Subatomic Particles 2008
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tamsThis document defines and describes subatomic particles like protons, neutrons, and electrons. It explains that atoms are made up of these subatomic particles, with protons and neutrons located in the atomic nucleus and electrons in orbitals outside the nucleus. The document also discusses atomic number, mass number, and isotopes, providing examples of writing out the number of protons, neutrons, and electrons for different atoms and ions.
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The three subatomic particles
1) Michael Faraday discovered cathode rays (now known as electrons) in 1838 through experiments with glass tubes containing rarefied air and electrodes.
2) The experiment showed a strange luminous arc near the anode and a dark space near the cathode, marking the beginning of research into cathode rays.
3) Other scientists like J.J. Thomson, R.A. Millikan, and J. Chadwick later discovered the subatomic particles proton, electron, and neutron through discharge tube and oil drop experiments.
Isotopes
This document discusses isotopes and atomic structure. It defines isotopes as atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes have the same chemical properties but slightly different physical properties. The document also discusses nucleon number, which is the total number of protons and neutrons in an atom's nucleus. The mass number equals the nucleon number. Radioactive isotopes are unstable and undergo nuclear decay over time into stable daughter isotopes.
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This document provides instructions for calculating the abundance of different isotopes within an element. It explains key concepts such as atomic mass, isotopes, and using proportions to calculate isotope percentages. As an example, it shows the calculation to find the percentage abundance of carbon-12 isotope. The document also provides sample exam questions and instructions for a student presentation on a given element.
Elements, compounds, molecules and subatomic particles
This document defines and describes the basic concepts of elements, compounds, molecules, and subatomic particles. It states that elements are substances made of atoms with the same number of protons, while compounds contain atoms of different elements chemically combined in fixed ratios. Molecules are the smallest units that retain a compound's characteristics. The three main subatomic particles are protons, neutrons, and electrons, which make up atoms. The document also provides examples and properties of these scientific terms.
Isotopes & Atomic Mass
Magnesium has three naturally occurring isotopes: magnesium-24, magnesium-25, and magnesium-26. They have the same number of protons and electrons but different numbers of neutrons, giving them different atomic masses. Magnesium-24 makes up 79% of magnesium and has the greatest influence in calculating magnesium's average atomic mass of 24.3 amu.
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Thank you for the report. I learned a lot about radioactive isotopes and their decay processes.
3.2 structure of atoms
- Thompson discovered electrons using cathode ray tubes. Rutherford discovered the nucleus and that it is positively charged through gold foil experiments.
- Chadwick discovered neutrons by observing particles in a beam that were not deflected by a magnetic field.
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit the nucleus. The number of protons defines the element.
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1) Michael Faraday discovered cathode rays (now known as electrons) in 1838 through experiments with glass tubes containing rarefied air and electrodes.
2) The experiment showed a strange luminous arc near the anode and a dark space near the cathode, marking the beginning of research into cathode rays.
3) Other scientists like J.J. Thomson, R.A. Millikan, and J. Chadwick later discovered the subatomic particles proton, electron, and neutron through discharge tube and oil drop experiments.
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This document discusses isotopes and atomic structure. It defines isotopes as atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes have the same chemical properties but slightly different physical properties. The document also discusses nucleon number, which is the total number of protons and neutrons in an atom's nucleus. The mass number equals the nucleon number. Radioactive isotopes are unstable and undergo nuclear decay over time into stable daughter isotopes.
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Elements, compounds, molecules and subatomic particles
This document defines and describes the basic concepts of elements, compounds, molecules, and subatomic particles. It states that elements are substances made of atoms with the same number of protons, while compounds contain atoms of different elements chemically combined in fixed ratios. Molecules are the smallest units that retain a compound's characteristics. The three main subatomic particles are protons, neutrons, and electrons, which make up atoms. The document also provides examples and properties of these scientific terms.
Isotopes & Atomic Mass
Magnesium has three naturally occurring isotopes: magnesium-24, magnesium-25, and magnesium-26. They have the same number of protons and electrons but different numbers of neutrons, giving them different atomic masses. Magnesium-24 makes up 79% of magnesium and has the greatest influence in calculating magnesium's average atomic mass of 24.3 amu.
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Thank you for the report. I learned a lot about radioactive isotopes and their decay processes.
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- Thompson discovered electrons using cathode ray tubes. Rutherford discovered the nucleus and that it is positively charged through gold foil experiments.
- Chadwick discovered neutrons by observing particles in a beam that were not deflected by a magnetic field.
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit the nucleus. The number of protons defines the element.
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Structure of the atoms
1) Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are in the nucleus, while electrons orbit the nucleus in shells.
2) Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same chemical properties.
3) Electrons fill the lowest available shell around the nucleus. The arrangement of electrons is shown in an element's electronic structure.
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This document summarizes key information about subatomic particles including protons, neutrons, electrons, isotopes, and ions.
Protons have a positive charge and are found in the nucleus. Neutrons have no charge and are also found in the nucleus. Electrons have a negative charge and are found outside the nucleus.
