This document discusses quantum numbers and atomic orbitals. It defines the key quantum numbers - principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (ml), and spin quantum number (ms) - and explains what each describes for an electron and orbital. It also covers topics like orbital shapes and sizes, electron configurations, degenerate orbitals, Hund's rule, Pauli exclusion principle, paramagnetism vs diamagnetism, and isoelectronic species. Several examples are provided to illustrate these concepts.
The document discusses the electronic configuration of atoms. It defines electronic configuration as the distribution of electrons in the energy levels, sublevels and orbitals of an atom. It reviews various principles that determine how electrons are arranged, including the Aufbau principle which states that electrons fill atomic orbitals from the lowest energy level upward, and the Pauli exclusion principle which specifies that no more than two electrons can occupy an orbital and that their spins must be opposite. The document provides examples of writing electronic configurations for different elements.
This document discusses quantum numbers and their role in describing the size, shape, and orientation of atomic orbitals. It explains that there are four quantum numbers - principal, angular, magnetic, and spin. The principal quantum number determines the electron shell or energy level, while the angular and magnetic quantum numbers further specify the subshell and orbital within that subshell. The spin quantum number refers to the spin of the electron. Factors that influence ionization energy such as atomic radius, nuclear charge, and electron shielding are also summarized.
12th Physics - Atoms Molecules and Nuclei for JEE Main 2014Ednexa
This document contains information about Thomson's atomic model, Rutherford's atomic model, and Bohr's atomic model. It discusses experiments that led to the development of these atomic models, such as Geiger and Marsden's gold foil experiment. The key points are:
1) Thomson proposed the earliest atomic model which had electrons distributed randomly in the atom.
2) Rutherford's gold foil experiment led him to propose the planetary model of the atom with a small, dense nucleus at the center.
3) Bohr improved upon Rutherford's model by incorporating Planck's quantum theory and proposing electron orbits and allowed energy levels. His model successfully explained atomic spectra.
This document discusses atomic structure and properties. It begins by defining the three main subatomic particles - protons, neutrons, and electrons - and their relative masses and charges. It then explains atomic mass units and discusses quantum numbers like principal, azimuthal, magnetic, and spin quantum numbers. The rest of the document covers electron configurations, orbital diagrams, atomic orbitals and subshells, ionization energy, electronegativity, and how these properties relate to an element's position on the periodic table.
This document provides information about electron configuration. It begins by defining electron configuration as the arrangement of electrons in an atom's orbitals, which is described using quantum numbers. It then discusses the three main rules for writing electron configurations: 1) Aufbau principle, which states that electrons fill the lowest available energy levels first, 2) Pauli exclusion principle, which limits each orbital to two electrons of opposite spin, and 3) Hund's rule, which states that degenerate orbitals will fill with one electron each before pairing. The document provides examples of writing full and condensed electron configurations and drawing orbital diagrams for various elements. It includes an activity for students to practice these skills.
This document provides an overview of atomic structure and quantum mechanics. It discusses early atomic models proposed by Rutherford and Bohr and limitations they faced. It then introduces the quantum mechanical model, which describes electrons as existing in distinct energy levels and orbitals. The document explains how electron configurations are written based on Aufbau principle, Hund's rule and Pauli exclusion principle. It also discusses atomic spectra and how light emitted during electron energy level transitions can be used to identify elements.
Electrons in atoms are arranged in energy levels (n), sublevels (l), and orbitals (ml). Quantum mechanics treats electrons as waves that can only gain or lose discrete amounts of energy called quanta when changing energy levels. Each energy level corresponds to a row on the periodic table and can contain one or more sublevels representing blocks. Sublevels include s, p, d and f orbitals which electrons fill according to specific rules. The electronic configuration notation specifies the distribution of electrons among the atomic orbitals.
This document provides information about an electronic devices course, including its objectives, outcomes, and content. The objectives are to study semiconductor physics, diode characteristics, bipolar junction transistors, field effect transistors, and integrated circuit fabrication. The outcomes include interpreting diode characteristics, designing rectifier circuits, analyzing transistor configurations, and distinguishing different transistor types. The content will cover semiconductor materials and doping, energy bands, carrier transport, generation and recombination, and continuity equations. It will also examine p-n junction diodes, bipolar junction transistors, and field effect transistors.
