How the matter is building up from the smallest parts until the greatest. A study the atom structure and a review along the History of the different theories and attemps in order to explain how our world works.
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
This document discusses several periodic trends including electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. It defines each trend and provides a brief explanation of how each trend relates to an element's chemical and physical properties based on its position in the periodic table.
This document discusses different types of chemical bonds:
1) Metallic bonds form when valence electrons are delocalized and shared between all metal atoms in a lattice, holding the positive ions together.
2) Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions that are attracted to each other.
3) Covalent bonds form when two nonmetals share valence electrons in a molecule through electron pairs. Lewis structures are used to represent electron sharing in covalent bonds.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
The document introduces the four main macromolecules (carbohydrates, proteins, lipids, nucleic acids) found in living things. It discusses that macromolecules are polymers composed of simple repeating units called monomers. Each macromolecule is described in terms of its monomer, examples being amino acids for proteins and nucleotides for nucleic acids. Key functions of each macromolecule are also outlined, such as carbohydrates and lipids being used for energy storage and proteins being used for structure and enzyme functions. The document aims to teach students to identify, draw, and describe the essential characteristics of the four biological macromolecules.
Each row of the periodic table is called a period. Elements in the same period have the same number of electron shells. Each column is called a group. Elements in the same group have the same number of valence electrons, except for helium which has two electrons. Valence electrons are the outermost electrons of an atom and are involved in bonding. Reactive elements bond easily to gain or lose valence electrons to achieve a full outer electron shell of eight electrons.
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
This document discusses several periodic trends including electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. It defines each trend and provides a brief explanation of how each trend relates to an element's chemical and physical properties based on its position in the periodic table.
This document discusses different types of chemical bonds:
1) Metallic bonds form when valence electrons are delocalized and shared between all metal atoms in a lattice, holding the positive ions together.
2) Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions that are attracted to each other.
3) Covalent bonds form when two nonmetals share valence electrons in a molecule through electron pairs. Lewis structures are used to represent electron sharing in covalent bonds.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
The document introduces the four main macromolecules (carbohydrates, proteins, lipids, nucleic acids) found in living things. It discusses that macromolecules are polymers composed of simple repeating units called monomers. Each macromolecule is described in terms of its monomer, examples being amino acids for proteins and nucleotides for nucleic acids. Key functions of each macromolecule are also outlined, such as carbohydrates and lipids being used for energy storage and proteins being used for structure and enzyme functions. The document aims to teach students to identify, draw, and describe the essential characteristics of the four biological macromolecules.
Each row of the periodic table is called a period. Elements in the same period have the same number of electron shells. Each column is called a group. Elements in the same group have the same number of valence electrons, except for helium which has two electrons. Valence electrons are the outermost electrons of an atom and are involved in bonding. Reactive elements bond easily to gain or lose valence electrons to achieve a full outer electron shell of eight electrons.
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
The document discusses the rules for naming binary covalent (molecular) compounds. It explains that these compounds are made of two nonmetals bonded together with covalent bonds. The naming involves identifying the elements present and using prefixes to indicate the number of atoms of each element, with the first word naming the first element and the second using "-ide" to name the second element. Examples are provided and worked through step-by-step.
The document summarizes the development of atomic models from Democritus to Bohr. It discusses key contributors including Democritus proposing atoms, Dalton establishing the atomic theory, Thomson proposing the plum pudding model, Rutherford discovering the nucleus through the gold foil experiment, and Bohr refining the model by proposing fixed electron orbits.
John Dalton performed experiments in 1800 that showed matter is made of indivisible particles called atoms. This led him to formulate Dalton's Atomic Theory which stated that atoms are identical for each element and compounds form when different types of atoms combine. While initially controversial, the theory became widely accepted after discoveries of subatomic particles like the electron and proton in the 1900s. These discoveries included J.J. Thomson finding the electron using cathode ray tubes in 1897 and identifying it as an atom's negatively charged component 2000 times smaller than hydrogen, and Rutherford proposing the nuclear model of the atom with a small, positively charged nucleus surrounded by orbiting electrons.
