Estructura electronica atomica
•Download as PPT, PDF•
3 likes•803 views
The document summarizes key concepts from Chapter 6 of the textbook, including: 1) Modern atomic theory arose from studies of radiation interacting with matter, and electromagnetic radiation has characteristic wavelengths and frequencies. 2) Planck proposed that atoms can only absorb or emit energy in discrete quanta, proportional to frequency via Planck's constant. 3) Einstein assumed light is composed of discrete energy packets called photons, helping explain the photoelectric effect. 4) Bohr incorporated Planck's quantization idea into his atomic model, where electrons orbit in distinct energy levels corresponding to line spectra wavelengths. 5) Later models including de Broglie's matter waves, Heisenberg's uncertainty principle, and
Report
Share
Report
Share
![Prentice Hall © 2003 Chapter 6 ,[object Object],[object Object],[object Object],[object Object],The Wave Nature of Light](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
Recommended
03b electronic structure of atoms
This document provides information about the electronic structure of atoms, including electron configurations and distribution of electrons in different atomic shells and orbitals. It defines shells and orbitals, and explains that electrons fill up lower energy shells and orbitals first according to the Aufbau principle. Tables provide the maximum number of electrons in each shell and the types of orbitals in each shell. Diagrams illustrate orbital shapes and energy level sequences. Examples of electronic configurations of the first 18 elements are given in both orbital and noble gas notation. An exercise section tests understanding of concepts covered.
Ch. 6 Electronic Structure of Atoms
1) The document discusses the electronic structure of atoms, including the quantum mechanical model of the atom and how it explains experimental observations.
2) Key aspects covered include the wave-particle duality of electrons and light, the development of quantum numbers to describe electron orbitals and energies, and how the organization of electrons in atoms is reflected in the periodic table.
3) The document also notes some anomalies that arise when s and d orbitals are partially filled due to their similar energies.
The quantum mechanical model of the atom
Here are the definitions:
1. Electronic configuration is the distribution of electrons of an atom or ion in atomic orbitals of the electron shells.
2. The aufbau principle states that electrons fill atomic orbitals of an atom in order of increasing energy level. Orbitals within a given energy level are filled first before the next energy level is begun.
3. Hund's rule states that when electrons are added to orbitals of the same energy in an atom or ion, they will occupy different orbitals singly, with their spins parallel, before any orbital is occupied by a second electron.
Quantum Mechanic Model
The four quantum numbers specify the location of electrons in an atom. The principal quantum number (n) determines the electron's energy level and orbital size. Higher n means a larger orbital farther from the nucleus, increasing the atom's energy. The angular momentum quantum number (l) corresponds to an orbital's subshell type (s, p, d, f). The third and fourth quantum numbers further specify an electron's orientation. Electrons fill atomic orbitals according to Aufbau principle, Pauli exclusion principle, and Hund's rule to achieve the lowest energy configuration.
Chapter 3 Arrangement of Electrons in the Atom
1) Niels Bohr proposed that electrons orbit the nucleus in fixed orbits called energy levels rather than in continuous orbits.
2) When electrons jump between energy levels, they absorb or emit photons of light with specific wavelengths corresponding to the energy difference between levels.
3) Each element has unique emission spectra because they have different numbers and arrangements of electrons, leading to different possible energy level transitions.
Electrons in Atoms
The document discusses the development of atomic models from Dalton to Bohr and beyond. It describes Rutherford's discovery of the nucleus and Bohr's model of electrons in fixed orbits around the nucleus. Later, the quantum mechanical model was developed, restricting electrons to specific energy levels rather than exact orbits. This modern model determines the probability of finding electrons in different locations around the nucleus.
AP Chemistry Chapter 6 Outline
The document discusses the electronic structure of atoms. It introduces quantum numbers like the principal quantum number n, angular momentum quantum number l, and magnetic quantum number ml, which describe the allowed orbitals for electrons. Orbitals include s, p, and d orbitals with different shapes. The Pauli exclusion principle states that no two electrons can have the same set of quantum numbers. Electron configurations show how electrons are arranged in orbitals based on increasing energy.
C H6
The document provides an overview of the key concepts in electronic structure of atoms, including:
1) Light and electromagnetic radiation can be described as waves or particles depending on how they are observed. Max Planck introduced the idea that energy is quantized in discrete units called quanta.
2) Niels Bohr combined classical physics and Planck's quantum theory to develop the Bohr model of the atom, in which electrons orbit the nucleus in fixed energy levels. This explained atomic emission spectra.
3) Later, quantum mechanics developed by Schrodinger, Heisenberg and others described electrons as waves rather than particles. This led to new models of electron orbitals and the filling of these orbitals in
Recommended
03b electronic structure of atoms
This document provides information about the electronic structure of atoms, including electron configurations and distribution of electrons in different atomic shells and orbitals. It defines shells and orbitals, and explains that electrons fill up lower energy shells and orbitals first according to the Aufbau principle. Tables provide the maximum number of electrons in each shell and the types of orbitals in each shell. Diagrams illustrate orbital shapes and energy level sequences. Examples of electronic configurations of the first 18 elements are given in both orbital and noble gas notation. An exercise section tests understanding of concepts covered.
Ch. 6 Electronic Structure of Atoms
1) The document discusses the electronic structure of atoms, including the quantum mechanical model of the atom and how it explains experimental observations.
2) Key aspects covered include the wave-particle duality of electrons and light, the development of quantum numbers to describe electron orbitals and energies, and how the organization of electrons in atoms is reflected in the periodic table.
3) The document also notes some anomalies that arise when s and d orbitals are partially filled due to their similar energies.
The quantum mechanical model of the atom
Here are the definitions:
1. Electronic configuration is the distribution of electrons of an atom or ion in atomic orbitals of the electron shells.
2. The aufbau principle states that electrons fill atomic orbitals of an atom in order of increasing energy level. Orbitals within a given energy level are filled first before the next energy level is begun.