The document discusses the electronic configuration of atoms. It defines electronic configuration as the distribution of electrons in the energy levels, sublevels and orbitals of an atom. It reviews various principles that determine how electrons are arranged, including the Aufbau principle which states that electrons fill atomic orbitals from the lowest energy level upward, and the Pauli exclusion principle which specifies that no more than two electrons can occupy an orbital and that their spins must be opposite. The document provides examples of writing electronic configurations for different elements.
This document discusses quantum numbers and their role in describing the size, shape, and orientation of atomic orbitals. It explains that there are four quantum numbers - principal, angular, magnetic, and spin. The principal quantum number determines the electron shell or energy level, while the angular and magnetic quantum numbers further specify the subshell and orbital within that subshell. The spin quantum number refers to the spin of the electron. Factors that influence ionization energy such as atomic radius, nuclear charge, and electron shielding are also summarized.
12th Physics - Atoms Molecules and Nuclei for JEE Main 2014Ednexa
This document contains information about Thomson's atomic model, Rutherford's atomic model, and Bohr's atomic model. It discusses experiments that led to the development of these atomic models, such as Geiger and Marsden's gold foil experiment. The key points are:
1) Thomson proposed the earliest atomic model which had electrons distributed randomly in the atom.
2) Rutherford's gold foil experiment led him to propose the planetary model of the atom with a small, dense nucleus at the center.
3) Bohr improved upon Rutherford's model by incorporating Planck's quantum theory and proposing electron orbits and allowed energy levels. His model successfully explained atomic spectra.
This document discusses atomic structure and properties. It begins by defining the three main subatomic particles - protons, neutrons, and electrons - and their relative masses and charges. It then explains atomic mass units and discusses quantum numbers like principal, azimuthal, magnetic, and spin quantum numbers. The rest of the document covers electron configurations, orbital diagrams, atomic orbitals and subshells, ionization energy, electronegativity, and how these properties relate to an element's position on the periodic table.
This document provides information about electron configuration. It begins by defining electron configuration as the arrangement of electrons in an atom's orbitals, which is described using quantum numbers. It then discusses the three main rules for writing electron configurations: 1) Aufbau principle, which states that electrons fill the lowest available energy levels first, 2) Pauli exclusion principle, which limits each orbital to two electrons of opposite spin, and 3) Hund's rule, which states that degenerate orbitals will fill with one electron each before pairing. The document provides examples of writing full and condensed electron configurations and drawing orbital diagrams for various elements. It includes an activity for students to practice these skills.
This document provides an overview of atomic structure and quantum mechanics. It discusses early atomic models proposed by Rutherford and Bohr and limitations they faced. It then introduces the quantum mechanical model, which describes electrons as existing in distinct energy levels and orbitals. The document explains how electron configurations are written based on Aufbau principle, Hund's rule and Pauli exclusion principle. It also discusses atomic spectra and how light emitted during electron energy level transitions can be used to identify elements.
Electrons in atoms are arranged in energy levels (n), sublevels (l), and orbitals (ml). Quantum mechanics treats electrons as waves that can only gain or lose discrete amounts of energy called quanta when changing energy levels. Each energy level corresponds to a row on the periodic table and can contain one or more sublevels representing blocks. Sublevels include s, p, d and f orbitals which electrons fill according to specific rules. The electronic configuration notation specifies the distribution of electrons among the atomic orbitals.
This document provides information about an electronic devices course, including its objectives, outcomes, and content. The objectives are to study semiconductor physics, diode characteristics, bipolar junction transistors, field effect transistors, and integrated circuit fabrication. The outcomes include interpreting diode characteristics, designing rectifier circuits, analyzing transistor configurations, and distinguishing different transistor types. The content will cover semiconductor materials and doping, energy bands, carrier transport, generation and recombination, and continuity equations. It will also examine p-n junction diodes, bipolar junction transistors, and field effect transistors.
Electron orbitals are regions where electrons are most likely to be found around the nucleus. Each energy sublevel has one or more orbitals that can contain a maximum of two electrons. The Pauli exclusion principle states that each orbital may contain no more than two electrons with opposite spin. Hund's rule states that single electrons will occupy all empty orbitals within a sublevel before electron pairs form in orbitals.