The document provides instructions for naming ionic and binary covalent compounds. Ionic compounds are formed from metals and nonmetals, with the metal ions taking positive charges and the nonmetal ions taking negative charges. Binary covalent compounds are formed from two nonmetals sharing electrons in ratios indicated by prefixes like di-, tri-, and tetra-. The naming process for ionic compounds involves writing the name of the metal ion followed by the name of the nonmetal ion. For binary covalent compounds, the process involves writing the names of the two nonmetals, changing the second to end in "-ide", and adding prefixes to indicate ratios.
The document defines key terms related to chemical equations:
- Chemical reactions represent changes where reactants are converted to products through chemical changes.
- Chemical equations express reactions using formulas, numbers, and symbols to represent reactants and products.
- Coefficients indicate the number of atoms or molecular units of each substance involved in the reaction.
John Dalton proposed the atomic theory in 1804, stating that all matter is composed of tiny, indivisible particles called atoms that cannot be divided further. Later discoveries found that atoms consist of even smaller subatomic particles, including electrons discovered by J.J. Thomson in 1897 and the nucleus discovered by Ernest Rutherford in 1910. The quantum mechanical model developed in 1926 by Schrodinger, Heisenberg and others proposed that electrons exist as waves of energy around the nucleus, rather than following fixed orbits as proposed by Niels Bohr's 1913 planetary model of the atom.
1. The document provides an overview of writing formulas and naming ionic and covalent compounds. It reviews the periodic table and properties of metals, nonmetals and metalloids.
2. Key concepts covered include ion formation, the octet rule, polyatomic ions, oxidation numbers, naming conventions for ionic compounds containing metals or transition metals, and prefixes used in naming covalent compounds.
3. The document distinguishes between ionic and covalent bonding, lattice structures, and molecular structures of compounds.
The document provides a history of discoveries related to the atom from ancient Greek philosophers to modern quantum mechanics. It describes key contributors such as Democritus proposing atoms, Dalton establishing atomic theory, Rutherford discovering the nucleus, Bohr introducing quantum mechanics, and Heisenberg establishing the uncertainty principle. The development of atomic models progressed from simple spheres to planetary structures to quantum mechanical probability distributions.
The document discusses Lewis dot structures, which use dots to represent valence electrons around an atomic symbol. It explains that ions have Lewis dot diagrams with fewer (for cations) or more (for anions) dots than the corresponding atom due to gaining or losing electrons. The document provides examples of Lewis dot diagrams for various ions, such as Ca2+ and O2-. It also includes practice problems asking students to draw Lewis dot diagrams for additional ions.
This document discusses ecological relationships between organisms in a forest reserve. It defines key terms like symbiosis, trophic levels, and food chains. The goal is to have students name plant and animal species in the forest, and identify an ecological relationship between two species that promotes a healthy environment. Students will learn about different types of symbiotic relationships like mutualism and how energy is transferred between trophic levels in a food chain.
1. Atoms are the basic building blocks of matter and consist of protons, neutrons, and electrons.
2. Atoms bond together through either primary bonds like ionic bonds, covalent bonds, and metallic bonds or secondary bonds like hydrogen bonds and van der Waals forces.
3. Materials can be crystalline, with a periodic arrangement of atoms, or noncrystalline, with short-range atomic order. The type of bonding and crystal structure determines a material's physical properties.
The document discusses the different phases of matter (solid, liquid, gas) and the phase changes between them. When energy is added to a solid, its bonds break and it melts into a liquid where particles can move freely. Adding more energy turns the liquid into a gas where particles move randomly. The phase changes - melting/freezing, vaporization/condensation, sublimation/deposition - describe the changes in particle arrangement that occur when energy is added or removed. Phase changes are classified as endothermic, where energy is absorbed during the change, or exothermic, where energy is released.
This document provides information about electron configuration. It begins by defining electron configuration as the arrangement of electrons in an atom's orbitals, which is described using quantum numbers. It then discusses the three main rules for writing electron configurations: 1) Aufbau principle, which states that electrons fill the lowest available energy levels first, 2) Pauli exclusion principle, which limits each orbital to two electrons of opposite spin, and 3) Hund's rule, which states that degenerate orbitals will fill with one electron each before pairing. The document provides examples of writing full and condensed electron configurations and drawing orbital diagrams for various elements. It includes an activity for students to practice these skills.
