The document discusses a super-resonance model of valence bonding that involves electrons resonating between atomic nuclei. It proposes that valence bonds form due to electrons jumping between nuclei connected by the bond, with each jump involving proton-electron-neutron resonance. It also notes that resonances can occur between resonances, with an unlimited number of hierarchical resonance levels. The model aims to explain the nature of valence bonding beyond traditional models involving electron exchange.
Problem of the direct quantum-information transformation of chemical substance Vasil Penchev
The “Trigger field” from sci-fi to science
ISPC’20 - 2016
Boca Raton, FL, USA: 1-4 August 2016
International Society for the Philosophy of Chemistry:20th Annual Conference
Arthur Clark and Michael Kube–McDowell (“The Triger”, 1999) suggested the sci-fi idea about the direct transformation from a chemical substance into another by the action of a newly physical, “Trigger” field
Karl Brohier, a Nobel Prize winner, who is a dramatic persona in the novel, elaborates a new theory, re-reading and re-writing Pauling’s “The Nature of the Chemical Bond”
According to Brohier: “Information organizes and differentiates energy. It regularizes and stabilizes matter. Information propagates through matter-energy and mediates the interactions of matter-energy”
Dr Horton, his collaborator in the novel replies: “If the universe consists of energy and information, then the Trigger somehow alters the information envelope of certain substances –“
“Alters it, scrambles it, overwhelms it, destabilizes it” Brohier adds. 'And crudely, too. The units we're building now are unimaginably wasteful - like hitting a computer with ten thousand volts of lightning to change a few bytes of its programming. It was a fluke, pure serendipity, that somewhere in the smear of informational noise describing your prototype were a few coherent words in the language of resonance mechanics - the new science of matter. You stumbled on the characteristic chemical signature of certain nitrate compounds, which picked your signal out of the air like a ham radio operator finding a voice in the static.'
One can suggest that any chemical substances and changes are fundamentally representable as quantum information and its transformations
If entanglement is interpreted as a physical field, though any group above seems to be unattachable to it, it might be identified as the “Triger field”
It might cause a direct transformation of any chemical substance from a remote distance
Is this possible in principle?
Particle physics is the branch of physics that studies subatomic particles and their interactions. By 1932, the four known elementary particles were the electron, proton, photon, and neutron. Elementary particles are the fundamental building blocks of the universe and have well-documented properties including mass, charge, spin, and lifetime. Some particles decay into others of smaller mass through weak interactions. Quarks are elementary particles that combine to form composite hadrons like protons and neutrons, and have properties like charge, mass, and six flavors including up, down, strange, charm, bottom, and top. Strangeness is a quantum number denoting the presence of a strange quark and is conserved in strong and electromagnetic interactions.
This document discusses intermolecular forces and how they relate to physical properties of substances. It defines intramolecular bonds as bonds within a molecule, and intermolecular forces as forces between molecules. The three main types of intermolecular forces are London dispersion forces, dipole-dipole forces, and hydrogen bonds. London dispersion forces are present in all molecules but strongest in nonpolar molecules. Dipole-dipole forces occur between polar molecules. Hydrogen bonds are the strongest intermolecular force and occur when hydrogen is bonded to an electronegative atom like oxygen, nitrogen or fluorine. Stronger intermolecular forces lead to higher melting and boiling points, as well as increased viscosity and surface tension in liquids.
This document discusses different types of chemical bonds, including ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between metals and nonmetals, forming oppositely charged ions that are attracted in a crystal lattice. Covalent bonds involve the sharing of electrons between nonmetal atoms. Lewis structures can represent electron and bond arrangements in molecules and ions using dots and lines. The octet rule describes atoms' tendency to bond so they have eight electrons in their valence shell, like noble gases. Exceptions include hydrogen following the duet rule and structures with underfilled or overfilled octets.
Hello everyone, I am Dr. Ujwalkumar Trivedi, Head of Biotechnology Department at Marwadi University Rajkot. I teach Molecular Biology to the students of M.Sc. Microbiology and Biotechnology.
The current presentation is like a history book of various discoveries that led to the development of quantum mechanics. The presentation also tries to address the debate between the radicals (supporters of quantum theory) and classical (supporters of Newtonian physics).
Valence shell electron pair repulsion (VSEPR) theory is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. It is also named the Gillespie-Nyholm theory after its two main developers, Ronald Gillespie and Ronald Nyholm
The document discusses the development of Bohr's model of the atom. It begins by describing some limitations of Rutherford's model, namely that electrons orbiting the nucleus should emit electromagnetic radiation and lose energy according to classical physics. Bohr proposed a quantum model where electrons can only orbit in certain fixed energy levels, avoiding this issue. His model incorporated postulates that electrons can only have specific allowed energies and move between levels by absorbing or emitting photons of exact frequencies. This explained the emission spectrum of hydrogen. However, the model only worked for hydrogen and grew cumbersome for larger atoms.
