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| The height of a wave from the origin to a crest or from the origin to a trough. |
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| Colors of light given off when atoms of an element absorb energy. When atoms become "excited" by heat or electricity, their electrons hop up to higher energy levels. And when the electrons fall back to their normal energy level, they emit photons. And this light given off by excited atoms has distinctive colors. |
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| A three-dimensional region all around the nucleus that helps us estimate where the possible location of an electron could be. First level is closest to the nucleus. |
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| Used to determine electron configuration of an atom. An atom builds up itself by adding more electrons, starting with the lowest electron level, until the atom assumes it's most stable condition |
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| A series of lines in the visible spectrum of hydrogen. |
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| The maximum displacement point of a wave. |
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| Also known as the visible spectrum. Different colors make up white light and this is the distribution of colors when light is dispersed by a prism. As we move up the frequency increases and wavelenght decreases. |
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this is an equation used the explain and describe the wave nature of an electron.
λ = h/mv
(wavelength= constant/mass x velocity) |
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| Electromagnetic Radiation |
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| this is a form of energy that comes from charged particles; it is described and categorized by the electromagnetic spectrum |
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| The range of wavelengths or frequencies over which electromagnetic radiation extends |
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| The electron configuration of an atom is the particular distribution of electrons among available shells. |
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| A structural formula in which electrons are represented by dots; two dots between atoms represent a covalent bond. Also known as electron-dot formula; Lewis formula. |
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| Energy Sub-levels are Energy levels divided up into four letter going s |
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| An experiment that identifies metals by the color the metal emits when heated |
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| the measurement of the number of times that a repeated event occurs per unit time |
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| The lowest energy state of an atom |
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| Heisenberg Uncertainty Principle |
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| This principle states that you can either know the position or momentum of an electron, but not both. |
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| Hunds rule is when every orbital In a subshell has one electron before a single orbital is double occupied with two. |
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| set of ultraviolet emission lines that go hand in hand with electron movement from higher energy levels to lower |
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| infrared wavelength series; a series of lines in the infrared spectrum; electrons drop in the N = 3 orbit |
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| Pauli's exclusion Principle |
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| Principle that states electrons cannot have the same four quantum numbers. At least the final quantum number has to be different. |
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Effect when electromagnetic radiation, such as light (photons), is exposed to matter, it causes electrons to be emitted from the matter (bounce off). |
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| A quantum amount of energy that an electron gains as it tracs around the nucleus and releases as the electron jumps back to its original energy level; it creates light and other waves |
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It's the constant proportion relating a photon's energy to its frequency; it's expressed by h.
The formula follows:
h=6.626069 EE -34 m^2 kg/s |
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| A major energy ring of an atom that is marked by the quantum number n. n varies in range for each element depending on how many of these there are in each element. |
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| the minimum amount of energy that can be gained or lost by an atom. 1 photon of light is equal to one quantum of energy. It's as measured amount. |
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| Quantum mechanical model of the atom |
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| A model that shows electrons having a movement that is associated with waves. The model is related to Schrodinger's equation and follows quantum theory. |
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| Electrons in a molecule ion or atom that aren't associated with a single atom or covalent bond |
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| The act of one giving a blowjob while the recipient is taking a shit. |
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