- J.J. Thomson's plum pudding model of the atom was modified based on evidence from experiments by Rutherford, Geiger, Marsden, and Bohr.
- In the gold foil experiment, Geiger and Marsden observed some alpha particles deflected at high angles from a thin gold foil, inconsistent with Thomson's model but evidence for a small, dense nucleus.
- Bohr incorporated Planck's quantum theory to explain the stability of atoms, suggesting electrons occupy discrete energy levels and jump between them.
The document summarizes the development of atomic theory over time through the contributions of several scientists. Democritus first proposed that all matter is composed of invisible particles called atoms. John Dalton viewed atoms as tiny spheres and discovered their relative masses. J.J. Thomson discovered electrons and evidence that something smaller than atoms exists. Ernest Rutherford determined that atoms have a small, dense nucleus containing their mass. Later models incorporated electrons orbiting the nucleus in certain orbits by Bohr and Schrodinger viewed them as waves within layers. James Chadwick discovered neutrons, completing the modern atomic model.
The atomic theory has evolved over time based on new discoveries. Early philosophers proposed that all matter is made of indivisible particles called atoms. In the early 1800s, scientists proposed that atoms of different elements have distinct properties and combine in fixed ratios. At the turn of the 20th century, experiments revealed internal structures of atoms including electrons, protons, and nuclei. Later work determined the composition and arrangement of these subatomic particles, leading to modern atomic theory that atoms are made of protons, neutrons, and electrons with electrons orbiting the nucleus.
The document discusses the history and development of atomic models from ancient Greek philosophers to modern scientific theories. It describes Democritus' idea that atoms are the smallest indivisible particles of matter. John Dalton proposed his atomic theory that all matter is composed of atoms of different elements that combine in fixed ratios. J.J. Thomson's experiments provided evidence that atoms contain smaller charged particles, leading to his "chocolate chip" atomic model. Finally, Rutherford discovered the atomic nucleus by observing alpha particle scattering, realizing that the positive charge and mass of atoms are concentrated in a tiny nucleus.
The document traces the history and development of atomic models from ancient Greek philosophers to modern quantum theory. It describes Democritus's early idea of indivisible atoms, followed by John Dalton formalizing the first atomic theory in the early 1800s. J.J. Thomson later discovered the electron and proposed that atoms are like "plum puddings" with positive matter and embedded electrons. Ernest Rutherford's gold foil experiment revealed that atoms have a small, dense positive nucleus, leading Niels Bohr to model electrons orbiting the nucleus in fixed shells. Modern quantum theory describes electrons as occupying probability clouds or orbitals around the nucleus.
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
The document provides a timeline of important discoveries and developments in the understanding of the atom from ancient Greek philosophers Democritus and Aristotle up to the early 20th century. It describes key contributions such as Democritus' idea that all matter is made of indivisible atoms, Dalton introducing atomic theory in 1802, Mendeleev organizing the periodic table in 1869, Thomson discovering the electron in 1897, Rutherford proposing the nuclear model of the atom in 1911, and Moseley ordering the elements by atomic number in 1913.
The Historical Development of Atomic ModelsDhen Bathan
The document traces the historical development of atomic models from ancient Greek philosophers Democritus and Leucippus proposing the first idea of atoms, to J.J. Thomson discovering the electron in 1903 and proposing atoms have a positively-charged sphere with electrons embedded, to Rutherford discovering the proton in 1911 and proving atoms have a nucleus, to Bohr solving problems with his 1913 model of electrons moving in shells around the nucleus, to Chadwick discovering the neutron in 1932 and establishing the modern nuclear model of the atom with protons and neutrons in the nucleus surrounded by electrons.
The document summarizes the development of atomic theory over time through the contributions of several scientists. Democritus first proposed that all matter is composed of invisible particles called atoms. John Dalton viewed atoms as tiny spheres and discovered their relative masses. J.J. Thomson discovered electrons and evidence that something smaller than atoms exists. Ernest Rutherford determined that atoms have a small, dense nucleus containing their mass. Later models incorporated electrons orbiting the nucleus in certain orbits by Bohr and Schrodinger viewed them as waves within layers. James Chadwick discovered neutrons, completing the modern atomic model.
The atomic theory has evolved over time based on new discoveries. Early philosophers proposed that all matter is made of indivisible particles called atoms. In the early 1800s, scientists proposed that atoms of different elements have distinct properties and combine in fixed ratios. At the turn of the 20th century, experiments revealed internal structures of atoms including electrons, protons, and nuclei. Later work determined the composition and arrangement of these subatomic particles, leading to modern atomic theory that atoms are made of protons, neutrons, and electrons with electrons orbiting the nucleus.
The document discusses the history and development of atomic models from ancient Greek philosophers to modern scientific theories. It describes Democritus' idea that atoms are the smallest indivisible particles of matter. John Dalton proposed his atomic theory that all matter is composed of atoms of different elements that combine in fixed ratios. J.J. Thomson's experiments provided evidence that atoms contain smaller charged particles, leading to his "chocolate chip" atomic model. Finally, Rutherford discovered the atomic nucleus by observing alpha particle scattering, realizing that the positive charge and mass of atoms are concentrated in a tiny nucleus.
The document traces the history and development of atomic models from ancient Greek philosophers to modern quantum theory. It describes Democritus's early idea of indivisible atoms, followed by John Dalton formalizing the first atomic theory in the early 1800s. J.J. Thomson later discovered the electron and proposed that atoms are like "plum puddings" with positive matter and embedded electrons. Ernest Rutherford's gold foil experiment revealed that atoms have a small, dense positive nucleus, leading Niels Bohr to model electrons orbiting the nucleus in fixed shells. Modern quantum theory describes electrons as occupying probability clouds or orbitals around the nucleus.
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
The document provides a timeline of important discoveries and developments in the understanding of the atom from ancient Greek philosophers Democritus and Aristotle up to the early 20th century. It describes key contributions such as Democritus' idea that all matter is made of indivisible atoms, Dalton introducing atomic theory in 1802, Mendeleev organizing the periodic table in 1869, Thomson discovering the electron in 1897, Rutherford proposing the nuclear model of the atom in 1911, and Moseley ordering the elements by atomic number in 1913.
The Historical Development of Atomic ModelsDhen Bathan
The document traces the historical development of atomic models from ancient Greek philosophers Democritus and Leucippus proposing the first idea of atoms, to J.J. Thomson discovering the electron in 1903 and proposing atoms have a positively-charged sphere with electrons embedded, to Rutherford discovering the proton in 1911 and proving atoms have a nucleus, to Bohr solving problems with his 1913 model of electrons moving in shells around the nucleus, to Chadwick discovering the neutron in 1932 and establishing the modern nuclear model of the atom with protons and neutrons in the nucleus surrounded by electrons.
The document discusses the history and development of atomic theory from Democritus' idea that matter is made of indivisible particles called atoms to modern atomic theory. Some key points are: Democritus first proposed atoms in ancient Greece; Dalton established his atomic theory in 1807 stating atoms are identical for each element and different between elements; Rutherford discovered the dense positively charged nucleus through his gold foil experiment in 1909; and Bohr incorporated electrons orbiting the nucleus in specific energy levels in 1913.
1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
1. J.J. Thomson discovered electrons in cathode ray tubes and concluded they were negatively charged particles smaller than atoms.
2. In the gold foil experiment, Rutherford expected alpha particles to pass through or be slightly deflected, but some were deflected at large angles or rebounded, indicating the positive charge was concentrated in a small nucleus.
3. This led Rutherford to propose the nuclear model of the atom with electrons orbiting a small, dense positively charged nucleus.
