With this rationale in mind, the electromagnetic spectrum is discussed first, followed by a discussion of particulate radiation. Both ends of the electromagnetic spectrum are used in medical imaging. \n Particle/wave nature of electromagnetic radiation \n \n The photoelectric effect is the emission of electrons when electromagnetic radiation, such as light, hits a material. Wavelength and frequency are discussed shortly. Particulate Radiation Define waves. Key Ideas and Terms Notes Define frequency. Wave-particle duality is a concept in quantum mechanics. Apply coupon WELCOME21 at checkout and avail 21% discount on your order. The energy of the electromagnetic spectrum ranges from 10-12 to 1010 eV. Wavelength, Only gold members can continue reading. This chapter introduces the nature of electromagnetic and particulate radiation. His work is considered by many to be one of the greatest advances of physics. The energy of electromagnetic radiation can be calculated by the following formula: In this formula, E is energy, h is Planck’s constant (equal to 4.15 × 10-15 eV-sec), and f is the frequency of the photon. The radiographer should consider him or herself as a resource for the public and should be able to dispel any myths or misconceptions about medical imaging in general. color) of radiant energy emitted by a blackbody depends on only its temperature, not its surface or composition. • Differentiate between electromagnetic and particulate radiation. They all have the same velocity—the speed of light—and vary only in their energy, wavelength, and frequency. Both ends of the electromagnetic spectrum are used in medical imaging. particulate radiation Planck’s constant Electromagnetic nature of radiations is explained by James Maxwell (1870). unit of frequency ( ν) is hertz (Hz, s −1 ). The radiographer should consider him or herself as a resource for the public and should be able to dispel any myths or misconceptions about medical imaging in general. In general, it is the radiographer’s role to be familiar with the different types of radiation to which patients may be exposed and to be able to answer questions and educate patients. Class 11: Chemistry: Structure of Atom-I: Particle Nature of Electromagnetic Radiation: Planck’s quantum Theory Chapter 3 DE Broglie, in his PhD thesis, proposed that if wave (light) has particle (quantum) nature, on the basis of natural symmetry, a particle must have the wave associated with it. Light, that is, visible, infrared and ultraviolet light, is usually described as though it is a wave. He or she should also understand the nature of radiation well enough to safely use it for medical imaging purposes. Sometimes, however, electromagnetic radiation seems to behave like discrete, or separate, particles rather than waves. Very soon, it was experimentally confirmed by Davisson and Germer that the electron shows the diffraction pattern and therefore has the wave associated with it. Since the energy of a particle of light depends on its frequency, an incoming particle with a high enough frequency will have a high enough energy to liberate an electron from a metal. The magnetic and the electric fields come at 90° to each other and the combined waves move perpendicular to both electric and magnetic oscillating fields occurring the disturbance. This chapter introduces the nature of electromagnetic and particulate radiation. I would like to throw some light to the history and developements of what led to the failure of the wave nature of light. Maxwell's equations were confirmed by Heinrich Hertz through experiments with radio waves. gamma rays Radio waves, microwaves, infrared, visible light, UV-rays, X-rays, gamma rays are electromagnetic radiation. beta particles The higher the intensity of light shining on a metal, the more packets, or particles, the metal absorbs and the more electrons are emitted. Summary • Explain wave-particle duality as it applies to the electromagnetic spectrum. The radiographer should consider him or herself as a resource for the public and should be able to dispel any myths or misconceptions about medical imaging in