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Vocabulary Unit 2

Periodic Trends

TermDefinition
Coulomb's Law =The force of attraction between charged particles depends on the amount of charge and the distance between them. Greater charge creates stronger attraction and greater distance creates weaker attraction.
Electron Shielding The blocking effect of inner electrons that reduces the attraction between the nucleus and the valence electrons.
Effective Nuclear Charge (Zeff)The net positive charge felt by an electron after accounting for electron shielding. A greater effective nuclear charge pulls electrons closer to the nucleus. The net positive charge felt by an electron after accounting for electron shielding. A greater effective nuclear charge pulls electrons closer to the nucleus.
Ionization EnergyThe energy required to remove an electron from a gaseous atom or ion. The energy required to remove an electron from a gaseous atom or ion.
First Ionization EnergyThe energy required to remove the first electron from a neutral gaseous atom. The energy required to remove the first electron from a neutral gaseous atom.
Successive Ionization Energy The energy required to remove additional electrons one at a time after the first electron has been removed. A large increase occurs when a core electron must be removed.
Photoelectron Spectroscopy (PES) A method that uses light to remove electrons from atoms and measure their binding energies to determine electron arrangement. A method that uses light to remove electrons from atoms and measure their binding energies to determine electron arrangement.
Binding Energy The energy required to remove an electron from an atom. Electrons held more strongly by the nucleus have greater binding energy.
Periodicity The repeating pattern of element properties that occurs across the periodic table.
Ionic Configuration The arrangement of electrons in an ion after an atom gains or loses electrons.
Isoelectronic Series A group of atoms or ions that have the same number of electrons but different numbers of protons. More protons results in a stronger attraction and smaller radius.
Atomic Radius The size of an atom based on the distance between its nucleus and outer electron cloud. Atomic radius decreases from left to right across a period and increases down a group.
Ionic Radius The size of an ion. Cations are smaller than their neutral atoms while anions are larger than their neutral atoms.
Electronegativity The ability of an atom to attract shared electrons in a chemical bond. Electronegativity increases from left to right across a period and decreases down a group.
Electron Affinity The energy change that occurs when a neutral gaseous atom gains an electron.
Anion A negatively charged ion formed when an atom gains electrons.
Cation A positively charged ion formed when an atom loses electrons.
Core Electrons Electrons in the inner energy levels that shield valence electrons from the full attraction of the nucleus.
Law of Conservation of Energy Energy cannot be created or destroyed. It can only be transferred or changed from one form to another.
Law of Conservation of Mass Matter cannot be created or destroyed during a chemical reaction. The total mass of the reactants is the same as the total mass of the products.
Ground State The lowest energy arrangement of electrons in an atom.
Ionization The process in which an atom gains or loses electrons and becomes an ion.
Octet Rule The tendency of atoms to gain lose or share electrons to obtain eight valence electrons and become more stable.
Created by: user-1920943
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