The document summarizes the history of atomic structure models from Thomson's "plum pudding" model to Bohr's model. It describes key scientists' contributions, including:
- Thomson's discovery of the electron and proposal that atoms contain positive charge with electrons distributed throughout
- Rutherford's gold foil experiment which led him to propose a small, dense nucleus with electrons in orbits around it
- Bohr's refinement incorporating quantum theory, explaining electron energy levels and spectral lines
Dalton's atomic theory proposed that matter is made of small indivisible particles called atoms, atoms of the same element are identical, and atoms of different elements have different masses and properties. Rutherford discovered the nucleus of the atom through his gold foil experiment, finding that some alpha particles bounced off the small, dense nucleus at the center of the atom. Chadwick discovered the neutron through experiments with excessively charged atoms, an uncharged particle that helped explain nuclear structure.
Atomic Theory Timeline Kyle, Justin, Mikekllrupp68
- Democritus first proposed the theory of materialism, that everything is composed of indivisible atoms. Antoine Lavoisier established the law of conservation of mass in 1789, stating that matter can be rearranged but not created or destroyed in chemical reactions. John Dalton created the first tables of relative atomic mass and established the law of definite proportions in 1805.
The document summarizes the major historical theories and models of the atom. It describes how ancient Greek philosophers first proposed the idea of indivisible atoms. In the early 1900s, scientists including J.J. Thomson, Ernest Rutherford, Niels Bohr, and Erwin Schrödinger developed models of the internal structure of atoms. Thomson's plum pudding model depicted atoms as positively charged spheres containing electrons. Rutherford's gold foil experiment led to the planetary model with a small, dense nucleus surrounded by orbiting electrons. Bohr added that electrons can only orbit in fixed energy levels. Later, Schrödinger developed the probabilistic cloud model still used today.
Democritus first proposed the existence of atoms in 460 BC, though the atomic theory was not widely accepted until John Dalton proposed it in 1803 based on the laws of multiple and constant proportions. The discovery of subatomic particles like the electron by J.J. Thomson in 1897 and proton by Rutherford in 1911 led to proposed atomic models like the plum pudding model and nuclear atom. Defining the mass and charge of these particles along with isotopes observed by Francis Aston and the neutron discovered by James Chadwick in 1932 completed the basic components of the modern atomic theory.
Physical science 4.1 : Development of Atomic TheoryChris Foltz
Democritus was one of the first to propose the idea of atoms in 440 BCE, suggesting that matter is made up of tiny indivisible particles called atoms. In the early 1900s, experiments led scientists to develop more accurate models of the atom. Rutherford discovered the nucleus in 1909 by firing positively charged particles at a gold foil and observing some particles deflecting, indicating a small, dense nucleus. Bohr then proposed in 1913 that electrons orbit the nucleus in distinct energy levels. The modern atomic theory describes the regions where electrons are likely to be found as electron clouds.
Ancient Greek philosophers proposed early models of atoms as fundamental elements like earth, air, fire and water. In the 17th century, Robert Boyle questioned these models and advocated experimentation over philosophy. John Dalton proposed atoms as indivisible, identical spheres that combine to form compounds. J.J. Thompson's "plum pudding" model depicted atoms as positive and negative charges. However, experiments by Ernest Rutherford, Hans Geiger and Ernest Marsden found most alpha particles passed through a gold foil with few deflected, leading Rutherford to propose the planetary model of a small, dense nucleus surrounded by electrons. Later, Henry Moseley arranged elements by atomic number, James Chadwick discovered the neutral neutron in the
1. The ancient Greek philosophers Empedocles and Democritus proposed early atomic theories, believing that all matter was made up of indivisible particles called atoms.
2. In the early 1900s, scientists such as Rutherford, Thomson, and Chadwick discovered the internal structure of atoms through experiments, finding that atoms consist of a small, dense nucleus surrounded by electrons.
3. Niels Bohr contributed to the modern atomic model in 1913 by proposing that electrons orbit the nucleus in fixed shells or energy levels.
1. The document outlines the development of atomic models from Dalton's atomic theory in 1803 to the quantum model in 1924. It describes key contributors including Dalton, Thomson, Millikan, Rutherford, Bohr, de Broglie, Schrodinger, and Born and their major discoveries.
2. Major milestones included Dalton establishing atoms as the basic unit of matter, Thomson discovering the electron, Rutherford discovering the nucleus, Bohr explaining electron energy levels, and the development of the quantum model explaining wave-particle duality of electrons.
3. Each new model built upon the previous work and corrected limitations, moving science closer to a full understanding of atomic structure.
This document discusses the atomic theory and properties of the three states of matter. It covers key scientists and their contributions, including Dalton formulating the atomic theory, Thomson discovering the electron, Rutherford naming the types of radiation, and Bohr proposing electron orbitals. The three states of matter - solid, liquid, gas - are compared in terms of particle motion and forces. Phase changes like melting, freezing and evaporation are explained. The development of the modern atomic model and discovery of subatomic particles like the proton and neutron are also summarized.
Democritus first proposed the idea of atoms as indivisible particles in 460 BC. John Dalton updated atomic theory in 1803, proposing that atoms of each element are identical and that chemical reactions involve combinations of atoms. J.J. Thomson discovered electrons in 1897, changing the model to include negatively charged electrons orbiting the atom's nucleus. Ernest Rutherford discovered the nucleus through alpha particle scattering experiments in 1911. Niels Bohr incorporated quantum theory in 1913, proposing electrons orbit in discrete energy levels. Erwin Schrodinger modeled electrons as probability clouds in 1926. James Chadwick discovered neutrons in 1932, completing the standard nuclear model.
Historical Development of Atomic Theorybill_wallace
The document summarizes the historical development of atomic theory from ancient Greece to the early 20th century. It describes the early ideas of Democritus and Aristotle, followed by John Dalton's atomic theory in the early 1800s which proposed that all matter is made up of atoms. It then discusses J.J. Thomson's discoveries of the electron using Crookes tubes and his "plum pudding" model of the atom. Finally, it outlines Ernest Rutherford's refinement of the atomic model through his gold foil experiment and discovery of the nucleus, and the later quantum mechanical model including the discovery of the neutron by James Chadwick.
- Democritus and Leucippus were ancient Greek philosophers who proposed the idea of atoms as indivisible and indestructible particles that all matter is composed of. They hypothesized that atoms come in different shapes and sizes and exist in empty space between them.
- John Dalton further developed atomic theory in 1804, proposing that atoms of a given element are identical and have fixed properties, while atoms of different elements have different properties and combine in simple whole number ratios.
- In the late 19th/early 20th century, experiments by Thomson, Rutherford, Bohr, Einstein, and Moseley revealed the internal structure of atoms, including the existence of electrons, photons, and that atoms have a
The document outlines the major theories in the development of atomic theory from ancient Greece to the 20th century. It describes the key contributors including:
Democritus who proposed that all matter is made of basic elements composed of indivisible atoms. John Dalton introduced the modern concept of atoms as basic units of elements that combine in fixed ratios. J.J. Thompson discovered the electron and proposed the plum pudding model where electrons are distributed in a positive charge. Ernest Rutherford discovered the nucleus through alpha particle experiments and proposed atoms have a small, dense positively charged nucleus. Niels Bohr incorporated quantum theory and proposed electrons orbit in fixed shells around the nucleus. Finally, Schrodinger and Heisenberg developed the quantum
This document provides an overview of atomic theory and the laws of chemical combination. It discusses the early Greek philosophers' debates on the nature of matter and whether it is continuous or made of discrete particles. John Dalton developed the modern atomic theory in the early 19th century, which included five main points. The document outlines the contributions of scientists like Thomson, Rutherford, and Bohr to models of atomic structure. It describes the three states of matter and defines the fundamental laws of conservation of mass, definite proportions, and multiple proportions discovered by scientists like Lavoisier, Proust, and Dalton. Examples are provided to illustrate applications of these laws.
John Dalton proposed the first atomic theory in the early 19th century, which stated that atoms are indivisible and identical for each element. JJ Thomson later discovered the electron using a cathode ray tube, showing that atoms have internal structure. His "plum pudding" model depicted electrons distributed throughout the atom. Rutherford's gold foil experiment revealed that atoms have a small, dense nucleus at their center. Bohr then proposed that electrons orbit the nucleus in distinct energy levels.
