Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
28 Cards in this Set
- Front
- Back
electromagnetic radiation
|
a form of energy that exhibits wavelike behavior as it travels through space (visible light)
|
|
wavelength
|
the shortest distance between equivalent points on a continuous wave
|
|
frequency
|
the number of waves that pass a given point per second (hertz or s^-1)
|
|
amplitude
|
the wave's height from the orgin to a crest, or from the origin to a trough
|
|
electromagnetic spectrum
|
(EM Spectrum) -- emcompasses all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths
|
|
quantum
|
the minimum amount of energy that can be gained or lost by an atom
|
|
planck's constant
|
Equantum = hv (Js)
6.626 x 10^-34 |
|
photoelectric effect
|
electrons, called photons, 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 Ephoton = hv
|
|
atomic emmission spectrum
|
the set of frequencies of the electromagnetic waves emitted by atoms of the element
|
|
speed of light
|
c= wavelengh *frequency
c = 3.00 x 10^8 m/s |
|
ground state
|
the lowest allowable energy state of an atom; when an atom gains energy it is said to be an excited state
|
|
de Broglie equation
|
predicts that all moving particles have wave characteristics (wavelength = plank's constant /mass*velocity
|
|
Heisenberg uncertainity principle
|
states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time
|
|
quantum mechanical model of the atom
|
the atomic model in which electrons are treated as waves
|
|
atomic orbital
|
a 3D region aroung the nucleus describes the electron's probable location
|
|
principal quantum number
|
(n) that indicate the relative sizes and energyies of atomic orbitals. Tha is as n increases, the orbital becomes large, the electron spends more time farther from the nucleus and the atom's energy level increases
|
|
principal energy level
|
n specifies the atom's major energy levels
|
|
energy sublevel
|
principal energy levels contain energy sublevels
|
|
visible series
|
balmer
|
|
ultra violet series
|
lyman
|
|
infared series
|
paschen
|
|
electron configuration
|
the arrangement of electrons in an atom
|
|
aufbau principle
|
state that each electron occupies the lowest energy orbital available
-all orbitals related to an energy sublevel are of equal energy -in a multi-electron atom, the sequence of energy sublevels within a principal energy level is s, p, d, and f. - orbitals related to energy sublevle within one principal energy level can overlap orbitals related to energy sublevle within another principal level |
|
Pauli exclusion principl
|
states that a max of 2 electrons may occuply a single atomic orbital, but only if the electrons have opposite spins
|
|
Hund's rule
|
state that singel electrons with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbitals
|
|
valence electron
|
electrons in the atom's outermost orbitals -- generally those orbitals associated with the atom's highest principal energy level
|
|
electron dot structure
|
consists of element's symbol, which represents the atomic nucleus and inner level electrons surrounded by dots representing the atom's valence electrons
|