This document provides an overview of atomic structure and theory. It begins by discussing how an understanding of atomic structure relates to materials properties. It then reviews the atomic models of Democritus, Dalton, Thomson, Rutherford, Bohr, and others. Key concepts covered include the nucleus, protons, neutrons, electrons, atomic number, mass number, and energy levels. The document also discusses atomic bonding mechanisms like ionic bonding, covalent bonding, and metallic bonding. Finally, it introduces topics like energy bands and the quantization of energy and light.
chapter 2 Atomic structure and bonding .pptxTsegaselase
This document discusses atomic structure and bonding. It begins by describing the atomic structure of elements, including subatomic particles like protons, neutrons, and electrons. It then discusses different types of atomic bonds including ionic bonds formed by electron transfer between atoms, covalent bonds formed by electron sharing, and metallic bonds formed by delocalized electrons bonding metal cations. It provides examples of different bond types and explains how bond type relates to material properties like conductivity and hardness. The document also briefly discusses secondary bonds like hydrogen bonds and van der Waals forces.
Module #22 discusses conductors, insulators, and semiconductors. It explains that conductors contain free electrons that allow electricity to flow through them easily. Insulators have electrons tightly bound and do not conduct electricity well. Semiconductors have properties between conductors and insulators, with fewer free electrons than conductors but more than insulators. Common semiconductors are silicon and germanium, which are used to make diodes and transistors.
The document discusses atomic structure and bonding. It covers the following key points in 3 sentences:
Atomic structure consists of electrons, protons, and neutrons, with electrons orbiting the nucleus. Elements are made of one type of atom, and molecules form when two or more atoms bond together through ionic, covalent, or metallic bonding. Ionic bonding occurs through electron transfer between atoms, covalent bonding involves electron sharing, and metallic bonding results from delocalized electrons interacting with positive ion cores.
The document is about the structure of an atom according to an 11th grade student named Shubham Kumar. It discusses that an atom is composed of a nucleus containing protons and neutrons, and electrons orbiting the nucleus. It also explains that protons have a positive charge, neutrons have no charge, and electrons have a negative charge, making the total charge of a neutral atom zero. The document then provides more details about the atomic nucleus, isotopes, electron configuration, and types of nuclear decay.
This document outlines the lectures for the course "Unit 1 Electronic and Photonic Materials". The lectures cover topics including:
- The importance of classical and quantum theories of free electrons.
- Fermi-Dirac statistics and how the Fermi energy level varies in semiconductors.
- The Hall effect and its applications in dilute magnetic semiconductors, superconductors, and their characteristics.
- Applications of superconductors and photonic materials.
- Photoconducting materials and non-linear optical materials and their applications.
The document discusses the development of atomic theory and models of atomic structure based on experiments. Key points include:
1. Early experiments with cathode ray tubes led Thomson to discover the electron and determine its small mass and negative charge.
2. Rutherford's gold foil experiment showed that the mass and positive charge of atoms are concentrated in a very small, dense nucleus.
3. Later experiments discovered the proton in the nucleus and the neutron, establishing the main subatomic particles that make up all elements.
4. Models evolved from Thomson's "plum pudding" model to Rutherford's nuclear model to better explain experimental results and the stability of atoms.
This document discusses basic semiconductor theory, including:
1. Semiconductors have conductivity between conductors and insulators and include materials like silicon, germanium, and gallium arsenide.
2. Doping semiconductors with impurities creates n-type or p-type materials by introducing excess electrons or holes.
3. The atomic structure of semiconductors includes valence and conduction energy bands separated by a bandgap through which electrons can jump with sufficient energy.
The document discusses the atomic structure and models of the atom. It begins with an acknowledgement and table of contents. It then covers Dalton's atomic theory, subatomic particles like electrons and protons, cathode rays and the discovery of electrons. It discusses the charge to mass ratio of electrons, the discovery of protons and neutrons, and models of the atom including Thomson's model and Rutherford's nuclear model. It also addresses isotopes, limitations of models, wave nature of radiation, and the electromagnetic spectrum.
chapter 2 Atomic structure and bonding .pptxTsegaselase
This document discusses atomic structure and bonding. It begins by describing the atomic structure of elements, including subatomic particles like protons, neutrons, and electrons. It then discusses different types of atomic bonds including ionic bonds formed by electron transfer between atoms, covalent bonds formed by electron sharing, and metallic bonds formed by delocalized electrons bonding metal cations. It provides examples of different bond types and explains how bond type relates to material properties like conductivity and hardness. The document also briefly discusses secondary bonds like hydrogen bonds and van der Waals forces.