The number of protons determines the element. The number of neutrons can vary between isotopes of the same element. Isotopes are identified using hyphen or nuclear notation. To find the number of neutrons in an isotope, subtract the atomic number from the atomic mass.
The number of electrons in a neutral atom equals the number of protons. Ions have a different number of electrons than
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The document discusses the structure and composition of atoms. It can be summarized as follows:
1) Atoms have a small, dense nucleus containing protons and neutrons, surrounded by an electron cloud where electrons are found.
2) The number of protons determines the element, and protons plus neutrons equals the mass number. Electrons equal protons for neutral atoms.
3) Atoms can gain or lose electrons to become ions with a positive or negative charge.
4) Isotopes of the same element have different numbers of neutrons but the same number of protons.
subatomic particles
Protons, neutrons, and electrons are the three main subatomic particles. Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The atomic number identifies the number of protons in an atom's nucleus, while atomic mass refers to the total number of protons and neutrons.
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1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
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Atoms are composed of protons, neutrons, and electrons. Protons and neutrons have mass while electrons have negligible mass. The number of protons is the atomic number and the total number of protons and neutrons is the mass number. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same atomic number and chemical properties. Examples provided are the isotopes of carbon, chlorine, and their atomic and mass numbers.
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The document explains how to determine the number of protons, electrons, and neutrons in an atom. It provides examples using the elements krypton, oxygen, xenon, and zirconium. For each element, the number of protons is equal to its atomic number. The number of electrons equals the number of protons. And the number of neutrons is calculated by taking the mass number and subtracting the number of protons.
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The document provides information about the fundamental particles that make up atoms, including protons, neutrons, electrons, and isotopes. It defines key atomic properties such as atomic number, which is the number of protons in an atom's nucleus, and mass number, which is the total number of protons and neutrons. It notes that atoms of the same element can have different numbers of neutrons, making them isotopes. As an example, it provides the particle makeup of several carbon isotopes: 12C, 13C, and 14C.
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To determine the subatomic particles of an atom, one must:
1. Gather the atomic number and mass, with the number representing protons and electrons and mass representing total protons and neutrons.
2. Identify protons as equal to the atomic number.
3. Identify electrons as equal to protons to maintain neutral charge.
4. Calculate neutrons by subtracting the atomic number from the rounded atomic mass.
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1) The document discusses the structure of atoms including subatomic particles like protons, neutrons, and electrons.
2) Atoms of the same element have the same number of protons but may have different numbers of neutrons, forming isotopes of that element.
3) The atomic number represents the number of protons in an atom, while the mass number counts both protons and neutrons.
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1) The document discusses the structure of atoms including subatomic particles like protons, neutrons, and electrons.
2) Atoms of the same element have the same number of protons but may have different numbers of neutrons, forming isotopes of that element.
3) The atomic number represents the number of protons in an atom, while the mass number counts both protons and neutrons.
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1) Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are in the nucleus, while electrons orbit the nucleus in shells.
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1) Atoms have a small, dense nucleus containing protons and neutrons, surrounded by an electron cloud where electrons are found.
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3) Atoms can gain or lose electrons to become ions with a positive or negative charge.
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1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
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Atoms are composed of protons, neutrons, and electrons. Protons and neutrons have mass while electrons have negligible mass. The number of protons is the atomic number and the total number of protons and neutrons is the mass number. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same atomic number and chemical properties. Examples provided are the isotopes of carbon, chlorine, and their atomic and mass numbers.
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The document explains how to determine the number of protons, electrons, and neutrons in an atom. It provides examples using the elements krypton, oxygen, xenon, and zirconium. For each element, the number of protons is equal to its atomic number. The number of electrons equals the number of protons. And the number of neutrons is calculated by taking the mass number and subtracting the number of protons.
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The document provides an overview of different types of alternative energy sources including renewable and non-renewable resources. It discusses key topics such as fossil fuels, nuclear energy, solar energy, wind energy, geothermal energy, hydroelectric energy, and biomass energy. For each type of energy, it covers concepts like energy sources, processes, advantages, disadvantages, and major historical events. The goal is to provide students with essential information to study alternative energy topics.
We've got the power instructions and rubric
Students will be split into groups and assigned a US state. They must research which single energy source (e.g. solar, wind, coal) would best power their assigned state. Groups will present their findings and reasoning in a PowerPoint or Glogster. The project aims to answer "If you were starting a town that could only run on one type of energy source, what energy source would you use and why?". Students will be graded on selecting an energy source, justifying their choice, and presenting their research.
Biomass energy
This document discusses biomass energy, identifying fuels like trees, grasses, crops and residues that can be used, and describing how biomass produces electricity by heating water into steam to turn a turbine. It lists current uses of biomass as ethanol, space heating and cooking, and notes pros as biomass being available worldwide and potentially sustainable, while cons include needing fossil fuels for harvesting and transport and high production costs.
Hydroelectric power
Hydroelectric energy is electricity generated from flowing water, which is influenced by gravity to turn turbines at hydroelectric dams and plants. The largest hydroelectric plant is China's Three Gorges Dam, while the largest in the US is the Grand Coulee Dam in Washington. Hydroelectric power has advantages like longevity and lack of pollution but also disadvantages like high costs, potential for damage if not built correctly, and geological effects of large dams.