3. Hund's rule states that when electrons are added to orbitals of the same energy in an atom or ion, they will occupy different orbitals singly, with their spins parallel, before any orbital is occupied by a second electron.
Quantum Mechanic Model
The four quantum numbers specify the location of electrons in an atom. The principal quantum number (n) determines the electron's energy level and orbital size. Higher n means a larger orbital farther from the nucleus, increasing the atom's energy. The angular momentum quantum number (l) corresponds to an orbital's subshell type (s, p, d, f). The third and fourth quantum numbers further specify an electron's orientation. Electrons fill atomic orbitals according to Aufbau principle, Pauli exclusion principle, and Hund's rule to achieve the lowest energy configuration.
Chapter 3 Arrangement of Electrons in the Atom
1) Niels Bohr proposed that electrons orbit the nucleus in fixed orbits called energy levels rather than in continuous orbits.
2) When electrons jump between energy levels, they absorb or emit photons of light with specific wavelengths corresponding to the energy difference between levels.
3) Each element has unique emission spectra because they have different numbers and arrangements of electrons, leading to different possible energy level transitions.
Electrons in Atoms
The document discusses the development of atomic models from Dalton to Bohr and beyond. It describes Rutherford's discovery of the nucleus and Bohr's model of electrons in fixed orbits around the nucleus. Later, the quantum mechanical model was developed, restricting electrons to specific energy levels rather than exact orbits. This modern model determines the probability of finding electrons in different locations around the nucleus.
AP Chemistry Chapter 6 Outline
The document discusses the electronic structure of atoms. It introduces quantum numbers like the principal quantum number n, angular momentum quantum number l, and magnetic quantum number ml, which describe the allowed orbitals for electrons. Orbitals include s, p, and d orbitals with different shapes. The Pauli exclusion principle states that no two electrons can have the same set of quantum numbers. Electron configurations show how electrons are arranged in orbitals based on increasing energy.
C H6
The document provides an overview of the key concepts in electronic structure of atoms, including:
1) Light and electromagnetic radiation can be described as waves or particles depending on how they are observed. Max Planck introduced the idea that energy is quantized in discrete units called quanta.
2) Niels Bohr combined classical physics and Planck's quantum theory to develop the Bohr model of the atom, in which electrons orbit the nucleus in fixed energy levels. This explained atomic emission spectra.
3) Later, quantum mechanics developed by Schrodinger, Heisenberg and others described electrons as waves rather than particles. This led to new models of electron orbitals and the filling of these orbitals in
Quantum theory and the atom
The highest energy level in Bohr's model of the atom is the one that is farthest from the nucleus. According to Bohr's model, electrons can only exist at certain discrete energy levels or orbits around the nucleus, with the lowest energy level being closest to the nucleus. When an electron gains energy, it moves to a higher energy level in an "excited state". It then releases energy as a photon when it falls back to its lower "ground state". Later, the quantum mechanical model improved on Bohr's model by treating electrons as waves rather than definite orbits, better explaining experimental observations.
ELECTRONS
1. Inside metals, electrons are weakly bound to atoms and move freely through the metal.
2. These free electrons move through a periodic potential created by the positive ions and other electrons.
3. The potential energy of the electrons is periodic inside the metal but rises suddenly at the boundaries, as shown in the figures. Electrons with energy below a binding energy Eb are tightly bound to atoms, while higher energy electrons between Eb and the Fermi energy Ef can move through the metal.
Chem 40Ss Unit 2 Notes
The document outlines the historical development of models of the atom from Democritus' solid indivisible atom model to the current quantum mechanical model. It discusses early models including Dalton's billiard ball model, Thomson's plum pudding model, and Rutherford's solar system model. It then focuses on the Bohr model where electrons orbit in distinct energy levels, and the development of the electron cloud or charge cloud model where electrons exist in probability clouds around the nucleus. The quantum mechanical model incorporates the uncertainty principle and probability functions to describe electron location and energy levels.
Pauli exclusion principle
The document discusses the Pauli Exclusion Principle and its importance in the periodic table. It explains that the principle states that no two electrons in an atom can have the same set of quantum numbers, and electrons must have opposite spins when occupying the same orbital. This principle allows electrons to be arranged in shells and is crucial for determining an element's chemical properties and for constructing the periodic table by blocks.
Bohr’s model for hydrogen atom
This document provides an overview of Niels Bohr's atomic model of the hydrogen atom. It describes Bohr's key postulates, including that electrons orbit the nucleus in fixed circular orbits called energy levels, and can only gain or lose energy by jumping between these discrete levels. The model accounted for the observed line spectrum of hydrogen. However, it had limitations and could not explain more complex atoms or effects like the Zeeman effect. It was replaced by later quantum mechanical models.
Quantum mechanical model_of_the_atom (1)
1) Bohr's model of electrons orbiting the nucleus in circular orbits was ineffective beyond simple atoms like hydrogen and lithium.
2) De Broglie, Heisenberg, and Schrödinger pioneered quantum mechanics, proposing that electrons behave as waves rather than particles in orbits.
3) In Schrödinger's wave mechanical model, electrons are described by wave functions that represent probability distributions of their location and discrete energy levels.
Lesson #1 quantum mechanical model
This lesson will help you know how atoms of each element are arranged in an orbital and where atoms are exactly located that give distinct characteristics to the element.
Orbital shape-orientationt
This document discusses different models of the atom, including Bohr's model, the quantum mechanical model, and atomic orbitals. It describes key aspects of each model, such as electrons occupying specific energy levels in Bohr's model and the probabilistic nature of electron location in the quantum mechanical model. It also explains atomic orbitals in more detail, defining principal and other quantum numbers that describe orbital shape and electron location probability. Diagrams are provided to illustrate orbital shapes like s, p, d, and f orbitals.
Quantum Numbers
The document discusses quantum numbers and their role in describing quantum states of electrons in atoms. It provides details on the principal quantum number n, the azimuthal quantum number l, the magnetic quantum number m, and the spin quantum number s. It also discusses the scientists who contributed to the development of these concepts, including Otto Stern, Walther Gerlach, and their Stern-Gerlach experiment demonstrating spin, as well as Wolfgang Pauli and his formulation of the Pauli exclusion principle.