Module #22 discusses conductors, insulators, and semiconductors. It explains that conductors contain free electrons that allow electricity to flow through them easily. Insulators have electrons tightly bound and do not conduct electricity well. Semiconductors have properties between conductors and insulators, with fewer free electrons than conductors but more than insulators. Common semiconductors are silicon and germanium, which are used to make diodes and transistors.
The document discusses atomic structure and bonding. It covers the following key points in 3 sentences:
Atomic structure consists of electrons, protons, and neutrons, with electrons orbiting the nucleus. Elements are made of one type of atom, and molecules form when two or more atoms bond together through ionic, covalent, or metallic bonding. Ionic bonding occurs through electron transfer between atoms, covalent bonding involves electron sharing, and metallic bonding results from delocalized electrons interacting with positive ion cores.
The document is about the structure of an atom according to an 11th grade student named Shubham Kumar. It discusses that an atom is composed of a nucleus containing protons and neutrons, and electrons orbiting the nucleus. It also explains that protons have a positive charge, neutrons have no charge, and electrons have a negative charge, making the total charge of a neutral atom zero. The document then provides more details about the atomic nucleus, isotopes, electron configuration, and types of nuclear decay.
This document outlines the lectures for the course "Unit 1 Electronic and Photonic Materials". The lectures cover topics including:
- The importance of classical and quantum theories of free electrons.
- Fermi-Dirac statistics and how the Fermi energy level varies in semiconductors.
- The Hall effect and its applications in dilute magnetic semiconductors, superconductors, and their characteristics.
- Applications of superconductors and photonic materials.
- Photoconducting materials and non-linear optical materials and their applications.
The document discusses the development of atomic theory and models of atomic structure based on experiments. Key points include:
1. Early experiments with cathode ray tubes led Thomson to discover the electron and determine its small mass and negative charge.
2. Rutherford's gold foil experiment showed that the mass and positive charge of atoms are concentrated in a very small, dense nucleus.
3. Later experiments discovered the proton in the nucleus and the neutron, establishing the main subatomic particles that make up all elements.
4. Models evolved from Thomson's "plum pudding" model to Rutherford's nuclear model to better explain experimental results and the stability of atoms.
This document discusses basic semiconductor theory, including:
1. Semiconductors have conductivity between conductors and insulators and include materials like silicon, germanium, and gallium arsenide.
2. Doping semiconductors with impurities creates n-type or p-type materials by introducing excess electrons or holes.
3. The atomic structure of semiconductors includes valence and conduction energy bands separated by a bandgap through which electrons can jump with sufficient energy.
The document discusses the atomic structure and models of the atom. It begins with an acknowledgement and table of contents. It then covers Dalton's atomic theory, subatomic particles like electrons and protons, cathode rays and the discovery of electrons. It discusses the charge to mass ratio of electrons, the discovery of protons and neutrons, and models of the atom including Thomson's model and Rutherford's nuclear model. It also addresses isotopes, limitations of models, wave nature of radiation, and the electromagnetic spectrum.
1. The document discusses intrinsic and extrinsic semiconductors. Intrinsic semiconductors are pure semiconductors without dopants, while extrinsic semiconductors are doped by adding donor or acceptor atoms.
2. Extrinsic semiconductors are classified as n-type or p-type based on whether electrons or holes are the majority carrier. N-type uses donor dopants to increase electron concentration, while p-type uses acceptor dopants to increase hole concentration.
3. Semiconductor devices like diodes and transistors make use of the different properties of n-type and p-type extrinsic semiconductors. Diodes consist of a p-n junction
1. Dalton's atomic theory proposed that matter consists of indivisible atoms and that atoms of different elements differ in mass. Compounds are formed by atoms combining in fixed ratios.
2. Rutherford's gold foil experiment showed that the positive charge and mass of an atom are concentrated in a very small nucleus, with electrons orbiting the nucleus.
3. The discovery of subatomic particles like electrons, protons, and neutrons led to modifications of atomic structure, with atoms composed of a nucleus surrounded by electrons.
- The document discusses atomic structure and the development of atomic models.
- Early experiments showed atoms were divisible, with Thomson discovering electrons and Rutherford discovering protons.
- Rutherford's gold foil experiment disproved Thomson's "plum pudding" atomic model and led Rutherford to propose a nuclear model with electrons in empty space around a tiny, dense nucleus.
1. The document discusses various topics related to atomic structure including classical theories of atomic structure, discovery of the proton and nucleus, electron shells, and electron dot structures.
2. It also discusses different types of chemical bonds including ionic bonds formed by electron transfer, covalent bonds formed by electron sharing, hydrogen bonds, and metallic bonds.
