 | Term | Definition |
| |
electromagnetic radiation |
form of energy that exhibits wavelike behavior as it travels through space |
| |
electromagntic spectrum |
formed from all the forms of electromagnetic radiation |
| |
wavelength |
the distance between corresponding points on adjacent waves |
| |
frequency |
the number of waves that pass a given point in a specific time, usually one second |
| |
photoelectric effect |
refers to the emission of electrons from a metal when light shines on the metal |
| |
quantum |
minimum quantity of energy that can be lost or gained by an atom |
| |
ground state |
the lowest energy state of an atom |
| |
excited state |
a state in which an atom has a higher potential energy than it has in its ground state |
| |
continuous spectrum |
emission of a continuous range of frequencies of electromagnetic radiation |
| |
diffraction |
bending of a wave as it passes by the edge of an object |
| |
interference |
occurs when waves overlap |
| |
Heisenberg Uncertainty principle |
states that it is impossible to deterine simultaneously both the position and velocity of an electron or any other particle |
| |
quantum theory |
describes mathematically the wave properties of electrons and other very small particles |
| |
orbital |
three-dimensional region around the nucleus that indicates the probable location of an electron |
| |
quantum numbers |
specify the properties of atomic orbitals and the properties of electrons in orbitals |
| |
principal quantum number |
symbolized by n, indicates the main energy level occupied by the electron, values are positive integers only |
| |
angular momentum quantum number |
symbolized by l, indicated the shape of the orbital |
| |
shape of s orbital |
spherical |
| |
shape of p orbital |
bowtie |
| |
shape of d orbital |
double bowtie |
| |
magnetic quantum number |
symbolized by m, indicates the orientation of an orbital around the nucleus, ie -1,0,1 |
| |
number of s orbitals |
one |
| |
number of p orbitals |
3 |
| |
number of d orbitals |
5 |
| |
number of f orbitals |
7 |
| |
spin quantum number |
accounts for the magnetic properties of the electron, has only two possible values (+1/2,-1/2)which indicate the two fundamental spin states of an electron in an orbital |
| |
electron configuration |
arrangement of electrons in an atom |
| |
Aufbau principle |
an electron occupies the lowest-energy orbital that can receive it |
| |
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 secoind electron, and all electrons in singly occupied orbitals must have the same spin |
| |
highest occupied level |
electron-containing main energy level with the highest principal quantum number |
| |
inner-shell electrons |
electrons that are not in the highest occupied energy level |
| |
noble gases |
group 18 elements (helium, neon, argon, krypton, xenon, and radon) |
| |
noble- gas configuration |
an outer main energy level fully occupied, in most cases, by eight electrons |
| |
line emission spectrum |
series of specific wavelengths of emitted light created when the visible portion of light from excited atoms in shined through a prism |
| |
photon |
a particle of electromagnetic radiation having zero mass and carrying a quantum of energy |
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