Problem of the direct quantum-information transformation of chemical substance Vasil Penchev
The “Trigger field” from sci-fi to science
ISPC’20 - 2016
Boca Raton, FL, USA: 1-4 August 2016
International Society for the Philosophy of Chemistry:20th Annual Conference
Arthur Clark and Michael Kube–McDowell (“The Triger”, 1999) suggested the sci-fi idea about the direct transformation from a chemical substance into another by the action of a newly physical, “Trigger” field
Karl Brohier, a Nobel Prize winner, who is a dramatic persona in the novel, elaborates a new theory, re-reading and re-writing Pauling’s “The Nature of the Chemical Bond”
According to Brohier: “Information organizes and differentiates energy. It regularizes and stabilizes matter. Information propagates through matter-energy and mediates the interactions of matter-energy”
Dr Horton, his collaborator in the novel replies: “If the universe consists of energy and information, then the Trigger somehow alters the information envelope of certain substances –“
“Alters it, scrambles it, overwhelms it, destabilizes it” Brohier adds. 'And crudely, too. The units we're building now are unimaginably wasteful - like hitting a computer with ten thousand volts of lightning to change a few bytes of its programming. It was a fluke, pure serendipity, that somewhere in the smear of informational noise describing your prototype were a few coherent words in the language of resonance mechanics - the new science of matter. You stumbled on the characteristic chemical signature of certain nitrate compounds, which picked your signal out of the air like a ham radio operator finding a voice in the static.'
One can suggest that any chemical substances and changes are fundamentally representable as quantum information and its transformations
If entanglement is interpreted as a physical field, though any group above seems to be unattachable to it, it might be identified as the “Triger field”
It might cause a direct transformation of any chemical substance from a remote distance
Is this possible in principle?
Particle physics is the branch of physics that studies subatomic particles and their interactions. By 1932, the four known elementary particles were the electron, proton, photon, and neutron. Elementary particles are the fundamental building blocks of the universe and have well-documented properties including mass, charge, spin, and lifetime. Some particles decay into others of smaller mass through weak interactions. Quarks are elementary particles that combine to form composite hadrons like protons and neutrons, and have properties like charge, mass, and six flavors including up, down, strange, charm, bottom, and top. Strangeness is a quantum number denoting the presence of a strange quark and is conserved in strong and electromagnetic interactions.
This document discusses intermolecular forces and how they relate to physical properties of substances. It defines intramolecular bonds as bonds within a molecule, and intermolecular forces as forces between molecules. The three main types of intermolecular forces are London dispersion forces, dipole-dipole forces, and hydrogen bonds. London dispersion forces are present in all molecules but strongest in nonpolar molecules. Dipole-dipole forces occur between polar molecules. Hydrogen bonds are the strongest intermolecular force and occur when hydrogen is bonded to an electronegative atom like oxygen, nitrogen or fluorine. Stronger intermolecular forces lead to higher melting and boiling points, as well as increased viscosity and surface tension in liquids.
This document discusses different types of chemical bonds, including ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between metals and nonmetals, forming oppositely charged ions that are attracted in a crystal lattice. Covalent bonds involve the sharing of electrons between nonmetal atoms. Lewis structures can represent electron and bond arrangements in molecules and ions using dots and lines. The octet rule describes atoms' tendency to bond so they have eight electrons in their valence shell, like noble gases. Exceptions include hydrogen following the duet rule and structures with underfilled or overfilled octets.
Hello everyone, I am Dr. Ujwalkumar Trivedi, Head of Biotechnology Department at Marwadi University Rajkot. I teach Molecular Biology to the students of M.Sc. Microbiology and Biotechnology.
The current presentation is like a history book of various discoveries that led to the development of quantum mechanics. The presentation also tries to address the debate between the radicals (supporters of quantum theory) and classical (supporters of Newtonian physics).
Valence shell electron pair repulsion (VSEPR) theory is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. It is also named the Gillespie-Nyholm theory after its two main developers, Ronald Gillespie and Ronald Nyholm
The document discusses the development of Bohr's model of the atom. It begins by describing some limitations of Rutherford's model, namely that electrons orbiting the nucleus should emit electromagnetic radiation and lose energy according to classical physics. Bohr proposed a quantum model where electrons can only orbit in certain fixed energy levels, avoiding this issue. His model incorporated postulates that electrons can only have specific allowed energies and move between levels by absorbing or emitting photons of exact frequencies. This explained the emission spectrum of hydrogen. However, the model only worked for hydrogen and grew cumbersome for larger atoms.
1) The document discusses the early development of atomic theory from ancient Greek philosophers to early 20th century scientists. It describes the atomic theories of Democritus, Aristotle, Dalton, Thomson, and Rutherford and how their models of the atom evolved based on new experimental evidence.
2) John Dalton combined previous experimental findings to propose his atomic theory that all matter is composed of indivisible atoms and that atoms of different elements have different properties. J.J. Thomson's experiments led him to propose that atoms are made of negatively charged electrons embedded in a sphere of positive charge, the "plum pudding" model.
3) Rutherford's gold foil experiment caused him to conclude that atoms have a very small
This document discusses how valence bond theory and hybrid orbital theory explain how bonds are formed at the quantum mechanical level. It begins by stating that Lewis structures, VSEPR theory, and bond dipoles do not fully describe how bonds are formed. It then introduces valence bond theory, which describes how atomic orbitals overlap to form bonding orbitals with electron pairs. Hybridization is introduced as the process where atomic orbitals combine to form new hybrid orbitals. Examples are given of sp, sp2, and sp3 hybrid orbitals and how they explain the bonding in molecules like methane, water, boron trifluoride, beryllium chloride, and ammonia. The document also distinguishes between sigma and pi bonds, and
This document discusses molecules and the different types of bonds that hold atoms together to form compounds. It describes ionic bonds, which form when one atom transfers electrons to another, and covalent bonds, which form when atoms share electrons. The document also discusses molecular spectra arising from rotational and vibrational energy levels of molecules, and how infrared spectroscopy can analyze molecular vibrations. Potential energy graphs illustrate the attractive and repulsive forces between atoms at different distances that determine molecular structure.