3. Additional topics covered include electromagnetic radiations, radioactivity, nuclear decay processes, medical and other applications of radioisotopes, and uses of radiation in agriculture and food preservation.
ELECTRON-theory ppt industrials arts part2GalangRoxanne
Electron theory aims to explain the structure and properties of matter through its electronic structure. It states that all matter is comprised of molecules made up of atoms, which contain protons, neutrons, and electrons. Electrons play a key role in electricity as their movement constitutes electric current. Within atoms, electrons exist in specific energy levels or shells around the nucleus, and their behavior is described by quantum mechanics.
1) The document discusses the topic-structure of an atom and summarizes the key discoveries that led to modern atomic theory, including the discovery of the electron, proton, neutron, and development of atomic models.
2) It describes Michael Faraday's experiments in the 1830s that provided early insights into atomic structure and the discovery of the electron in the 1850s from cathode ray experiments.
3) The document also summarizes Bohr's 1913 model of the hydrogen atom which explained its spectral lines by postulating stable electron orbits, and the development of quantum mechanics and Schrodinger's equation to more fully describe atomic structure.
Secondary Education
Chemistry
Chapter 1
Lesson 1
if you have any question don't hesitate to contact me
join the facebook group
http://www.facebook.com/#!/group.php?gid=17663120872&v=info
Best of luck
Mr.Ehab Mohamed
The atomic mass of an element can vary because the number of neutrons in the nucleus may be variable, even though the number of protons remains the same for a given element. There are four main types of atomic bonding - ionic, covalent, metallic, and van der Waals - which determine key material properties like hardness, melting point, and whether a material is a metal, polymer, or ceramic based on electron configuration and bonding forces between atoms. These bonding types arise from atoms seeking stable electron configurations through gaining, losing, or sharing valence electrons.
The document discusses key concepts related to electricity and electrical systems, including:
- Electricity is the movement of electrons between atoms. Volts, amps, and ohms are the main units of electrical measurement.
- Conductors allow electron flow, insulators do not, and semiconductors are in between. Common materials for each are described.
- Current is the flow of electrons measured in amps. Voltage is electrical pressure measured in volts. Resistance is measured in ohms.
- Sources of electricity include static, heat, light, pressure, and chemistry. Batteries use electrochemistry to generate voltage.
Chemistry Basic understanding for LIKE WHAT?ArafathIslam4
Dalton's atomic theory proposed that all matter is made of indivisible atoms and that atoms of different elements have different masses. However, later discoveries showed limitations of this theory. Atoms were found to be divisible into subatomic particles and isotopes of the same element can have different masses. Rutherford's gold foil experiment provided evidence that the mass of an atom is concentrated in a small, positively charged nucleus. This led to Rutherford's model of the atom with electrons orbiting the nucleus, like planets around the sun. However, this model could not explain the stability of atoms and quantum theory was needed to fully explain atomic structure.
Atoms are the fundamental units that make up elements. John Dalton proposed the atomic theory which states that elements are made of atoms and atoms of the same element are identical. Atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The discovery of the electron, proton, neutron, and development of quantum theory led to modern atomic structure and periodic table. The periodic table organizes elements based on atomic structure including atomic number and trends in properties.
The document provides information on the structure of atoms, including key experiments and models that helped reveal the internal structure of atoms. It discusses J.J. Thomson's cathode ray experiment that discovered electrons, Rutherford's alpha particle scattering experiment that showed atoms have a small, dense nucleus, and Bohr's model of electron orbits around the nucleus. It also covers topics like isotopes, mass number, atomic number, electron configuration, and valency.
The document discusses the history of atomic structure models from Democritus' idea of atoms to Bohr's model. Some key points:
1. J.J. Thomson's experiments in 1897 led him to propose the "plum pudding" model where electrons were embedded in a uniform positive charge.
2. Rutherford's gold foil experiment in 1911 showed that the atom has a small, dense, positively charged nucleus at its center.
3. Bohr modified Rutherford's model in 1913 to propose that electrons orbit the nucleus in discrete energy levels, explaining atomic line spectra. When electrons fall from higher to lower orbits, photons are emitted.
Indeed, the structure of an atom is fundamental to understanding the properties and behaviour of matter. At its core, an atom consists of three primary subatomic particles: protons, neutrons, and electrons. These constituents collectively determine the atom's mass and charge.
To learn more about VAVA Classes, visit: www.vavaclasses.com
1. The document outlines the development of atomic models from Dalton's atomic theory in 1803 to the quantum model in 1924. It describes key contributors including Dalton, Thomson, Millikan, Rutherford, Bohr, de Broglie, Schrodinger, and Born and their major discoveries.
