Isotopes
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The document discusses how to use the periodic table to find information about the element iodine (I). It provides iodine's number of protons (53), electrons (53), neutrons (74), energy shells (5), and valence electrons (7). It also explains that isotopes are atoms of the same element that have different numbers of neutrons, and how to calculate the number of neutrons using the atomic number and mass.
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The document contains questions about various topics in chemistry including:
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When a neutral atom loses or gains electrons, it is no longer neutral. It becomes an ion that has a positive or negative charge depending on whether electrons were lost or gained:
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing or gaining electrons changes a neutral atom's charge balance between protons and electrons, making it an ion that is positively or negatively charged. The number of protons does not change, only the number of electrons.
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Unit 1 lesson 12ppt
When a neutral atom loses or gains electrons, it is no longer electrically balanced. It will have either a positive or negative charge depending on whether it lost or gained electrons.
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing electrons creates a positive ion and gaining electrons creates a negative ion. The charge depends on the relative numbers of protons and electrons after gaining or losing electrons from the neutral atom.
Atomic structure part 1 fundamental particles
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.
Isotopes
Isotopes are atoms of the same element that have different numbers of neutrons. They have the same number of protons and electrons, so they have the same chemical properties. Some isotopes are stable while others are unstable and radioactive. Both stable and radioactive isotopes occur naturally, but radioisotopes are also produced artificially. Radioisotopes have important applications in medicine, industry, research and other areas due to their radioactive properties.
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Atomic weight is the weighted average mass of an element's naturally occurring isotopes. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The number of protons defines an element and never changes, while the number of neutrons can vary between isotopes of an element. Isotopes are represented by a symbol noting the number of protons and neutrons.
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The document contains questions about various topics in chemistry including:
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3) Structure of atoms including electrons, protons, neutrons, isotopes and the periodic table.
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When a neutral atom loses or gains electrons, it is no longer neutral. It becomes an ion that has a positive or negative charge depending on whether electrons were lost or gained:
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
So in summary, losing or gaining electrons changes a neutral atom's charge balance between protons and electrons, making it an ion that is positively or negatively charged. The number of protons does not change, only the number of electrons.
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This document discusses molecular geometry and polarity using valence shell electron pair repulsion (VSEPR) theory and hybridization theory. It begins by explaining the objectives and defining molecular polarity in terms of bond polarity and molecular geometry. It then applies VSEPR theory to predict the shapes of different molecules and polyatomic ions. The document continues by introducing hybridization theory to explain bonding orbitals and different hybridizations like sp3, sp2, and sp. It concludes by describing various intermolecular forces like dipole-dipole forces, hydrogen bonding, London dispersion forces, and how they relate to boiling points.
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When a neutral atom loses or gains electrons, it is no longer electrically balanced. It will have either a positive or negative charge depending on whether it lost or gained electrons.
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
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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.
Isotopes
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Physics 22 - The Nuclear Atom.pptx
1) Atoms consist of a small, dense nucleus surrounded by electrons. The nucleus contains positively charged protons and neutral neutrons, while electrons are negatively charged and orbit the nucleus.
2) The number of protons determines the element and is known as the atomic number. The total number of protons and neutrons is the mass number. Isotopes are atoms of the same element with different numbers of neutrons.
3) Evidence for the nuclear model includes Rutherford's gold foil experiment, which showed that most alpha particles passed through but some were deflected at large angles, indicating a small, dense nucleus.
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Atoms and the periodic table
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The document provides information about the structure of atoms, including:
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Physical science 4.2 : The Atom
1) An atom is the smallest particle of an element and is approximately 0.00000003 cm in diameter.
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The document discusses the structure of atoms and their subatomic particles. It defines atoms as consisting of a nucleus surrounded by electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. Atoms are made up of subatomic particles including protons, neutrons and electrons. Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Isotopes are defined as atoms of the same element that have the same number of protons but different numbers of neutrons. The periodic table arranges elements in order of increasing proton number and groups elements with similar chemical properties together.