Quantum mechanical model
Want a better understanding of quantum mechanics and the people behind it? Do you want to know what Einstein's part in quantum mechanics? Get it here.
Electronic structure of the atom
In this presentation you will be able to, describe how atomic orbitals arise from the Schrodinger's equation, relate orbital shapes to electron density distribution and interpret the information obtained from a four set of quantum numbers.
Periodic relationships among elements
At the end of this chapter you should be able to sketch the periodic table showing the groups and periods; identify the metals, metalloids and non-metals in the periodic table. Identify the representative elements, the transition elements, the transition metals, the lanthanides and actinides in the periodic table. Also, give the electron configuration of cations and anions; determine the trends in the physical properties of elements in a group; describe and explain the trends in atomic properties in the periodic table; compare the properties of families and elements; predict the properties of individual elements based on their position in the periodic table; and perform exercises and collaborative work with peers.
Chapter 4 electrons in atoms
This chapter discusses the evolution of atomic models and the arrangement of electrons in atoms. It covers difficult concepts such as electrons occupying specific energy levels and orbitals. Students are advised to do all assigned homework and bring their textbook to class to fully understand these abstract ideas. Key models discussed include the Rutherford model, the planetary model, Bohr's model linking electrons and photon emission, and the modern quantum mechanical model based on probability.
Quantum mechanical model of atom
Quantum mechanical model of atom belongs to XI standard Chemistry which describes the quantum mechanics concept of atom, quantum numbers, shape and energies of atomic orbitals.
Atomic bonding
Interatomic forces present in atomic bonding can predict many physical properties of materials such as melting temperature, elasticity, thermal expansion, and strength. These interatomic forces include attractive and repulsive forces that are functions of interatomic distance, and determine the bonding energy between atoms when they form bonds. Different types of bonding like ionic, covalent, metallic, and secondary bonding are characterized by different bonding energies and influence material properties.
Electronic Structure of Atoms
Hello! I've created this PowerPoint presentation as a requisite in General Chemistry 1 subject during SY 2019–2020.
Electronic Structure of Atoms
- Quantum Mechanical Description of Atom
- Schrödinger’s Model of Hydrogen Atom and Wave Functions
- Main Energy Levels, Sublevels, and Orbitals
- Quantum Numbers
- Electron Configuration
Should you need a .pptx file, kindly email me at rd.chrxlr@gmail.com.
Chapter4electronsinatoms 111110092817-phpapp02
This document provides a summary of key concepts about electrons in atoms, including:
1) It discusses the evolution of atomic models from Rutherford to Bohr, focusing on explaining the arrangement of electrons. The quantum mechanical model describes electron probability clouds rather than fixed orbits.
2) It covers atomic orbitals and how electrons fill different orbitals based on their principal and angular momentum quantum numbers. Higher principal quantum numbers correspond to higher energy levels further from the nucleus.
3) The document emphasizes that electrons fill orbitals based on the Aufbau principle to achieve the lowest possible energy configuration. Understanding electron configurations is essential to describing elements and their properties.
Structure of atom plus one focus area notes
The document discusses the structure of the atom, including:
1) Rutherford's nuclear model of the atom based on alpha particle scattering experiments. This established the atom's small, dense nucleus at the center with electrons in orbits around it.
2) Planck's quantum theory and the photoelectric effect, which demonstrated light behaving as discrete packets of energy called quanta and supported the nuclear model.
3) Bohr's model of the hydrogen atom incorporating Planck's quanta and explaining atomic spectra through electron transitions between discrete energy levels.
4) Later developments including de Broglie's matter waves, Heisenberg's uncertainty principle, and Schrodinger's wave mechanical model describing electrons as
Quantum theory and the atom
This document provides an overview of Bohr's model of the atom and the development of the quantum mechanical model. It discusses key aspects of Bohr's model including discrete energy levels and allowed electron orbits. It then describes limitations of Bohr's model and the proposal of the quantum mechanical model treating electrons as waves. The quantum mechanical model uses wave functions and orbitals to describe electron location probabilities rather than defined orbits. It introduces the concepts of principal and subenergy levels characterized by quantum numbers that specify allowed electron configurations.
Bohr model and electron configuration
Bohr's model proposed that electrons orbit the nucleus in fixed, quantized energy levels. Later models, like the quantum mechanical model, provided a more accurate description of electron behavior. Electrons fill atomic orbitals according to specific rules, building up the electron configuration of elements in a predictable order based on energy levels. Exceptions occur when half or completely filled orbitals result in a lower energy configuration. Practice filling electron configurations to understand these patterns.
Writing a full research paper part 1
This session will give researchers some tips on the first part of the paper including the introduction, literature review, research question & purpose of the study.
Structure Of Atoms Part 2
1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
2) Electrons are arranged in shells around the nucleus numbered 1, 2, 3, etc. The first shell can hold up to 2 electrons and subsequent shells can hold up to 8 electrons.
3) To find an element's electronic configuration, electrons are filled into the lowest available energy shell first.
More Related Content
What's hot
Quantum theory and the atom
The highest energy level in Bohr's model of the atom is the one that is farthest from the nucleus. According to Bohr's model, electrons can only exist at certain discrete energy levels or orbits around the nucleus, with the lowest energy level being closest to the nucleus. When an electron gains energy, it moves to a higher energy level in an "excited state". It then releases energy as a photon when it falls back to its lower "ground state". Later, the quantum mechanical model improved on Bohr's model by treating electrons as waves rather than definite orbits, better explaining experimental observations.
ELECTRONS
1. Inside metals, electrons are weakly bound to atoms and move freely through the metal.
2. These free electrons move through a periodic potential created by the positive ions and other electrons.
3. The potential energy of the electrons is periodic inside the metal but rises suddenly at the boundaries, as shown in the figures. Electrons with energy below a binding energy Eb are tightly bound to atoms, while higher energy electrons between Eb and the Fermi energy Ef can move through the metal.