This document provides instructions on writing chemical formulas. It explains that chemical symbols represent elements and come from the element name. Subscript numbers indicate the number of atoms in a compound. Ionic formulas are written with the metal first followed by the nonmetal and hyphenated name. Covalent prefixes like mono, di and tri are used to denote the number of atoms bonded to the central element. Roman numerals specify the metal's oxidation state in some compounds. The document uses examples to demonstrate how to apply these rules to write correct chemical formulas.
This document discusses ions and how they are formed. It explains that atoms become ions by gaining or losing electrons to obtain a full outer electron shell. Atoms that gain electrons become negatively charged ions and atoms that lose electrons become positively charged ions. The document also discusses different types of ions including monatomic ions, polyatomic ions, and how to name compound ions that contain multiple atoms like sulfate, nitrate, and hydroxide ions.
The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
This document discusses quantum numbers and their role in describing electron orbitals and configurations. It covers the principal (n), azimuthal (l), and magnetic (ml) quantum numbers, as well as electron spin (ms). The document defines orbitals for the first five energy levels, discusses how electrons fill orbitals based on the Aufbau principle and Hund's rule, and notes exceptions like chromium and copper. It asks the reader to write electron configurations and diagrams for chlorine, osmium, and cesium.
The document discusses the history and development of atomic theory and the periodic table. It describes early atomic models proposed by Democritus and Dalton. Rutherford's gold foil experiment provided evidence that atoms have a small, dense nucleus containing protons and neutrons. Elements are distinguished by their atomic number and isotopes differ in their number of neutrons. The periodic table organizes elements according to recurring trends in their physical and chemical properties, allowing relationships between elements to be identified.
This document outlines the key concepts and objectives for a unit on atoms, molecules, and ions. It will cover early atomic theories like Dalton's atomic theory, discoveries leading to the nuclear model of the atom including cathode rays and Rutherford's gold foil experiment. Students will learn about atomic structure including atomic and mass numbers. The periodic table is introduced along with chemical bonds like ionic and covalent bonds. The document also outlines naming ionic and molecular compounds as well as writing chemical formulas.
The universe is composed of ordinary visible matter (4%), dark matter (21%), and dark energy (75%). Dark matter's existence was postulated to explain gravitational forces, while dark energy causes the accelerated expansion of the universe. The Big Bang theory proposes that approximately 13.7 billion years ago, the universe began as a very dense, hot mass that exploded and expanded. Evidence for this includes the cosmic microwave background radiation and the formation of light elements. Galaxies formed over time and come in elliptical, spiral, and irregular shapes. Stars form from clouds of dust and gas through gravitational collapse and nuclear fusion.
The document discusses the rules for naming binary covalent (molecular) compounds. It explains that these compounds are made of two nonmetals bonded together with covalent bonds. The naming involves identifying the elements present and using prefixes to indicate the number of atoms of each element, with the first word naming the first element and the second using "-ide" to name the second element. Examples are provided and worked through step-by-step.
The document summarizes the development of atomic models from Democritus to Bohr. It discusses key contributors including Democritus proposing atoms, Dalton establishing the atomic theory, Thomson proposing the plum pudding model, Rutherford discovering the nucleus through the gold foil experiment, and Bohr refining the model by proposing fixed electron orbits.
John Dalton performed experiments in 1800 that showed matter is made of indivisible particles called atoms. This led him to formulate Dalton's Atomic Theory which stated that atoms are identical for each element and compounds form when different types of atoms combine. While initially controversial, the theory became widely accepted after discoveries of subatomic particles like the electron and proton in the 1900s. These discoveries included J.J. Thomson finding the electron using cathode ray tubes in 1897 and identifying it as an atom's negatively charged component 2000 times smaller than hydrogen, and Rutherford proposing the nuclear model of the atom with a small, positively charged nucleus surrounded by orbiting electrons.