general. The energy of electromagnetic radiation can be calculated by the following formula: The wave-particle duality of photons and electromagnetic radiation is enshrined in an equation first proposed by the German physicist Max Planck (1858 to 1947). Students may wonder why it is necessary for the radiographer to understand the entire spectrum of radiation. Objectives As previously stated, the velocity for all electromagnetic radiation is the same: 3 × 108 m/s. Related In the latter half of the 19th century, the physicist James Maxwell developed his electromagnetic theory, significantly advancing the world of physics. • Describe the nature of particulate radiation. radioactivity ultraviolet light FIGURE 3-1 Electromagnetic Radiation.Electromagnetic radiation is energy traveling at the speed of light in waves as an electric and magnetic disturbance in space. This chapter introduces the nature of electromagnetic and particulate radiation. Conceptually we can talk about electromagnetic radiation based on its wave characteristics of velocity, amplitude, wavelength, and frequency. The physicist Max Planck first described the direct proportionality between energy and frequency; that is, as the frequency increases, so does the energy. Critical Concept 3-2 Difference between Electromagnetic and Mechanical Energy Introduction Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. Unlike mechanical energy, which requires an object or matter to act through, electromagnetic energy can exist apart from matter and can travel through a vacuum. Electromagnetic radiation is a form of energy that originates from the atom. Applying Einstein's special theory of relativity, the relationship between energy (E) and momentum (p) of a particle is E = [ (pc) 2 + (mc 2) 2] (1/2) where m is the rest mass of the particle and c is the velocity of light in a vacuum. In the absence of the intervening air molecules, no sound would reach the ear. Describe the nature of the electromagnetic spectrum. Chemistry Journal 2.2 Electromagnetic Radiation Driving Question: How does the nature of particles, waves, and energy explain phenomena such as lightning? Einstein proposed that electromagnetic radiation has a wave-particle nature, that the energy of a quantum, or photon, depends on the frequency of the radiation, and that the energy of the photon is given by the formula Ephoton=hv. For example, sound is a form of mechanical energy. electromagnetic radiation EM radiation can exhibit interference patterns. The photon is now regarded as a particle in fields related to the interaction of material with light that is absorbed and emitted; and regarded as a wave in regions relating to light propagation. Log In or Register to continue hertz (Hz) In general, it is the radiographer’s role to be familiar with the different types of radiation to which patients may be exposed and to be able to answer questions and educate patients. FIGURE 3-2 Electromagnetic Spectrum.The electromagnetic spectrum energy, frequency, and wavelength ranges are continuous, with energies from 10−12 to 1010 eV. With this rationale in mind, the electromagnetic spectrum is discussed first, followed by a discussion of particulate radiation. In general, it is the radiographer’s role to be familiar with the different types of radiation to which patients may be exposed and to be able to answer questions and educate patients. In phenomenon like reflection, refraction and diffraction it shows wave nature and in phenomenon like photoelectric effects, it shows particle nature. For a photon: P = h v c. Therefore, h p = c v = λ. Key Terms While investigating the scattering of X-rays, he observed that such rays lose some of their energy in the scattering process and emerge with slightly decreased frequency. Electromagnetic energy differs from mechanical energy in that it does not require a medium in which to travel. This question about the nature of electromagnetic radiation was debated by scientists for more than two centuries, starting in the 1600s. • Calculate the wavelength or frequency of electromagnetic radiation. infrared light The key difference between wave and particle nature of light is that the wave nature of light states that light can behave as an electromagnetic wave, whereas the particle nature of light states that light consists of particles called photons. 