The document discusses Valence Shell Electron Pair Repulsion (VSEPR) Theory. VSEPR Theory states that the shape of a molecule is determined by the number of electron pairs around the central atom. Electron pairs repel each other and arrange as far apart as possible. Bond pairs and lone pairs cause repulsion, with lone pairs causing more repulsion than bond pairs. The geometry that results in the lowest repulsion determines the molecular shape. Common molecular shapes include linear, trigonal planar, and tetrahedral.
This document discusses key concepts in chemistry including thermal energy, the kinetic molecular theory of matter, and states of matter. It begins by defining thermal energy as the energy of a body due to the motion of its particles, which is directly proportional to temperature. It then explains kinetic and potential energy. The document goes on to discuss how the three states of matter arise from a competition between intermolecular forces and thermal energy. It also summarizes the kinetic molecular theory and how it applies to solids, liquids, and gases. Finally, it briefly defines and compares the processes of diffusion and effusion.
The document summarizes key concepts about the nature of matter including:
- Matter is anything that has mass and takes up space. Physical properties like color, size and state can be observed without changing the substance.
- Elements are substances made of only one type of atom. Compounds contain two or more elements chemically bonded together.
- Atoms are the basic building blocks of matter and contain protons, neutrons and electrons. The number of protons determines the element.
This document discusses the nature of gravity and its relationship to other forces and fields. It provides evidence that gravity is an emergent phenomenon that arises from an underlying non-gravitational theory. Specifically:
1) Gravity behaves differently than other forces in that it curves spacetime itself rather than being mediated by particle exchanges. However, quantum gravity theories propose gravitons as force-carrying particles.
2) Holographic duality theories from the 1990s demonstrated that gravitational theories in higher dimensions are equivalent to non-gravitational theories in lower dimensions.
3) Modern developments like string theory and the AdS/CFT correspondence provide concrete examples of holography and establish gravity as an emer
This document summarizes key concepts about atoms, molecules, and chemical bonds. It defines atoms as the smallest unit of an element, consisting of a nucleus with protons and neutrons surrounded by electrons. Molecules are formed when two or more atoms bond together, such as through covalent bonds where atoms share electrons. The document also outlines Dalton's atomic theory and the laws of chemical combination, including the law of conservation of mass and the law of constant proportions.
The quantum mechanical model of the atom developed from the ideas of three physicists: Erwin Schrodinger, Louis de Broglie, and Werner Heisenberg. De Broglie and Schrodinger proposed that electrons have both particle and wave properties, resembling standing waves around the nucleus. Only certain orbits allow an integer number of wavelengths to fit, determining electron energy levels. Schrodinger developed an equation to calculate these quantized energy levels. Heisenberg's uncertainty principle holds that the exact position and momentum of an electron cannot be known simultaneously. Orbitals describe the probability of finding an electron in a region as determined by wave functions, rather than definite orbits.
This document discusses valence shell electron pair repulsion (VSEPR) theory, which is used to predict the shape of covalent molecules and polyatomic ions based on the arrangement of electron pairs around the central atom. According to VSEPR theory, electron pairs around the central atom repel each other and arrange themselves as far apart as possible to minimize repulsion. The type of electron pair repulsion determines the molecular shape, with lone pairs repelling each other more than lone pairs and bonding pairs or just bonding pairs alone. Examples are provided to illustrate VSEPR theory predictions of molecular geometry.
The periodic table arranges elements based on electron configuration in atoms. Elements in the same group have similar valence electron structures and chemical properties. Electrons fill atomic orbitals according to the Aufbau principle and Hund's rule. Valence electrons determine how elements bond and react. Ion charges form when atoms gain or lose valence electrons to achieve stable full shells like noble gases. Magnetism results from aligned spins of unpaired electrons.
Valence shell electron pair repulsion theory (VSEPR THEORY)Altamash Ali
Designed in a very easy manner so that u all are able to understand each and everything easily.
Gillespie & Nyholm proposed this theory ion 1957 and its is based on the direction of bonds in a polyatomic molecule.
Based on this there are several postulate that are very necessary to know before any molecule to study.
Resonance effect occurs when a compound can be represented by two or more Lewis structures with the same arrangement of atoms. These contributing structures are called resonance structures.
The resonance structures are hypothetical and do not represent real molecules individually. Together they contribute to a resonance hybrid structure that is more stable than any individual resonance structure. The most stable contributing structure contributes the most to the resonance hybrid.
Conditions for resonance include sp or sp2 hybridized atoms involved, overlapping parallel p-orbitals to form a conjugated system. The sigma bond framework remains the same between structures, atomic positions do not change, and electron counts are equal.
The document discusses elementary particles and their classification. It describes how elementary particles are divided into two main groups: fermions and bosons. Fermions include quarks and leptons, which have half-integer spin and obey the Pauli exclusion principle. Bosons have integer spin and obey Bose-Einstein statistics, carrying the fundamental forces. The standard model of particle physics describes three of the four fundamental forces and all known elementary particles.
