Chemistry 12 Definitions

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21 Terms

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alpha Particles

negatively charged particles

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beta Particles

postively charged particles

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gamma radiation

electromagnetic energy

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Light

a form of EM radiation 

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Quanta

fixed value of energy

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photon

a packet of light

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Emission or line spectrum

a series of lines of different colored lights emitted by atoms of a specific element as they lose excitation energy

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Isoelectronic

same electron configuration = same number of electrons

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Aufbau Principle (building up)

electrons are added to the lowest energy orbital

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Pauli Exclusion Principle

an orbital can be empty have one electron or have two electrons at most

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Hunds Rule

electrons in the same sub-level will not pair up until all orbitals in the sub-level are half filled.

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Carbon atoms

has four valence electrons, it can form covalent bonds with four other atoms. A property which allows it to be bonded with a wide variety of molecules. 

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Linus Pauling

developed the valence bond theory

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Valence bond theory

atomic orbitals or hybrid orbitals overlap to form a new orbital 

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Crystal lattice

a regular repeating pattern of atoms, ions, or molecules in a crystal. 

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Isomers

chemicals with the same molecular formula but different structural diagrams and different names.

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Constitutional Isomers

same molecular formular but different sequence. 

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Diastereomer

differ in structure only by the position of groups with double bonds (cis & trans).

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Functional group

a special arrangement of atoms that is responsible for the chemical behavior of a molecule.

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Markinov’s rule

hydrogen bonds to atom with more hydrogen atoms (the rich gets richer) 

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Le Chatelier’s Principle

When a chemical system at equilibrium is disturbed by a change in property, the system adjusts in a way that opposes the change.