6.11 Hess’s Law and Enthalpies for Different Types of Reactions, 06.13 Enthalpy of solution and Lattice Enthalpy, 6.13 Enthalpy of Solution and Lattice Enthalpy, 07.02 Equilibrium In Physical Processes – I, 7.02 Equilibrium In Physical Processes - I, 07.03 Equilibrium In Physical Processes – II, 7.03 Equilibrium In Physical Processes - II, 07.04 Equilibrium in Chemical Processes – Dynamic Equilibrium, 7.04 Equilibrium in Chemical Processes - Dynamic Equilibrium, 07.05 Law of Chemical Equilibrium and Equilibrium Constant, 7.05 Law of Chemical Equilibrium and Equilibrium Constant, 07.08 Characteristics and Applications of Equilibrium Constants, 7.08 Characteristics and Applications of Equilibrium Constants - I, 07.09 Characteristics and Applications of Equilibrium Constants – II, 7.09 Characteristics and Applications of Equilibrium Constants - II, 07.10 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G, 7.10 Relationship Between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G, 07.14 Acids, Bases and Salts – Arrhenius Concept, 7.14 Acids, Bases and Salts - Arrhenius Concept, 07.15 Acids, Bases and Salts – Brönsted-Lowry Concept and Lewis Concept, 7.15 Acids, Bases and Salts - Brönsted-Lowry Concept and Lewis Concept, 07.16 Ionization of Acids and Bases and KW of Water, 7.16 Ionization of Acids and Bases and KW of Water, 07.18 Ionization Constants of Weak Acids and Weak Bases, 7.18 Ionization Constants of Weak Acids and Weak Bases, 07.19 Factors Affecting Acid Strength and Common Ion Effect, 7.19 Factors Affecting Acid Strength and Common Ion Effect, 07.20 Hydrolysis of Salts and the pH of their solutions, 7.20 Hydrolysis of Salts and the pH of their solutions, 08.02 Redox Reaction in terms of Electron Transfer Reaction, 8.02 Redox Reaction in Terms of Electron Transfer, 08.08 Redox Reactions as Basis for Titration, 8.08 Redox Reactions as Basis for Titration, 08.09 Redox Reactions and Electrode processes, 8.09 Redox Reactions and Electrode Processes, 09.01 Introduction to Hydrogen and its Isotopes, 9.01 Introduction to Hydrogen and Its Isotopes, 09.06 Structure of Water and Ice, Hard and Soft water, 9.06 Structure of Water and Ice, Hard and Soft water, 10.02 Group I Elements /Alkali Metals: Properties – I, 10.02 Group I Elements (Alkali Metals) Properties - I, 10.03 Group I Elements /Alkali Metals: Properties – II, 10.03 Group I Elements (Alkali Metals) Properties - II, 10.04 General Characteristics of Compounds of Alkali Metals, 10.05 Anomalous Properties of Lithium and diagonal relationship, 10.05 Anomalous Properties of Lithium and Diagonal Relationship, 10.06 Compounds of Sodium: Na2CO3 and NaHCO3, 10.06 Compounds of Sodium - Na2CO3 and NaHCO3, 10.07 Compounds of Sodium - NaCl and NaOH, 10.08 Group II Elements “Alkaline Earth Metals”- I, 10.08 Group II Elements (Alkaline Earth Metals) - I, 10.09 Group II Elements “Alkaline Earth Metals”- II, 10.09 Group II Elements (Alkaline Earth Metals) - II, 10.10 Uses of Alkali Metals and Alkaline Earth Metals, 10.11 General Characteristics of Compounds of Alkaline Earth Metals, 10.12 Anomalous Behaviour of Beryllium and Diagonal Relationship, 10.13 Some Important Compounds of Calcium: CaO and Ca(OH)2, 10.13 Some Important Compounds of Calcium - CaO and Ca(OH)2, 10.14 Important Compounds of Calcium: CaCO3, CaSO4 and Cement, 10.14 Important Compounds of Calcium - CaCO3, CaSO4 and Cement, 11.03 Group 13 Elements: The Boron Family, 11.03 Group 13 Elements - The Boron Family, 11.04 The Boron Family: Chemical Properties, 11.04 The Boron Family - Chemical Properties, 11.06 Boron and its compounds – Ortho Boric Acid and Diborane, 11.06 Boron and Its Compounds - Ortho Boric Acid and Diborane, 11.07 Uses of Boron and Aluminium And their Compounds, 11.07 Uses of Boron and Aluminium and Their Compounds, 11.08 The Carbon Family Overview and Physical Properties, 11.09 The Carbon Family Overview and Chemical Properties, 