum. See Fig. 7.3, pg. 271. (b) the particle nature of light — be able to use Planck’s equation (h x v : E) for determination of energy of a photon if given the frequency or wavelength. Be able to work out problems using the Einstein’s equation from the photoelectric effect ( E = K.E. + W ) to determine work function for a metal (W) or the energy or velocity of an ejected electron, or the energy or wavelength of a photon which is needed to eject the electron from a metal. 2. Atomic Spectra (Section 7.2) — You should be able to understand how the Bohr model of the atom explains why H and other atoms have a line spectra and know the three postulates proposed (See pg. 277). Be able to calculate the energy of an electron in a H atom using the relation, E = —2.18 X 10‘18 J [l/nz]. Calculate also the change in energy of an electron when a photon is emitted or absorbed using, A E = Em; — Emma = -2.18 X 1048 J [l/(nﬁmﬂ)2 e l/(niniaa)2]. Practice with sample problem 7.3. 3. Wave-Particle Duality of Matter and Energy (Section 7.3) — Be able to work problems with deBroglie equation (it = h / mv) to calculate wavelengths (see sample problem 7.4). You should be able to apply the uncertainty principle (see sample problem 7.5). 4. The quantum mechanical model of the atom (Section 7.4) —- Wave functions are solutions to the Schrodinger equation. Understand what is meant by an orbital. Orbitals are spatial representations of the wave functions. Be able to describe the energy and shape of orbitals using 3 quantum numbers, (n, 1, m1). Deﬁne each quantum number. Understand how you can use all the quantum numbers to describe the level, sub—level, and orbital of an electron in an atom. Know the shapes of s, p and d orbitals and what is a node. Suggested problems for Ch. 7 — /2,/ 7, 16, 20, 23, 27, 31, 36, 43, 48, #71, 5/1/99), 75. [.5 ...
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