Electromagnetic radiation can be defined as a form of energy that is produced by the movement of electrically charged particles traveling through a matter or vacuum or by oscillating magnetic and electric disturbance. Differentiate between electromagnetic and particulate radiation. frequency Sub Atomic Particles; 2.1.1. The Rest of the 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. microwaves The constant, h, which is named for Planck, is a mathematical value used to calculate photon energies based on frequency. 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. Both ends of the electromagnetic spectrum are used in medical imaging. inverse square law radiowaves radioactivity Wave-particle duality is a concept in quantum mechanics. Critical Concept 3-1 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. • Explain the relationship between energy and frequency of electromagnetic radiation. His work is considered by many to be one of the greatest advances of physics. 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 members of the electromagnetic spectrum from lowest energy to highest are radiowaves, microwaves, infrared light, visible light, ultraviolet light, x-rays, and gamma rays. Wavelength and frequency are discussed shortly. 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. Video explain methods & techniques to solve numericals on particle nature of electromagnetic radiations helpful for CBSE 11 Chemistry Ch.2 structure of atom All electromagnetic radiations have the same nature in that they are electric and magnetic disturbances traveling through space. They all have the same velocity—the speed of light—and vary only in their energy, wavelength, and frequency. Critical Concept 3-2 • Explain the relationship between energy and frequency of electromagnetic radiation. Electromagnetic waves travel at the speed of 3.0 × 10 8 m/s, which is the speed of light (denoted by c ). Differentiate between x-rays and gamma rays and the rest of the electromagnetic spectrum. Rather, the energy itself vibrates. As previously stated, the velocity for all electromagnetic radiation is the same: 3 × 108 m/s. • Differentiate between x-rays and gamma rays and the rest of the electromagnetic spectrum. Planck theorized that electromagnetic radiation can only exist as “packets” of energy, later called photons. Explain the relationship between energy and frequency of electromagnetic radiation. Electromagnetic Radiation It is a form of energy that can propagate in vacuum or material medium and shows both wave like and particle like properties. The Particle Nature of Light 1. Students may wonder why it is necessary for the radiographer to understand the entire spectrum of radiation. Only gold members can continue reading. particle nature of electromagnetic radiation and planck's quantum theory The electromagnetic wave theory of radiation believed in the continuous generation of energy. 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) • Calculate the wavelength or frequency of electromagnetic radiation. 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. particulate radiation The energy of the electromagnetic spectrum ranges from 10-12 to 1010 eV. • Discuss the energy, wavelength, and frequency of each member of the electromagnetic spectrum and how these characteristics affect its behavior in interacting with matter. Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. This ability to describe reality in the form of waves is at the heart of quantum mechanics. The amplitude refers to the maximum height of a wave. 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. 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. The energy of the electromagnetic spectrum ranges from 10-12 to 1010 eV. One way in which light interacts with matter is via the photoelectric effect, which will be studied in detail in . This chapter introduces the nature of electromagnetic and particulate radiation. In the absence of the intervening air molecules, no sound would reach the ear. \n Particle/wave nature of electromagnetic radiation \n \n Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. The S.I. • Differentiate between electromagnetic and particulate radiation. In the latter half of the 19th century, the physicist James Maxwell developed his electromagnetic theory, significantly advancing the world of physics. 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. • Describe the nature of the electromagnetic spectrum. 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. v = particle speed. He or she should also understand the nature of radiation well enough to safely use it for medical imaging purposes. The Nature of Electromagnetic Radiation Log In or Register to continue Radiowaves are used in conjunction with a magnetic field in magnetic resonance imaging (MRI) to create images of the body. color) of radiant energy emitted by a blackbody depends on only its temperature, not its surface or composition. Blackbody Radiation. Conceptually we can talk about electromagnetic radiation based on its wave characteristics of velocity, amplitude, wavelength, and frequency. Describe the nature of the electromagnetic spectrum. Discovery of Electron; 2.1.2. Particulate Radiation 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. 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. With this rationale in mind, the electromagnetic spectrum is discussed first, followed by a discussion of particulate radiation. One phenomenon that seemed to contradict the theories of classical physics was blackbody radiation, which is electromagnetic radiation given off by a hot object. 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. 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 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). Planck theorized that electromagnetic radiation can only exist as “packets” of energy, later called photons. With this rationale in mind, the electromagnetic spectrum is discussed first, followed by a discussion of particulate radiation. Only photons whose energy exceeds a threshold value will cause emission of photoelectrons. Offer ending soon! Key Terms I would like to throw some light to the history and developements of what led to the failure of the wave nature of light. 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. • Identify concepts regarding the electromagnetic spectrum important for the radiographer. For example, sound is a form of mechanical energy. 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. gamma rays 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. 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. Introduction For a photon: P = h v c. Therefore, h p = c v = λ. This property is explained in this chapter. 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. 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 photoelectric effect is the emission of electrons when electromagnetic radiation, such as light, hits a material. X-rays and gamma rays are used for imaging in radiology and nuclear medicine, respectively. The physicist Max Planck first described the direct proportionality between energy and frequency; that is, as the frequency increases, so does the energy. When electromagnetic (EM) radiation is explained using the particle model, which particle-like behavior is being described? 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. The energy of a photon E and the frequency of the electromagnetic radiation associated with it are related in the following way: \[E=h \upsilon \label{2}\] • Calculate the wavelength or frequency of electromagnetic radiation. Objectives So does electromagnetic radiation consist of waves or particles? Maxwell's equations were confirmed by Heinrich Hertz through experiments with radio waves. Thus, De-Broglie equation equals the wavelength of em radiation of which the photon is a quantum of energy and momentum. electromagnetic radiation Log In or. Hurry! 