The document provides instructions for naming ionic and binary covalent compounds. Ionic compounds are formed from metals and nonmetals, with the metal ions taking positive charges and the nonmetal ions taking negative charges. Binary covalent compounds are formed from two nonmetals sharing electrons in ratios indicated by prefixes like di-, tri-, and tetra-. The naming process for ionic compounds involves writing the name of the metal ion followed by the name of the nonmetal ion. For binary covalent compounds, the process involves writing the names of the two nonmetals, changing the second to end in "-ide", and adding prefixes to indicate ratios.
The document defines key terms related to chemical equations:
- Chemical reactions represent changes where reactants are converted to products through chemical changes.
- Chemical equations express reactions using formulas, numbers, and symbols to represent reactants and products.
- Coefficients indicate the number of atoms or molecular units of each substance involved in the reaction.
John Dalton proposed the atomic theory in 1804, stating that all matter is composed of tiny, indivisible particles called atoms that cannot be divided further. Later discoveries found that atoms consist of even smaller subatomic particles, including electrons discovered by J.J. Thomson in 1897 and the nucleus discovered by Ernest Rutherford in 1910. The quantum mechanical model developed in 1926 by Schrodinger, Heisenberg and others proposed that electrons exist as waves of energy around the nucleus, rather than following fixed orbits as proposed by Niels Bohr's 1913 planetary model of the atom.
1. The document provides an overview of writing formulas and naming ionic and covalent compounds. It reviews the periodic table and properties of metals, nonmetals and metalloids.
2. Key concepts covered include ion formation, the octet rule, polyatomic ions, oxidation numbers, naming conventions for ionic compounds containing metals or transition metals, and prefixes used in naming covalent compounds.
3. The document distinguishes between ionic and covalent bonding, lattice structures, and molecular structures of compounds.
The document provides a history of discoveries related to the atom from ancient Greek philosophers to modern quantum mechanics. It describes key contributors such as Democritus proposing atoms, Dalton establishing atomic theory, Rutherford discovering the nucleus, Bohr introducing quantum mechanics, and Heisenberg establishing the uncertainty principle. The development of atomic models progressed from simple spheres to planetary structures to quantum mechanical probability distributions.
The document discusses Lewis dot structures, which use dots to represent valence electrons around an atomic symbol. It explains that ions have Lewis dot diagrams with fewer (for cations) or more (for anions) dots than the corresponding atom due to gaining or losing electrons. The document provides examples of Lewis dot diagrams for various ions, such as Ca2+ and O2-. It also includes practice problems asking students to draw Lewis dot diagrams for additional ions.
This document discusses ecological relationships between organisms in a forest reserve. It defines key terms like symbiosis, trophic levels, and food chains. The goal is to have students name plant and animal species in the forest, and identify an ecological relationship between two species that promotes a healthy environment. Students will learn about different types of symbiotic relationships like mutualism and how energy is transferred between trophic levels in a food chain.
1. Atoms are the basic building blocks of matter and consist of protons, neutrons, and electrons.
2. Atoms bond together through either primary bonds like ionic bonds, covalent bonds, and metallic bonds or secondary bonds like hydrogen bonds and van der Waals forces.
3. Materials can be crystalline, with a periodic arrangement of atoms, or noncrystalline, with short-range atomic order. The type of bonding and crystal structure determines a material's physical properties.
The document discusses the different phases of matter (solid, liquid, gas) and the phase changes between them. When energy is added to a solid, its bonds break and it melts into a liquid where particles can move freely. Adding more energy turns the liquid into a gas where particles move randomly. The phase changes - melting/freezing, vaporization/condensation, sublimation/deposition - describe the changes in particle arrangement that occur when energy is added or removed. Phase changes are classified as endothermic, where energy is absorbed during the change, or exothermic, where energy is released.
This document provides information about electron configuration. It begins by defining electron configuration as the arrangement of electrons in an atom's orbitals, which is described using quantum numbers. It then discusses the three main rules for writing electron configurations: 1) Aufbau principle, which states that electrons fill the lowest available energy levels first, 2) Pauli exclusion principle, which limits each orbital to two electrons of opposite spin, and 3) Hund's rule, which states that degenerate orbitals will fill with one electron each before pairing. The document provides examples of writing full and condensed electron configurations and drawing orbital diagrams for various elements. It includes an activity for students to practice these skills.