The document discusses the history and development of atomic theory from ancient Greek philosophers like Democritus and Leucippus, who first proposed the idea of indivisible particles called atoms, to modern scientists like Dalton, Thomson, Rutherford, and Bohr who contributed key discoveries and models that led to our current understanding. It explains concepts like atoms, elements, isotopes, atomic number, atomic mass, ions, and different atomic models including the plum pudding model, Bohr model, and electron cloud model.
Atomic Models: Everything You Need to Knowjane1015
The document traces the development of atomic models from ancient Greek philosophers to modern quantum mechanics. It describes early ideas that atoms were indivisible spheres (Democritus), John Dalton's model of atoms as hard spheres, J.J. Thomson's "plum pudding" model with electrons in a positively charged substance, Ernest Rutherford's discovery of the nucleus from his gold foil experiment, Niels Bohr's model with electrons in specific energy levels around the nucleus, and the modern wave model where electrons exist as probability clouds.
The document traces the history of atomic models from ancient Greek philosophers to modern quantum mechanics. It describes key experiments and findings that led scientists like Dalton, Thomson, Rutherford, Bohr, and Schrödinger to develop successively more accurate models of the atom. Dalton proposed atoms as indivisible particles, Thomson discovered electrons within the atom, Rutherford found the dense nucleus through gold foil experiments, Bohr incorporated electron orbits, and Schrödinger introduced the wave-like electron cloud model still used today.
The document discusses the history and development of atomic theory from Democritus' idea that matter is made of indivisible particles called atoms to modern atomic theory. Some key points are: Democritus first proposed atoms in ancient Greece; Dalton established his atomic theory in 1807 stating atoms are identical for each element and different between elements; Rutherford discovered the dense positively charged nucleus through his gold foil experiment in 1909; and Bohr incorporated electrons orbiting the nucleus in specific energy levels in 1913.
1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
1. J.J. Thomson discovered electrons in cathode ray tubes and concluded they were negatively charged particles smaller than atoms.
2. In the gold foil experiment, Rutherford expected alpha particles to pass through or be slightly deflected, but some were deflected at large angles or rebounded, indicating the positive charge was concentrated in a small nucleus.
3. This led Rutherford to propose the nuclear model of the atom with electrons orbiting a small, dense positively charged nucleus.
The document summarizes the history of atomic structure models from Thomson's "plum pudding" model to Bohr's model. It describes key scientists' contributions, including:
- Thomson's discovery of the electron and proposal that atoms contain positive charge with electrons distributed throughout
- Rutherford's gold foil experiment which led him to propose a small, dense nucleus with electrons in orbits around it
- Bohr's refinement incorporating quantum theory, explaining electron energy levels and spectral lines
Dalton's atomic theory proposed that matter is made of small indivisible particles called atoms, atoms of the same element are identical, and atoms of different elements have different masses and properties. Rutherford discovered the nucleus of the atom through his gold foil experiment, finding that some alpha particles bounced off the small, dense nucleus at the center of the atom. Chadwick discovered the neutron through experiments with excessively charged atoms, an uncharged particle that helped explain nuclear structure.
Atomic Theory Timeline Kyle, Justin, Mikekllrupp68
- Democritus first proposed the theory of materialism, that everything is composed of indivisible atoms. Antoine Lavoisier established the law of conservation of mass in 1789, stating that matter can be rearranged but not created or destroyed in chemical reactions. John Dalton created the first tables of relative atomic mass and established the law of definite proportions in 1805.
The document summarizes the major historical theories and models of the atom. It describes how ancient Greek philosophers first proposed the idea of indivisible atoms. In the early 1900s, scientists including J.J. Thomson, Ernest Rutherford, Niels Bohr, and Erwin Schrödinger developed models of the internal structure of atoms. Thomson's plum pudding model depicted atoms as positively charged spheres containing electrons. Rutherford's gold foil experiment led to the planetary model with a small, dense nucleus surrounded by orbiting electrons. Bohr added that electrons can only orbit in fixed energy levels. Later, Schrödinger developed the probabilistic cloud model still used today.
Democritus first proposed the existence of atoms in 460 BC, though the atomic theory was not widely accepted until John Dalton proposed it in 1803 based on the laws of multiple and constant proportions. The discovery of subatomic particles like the electron by J.J. Thomson in 1897 and proton by Rutherford in 1911 led to proposed atomic models like the plum pudding model and nuclear atom. Defining the mass and charge of these particles along with isotopes observed by Francis Aston and the neutron discovered by James Chadwick in 1932 completed the basic components of the modern atomic theory.
Physical science 4.1 : Development of Atomic TheoryChris Foltz
Democritus was one of the first to propose the idea of atoms in 440 BCE, suggesting that matter is made up of tiny indivisible particles called atoms. In the early 1900s, experiments led scientists to develop more accurate models of the atom. Rutherford discovered the nucleus in 1909 by firing positively charged particles at a gold foil and observing some particles deflecting, indicating a small, dense nucleus. Bohr then proposed in 1913 that electrons orbit the nucleus in distinct energy levels. The modern atomic theory describes the regions where electrons are likely to be found as electron clouds.
Ancient Greek philosophers proposed early models of atoms as fundamental elements like earth, air, fire and water. In the 17th century, Robert Boyle questioned these models and advocated experimentation over philosophy. John Dalton proposed atoms as indivisible, identical spheres that combine to form compounds. J.J. Thompson's "plum pudding" model depicted atoms as positive and negative charges. However, experiments by Ernest Rutherford, Hans Geiger and Ernest Marsden found most alpha particles passed through a gold foil with few deflected, leading Rutherford to propose the planetary model of a small, dense nucleus surrounded by electrons. Later, Henry Moseley arranged elements by atomic number, James Chadwick discovered the neutral neutron in the
1. The ancient Greek philosophers Empedocles and Democritus proposed early atomic theories, believing that all matter was made up of indivisible particles called atoms.
2. In the early 1900s, scientists such as Rutherford, Thomson, and Chadwick discovered the internal structure of atoms through experiments, finding that atoms consist of a small, dense nucleus surrounded by electrons.
3. Niels Bohr contributed to the modern atomic model in 1913 by proposing that electrons orbit the nucleus in fixed shells or energy levels.
1. The document outlines the development of atomic models from Dalton's atomic theory in 1803 to the quantum model in 1924. It describes key contributors including Dalton, Thomson, Millikan, Rutherford, Bohr, de Broglie, Schrodinger, and Born and their major discoveries.
2. Major milestones included Dalton establishing atoms as the basic unit of matter, Thomson discovering the electron, Rutherford discovering the nucleus, Bohr explaining electron energy levels, and the development of the quantum model explaining wave-particle duality of electrons.
3. Each new model built upon the previous work and corrected limitations, moving science closer to a full understanding of atomic structure.
This document discusses the atomic theory and properties of the three states of matter. It covers key scientists and their contributions, including Dalton formulating the atomic theory, Thomson discovering the electron, Rutherford naming the types of radiation, and Bohr proposing electron orbitals. The three states of matter - solid, liquid, gas - are compared in terms of particle motion and forces. Phase changes like melting, freezing and evaporation are explained. The development of the modern atomic model and discovery of subatomic particles like the proton and neutron are also summarized.
Democritus first proposed the idea of atoms as indivisible particles in 460 BC. John Dalton updated atomic theory in 1803, proposing that atoms of each element are identical and that chemical reactions involve combinations of atoms. J.J. Thomson discovered electrons in 1897, changing the model to include negatively charged electrons orbiting the atom's nucleus. Ernest Rutherford discovered the nucleus through alpha particle scattering experiments in 1911. Niels Bohr incorporated quantum theory in 1913, proposing electrons orbit in discrete energy levels. Erwin Schrodinger modeled electrons as probability clouds in 1926. James Chadwick discovered neutrons in 1932, completing the standard nuclear model.
