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Arrangement of Atoms
| Question | Answer |
|---|---|
| Electromagnetic Radiation | Form of energy that exhibits wavelike behavior as it travels through space |
| Electromagnetic Spectrum | Electromagnetic spectrum |
| Frequency | Number of waves that pass a given point in a specific time, typically one second |
| Visible Light | Spectrum that is used by most organisms to be able to see |
| Velocity of a Wave | Product of wavelength and frequency part of the electromagnetic spectrum that is roughly in the middle |
| Photoelectric Effect | Emission of electrons from a metal when light shines on the metal |
| Quantum | Minimum quantity of energy that can be gained or lost by an atom |
| Planck’s Constant | Fundamental physical constant; h=6.626 × 10-34 J⋅s |
| Photon | Particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
| Energy of a Photon | E(photon)=hv |
| Ground State | Lowest energy state of an atom |
| Excited State | State in which an atom has a higher potential energy than it has in its ground state |
| Line-Emission spectrum | Series specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism |
| Continuous Spectrum | Emission of continuous range of frequencies of electromagnetic radiation |
| Bohr Radius | Radius of the s orbital in hydrogen |
| Interference | Waves overlapping that results in a reduction of energy in some areas and an increase of energy in others |
| Heisenberg Uncertainty Principle | “It is impossible to determine simultaneously both the position and velocity of an electron or any other particle” |
| Quantum Theory or Quantum Mechanics | Mathematical description of the wave properties of electrons and and other very small particles |
| Orbital | Three-dimensional region around the nucleus that indicates the probable location of an electron |
| Quantum Numbers | Number that specifies the properties of atomic orbitals and the properties of electrons in orbitals |
| Principle Quantum Number (n) | Quantum number that indicates the main energy level occupied by the electron |
| Angular Momentum Quantum Number (l ) | Quantum number that indicates the shape of the orbital |
| Magnetic Quantum Number (m) | Quantum number that indicates the orientation of an orbital around the nucleus |
| Spin Quantum Number (s) | Spin quantum number (s) |
| Electron Configuration | Arrangement of electrons in an atom |
| Pauli Exclusion Principle | "No two electrons in the same atom can have the same set of four quantum numbers" |
| Hund’s Rule | Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin |
| Valence Electron | Electron that is available to be lost, gained, or shared in the formation of chemical compounds |
| Inner-Shell electrons | Electron that is not in the highest occupied energy level |
| Highest Occupied level | Electron-containing main energy level with the highest principal quantum number |
| Noble Gas Configuration | Outer main energy level fully occupied, in most cases, by eight electrons |
| S Sublevel or Sub-Orbita | Spherical shaped; only one sublevel is possible per n value |
| P Sublevel or Sub-Orbital | Dumbbell shaped; three sub levels possible per n value (x, y, z axis) |
| F Sublevel or Sub-orbita | More complex shaped; seven sub levels possible per n value |
Created by:
30Leigh
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