This document provides instructions on writing chemical formulas. It explains that chemical symbols represent elements and come from the element name. Subscript numbers indicate the number of atoms in a compound. Ionic formulas are written with the metal first followed by the nonmetal and hyphenated name. Covalent prefixes like mono, di and tri are used to denote the number of atoms bonded to the central element. Roman numerals specify the metal's oxidation state in some compounds. The document uses examples to demonstrate how to apply these rules to write correct chemical formulas.
This document discusses ions and how they are formed. It explains that atoms become ions by gaining or losing electrons to obtain a full outer electron shell. Atoms that gain electrons become negatively charged ions and atoms that lose electrons become positively charged ions. The document also discusses different types of ions including monatomic ions, polyatomic ions, and how to name compound ions that contain multiple atoms like sulfate, nitrate, and hydroxide ions.
The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
This document discusses quantum numbers and their role in describing electron orbitals and configurations. It covers the principal (n), azimuthal (l), and magnetic (ml) quantum numbers, as well as electron spin (ms). The document defines orbitals for the first five energy levels, discusses how electrons fill orbitals based on the Aufbau principle and Hund's rule, and notes exceptions like chromium and copper. It asks the reader to write electron configurations and diagrams for chlorine, osmium, and cesium.
The document discusses the history and development of atomic theory and the periodic table. It describes early atomic models proposed by Democritus and Dalton. Rutherford's gold foil experiment provided evidence that atoms have a small, dense nucleus containing protons and neutrons. Elements are distinguished by their atomic number and isotopes differ in their number of neutrons. The periodic table organizes elements according to recurring trends in their physical and chemical properties, allowing relationships between elements to be identified.
This document outlines the key concepts and objectives for a unit on atoms, molecules, and ions. It will cover early atomic theories like Dalton's atomic theory, discoveries leading to the nuclear model of the atom including cathode rays and Rutherford's gold foil experiment. Students will learn about atomic structure including atomic and mass numbers. The periodic table is introduced along with chemical bonds like ionic and covalent bonds. The document also outlines naming ionic and molecular compounds as well as writing chemical formulas.
The universe is composed of ordinary visible matter (4%), dark matter (21%), and dark energy (75%). Dark matter's existence was postulated to explain gravitational forces, while dark energy causes the accelerated expansion of the universe. The Big Bang theory proposes that approximately 13.7 billion years ago, the universe began as a very dense, hot mass that exploded and expanded. Evidence for this includes the cosmic microwave background radiation and the formation of light elements. Galaxies formed over time and come in elliptical, spiral, and irregular shapes. Stars form from clouds of dust and gas through gravitational collapse and nuclear fusion.
The document summarizes the Big Bang theory, which proposes that approximately 13.8 billion years ago the observable universe was extremely hot and dense and has been expanding and cooling ever since. It provides evidence for this theory, including the cosmic microwave background radiation, Hubble's discovery of the expansion of the universe, and the abundance of light elements produced in the early universe. It also notes some problems with the theory, such as uneven distribution of matter, and possibilities for the ultimate fate of the universe.
This document provides an overview of basic chemistry concepts including:
1) Definitions of key terms like matter, atoms, molecules, elements, compounds, and mixtures.
2) Descriptions of the three states of matter - solids, liquids, and gases - and physical and chemical properties.
3) Explanations of units and measurements in chemistry including the SI system and exponential notation.
4) A brief history of atomic structure theories from Greek philosophers to Rutherford's model of the atom.
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 discusses isotope fractionation in ozone and its cosmochemical implications. It presents theoretical calculations showing mass-independent isotope effects can arise from scattering processes involving indistinguishable isotopes.
- Numerical simulations of ozone formation reactions reproduce observed fractionation factors without adjustable parameters, supporting this quantum mechanical explanation.
- This process could explain other isotopic anomalies if certain gas-solid reactions are quenched before completion, and warrants further experimental study.
