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Definition
the size of the atom. is determined by how far the outermost electrons are from the nucleus pg.301 |
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Definition
explians how electrons exists in atoms and how those electrons affect the chemical and physical properties of elements pg.278 |
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Definition
the e- that are not in the outermost principal shell pg.278 |
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| electromagnetic radiation |
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Definition
a type of energy thattravels through space at a constant speed of 3.0 x 108 m/s pg.279 |
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Definition
includes all wavelenghts of electromagnetic radiation pg.280 |
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Definition
simply shows the occupation of orbitals by electrons for a particular atom pg.291 |
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a fundamental property of all electrons that causes them to have magnetic fields associated with them. the spin of an e- can either be oriented up (+1/2) or down (-1/2) pg.292 |
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Definition
| a spectrum associated with the emission of electromagnetic radiation by elements or compounds |
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| an unstable state for an atom or molecule in which energy has been absorbed but not not re-emitted, raising an electron from the ground state into a higher energy orbital |
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the number of wave cycles or crests that pass through a stationary point in one second pg.280 |
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Definition
the most energetic and shortest wavelenght photons (sun,stars) pg.281 |
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lowest energy state pg.289 |
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Definition
when filling orbitals of equal energy, electrons fill them singly first with parallel spins pg.293 |
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Definition
the fraction of the electromagnetic spectrum between visible light and microwaves. infrared light is invisible to the humans eye pg.281 |
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Definition
| the energy required to remove an electron from an atom in the gaseous state |
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the properties typical of a metal, especially the tendency to loose electron in chemical reactions. elements become more metallic as you move from right to left across the perioic table |
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Definition
| the part of electromagnetic spectrum between the infrared region and the radio wave region. microwaves are efficiently absorbed by water mol, and can therefore be used to heat water-containing substances |
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Term
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Definition
| an e(-) configuration in which the e(-) is represented as arrows in boxes corresponding to orbitals of a particular atom |
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Definition
| the regions around the nucleus of an atom where an e- is most likely to be found |
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Term
| Pauli exclusion principle |
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Definition
| a principle stating that no more than two e- can occupy an orbital and that the two e- must have opposite spin |
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Definition
| a particle of light or a packet of light energy |
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Term
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Definition
| a number that indicates the shell that an e- occupies |
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Definition
| the shell indicated by the principal quantum number |
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Definition
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| ther percise ammount of energy possesed by a photon; the difference in energy between two atomis orbitals |
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Definition
| the foundation of modern chem...; explains how e- exist in atoms, and they affect the chemistry and physical properties of elements |
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Definition
| an integer that specifies the energy of am orbital. The higher the quantum number, the greater the distance between the e- and the nucleus and the higher its energy |
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| the longest wavelength and least energetic form of electromagnetic radiation |
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Definition
in quantum mechanics, specifies the shape of the orbital and its represented by differnt letters s,p,d,f |
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Definition
| the fraction of the electromagnetic spectrum between visible region and the x-ray region |
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Definition
| the e- in the outermost principal shell of an atom, they are involved in chemical bonding |
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Definition
the fraction of the electromagnetic spectrum that is visible to the human eye bounded by wavelenghts of 400nm(violet) and 780nm (red) |
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| the distance between adjacent wave crests in a wavelength |
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Definition
| the portion of the electromagnetic spectrum between the UV region and the gamma-ray region |
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