Chem 40Ss Unit 2 Notes
The document outlines the historical development of models of the atom from Democritus' solid indivisible atom model to the current quantum mechanical model. It discusses early models including Dalton's billiard ball model, Thomson's plum pudding model, and Rutherford's solar system model. It then focuses on the Bohr model where electrons orbit in distinct energy levels, and the development of the electron cloud or charge cloud model where electrons exist in probability clouds around the nucleus. The quantum mechanical model incorporates the uncertainty principle and probability functions to describe electron location and energy levels.
Pauli exclusion principle
The document discusses the Pauli Exclusion Principle and its importance in the periodic table. It explains that the principle states that no two electrons in an atom can have the same set of quantum numbers, and electrons must have opposite spins when occupying the same orbital. This principle allows electrons to be arranged in shells and is crucial for determining an element's chemical properties and for constructing the periodic table by blocks.
Bohr’s model for hydrogen atom
This document provides an overview of Niels Bohr's atomic model of the hydrogen atom. It describes Bohr's key postulates, including that electrons orbit the nucleus in fixed circular orbits called energy levels, and can only gain or lose energy by jumping between these discrete levels. The model accounted for the observed line spectrum of hydrogen. However, it had limitations and could not explain more complex atoms or effects like the Zeeman effect. It was replaced by later quantum mechanical models.
Quantum mechanical model_of_the_atom (1)
1) Bohr's model of electrons orbiting the nucleus in circular orbits was ineffective beyond simple atoms like hydrogen and lithium.
2) De Broglie, Heisenberg, and Schrödinger pioneered quantum mechanics, proposing that electrons behave as waves rather than particles in orbits.
3) In Schrödinger's wave mechanical model, electrons are described by wave functions that represent probability distributions of their location and discrete energy levels.
Lesson #1 quantum mechanical model
This lesson will help you know how atoms of each element are arranged in an orbital and where atoms are exactly located that give distinct characteristics to the element.
Orbital shape-orientationt
This document discusses different models of the atom, including Bohr's model, the quantum mechanical model, and atomic orbitals. It describes key aspects of each model, such as electrons occupying specific energy levels in Bohr's model and the probabilistic nature of electron location in the quantum mechanical model. It also explains atomic orbitals in more detail, defining principal and other quantum numbers that describe orbital shape and electron location probability. Diagrams are provided to illustrate orbital shapes like s, p, d, and f orbitals.
Quantum Numbers
The document discusses quantum numbers and their role in describing quantum states of electrons in atoms. It provides details on the principal quantum number n, the azimuthal quantum number l, the magnetic quantum number m, and the spin quantum number s. It also discusses the scientists who contributed to the development of these concepts, including Otto Stern, Walther Gerlach, and their Stern-Gerlach experiment demonstrating spin, as well as Wolfgang Pauli and his formulation of the Pauli exclusion principle.
Quantum mechanical model
Want a better understanding of quantum mechanics and the people behind it? Do you want to know what Einstein's part in quantum mechanics? Get it here.
Electronic structure of the atom
In this presentation you will be able to, describe how atomic orbitals arise from the Schrodinger's equation, relate orbital shapes to electron density distribution and interpret the information obtained from a four set of quantum numbers.
Periodic relationships among elements
At the end of this chapter you should be able to sketch the periodic table showing the groups and periods; identify the metals, metalloids and non-metals in the periodic table. Identify the representative elements, the transition elements, the transition metals, the lanthanides and actinides in the periodic table. Also, give the electron configuration of cations and anions; determine the trends in the physical properties of elements in a group; describe and explain the trends in atomic properties in the periodic table; compare the properties of families and elements; predict the properties of individual elements based on their position in the periodic table; and perform exercises and collaborative work with peers.
Chapter 4 electrons in atoms
This chapter discusses the evolution of atomic models and the arrangement of electrons in atoms. It covers difficult concepts such as electrons occupying specific energy levels and orbitals. Students are advised to do all assigned homework and bring their textbook to class to fully understand these abstract ideas. Key models discussed include the Rutherford model, the planetary model, Bohr's model linking electrons and photon emission, and the modern quantum mechanical model based on probability.
Quantum mechanical model of atom
Quantum mechanical model of atom belongs to XI standard Chemistry which describes the quantum mechanics concept of atom, quantum numbers, shape and energies of atomic orbitals.
Atomic bonding
Interatomic forces present in atomic bonding can predict many physical properties of materials such as melting temperature, elasticity, thermal expansion, and strength. These interatomic forces include attractive and repulsive forces that are functions of interatomic distance, and determine the bonding energy between atoms when they form bonds. Different types of bonding like ionic, covalent, metallic, and secondary bonding are characterized by different bonding energies and influence material properties.
Electronic Structure of Atoms
Hello! I've created this PowerPoint presentation as a requisite in General Chemistry 1 subject during SY 2019–2020.
Electronic Structure of Atoms
- Quantum Mechanical Description of Atom
- Schrödinger’s Model of Hydrogen Atom and Wave Functions
- Main Energy Levels, Sublevels, and Orbitals
- Quantum Numbers
- Electron Configuration
Should you need a .pptx file, kindly email me at rd.chrxlr@gmail.com.
Chapter4electronsinatoms 111110092817-phpapp02
This document provides a summary of key concepts about electrons in atoms, including:
1) It discusses the evolution of atomic models from Rutherford to Bohr, focusing on explaining the arrangement of electrons. The quantum mechanical model describes electron probability clouds rather than fixed orbits.
2) It covers atomic orbitals and how electrons fill different orbitals based on their principal and angular momentum quantum numbers. Higher principal quantum numbers correspond to higher energy levels further from the nucleus.
3) The document emphasizes that electrons fill orbitals based on the Aufbau principle to achieve the lowest possible energy configuration. Understanding electron configurations is essential to describing elements and their properties.