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. This phenomenon is called wave-particle duality, which is essentially the idea that there are two equally correct ways to describe electromagnetic radiation. ultraviolet light Chapter 3 Electromagnetic and Particulate Radiation The particle nature of light can be demonstrated by the interaction of photons with matter. Electromagnetic radiations are characterized by the properties − frequency ( v) and wave length (λ). The wavelength (i.e. His work is considered by many to be one of the greatest advances of physics. 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. unit of frequency ( ν) is hertz (Hz, s −1 ). It states that all the particles and quantum entities have not only a wave behaviour but also a particle … Describe the nature of particulate radiation. Outline It also is a spectrum consisting of radio waves, microwaves, infrared waves, visible light, ultraviolet radiation, X-rays, and gamma rays. photon alpha particles electromagnetic spectrum This phenomenon is called wave-particle duality, which is essentially the idea that there are two equally correct ways to describe electromagnetic radiation. Compton effect Convincing evidence of the particle nature of electromagnetic radiation was found in 1922 by the American physicist Arthur Holly Compton. The major significance of the wave-particle duality is that all behavior of light and matter can be explained through the use of a differential equation which represents a wave function, generally in the form of the Schrodinger equation. Difference between Electromagnetic and Mechanical 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. 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. Conceptually we can talk about electromagnetic radiation based on its wave characteristics of velocity, amplitude, wavelength, and frequency. Charge to Mass Ratio of Electron; 2.1.3. The energy of electromagnetic radiation can be calculated by the following formula: This question can be answered both broadly and specifically. With electromagnetic radiation, it is the energy itself that is vibrating as a combination of electric and magnetic fields; it is pure energy. infrared light He or she should also understand the nature of radiation well enough to safely use it for medical imaging purposes. Refraction, diffraction and the Doppler effect are all behaviors of light that can only be explained by wave mechanics. 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. 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. Explain wave-particle duality as it applies to the electromagnetic spectrum. In this theory he explained that all. In the absence of the intervening air molecules, no sound would reach the ear. 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. There are only two ways to transfer energy from one place to another place. In fact, energy and frequency of electromagnetic radiation are related mathematically. Define waves. • Identify concepts regarding the electromagnetic spectrum important for the radiographer. This chapter introduces the nature of electromagnetic and particulate radiation. Electromagnetic Radiation is basically light, which is present in a rainbow or a double rainbow. Electromagnetic energy differs from mechanical energy in that it does not require a medium in which to travel. 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 about the nature of electromagnetic radiation was debated by scientists for more than two centuries, starting in the 1600s. They all have the same velocity—the speed of light—and vary only in their energy, wavelength, and frequency. X-rays and gamma rays are used for imaging in radiology and nuclear medicine, respectively. • Explain wave-particle duality as it applies to the electromagnetic spectrum. Conceptually we can talk about electromagnetic radiation based on its wave characteristics of … The amplitude refers to the maximum height of a wave. 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. This phenomenon is called, Essentials of Radiographic Physics and Imaging. Electromagnetic radiation exhibits properties of a wave or a particle depending on its energy and in some cases its environment. The constant, h, which is named for Planck, is a mathematical value used to calculate photon energies based on frequency. For example, sound is a form of mechanical energy. Key Features of the Photoelectric Effect 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. Difference between Electromagnetic and Mechanical Energy. FIGURE 3-2 Electromagnetic Spectrum.The electromagnetic spectrum energy, frequency, and wavelength ranges are continuous, with energies from 10−12 to 1010 eV. • Explain wave-particle duality as it applies to the electromagnetic spectrum. Light, that is, visible, infrared and ultraviolet light, is usually described as though it is a wave. EM radiation has a wavelength. 3.6 The Dual Nature of Electromagnetic Energy Learning Objectives Explain how the double slit experiment demonstrates wave-particle duality at the quantum scale. This question can be answered both broadly and specifically. 06.11 Hess’s Law and Enthalpies for Different Types of Reactions. 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. Summary In phenomenon like reflection, refraction and diffraction it shows wave nature and in phenomenon like photoelectric effects, it shows particle nature. Electromagnetic radiation is energy traveling at the speed of light in waves as an electric and magnetic disturbance in space. Related James Clerk Maxwell derived a wave form of the electric and magnetic equations, thus uncovering the wave-like nature of electric and magnetic fields and their symmetry. Identify concepts regarding the electromagnetic spectrum important for the radiographer. 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). Electrons in Atoms: Particle Nature Directions: Using this linked PDF, complete the following questions.They are in order with the reading. (1 point) EM radiation has a frequency EM radiation can move through space without a medium. He introduced a new concept that light shows dual nature. Introduction In fact, energy and frequency of electromagnetic radiation are related mathematically. 2.0.Introduction; 2.1. Sometimes, however, electromagnetic radiation seems to behave like discrete, or separate, particles rather than waves. This property is explained in this chapter. • Differentiate between electromagnetic and particulate radiation. All electromagnetic radiations have the same nature in that they are electric and magnetic disturbances traveling through space. • 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 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. • Describe the nature of particulate radiation. Electromagnetic Radiation unit of wavelength is metre (m). With electromagnetic radiation, it is the energy itself that is vibrating as a combination of electric and magnetic fields; it is pure energy. You may also needX-ray Interactions with MatterImage ProductionThe X-ray CircuitRadiographic Exposure TechniqueIntroduction to the Imaging SciencesX-ray ProductionAdditional EquipmentStructure of the Atom As a result, the particle nature of light comes into play when it interacts with metals and irradiates free electrons. Chemistry Journal 2.2 Electromagnetic Radiation Driving Question: How does the nature of particles, waves, and energy explain phenomena such as lightning? 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. 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