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The document provides an overview of key concepts in atomic structure and chemical bonding. It defines the electron cloud model and notes electrons are found in energy levels around the nucleus. The nucleus contains protons and neutrons, which are similar in size. An element is defined by its atomic number, while isotopes have different numbers of neutrons. Atoms form ionic bonds by gaining or losing electrons or covalent bonds by sharing electrons. Metals bond through metallic bonds and are found on the left side of the periodic table, while nonmetals are on the right and form ionic or covalent bonds.
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This document provides an overview of a 10th grade chemistry lesson on atoms, isotopes, and atomic mass. The objectives are for students to understand isotopes, the difference between chemical and nuclear reactions, and three types of nuclear decay. An interactive simulation is used to teach students about building atoms and isotopes. The lesson includes defining isotopes using subatomic particles, finding isotope names and masses, calculating average atomic mass from isotope data, and common uses of radioactive isotopes. Videos and activities reinforce these concepts.
isotopes
This document discusses isotopes and their properties. It defines isotopes as forms of the same element that have different numbers of neutrons but the same number of protons. It provides examples of carbon isotopes and explains that isotope notation specifies the element name or symbol followed by the mass number. Isotopes can be naturally occurring or artificially made, and they have various medical and dating uses. The document also includes questions to test the reader's understanding of isotopes.
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This presentation provides information about atoms and atomic structure through a series of slides:
1. It begins with slides introducing John Dalton's atomic theory from the 1800s and experiments by Thomson, Rutherford, and Bohr that led to discoveries about the electron and nuclear structure of atoms.
2. Later slides discuss the composition of atoms in terms of protons, neutrons, and electrons, and define key terms like isotope, atomic number, and mass number.
3. The presentation concludes by explaining the four fundamental forces that govern atomic structure and providing a concept map to summarize what was learned about atoms.
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The periodic table is a chart that arranges the elements by atomic number in rows and columns according to their chemical and physical properties. It provides important information about each element, such as the number of protons, neutrons, and electrons. The position of an element on the periodic table can reveal whether it is a metal or nonmetal based on its location left or right of the zigzag line. Metals are generally solids, shiny, ductile, malleable, good conductors of heat and electricity, and have high melting points. Compounds are formed when atoms of different elements bond together chemically, resulting in a substance with different properties than the individual elements.
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The document provides information about atomic structure including:
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This document provides an overview of atomic structure and the periodic table. It discusses key topics including:
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- Atoms contain protons, neutrons, and electrons. The number of protons determines an element's identity.
- Isotopes are atoms of the same element with different numbers of neutrons.
- Electrons can have distinct energy levels, emitting light of specific frequencies when changing levels.
- The periodic table arranges elements by proton number and electron configuration in shells.
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This document summarizes key concepts from Chapter 4 on atomic structure:
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2) It outlines the discovery of subatomic particles like electrons, protons, and neutrons through experiments by Thomson, Rutherford, and Chadwick.
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Isotopes
- 1. Use the periodic table to find the missing information Iodine (I) 1.Number of protons 2.Number of electrons 3.Number of neutrons 4.Number of energy shells 5.Number of valence electron(s) 53 53 74 5 7
- 2. ReviewReview Elements Periodic Table Trends and patterns on the table
- 4. IsotopesIsotopes Atoms of the same element withAtoms of the same element with different numbers of neutronsdifferent numbers of neutrons They also have a differentThey also have a different atomic mass than the majorityatomic mass than the majority
- 5. IsotopesIsotopes The atomic number tells you: The number of protons and The number of electrons 13 Al Aluminum 26.98
- 6. IsotopesIsotopes Number of neutrons? Atomic mass minus the atomic number Atomic mass to the nearest whole number! 13 Al Aluminum 26.98
- 7. IsotopesIsotopes Number of neutrons? Atomic mass minus the atomic number Atomic mass to the nearest whole number! 13 Al Aluminum 26.98