The document discusses the scientific method and how it has evolved over time. It begins by defining science as the empirical study of nature. It then discusses three main methodologies in science: reductionism, which explains phenomena in terms of underlying mechanisms; structuralism, which studies complex phenomena as original systems; and "universalism", which makes statistical predictions about classes of similar systems. The document traces how these methodologies have developed from classical physics to modern fields like quantum mechanics and biology. It also explores how mythologies can provide metaphorical insights that inspire scientific hypotheses.
This document discusses a university course on nuclear physics and its goals of educating the public on basic nuclear concepts and issues. It outlines the course schedule which includes lectures on radiation properties, nuclear creation in the cosmos, applications of nuclear physics, and modern research frontiers. Laboratory sessions are planned to demonstrate radiation detection, half-life measurement, shielding, and source identification. The document also provides information on alpha, beta, gamma, and neutron radiation, and examples of isotope half-lives and their applications.
This document discusses the atomic structure of protons, neutrons, and electrons. It explains that protons and neutrons make up the nucleus at the center of the atom, which contains most of the atom's mass. Electrons orbit around the nucleus. The number of protons determines the element and its properties. Chemical bonds are formed through the interaction of electrons between atoms. Ionic bonds are formed when electrons are transferred, and covalent bonds are formed through shared electron pairs. Hydrogen bonds also involve the interaction of electrons. Chemical reactions involve the breaking and forming of bonds between molecules.
- Aristotle proposed that matter was made of four elements: earth, fire, water, and air. This theory persisted for over 2000 years despite being incorrect.
- In the early 1800s, Dalton proposed his modern atomic theory which stated that all matter is made of atoms, atoms of the same element are identical, and atoms combine in fixed ratios.
- Rutherford's gold foil experiment in the early 1900s showed that atoms have a small, dense nucleus containing positive charge, overturning the plum pudding model of atoms.
This document provides an overview of the history and development of the atomic theory. It discusses early Greek philosophers like Democritus who proposed that all matter is composed of indivisible atoms. Later, scientists like John Dalton developed atomic theory further by proposing that atoms are tiny, indivisible particles that combine to form all substances. The document then outlines evidence for subatomic particles like J.J. Thomson's discovery of electrons and Rutherford's discovery of the nucleus. It defines key subatomic particles like protons, neutrons, and electrons and how they combine to form different atoms and isotopes.
A presentation on Piezoelectricity by JaTin. Including what is piezoelectricity, how and why it happens, applications, and detailed application of quartz watches.
The overwhelming observational evidence for the existence of dark matter is only matched by the awkward scarcity of information about what it might actually be. Laboratory searches for dark matter now appear to exclude many of the "weakly interacting massive particle" models that were favored by particle physicists for decades. Where does that leave the hunt for dark matter? If we've left the WIMP behind, what are we looking for? We give a brief, biased, and largely fictional history of the WIMP in order to establish what has and has not been excluded, and why it matters.
This general-interest presentation grew out of discussions with astronomers who wanted to understand why some of their particle physics colleagues are "searching for WIMPs" while the others
have decided to live in a "post-WIMP world."
This self-guided computer activity introduces students to the topic of atoms through interactive lessons and websites. It is divided into two parts, with part one covering the atomic-molecular theory of matter and how scientists gather evidence about atoms through models and indirect observation. Part two discusses the structure of atoms including the nucleus, electrons, and subatomic particles, as well as isotopes and radioactive decay. Students are instructed to complete a study guide as they proceed through the lessons.
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.
This document provides an overview of the history and development of atomic structure and the atomic model. It discusses early Greek philosophers like Democritus who proposed that all matter is made of invisible indivisible particles called atoms. It then summarizes key discoveries and models proposed by scientists like Dalton, Thomson, Rutherford, Bohr, Schrodinger that refined our understanding of atomic structure, such as discovering the electron, proposing the planetary model of electrons orbiting the nucleus, and the wave mechanical model. The document also defines the basic subatomic particles of protons, neutrons and electrons, isotopes, and provides examples of how atomic mass and ions are related to atomic structure.