This document summarizes key concepts from a chapter on the atomic structure and quantum mechanical model of the atom. It describes early atomic models proposed by Rutherford, Bohr, and Schrodinger, and how they led to the current quantum mechanical model. It discusses how electrons occupy specific energy levels and orbitals, and how transitions between these levels result in the emission of photons of light at characteristic frequencies, producing atomic emission spectra.
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, rather than defined circular orbits. Electrons have wave-like properties.
- The shapes of s, p, d and f orbitals and how electrons fill these orbitals according to various principles like Aufbau and Hund's rule.
- Exceptions to the Aufbau principle seen in some elements.
- How to represent electron configurations using both energy level diagrams and shorthand notation.
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, with specific shapes defined by Schrodinger's wave equation.
- Rules for building up electron configurations, including Hund's rule and the Aufbau principle for filling orbitals in order of increasing energy.
- Exceptions to the Aufbau principle seen in some transition metals where half or fully filled subshells are more stable.
- How electron configurations are written using shorthand notation based on noble gas cores.
This document provides an outline and overview of solid state physics concepts including ionic and covalent bonding, types of solids, band theory, and free electron models. Band theory describes how the energy levels of isolated atoms combine and split into allowed energy bands as atoms are brought together in a solid. Key concepts covered include the formation of valence and conduction bands, density of states, and Fermi energy. Free electron models are discussed as approximations to describe conduction in metals, along with limitations like Bragg reflection. The nearly-free electron model incorporates effects of the periodic lattice potential through concepts like Bloch waves and effective mass.
This document provides an outline and overview of solid state physics concepts including ionic and covalent bonding, types of solids, band theory, and free electron models. Band theory describes how the energy levels of isolated atoms combine and split into allowed energy bands as atoms are brought together in a solid. Key concepts covered include the formation of valence and conduction bands, density of states, and Fermi energy. Free electron models are discussed as approximations to describe conduction in metals, but limitations are noted. The nearly-free electron model incorporates effects of the periodic lattice potential through concepts such as Bloch waves and effective mass.
The document discusses the electronic structure of atoms based on various atomic models and theories. It describes Bohr's atomic model and theory, which explained the stability of atoms and formation of line spectra in hydrogen atoms. Bohr's model introduced quantized, discrete energy levels for electrons in atoms. The energy of an electron is determined by its principal quantum number. Electrons can absorb or emit photons of specific frequencies when transitioning between energy levels.
The document discusses several topics related to the electronic structures of atoms and electromagnetic radiation:
1. It defines wavelength and frequency of electromagnetic radiation and describes the relationship between them.
2. It discusses Max Planck's realization that energy is quantized and light has particle characteristics based on his study of blackbody radiation.
3. It explains Bohr's model of the hydrogen atom which incorporated Planck's quantum theory and correctly explained hydrogen's emission spectrum using discrete energy levels. However, the model failed for other elements.
The document discusses different types of radioactive decay and radiation. It describes alpha, beta, and gamma radiation, and how they interact with and penetrate matter differently due to their mass, charge, and energy. Alpha particles interact strongly, penetrate only a short distance, and produce many ion pairs. Beta particles penetrate farther than alphas as they are lighter and slower. Gamma rays interact weakly and penetrate the deepest as they are uncharged photons. The document also defines half-life as the time for half the nuclei in a sample or half the sample's activity to decay.
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
This document discusses the concepts of electric fields and electric field intensity. It defines electric field as a region of space around charged particles that exert electrostatic forces on other charges. Electric field intensity is defined as the electrostatic force per unit positive test charge. The electric field due to a point charge is discussed, along with the superposition principle and electric field lines. Electric dipoles are introduced as pairs of equal and opposite charges, with discussions of dipole moment, and the electric field intensity and torque experienced by dipoles.
Chapter 8 electron configuration and periodicity (1)ElizabethAyala45
The document discusses electron configurations and periodic trends in atomic properties. It describes how electrons fill atomic orbitals according to the building-up principle and Hund's rule. Trends in atomic radius, ionization energy, and electron affinity across the periodic table are also explained, with atomic radius generally decreasing and ionization energy and electron affinity (becoming more negative) generally increasing within a period. Exceptions to trends are seen for some p-block elements.
This document provides an overview of the history of atomic structure models. It begins with early Greek philosophers' concept of atoms. In the 19th century, Dalton proposed that elements are made of unique atom types that can combine. Experiments by Thomson, Rutherford and Bohr led to discoveries about the electron and nuclear structure of atoms. Bohr's 1913 model improved on Rutherford's by proposing discrete electron orbits. Later, the developments of quantum mechanics by Heisenberg, Schrodinger, de Broglie and others explained atomic structure and spectra through wave functions and quantum numbers. This allowed visualization of electron orbitals in atoms.
