Chemistry: Unit 3, Atomic Structure, Theory, & Electron Configuration Answers – Flashcards
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De Brogile
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suggested that electrons be considered waves confined to the space around an atomic nucleus.
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uncertainty principle
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States that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time
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Moseley
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contribution to the science of physics was the justification from physical laws of the previous empirical and chemical concept of the atomic number
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Pauli
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physicist noted for his work on spin theory and quantum theory, and for the important discovery of the Pauli exclusion principle, which underpins the structure of matter and the whole of chemistry.
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Cannizzaro
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he discovered that aromatic aldehydes are decomposed by an alcoholic solution of potassium hydroxide into a mixture of the corresponding acid and alcohol
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Periodic Law
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the law that states that the repeating chemical and physical properties of elements change periodically with the atomic numbers of the elements
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Ionic Radius
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The radius exhibited by an ion in an ionic crystal where the ions are packed together to a point where their outermost electronic orbitals are in contact with each other
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Aufbau
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Each electron occupies the lowest energy orbital available
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Wave-particle duality
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The behaviors of the electron does not allow for it to be observable as a particle and as a wave. The two sided nature of the electron is known as the Wave-Particle Duality: The property of particles behaving as waves and the property of waves behaving as particles as well as waves.
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Schrodinger
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significant work—in quantum statistics, the dynamics of crystal lattices, the theory of color vision, and quantum theory.
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electron cloud
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used to describe where electrons are when they go around the nucleus of an atom.
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exclusion principle
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A maximum of two electrons can occupy a single atomic orbital, but only if the electrons have opposite spins
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Mendeleev
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most important contributor to the development of the periodic table. His version of the periodic table organized elements into rows according to their atomic mass and into columns based on chemical and physical properties.
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Periodic table
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a table of the chemical elements arranged in order of atomic number, usually in rows, so that elements with similar atomic structure (and hence similar chemical properties) appear in vertical columns.
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ionization energy
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the amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated gaseous atom to form a cation.
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Hund
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German physicist known for his work on the electronic structure of atoms and molecules. He helped introduce the method of using molecular orbitals to determine the electronic structure of molecules and chemical bond formation.
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Hund's rule
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Single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals
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Heisenberg
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German physicist and philosopher who is noted for his crucial contributions to quantum mechanics. He devised a method to formulate quantum mechanics in terms of matrices
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Quantum number
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Indicates the relative size and energy of atomic orbitals
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sublevel
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an electron orbital. Sublevels are designated s, p, d or f. These sublevels or orbitals have characteristic shapes which can be used to explain and predict the chemical bonds that atoms can form.
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Lewis dot diagram
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diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.
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electronegativity
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a measure of the tendency of an atom to attract a bonding pair of electrons
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atomic radius
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of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding cloud of electrons.
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electron affinity
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the amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion.