Historical Development of Atomic Theorybill_wallace
The document summarizes the historical development of atomic theory from ancient Greece to the early 20th century. It describes the early ideas of Democritus and Aristotle, followed by John Dalton's atomic theory in the early 1800s which proposed that all matter is made up of atoms. It then discusses J.J. Thomson's discoveries of the electron using Crookes tubes and his "plum pudding" model of the atom. Finally, it outlines Ernest Rutherford's refinement of the atomic model through his gold foil experiment and discovery of the nucleus, and the later quantum mechanical model including the discovery of the neutron by James Chadwick.
- Democritus and Leucippus were ancient Greek philosophers who proposed the idea of atoms as indivisible and indestructible particles that all matter is composed of. They hypothesized that atoms come in different shapes and sizes and exist in empty space between them.
- John Dalton further developed atomic theory in 1804, proposing that atoms of a given element are identical and have fixed properties, while atoms of different elements have different properties and combine in simple whole number ratios.
- In the late 19th/early 20th century, experiments by Thomson, Rutherford, Bohr, Einstein, and Moseley revealed the internal structure of atoms, including the existence of electrons, photons, and that atoms have a
The document outlines the major theories in the development of atomic theory from ancient Greece to the 20th century. It describes the key contributors including:
Democritus who proposed that all matter is made of basic elements composed of indivisible atoms. John Dalton introduced the modern concept of atoms as basic units of elements that combine in fixed ratios. J.J. Thompson discovered the electron and proposed the plum pudding model where electrons are distributed in a positive charge. Ernest Rutherford discovered the nucleus through alpha particle experiments and proposed atoms have a small, dense positively charged nucleus. Niels Bohr incorporated quantum theory and proposed electrons orbit in fixed shells around the nucleus. Finally, Schrodinger and Heisenberg developed the quantum
This document provides an overview of atomic theory and the laws of chemical combination. It discusses the early Greek philosophers' debates on the nature of matter and whether it is continuous or made of discrete particles. John Dalton developed the modern atomic theory in the early 19th century, which included five main points. The document outlines the contributions of scientists like Thomson, Rutherford, and Bohr to models of atomic structure. It describes the three states of matter and defines the fundamental laws of conservation of mass, definite proportions, and multiple proportions discovered by scientists like Lavoisier, Proust, and Dalton. Examples are provided to illustrate applications of these laws.
John Dalton proposed the first atomic theory in the early 19th century, which stated that atoms are indivisible and identical for each element. JJ Thomson later discovered the electron using a cathode ray tube, showing that atoms have internal structure. His "plum pudding" model depicted electrons distributed throughout the atom. Rutherford's gold foil experiment revealed that atoms have a small, dense nucleus at their center. Bohr then proposed that electrons orbit the nucleus in distinct energy levels.
The document discusses the history and development of atomic theory from ancient Greek philosophers like Democritus and Leucippus, who first proposed the idea of indivisible particles called atoms, to modern scientists like Dalton, Thomson, Rutherford, and Bohr who contributed key discoveries and models that led to our current understanding. It explains concepts like atoms, elements, isotopes, atomic number, atomic mass, ions, and different atomic models including the plum pudding model, Bohr model, and electron cloud model.
Atomic Models: Everything You Need to Knowjane1015
The document traces the development of atomic models from ancient Greek philosophers to modern quantum mechanics. It describes early ideas that atoms were indivisible spheres (Democritus), John Dalton's model of atoms as hard spheres, J.J. Thomson's "plum pudding" model with electrons in a positively charged substance, Ernest Rutherford's discovery of the nucleus from his gold foil experiment, Niels Bohr's model with electrons in specific energy levels around the nucleus, and the modern wave model where electrons exist as probability clouds.
The document traces the history of atomic models from ancient Greek philosophers to modern quantum mechanics. It describes key experiments and findings that led scientists like Dalton, Thomson, Rutherford, Bohr, and Schrödinger to develop successively more accurate models of the atom. Dalton proposed atoms as indivisible particles, Thomson discovered electrons within the atom, Rutherford found the dense nucleus through gold foil experiments, Bohr incorporated electron orbits, and Schrödinger introduced the wave-like electron cloud model still used today.
1) The document traces the history of atomic theory from ancient Greece to modern times, starting with Democritus' idea of atoms that was rejected by Aristotle.
2) In the 1600s, chemistry emerged as a science, with Antoine Lavoisier distinguishing elements and compounds. John Dalton further developed atomic theory in 1803, proposing atoms of different elements have different properties.
3) Ernest Rutherford's 1909 gold foil experiment discovered the atomic nucleus, replacing the plum pudding model and showing atoms have mostly empty space. This led to models placing electrons in distinct orbits around the nucleus.
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's model of atoms as indivisible spheres, Thomson's "plum pudding" model with electrons scattered in a positively charged substance, Rutherford's gold foil experiment showing atoms are mostly empty space with a dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus like planets, and the modern wave model where electrons exist as probability clouds rather than definite orbits.
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
The document discusses the historical development of atomic models from Thomson's plum pudding model to Rutherford's nuclear model to Bohr's orbital model. It describes each scientist's key contributions and experimental findings that improved the understanding of atomic structure, such as Thomson discovering the electron, Rutherford showing the small, dense nucleus, and Bohr explaining electron orbitals. The document concludes that chemistry is fundamentally concerned with understanding atomic and molecular interactions and properties.
J.J. Thomson discovered the electron in 1897 through experiments with cathode rays. He proposed the "plum pudding" model of the atom, where electrons were embedded in a uniform sphere of positive charge. Ernest Rutherford performed the gold foil experiment in 1909, which led him to propose the Rutherford model of the atom in 1911 - a small, dense nucleus surrounded by orbiting electrons. Neils Bohr improved on this model in 1913 by incorporating quantum theory, explaining the Rydberg formula for hydrogen spectra. In the Bohr model, electrons orbit in discrete energy levels and jump between them, emitting or absorbing photons of specific frequencies.
The document summarizes the history of atomic theory from ancient Greek philosophers to modern physics. It describes early atomic models proposed by Democritus, Dalton, Thomson, and Rutherford, and refinements made by Bohr and Schrodinger. Key developments include Thomson's discovery of the electron, Rutherford's nuclear model from his gold foil experiment, Bohr incorporating quantum theory and the concept of electron shells, and Schrodinger's probabilistic "cloud" model of electron orbits. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in energy levels.
Contributions of j.j thomas, ernst rutherford and neil bohr in the field of c...Meeran Banday
The document discusses the historical development of atomic models from Thomson's plum pudding model to Rutherford's nuclear model to Bohr's planetary model. It describes key experiments and contributions from Thomson, Rutherford, and Bohr that led to advances in understanding the structure of the atom, including Thomson discovering the electron, Rutherford showing the nucleus, and Bohr incorporating quantum theory. The models progressed from electrons distributed in a positive cloud to orbiting a dense nucleus to orbiting in discrete shells.
This document summarizes the key developments in the models of the atom over time. It discusses early Greek philosophers' idea that matter is made of tiny particles called atoms. John Dalton proposed the first modern atomic theory that atoms are tiny, hard spheres that cannot be divided further. J.J. Thomson discovered the electron through experiments with cathode rays. Rutherford's experiments showed that the atom has a tiny, dense nucleus. Later, the neutron was discovered, completing the nuclear model of the atom.
This power point presentation is created for Science 8 learners. This presentation tackles on the three sub atomic particles of atom, the one who discovers them, how do they discover them and the different atomic theory models.
1. The document discusses the historical development of atomic theory from Democritus' idea of indivisible atoms to the modern atomic model.
2. Key contributors included Dalton who proposed atoms of different elements have different properties, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed the atom has a small, dense nucleus.
3. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in energy levels or an electron cloud. Atoms of the same element can have different numbers of neutrons, known as isotopes.
1. The document discusses the historical development of atomic theory from Democritus' idea of indivisible atoms to the modern atomic model.
2. Key contributors included Dalton who proposed atoms of different elements have different properties, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed the atom's small, dense nucleus.
3. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in regions of probable location called electron clouds.
The document discusses the development of atomic models from ancient Greek philosophers to modern scientific theories. It describes early ideas that matter was made of tiny indivisible particles called atoms. John Dalton proposed the first modern atomic theory in the 1800s, modeling atoms as hard spheres. J.J. Thomson's experiments showed atoms contain negatively charged electrons. Ernest Rutherford's experiments revealed atoms have a small, dense nucleus containing positive charge. Neutrons were later discovered in atomic nuclei. Modern atomic theory pictures electrons in electron clouds surrounding atomic nuclei.
The document traces the development of atomic theory from ancient Greek philosophers to modern physics. Democritus first proposed that matter is made of indivisible "atoms" around 400 BC. In the early 1800s, John Dalton provided experimental evidence supporting atoms and proposed that atoms of different elements have different properties. In the late 1800s and early 1900s, experiments by J.J. Thomson, Ernest Rutherford, and Niels Bohr led to discoveries of the electron and development of the nuclear model of the atom. Today's atomic model is based on quantum mechanics and depicts electrons as existing in electron clouds or energy levels rather than definite orbits.
The document summarizes the development of atomic theory over time from Democritus' idea of indivisible atoms to the current wave model. It describes early atomic models including Democritus, Dalton, Thomson's plum pudding model, Rutherford's gold foil experiment leading to the discovery of the nucleus, and Bohr's model of electrons in orbits around the nucleus. The modern wave model views electrons as existing in electron clouds or orbitals around the nucleus rather than defined orbits.
This document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat is given out to the surroundings, while endothermic reactions absorb heat from the surroundings. The amount of heat given out or absorbed during a reaction is called the enthalpy change. Whether a reaction is exothermic or endothermic depends on whether bond breaking absorbs more energy than bond forming releases, or vice versa.
This chapter discusses rates of reactions. It defines rate of reaction as how fast or slow a reaction is taking place. There are three main ways to measure rate of reaction: measuring time taken for reaction to complete, measuring amount of product formed per unit time, and measuring amount of reactant used up or remaining per unit time. The rate of reaction is affected by several factors like temperature, concentration, particle size, catalyst, and pressure. Temperature has the greatest effect as increasing temperature increases the kinetic energy of particles, leading to more successful collisions. Catalysts are substances that increase reaction rate without being used up in the reaction. They provide alternative reaction pathways or increase surface area for contact between reactants.
C06 concentration of solutions and volumetric analysisChemrcwss
This document provides information on concentration of solutions and volumetric analysis. It defines key terms like solute, solvent, concentrated and dilute solutions. It explains how to calculate concentration in g/dm3 and mol/dm3 and includes examples. The document also describes the process of volumetric analysis including using a pipette and burette accurately. It explains how to perform and record a titration experiment to determine the concentration of an unknown acid solution.
This chapter discusses the mole concept, including defining the mole, deriving empirical and molecular formulas, stating Avogadro's Law, and applying the mole concept to ionic and molecular equations. It introduces the mole as the amount of substance containing 6x1023 particles. It provides examples of how to determine the empirical formula, molecular formula, and formula of a compound from composition data. It also discusses molar volume of gases and limiting reactants. Worked examples are included for many of these concepts.
The document is a chapter about elements and compounds from a chemistry textbook. It contains the following key points in 3 sentences:
The chapter defines elements as substances that cannot be broken down further, while compounds are substances made of two or more elements chemically bonded together. It explains that elements are represented by chemical symbols and compounds by chemical formulas showing the ratios of atoms present. The chapter also discusses writing and balancing chemical equations to represent chemical reactions in terms of reactants and products.
C03 relative masses of atoms and moleculesChemrcwss
The document discusses relative atomic mass and relative molecular mass. It defines relative atomic mass as the average mass of an atom compared to 1/12 the mass of one carbon-12 atom. Relative molecular mass is defined similarly on a molecular level. Examples are provided for calculating relative atomic masses from the periodic table and relative molecular masses by adding atomic masses. Percentage composition, yield, and purity calculations involving relative masses are also illustrated.
This document provides an overview of chemical bonding and macromolecular structures. It discusses the different types of bonds including ionic bonds formed by transfer of electrons between metals and non-metals, and covalent bonds formed by sharing of electrons between non-metals. Ionic compounds have high melting and boiling points and conduct electricity when molten or dissolved, while covalent compounds have low melting and boiling points and do not conduct electricity. It also describes macromolecular and metallic structures, noting that macromolecules have very high melting points due to their large size, while metals form lattice structures with positive ions in a sea of delocalized electrons, making them malleable.
The document discusses various topics related to mixtures and separations:
- It identifies different types of solutions, suspensions, and colloids.
- It investigates how structure and temperature affect solubility of solids in water.
- It distinguishes among solutions, suspensions, and colloids and identifies suitable separation techniques based on differences in component properties of mixtures.
- It describes the extraction of sucrose from sugar cane.
This chapter discusses the properties and reactions of non-metals. It describes the differences between metals and non-metals, and provides details on the structure and properties of common non-metals like hydrogen, oxygen, nitrogen, carbon, chlorine and sulfur. It also explains methods for producing important compounds from non-metals like sulfuric acid, chlorine and ammonia.
This chapter discusses the extraction of metals from ores. It explains that metals higher in the reactivity series like sodium and aluminium are extracted via electrolysis, while metals lower in the series like iron and copper are extracted by reduction with carbon. The extraction of aluminium, iron, and the uses and corrosion of these metals are described in detail. The chapter also covers how metals are protected from corrosion through various methods like painting, galvanization, and cathodic protection.
This chapter discusses the physical and chemical properties of metals. Metals are usually hard, shiny, malleable and ductile. They are good conductors of heat and electricity. Chemically, metals form positive ions and react with acids, oxygen, water and steam to form salts and release hydrogen gas. The reactivity of metals can be predicted based on their reactivity series, with more reactive metals displacing less reactive ones from their compounds. Alloys are stronger than pure metals due to disrupted atomic layers.
Here are the answers:
1. (a) Carbon monoxide, methane
(b) Sulphur dioxide, nitrogen oxides
2. (a) Sulphur dioxide
(b) Methane
(c) Carbon monoxide
(d) Carbon monoxide, nitrogen oxides
3. (a) O3
(b) (i) A layer of ozone surrounds the Earth at high altitudes and protects us from the harmful radiation of the Sun.
(ii) At ground level, ozone is a harmful pollutant that causes irritation to the eyes and throat. It also causes breathing difficulties and asthma attacks.
This chapter discusses polymers, which are large molecules composed of repeating structural units called monomers. It covers the different types of polymerization reactions, examples of natural and synthetic polymers, and their properties and uses. The chapter also addresses issues with plastic waste and ways to reduce pollution from plastics.
This chapter discusses sources of carbon compounds. It describes fossil fuels like coal, petroleum and natural gas, which are formed from remains of ancient plants and animals. Natural gas is a cleaner burning fuel than coal. Petroleum is refined using fractional distillation to separate it into fractions with different boiling points. Cracking converts heavier fractions into lighter, more useful ones. Fossil fuels are finite, so alternatives like solar, wind and biodiesel from algae are being explored.
Here are the answers to the quick check questions:
1. Raw materials required for ethanol production by fermentation are carbohydrates such as starch or sugar, water, yeast and a source of enzymes.
2. The chemical equations for the fermentation of sugar are:
C6H12O6 → 2C2H5OH + 2CO2
Glucose → Ethanol + Carbon dioxide
This document provides an overview of hydrocarbons and outlines the key learning outcomes of Chapter 15. It discusses the bonding ability of carbon and how carbon can form chains, branches, and rings. It then focuses on two major classes of hydrocarbons - alkanes and alkenes. For each, it defines the homologous series, provides examples, and describes their structures, properties, reactions, and uses. It also introduces topics like isomerism that are important for understanding organic compounds.