1. Electrons in atoms are arranged in shells, subshells, and orbitals according to their quantum numbers. Each orbital can contain a maximum of two electrons with opposing spins.
2. Atoms experience an effective nuclear charge that increases across a period, leading to higher ionization energies and smaller atomic and ionic sizes as more protons are exposed.
3. Trends in properties like ionization energy, atomic size, and electron affinity are explained by the changing effective nuclear charge experienced by valence electrons.
F.Sc. Part 1 Chemistry.Ch.05.Test (Malik Xufyan)Malik Xufyan
The document contains information about Malik's Chemistry test series books for classes 9th, 10th, F.Sc part 1 and part 2. It offers both chapter-wise and board paper-wise test series. It provides the contact details of JIAS Academy and Malik Xufyan. It also lists some other publications of Jhang Institute for Advanced Studies on chemistry.
This document provides an overview of key concepts in semiconductor physics. It begins by introducing the crystal structure of silicon and how dopants can create an excess or deficiency of electrons (N-type or P-type silicon). It then discusses the energy band model and defines important terms like the band gap, Fermi energy level, density of states, and thermal equilibrium. The document derives expressions for the concentrations of electrons and holes as a function of doping, temperature, and the Fermi level position. It also examines intrinsic carrier concentration and how doping affects charge neutrality. Overall, the document establishes fundamental principles for understanding how electrons and holes behave in semiconductors.
The document discusses three types of radioactive decay: alpha, beta, and gamma decay. Alpha decay occurs when a nucleus ejects an alpha particle, consisting of two protons and two neutrons. Beta decay can occur in two ways - beta minus decay where a neutron is converted to a proton and an electron is emitted, and beta plus decay where a proton is converted to a neutron and a positron is emitted. Gamma decay occurs when a nucleus in an excited state drops to a lower energy state by emitting a high energy photon.
Ideas about the structure of the atom have changed over the years. The Bohr theory thought of it as a small nucleus of protons and neutrons surrounded by circulating electrons.
Each shell or energy level could hold a maximum number of electrons.
The energy of levels became greater as they got further from the nucleus and electrons filled energy levels in order.
1) The document discusses the quantum mechanical model of the atom, including atomic orbitals and electron configurations.
2) It describes how electrons can occupy different atomic orbitals based on their energy levels and how the electron configuration notation is used to show the filling of these orbitals.
3) It also mentions exceptions to the expected electron configuration filling order that result in more stable half-filled or filled orbitals.
1) The document discusses the electronic configuration of atoms, including the development of wave mechanics and quantum theory to explain the structure of atoms. It introduces concepts like the de Broglie wavelength, quantum numbers, atomic orbitals and shapes, Pauli's exclusion principle, and Hund's rule for electron configuration.
2) Key scientists discussed include de Broglie, Heisenberg, Schrodinger, Pauli, and their contributions to developing models of the atom and allowing prediction of electron configurations.
3) The document provides examples of writing out electron configurations for elements and explaining the rules for filling atomic orbitals in the Aufbau principle.
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
-------------------------------------------------------------------------------
Find out more about ISO training and certification services
Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
-------------------------------------------------------------------------------
For more information about PECB:
Website: https://pecb.com/
LinkedIn: https://www.linkedin.com/company/pecb/
Facebook: https://www.facebook.com/PECBInternational/
Slideshare: http://www.slideshare.net/PECBCERTIFICATION
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.
Electron orbitals are regions where electrons are most likely to be found around the nucleus. Each energy sublevel has one or more orbitals that can contain a maximum of two electrons. The Pauli exclusion principle states that each orbital may contain no more than two electrons with opposite spin. Hund's rule states that single electrons will occupy all empty orbitals within a sublevel before electron pairs form in orbitals.
This document summarizes key concepts from a chapter on the atomic structure and quantum mechanical model of the atom. It describes early atomic models proposed by Rutherford, Bohr, and Schrodinger, and how they led to the current quantum mechanical model. It discusses how electrons occupy specific energy levels and orbitals, and how transitions between these levels result in the emission of photons of light at characteristic frequencies, producing atomic emission spectra.
