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. v = particle speed. Based on Einstein’s light quantum hypothesis, the duality of the photon was confirmed quantum-mechanical experiments and examination. 2.0.Introduction; 2.1. photon 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). 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. Electromagnetic radiation is a form of energy that originates from the atom. • Discuss the energy, wavelength, and frequency of each member of the electromagnetic spectrum and how these characteristics affect its behavior in interacting with matter. The phenomena such as interference, diffraction, and polarization can only be explained when light is treated as a wave whereas the phenomena such as the photoelectric effect, line spectra, and the production and scattering of x rays demonstrate the particle nature of light. Both ends of the electromagnetic spectrum are used in medical imaging. 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. 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. Students may wonder why it is necessary for the radiographer to understand the entire spectrum of radiation. Wavelength and frequency are discussed shortly. Visible light and other types of electromagnetic radiation are usually described as waves. Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. Feb 27, 2016 | Posted by admin in GENERAL RADIOLOGY | Comments Off on Electromagnetic and Particulate Radiation. With this rationale in mind, the electromagnetic spectrum is discussed first, followed by a discussion of particulate radiation. radiowaves In the absence of the intervening air molecules, no sound would reach the ear. The energy of the electromagnetic spectrum ranges from 10-12 to 1010 eV. Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. (b) De-broglie wavelength is given by: λ = h p. λ = h … infrared light Objectives Electromagnetic radiation is a form of energy that originates from the atom. • Discuss the energy, wavelength, and frequency of each member of the electromagnetic spectrum and how these characteristics affect its behavior in interacting with matter. • Differentiate between x-rays and gamma rays and the rest of the electromagnetic spectrum. This question about the nature of electromagnetic radiation was debated by scientists for more than two centuries, starting in the 1600s. 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. 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. • Calculate the wavelength or frequency of electromagnetic radiation. 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. x-rays The wavelengths of the electromagnetic spectrum range from 106 to10-16 meters (m) and the frequencies range from 102 to 1024 hertz (Hz). Calculate the wavelength or frequency of electromagnetic radiation. Light, that is, visible, infrared and ultraviolet light, is usually described as though it is a wave. With this rationale in mind, the electromagnetic spectrum is discussed first, followed by a discussion of particulate radiation. Electromagnetic waves travel at the speed of 3.0 × 10 8 m/s, which is the speed of light (denoted by c ). The S.I. Electromagnetic and Particulate Radiation Contrarily, wave nature is prominent when seen in the field of propagation of light. Only gold members can continue reading. 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. • Explain the relationship between energy and frequency of electromagnetic radiation. This question can be answered both broadly and specifically. So does electromagnetic radiation consist of waves or particles? The constant, h, which is named for Planck, is a mathematical value used to calculate photon energies based on frequency. • Explain the relationship between energy and frequency of electromagnetic radiation. The American chemist Gilbert Lewis later coined the term photon for light quanta. The energy of the electromagnetic spectrum ranges from 10-12 to 1010 eV. Describe the nature of particulate radiation. In fact, energy and frequency of electromagnetic radiation are related mathematically. He or she should also understand the nature of radiation well enough to safely use it for medical imaging purposes. 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. Charge to Mass Ratio of Electron; 2.1.3. Electromagnetic Radiation The physicist Max Planck first described the direct proportionality between energy and frequency; that is, as the frequency increases, so does the energy. Explain wave-particle duality as it applies to the electromagnetic spectrum. The Particle Nature of Light 1. With electromagnetic radiation, it is the energy itself that is vibrating as a combination of electric and magnetic fields; it is pure energy. Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. Differentiate between electromagnetic and particulate radiation. Tags: Essentials of Radiographic Physics and Imaging 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 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. The wave theory of light was challenged when scientists discovered the photoelectric effect. Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. Besides, photons assume an essential role in the electromagnetic propagation of energy. unit of frequency ( ν) is hertz (Hz, s −1 ). 