2. Major milestones included Dalton establishing atoms as the basic unit of matter, Thomson discovering the electron, Rutherford discovering the nucleus, Bohr explaining electron energy levels, and the development of the quantum model explaining wave-particle duality of electrons.
3. Each new model built upon the previous work and corrected limitations, moving science closer to a full understanding of atomic structure.
Ernst Goldstein discovered positive rays (protons) in 1886 by passing cathode rays through a perforated cathode. Positive rays were produced and carried a positive charge. J.J. Thomson later determined the e/m ratio of protons depends on the gas used, with hydrogen giving the maximum ratio and identifying the lightest particle as the proton. In 1932, James Chadwick discovered the neutron through bombarding beryllium with alpha particles. The neutron was later found to be neutral and able to induce nuclear reactions. Rutherford proposed atoms consisted of electrons and protons in 1911 based on alpha scattering experiments, but the planetary model was defective as it did not explain the stability of electron orbits.
This pdf is written to describe structure of atom for school students of grades 9 to 10. In this the basics of atomic structure has been described. Starting from Dalton's atomic model to Rutherford's scatering of alpha particles, JJ Thomson and Bohr's models with photos.
Students can download and use it for studying atomic structure.
Matter is anything that occupies space and has weight. It may consist of elements or a single element. An element cannot be split into simpler substances, such as copper, oxygen, carbon, and gold. Atoms are the smallest particles of an element and are made up of protons, neutrons, and electrons. Protons are positively charged, electrons are negatively charged, and neutrons have no charge. Electricity is a branch of science concerned with charges. It can be drawn from devices like dry cells, solar cells, acid batteries, and dynamos. Conductors allow electricity to pass through easily, while insulators do not. Common terms in electricity include static electricity, current electricity, electric current, electric circuit, amp
The document discusses energy gaps between electron shells in atoms. Electrons occupy discrete energy levels organized into shells. The energy required to excite an electron to a higher shell is equal to the energy released as light when the electron returns to a lower shell. Different elements emit different colors of light corresponding to their unique electron shell energy gaps. Fireworks emit various colors from metal salts as the metals' electrons move between shells and release energy as light.
This document provides an overview of time synchronization over Ethernet for power applications using Precision Time Protocol (PTP). It discusses the IEEE 1588-2008 standard which specifies PTP, and how industry-specific PTP profiles have been developed, including IEEE C37.238-2011 which specified the initial profile for power system applications. It describes how IEEE C37.238-2011 was later split into two standards: IEC/IEEE 61850-9-3:2016 which specifies a base profile, and IEEE C37.238-2017 which specifies an extended profile with additional functionality. The document outlines some of the key aspects and changes between these standards, and discusses testing and certification efforts through the IEEE ICAP program to help facilitate
This document discusses overhead contact line systems used in rail transport. It describes trolley-type contact line systems which have a simple structure without a continuous catenary wire. These systems have a large contact wire sag and require short distances between supports to maintain a constant contact height. Various trolley-type contact line configurations are presented, including single-point suspensions, suspensions with fixed anchors, suspensions with stitch wires, and suspensions with tensioning devices to compensate for thermal expansion. The advantages of simple structures and installation are noted, along with the disadvantages of greater sag and tension variation compared to catenary systems.
1. The document discusses intrinsic and extrinsic semiconductors. Intrinsic semiconductors are pure semiconductors without dopants, while extrinsic semiconductors are doped by adding donor or acceptor atoms.
2. Extrinsic semiconductors are classified as n-type or p-type based on whether electrons or holes are the majority carrier. N-type uses donor dopants to increase electron concentration, while p-type uses acceptor dopants to increase hole concentration.
3. Semiconductor devices like diodes and transistors make use of the different properties of n-type and p-type extrinsic semiconductors. Diodes consist of a p-n junction
1. Dalton's atomic theory proposed that matter consists of indivisible atoms and that atoms of different elements differ in mass. Compounds are formed by atoms combining in fixed ratios.
2. Rutherford's gold foil experiment showed that the positive charge and mass of an atom are concentrated in a very small nucleus, with electrons orbiting the nucleus.
3. The discovery of subatomic particles like electrons, protons, and neutrons led to modifications of atomic structure, with atoms composed of a nucleus surrounded by electrons.
- The document discusses atomic structure and the development of atomic models.
- Early experiments showed atoms were divisible, with Thomson discovering electrons and Rutherford discovering protons.
- Rutherford's gold foil experiment disproved Thomson's "plum pudding" atomic model and led Rutherford to propose a nuclear model with electrons in empty space around a tiny, dense nucleus.
1. The document discusses various topics related to atomic structure including classical theories of atomic structure, discovery of the proton and nucleus, electron shells, and electron dot structures.