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, rather than defined circular orbits. Electrons have wave-like properties.
- The shapes of s, p, d and f orbitals and how electrons fill these orbitals according to various principles like Aufbau and Hund's rule.
- Exceptions to the Aufbau principle seen in some elements.
- How to represent electron configurations using both energy level diagrams and shorthand notation.
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, with specific shapes defined by Schrodinger's wave equation.
- Rules for building up electron configurations, including Hund's rule and the Aufbau principle for filling orbitals in order of increasing energy.
- Exceptions to the Aufbau principle seen in some transition metals where half or fully filled subshells are more stable.
- How electron configurations are written using shorthand notation based on noble gas cores.
This document provides an outline and overview of solid state physics concepts including ionic and covalent bonding, types of solids, band theory, and free electron models. Band theory describes how the energy levels of isolated atoms combine and split into allowed energy bands as atoms are brought together in a solid. Key concepts covered include the formation of valence and conduction bands, density of states, and Fermi energy. Free electron models are discussed as approximations to describe conduction in metals, along with limitations like Bragg reflection. The nearly-free electron model incorporates effects of the periodic lattice potential through concepts like Bloch waves and effective mass.
This document provides an outline and overview of solid state physics concepts including ionic and covalent bonding, types of solids, band theory, and free electron models. Band theory describes how the energy levels of isolated atoms combine and split into allowed energy bands as atoms are brought together in a solid. Key concepts covered include the formation of valence and conduction bands, density of states, and Fermi energy. Free electron models are discussed as approximations to describe conduction in metals, but limitations are noted. The nearly-free electron model incorporates effects of the periodic lattice potential through concepts such as Bloch waves and effective mass.
The document discusses the electronic structure of atoms based on various atomic models and theories. It describes Bohr's atomic model and theory, which explained the stability of atoms and formation of line spectra in hydrogen atoms. Bohr's model introduced quantized, discrete energy levels for electrons in atoms. The energy of an electron is determined by its principal quantum number. Electrons can absorb or emit photons of specific frequencies when transitioning between energy levels.
The document discusses several topics related to the electronic structures of atoms and electromagnetic radiation:
1. It defines wavelength and frequency of electromagnetic radiation and describes the relationship between them.
2. It discusses Max Planck's realization that energy is quantized and light has particle characteristics based on his study of blackbody radiation.
3. It explains Bohr's model of the hydrogen atom which incorporated Planck's quantum theory and correctly explained hydrogen's emission spectrum using discrete energy levels. However, the model failed for other elements.
The document discusses different types of radioactive decay and radiation. It describes alpha, beta, and gamma radiation, and how they interact with and penetrate matter differently due to their mass, charge, and energy. Alpha particles interact strongly, penetrate only a short distance, and produce many ion pairs. Beta particles penetrate farther than alphas as they are lighter and slower. Gamma rays interact weakly and penetrate the deepest as they are uncharged photons. The document also defines half-life as the time for half the nuclei in a sample or half the sample's activity to decay.
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
This document discusses the concepts of electric fields and electric field intensity. It defines electric field as a region of space around charged particles that exert electrostatic forces on other charges. Electric field intensity is defined as the electrostatic force per unit positive test charge. The electric field due to a point charge is discussed, along with the superposition principle and electric field lines. Electric dipoles are introduced as pairs of equal and opposite charges, with discussions of dipole moment, and the electric field intensity and torque experienced by dipoles.
Chapter 8 electron configuration and periodicity (1)ElizabethAyala45
The document discusses electron configurations and periodic trends in atomic properties. It describes how electrons fill atomic orbitals according to the building-up principle and Hund's rule. Trends in atomic radius, ionization energy, and electron affinity across the periodic table are also explained, with atomic radius generally decreasing and ionization energy and electron affinity (becoming more negative) generally increasing within a period. Exceptions to trends are seen for some p-block elements.
This document provides an overview of the history of atomic structure models. It begins with early Greek philosophers' concept of atoms. In the 19th century, Dalton proposed that elements are made of unique atom types that can combine. Experiments by Thomson, Rutherford and Bohr led to discoveries about the electron and nuclear structure of atoms. Bohr's 1913 model improved on Rutherford's by proposing discrete electron orbits. Later, the developments of quantum mechanics by Heisenberg, Schrodinger, de Broglie and others explained atomic structure and spectra through wave functions and quantum numbers. This allowed visualization of electron orbitals in atoms.
