The atom has a small dense nucleus which. contains protons (+1 charge). contains electrons ( 1 charge).
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1 Section 11.1 Rutherford s Atom Nuclear Model of the Atom Chapter 11 Modern Atomic Theory The atom has a small dense nucleus which is positively charged. contains protons (+1 charge). contains neutrons (no charge). The remainder of the atom is mostly empty space. contains electrons ( 1 charge). Copyright Cengage Learning. All rights reserved 2 Section 11.1 Rutherford s Atom The nuclear charge (n+) is balanced by the presence of n electrons moving in some way around the nucleus. One of the ways that energy travels through space. What are the electrons doing? How are the electrons arranged and how do they move? Copyright Cengage Learning. All rights reserved 3 Copyright Cengage Learning. All rights reserved 4
2 Characteristics Wavelength ( λ) distance between two peaks or troughs in a wave. Characteristics Frequency ( ν ) number of waves (cycles) per second that pass a given point in space Speed (c) speed of light ( m/s) c = λν Copyright Cengage Learning. All rights reserved 5 Copyright Cengage Learning. All rights reserved 6 Dual Nature of Light Wave Photon packet of energy Different Wavelengths Carry Different Amounts of Energy Copyright Cengage Learning. All rights reserved 7 Copyright Cengage Learning. All rights reserved 8
3 Section 11.3 Emission of Energy by Atoms Atoms can give off light. They first must receive energy and become excited. The energy is released in the form of a photon. The energy of the photon corresponds exactly to the energy change experienced by the emitting atom. Atomic states Excited state t atom with excess energy Ground state atom in the lowest possible state When an H atom absorbs energy from an outside source it enters an excited state. Copyright Cengage Learning. All rights reserved 9 Copyright Cengage Learning. All rights reserved 10 Energy Level Diagram Energy in the photon corresponds to the energy used by the atom to get to the excited state. Only certain types of photons are produced when H atoms release energy. Why? Copyright Cengage Learning. All rights reserved 11 Copyright Cengage Learning. All rights reserved 12
4 Quantized Energy Levels Since only certain energy changes occur, the H atom must contain discrete energy levels. Quantized Energy Levels The energy levels of all atoms are quantized. Copyright Cengage Learning. All rights reserved 13 Copyright Cengage Learning. All rights reserved 14 Concept Check Concept Check Why is it significant that the color emitted from the hydrogen emission spectrum is not white? How does the emission spectrum support the idea of quantized energy levels? When an electron is excited in an atom or ion a) only specific quantities of energy are released in order for the electron to return to its ground state. b) white light is never observed when the electron returns to its ground state. c) the electron is only excited to certain energy levels. d) All of the above statements are true when an electron is excited. Copyright Cengage Learning. All rights reserved 15 Copyright Cengage Learning. All rights reserved 16
5 Section 11.5 The Bohr Model of the Atom Quantized energy levels Electron moves in a circular orbit. Electron jumps between levels by absorbing or emitting a photon of a particular wavelength. Section 11.5 The Bohr Model of the Atom Bohr s model of the atom was incorrect. Electron does not move in a circular orbit. Copyright Cengage Learning. All rights reserved 17 Copyright Cengage Learning. All rights reserved 18 Section 11.6 The Wave Mechanical Model of the Atom Orbitals Nothing like orbits Probability of finding the electron within a certain space This model gives no information about when the electron occupies a certain point in space or how it moves. Orbitals Orbitals do not have sharp boundaries. Chemists arbitrarily define an orbital s size as the sphere that contains 90% of the total electron probability. Copyright Cengage Learning. All rights reserved 19 Copyright Cengage Learning. All rights reserved 20
6 Hydrogen Energy Levels Hydrogen has discrete energy levels. Called principal energy levels Labeled with whole numbers Hydrogen Energy Levels Each principal energy level is divided into sublevels. Labeled with numbers and letters Indicate the shape of the orbital Copyright Cengage Learning. All rights reserved 21 Copyright Cengage Learning. All rights reserved 22 Hydrogen Energy Levels The s and p types of sublevel Orbital Labels 1. The number tells the principal energy level. 2. The letter tells the shape. The letter s means a spherical orbital. The letter p means a two lobed orbital. The x, y, or z subscript on a p orbital label tells along which h of the coordinate axes the two lobes lie. Copyright Cengage Learning. All rights reserved 23 Copyright Cengage Learning. All rights reserved 24
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