2. It also discusses different types of chemical bonds including ionic bonds formed by electron transfer, covalent bonds formed by electron sharing, hydrogen bonds, and metallic bonds.
3. Additional topics covered include electromagnetic radiations, radioactivity, nuclear decay processes, medical and other applications of radioisotopes, and uses of radiation in agriculture and food preservation.
ELECTRON-theory ppt industrials arts part2GalangRoxanne
Electron theory aims to explain the structure and properties of matter through its electronic structure. It states that all matter is comprised of molecules made up of atoms, which contain protons, neutrons, and electrons. Electrons play a key role in electricity as their movement constitutes electric current. Within atoms, electrons exist in specific energy levels or shells around the nucleus, and their behavior is described by quantum mechanics.
1) The document discusses the topic-structure of an atom and summarizes the key discoveries that led to modern atomic theory, including the discovery of the electron, proton, neutron, and development of atomic models.
2) It describes Michael Faraday's experiments in the 1830s that provided early insights into atomic structure and the discovery of the electron in the 1850s from cathode ray experiments.
3) The document also summarizes Bohr's 1913 model of the hydrogen atom which explained its spectral lines by postulating stable electron orbits, and the development of quantum mechanics and Schrodinger's equation to more fully describe atomic structure.
Secondary Education
Chemistry
Chapter 1
Lesson 1
if you have any question don't hesitate to contact me
join the facebook group
http://www.facebook.com/#!/group.php?gid=17663120872&v=info
Best of luck
Mr.Ehab Mohamed
The atomic mass of an element can vary because the number of neutrons in the nucleus may be variable, even though the number of protons remains the same for a given element. There are four main types of atomic bonding - ionic, covalent, metallic, and van der Waals - which determine key material properties like hardness, melting point, and whether a material is a metal, polymer, or ceramic based on electron configuration and bonding forces between atoms. These bonding types arise from atoms seeking stable electron configurations through gaining, losing, or sharing valence electrons.
The document discusses key concepts related to electricity and electrical systems, including:
- Electricity is the movement of electrons between atoms. Volts, amps, and ohms are the main units of electrical measurement.
- Conductors allow electron flow, insulators do not, and semiconductors are in between. Common materials for each are described.
- Current is the flow of electrons measured in amps. Voltage is electrical pressure measured in volts. Resistance is measured in ohms.
- Sources of electricity include static, heat, light, pressure, and chemistry. Batteries use electrochemistry to generate voltage.
Chemistry Basic understanding for LIKE WHAT?ArafathIslam4
Dalton's atomic theory proposed that all matter is made of indivisible atoms and that atoms of different elements have different masses. However, later discoveries showed limitations of this theory. Atoms were found to be divisible into subatomic particles and isotopes of the same element can have different masses. Rutherford's gold foil experiment provided evidence that the mass of an atom is concentrated in a small, positively charged nucleus. This led to Rutherford's model of the atom with electrons orbiting the nucleus, like planets around the sun. However, this model could not explain the stability of atoms and quantum theory was needed to fully explain atomic structure.
Atoms are the fundamental units that make up elements. John Dalton proposed the atomic theory which states that elements are made of atoms and atoms of the same element are identical. Atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The discovery of the electron, proton, neutron, and development of quantum theory led to modern atomic structure and periodic table. The periodic table organizes elements based on atomic structure including atomic number and trends in properties.
The document provides information on the structure of atoms, including key experiments and models that helped reveal the internal structure of atoms. It discusses J.J. Thomson's cathode ray experiment that discovered electrons, Rutherford's alpha particle scattering experiment that showed atoms have a small, dense nucleus, and Bohr's model of electron orbits around the nucleus. It also covers topics like isotopes, mass number, atomic number, electron configuration, and valency.
The document discusses the history of atomic structure models from Democritus' idea of atoms to Bohr's model. Some key points:
1. J.J. Thomson's experiments in 1897 led him to propose the "plum pudding" model where electrons were embedded in a uniform positive charge.
2. Rutherford's gold foil experiment in 1911 showed that the atom has a small, dense, positively charged nucleus at its center.
3. Bohr modified Rutherford's model in 1913 to propose that electrons orbit the nucleus in discrete energy levels, explaining atomic line spectra. When electrons fall from higher to lower orbits, photons are emitted.
Indeed, the structure of an atom is fundamental to understanding the properties and behaviour of matter. At its core, an atom consists of three primary subatomic particles: protons, neutrons, and electrons. These constituents collectively determine the atom's mass and charge.