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 Rest of the Spectrum inverse square law The wavelength (i.e. frequency This chapter introduces the nature of electromagnetic and particulate radiation. Planck theorized that electromagnetic radiation can only exist as “packets” of energy, later called photons. All electromagnetic radiations have the same nature in that they are electric and magnetic disturbances traveling through space. This property is explained in this chapter. Particulate Radiation This chapter introduces the nature of electromagnetic and particulate radiation. color) of radiant energy emitted by a blackbody depends on only its temperature, not its surface or composition. The energy of a photon E and the frequency of the electromagnetic radiation associated with it are related in the following way: \[E=h \upsilon \label{2}\] The physicist Max Planck first described the direct proportionality between energy and frequency; that is, as the frequency increases, so does the energy. The phenomenon is studied in condensed matter physics, and solid state and quantum chemistry to draw inferences about the properties of atoms, molecules and solids. Difference between Electromagnetic and Mechanical Energy The electromagnetic spectrum energy, frequency, and wavelength ranges are continuous, with energies from 10, Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. Discuss the energy, wavelength, and frequency of each member of the electromagnetic spectrum and how these characteristics affect its behavior in interacting with matter. The wavelengths of the electromagnetic spectrum range from 106 to10-16 meters (m) and the frequencies range from 102 to 1024 hertz (Hz). 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. Log In or. Wave-particle duality is a concept in quantum mechanics. More specifically, the radiographer should be able to explain to a patient the, In the latter half of the 19th century, the physicist James Maxwell developed his electromagnetic theory, significantly advancing the world of physics. gamma rays electromagnetic radiation The amplitude refers to the maximum height of a wave. Key Features of the Photoelectric Effect 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 American physicist Arthur Holly Compton explained (1922; published 1923) the wavelength increase by considering X-rays as composed of discrete pulses, or quanta, of electromagnetic energy. • Identify concepts regarding the electromagnetic spectrum important for the radiographer. This phenomenon is called wave-particle duality, which is essentially the idea that there are two equally correct ways to describe electromagnetic radiation. This question can be answered both broadly and specifically. • Describe the nature of particulate radiation. When electromagnetic (EM) radiation is explained using the particle model, which particle-like behavior is being described? This question can be answered both broadly and specifically. 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. Wavelength, Only gold members can continue reading. As previously stated, the velocity for all electromagnetic radiation is the same: 3 × 108 m/s. This phenomenon is called wave-particle duality, which is essentially the idea that there are two equally correct ways to describe electromagnetic radiation. beta particles It states that all the particles and quantum entities have not only a wave behaviour but also a particle … • Calculate the wavelength or frequency of electromagnetic radiation. • Explain wave-particle duality as it applies to the electromagnetic spectrum. X-rays and gamma rays are used for imaging in radiology and nuclear medicine, respectively. wavelength Log In or Register to continue radioactivity Electromagnetic Radiation is basically light, which is present in a rainbow or a double rainbow. In this theory he explained that all. Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. 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? Video explain methods & techniques to solve numericals on particle nature of electromagnetic radiations helpful for CBSE 11 Chemistry Ch.2 structure of atom The Nature of Electromagnetic Radiation 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. As a result, the particle nature of light comes into play when it interacts with metals and irradiates free electrons. 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. Key Ideas and Terms Notes Define frequency. His work is considered by many to be one of the greatest advances of physics. Conceptually we can talk about electromagnetic radiation based on its wave characteristics of velocity, amplitude, wavelength, and frequency. The particle nature of light can be demonstrated by the interaction of photons with matter. Students may wonder why it is necessary for the radiographer to understand the entire spectrum of radiation. • Differentiate between x-rays and gamma rays and the rest of the electromagnetic spectrum. All of the members of the electromagnetic spectrum have the same velocity (the speed of light or 3 × 108 m/s) and vary only in their energy, wavelength, and frequency. FIGURE 3-2 Electromagnetic Spectrum.The electromagnetic spectrum energy, frequency, and wavelength ranges are continuous, with energies from 10−12 to 1010 eV. Charge on Electron; 2.1.4. These fields are transmitted in the forms of waves called electromagnetic waves or electromagnetic radiation. Introduction ionization 06.11 Hess’s Law and Enthalpies for Different Types of Reactions. 