1. The document provides an overview of concepts relevant to nanochemistry including the periodic table, atomic structure, size of atoms, molecules and phases, types of chemical bonds, quantum mechanics principles, and solid-state band theory.
2. Key topics covered include the periodic arrangement of elements, subatomic particles that make up atoms, sizes of atoms ranging from 0.1-0.5 nanometers, different states of matter, various types of chemical bonds between atoms, the four quantum numbers that describe electrons, Heisenberg's uncertainty principle, and how materials behave as semiconductors, conductors or insulators depending on their band structure.
3. The document also defines nano as a prefix meaning one billion
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.
This document provides instructions for a science lesson on the states of matter. It includes:
1) A list of materials needed for the lesson, including worksheets and online activities.
2) Directions for students to play an online game to sort examples of solids, liquids, gases and plasma.
3) Background information on the four states of matter and how atoms and molecules move differently in each state.
4) Worksheets for students to complete, including illustrations of atomic movement in each state and a Venn diagram to organize characteristics of the three states.
The document discusses the history and key concepts of molecular orbital theory. It was developed in the early 20th century to explain bonding in molecules beyond what valence bond theory could. Molecular orbital theory describes how atomic orbitals combine to form new molecular orbitals via quantum mechanics. There are bonding, antibonding, and nonbonding molecular orbitals. Electrons fill these orbitals based on energy level, with bonding orbitals having lower energy than atomic orbitals and antibonding orbitals having higher energy.
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.
1) The document discusses the early development of atomic theory from ancient Greek philosophers to early 20th century scientists. It describes the atomic theories of Democritus, Aristotle, Dalton, Thomson, and Rutherford and how their models of the atom evolved based on new experimental evidence.
2) John Dalton combined previous experimental findings to propose his atomic theory that all matter is composed of indivisible atoms and that atoms of different elements have different properties. J.J. Thomson's experiments led him to propose that atoms are made of negatively charged electrons embedded in a sphere of positive charge, the "plum pudding" model.
3) Rutherford's gold foil experiment caused him to conclude that atoms have a very small
This document discusses how valence bond theory and hybrid orbital theory explain how bonds are formed at the quantum mechanical level. It begins by stating that Lewis structures, VSEPR theory, and bond dipoles do not fully describe how bonds are formed. It then introduces valence bond theory, which describes how atomic orbitals overlap to form bonding orbitals with electron pairs. Hybridization is introduced as the process where atomic orbitals combine to form new hybrid orbitals. Examples are given of sp, sp2, and sp3 hybrid orbitals and how they explain the bonding in molecules like methane, water, boron trifluoride, beryllium chloride, and ammonia. The document also distinguishes between sigma and pi bonds, and
This document discusses molecules and the different types of bonds that hold atoms together to form compounds. It describes ionic bonds, which form when one atom transfers electrons to another, and covalent bonds, which form when atoms share electrons. The document also discusses molecular spectra arising from rotational and vibrational energy levels of molecules, and how infrared spectroscopy can analyze molecular vibrations. Potential energy graphs illustrate the attractive and repulsive forces between atoms at different distances that determine molecular structure.
The document discusses Valence Shell Electron Pair Repulsion (VSEPR) Theory. VSEPR Theory states that the shape of a molecule is determined by the number of electron pairs around the central atom. Electron pairs repel each other and arrange as far apart as possible. Bond pairs and lone pairs cause repulsion, with lone pairs causing more repulsion than bond pairs. The geometry that results in the lowest repulsion determines the molecular shape. Common molecular shapes include linear, trigonal planar, and tetrahedral.
This document discusses key concepts in chemistry including thermal energy, the kinetic molecular theory of matter, and states of matter. It begins by defining thermal energy as the energy of a body due to the motion of its particles, which is directly proportional to temperature. It then explains kinetic and potential energy. The document goes on to discuss how the three states of matter arise from a competition between intermolecular forces and thermal energy. It also summarizes the kinetic molecular theory and how it applies to solids, liquids, and gases. Finally, it briefly defines and compares the processes of diffusion and effusion.
The document summarizes key concepts about the nature of matter including:
- Matter is anything that has mass and takes up space. Physical properties like color, size and state can be observed without changing the substance.
- Elements are substances made of only one type of atom. Compounds contain two or more elements chemically bonded together.
- Atoms are the basic building blocks of matter and contain protons, neutrons and electrons. The number of protons determines the element.
This document discusses the nature of gravity and its relationship to other forces and fields. It provides evidence that gravity is an emergent phenomenon that arises from an underlying non-gravitational theory. Specifically:
1) Gravity behaves differently than other forces in that it curves spacetime itself rather than being mediated by particle exchanges. However, quantum gravity theories propose gravitons as force-carrying particles.
2) Holographic duality theories from the 1990s demonstrated that gravitational theories in higher dimensions are equivalent to non-gravitational theories in lower dimensions.
3) Modern developments like string theory and the AdS/CFT correspondence provide concrete examples of holography and establish gravity as an emer
This document summarizes key concepts about atoms, molecules, and chemical bonds. It defines atoms as the smallest unit of an element, consisting of a nucleus with protons and neutrons surrounded by electrons. Molecules are formed when two or more atoms bond together, such as through covalent bonds where atoms share electrons. The document also outlines Dalton's atomic theory and the laws of chemical combination, including the law of conservation of mass and the law of constant proportions.
