periodic properties and trends
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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.
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1. The document discusses periodic trends in atomic properties such as size, ionization energy, and electron affinity across the periodic table.
2. Key periodic trends described include decreasing atomic size and increasing ionization energy from left to right across a period, and decreasing ionization energy from top to bottom in a group.
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1) Atomic radius decreases across a period as atomic number increases, leading to higher effective nuclear charge and stronger attraction of the nucleus. Atomic radius increases down a group as shielding electrons increase.
2) Ionization energy increases across a period as effective nuclear charge increases, making it harder to remove electrons. Ionization energy decreases down a group as shielding increases and atomic radius gets larger.
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Periodic Trends
Dimitri Mendeleev was the first to publish an organized periodic table of elements in 1869. He understood the periodic law - that elements arranged by atomic number display a repeating pattern of chemical and physical properties in vertical columns due to their valence electrons. Mendeleev even predicted properties of undiscovered elements, which were later confirmed. The periodic table shows trends in atomic radius, ionization energy, electron affinity, and electronegativity that relate to chemical reactivity. Metals are on the left and are characterized by properties like conductivity, while nonmetals are on the right and have opposing properties.
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The document discusses several periodic trends:
1. Atomic radius generally increases moving down a group and decreases moving across a period, due to shielding and nuclear charge effects.
2. Ionization energy increases moving across a period as the effective nuclear charge increases, and decreases moving down a group as the distance from the nucleus increases.
3. Electronegativity increases moving across a period as it is easier to gain than lose electrons, and decreases moving down a group with increased atomic radius.
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The document summarizes the development and key features of the periodic table. It traces how early scientists like Newlands and Mendeleev organized the elements and developed periodic trends. The modern periodic table is arranged by atomic number and contains metals, nonmetals, and metalloids organized into blocks and groups. Elements in the same group have similar properties due to their electron configurations, and properties vary periodically according to trends like atomic radius and ionization energy.
Ppt periodic trends
The document discusses the periodic table, its history, organization, and the trends in various elemental properties that can be predicted from it. The periodic table was developed by Mendeleev in 1869 and organizes elements by atomic number. It allows prediction of trends in properties like atomic radius, ionization energy, and electronegativity across periods and down groups. The periodic table classifies elements as metals, nonmetals, metalloids and noble gases and notes important families like alkali metals, alkaline earth metals, and halogens.
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The document summarizes the development and key features of the periodic table. It discusses how early chemists like Newlands, Meyer, and Mendeleev arranged elements in order of atomic mass and properties, recognizing repeating patterns. Mendeleev predicted new elements and Moseley later arranged elements by atomic number. The periodic table is organized into blocks by electron configuration and periods and groups that demonstrate trends in properties. Metals are on the left, nonmetals on the right, and metalloids border the stair-step line between them.
Periodic trends
This document defines and discusses several periodic properties including atomic and ionic radii, ionization energy, electron affinity, and electronegativity. It states that atomic radii decrease across a period and increase down a group due to the increasing nuclear charge and electron cloud size. Ionization energies increase across a period as it is harder to remove electrons that are closer to the nucleus, and decrease down a group as the electrons are farther away. Electron affinity and electronegativity generally increase across periods and decrease down groups due to the effective nuclear charge and electron distance from the nucleus. Valence electrons are the outermost electrons involved in bonding, with atoms seeking to obtain a full outer shell of 8 electrons.
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Unit 1-electrochemistrymaterial
1. Electrochemistry deals with chemical applications of electricity and electrical conductance.
2. There are two types of electrical conductors: metallic and electrolytic. Metallic conductors involve electron movement while electrolytic conductors involve ion movement in solutions.
3. A galvanic cell generates electricity from a spontaneous redox reaction. It consists of two half-cells, each with a different metal electrode immersed in solutions separated by a salt bridge. Electrons flow from the anode where oxidation occurs to the cathode where reduction occurs.
ELECTRON-theory ppt industrials arts part2
Electron theory aims to explain the structure and properties of matter through its electronic structure. It states that all matter is comprised of molecules made up of atoms, which contain protons, neutrons, and electrons. Electrons play a key role in electricity as their movement constitutes electric current. Within atoms, electrons exist in specific energy levels or shells around the nucleus, and their behavior is described by quantum mechanics.
8 152-2-7-2011 slides
Spectroscopy techniques provide information about different regions of the electromagnetic spectrum:
1) Radio astronomy studies radio waves and is used for molecular vibrations.
2) Infrared studies bond interactions and is characteristic of molecular compounds.
3) Visible light energizes electrons.
4) Ultraviolet light energizes electrons and can ionize electrons.
5) X-rays can knock off interior electrons and is used for X-ray diffraction of crystal structures.
6) Gamma rays study nuclear energy states.
Lecture 14
The document discusses key concepts related to electrical conduction, including:
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2) How available electron energy states change from atoms to molecules to solids, and how this impacts conductivity. Band structures determine whether a material is a metal, semiconductor, or insulator.
3) Factors that influence resistivity like temperature, impurities, and defects. Electronic structure and scattering events are important to understanding variations in conductivity between materials.
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- 1. Presented by: Dave Rushel T. Romero
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