2 The Development of Atomic Models 5.1The Development of Atomic ModelsThe Development of Atomic ModelsWhat was inadequate about Rutherford’s atomic model?
3 The Development of Atomic Models 5.1The Development of Atomic ModelsRutherford’s atomic model could not explain the chemical properties of elements.Rutherford’s atomic model could not explain why objects change color when heated.Rutherford’s model fails to explain why objects change color when heated. As the temperature of this horseshoe is increased, it first appears black, then red, then yellow, and then white. The observed behavior could be explained only if the atoms in the iron gave off light in specific amounts of energy. A better atomic model was needed to explain this observation.
4 The Development of Atomic Models 5.1The Development of Atomic ModelsThe timeline shoes the development of atomic models from 1803 to 1911.These illustrations show how the atomic model has changed as scientists learned more about the atom’s structure.
5 The Development of Atomic Models 5.1The Development of Atomic ModelsThe timeline shows the development of atomic models from 1913 to 1932.These illustrations show how the atomic model has changed as scientists learned more about the atom’s structure.
6 5.1The Bohr ModelThe Bohr ModelWhat was the new proposal in the Bohr model of the atom?
7 5.1The Bohr ModelBohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
8 Each possible electron orbit in Bohr’s model has a fixed energy. 5.1The Bohr ModelEach possible electron orbit in Bohr’s model has a fixed energy.The fixed energies an electron can have are called energy levels.A quantum of energy is the amount of energy required to move an electron from one energy level to another energy level.
9 5.1The Bohr ModelLike the rungs of the strange ladder, the energy levels in an atom are not equally spaced.The higher the energy level occupied by an electron, the less energy it takes to move from that energy level to the next higher energy level.These ladder steps are somewhat like energy levels. In an ordinary ladder, the rungs are equally spaced. The energy levels in atoms are unequally spaced, like the rungs in this ladder. The higher energy levels are closer together.
10 The Quantum Mechanical Model 5.1The Quantum Mechanical ModelThe Quantum Mechanical ModelWhat does the quantum mechanical model determine about the electrons in an atom?
11 The Quantum Mechanical Model 5.1The Quantum Mechanical ModelThe quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus.
12 The Quantum Mechanical Model 5.1The Quantum Mechanical ModelAustrian physicist Erwin Schrödinger (1887– 1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom.The modern description of the electrons in atoms, the quantum mechanical model, comes from the mathematical solutions to the Schrödinger equation.
13 The Quantum Mechanical Model 5.1The Quantum Mechanical ModelIn the quantum mechanical model, the probability of finding an electron within a certain volume of space surrounding the nucleus can be represented as a fuzzy cloud. The cloud is more dense where the probability of finding the electron is high.The electron cloud of an atom is compared here to photographs of a spinning airplane propeller. a) The airplane propeller is somewhere in the blurry region it produces in this picture, but the picture does not tell you its exact position at any instant. b) Similarly, the electron cloud of an atom represents the locations where an electron is likely to be found.
14 Atomic Orbitals How do sublevels of principal energy levels differ? 5.1Atomic OrbitalsAtomic OrbitalsHow do sublevels of principal energy levels differ?
15 5.1Atomic OrbitalsAn atomic orbital is often thought of as a region of space in which there is a high probability of finding an electron.Each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found.
16 5.1Atomic OrbitalsDifferent atomic orbitals are denoted by letters. The s orbitals are spherical, and p orbitals are dumbbell-shaped.The electron clouds for the s orbital and the p orbitals are shown here.
17 5.1Atomic OrbitalsFour of the five d orbitals have the same shape but different orientations in space.The d orbitals are illustrated here. Four of the five d orbitals have the same shape but different orientations in space. Interpreting Diagrams How are the orientations of the dxy and dx2 – y2 orbitals similar? How are they different?
18 5.1Atomic OrbitalsThe numbers and kinds of atomic orbitals depend on the energy sublevel.
19 5.1Atomic OrbitalsThe number of electrons allowed in each of the first four energy levels are shown here.
20 Electron Configurations 5.2Electron ConfigurationsElectron ConfigurationsWhat are the three rules for writing the electron configurations of elements?
21 Electron Configurations 5.2Electron ConfigurationsThe ways in which electrons are arranged in various orbitals around the nuclei of atoms are called electron configurations.Three rules—the aufbau principle, the Pauli exclusion principle, and Hund’s rule—tell you how to find the electron configurations of atoms.
22 Electron Configurations 5.2Electron ConfigurationsAufbau PrincipleAccording to the aufbau principle, electrons occupy the orbitals of lowest energy first. In the aufbau diagram below, each box represents an atomic orbital.This aufbau diagram shows the energy levels of the various atomic orbitals. Orbitals of greater energy are higher on the diagram. Using Tables Which is of higher energy, a 4d or a 5s orbital?
23 Electron Configurations 5.2Electron ConfigurationsPauli Exclusion PrincipleAccording to the Pauli exclusion principle, an atomic orbital may describe at most two electrons. To occupy the same orbital, two electrons must have opposite spins; that is, the electron spins must be paired.
24 Electron Configurations 5.2Electron ConfigurationsHund’s RuleHund’s rule states that electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible.
25 Electron Configurations 5.2Electron ConfigurationsOrbital Filling Diagram
26 Electron Configurations Simulation 2Fill atomic orbitals to build the ground state of several atoms.
30 for Conceptual Problem 1.1 Problem Solving 5.9 Solve Problem 9 with the help of an interactive guided tutorial.