11.10 Important Trends and Anomalous Behaviour of Carbon, 11.12 Important Compounds of Carbon: Carbon Monoxide, 11.12 Important Compounds of Carbon - Carbon Monoxide, 11.13 Important Compounds of Carbon: Carbon dioxide, 11.13 Important Compounds of Carbon - Carbon Dioxide, 11.14 Important Compounds of Silicon: Silicon dioxide, 11.14 Important Compounds of Silicon - Silicon Dioxide, 11.15 Important Compounds of Carbon: Silicones, Silicates, Zeolites, 11.15 Important Compounds of Carbon - Silicones, Silicates, Zeolites, 12 Organic Chemistry - Some Basic Principles and Techniques, 12.01 Organic Chemistry and Tetravalence of Carbon, 12.02 Structural Representation of Organic Compounds, 12.03 Classification of Organic Compounds, 12.05 Nomenclature of branched chain alkanes, 12.05 Nomenclature of Branched Chain Alkanes, 12.06 Nomenclature of Organic Compounds with Functional Group, 12.06 Nomenclature of Organic Compounds with Functional Group, 12.07 Nomenclature of Substituted Benzene Compounds, 12.12 Resonance Structure and Resonance Effect, 12.12 Resonance Structure and Resonance Effect, 12.13 Electromeric Effect and Hyperconjugation, 12.14 Methods of purification of organic compound – Sublimation, Crystallisation, Distillation, 12.14 Methods of Purification of Organic Compound, 12.15 Methods of purification of organic compound – Fractional Distillation and Steam Distillation, 12.15 Methods of Purification of Organic Compound, 12.16 Methods of purification of organic compound – Differential Extraction and Chromatography, 12.16 Methods of Purification of Organic Compound, 12.17 Methods of purification of organic compound- Column, Thin layer and Partition Chromatography, 12.17 Methods of Purification of Organic Compound, 12.18 Qualitative analysis of organic compounds, 12.18 Qualitative Analysis of Organic Compounds, 12.19 Quantitative analysis of Carbon and Hydrogen, 12.19 Quantitative Analysis of Carbon and Hydrogen, 13.01 Hydrocarbons Overview and Classification, 13.04 Physical and Chemical Properties of Alkanes – I, 13.04 Physical and Chemical Properties of Alkanes - I, 13.05 Physical and Chemical Properties of Alkanes – II, 13.05 Physical and Chemical Properties of Alkanes - II, 13.07 Alkenes – Structure, Nomenclature, And Isomerism, 13.07 Alkenes - Structure, Nomenclature and Isomerism, 13.09 Physical and Chemical Properties of Alkenes – I, 13.09 Physical and Chemical Properties of Alkenes, 13.10 Physical and Chemical Properties of Alkenes – II, 13.10 Physical and Chemical Properties of Alkenes, 13.11 Alkynes – Structure, Nomenclature and Isomerism, 13.11 Alkynes - Structure, Nomenclature and Isomerism, 13.13 Physical and Chemical Properties of Alkynes – I, 13.13 Physical and Chemical Properties of Alkynes, 13.14 Physical and Chemical Properties of Alkynes – II, 13.14 Physical and Chemical Properties of Alkynes, 13.15 Benzene, Preparation and Physical Properties, 13.16 Aromatic Hydrocarbons – Structure, Nomenclature and Isomerism, 13.16 Aromatic Hydrocarbons - Structure, Nomenclature and Isomerism, 13.19 Mechanism of Electrophilic Substitution Reactions, 13.19 Mechanism of Electrophilic Substitution Reaction, 13.20 Directive influence of a functional group in Monosubstituted Benzene, 13.20 Directive Influence of a Functional Group in Mono substituted Benzene, 14.02 Tropospheric pollutants : Gaseous air pollutant – I, 14.2 Tropospheric Pollutants - Gaseous air Pollutant, 14.03 Tropospheric pollutants : Gaseous air pollutant – II, 14.03 Tropospheric Pollutants - Gaseous Air Pollutant, 14.04 Global Warming and Greenhouse Effect, 14.06 Tropospheric pollutants : Particulate pollutant, 14.06 Tropospheric Pollutants - Particulate Pollutant, 14.10 Water Pollution: Chemical Pollutant, 14.10 Water Pollution - Chemical Pollutant, 14.11 Soil Pollution, Pesticides and Industrial Waste, 14.12 Strategies to control environmental pollution, 14.12 Strategies to Control Environmental Pollution, Chapter 14 Environmental Chemistry - Test. Refraction, diffraction and the Doppler effect are all behaviors of light that can only be explained by wave mechanics. Electromagnetic radiation may be defined as “an electric and magnetic disturbance traveling through space at the speed of light.” The electromagnetic spectrum is a way of ordering or grouping the different electromagnetic radiations. He or she should also understand the nature of radiation well enough to safely use it for medical imaging purposes. Electrons emitted in this manner are called photoelectrons. Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. There are only two ways to transfer energy from one place to another place. The energy is measured in electron volts (eV). Compton effect Convincing evidence of the particle nature of electromagnetic radiation was found in 1922 by the American physicist Arthur Holly Compton. Hurry! Dismiss, 01.05 Properties of Matter and their Measurement, 1.05 Properties of Matter and their Measurement, 01.06 The International System of Units (SI Units), 01.08 Uncertainty in Measurement: Scientific Notation, 1.08 Uncertainty in Measurement: Scientific Notation, 01.09 Arithmetic Operations using Scientific Notation, 1.09 Arithmetic Operations Using Scientific Notation, 01.12 Arithmetic Operations of Significant Figures, 1.12 Arithmetic Operations of Significant Figures, 01.17 Atomic Mass and Average Atomic Mass, 02.22 Dual Behaviour of Electromagnetic Radiation, 2.22 Dual Behaviour of Electromagnetic Radiation, 02.23 Particle Nature of Electromagnetic Radiation: Numericals, 2.23 Particle Nature of Electromagnetic Radiation - Numericals, 02.24 Evidence for the quantized Electronic Energy Levels: Atomic Spectra, 2.24 Evidence for the Quantized Electronic Energy Levels - Atomic Spectra, 02.28 Importance of Bohr’s Theory of Hydrogen Atom, 2.28 Importance of Bohr’s Theory of Hydrogen Atom, 02.29 Bohr’s Theory and Line Spectrum of Hydrogen – I, 2.29 Bohr’s Theory and Line Spectrum of Hydrogen - I, 02.30 Bohr’s Theory and Line Spectrum of Hydrogen – II, 2.30 Bohr’s Theory and Line Spectrum of Hydrogen - II, 02.33 Dual Behaviour of Matter: Numericals, 2.33 Dual Behaviour of Matter - Numerical, 02.35 Significance of Heisenberg’s Uncertainty Principle, 2.35 Significance of Heisenberg’s Uncertainty Principle, 02.36 Heisenberg’s Uncertainty Principle: Numericals, 2.36 Heisenberg's Uncertainty Principle - Numerical, 02.38 Quantum Mechanical Model of Atom: Introduction, 2.38 Quantum Mechanical Model of Atom - Introduction, 02.39 Hydrogen Atom and the Schrödinger Equation, 2.39 Hydrogen Atom and the Schrödinger Equation, 02.40 Important Features of Quantum Mechanical Model of Atom, 2.40 Important Features of Quantum Mechanical Model of Atom, 03 Classification of Elements and Periodicity in Properties, 03.01 Why do we need to classify elements, 03.02 Genesis of Periodic classification – I, 3.02 Genesis of Periodic Classification - I, 03.03 Genesis of Periodic classification – II, 3.03 Genesis of Periodic Classification - II, 03.04 Modern Periodic Law and Present Form of Periodic Table, 3.04 Modern Periodic Law and Present Form of Periodic Table, 03.05 Nomenclature of Elements with Atomic Numbers > 100, 3.05 Nomenclature of Elements with Atomic Numbers > 100, 03.06 Electronic Configurations of Elements and the Periodic Table – I, 3.06 Electronic Configurations of Elements and the Periodic Table - I, 03.07 Electronic Configurations of Elements and the Periodic Table – II, 3.07 Electronic Configurations of Elements and the Periodic Table - II, 03.08 Electronic Configurations and Types of Elements: s-block – I, 3.08 Electronic Configurations and Types of Elements - s-block - I, 03.09 Electronic Configurations and Types of Elements: p-blocks – II, 3.09 Electronic Configurations and Types of Elements - p-blocks - II, 03.10 Electronic Configurations and Types of Elements: Exceptions in periodic table – III, 3.10 Electronic Configurations and Types of Elements - Exceptions in Periodic Table - III, 03.11 Electronic Configurations and Types of Elements: d-block – IV, 3.11 Electronic Configurations and Types of Elements - d-block - IV, 03.12 Electronic Configurations and Types of Elements: f-block – V, 3.12 Electronic Configurations and Types of Elements - f-block - V, 03.18 Factors