Structure of atom plus one focus area notes
The document discusses the structure of the atom, including:
1) Rutherford's nuclear model of the atom based on alpha particle scattering experiments. This established the atom's small, dense nucleus at the center with electrons in orbits around it.
2) Planck's quantum theory and the photoelectric effect, which demonstrated light behaving as discrete packets of energy called quanta and supported the nuclear model.
3) Bohr's model of the hydrogen atom incorporating Planck's quanta and explaining atomic spectra through electron transitions between discrete energy levels.
4) Later developments including de Broglie's matter waves, Heisenberg's uncertainty principle, and Schrodinger's wave mechanical model describing electrons as
Quantum theory and the atom
This document provides an overview of Bohr's model of the atom and the development of the quantum mechanical model. It discusses key aspects of Bohr's model including discrete energy levels and allowed electron orbits. It then describes limitations of Bohr's model and the proposal of the quantum mechanical model treating electrons as waves. The quantum mechanical model uses wave functions and orbitals to describe electron location probabilities rather than defined orbits. It introduces the concepts of principal and subenergy levels characterized by quantum numbers that specify allowed electron configurations.
Bohr model and electron configuration
Bohr's model proposed that electrons orbit the nucleus in fixed, quantized energy levels. Later models, like the quantum mechanical model, provided a more accurate description of electron behavior. Electrons fill atomic orbitals according to specific rules, building up the electron configuration of elements in a predictable order based on energy levels. Exceptions occur when half or completely filled orbitals result in a lower energy configuration. Practice filling electron configurations to understand these patterns.
What's hot (20)
Viewers also liked
Writing a full research paper part 1
This session will give researchers some tips on the first part of the paper including the introduction, literature review, research question & purpose of the study.
Structure Of Atoms Part 2
1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
2) Electrons are arranged in shells around the nucleus numbered 1, 2, 3, etc. The first shell can hold up to 2 electrons and subsequent shells can hold up to 8 electrons.
3) To find an element's electronic configuration, electrons are filled into the lowest available energy shell first.
Organic Compounds
The document discusses the four main types of organic compounds: lipids, proteins, carbohydrates, and nucleic acids. It defines each type, their compositions, functions, and examples. Lipids are made up of carbon, hydrogen, and oxygen and include fats, oils, and waxes. They store and release energy. Proteins contain carbon, hydrogen, oxygen, and nitrogen, and perform essential functions in the body like structure, movement, and immunity. Carbohydrates provide energy and are made of carbon, hydrogen, and oxygen in monosaccharides, disaccharides and polysaccharides like glucose, starch and cellulose. Nucleic acids contain carbon, hydrogen, oxygen, nitrogen and phosphorus and include DNA and RNA
Chemical equations & reactions
The document discusses chemical equations and reactions. It defines key terms like reactants, products, and coefficients. It explains how to write and balance chemical equations. It also describes different types of chemical reactions like synthesis, decomposition, and single/double replacement reactions. Guidelines are provided for predicting products and writing balanced equations.
CHEMICAL REACTIONS AND EQUATIONS
This document provides information on chemical reactions and equations. It defines a chemical reaction as a process that transforms one set of substances into another. It explains the different types of chemical equations like word equations, skeletal equations, and balanced equations. It also describes the different types of chemical reactions such as combination, decomposition, displacement, and redox reactions. It discusses oxidation and reduction processes and defines oxidizing and reducing agents. Examples of chemical equations are also provided.
Writing A Research Paper Dr. Nguyen Thi Thuy Minh
The document provides guidance on writing a research paper, including defining a rhetorical goal, structuring the paper with sections like introduction, literature review, methodology, results, and conclusion, and how to write each section. It emphasizes that each section should have a clear purpose and guide the reader. The methodology section should describe procedures and justify methods, while results should present findings objectively and discussion should interpret results and consider implications.
Atomic Structure
This document provides an overview of atomic structure, quantum theory, and electronic configuration of atoms. It discusses subatomic particles like protons, neutrons, and electrons. It describes Rutherford's experiments that showed atoms are mostly empty space with a small, dense nucleus. The number of protons determines an element, while the number of neutrons can vary between isotopes of the same element. Electrons occupy energy levels outside the nucleus. The document also discusses ion formation and how electron configuration explains how atoms combine to form molecules.
Chemical bonding chapter 6
The document summarizes different types of chemical bonding:
1. Ionic bonding results from the attraction between oppositely charged ions
2. Covalent bonding results from the sharing of electron pairs between atoms
3. Metallic bonding allows for electron delocalization and mobility in metal solids due to overlapping vacant orbitals, contributing to metals' electrical and thermal conductivity properties.
Chemical reaction types_grade_10
This document discusses types of chemical reactions, including:
1) Combination reactions where two or more reactants combine to form products, such as magnesium combining with oxygen to form magnesium oxide.
2) Displacement reactions which can be metal-metal, where a more reactive metal displaces a less reactive one, or metal-nonmetal where a metal displaces a nonmetal.
3) The document provides examples of combination and displacement reactions and classifies common types of chemical reactions like decomposition, double displacement, and oxidation-reduction reactions.
Chapter 6 Lecture- Electrons in Atoms
This document discusses electromagnetic radiation and the wave-particle duality of light. It explains that electromagnetic radiation travels as waves with characteristics of wavelength and frequency. The energy of individual photons is related to their frequency by Planck's constant. Electrons in atoms can only occupy certain allowed energy levels, absorbing or emitting photons of specific frequencies as they transition between levels. This explains atomic emission spectra and helped develop the theories of quantum mechanics.
Chemical reactions and equations
This document provides an overview of chemical reactions and equations. It discusses chemical changes and how they can be represented by balanced chemical equations. The main types of chemical reactions covered are combination reactions, decomposition reactions, displacement reactions, and oxidation-reduction reactions. Examples of each type of reaction are given. The document also explains how to balance chemical equations by ensuring equal numbers of each type of atom on both sides of the reaction equation.
