vocab for atoms
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| Electromagnetic radiation | a form of energy that exhibits wavelike behavior as it travels through space.
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| Electromagnetic spectrum | all the forms of electromagnetic radiation.
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| Wavelength | the distance between corresponding points on adjacent waves.
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| Frequency | the number of waves that pass a given point in a specific time, usually one second.
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| Visible Light | reflect IR light and transmit visible.
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| Velocity of a wave | distance traversed by a periodic, or cyclic, motion per unit time (in any direction).
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| photoelectric effect | the emission of electrons from a metal when light shines on the metal.
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| quantum | the minimum quantity of energy that can be gained or lost by an atom.
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| Planck’s Constant | is a physical constant reflecting the sizes of quanta in quantum mechanics.
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| Photon | a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy.
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| Energy of a Photon | symbolized by hv.
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| Ground State | the lowest energy state of an atom.
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| Excited State | a state in which an atom has a higher potential energy than it has in its ground state.
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| Line emission spectrum | a series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is shines through a prism.
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| continuous spectrum | the emission of a continuous range of frequencies of electromagnetic radiation.
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| Bohr radius | the radius of the ground state orbit of the hydrogen atom in the bohr theory.
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| Interference | in physics the superpostion of two or more waves resulting in a new wave pattern.
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| Heisenberg Uncertainty Principle | it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.
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| Quantum Theory | a mathematical description of the wave properties of electrons and other very small particles.
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| Quantum Mechanics | a mathematical description of the wave properties of electrons and other very small particles.
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| Orbital | a threedimensional region around the nucleus that indicates the probable location of an electron.
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| Quantum numbers | a number that specifies the properties of atomic orbitals and the properties of electrons in orbitals.
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| Principle Quantum number (n) | the quantum number that indicates the main energy level occupied by the electron.
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| Angular momentum quantum number (l ) | the quantum number that indicates the shape of the orbital.
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| Magnetic quantum number (m) | the quantum number that indicates the orientation of an orbital around the nucleus.
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| Spin quantum number (s) | the quantum number that has only two possible values, + ½ and
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| Aufban Principle | an electron occupies the lowest
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| Electron Configuration | the arrangement of electrons in an atom.
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| Pauli Exclusion Principle | no two electrons in the same atom can have the same set of four quantum numbers.
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| Hund’s Rule | orbitals of equal energy are each occupied by in electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.
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| Valence Electron | an electron that is available to be lost, gained, or shared in the formation of chemical compounds.
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| Inner | shell electrons
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| Highest occupied level | the electron containing main energy lecel with the highest principal quantum number.
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| Noble Gas Configuration | an outer main energy level fully occupied in most cases by eight electrons.
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| s sublevel or suborbital | is the lowest energy.
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| p sublevel or suborbital | middle level
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| f sublevel or suborbital | highst energy level
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