This document outlines the process of qualitative analysis, which involves identifying unknown substances by determining the cations and anions present. It describes preliminary observations, tests to identify common gases, and reactions using sodium hydroxide and ammonia solutions to identify cations based on the color and solubility of precipitates formed. The goal is to draw conclusions and identify the unknown based on a systematic analysis and recording of observations from chemical tests.
The document outlines learning outcomes for a chapter on electrochemistry. It will describe investigations into classifying substances as conductors or non-conductors, distinguish between metallic and electrolytic conduction, define key terms like electrolysis, electrodes, and ions. It will also cover predicting reactions and products of electrolysis, calculating quantities produced using Faraday's constant, and discussing industrial applications of electrolysis.
This hymn expresses the singer's faith and trust in God despite not knowing or understanding fully why God chose them or how their faith was imparted. Over four verses, the singer acknowledges not knowing why God showed grace to them, how their faith was given or peace was brought to their heart, how the Spirit works, or when Jesus may return. However, the refrain emphasizes that they know and are convinced of who they have believed in and that God will keep safe what is committed to him until that final day.
Dalton's original atomic theory proposed that atoms were indivisible and identical for each element. Later evidence from experiments by scientists like J.J. Thomson, Ernest Rutherford, Niels Bohr, and James Chadwick modified Dalton's theory by showing that atoms have internal structure consisting of subatomic particles and that isotopes of the same element can have different atomic masses. These discoveries helped establish modern atomic theory and understanding of the structure of atoms and nuclei.
Generating privacy-protected synthetic data using Secludy and MilvusZilliz
During this demo, the founders of Secludy will demonstrate how their system utilizes Milvus to store and manipulate embeddings for generating privacy-protected synthetic data. Their approach not only maintains the confidentiality of the original data but also enhances the utility and scalability of LLMs under privacy constraints. Attendees, including machine learning engineers, data scientists, and data managers, will witness first-hand how Secludy's integration with Milvus empowers organizations to harness the power of LLMs securely and efficiently.
Driving Business Innovation: Latest Generative AI Advancements & Success StorySafe Software
Are you ready to revolutionize how you handle data? Join us for a webinar where we’ll bring you up to speed with the latest advancements in Generative AI technology and discover how leveraging FME with tools from giants like Google Gemini, Amazon, and Microsoft OpenAI can supercharge your workflow efficiency.
During the hour, we’ll take you through:
Guest Speaker Segment with Hannah Barrington: Dive into the world of dynamic real estate marketing with Hannah, the Marketing Manager at Workspace Group. Hear firsthand how their team generates engaging descriptions for thousands of office units by integrating diverse data sources—from PDF floorplans to web pages—using FME transformers, like OpenAIVisionConnector and AnthropicVisionConnector. This use case will show you how GenAI can streamline content creation for marketing across the board.
Ollama Use Case: Learn how Scenario Specialist Dmitri Bagh has utilized Ollama within FME to input data, create custom models, and enhance security protocols. This segment will include demos to illustrate the full capabilities of FME in AI-driven processes.
Custom AI Models: Discover how to leverage FME to build personalized AI models using your data. Whether it’s populating a model with local data for added security or integrating public AI tools, find out how FME facilitates a versatile and secure approach to AI.
We’ll wrap up with a live Q&A session where you can engage with our experts on your specific use cases, and learn more about optimizing your data workflows with AI.
This webinar is ideal for professionals seeking to harness the power of AI within their data management systems while ensuring high levels of customization and security. Whether you're a novice or an expert, gain actionable insights and strategies to elevate your data processes. Join us to see how FME and AI can revolutionize how you work with data!
What is an RPA CoE? Session 1 – CoE VisionDianaGray10
In the first session, we will review the organization's vision and how this has an impact on the COE Structure.
Topics covered:
• The role of a steering committee
• How do the organization’s priorities determine CoE Structure?
Speaker:
Chris Bolin, Senior Intelligent Automation Architect Anika Systems
Skybuffer SAM4U tool for SAP license adoptionTatiana Kojar
Manage and optimize your license adoption and consumption with SAM4U, an SAP free customer software asset management tool.
SAM4U, an SAP complimentary software asset management tool for customers, delivers a detailed and well-structured overview of license inventory and usage with a user-friendly interface. We offer a hosted, cost-effective, and performance-optimized SAM4U setup in the Skybuffer Cloud environment. You retain ownership of the system and data, while we manage the ABAP 7.58 infrastructure, ensuring fixed Total Cost of Ownership (TCO) and exceptional services through the SAP Fiori interface.
In the realm of cybersecurity, offensive security practices act as a critical shield. By simulating real-world attacks in a controlled environment, these techniques expose vulnerabilities before malicious actors can exploit them. This proactive approach allows manufacturers to identify and fix weaknesses, significantly enhancing system security.
This presentation delves into the development of a system designed to mimic Galileo's Open Service signal using software-defined radio (SDR) technology. We'll begin with a foundational overview of both Global Navigation Satellite Systems (GNSS) and the intricacies of digital signal processing.
The presentation culminates in a live demonstration. We'll showcase the manipulation of Galileo's Open Service pilot signal, simulating an attack on various software and hardware systems. This practical demonstration serves to highlight the potential consequences of unaddressed vulnerabilities, emphasizing the importance of offensive security practices in safeguarding critical infrastructure.
For the full video of this presentation, please visit: https://www.edge-ai-vision.com/2024/06/temporal-event-neural-networks-a-more-efficient-alternative-to-the-transformer-a-presentation-from-brainchip/
Chris Jones, Director of Product Management at BrainChip , presents the “Temporal Event Neural Networks: A More Efficient Alternative to the Transformer” tutorial at the May 2024 Embedded Vision Summit.
The expansion of AI services necessitates enhanced computational capabilities on edge devices. Temporal Event Neural Networks (TENNs), developed by BrainChip, represent a novel and highly efficient state-space network. TENNs demonstrate exceptional proficiency in handling multi-dimensional streaming data, facilitating advancements in object detection, action recognition, speech enhancement and language model/sequence generation. Through the utilization of polynomial-based continuous convolutions, TENNs streamline models, expedite training processes and significantly diminish memory requirements, achieving notable reductions of up to 50x in parameters and 5,000x in energy consumption compared to prevailing methodologies like transformers.
Integration with BrainChip’s Akida neuromorphic hardware IP further enhances TENNs’ capabilities, enabling the realization of highly capable, portable and passively cooled edge devices. This presentation delves into the technical innovations underlying TENNs, presents real-world benchmarks, and elucidates how this cutting-edge approach is positioned to revolutionize edge AI across diverse applications.
How to Interpret Trends in the Kalyan Rajdhani Mix Chart.pdfChart Kalyan
A Mix Chart displays historical data of numbers in a graphical or tabular form. The Kalyan Rajdhani Mix Chart specifically shows the results of a sequence of numbers over different periods.
Monitoring and Managing Anomaly Detection on OpenShift.pdfTosin Akinosho
Monitoring and Managing Anomaly Detection on OpenShift
Overview
Dive into the world of anomaly detection on edge devices with our comprehensive hands-on tutorial. This SlideShare presentation will guide you through the entire process, from data collection and model training to edge deployment and real-time monitoring. Perfect for those looking to implement robust anomaly detection systems on resource-constrained IoT/edge devices.
Key Topics Covered
1. Introduction to Anomaly Detection
- Understand the fundamentals of anomaly detection and its importance in identifying unusual behavior or failures in systems.
2. Understanding Edge (IoT)
- Learn about edge computing and IoT, and how they enable real-time data processing and decision-making at the source.
3. What is ArgoCD?
- Discover ArgoCD, a declarative, GitOps continuous delivery tool for Kubernetes, and its role in deploying applications on edge devices.
4. Deployment Using ArgoCD for Edge Devices
- Step-by-step guide on deploying anomaly detection models on edge devices using ArgoCD.
5. Introduction to Apache Kafka and S3
- Explore Apache Kafka for real-time data streaming and Amazon S3 for scalable storage solutions.