1. Electrons in atoms are arranged in shells, subshells, and orbitals according to their quantum numbers. Each orbital can contain a maximum of two electrons with opposing spins.
2. Atoms experience an effective nuclear charge that increases across a period, leading to higher ionization energies and smaller atomic and ionic sizes as more protons are exposed.
3. Trends in properties like ionization energy, atomic size, and electron affinity are explained by the changing effective nuclear charge experienced by valence electrons.
F.Sc. Part 1 Chemistry.Ch.05.Test (Malik Xufyan)Malik Xufyan
The document contains information about Malik's Chemistry test series books for classes 9th, 10th, F.Sc part 1 and part 2. It offers both chapter-wise and board paper-wise test series. It provides the contact details of JIAS Academy and Malik Xufyan. It also lists some other publications of Jhang Institute for Advanced Studies on chemistry.
This document provides an overview of key concepts in semiconductor physics. It begins by introducing the crystal structure of silicon and how dopants can create an excess or deficiency of electrons (N-type or P-type silicon). It then discusses the energy band model and defines important terms like the band gap, Fermi energy level, density of states, and thermal equilibrium. The document derives expressions for the concentrations of electrons and holes as a function of doping, temperature, and the Fermi level position. It also examines intrinsic carrier concentration and how doping affects charge neutrality. Overall, the document establishes fundamental principles for understanding how electrons and holes behave in semiconductors.
The document discusses three types of radioactive decay: alpha, beta, and gamma decay. Alpha decay occurs when a nucleus ejects an alpha particle, consisting of two protons and two neutrons. Beta decay can occur in two ways - beta minus decay where a neutron is converted to a proton and an electron is emitted, and beta plus decay where a proton is converted to a neutron and a positron is emitted. Gamma decay occurs when a nucleus in an excited state drops to a lower energy state by emitting a high energy photon.
Ideas about the structure of the atom have changed over the years. The Bohr theory thought of it as a small nucleus of protons and neutrons surrounded by circulating electrons.
Each shell or energy level could hold a maximum number of electrons.
The energy of levels became greater as they got further from the nucleus and electrons filled energy levels in order.
1) The document discusses the quantum mechanical model of the atom, including atomic orbitals and electron configurations.
2) It describes how electrons can occupy different atomic orbitals based on their energy levels and how the electron configuration notation is used to show the filling of these orbitals.
3) It also mentions exceptions to the expected electron configuration filling order that result in more stable half-filled or filled orbitals.
1) The document discusses the electronic configuration of atoms, including the development of wave mechanics and quantum theory to explain the structure of atoms. It introduces concepts like the de Broglie wavelength, quantum numbers, atomic orbitals and shapes, Pauli's exclusion principle, and Hund's rule for electron configuration.
2) Key scientists discussed include de Broglie, Heisenberg, Schrodinger, Pauli, and their contributions to developing models of the atom and allowing prediction of electron configurations.
3) The document provides examples of writing out electron configurations for elements and explaining the rules for filling atomic orbitals in the Aufbau principle.
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
-------------------------------------------------------------------------------
Find out more about ISO training and certification services
Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
-------------------------------------------------------------------------------
For more information about PECB:
Website: https://pecb.com/
LinkedIn: https://www.linkedin.com/company/pecb/
Facebook: https://www.facebook.com/PECBInternational/
Slideshare: http://www.slideshare.net/PECBCERTIFICATION
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.
How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
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.
How to Build a Module in Odoo 17 Using the Scaffold MethodCeline George
Odoo provides an option for creating a module by using a single line command. By using this command the user can make a whole structure of a module. It is very easy for a beginner to make a module. There is no need to make each file manually. This slide will show how to create a module using the scaffold method.
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
How to Manage Your Lost Opportunities in Odoo 17 CRMCeline George
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
2. FACEBOOK: VIRTUAL CLASS PROF. JULIO ORIA
CONCEPTO :
Los números cuánticos son parámetros matemáticos que determinan un orbital
(su ubicación, forma, energía)
Observación: Definen las características: De un orbital: Ψ (n, l, m ) ; De un electrón: Ψ (n, l, m , m )
3. FACEBOOK: VIRTUAL CLASS PROF. JULIO ORIA
CARACTERISTICAS :
n = 2 El o los electrones se encuentran en el segundo nivel de energía
n = 5 El o los electrones se encuentran en el quinto nivel de energía
1) N.C. PRINCIPAL (n) :
Para el electrón:
El número máximo de electrones que contiene
un nivel “n” se halla por la siguiente relación:
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Para el orbital:
A mayor valor de “n”, mayor es el tamaño del orbital.