The quantum mechanical model of the atom developed from the ideas of three physicists: Erwin Schrodinger, Louis de Broglie, and Werner Heisenberg. De Broglie and Schrodinger proposed that electrons have both particle and wave properties, resembling standing waves around the nucleus. Only certain orbits allow an integer number of wavelengths to fit, determining electron energy levels. Schrodinger developed an equation to calculate these quantized energy levels. Heisenberg's uncertainty principle holds that the exact position and momentum of an electron cannot be known simultaneously. Orbitals describe the probability of finding an electron in a region as determined by wave functions, rather than definite orbits.
This document discusses valence shell electron pair repulsion (VSEPR) theory, which is used to predict the shape of covalent molecules and polyatomic ions based on the arrangement of electron pairs around the central atom. According to VSEPR theory, electron pairs around the central atom repel each other and arrange themselves as far apart as possible to minimize repulsion. The type of electron pair repulsion determines the molecular shape, with lone pairs repelling each other more than lone pairs and bonding pairs or just bonding pairs alone. Examples are provided to illustrate VSEPR theory predictions of molecular geometry.
The periodic table arranges elements based on electron configuration in atoms. Elements in the same group have similar valence electron structures and chemical properties. Electrons fill atomic orbitals according to the Aufbau principle and Hund's rule. Valence electrons determine how elements bond and react. Ion charges form when atoms gain or lose valence electrons to achieve stable full shells like noble gases. Magnetism results from aligned spins of unpaired electrons.
Valence shell electron pair repulsion theory (VSEPR THEORY)Altamash Ali
Designed in a very easy manner so that u all are able to understand each and everything easily.
Gillespie & Nyholm proposed this theory ion 1957 and its is based on the direction of bonds in a polyatomic molecule.
Based on this there are several postulate that are very necessary to know before any molecule to study.
Resonance effect occurs when a compound can be represented by two or more Lewis structures with the same arrangement of atoms. These contributing structures are called resonance structures.
The resonance structures are hypothetical and do not represent real molecules individually. Together they contribute to a resonance hybrid structure that is more stable than any individual resonance structure. The most stable contributing structure contributes the most to the resonance hybrid.
Conditions for resonance include sp or sp2 hybridized atoms involved, overlapping parallel p-orbitals to form a conjugated system. The sigma bond framework remains the same between structures, atomic positions do not change, and electron counts are equal.
The document discusses elementary particles and their classification. It describes how elementary particles are divided into two main groups: fermions and bosons. Fermions include quarks and leptons, which have half-integer spin and obey the Pauli exclusion principle. Bosons have integer spin and obey Bose-Einstein statistics, carrying the fundamental forces. The standard model of particle physics describes three of the four fundamental forces and all known elementary particles.
1. The document provides an overview of concepts relevant to nanochemistry including the periodic table, atomic structure, size of atoms, molecules and phases, types of chemical bonds, quantum mechanics principles, and solid-state band theory.
2. Key topics covered include the periodic arrangement of elements, subatomic particles that make up atoms, sizes of atoms ranging from 0.1-0.5 nanometers, different states of matter, various types of chemical bonds between atoms, the four quantum numbers that describe electrons, Heisenberg's uncertainty principle, and how materials behave as semiconductors, conductors or insulators depending on their band structure.
3. The document also defines nano as a prefix meaning one billion
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.
This document provides instructions for a science lesson on the states of matter. It includes:
1) A list of materials needed for the lesson, including worksheets and online activities.
2) Directions for students to play an online game to sort examples of solids, liquids, gases and plasma.
3) Background information on the four states of matter and how atoms and molecules move differently in each state.
4) Worksheets for students to complete, including illustrations of atomic movement in each state and a Venn diagram to organize characteristics of the three states.
The document discusses the history and key concepts of molecular orbital theory. It was developed in the early 20th century to explain bonding in molecules beyond what valence bond theory could. Molecular orbital theory describes how atomic orbitals combine to form new molecular orbitals via quantum mechanics. There are bonding, antibonding, and nonbonding molecular orbitals. Electrons fill these orbitals based on energy level, with bonding orbitals having lower energy than atomic orbitals and antibonding orbitals having higher energy.
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.
This document provides an overview of infrared spectroscopy. It discusses how infrared radiation interacts with molecules by causing vibrations between their atomic bonds. The absorption of infrared radiation depends on characteristics like the mass of the atoms in the bond and the stiffness of the chemical bond. Quantum mechanics describes the vibrational energy levels of molecules as discrete, quantized values. Even at absolute zero, molecules will possess a minimum vibrational energy called zero-point energy due to their quantum nature. Infrared spectroscopy can reveal information about molecular structure by examining their characteristic vibrational frequencies.
Relativity and Quantum Mechanics Are Not "Incompatible"John47Wind
Many scientific journals, books, magazines and science web sites state that since Einstein’s theory of gravity doesn’t “fit” into the quantum theory of forces, a new quantum theory of gravity must be found. This essay explodes the prevailing scientific myth that relativity and quantum mechanics are somehow incompatible. The simple fact of the matter is that gravity is not a force at all, so trying to make it “fit” into quantum theory is impossible. This essay demonstrates that relativity and quantum physics are indeed different, but it’s simply a matter of scale. In fact they are perfect reflections of each other.