6. Viewing Kafka Messages in the Data Lake
- Learn how to view and analyze Kafka messages stored in a data lake for better insights.
7. What is Prometheus?
- Get to know Prometheus, an open-source monitoring and alerting toolkit, and its application in monitoring edge devices.
8. Monitoring Application Metrics with Prometheus
- Detailed instructions on setting up Prometheus to monitor the performance and health of your anomaly detection system.
9. What is Camel K?
- Introduction to Camel K, a lightweight integration framework built on Apache Camel, designed for Kubernetes.
10. Configuring Camel K Integrations for Data Pipelines
- Learn how to configure Camel K for seamless data pipeline integrations in your anomaly detection workflow.
11. What is a Jupyter Notebook?
- Overview of Jupyter Notebooks, an open-source web application for creating and sharing documents with live code, equations, visualizations, and narrative text.
12. Jupyter Notebooks with Code Examples
- Hands-on examples and code snippets in Jupyter Notebooks to help you implement and test anomaly detection models.
Ivanti’s Patch Tuesday breakdown goes beyond patching your applications and brings you the intelligence and guidance needed to prioritize where to focus your attention first. Catch early analysis on our Ivanti blog, then join industry expert Chris Goettl for the Patch Tuesday Webinar Event. There we’ll do a deep dive into each of the bulletins and give guidance on the risks associated with the newly-identified vulnerabilities.
Fueling AI with Great Data with Airbyte WebinarZilliz
This talk will focus on how to collect data from a variety of sources, leveraging this data for RAG and other GenAI use cases, and finally charting your course to productionalization.
HCL Notes and Domino License Cost Reduction in the World of DLAUpanagenda
Webinar Recording: https://www.panagenda.com/webinars/hcl-notes-and-domino-license-cost-reduction-in-the-world-of-dlau/
The introduction of DLAU and the CCB & CCX licensing model caused quite a stir in the HCL community. As a Notes and Domino customer, you may have faced challenges with unexpected user counts and license costs. You probably have questions on how this new licensing approach works and how to benefit from it. Most importantly, you likely have budget constraints and want to save money where possible. Don’t worry, we can help with all of this!
We’ll show you how to fix common misconfigurations that cause higher-than-expected user counts, and how to identify accounts which you can deactivate to save money. There are also frequent patterns that can cause unnecessary cost, like using a person document instead of a mail-in for shared mailboxes. We’ll provide examples and solutions for those as well. And naturally we’ll explain the new licensing model.
Join HCL Ambassador Marc Thomas in this webinar with a special guest appearance from Franz Walder. It will give you the tools and know-how to stay on top of what is going on with Domino licensing. You will be able lower your cost through an optimized configuration and keep it low going forward.
These topics will be covered
- Reducing license cost by finding and fixing misconfigurations and superfluous accounts
- How do CCB and CCX licenses really work?
- Understanding the DLAU tool and how to best utilize it
- Tips for common problem areas, like team mailboxes, functional/test users, etc
- Practical examples and best practices to implement right away
"Frontline Battles with DDoS: Best practices and Lessons Learned", Igor IvaniukFwdays
At this talk we will discuss DDoS protection tools and best practices, discuss network architectures and what AWS has to offer. Also, we will look into one of the largest DDoS attacks on Ukrainian infrastructure that happened in February 2022. We'll see, what techniques helped to keep the web resources available for Ukrainians and how AWS improved DDoS protection for all customers based on Ukraine experience
How information systems are built or acquired puts information, which is what they should be about, in a secondary place. Our language adapted accordingly, and we no longer talk about information systems but applications. Applications evolved in a way to break data into diverse fragments, tightly coupled with applications and expensive to integrate. The result is technical debt, which is re-paid by taking even bigger "loans", resulting in an ever-increasing technical debt. Software engineering and procurement practices work in sync with market forces to maintain this trend. This talk demonstrates how natural this situation is. The question is: can something be done to reverse the trend?
Taking AI to the Next Level in Manufacturing.pdfssuserfac0301
Read Taking AI to the Next Level in Manufacturing to gain insights on AI adoption in the manufacturing industry, such as:
1. How quickly AI is being implemented in manufacturing.
2. Which barriers stand in the way of AI adoption.
3. How data quality and governance form the backbone of AI.
4. Organizational processes and structures that may inhibit effective AI adoption.
6. Ideas and approaches to help build your organization's AI strategy.
The Microsoft 365 Migration Tutorial For Beginner.pptxoperationspcvita
This presentation will help you understand the power of Microsoft 365. However, we have mentioned every productivity app included in Office 365. Additionally, we have suggested the migration situation related to Office 365 and how we can help you.
You can also read: https://www.systoolsgroup.com/updates/office-365-tenant-to-tenant-migration-step-by-step-complete-guide/
2. THE ATOM In 580 BC, the ancient Greek philosopher Thales suggested that water was the fundamental ‘element’ from which all matter in the universe was composed
3. THE ATOM Then, 200 years later, another philosopher by the name of Aristotle proposed that along with water, earth, air and fire were the four main elements that made up the world. In addition to this, he also proposed that there was a fifth element, ‘aether’, that made up the heavens
4. THE ATOM This suggestion made by Aristotle persisted for almost 2000 years until in 1961 a man named Robert Boyle wrote and published a book called ‘The Sceptical Chymist’ which was a turning point in chemistry. It was the first modern definition of an element as being something that cannot be changed into anything simpler rather than just merely a substance that the world was comprised of. Boyle also urged chemists to carry out practical investigations rather than just observing and making deductions as the Greeks had been doing earlier
6. Dalton's theory was based on the premise that the atoms of different elements could be distinguished by differences in their weights. He stated his theory in a lecture to the Royal Institution in 1803. The theory proposed a number of basic ideas:All matter is composed of atomsAtoms cannot be made or destroyedAll atoms of the same element are identicalDifferent elements have different types of atomsChemical reactions occur when atoms are rearrangedCompounds are formed from atoms of the constituent elements.Using his theory, Dalton rationalised the various laws of chemical combination which were in existence at that time. However, he made a mistake in assuming that the simplest compound of two elements must be binary, formed from atoms of each element in a 1:1 ratio, and his system of atomic weights was not very accurate - he gave oxygen an atomic weight of seven instead of eight.Despite these errors, Dalton's theory provided a logical explanation of concepts, and led the way into new fields of experimentation.
8. The Plum Pudding Model/Chocolate Chip Cookie Model was developed by J.J. Thomson. This is how Thomson discovered the electron in 1897. Thomson suggested this theory in 1904. The theory said that atoms as a whole were neutrally charged. He also suggested that the atom was made up electrons embedded into a cloud of positive particles. This was known as the Chocolate Chip Cookie Model because the electrons are like the chocolate chips embedded into the cookie and the dough is like the cloud of positive particles surrounding the chocolate chips(electrons).
9.
10. Atoms as a whole are neutrally charged because the amount of positive charge in it cancels out the amount of negatively charged electrons. This means as a whole atoms are neutrally charged.
11. The electrons are randomly scattered throughout the atom just like chocolate chips in a cookie. The rest of the atom is a positive charge which surrounds the electrons, like the dough in a cookie.
12.
13. Experiment that Proved the Theory The Crooke's tube experiment showed J.J. Thomson that there were electrons in an atom. This experiment also showed him that electrons were negatively charged. This meant that if atoms are neutrally charged as a whole and elctrons are negatively charged then there must be a positive charge in the atom to cancel out the negative charge of the electrons. Thomson experiment worked like this: - The Crooke's tube showed Thomson that he could bend a beam of "Cathode Rays"( electrons) using a set of negative and positively charged plates. Because the beam of "Cathode Rays" bent towards the positively charged plate it meant that the beam was negatively charged because opposites attract. - Thomson called the particles in the beam electrons. -Now that Thomson knew there were electrons in the atom he knew that there had to be a positive charge in the atom to offset the negative charge of the electrons to make the atom neutrally charged.