Se tienen los orbitales: Ψ (1s) y Ψ (2s)
luego el tamaño del orbital 2s es mayor
que el 1s por tener mayor valor de “n”
Ejemplos:
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2) N.C. SECUNDARIO O AZIMUTAL (l) :
Para el electrón:
n = 5 l =
n = 3 l =
n = 6 l=
Ejemplos: La secuencia especial de letras (s, p y d) tiene origen histórico.
Los físicos que estudiaron los espectros de emisión atómica
intentaban relacionar las líneas espectrales detectadas con los
estados de energía asociados a las transiciones. Observaron
que algunas líneas eran finas (sharp, en inglés), otras eran más
bien difusas, y algunas eran muy intensas y se referían a ellas
como principales. Por esta razón, asignaron las letras iniciales
del adjetivo que calificaba a cada línea con dichos estados de
energía. Sin embargo, después de la letra d, el orbital se
designa siguiendo un orden alfabético, comenzando con la
letra f (para el estado fundamental).
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Para el orbital:
A mayor valor de “n”, mayor es el tamaño del orbital.
Ejemplos:
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2) N.C. SPIN (mS) :
Para el electrón: Tiene dos valores: -1/2 y +1/2
El spin positivo genera un campo eléctrico positivo y
viceversa
La determinación experimental del Spin fue realizada por Stern y Gerlach en 1920; al hacer vaporizar
átomos de plata y colocarlos en un campo magnético no uniforme, observaron que el haz de plata de
desdoblada en 2 haces, los cuales se dirigían hacia los polos
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CONFIGURACIÓN ELECTRÓNICA :
Es la representación simbólica y numérica, que consiste en distribuir a los
electrones en las diferentes regiones de máxima probabilidad que existen en
la nube electrónica, como son: niveles, subniveles y orbitales; en función a
criterios de menor a mayor energía relativa.
PRINCIPIO DE AUFBAU:
Aufbau (verbo alemán que significa construcción progresiva), establece que los
electrones en un átomo se deben distribuir en sus diferentes niveles, subniveles
y orbitales de energía, atendiendo a la energía relativa del orbital (la cual debe ir
de menor a mayor).
E.R : Energía relativa de un orbital
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Características:
▪ Un orbital es más estable cuando la E.R es la
más baja posible.
▪ Si dos orbitales poseen la misma E.R es más
estable, aquel que tiene el menor valor de “n”.
Ordenar los siguientes orbitales de menor a mayor
E.R 4s, 3d, 5p, 4f
Ejemplo :
Ejemplo :
ORBITALES DEGENERADOS:
Son aquellos que tienen igual
E.R y pertenecen al mismo nivel y
subnivel de energía.
• ¿Cuál de los siguientes orbitales posee
mayor energía?
• ¿Qué orbital es el más estable? : 5d, 7s, 4f
ó 6p
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EJERCICIO 01:
Si 2a=x - 1; y además 3x – 2 ≥13; halla
el menor valor entero de "a".
EJERCICIO 02:
Resuelve: 2x-3 + 5 ≤ 17
2 2
e indica el mayor valor entero de "x".
Solución :
Solución :
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¿Cuál es el último nivel energético del 20Ca?
A) K B) L C) M D) N E) O
Ejemplo :
Para el 25Mn. ¿Qué cantidad de electrones existirá
en sus subniveles principales?
A) 12 B) 5 C) 17 D) 11 E) 25
Ejemplo :
La diferencia entre neutrones y protones
de un átomo es 20. Si A -Z = 60, ¿Cuántos
electrones posee en la capa “N”?
A) 8 B) 14 C) 10 D) 16 E) 12
Ejemplo :
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C.E. DE IONES :
• Se efectúa la CE del átomo neutro.
• Los electrones que pierde el átomo son del último nivel de energía, si faltase e- por
perder, se elimina respecto al subnivel de mayor ER
1. Cationes:
Ejemplo :
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• Se efectúa la CE respecto al número total de electrones.
