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alpha Particles
negatively charged particles
beta Particles
postively charged particles
gamma radiation
electromagnetic energy
Light
a form of EM radiation
Quanta
fixed value of energy
photon
a packet of light
Emission or line spectrum
a series of lines of different colored lights emitted by atoms of a specific element as they lose excitation energy
Isoelectronic
same electron configuration = same number of electrons
Aufbau Principle (building up)
electrons are added to the lowest energy orbital
Pauli Exclusion Principle
an orbital can be empty have one electron or have two electrons at most
Hunds Rule
electrons in the same sub-level will not pair up until all orbitals in the sub-level are half filled.
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.
Linus Pauling
developed the valence bond theory
Valence bond theory
atomic orbitals or hybrid orbitals overlap to form a new orbital
Crystal lattice
a regular repeating pattern of atoms, ions, or molecules in a crystal.
Isomers
chemicals with the same molecular formula but different structural diagrams and different names.
Constitutional Isomers
same molecular formular but different sequence.
Diastereomer
differ in structure only by the position of groups with double bonds (cis & trans).
Functional group
a special arrangement of atoms that is responsible for the chemical behavior of a molecule.
Markinov’s rule
hydrogen bonds to atom with more hydrogen atoms (the rich gets richer)
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.