To learn more about VAVA Classes, visit: www.vavaclasses.com
1. The document outlines the development of atomic models from Dalton's atomic theory in 1803 to the quantum model in 1924. It describes key contributors including Dalton, Thomson, Millikan, Rutherford, Bohr, de Broglie, Schrodinger, and Born and their major discoveries.
2. Major milestones included Dalton establishing atoms as the basic unit of matter, Thomson discovering the electron, Rutherford discovering the nucleus, Bohr explaining electron energy levels, and the development of the quantum model explaining wave-particle duality of electrons.
3. Each new model built upon the previous work and corrected limitations, moving science closer to a full understanding of atomic structure.
Ernst Goldstein discovered positive rays (protons) in 1886 by passing cathode rays through a perforated cathode. Positive rays were produced and carried a positive charge. J.J. Thomson later determined the e/m ratio of protons depends on the gas used, with hydrogen giving the maximum ratio and identifying the lightest particle as the proton. In 1932, James Chadwick discovered the neutron through bombarding beryllium with alpha particles. The neutron was later found to be neutral and able to induce nuclear reactions. Rutherford proposed atoms consisted of electrons and protons in 1911 based on alpha scattering experiments, but the planetary model was defective as it did not explain the stability of electron orbits.
This pdf is written to describe structure of atom for school students of grades 9 to 10. In this the basics of atomic structure has been described. Starting from Dalton's atomic model to Rutherford's scatering of alpha particles, JJ Thomson and Bohr's models with photos.
Students can download and use it for studying atomic structure.
Matter is anything that occupies space and has weight. It may consist of elements or a single element. An element cannot be split into simpler substances, such as copper, oxygen, carbon, and gold. Atoms are the smallest particles of an element and are made up of protons, neutrons, and electrons. Protons are positively charged, electrons are negatively charged, and neutrons have no charge. Electricity is a branch of science concerned with charges. It can be drawn from devices like dry cells, solar cells, acid batteries, and dynamos. Conductors allow electricity to pass through easily, while insulators do not. Common terms in electricity include static electricity, current electricity, electric current, electric circuit, amp
The document discusses energy gaps between electron shells in atoms. Electrons occupy discrete energy levels organized into shells. The energy required to excite an electron to a higher shell is equal to the energy released as light when the electron returns to a lower shell. Different elements emit different colors of light corresponding to their unique electron shell energy gaps. Fireworks emit various colors from metal salts as the metals' electrons move between shells and release energy as light.
This document provides an overview of time synchronization over Ethernet for power applications using Precision Time Protocol (PTP). It discusses the IEEE 1588-2008 standard which specifies PTP, and how industry-specific PTP profiles have been developed, including IEEE C37.238-2011 which specified the initial profile for power system applications. It describes how IEEE C37.238-2011 was later split into two standards: IEC/IEEE 61850-9-3:2016 which specifies a base profile, and IEEE C37.238-2017 which specifies an extended profile with additional functionality. The document outlines some of the key aspects and changes between these standards, and discusses testing and certification efforts through the IEEE ICAP program to help facilitate
This document discusses overhead contact line systems used in rail transport. It describes trolley-type contact line systems which have a simple structure without a continuous catenary wire. These systems have a large contact wire sag and require short distances between supports to maintain a constant contact height. Various trolley-type contact line configurations are presented, including single-point suspensions, suspensions with fixed anchors, suspensions with stitch wires, and suspensions with tensioning devices to compensate for thermal expansion. The advantages of simple structures and installation are noted, along with the disadvantages of greater sag and tension variation compared to catenary systems.
This document discusses key concepts related to entrepreneurship including:
- The meaning of entrepreneur, entrepreneurship, and intrapreneurs. Entrepreneurs start businesses and take on risk, while intrapreneurs promote innovation within organizations.
- The entrepreneurial decision process can be driven by both "pull factors" like pursuing an opportunity, and "push factors" like unemployment.
- Advantages of entrepreneurship include self-employment, job creation, and economic growth. Drawbacks include risk of failure and stress.
- Creativity and innovation are important for entrepreneurship. Techniques to develop creative thinking include brainstorming, changing existing ideas, and increasing awareness of one's environment.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
This document discusses electric drive systems. It outlines the basic elements, which include a power source, electric motor, converter, controller, and mechanical load. It describes the torque-speed characteristics of different types of motors and loads. It also covers power supplies for electric drives, including alternating current and direct current sources. Control of electric drives is also mentioned.
A DC-DC converter, also known as a chopper, can step up or step down a DC voltage source. It is widely used for traction motor control in electric vehicles, trolleys, marine lifts, forklifts, and mine haulers. DC-DC converters are also used to return energy through regenerative braking of DC motors back into the supply system, resulting in energy savings for transportation with frequent stops. They can also be used in DC voltage regulators.
