vocab
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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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 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 specific point in a certain amount of time
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| Visible Light | Electromagnetic radiation that can produce a visual image that can be seen with the naked eye
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| Velocity of a wave | Measure of the rate of change of a wave
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| Photoelectric effect | The emission of an electron from a metal when light shines on the metal
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| quantum | The minimum amount of energy that can be lost or gained by an atom
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| Planck’s Constant | This relates the energy of a photon to the frequency of that photon. Its value is approximately 6.626 × 10 -34 joule-seconds
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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 | The capability to transfer heat to a photon
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| Ground State | Lowest energy state of an atom
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| Excited State | A state where an atom has a higher potential energy than it has in its ground state
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| Line-emission spectrum | A series of specified wavelenghts of emitted light is separated into a series of specific frequencies of visible light
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| continuous spectrum | Emission of a continuous range of frequencies of electromagnetic radiation
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| Bohr radius | The radius of the n=1 orbital in hydrogen
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| Interference | Waves overlap which causes a reduction of energy in some areas and an increase in others
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| Heisenberg Uncertainty Principle | States it is impossible to determine the position and velocity of an electron or other particle
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| Quantum Theory or Quantum Mechanics (same definition for both of these so list them together) | Describes wave properties of electrons and other particles
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| Orbital | 3-D region around the nucleus and the probable place of an electron
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| Quantum numbers | specify the properties of atomic orbitals and the properties of electrons in orbitals
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| Principle Quantum number (n) | Indicates the main energy level occupied by electrons
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| Angular momentum quantum number (l ) | Indicates shape of the orbital
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| Magnetic quantum number (m) | Indicates the orientation of an orbital around the nucleus
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| Spin quantum number (s) | Indicates the two fundamental spin states of an electron in a orbital
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| Aufban Principle | An electron occupies the lowest energy orbital that can receive it
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| Electron Configuration | 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 one electron before any orbitals must have the same spin
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| Valence Electron | the electrons of an atom that can participate in the formation of chemical bonds with other atoms
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| Inner-shell electrons | Electrons that are not in the highest energy level
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| Highest occupied level | The electron containing main energy level with the highest principal quantum number
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| Noble Gas Configuration | Outer main energy level fully occupied in most cases by 8 electrons
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| s sublevel or sub-orbital | A spherically symmetrical atomic orbital
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| p sublevel or sub-orbital | The orbital of an atomic electron with an orbital angular momentum quantum number of unity
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| f sublevel or sub-orbital | corresponds to an electron orbital with angle momentum quantum number l = 3.
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