Organic Compounds
This document provides information about organic compounds and their components. It defines organic compounds as those containing carbon bonded to itself, hydrogen, and other elements like oxygen, nitrogen, phosphorus or sulfur. Examples of organic compounds that make up living things are described, including carbohydrates, lipids, proteins, and nucleic acids. These compounds are composed of combinations of the elements carbon, hydrogen, oxygen, nitrogen, phosphorus and sometimes sulfur. The document emphasizes carbon's unique ability to form many diverse molecules by bonding to itself and other elements.
Structure Of Atoms
The document discusses the structure of atoms. Atoms consist of a nucleus containing protons and neutrons, surrounded by electrons in shells. The nucleus is made up of positively charged protons and neutral neutrons, while electrons have a negative charge. The symbol for each element indicates the number of protons and total nucleons (protons + neutrons).
Parts of a Research Paper
This document outlines the key parts of a research paper, including the title page, abstract, introduction, area of focus, related literature review, research questions, data analysis and interpretation, interpretation of data, action plan, and recommendations. The abstract provides a brief summary of the research. The introduction gives context and background. The area of focus describes who will benefit from the study. The literature review covers related published materials. The research questions reflect the problem being studied. Data analysis and interpretation examine the data both quantitatively and qualitatively. The interpretation of data establishes connections between findings and previous literature. The action plan describes the problem, design, and findings. Finally, recommendations are based on the conclusions and suggest further studies.
Chemical bonding by Ms Rashmi Bhatia
The document discusses chemical bonding, including:
1. Defining ionic and covalent bonding, and explaining how different types of bonds are formed through electron sharing or transfer.
2. Describing the properties of ionic and covalent compounds, such as high melting points for ionic solids and variable states of matter for covalent substances.
3. Illustrating examples of single, double, and triple covalent bonds through Lewis dot structures of molecules like H2, O2, and N2.
Organic Compounds
The document discusses organic compounds and their properties. It defines organic compounds as those containing carbon and highlights that carbon can bond with many other elements. It also distinguishes between organic and inorganic compounds, monomer and polymers, and provides examples of element, compounds and mixtures. The document encourages reflecting on what was learned about organic compounds using a KWL chart.
Curriculum design
The document discusses the definition and components of curriculum design, including the types of curriculum designs, elements such as objectives, content, and learning experiences. It also examines different philosophies that influence curriculum as well as domains and taxonomies for defining objectives and evaluating learning outcomes.
Viewers also liked (17)
Similar to Estructura electronica atomica
Ch06 outline
The document discusses the electronic structure of atoms. It introduces quantum numbers like the principal quantum number n, angular momentum quantum number l, and magnetic quantum number ml, which describe the allowed electron orbitals in an atom. The Pauli exclusion principle states that no two electrons can have the same set of quantum numbers. Electron configurations show how electrons are arranged among the orbitals in an atom based on filling orbitals in order of increasing energy.
Ap chem unit 7
This document discusses atomic structure and periodicity. It begins by explaining electromagnetic radiation and its wave characteristics. It then discusses Planck's discovery that energy is quantized and Einstein's proposal that light can be viewed as particles called photons. Next, it explains the photoelectric effect and how it provided evidence that light behaves as particles. It discusses the Bohr model of the hydrogen atom and how it correctly predicted the atom's quantized energy levels but was fundamentally incorrect. Finally, it summarizes the development of the modern quantum mechanical model of the atom and periodic trends in atomic properties such as ionization energy and atomic radius.
Chem chapt 5
The document discusses electrons in atoms and their arrangement. It begins by explaining the wave-particle duality of light and electrons. It then discusses the historical atomic models of Rutherford, Bohr, and the quantum mechanical model. The quantum mechanical model treats electrons as waves and describes their location in terms of probability distributions within orbitals. The document concludes by explaining the rules that determine electron configuration, including the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Adv chem chapt 7
This document discusses the development of atomic structure models from the early 20th century to the present. It describes experiments that showed light and matter have both wave-like and particle-like properties. This led to the development of quantum mechanics and quantum numbers to describe electron orbitals. The Bohr model of the hydrogen atom was an early success but did not apply to other atoms. Modern quantum mechanics uses probability distributions and accounts for electron spin and the Pauli exclusion principle.
Atom1
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.
Chapter6
This document discusses the electronic structure of atoms and the periodic table. It covers:
- Electrons arranged in energy levels and orbitals defined by quantum numbers
- Atomic spectra produced when electrons change energy levels
- Bohr and quantum mechanical models of the atom explaining electron arrangements
- Electron configurations written using quantum numbers that relate to positions on the periodic table.
Quantum_Mechanical_Model_of_the_Atom.pdf
1) Bohr's model of electrons orbiting the nucleus in circular orbits was ineffective beyond simple atoms like hydrogen and lithium.
2) De Broglie, Heisenberg, and Schrödinger pioneered quantum mechanics, modeling electrons as waves rather than particles in orbits.
3) Schrödinger's wave equation described electron wave functions and allowed electrons to exist in discrete energy levels around the nucleus.
202006151236284892NK-Bohr Model of Hydrogen Atom.pdf
The document summarizes the Bohr model of the hydrogen atom. It describes the key postulates of the Bohr model, including that electrons revolve in discrete orbits without radiating energy. It explains that the angular momentum of electrons in these orbits is an integral multiple of Planck's constant. The model holds that electrons can only exist in these discrete energy levels and radiate energy when jumping between levels. However, the model has limitations and fails to explain phenomena like hyperfine structure. It was later replaced by quantum mechanical models developed by Schrodinger and others.
Apchemunit7 111006100549-phpapp02
The document discusses several key concepts in atomic structure and periodicity:
1. It describes the development of atomic models from the Bohr model to the quantum mechanical model, explaining concepts like wave-particle duality, quantum numbers, and orbital shapes and energies.