The document outlines the history of the atomic model from ancient Greek philosophers' idea of indivisible atoms to modern atomic structure. It discusses early atomic theorists like Democritus, Dalton, Thompson, Rutherford, and Bohr and how their work refined understanding of atoms. Key developments included discovering the electron and proposing nuclear and planetary models of the atom. The document then explains atomic structure, defining protons, neutrons, electrons, and their arrangement in shells according to electronic configuration and dot-and-cross diagrams.
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.
Atoms are too small to see even with a powerful microscope and too light to be weighed even on the most sensitive balance. The history of the discovery of the structure of an atom is fascinating but a complicated subject. Only 100 years ago, scientists believed that atoms were solid, indestructible particles. Since then many great scientists had contributed brilliantly to give us the today’s model of an atom. Over the centuries, many philosophers and scientists tried to develop a model of the atom.
All matters are in nature is made up of only a few elements. The elements exist as atoms and/or molecules. Molecules of an atom are made up of atoms of the same type. Compounds contain two or more elements. Thus, the molecules of compounds contain atoms of different elements.
The document outlines the history of the atomic model from ancient Greek philosophers to modern atomic theory. It describes early atomic theories from Democritus and Dalton who proposed atoms as indivisible and spherical particles. It then discusses the discoveries of J.J. Thompson, Rutherford, and Bohr that led to developments in atomic structure. Key developments included the discovery of the electron by Thompson, Rutherford's nuclear model from alpha scattering experiments, and Bohr's refinement incorporating electron orbits around the nucleus. The document concludes with explanations of atomic structure including electronic configurations and dot and cross diagrams.
All matters are in nature is made up of only a few elements. The elements exist as atoms and/or molecules. Molecules of an atom are made up of atoms of the same type. Compounds contain two or more elements. Thus, the molecules of compounds contain atoms of different elements.
https://thegeneralscience.com/atomic-structure-pdf/
Rutherford's experiment involved firing alpha particles at a thin gold foil. Most passed straight through, showing the atom is mostly empty space. Some were deflected, showing a small, dense central nucleus. Very few bounced straight back, showing the nucleus is very small compared to the atom. This led to the discovery of the nuclear model of the atom, with a small, dense nucleus surrounded by electrons.
Atomic and nuclear physics are related but distinct fields that describe the structure and behavior of atoms and their nuclei. Atomic physics deals with atoms as systems of electrons and an atomic nucleus, while nuclear physics focuses on the nucleus as a system of nucleons (protons and neutrons). A knowledge of these fields is important for nuclear engineers working with nuclear reactors. The document then provides details on the key topics in atomic and nuclear physics, including fundamental particles, atomic and nuclear structure, mass and energy, radiation, nuclear stability, radioactive decay, and nuclear reactions.
El documento describe brevemente la química del amor. Explica que el amor se ve afectado por procesos eléctricos y químicos en el cuerpo, como las hormonas y sustancias químicas en el cerebro y sistema endocrino. Luego resume algunas de las hormonas clave y glándulas endocrinas involucradas como la hipófisis, tiroides, paratiroides y suprarrenales.
Este documento presenta un resumen de conceptos astronómicos básicos como galaxias, estrellas, planetas y otros objetos del universo. Explica la estructura y evolución de las galaxias, estrellas y sistemas planetarios, así como conceptos como nebulosas, cúmulos estelares, supernovas y agujeros negros. El documento concluye con una breve descripción de los objetos del Sistema Solar como planetas, asteroides y cometas.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
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Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptxEduSkills OECD
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
Main Java[All of the Base Concepts}.docxadhitya5119
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
5. So, if string theory is correct, the entire
world is made of strings!
Perhaps the most remarkable thing about string
theory is that such a simple idea works.
But it should also be said that, to date, there is
no direct experimental evidence that string
theory itself is the correct description of Nature.
A important part has been verified
experimentally with incredible precision but not
the whole theory as it is still under development.
20. ANCIENT GREEK
PHILOSOPHY SCHOOLS
EMPEDOCLES & ARISTOTLE
All matter is a combination of 4 elements:
earth, water, air & fire
21. DDEEMMOOCCRRIITTUUSS
((446600 bb..cc.. –– 337700 bb..cc))
Proposed that matter was composed of
tiny indivisible particles = atoms
ATOM → from the greek a=without +
tomus = division
Not based on experimental data
22. Alchemy (next 2000 years)
Mixture of science and mysticism.