affecting Ionization Enthalpy, 3.18 Factors Affecting Ionization Enthalpy, 03.20 Trends in Ionization Enthalpy – II, 04 Chemical Bonding and Molecular Structure, 04.01 Kossel-Lewis approach to Chemical Bonding, 4.01 Kössel-Lewis Approach to Chemical Bonding, 04.03 The Lewis Structures and Formal Charge, 4.03 The Lewis Structures and Formal Charge, 04.06 Bond Length, Bond Angle and Bond Order, 4.06 Bond Length, Bond Angle and Bond Order, 04.10 The Valence Shell Electron Pair Repulsion (VSEPR) Theory, 4.10 The Valence Shell Electron Pair Repulsion (VSEPR) Theory, 04.12 Types of Overlapping and Nature of Covalent Bonds, 4.12 Types of Overlapping and Nature of Covalent Bonds, 04.17 Formation of Molecular Orbitals (LCAO Method), 4.17 Formation of Molecular Orbitals (LCAO Method), 04.18 Types of Molecular Orbitals and Energy Level Diagram, 4.18 Types of Molecular Orbitals and Energy Level Diagram, 04.19 Electronic Configuration and Molecular Behavior, 4.19 Electronic Configuration and Molecular Behaviour, Chapter 4 Chemical Bonding and Molecular Structure - Test, 05.02 Dipole-Dipole Forces And Hydrogen Bond, 5.02 Dipole-Dipole Forces and Hydrogen Bond, 05.03 Dipole-Induced Dipole Forces and Repulsive Intermolecular Forces, 5.03 Dipole-Induced Dipole Forces and Repulsive Intermolecular Forces, 05.04 Thermal Interaction and Intermolecular Forces, 5.04 Thermal Interaction and Intermolecular Forces, 05.08 The Gas Laws : Gay Lussac’s Law and Avogadro’s Law, 5.08 The Gas Laws - Gay Lussac’s Law and Avogadro’s Law, 05.10 Dalton’s Law of Partial Pressure – I, 05.12 Deviation of Real Gases from Ideal Gas Behaviour, 5.12 Deviation of Real Gases from Ideal Gas Behaviour, 05.13 Pressure -Volume Correction and Compressibility Factor, 5.13 Pressure - Volume Correction and Compressibility Factor, 06.02 Internal Energy as a State Function – I, 6.02 Internal Energy as a State Function - I, 06.03 Internal Energy as a State Function – II, 6.03 Internal Energy as a State Function - II, 06.06 Extensive and Intensive properties, Heat Capacity and their Relations, 6.06 Extensive and Intensive Properties, Heat Capacity and their Relations, 06.07 Measurement of ΔU and ΔH : Calorimetry, 6.07 Measurement of ΔU and ΔH - Calorimetry, 06.08 Enthalpy change, ΔrH of Reaction – I, 6.08 Enthalpy change, ΔrH of Reaction - I, 06.09 Enthalpy change, ΔrH of Reaction – II, 6.09 Enthalpy Change, ΔrH of Reaction - II, 06.10 Enthalpy change, ΔrH of Reaction – III, 6.10 Enthalpy Change, ΔrH of Reaction - III. Electromagnetic and Particulate Radiation One difference between the “ends” of the spectrum is that only high-energy radiation (x-rays and gamma rays) has the ability to ionize matter. He or she should also understand the nature of radiation well enough to safely use it for medical imaging purposes. 3.6 The Dual Nature of Electromagnetic Energy Learning Objectives Explain how the double slit experiment demonstrates wave-particle duality at the quantum scale. radiowaves • Discuss the energy, wavelength, and frequency of each member of the electromagnetic spectrum and how these characteristics affect its behavior in interacting with matter. More specifically, the radiographer should be able to explain to a patient the nature of ionizing radiation as well as any risks and benefits, and should be an advocate for the patient in such discussions with other professionals. the number of waves that pass by a fixed point during a given amount of time FQ: In what ways do electrons act as particles and waves? Explain wave-particle duality as it applies to the electromagnetic spectrum. Electromagnetic radiation is a form of energy that originates from the atom. Tags: Essentials of Radiographic Physics and Imaging That is, electromagnetic radiations are emitted when changes in atoms occur, such as when electrons undergo orbital transitions or atomic nuclei emit excess energy to regain stability. Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. The ranges of energy, frequency, and wavelength of the electromagnetic spectrum are continuous—that is, one constituent blends into the next (Figure 3-2). The American chemist Gilbert Lewis later coined the term photon for light quanta. X-rays and gamma rays are used for imaging in radiology and nuclear medicine, respectively. Electromagnetic Radiation Both ends of the electromagnetic spectrum are used in medical imaging. The particle nature of light can be demonstrated by the interaction of photons with matter. In this theory he explained that all. The members of the electromagnetic spectrum from lowest energy to highest are radiowaves, microwaves, infrared light, visible light, ultraviolet light, x-rays, and gamma rays. nature of ionizing radiation as well as any risks and benefits, and should be an advocate for the patient in such discussions with other professionals. Because the speed of EM waves predicted by the wave equation coincided with the measured speed of light, Maxwell concluded that light itself is an EM wave. The Rest of the Spectrum One phenomenon that seemed to contradict the theories of classical physics was blackbody radiation, which is electromagnetic radiation given off by a hot object. As a result, the particle nature of light comes into play when it interacts with metals and irradiates free electrons. All electromagnetic radiations have the same nature in that they are electric and magnetic disturbances traveling through space. • Describe the nature of the electromagnetic spectrum. Share this:Click to share on Twitter (Opens in new window)Click to share on Facebook (Opens in new window)Click to share on Google+ (Opens in new window) Introduction This property is explained in this chapter. • Differentiate between electromagnetic and particulate radiation. The sound from a speaker vibrates molecules of air adjacent to the speaker, which then pass the vibration to other nearby molecules until they reach the listener’s ear. v = particle speed. unit of wavelength is metre (m). When electromagnetic (EM) radiation is explained using the particle model, which particle-like behavior is being described? Difference between Electromagnetic and Mechanical Energy. that electromagnetic radiation can only exist as “packets” of energy, later called, Click to share on Twitter (Opens in new window), Click to share on Facebook (Opens in new window), Click to share on Google+ (Opens in new window), on Electromagnetic and Particulate Radiation. (b) De-broglie wavelength is given by: λ = h p. λ = h … Thus, De-Broglie equation equals the wavelength of em radiation of which the photon is a quantum of energy and momentum. Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. ionization • Explain wave-particle duality as it applies to the electromagnetic spectrum. Electromagnetic Radiation • Differentiate between x-rays and gamma rays and the rest of the electromagnetic spectrum. Visible light and other types of electromagnetic radiation are usually described as waves. This phenomenon is called wave-particle duality, which is essentially the idea that there are two equally correct ways to describe electromagnetic radiation. In this theory he explained that all electromagnetic radiation is very similar in that it has no mass, carries energy in waves as electric and magnetic disturbances in space, and travels at the speed of light (Figure 3-1). The energy of a photon E and the frequency of the electromagnetic radiation associated with it are related in the following way: \[E=h \upsilon \label{2}\] So does electromagnetic radiation consist of waves or particles? Electrons in Atoms: Particle Nature Directions: Using this linked PDF, complete the following questions.They are in order with the reading. The wavelengths of the electromagnetic spectrum range from 106 to10-16 meters (m) and the frequencies range from 102 to 1024 hertz (Hz). photon Wave Nature of Electromagnetic Radiation: James Maxwell (1870) was the first to give a comprehensive explanation about the interaction between the charged bodies and the behavior of electrical and magnetic fields on the macroscopic level. All electromagnetic radiations have the same nature in that they are electric and magnetic disturbances traveling through space. 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