2. It discusses how the periodic table evolved from early recognitions of patterns by scientists like Dobereiner to the modern periodic table developed by Meyer and Mendeleev which is organized based on atomic structure.
3. It explains the Aufbau principle and how orbitals fill in order of increasing energy, along with concepts like valence electrons and exceptions seen in transition metals.
The Atom & Spectra
1. The document discusses the development of atomic spectroscopy from 1860 to 1913, including Balmer's empirical formula for the emission spectrum of hydrogen and Bohr's theoretical model of the atom.
2. Bohr postulated that electrons orbit in stable, quantized energy levels and emit or absorb photons of specific frequencies when transitioning between levels.
3. Bohr's model accounted for the Rydberg formula and emission spectrum of hydrogen and was later extended to ions of other elements.
Quantum no.ppt
The Electron Cloud Model describes an atom as consisting of a dense nucleus surrounded by electrons that exist in different probability clouds or regions at various energy levels, as developed by Erwin Schrodinger and Werner Heisenburg. The Heisenberg Uncertainty Principle states that it is impossible to know both the momentum and position of a particle like an electron at the same time. To measure an electron's position requires striking it with a photon, which affects its motion and makes its momentum uncertain. Quantum numbers describe an electron's unique state and include the principal, angular, magnetic, and spin quantum numbers.
1. 2. Atomic structure.pptx
This document discusses the quantum mechanical model of the atom. It describes how the model considers the atom as a positively charged nucleus surrounded by electron waves that extend in space around the nucleus. Some key points of the model are that it considers the wave-like properties of electrons, describes the probabilistic nature of finding electrons in different regions, and is based on developments like de Broglie's equation and Schrodinger's wave equation. The model emphasizes that the path of an electron can never be known accurately and describes electron states in terms of probability distributions in different atomic orbitals.
Unit-IV_22UCH101_Theory-1.pptx
The document provides information on quantum theory and its application to atomic structure. It discusses key concepts such as:
1) Energy is quantized and can only be emitted or absorbed in discrete packets called quanta.
2) Electrons in atoms exist in discrete energy levels called shells or orbitals. They can only transition between these levels by absorbing or emitting quanta of energy.
3) Quantum numbers are used to describe the specific energy state of each electron in an atom, including its distance from the nucleus, energy, and orientation.
Emission spectrum of hydrogen
This would enable students to explain the emission spectrum of hydrogen using the Bohr model of the hydrogen atom; calculate the energy, wavelength, and frequencies involved in the electron transitions in the hydrogen atom; relate the emission spectra to common occurrences like fireworks and neon lights; and describe the Bohr model of the atom and the inadequacies of the Bohr model.
Bhor's Atomic model
1. Electromagnetic radiation travels as waves through space at the speed of light and includes radio waves, microwaves, infrared, visible light, ultraviolet, X-rays and gamma rays.
2. Wavelength is the distance between peaks of a wave and frequency is the number of waves passing a point per second.
3. The Bohr model describes atoms with electrons orbiting the nucleus in discrete energy levels, absorbing or emitting energy when changing orbits.
Electrons in atoms notes
The document summarizes the development of atomic models from Rutherford to the current quantum mechanical model. It discusses inadequacies in Rutherford's model that could not explain atomic properties and emissions. Bohr proposed electrons orbit in distinct energy levels, but this failed to explain multi-electron atoms. The quantum mechanical model treats electrons as waves using Schrodinger's equation, describing electrons as probability distributions rather than particles. It introduces quantum numbers to characterize electron states and explains how orbitals are filled according to various rules.
Reduced mass
1. Niels Bohr developed his model of the hydrogen atom in 1913 based on four postulates, including that an electron's orbit must have an integral angular momentum and that it does not radiate energy while in these orbits.
2. The Bohr model successfully predicted the spectrum of hydrogen but was ultimately incomplete and unsatisfying as it was a mixture of classical and quantum ideas.
3. While it worked for hydrogen, the Bohr model failed for other atoms and did not explain transition rates between energy levels. A fully quantum mechanical approach like Schrodinger's theory was needed.
B.tech. ii engineering chemistry Unit 1 atoms and molecules
1) The document describes the potential energy diagram and mathematical expression for a particle confined in a 1D box between 0 and L.
2) It shows that the Schrodinger equation inside the box is similar to the free particle equation, and the solutions are sine waves with allowed energies of En = n^2*h^2/8mL^2.
3) This particle in a box model is used to understand the quantization of energy levels for electrons in an atom.
G9_Baroque design _20240407_094241_0000.pdf
The document discusses the quantum mechanical model of the atom. It explains how Bohr's early model was replaced by a quantum mechanical model based on the work of de Broglie, Heisenberg, and Schrodinger. Key points include:
- Electrons behave as waves and orbitals represent the probability of finding electrons in different regions, rather than fixed orbits.
- Orbitals are specified by principal, azimuthal, and magnetic quantum numbers.
- The 1s orbital is the lowest energy state for hydrogen's single electron.
G9_Baroque design _20240407_094241_0000.pdf
The document discusses the Bohr and quantum mechanical models of the atom. It explains that Bohr's model improved on earlier models by proposing that electrons orbit the nucleus in fixed, quantized energy levels. However, it did not adequately explain atomic spectra. The quantum mechanical model developed the idea that electrons can be described as waves rather than particles, based on the work of de Broglie and Heisenberg. Electrons occupy atomic orbitals that are probability maps showing where electrons are likely to be found, rather than defined orbits. The quantum mechanical model uses quantum numbers to specify atomic orbitals and is able to explain atomic spectra for all elements.
Similar to Estructura electronica atomica (20)
202006151236284892NK-Bohr Model of Hydrogen Atom.pdf
202006151236284892NK-Bohr Model of Hydrogen Atom.pdf
B.tech. ii engineering chemistry Unit 1 atoms and molecules
B.tech. ii engineering chemistry Unit 1 atoms and molecules
Recently uploaded
Introduction to AI for Nonprofits with Tapp Network
Dive into the world of AI! Experts Jon Hill and Tareq Monaur will guide you through AI's role in enhancing nonprofit websites and basic marketing strategies, making it easy to understand and apply.
