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Chem Ch. 5
| Question | Answer |
|---|---|
| Electromagnetic Radiation | A form of energy exhibiting wavelike behavior as it travels through space; can be described by wavelength, frequency, amplitude, and speed and includes visible light, microwaves, X rays, and radio waves. |
| Wavelength | Distance between points on two consecutive waves. |
| Frequency | The number of waves that hit this point in one second. |
| Amplitude | The intensity of a wave. |
| Electromagnetic Spectrum | Includes all forms of electromagnetic radiation,with the only differences between the types of radiation being their frequencies and wavelengths. |
| Quantum | The minimum amount of energy (in Joules) that can be gained or lost by an atom. |
| Planck’s Constant | h = 6.63 x 10-34 J*s |
| Photoelectric Effect | A phenomenon in which photo electrons are emitted from a metal's surface when light of a certain frequency shines on the surface. |
| Photon | A particle of electromagnetic radiation with no mass that carries a quantum of energy. |
| Atomic Emission Spectrum | A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors. |
| Ground State | Electrons in their lowest allowable energy levels are in ther _____________. |
| De Broglie Equation | The velocity of a mass, mv, is a particle property, whereas lambda is a wave property or lambda=h/mv. |
| Heisenberg Uncertainty Principle | States that it is not possible to know precisely both the velocity and the position of a particle at the same time. |
| Quantum Mechanical Model of the Atom | An atomic model in which electrons are treated as waves. |
| Atomic Orbitals | A three-dimensional region around the nucleus of an atom that describes an electron's probable location. |
| Principal Quantum Number | Number which the quantum mechanical model assigns to indicate the relative sizes and energies of atomic orbitals. |
| Principal Energy Levels | The major energy levels of an atom. |
| Energy Sublevels | The energy levels contained within a principal energy level. |
| Electron Configuration | The arrangements of electrons in the atom. |
| Aufbau Principle | States that electrons fill up the lowest energies possible first. |
| Pauli Exclusion Principle | States that a maximum of two electrons may occupy a single orbital, but only if the electrons have opposite spins. |
| Hund’s Rule | States that for sublevels with multiple orbitals, an electron with the same spin occupies each orbital before a 2nd electron with the opposite spin enters each orbital. |
| Valence Electrons | The electrons in an atom's outermost orbitals. |
| Electron Dot Structure | Consists of an elements symbol, representing the atomic nucleus and inner-level electrons, that is surrounded by dots, representing the atom's valence electrons. |
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