This document provides a summary of key concepts from 11 chapters of a chemistry textbook. It outlines fundamental chemistry topics like matter, elements, compounds, chemical bonds and reactions. Specific concepts covered include the nature of chemistry, atomic theory, the periodic table, stoichiometry, gases and more. Formulas, equations and models are explained that are important for understanding the structure and behavior of matter at the molecular level.
The Pauli Exclusion Principle states that no two electrons in an atom can exist in the same quantum state. Each electron must have a different set of quantum numbers (n, l, ml, ms). Pauli concluded this empirically from studying atomic spectra. The principle governs the electronic configuration of atoms with more than one electron. It explains why certain atomic transitions are observed, depending on whether the spins of the electrons are parallel or antiparallel. The principle extends to all fermions, which have half-integer spin and obey Fermi-Dirac statistics.
This is a schrodinger equation and also Heiseinberg's uncertainty principle.
It is necessary to know this equation for the quantum mechanic. The wave equation, uncertainty principle of Heisenberg, time dependent and independent of schrodinguer...
B.tech. ii engineering chemistry Unit 1 atoms and moleculesRai University
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.
This document provides a summary of key concepts from the first 7 chapters of a chemistry textbook. It covers topics such as the nature of chemistry, matter and its composition, atomic theory, electronic configuration, the periodic table, and chemical bonds. Specifically, it defines chemistry as the study of matter and its changes. It also discusses the organization of the periodic table and how elements are arranged based on their atomic structure and properties. Finally, it describes different types of chemical bonds such as ionic bonds and covalent bonds that form through the sharing or transfer of electrons between atoms.
This document provides an overview of key concepts from 10 chapters on chemistry. It covers topics such as the nature of chemistry, matter and its composition, atomic theory, electronic configuration, the periodic table, chemical bonds, molecular geometry, naming chemicals, chemical reactions, and stoichiometry. For each chapter, it lists important concepts in bullet points along with brief definitions or explanations.
The Standard Model and the LHC in the Higgs Boson Erajuanrojochacon
The document discusses the Standard Model of particle physics and the role of the Large Hadron Collider (LHC) following the discovery of the Higgs boson. It provides background on the development of the Standard Model and discovery of its key particles like quarks, gluons, and weak bosons. It describes the LHC as the most powerful particle collider built to explore physics at the highest energies and probe unanswered questions left by the Standard Model. Four main detectors at the LHC, including ATLAS and CMS, precisely measure collision products to explore fundamental particles and forces.
Study on the Energy Level Splitting of the Francium Atom Fr in an External Ma...ijtsrd
In This paper the normal Francium atom is considered with the use of non relativistic quantum mechanical approach and the Bohrs atomic model. We study the energy shift values of a Francium atom by the external magnetic fields effect we considered the two cases that effect without external magnetic fields and those of with the external magnetic fields. Win Moe Thant "Study on the Energy Level Splitting of the Francium Atom (Fr) in an External Magnetic Field" Published in International Journal of Trend in Scientific Research and Development (ijtsrd), ISSN: 2456-6470, Volume-3 | Issue-5 , August 2019, URL: https://www.ijtsrd.com/papers/ijtsrd26730.pdf Paper URL: https://www.ijtsrd.com/physics/atomic-physics/26730/study-on-the-energy-level-splitting-of-the-francium-atom-fr-in-an-external-magnetic-field/win-moe-thant
- The document discusses molecular orbital theory, which describes chemical bonding through the combination of atomic orbitals into molecular orbitals.
- Key features include molecular orbitals being formed from linear combinations of atomic orbitals, with bonding, antibonding, and nonbonding molecular orbitals resulting. Electrons fill these orbitals based on orbital energy.
- The formation of molecular orbitals from atomic orbitals of hydrogen is used as an example, with bonding and antibonding molecular orbitals illustrated.
Molecular orbital theory provides an approach to calculate molecular orbitals through a variational method. This involves taking linear combinations of atomic orbitals to form molecular orbitals. Electrons occupy these molecular orbitals according to certain rules. The molecular orbital theory can explain properties such as why some molecules are paramagnetic that valence bond theory cannot. Calculating molecular orbitals variationally involves using trial wave functions in the Schrodinger equation to find the lowest possible energy state.
This document provides an overview of molecules, atoms, and nuclei from a quantum physics perspective. It describes:
1) How molecules are formed from atoms bonding together and the sizes of molecules, atoms, and nuclei differ in orders of magnitude.
2) How quantum mechanics is used to describe atoms like hydrogen and the allowed energy levels and probability distributions of electrons.
3) Additional concepts like an atom's spin, spin-orbit interaction, and the need for symmetric/antisymmetric wavefunctions for indistinguishable particles in multielectron atoms.
Matter antimatter - an accentuation-attrition modelAlexander Decker
1) The document discusses a model of matter and antimatter interaction where antimatter dissipates matter and vice versa, reaching an equilibrium.
2) It suggests antimatter may be an integral part of electromagnetism and could explain galaxy rotation curves if antimatter constitutes dark matter.
3) However, most scientists believe dark matter is not antimatter since their annihilation would produce bursts of energy not observed.
Applied Chemistry, atomic and molecular structure, part 1, by Shiraz mahbob PhDMaqsoodAhmadKhan5
applied chemistry lecture and slide,
Applied Chemistry, atomic and molecular structure, part 1, by Shiraz mahbob PhD, lecturer in chemistry in pakistan institute of engineering and applied sciences
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Gough plus bara atom model september 2007
1.