This chapter introduces analog computing techniques. It discusses the components of an analog computer including operational amplifiers, resistors, capacitors and inductors. It describes how operational amplifiers can be used to simulate linear systems using inverting amplifiers, non-inverting amplifiers, summer amplifiers, integrators and differentiators. The chapter also covers how to apply magnitude and time scaling to model systems within the voltage range of an analog computer. An example shows how to derive the scaled dynamic model of a system and realize it using operational amplifiers.
Gender and Mental Health - Counselling and Family Therapy Applications and In...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
How to Setup Warehouse & Location in Odoo 17 InventoryCeline George
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptxEduSkills OECD
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Mat ch-1.pptx
1. Electrical Materials and Technology
PCE3302
Chapter One
Review of atomic theory of matters
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2. Introduction
Selection of appropriate material for the intended purpose depends on the
knowledge of properties of materials. i.e.,
Physical properties
Electrical
Mechanical
Thermal and
Chemical
These properties of materials depend on the atomic structure of that material.
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3. Atomic Structure
All matter is composed of atoms.
Understanding the structure of atoms is critical to understanding the
properties of matter
Atom – smallest particle of an element that can exist alone
Two regions of an atom
Nucleus
Center of atom
Protons and neutrons
Electron “cloud”
Area surrounding nucleus containing electrons
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4. cont’d…………
Proton – Positive charge (+), 1 atomic mass unit (amu); found in the nucleus
amu -Approximate mass of a proton or a neutron
Neutron – Neutral charge (0), 1 amu; found in the nucleus
Electron – Negative charge (-), mass is VERY small
In a neutral atom, the number of protons equals the number of electrons, so the
overall charge is zero (0)
Example/ Helium, with an atomic number of 2, has 2 protons and 2 electrons
when stable
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5. Counting Atoms
Atomic Number
Number of protons in nucleus
The number of protons determines identity of the element!!
Mass Number (Atomic Mass)
Number of protons + neutrons
Units are g/mol
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6. Atomic model
Democritus 460 BC
Greek Philosopher
Suggested world was made of two things – empty space and “atomos”
Atomos – Greek word for uncuttable
2 Main ideas
Atoms are the smallest possible particle of matter
There are different types of atoms for each material
His ideas did agree with later scientific theory, but did
not explain chemical behavior, and was not based
on the scientific method – but just philosophy
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7. Cont’d……
John Dalton’s Atomic Theory (1766 - 1844)
Dalton was an English school teacher who performed
many experiments on atoms.
All matter is made of atoms.
Atoms of one element are all the same.
Atoms cannot be broken down into smaller parts
Compounds form by combining atoms
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8. Dalton’s Early Atomic Mode
“Billiard Ball” model
He envisioned atoms as solid, hard spheres, like billiard(pool) balls
So he used wooden balls to model them
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9. J.J. Thomson (1856 - 1940)
Discovered the electron
He was the first scientist to show the atom was made of even smaller things
Used the Cathode ray tube to discover electrons
1897
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16. cont’d………
Adding an electric field cause the beam to move toward the positive plate.
Thomson concluded the beam was made of negative moving pieces.
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+
-
Voltage source
17. Thomson’s “Plum Pudding” Atom Model
Plum and pudding atom modeling
..DownloadsCathode Rays Lead to Thomson's Model of the Atom.mp4
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18. Ernest Rutherford (1871 - 1937)
Discovered the nucleus of a gold atom
with his “gold foil” experiment
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19. cont’d………
Using J.J Thomson’s Plum Pudding atomic model, Rutherford
predicted the alpha particles would pass straight though the gold foil.
That’s not what happened.
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20. cont’d………
Gold Foil Experiment Results
Most alpha particles go straight through the gold foil A few alpha
particles are sharply deflected
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21. Rutherford’s Conclusion
The atom is mostly empty space.
There is a small, dense center with a positive charge.
Rutherford discovered the nucleus in atoms
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23. Rutherford’s Contribution to the Atomic Theory
The atom is mostly empty space.
The nucleus is a small, dense core with a positive charge.
..DownloadsRuther's Alpha Scattering Experiment2.mp4
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24. Bohr Model (1871 - 1937)
In 1913, the Danish scientist Niels Bohr proposed an improvement.
In his model, he placed each electron in a specific energy level.
According to Bohr’s atomic model, electrons move in definite orbits
around the nucleus, much like planets circle the sun.
These orbits, or energy levels, are located at certain distances from the
nucleus.
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25. Cont’d…….
Additionally, the electrons can jump from a path in one level to a path in
another level (depending on their energy).