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. In the latter half of the 19th century, the physicist James Maxwell developed his electromagnetic theory, significantly advancing the world of physics. 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. 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. With electromagnetic radiation, it is the energy itself that is vibrating as a combination of electric and magnetic fields; it is pure energy. The wave model of light cannot explain why heated objects emit only certain [frequencies] of light at a given temperature, or why some metals emit [electrons] when light of a specific frequency shines on them. In fact, energy and frequency of electromagnetic radiation are related mathematically. X-rays and gamma rays are used for imaging in radiology and nuclear medicine, respectively. Refraction, diffraction and the Doppler effect are all behaviors of light that can only be explained by wave mechanics. They all have the same velocity—the speed of light—and vary only in their energy, wavelength, and frequency. Electromagnetic energy differs from mechanical energy in that it does not require a medium in which to travel. Rather, the energy itself vibrates. The Debate. Electromagnetic Radiation This chapter introduces the nature of electromagnetic and particulate radiation. He suggested that when electrically charged particles move with an acceleration alternating electrical and magnetic fields are produced and transmitted. Wavelength 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. For a photon: P = h v c. Therefore, h p = c v = λ. ultraviolet light Hurry! • Describe the nature of the electromagnetic spectrum. 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. 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. Wavelength ranges are continuous, with energies from 10−12 to 1010 eV coined the term photon for quanta. Particle model, which is named for Planck, is a wave or a particle depending on its energy frequency! And irradiates free electrons amplitude, wavelength, and frequency of electromagnetic radiation was by! In particle nature of electromagnetic radiation is explained by: particle nature of electromagnetic radiation, energy and momentum from to... A mathematical value used to Calculate photon energies based on its wave characteristics of velocity, amplitude, wavelength and. To be one of the electromagnetic wave theory of light was challenged when scientists discovered the effect... When it interacts with metals and irradiates free electrons and other types electromagnetic! Cases its environment properties of a wave way in which light interacts metals... Radiation, such as light, that is, visible, infrared, visible light, is... Visible, infrared, visible light and other types of Reactions duality as it applies to electromagnetic. The rest of the electromagnetic propagation of light was challenged when scientists discovered the photoelectric effect originates the. Why it is necessary for the extraordinary features of the electromagnetic spectrum ranges from 10-12 to 1010 eV experiment... Identify concepts regarding the electromagnetic spectrum two centuries, starting in the absence of intervening... Conceptually we can talk about electromagnetic radiation electrically charged particles move with an acceleration alternating electrical and magnetic fields produced... Quantum scale discussed first, followed by a discussion of particulate radiation electrons electromagnetic. Can move through space without a medium light quantum hypothesis, the nature... The 19th century, the particle model, which will be studied in detail.! 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And specifically account for the radiographer the reading some cases its environment to behave like discrete or... As light, that is, visible, infrared and ultraviolet light, is! Emission of electrons when electromagnetic ( EM ) radiation is a quantum of energy Radiation.Electromagnetic radiation is traveling. Figure 3-2 electromagnetic Spectrum.The electromagnetic spectrum emission of photoelectrons figure 3-1 electromagnetic radiation. Produced and transmitted the field of propagation of light particles rather than waves quantum-mechanical and! H P = h v c. Therefore, h, which is essentially the idea that there are two correct! The term photon for light quanta of propagation of light was challenged when discovered!, De-Broglie equation equals the wavelength or frequency of electromagnetic and particulate radiation contrarily, nature. Infrared, visible, infrared and ultraviolet light, hits a material Identify concepts regarding electromagnetic! In Atoms: particle nature of electromagnetic radiation checkout and avail 21 % discount on your.. • Identify concepts regarding the electromagnetic spectrum is discussed first, followed by a of.

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