2. Super-resonance Model of Valence Bond
• Yuri Magarshak Electron-Nucleon Resonance Model of Valence Bond
http://theor.jinr.ru/~vinitsky/Magarshak.pdf Biophyzika, to appear
• F.Bogomolov Y.Magarshak Chemical Elements as the States of I-particle
Scientific Israel-Technological Advantages, vol 8, issue 3-4, 2007, to appear.
• Y.Magarshak, Resonance Atom Model and the Formation of Valence Bonds;
Scientific Israel-Technological Advantages, vol 8, issue 3-4, 2007, to appear.
• F.Bogomolov, Y.Magarshak, On commuting operators related to asymptotic
symmetries in the atomic theory; Scientific Israel-Technological
Advantages, vol 8, issues 1-2, pp. 161-165 (2006)
• Y.Magarshak, "Four-Dimensional Pyramidal Structure of the Periodic
Properties of Atoms and Chemical Elements", Scientific Israel -
Technological Advantages vol. 7, No.1,2 , pp. 134-150 (2006)
• Yu. Magarshak, J.Malinsky,"A Three-Dimensional Periodic Table ", Nature,
vol.360: 113-114 (1992).
72. The set of atomic electron configurations can be structured
in two systems of coordinates (n, l) and (n + l, n – l), which are
rotated by an angle of /4 in the plane of the principal and
orbital quantum numbers. This property of the system is not
trivial. A question of under which conditions a physical
system (and the corresponding differential equations and
Hamiltonians describing it) has two coexisting symmetries
that do not asymptotically displace one another in the t
limit seems to be very important. When searching for an
answer to this question, it was proved that, for two
symmetries to coexist in the system described by
differential equations (and/or by Hamiltonians), operators
generating these symmetries must commute with one
another.
73. Let the structures and symmetries that are described above and shown
in Fig. 1 be generated by a pair of Hamiltonian-type operators, which
naturally appear in the presence of two commutative Lie symmetry
algebras in the quantum system. From the existence of simple
commutative Lie symmetry algebras in a physical problem, it follows
the existence of a single commuting pair of energy-type operators for
localized quantum states.
Let us consider a finite-dimensional complex representation of the
product of semisimple Lie algebras. Any such representation V of
g1
g2
decomposes into a direct sum of tensor products Vk
Wj
where Vk
are irreducible representations of g1
and Wj
are representations of g2
.
Theorem: Assume that g1
,g2
are simple Lie algebras. Then there is a
canonically defined pair of commuting operators 1
, 2
such that both
i
, i=1,2 commute also with the action of g1
,g2
and have integer
nonnegative eigenvalues on V.
74. Note that the above decomposition may exist in the compexification of
the symmetry algebra and not in the algebra itself. Since finite-
dimensional representations of the complexified Lie algebra are the same
as of it's real form and the above decomposition holds anyway. In our
application the complexification of both real algebras are presumably
isomoprhic to so(3,C)= sl(2,C) after a complexification and hence have
rank 1. Thus there are two natural options:
1) both algebras are coming from the independent rotation invariance of
both the nucleus and the electron envelope.
2) the local symmetry group is the Lorentz group SO(3,1) and
though it's Lie algebra so(3,1) has no such a decompostion but the
complexification so(3,1) x C = sl(2,C) + sl(2,C).
The actual Hamiltonian operator of the problem splits into a sum of
two commuting energy time operators.
In our opinion second case is physically more plausible
75. How could such a symmetry appear in reality? Currently the standard
answer to such question is symmetry break. Namely the existence of
symmetry within an ensemble of different particles is usually explained
by considering them as different states of an "ideal object" with the
above symmetry so that the particles are degenerate states of the above
object where the symmetry is broken due to some process of natural
degeneration.
If we try to apply similar explanation we are brought to the idea to view
the atom as one of the possible states of an ideal particle which we will
be denoting as I-particle. This particle has Lorentz symmetry algebra
within a bigger algebra of local symmetries and supersymmetries
corresponding to other potential fields. The I-particle exists in this
ideal state only 0-time which in practice means a very short time
depending on the total energy of the I-particle according to the
"uncertainty principle". While degenerating the I-particle creates an
avalanche of intermediate particles which retain only pieces of the
initial symmetry but previous symmetry is manifested in the set of
possible degenerate states.
76. The energy dissipation in Hamilton formalism is absent.
The most of the molecular-biological processes are non-ergodic and non-
reversible.
As has been shown by Gribov, Schrodinger equation is not applicable on
nonadiabatic (diabatic) processes in chemistry and molecular biology, in which
precise rather than average values of variables are substantial.
The presence of the dynamics of valence bonds (polar <–> covalent,
ion <–> covalent) in the femto second range.
The number of atoms, which can be connected with the central atom in the
coordination compounds, can be as large as 12
Hidden symmetries. In particular, the presence of two symmetries on the plane
of the principal and orbital quantum numbers, rotated relative to each other by
/4. As has been shown above, in this case one needs two commutative
operators.
77. To the Problem of Formulation of Basic Principles
in the Theory of the Molecular Structure and Dynamics
L. A. Gribov (Institute of Geochemistry and Analytical
Chemistry, Russian Academy of Science, Moscow)
Y. B. Magarshak (MathTech, Inc., New York)
It has been shown that the separation of electronic and nuclear
parts in nuclear-electronic problem of quantum chemistry can
be performed in the adiabatic approximation only. The
Schrödinger equation with the stationary operator , common
for all isomers of any molecule, can not be written as well.