He proposed the following
Protons and neutrons are in the nucleus
Electrons can only be certain distances from the nucleus
The electrons orbit the nucleus at fixed energy levels
The electrons must absorb or emit a fixed amount of energy to travel
between these energy levels
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26. Atomic bonding
Chemical bonds :-forces that hold together atoms when they combine
produce by interaction of electrons in outer levels of two or more atoms
can form by sharing or transferring electrons
All atoms will try to achieve a stable octet
Two Major Types of Bonding
Ionic Bonding
Form when electrons are transferred from one atom to another
Forms ionic compounds ,
Transfer of e- 11/13/2022 26
27. Ionic Bonding
Two neutral atoms close to each can undergo an ionization process in
order to obtain a full valence shell
Due to ionization, electrons are transferred from one atom to the
other
The atom giving up the electron becomes positively charged (cation)
The atom taking up the electron becomes negatively charged (anion)
The ions are bonded due to coulombic forces of attraction
Generally, metallic atoms donate electrons to non-metallic atoms
Examples: NaCl, KCl, MgBr2 etc.
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29. Covalent Bonding
The outer electron levels of atoms, which are close to each other, can
interact
The interaction leads to a sharing of electrons between the atoms
One pair of electrons shared => single covalent bond
Two pairs of electrons shared => double covalent bond and so on
The shared electrons are said to be delocalized i.e. they do not belong
to any particular atom
Generally, between non-metallic atoms
Examples: H2, CO2, C6H12O6 and other molecules
polar molecule :- have covalent bonds between but atoms do not share
electrons equally
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30. Cont’d….
Single hydrogen atom (left) and two hydrogen atoms forming a covalent
bond with a shared electron pair (right)
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31. Metallic bonds
Atoms come together, electrons from outer shell of atoms share space
with neighboring atoms.
The electrons can move freely within the atom orbitals.
Sharing of ‘free’ electrons among a lattice of positively charged ions
(An array of positive ions in a sea of electrons)
Electrostatic attractive forces between delocalized electrons and
positively charged metal ions.
Between metallic atoms
Examples: Ni, Fe and other metals
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32. Cont’d….
The outer electrons are so weakly bound to metal atoms that they are free
to roam across the entire metal.
This results in a lattice of positively ions in a sea of communal electrons
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33. Energy Bands
Electrons try to occupy the
lowest energy band possible
Not every energy level is a
legal state for an electron to
occupy
These legal states tend to
arrange themselves in bands
Allowed
Energy
States
Disallowed
Energy
States
Increasing
Electron
Energy
Energy Bands
}
}
35. Band Diagrams
Band Diagram Representation
Energy plotted as a function of position
EC Conduction band
Lowest energy state for a free electron
EV Valence band
Highest energy state for filled outer shells
EG Band gap
Difference in energy levels between EC and EV
No electrons (e-) in the bandgap (only above EC or below EV)
EG = 1.12eV in Silicon
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EG
EC
EV
Increasing electron energy
Increasing voltage
36. Energy Bands In Solids
Explains and distinguish between conductors, insulators and semi
conductors
Conduction Band – small energy can remove an electron from an atom
Valence Band – Below the conduction band
Filled Band- Near the nucleus
Insulators- Conduction band is empty but valence is almost
completely filled+ wide energy gap between the two bands (Poor
conductivity)
Conductors- Overlapping of both conduction and valence bands
Conduction es move almost twice as fast as holes
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37. Example 1
Aluminum (Al) (no periodic table)
Protons = 13
Electrons =
Neutrons = 14
Atomic Number =
Atomic Mass =
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38. Quantization of Energy
Energy is quantized in some systems, meaning that the system can
have only certain energies and not a continuum of energies, unlike the
classical case
The quantum view of the atom
Observation: An atom will only absorb or release light at discrete
frequencies
Explanation:
Absorption or emission of light is caused by electron energy
transitions within the atom
The energy carried by light is connected with its frequency.
Electrons are only allowed to move between discrete energy levels in
the atom
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40. Light is also quantized
Light seems to carry energy in discrete packets
We call these packets photons
In this sense, light behaves like a particle
But light also has many wave-like properties
Particle-wave duality: it is both at the same time!
The photoelectric effect
Metal plate illuminated by a light beam
If UV light is used, electrons are emitted
If visible light is used, no electrons are emitted no matter how bright
the light
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41. Cont’d…..
Explanation:
A minimum amount of energy is needed to remove an electron from
the metal
The energy of UV light must be greater than the energy of visible light
Energy and frequency are related by
E = hn
where h is called Plank’s constant
h = 6.625 x 10–34 J s
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