2. Aniones:
Ejemplo :
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PRINCIPIO DE MAXIMA MULTIPLICIDAD (HUND):
Ejemplo :
Ningún orbital de un mismo nivel y subnivel (degenerados) puede contener dos
electrones antes que los demás contengan por lo menos uno, es decir, primero se
debe dejar todos los orbitales a medio llenar y luego empezar el llenado con spines
opuestos.
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PRINCIPIO DE EXCLUSION (PAULI):
Ejemplo :
En un átomo no pueden haber dos electrones con sus cuatro números cuánticos
idénticos. Dicho de otra forma: dos electrones de un mismo átomo pueden
tener a los más tres números cuánticos idénticos, deben diferenciarse al menos
en el spin.
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Ejemplo : Ejemplo :
Al hacer la distribución electrónica del
átomo neutro del 16S , señale que
proposiciones muestran correctamente la
distribución de electrones en los orbitales
degenerados , cuya energía relativa es 4.
I) ↑↓ ↑↓
↑↓ ↑ ↑
II)
III) ↓ ↑↓ ↓
↑↑ ↑ ↑
IV)
A) Solo II
B) I , III y IV
C) Solo III
D) III y IV
E) II y III
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MAGNETISMO Y PARAMAGNETISMO
SUSTANCIA DIAMAGNETICA :
Este principio se fundamenta en el hecho de que 2 electrones que están en el mismo
orbital y poseen el mismo sentido del spin presentan repulsiones muy fuertes entre sí,
debido a sus campos magnéticos iguales.
Es atraída o débilmente repelida por un campo magnético externo (generado por un
imán o electroimán). Debido a que sus orbitales se encuentran todos llenos o
apareados. Ejemplo: 4Be, 12Mg
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SUSTANCIA PARAMAGNETICA :
Es atraída por un campo magnético externo. Debido a que poseen uno o más orbitales
semillenos o desapareados. El efecto se pierde tan pronto como se retira el campo
magnético. Ejemplos: 9F, 13Al , 11Na, 29Cu , ..
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Ejemplo : Ejemplo :
Respecto al paramagnetismo y diamagnetismo,
marque verdadero (V) o falso (F) las siguientes
proposiciones.
I) El elemento E (Z=12) es paramagnético.
II) En paramagnetismo se cumple: 25Mn > 13Al
III) En el elemento diamagnético solo hay
electrones desapareados.
A) VVV
B) VFF
C) VFV
D) FVV
E) FVF
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SUSTANCIAS FERROMAGNÉTICAS :
Son aquellas que sometidas a la acción de un campo magnético externo, sufren una
atracción fuerte y se imantan de forma permanente. El paramagnetismo es ciento de
miles de veces más débil que el ferromagnetismo.
Ejemplo : Fe, Co, Ni, Gd y alguna de sus aleaciones
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C.E. DE ELEMENTOS QUÍMICOS ANÓMALOS
Existen 19 C.E. anómalas, y corresponden a elementos químicos del GRUPO B
Estás anomalías observadas espectroscópicamente,
se dan, debido a que la diferencia de energía entre
los subniveles son pequeñas. En todos los casos, la
transferencia de un electrón de un subnivel a otro
reduce la energía del átomo debido a la
disminución de repulsiones entre un electrón y otro
Ejemplo :
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Ejemplo : Ejemplo :
El paladio (Z=46) usado en aleaciones y
como catalizador es un elemento
diamagnético . Según lo anterior determine si
es verdadero (V) o falso (F) las siguientes
proposiciones.
I) Su configuración electrónica es 𝐾𝑟 4d10
II) Presenta 2 electrones en el quinto nivel.
III) Presenta 23 orbitales con electrones
apareados.
A) VVV
B) VFV
C) VFF
D) FVV
E) FVF
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Ejemplo : Ejemplo :
Del siguiente par de especies químicas que
se da en cada proposición, indique en que
proposiciones los pares son isoelectrónicos.
I) 16S4- y 22Ti2+
II) 25Mn2+ y 26Fe3+
III) 7N3- y 9F-
A) Solo I
B) I y III
C) Solo III
D) II y III
E) I, II y III
38. 38
PROBLEMA 5
Clave A
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Para que un átomo tenga tres niveles definidos, ¿Cuántos electrones como mínimo
debe tener?
A) 11 B) 12 C) 13 D) 14 E) 15