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15. Before J.J Thomson’s atomic theory John Dalton had an atomic theory that said that atoms couldn't be destroyed or broken but J.J. Thomson proved that wrong when he extracted the electrons from the atom in his Crooke's tube experiment. Thomson extracted the electrons from the atom, hence, disproving John Daltons theory that atoms were one solid thing.
17. Rutherford's model did not make any new headway in explaining the electron-structure of the atom; in this regard Rutherford merely mentioned earlier atomic models in which a number of tiny electrons circled the nucleus like planets around the sun, or a ring around a planet (such as Saturn). However, by implication, Rutherford's concentration of most of the atom's mass into a very small core made a planetary model an even more likely metaphor than before, as such a core would contain most of the atom's mass, in an analogous way to the Sun containing most of the solar systems' mass.
18. Rutherford also directed the famous Geiger-Marsden experiment in 1909, which suggested on Rutherford's 1911 analysis that the so-called "plum pudding model" of J. J. Thomson of the atom was incorrect. Rutherford's new modelfor the atom, based on the experimental results, had the new features of a relatively high central charge concentrated into a very small volume in comparison to the rest of the atom and containing the bulk of the atomic mass (the nucleus of the atom).
21. In 1909, Hans Geiger and Ernest Marsden carried out an experiment called the Hans/Geiger Experiment (also called the Gold foil experiment or the Rutherford experiment) which was to probe the structure of the atom, under the direction of Ernest Rutherford at the Physical Laboratories of the University of Manchester. The unexpected results of the experiment demonstrated for the first time the existence of the atomic nucleus, leading to the downfall of the plum- pudding modelof the atom, and the development of the Rutherford(planetary) model.
22. The gold foil experiment consisted of a series of tests in which positively charged helium nuclei were directed at a very thin layer of gold foil. The expected result was that the positive particles would be moved just a few degrees from their path as they passed through the sea of positive charge proposed in the plum pudding model. The result, however, was that the positive particles were repelled from gold foil at very high angles, up to 180 degrees. However, most of the remaining particles were not deflected at all, but rather, passed through the foil. In detail, a beam of alpha particles, generated by the radioactive decay of radium was directed normally onto a sheet of very thin gold foil. The gold foil was surrounded by a circular sheet of zinc sulphide (ZnS) which was used as a detector: the ZnS sheet would light up when hit with alpha particles. Under the prevailing plum pudding model, the alpha particles should all have been deflected by, at most, a few degrees; measuring the pattern of scattered particles was expected to provide information about the distribution of charge within the atom. However they observed that a very small percentage of particles were deflected through angles much larger than 90 degrees. According to Rutherford: It was quite the most incredible event that has ever happened to me in my life. It was almost as incredible as if you fired a 15-inch shell at a piece of tissue paper and it came back and hit you. On consideration, I realized that this scattering backward must be the result of a single collision, and when I made calculations I saw that it was impossible to get anything of that order of magnitude unless you took a system in which the greater part of the mass of the atom was concentrated in a minute nucleus. It was then that I had the idea of an atom with a minute massive center, carrying a charge.
26. In 1911, Niels Bohr went to England to study with J.J. Thomson, who had discovered the electron in 1897. Most physicists in the early years of the twentieth century were engrossed by the electron, such a new and fascinating discovery. Few concerned themselves much with the work of Max Planck or Albert Einstein. Thomson wasn't that interested in these new ideas, but Bohr had an open mind. Bohr soon went to visit Ernest Rutherford (a former student of Thomson's) in another part of England, where Rutherford had made a brand-new discovery about the atom.
27. When Bohr joined Rutherford he realized that Rutherford's model wasn't quite right. By all rules of classical physics, it should be very unstable. For one thing, the orbiting electrons should give off energy and eventually spiral down into the nucleus, making the atom collapse. Or the electrons could be knocked out of position if a charged particle passed by. Bohr turned to Planck's quantum theory to explain the stability of most atoms. He found that the ratio of energy in electrons and the frequency of their orbits around the nucleus was equal to Planck's constant (the proportion of light's energy to its wave frequency, or approximately 6.626 x 10-23 ). Bohr suggested the revolutionary idea that electrons "jump" between energy levels (orbits) in a quantum fashion, that is, without ever existing in an in-between state. Thus when an atom absorbs or gives off energy (as in light or heat), the electron jumps to higher or lower orbits. Bohr published these ideas in 1913 to mixed reaction. Many people still hadn't accepted the idea of quanta, or they found other flaws in the theory because Bohr had based it on very simple atoms. But there was good evidence he was right: the electrons in his model lined up with the regular patterns (spectral series) of light emitted by real hydrogen atoms.
28. Bohr's theory that electrons existed in set orbits around the nucleus was the key to the periodic repetition of properties of the elements. The shells in which electrons orbit have different quantum numbers and hold only certain numbers of electrons -- the first shell holds no more than 2, the second shell up to 8, the third 10, the fourth 14. Atoms with less than the maximum number in their outer shells are less stable than those with "full" outer shells. Elements that have the same number of electrons in their outermost shells appear in the same column in the periodic table of elements and tend to have similar chemical properties. Over the years other investigators refined Bohr's theory, but his bold application of new ideas paved the way for the development of quantum mechanics. Bohr went on to make enormous contributions to physics and, like Rutherford, to train a new generation of physicists. But his atomic model remains the best known work of his very long career.
29. HENRY g. j. MOSELEY Five years before Rutherford announced the discovery of the proton, Henry Moseley, a scientist from Rutherford’s research team, carried out an experiment by bombarding different metal targets with cathode rays and measured the frequency of the X-rays that emerged from the anode. He discovered that the energy of x-rays emitted by the elements and frequency increased in a linear fashion with each successive element in the periodic table, with an increase in the mass of the metal atom. In 1913, he proposed that the relationship was a function of the positive charge on the nucleus( which Rutherford called the Atomic Number).This rearranged the periodic table by using the atomic number instead of atomic mass to represent the progression of the elements. This new table left additional holes for elements that would soon be discovered.
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31. The element’s numbered position in the Periodic Table is arranged in atomic order from the smallest to largest.
32.
33. In 1932, English Physicist James Chadwick, another member of Ernest Rutherford’s research team, after a decade-long struggle to track down this tricky particle (all the methods available at the time were used only to detect charged particles), performed tests on a new type of radiation which had been baffling physicists for years, and which had previously been mistaken for “gamma rays” (a form of radiation consisting of high-energy photons) along
34. The test, to simplify as much as possible, went like this: A sample of Beryllium was bombarded with alpha particles (another type of naturally occurring radiation which are technically just ionized helium nuclei), which causes it to emit this mysterious radiation. It was then discovered by Irene Joliot-Curie (daughter of Marie and Pierre Curie) and her husband Frederic Joliot-Curie that this radiation, upon striking a proton-rich surface (paraffin was the preferred example), would discharge some of the protons, which could then be detected using a Geiger counter (a device that measures radiation). This was the premise, and from here, Chadwick simply had to play detective and put all the pieces of the puzzle together. For instance, he could tell that the mysterious radiation in question was neutral due to the fact that it was not affected by proximity to a magnetic field, and, unlike standard gamma radiation, did not invoke the photoelectric effect (when photons, such as gamma rays, strike certain surfaces, they discharge electrons, which can be simply measured), but rather discharged protons, which meant that the particles had to be more massive than previously expected.
35. Rutherford guessed that the protons were coming from the parrafin because some sort of radiation was hitting it. He said that this radiation was like the effect of an invisible man who cannot be seen directly, but who is known to be there because he collides with other people in a crowd. The invisible particle of Chadwick’s experiment (with no charge and with its mass equal to that of a proton), was named the neutron. Hence, this completed the long search by many scientists to come up with the perfect model and of the atom. An atom is now known to be, the smallest part of an element which contains a minute central nucelus of positively charged protons and neutral neutons surrounded by negatively charged elctrons orbiting in fixed shells of different energy levels around the nucleus.