Main Java[All of the Base Concepts}.docx
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
How to Build a Module in Odoo 17 Using the Scaffold Method
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.
Chapter 4 - Islamic Financial Institutions in Malaysia.pptx
Chapter 4 - Islamic Financial Institutions in Malaysia.pptxMohd Adib Abd Muin, Senior Lecturer at Universiti Utara Malaysia
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.
Azure Interview Questions and Answers PDF By ScholarHat
Azure Interview Questions and Answers PDF By ScholarHat
CACJapan - GROUP Presentation 1- Wk 4.pdf
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
The simplified electron and muon model, Oscillating Spacetime: The Foundation...
Discover the Simplified Electron and Muon Model: A New Wave-Based Approach to Understanding Particles delves into a groundbreaking theory that presents electrons and muons as rotating soliton waves within oscillating spacetime. Geared towards students, researchers, and science buffs, this book breaks down complex ideas into simple explanations. It covers topics such as electron waves, temporal dynamics, and the implications of this model on particle physics. With clear illustrations and easy-to-follow explanations, readers will gain a new outlook on the universe's fundamental nature.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
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
Digital Artifact 1 - 10VCD Environments Unit
Digital Artifact 1 - 10VCD Environments Unit - NGV Pavilion Concept Design
ANATOMY AND BIOMECHANICS OF HIP JOINT.pdf
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.
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Natural birth techniques - Mrs.Akanksha Trivedi Rama UniversityAkanksha trivedi rama nursing college kanpur.
Natural birth techniques are various type such as/ water birth , alexender method, hypnosis, bradley method, lamaze method etcHow to Fix the Import Error in the Odoo 17
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective UpskillingExcellence Foundation for South Sudan
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.Advanced Java[Extra Concepts, Not Difficult].docx
This is part 2 of my Java Learning Journey. This contains Hashing, ArrayList, LinkedList, Date and Time Classes, Calendar Class and more.
DRUGS AND ITS classification slide share
Any substance (other than food) that is used to prevent, diagnose, treat, or relieve symptoms of a
disease or abnormal condition
A Survey of Techniques for Maximizing LLM Performance.pptx
A Survey of Techniques for Maximizing LLM Performance
Recently uploaded (20)
Introduction to AI for Nonprofits with Tapp Network
Introduction to AI for Nonprofits with Tapp Network
How to Build a Module in Odoo 17 Using the Scaffold Method
How to Build a Module in Odoo 17 Using the Scaffold Method
Chapter 4 - Islamic Financial Institutions in Malaysia.pptx
Chapter 4 - Islamic Financial Institutions in Malaysia.pptx
Azure Interview Questions and Answers PDF By ScholarHat
Azure Interview Questions and Answers PDF By ScholarHat
Film vocab for eal 3 students: Australia the movie
Film vocab for eal 3 students: Australia the movie
The simplified electron and muon model, Oscillating Spacetime: The Foundation...
The simplified electron and muon model, Oscillating Spacetime: The Foundation...
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Digital Artefact 1 - Tiny Home Environmental Design
Digital Artefact 1 - Tiny Home Environmental Design
Liberal Approach to the Study of Indian Politics.pdf
Liberal Approach to the Study of Indian Politics.pdf
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective Upskilling
A Survey of Techniques for Maximizing LLM Performance.pptx
A Survey of Techniques for Maximizing LLM Performance.pptx
Estructura electronica atomica
- 1. Chapter 6 Electronic Structure of Atoms Prentice Hall © 2003 Chapter 6 CHEMISTRY The Central Science 9th Edition David P. White
- 3. Prentice Hall © 2003 Chapter 6 The Wave Nature of Light
- 4. The Wave Nature of Light
- 6. The Wave Nature of Light
- 7. Prentice Hall © 2003 Chapter 6
- 8. Prentice Hall © 2003 Chapter 6 The Wave Nature of Light
- 9. Prentice Hall © 2003 Chapter 6
- 14. Prentice Hall © 2003 Chapter 6
- 15. Prentice Hall © 2003 Chapter 6
- 16. Prentice Hall © 2003 Chapter 6
- 18. Prentice Hall © 2003 Chapter 6
- 20. Prentice Hall © 2003 Chapter 6
- 26. Prentice Hall © 2003 Chapter 6
- 27. Prentice Hall © 2003 Chapter 6
- 29. Bohr Model Line Spectra and the Bohr Model
- 30. Prentice Hall © 2003 Chapter 6
- 31. Prentice Hall © 2003 Chapter 6
- 34. Prentice Hall © 2003 Chapter 6
- 35. Prentice Hall © 2003 Chapter 6
- 36. Prentice Hall © 2003 Chapter 6
- 38. Prentice Hall © 2003 Chapter 6 H = x
- 40. Prentice Hall © 2003 Chapter 6 Quantum Mechanics and Atomic Orbitals
- 43. Prentice Hall © 2003 Chapter 6
- 44. Prentice Hall © 2003 Chapter 6
- 45. Prentice Hall © 2003 Chapter 6
- 46. Prentice Hall © 2003 Chapter 6
- 47. Prentice Hall © 2003 Chapter 6
- 53. Prentice Hall © 2003 Chapter 6 The s-Orbitals Representations of Orbitals
- 55. Prentice Hall © 2003 Chapter 6 The p-Orbitals Representations of Orbitals
- 60. Electron Spin and the Pauli Exclusion Principle
- 64. Prentice Hall © 2003 Chapter 6
- 65. Prentice Hall © 2003 Chapter 6
- 66. Prentice Hall © 2003 Chapter 6
- 67. Many-Electron Atoms Orbitals and Their Energies
- 68. Prentice Hall © 2003 Chapter 6
- 69. Prentice Hall © 2003 Chapter 6
- 77. End of Chapter 6: Electronic Structure of Atoms Prentice Hall © 2003 Chapter 6