Solar energy
The document discusses solar energy, explaining that the sun produces energy through nuclear fusion, and that this energy radiates from the sun as light. It describes how solar panels can collect the sun's energy by using photovoltaic cells to convert sunlight into electricity or heat. Finally, it notes that solar energy would be most profitable in areas that receive strong, consistent sunlight and have the space needed for large solar installations.
Nuclear power plants
The document summarizes the key components and process of a nuclear power plant. It describes how nuclear fission in the core produces heat that is used to heat water into steam in a heat exchanger. The steam then powers turbines that generate electricity. After being used, the steam is cooled, usually using water or air, and the cycle repeats. A limiting factor of nuclear power is that the radioactive waste from uranium and plutonium fuel takes thousands of years to become stable, posing challenges for long-term storage and disposal.
Nuclear energy
This document summarizes key aspects of nuclear energy including: how nuclear fission produces energy from atoms; the most common nuclear fuels of uranium and plutonium; the two major nuclear accidents being Three Mile Island in the US and Chernobyl in Ukraine; and both the advantages of nuclear providing large amounts of energy without air pollution and the disadvantages of nuclear waste and use of non-renewable resources.
Fossil fuels
The document discusses the three main types of fossil fuels - petroleum, natural gas, and coal. It explains how they were formed from ancient plant and animal matter, and their different characteristics and uses. It also addresses the dangers of burning fossil fuels and ideas for conservation, since fossil fuels are non-renewable resources that could run out within a century if not properly managed.
2010 Speed And Velocity
Distance is the separation between positions, time is the period between events, and speed is a measure of how fast an object moves and changes position. Speed is calculated as distance divided by time and is commonly measured in meters per minute or kilometers per hour. Velocity differs from speed in that it includes both the speed of an object's motion as well as its direction.
2010 Motion
This document discusses frames of reference and their use in describing position and motion. It defines key terms like position, frame of reference, and motion. The most common frame of reference is the earth, but frames can also include moving objects like cars, cameras, or airplanes. Motion is described as a change in position relative to the chosen frame of reference.
Collaboration
This document lists various tools for video conversion, adding video capabilities to web browsers, downloading video add-ons, sharing presentations, using open source office software, and creating and sharing documents and presentations online for free. It also provides the URL for the class wiki site that will be used to distribute tutorials and showcase student work.
2010 Balancing Equations
This document discusses balancing chemical equations by making the number of atoms equal on both sides of the equation. It explains that chemical equations depict the reactants and products of a reaction and their relative amounts. It also discusses that chemical equations must be balanced according to the law of conservation of mass, so that the same number of atoms of each element exist on both sides of the balanced equation. Coefficients are used to balance equations by adjusting the relative quantities of compounds, but subscripts cannot be changed.
Periodic Table Project
The document provides requirements and guidelines for a periodic table unit project where students create a "Wanted" poster for a chosen element. The poster must be half a standard poster board size and include: an illustration of the element or its uses; descriptions in the student's words of the element's "crimes," aliases, physical properties, discoverer, discovery details, location, common compounds and reactivity, dangers, and a picture; and be neatly presented with correct spelling. Sections are worth various point values totaling 100 points.
Periodic Table Project
The document provides requirements and guidelines for a periodic table unit project where students create a "Wanted" poster for a chosen element. The poster must be half a standard poster board size and include an illustration of the element. It should contain 9 items of information written in the student's own words: 1) what the element is "wanted for", 2) aliases, 3) a description, 4) the discovering officer, 5) the discovery report, 6) where it was last seen, 7) known associates, 8) a warning label, and 9) a picture. Each item is worth a certain number of points out of a total 100.
2009 Compounds2
The document provides information about chemical compounds and formulas:
1. It defines a compound as two or more elements chemically joined together to form a new substance with different properties than the elements.
2. It explains that a molecule is the smallest piece of a compound that retains the compound's properties.
3. It describes how chemical formulas use subscripts to indicate the number of atoms of each element in a compound, and coefficients to indicate the number of molecules.
Reactions2010
The document discusses chemical reactions and the four main types: synthesis, decomposition, single replacement, and double replacement. It defines key terms like reactants and products. Synthesis reactions combine two elements to form a compound. Decomposition reactions involve a single reactant breaking down into simpler products. Single replacement reactions involve one element replacing another in a compound. Double replacement reactions swap ions between two compounds. The law of conservation of mass is also mentioned.
Classification Of Elements
This document describes how elements are classified and organized on the periodic table. It defines metals, nonmetals, and metalloids, and explains their characteristic properties. Metals are shiny, solid conductors that are malleable and ductile, while nonmetals exhibit varying states, are dull, and are poor conductors. Metalloids have some properties of both. Elements are arranged vertically in groups with the same number of valence electrons and horizontally in periods with the same number of electron shells. The periodic law states that properties repeat periodically with increasing atomic number.
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