31 Exceptional Electron Configurations 5.2Exceptional Electron ConfigurationsExceptional Electron ConfigurationsWhy do actual electron configurations for some elements differ from those assigned using the aufbau principle?
32 Exceptional Electron Configurations 5.2Exceptional Electron ConfigurationsSome actual electron configurations differ from those assigned using the aufbau principle because half-filled sublevels are not as stable as filled sublevels, but they are more stable than other configurations.
33 Exceptional Electron Configurations 5.2Exceptional Electron ConfigurationsExceptions to the aufbau principle are due to subtle electron-electron interactions in orbitals with very similar energies.Copper has an electron configuration that is an exception to the aufbau principle.Copper is a good conductor of electricity and is commonly used in electrical wiring.
35 5.2 Section Quiz.1. Identify the element that corresponds to the following electron configuration: 1s22s22p5.FClNeO
36 5.2 Section Quiz. 2. Write the electron configuration for the atom N. 1s22s22p51s22s22p31s22s1p21s22s22p1
37 5.2 Section Quiz.3. The electron configurations for some elements differ from those predicted by the aufbau principle because thethe lowest energy level is completely filled.none of the energy levels are completely filled.half-filled sublevels are less stable than filled energy levels.half-filled sublevels are more stable than some other arrangements.`
39 Physics and the Quantum Mechanical Model 5.3Physics and the Quantum Mechanical ModelNeon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube makes the gas glow with its own characteristic color. You will learn why each gas glows with a specific color of light.
40 5.3LightLightHow are the wavelength and frequency of light related?
41 5.3LightThe amplitude of a wave is the wave’s height from zero to the crest.The wavelength, represented by (the Greek letter lambda), is the distance between the crests.
42 5.3LightThe frequency, represented by (the Greek letter nu), is the number of wave cycles to pass a given point per unit of time.The SI unit of cycles per second is called a hertz (Hz).
43 5.3LightThe wavelength and frequency of light are inversely proportional to each other.The frequency and wavelength of light waves are inversely related. As the wavelength increases, the frequency decreases.
44 5.3LightThe product of the frequency and wavelength always equals a constant (c), the speed of light.
45 5.3LightAccording to the wave model, light consists of electromagnetic waves.Electromagnetic radiation includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays.All electromagnetic waves travel in a vacuum at a speed of 108 m/s.
46 5.3LightSunlight consists of light with a continuous range of wavelengths and frequencies.When sunlight passes through a prism, the different frequencies separate into a spectrum of colors.In the visible spectrum, red light has the longest wavelength and the lowest frequency.
47 5.3LightThe electromagnetic spectrum consists of radiation over a broad band of wavelengths.The electromagnetic spectrum consists of radiation over a broad band of wavelengths. The visible light portion is very small. It is in the 10-7m wavelength range and 1015 Hz (s-1) frequency range. Interpreting Diagrams What types of nonvisible radiation have wavelengths close to those of red light? To those of blue light?
48 LightSimulation 3Explore the properties of electromagnetic radiation.
55 5.3Atomic SpectraWhen atoms absorb energy, electrons move into higher energy levels. These electrons then lose energy by emitting light when they return to lower energy levels.
56 5.3Atomic SpectraA prism separates light into the colors it contains. When white light passes through a prism, it produces a rainbow of colors.A prism separates light into the colors it contains. For white light this produces a rainbow of colors.
57 5.3Atomic SpectraWhen light from a helium lamp passes through a prism, discrete lines are produced.A prism separates light into the colors it contains. Light from a helium lamp produces discrete lines. Identifying Which color has the highest frequency?
58 5.3Atomic SpectraThe frequencies of light emitted by an element separate into discrete lines to give the atomic emission spectrum of the element.MercuryNitrogenNo two elements have the same emission spectrum. a) Mercury vapor lamps produce a blue glow. b) Nitrogen gas gives off a yellowish-orange light.
59 An Explanation of Atomic Spectra 5.3An Explanation of Atomic SpectraAn Explanation of Atomic SpectraHow are the frequencies of light an atom emits related to changes of electron energies?
60 An Explanation of Atomic Spectra 5.3An Explanation of Atomic SpectraIn the Bohr model, the lone electron in the hydrogen atom can have only certain specific energies.When the electron has its lowest possible energy, the atom is in its ground state.Excitation of the electron by absorbing energy raises the atom from the ground state to an excited state.A quantum of energy in the form of light is emitted when the electron drops back to a lower energy level.
61 An Explanation of Atomic Spectra 5.3An Explanation of Atomic SpectraThe light emitted by an electron moving from a higher to a lower energy level has a frequency directly proportional to the energy change of the electron.
62 An Explanation of Atomic Spectra 5.3An Explanation of Atomic SpectraThe three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels.The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. The Lyman series corresponds to the transition to the n 1 energy level. The Balmer series corresponds to the transition to the n 2 energy level. The Paschen series corresponds to the transition to the n 3 energy level.
63 An Explanation of Atomic Spectra Animation 6Learn about atomic emission spectra and how neon lights work.
64 Quantum Mechanics Quantum Mechanics 5.3Quantum MechanicsQuantum MechanicsHow does quantum mechanics differ from classical mechanics?
65 5.3Quantum MechanicsIn 1905, Albert Einstein successfully explained experimental data by proposing that light could be described as quanta of energy.The quanta behave as if they were particles.Light quanta are called photons.
66 The Planck EquationThe energy of electromagnetic radiation is directly related to the frequencyE = hnh is the Planck constant = x J.sn is the frequency in Hz