Lab procedures were developed, but
alchemists did not perform controlled
experiments like true scientists.
23. DDAALLTTOONN
((11880088))
British Schoolteacher
– based his theory on others’ experimental data
Billiard Ball Model
– atom is a
uniform,
solid sphere
(protons, neutron & electrons
not discovered yet!!!)
24. Dalton’s Four
Postulates
1. Elements are composed of small indivisible
particles called atoms. (*** not true)
2. Atoms of the same element are identical.
Atoms of different elements are different.
3. Atoms of different elements combine
together in simple proportions to create a
compound. (*)
4. In a chemical reaction,
atoms are rearranged,
but not changed.
25. TTHHOOMMSSOONN
11889977
Discovered Electrons = negative particles
within the atom → so atom divisible
Plum-pudding Model
“plum cake”
26. Plum-pudding Model
– positive sphere (pudding) with
negative electrons (plums) dispersed
throughout
– So,
atom = neutral
27. RRUUTTHHEERRFFOORRDD
11991111
Gold Foil Experiment
Discovered the nucleus
– Small, dense, positive
charge in the center of
the atom = nucleus
– Most of the atom
is empty
Nuclear Model
28. Nuclear Model
Small, dense, positive nucleus (with
protons) surrounded by negative electrons
(where?? not clear)
29. BBOOHHRR
11991133
- Energy Levels
– electrons can only exist in specific energy
states →
Planetary Model: electrons orbit the
nucleus, like planets orbiting the Sun.
31. SCHRÖDINGER
1926
Quantum mechanics
– electrons can only exist in specified energy
states
Electron cloud model
– ORBITAL: region around
the nucleus where e- are
likely to be found
32. CHADWICK
1932
Discovered neutrons
– neutral particles in the nucleus of an atom
33. ATOMIC STRUCTURE
So the ATOMIC STRUCTURE is:
made up of a central nucleus (containing
protons and neutrons), surrounded by
electrons in diferent shells. Most of the
atom is empty space.
38. NNUUCCLLII
The central nucleus contains protons
and neutrons
The atomic number (Z) is the number of
protons in an atom.
AAttoommiicc nnuummbbeerr
ZZ == pp++
39. TThhee aattoommiicc mmaassss nnuummbbeerr ((AA)) iiss tthhee
nnuummbbeerr ooff pprroottoonnss aanndd nneeuuttrroonnss iinn tthhee
nnuucclleeuuss ooff aann aattoomm..
MMaassss nnuummbbeerr
AA == pp++ ++ nn00
The standard notation that is used to
write an element, where X is the element
symbol, A is the atomic mass number and
Z is the atomic number.
40. Every element is distinguished from the orders bbeeccaauussee ooff iitt aattoommiicc
nnuummbbeerr,, tthheerreeffoorree bbeeccaauussee ooff iitt nnuummbbeerr ooff pprroottoonnss..
41. ISOTOPES
The isotope of a particular element is made up of atoms which
have the same number of protons as the atoms in the original
element, but a different number of neutrons. This means that not all
atoms of an element will have the same atomic mass.
They have = Z i ǂ A
42. The relative atomic mass of an
element is the average mass of all the
naturally occurring isotopes of that
element.
The units for relative atomic mass are
atomic mass units.
The relative atomic mass is written under
the elements' symbol on the periodic
table.
So, the relative atomic mass
has “comes”
43. Carbon-14 dating is a
way of determining the
age of certain archeological
artifacts of a biological
Origin up to about 50,000
years old.
It is used in dating things such
as bone, cloth, wood and plant fibers that
were created in the relatively recent past
by human activities.
51. The electrons in the outermost energy
level are called valence electrons.
The electrons in an atom that are not
valence electrons are called core
electrons.
53. Atoms whose outermost energy level is
full, are less chemically reactive and
therefore more stable, than those atoms
whose outermost energy level is not full.
These are the NOBLE GASOS
54. The other elements are unstable and need
to gain, lose or share valence electron in
order to be more energetically stable.