ˆ
enH
78.
79.
80.
81.
82.
83. RESONANT ATOM MODEL.
Postulate 1: In atoms there are no stationary electronic states.
Postulate 2.All electrons, which constitute the shell of the atom, are
involved in the process with the following basic steps (collectively
called resonant path):
(i) The -capture of a shell electron by atom nuclei.
(ii) Proton-Electron Neutron resonance interaction (epn-
resonance) of the shell electron with the proton of the nucleus:
e + p n
(iii) -release of the electron from the nuclei and its return to
(iv) nonlocalized -state in the shell.
Postulate 3. The physical nature of -shell electron capture by
nuclei, and -electron release from nuclei, is not the same.
-capture takes place due to the overlap of the electronic -
function with the volume occupied by atom nuclei.
-release of the electron from nuclei is possible only at
84. SUPERRESONANT NATURE OF THE VALENCE BOND
Postulate 1. In the valence interaction between the atoms in a
molecule, an electron on the shell of one of the atoms is involved in
the epn-resonant interaction with a proton in the nucleus of another
atom.
Postulate 2. A valence bond is formed due to jumps of the electron of
the shell between the nuclei connected by the valence bond, and each
of jumps to a certain nucleus is of epn-resonance nature.
Postulate 3. In molecules consisting of more than two atoms,
resonances between resonances can occur. The number of the
hierarchical levels of resonances in nature is unlimited.
85. HISTORY OF THE DEVELOPMENT OF
REPRESENTATIONS OF THE NATURE
OF THE VALENCE BOND
Walter Heitler and Fritz London were the first physicists who applied
the principles of quantum mechanics to determine the nature of the
chemical bond in the hydrogen molecule. According to their model,
when atoms approach each other, a negatively charged electron of one
atom is attracted to the positive nucleus of another atom due to the
Heisenberg exchange energy. As a result, beginning with a certain
distance between the atoms, electrons oscillate between the nuclei of the
atoms. Thus, according to the model, electrons in the hydrogen molecule
belong to both atoms, forming the valence bond, whose length and
energy are calculated from the Schrodinger equation.
In 1928, London applied an approach based on the Heisenberg
exchange energy to H3
triatomic molecule. He showed that electrons in
this case also oscillate between the nuclei. In the next several years,
Polanyi and Wigner [18] and Henry Eyring and Michael Polanyi
formulated transition-state theory.
86.
87. In the standard model, the explanation of the coordination
numbers is artificial. In the super-resonant (Bara)-atom model
the explanation is natural. Electron has sufficient time to be
connected with several atoms in a sequence.
88. Diabatic (non-a-diabatic) problems
in the super resonant model.
As has been shown by Gribov, in nonadiabatic (diabatic)
systems one can not separate the calculation of electonic
configuration from the motion of nucleus. The Schrodinger
equation gives average values (in particular, the agerage
energy). The presence of epn-interactions (Bara model) can
provide exact values and is applicable to diabatic (non-a-
diabatic) systems.
89.
90.
91.
92. Superconductivity in Bara atom model
Accoridng to Bara atom model, atoms, which constitute the
molecules, at absolute zero temperature continue to oscillate because
of bara interactions between nucleus of atoms, connected by valence
bonds.
Traditional explanation of the superconductivity: Cooper pair of
electrons travels from atom to atom. In Bara model, the Cooper
pair is traveling from nucleus to nucleus.
93.
94. The entropy increase and energy dissipation
In Bara Atom Model.
The entropy of closed quantum mechanical systems can not increase
(Von Neumann theorem), whereas all real processes dissipate.
In statistical mechanics, as a rule, the entropy of the nucleus is not taken
into account. The barrier between the nucleus, in which protons and
electrons are moving with speeds > 50,000 km/c, and the motion of
atoms in gases and solids (at room temperature in the range <1 km/c) is
infinitely large. To the contrary, in the Bara atom model, the reason of
the entropy increase is the finiteness of the barrier between the motion
of nuclons in the nucleus and the motion of atoms in 3D space. The
reversibility in time (which follows both from Newtonian and
Hamiltonian formalisms), in the Bara atom model disappears. The
entropy increase and energy dissipation in closed systems is a natural
consequence of the Bara model postulates.
95.
96.
97.
98.
99.
100.
101. Conclusions
•Bara atom model explains why the number of neutrons in any
atom, which do have neutrons in the nucleus, is larger or equal than the
number of protons.
•Bara atom model identifies Cooper pair with Pauli pair of electrons with
opposite spines. In contrast to the standard model, Bara amom mdel
suggests that Cooper pair travels from nucleus to nucleus.
• Bara atom model explains entropy increase and dissipation of energy
by finiteness of the entropy barrier between the nucleus of different
atoms.
•Bara atom model considers cooper pairs, subshells and shells as quasi
particles, generated in the atom nucleus and related to the shell structure
of atom nucleus.
•Bara atom model predicts zero temperature oscillations of molecules
and explains low temperature superconductivity by traveling of Cooper
electron pair (Pauli orbital) from nucleus to nucleus.
•Bara atom model explains coordination bonds and resonance bonds in
chemistry.