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Download Intro to Chapter 5 Development of the Periodic Table
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Chapter 5: Periodicity and Atomic Structure 5.1 5.2 5.3 5.4 5.5 5.6 5.7 5.8 5.9 5.10 5.11 5.12 5.13 5.14 5.15 Development of the Periodic Table Light and Electromagnetic Spectrum Electromagnetic Radiation and Atomic Spectra Particlelike Properties of Electromagnetic Radiation: The Planck Equation Wavelike Properties of Matter: The de Broglie Equation Quantum Mechanics and the Heisenberg Uncertainty Principle Wave Functions and Quantum Numbers The Shapes of Orbitals Quantum Mechanics and the Atomic Spectra Electron Spin and Pauli Exclusion Principle Orbital Energy Levels in Multielectron Atoms Electron Configurations of Multielectron Atoms Electron Configurations and the Periodic Table Some Anomalous Electron Configurations Electron Configurations and Periodic Properties: Atomic Radii Intro to Chapter 5 The periodic table is the most important organized principle in chemistry. If you know the properties of any one element in a group, or column, you can make a good guess at the properties of every other other element in the same group. In this chapter we will discover why the elements follow specific periodic trends by examining the intriguing atomic structures of the elements. Development of the Periodic Table A. Creation of the Periodic Table by Mendeleev in 1869 is an ideal example of how scientific theory comes into being. Through random observations followed by organization of data into trends resulted in a consistent hypothesis which could explain known facts and makes correct predictions of the elements. B. Mendeleev s organized chemical information by: 1) listing elements by atomic weight 2) grouping them together according to chemical reactivity 1 Light and the Electromagnetic Spectrum What properties of atoms is responsible for the periodic variations? To understand how, it s necessary to look first at the nature of visible line and other forms of radiant energy. Historically, studies of the interaction of radiant energy with matter provided immense insight into the atomic structures. Visible light, infrared, microwaves, X-rays etc are all different kinds of electromagnetic radiation . Collectively they make up the Electromagnetic spectrum. A. Radiant Energy- has wavelike properties. Three components: 1) frequency ( ) - the number of peaks that pass by a fixed point per unit of time [ s-1 or Hz] 2) Wavelength ( ) - the length from one wave maximum to the next 3) Amplitude- the height measured from the middle to the maximum the intensity of energy is proportional to its amplitude 2 B. Speed of light ( c ) - rate of travel of all electromagnetic radiation in a vacuum. 1. c = 3.00 x 108 m/s 2. Wavelength x frequency = speed of light (m) x (s-1) = c (m/s) Frequency and wavelength are inversely related = c long ; low short ; high EXAMPLE: Calculate the wavelength , in meters and nanometers, of radiation with a frequency of 1.18 x 1014 s-1 What region of the electromagnetic spectrum is it? ANSWER: Using = c = 3.00 x 108 m/s = 2.54 x 10-6 m 1.18 x 1014 s-1 = 2.54 x 10-6 m x 109 nm = 2,540 nm 1m This wavelength found in infrared region (see Figure 5.3). Electromagnetic Radiation and Atomic Spectra A. Individual atoms give off radiation when heated or otherwise excited energetically. 1. Provides important clues to the atomic makeup 2. Electromagnetic radiation from excited atom consists of only a few . 3. The resulting Line Spectrum- series of discrete lines (or wavelengths) separated by blank areas (no radiation). 4. Each element has its own unique line spectrum B. Balmer and Rydberg- discovered a pattern in atomic line spectra for the hydrogen which fits the generalized equation: 1=R( 1 - 1) m2 n2 This equation will be discussed again, in detail. when we deal the concept of Quantized energy 3 Line spectra for (a) sodium and (b) hydrogen 4 This document was created with Win2PDF available at http://www.daneprairie.com. The unregistered version of Win2PDF is for evaluation or non-commercial use only.