Reading...
Play button
Play button
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;
71 Cards in this Set
- Front
- Back
|
Electromagnetic (EM) radiation
|
Energy transmitted by wave propagation of electric and magnetic fields
|
|
|
Wavelength
|
Distance wave travels in one cycle
|
|
|
Frequency
|
Number of cycles per unit time
|
|
|
Velocity
|
Distance per unit time
|
|
|
Diffraction
|
Dispersion (separation) of different wavelengths of light by reflection from a grooved surface
|
|
|
Diffraction: constructive interference
|
waves interact in-phase (amplitude increase)
|
|
|
Diffraction: destructive interference
|
waves interact out of phase (amplitude reduction)
|
|
|
Diffraction: grooved surface (grating)
|
results in interference between reflected wavelenths
|
|
|
Refraction
|
dispersion of light as it passes through a different medium (material)
|
|
|
Refraction: velocity of light
|
reduced by interaction with atoms and molecules matter
|
|
|
Refraction: degree of refraction
|
dependent of frequency of light
|
|
|
Spectrum
|
band of different wavelenths from dispersed EM radiation
|
|
|
continuous spectrum
|
contains approximately all wavelengths in a given range
|
|
|
discontinuous specrum
|
contains small number of discrete wavelength
|
|
|
Atomic line spectrum
|
discontinuous spectrum produced by excited atoms
|
|
|
atomic emission
|
gas phase atoms emit light when thermally or electrically excited
|
|
|
line spectra
|
wavelenghts specific to particular elements
|
|
|
Balmer
|
fit oberseved wavelengths (visible) of H-atom line spectrum to mathematical equation
|
|
|
Plank
|
atoms emit/absorb only discrete amounts (quanta) of energy
|
|
|
Photoelectric effect
|
ejection of electrons when photons strike a metal surface
|
|
|
light intensity
|
number of photons per unit time (no effect unless above threshold frequency)
|
|
|
Bohr
|
Developed model to explain line spectrum of the hydrogen atom
|
|
|
atomic energy levels
|
fixed orbits of electrons around the nucleus (discrete allowed states)
|
|
|
photon absorbtion
|
e- moves to higher orbit
|
|
|
photon emission
|
e- moves to lower orbit
|
|
|
line spectra
|
discrete wavelengths correspond to electrons changing orbits (photon emission)
|
|
|
Why is the Bohr model limited and inaccurate
|
only predicts spectra for one-electron systems
electrons do NOT move in fixed orbits |
|
|
Energy states of an ato (Bohr model)
|
ground state=lowest energy level
excited state=energy level higher than ground state |
|
|
Z
|
numlear charge (atomic #)
|
|
|
n
|
energy level (integer for allowed state)
|
|
|
Photon energy
|
difference in energy between state (consevation of energy)
|
|
|
Quantum mechanics
|
application of wave properties to matter
|
|
|
Wave-particle duality
|
light exhibits both wave and particle properties and behavior
|
|
|
de Broglie
|
matter exhibits both partible and wave properties
|
|
|
Mater waves
|
waves associated with material particles of nuclear or atomic dimensions
|
|
|
Standing waves
|
crests and troughs occur at fixes positions (amplitude at fixed endpoints)
|
|
|
nodes
|
points in wave with constant zero amplitude (no displacement during wave oscillation)
|
|
|
wavefunction
|
mathematical function describing wave motion of a particle
|
|
|
schrodinger equation
|
extracts physically relevant information from allowed wavefunctions
|
|
|
principal quantum #(n)
|
describes average radial distance of electron from nucleus
n=positive, non zero integer |
|
|
Orbital angular momentum quantum # (l)
|
determines angular distribution fo orbital
|
|
|
energy sublevel(subshell)
|
subset of principal energy level
|
|
|
sublevel notation
|
n value followed by sublevel name
|
|
|
Magnetic quantum # (ml)
|
determines orientation of electron orbital
|
|
|
# values for ml
|
# electron orbitals within particular sublevel
|
|
|
Orbital energies (one-electron system)
|
defined by principal quantum number (n)
sublevels=degenerate (same energy) within principal level for one-electron system |
|
|
Electron charge density
|
probability density of finding e- at a point
|
|
|
probability density distribution
|
three dimensional "shape" or orbital
|
|
|
s orbital
|
greatest electron density at the nucleus; spherical shape
|
|
|
p orbital
|
no electron density at the nucleus; non-spherical shape
|
|
|
d orbital
|
no electron density at nucleus; various (non-spherical) shapes
|
|
|
orbital energies
|
affected by charge interactions within atom
|
|
|
nuclear charge (Z)
|
positive charge of nucleus (attracts negative electrons)
|
|
|
Electron shielding
|
one electron shields another electron from the full nuclear charge
|
|
|
effective nuclear charge
|
nuclear charge actually experienced by electron
|
|
|
Electron penetration
|
ability of an electron to approach nucleus (depends on l)
|
|
|
radial probability distribution
|
probability of finding e- at a certain radius from nucleus
|
|
|
orbital energies (multi-electron system)
|
sublevel energies altered by electron penetration and shielding
one electron system=no electon-electron relulsion--sublevel energies degenerate (same energy) |
|
|
multi-electron system
|
sublevel energies separated due to electron penetrarion and shielding
|
|
|
Electron spin
|
movement of electron on tis ezis generates magnetic field
|
|
|
electron spin quantum number (ms)
|
indicates direction of electron spin
|
|
|
electron configuration
|
designation of how electrons are distributed in orbitals
|
|
|
orbital filling order
|
in terms of increasing orbital energy
|
|
|
pauli exclusion principle
|
each electron must have a unique set of quantum numbers
|
|
|
Hund's rule
|
if degenerate orbitals are avaiable electron-electron repulsion is minimized
|
|
|
Aufbau method
|
distribute electrons to minimize energy
|
|
|
periodic table
|
indicates filling order in terms of increasing orbital energy
|
|
|
principle quantum # (n)
|
related to period (row) number
|
|
|
abbreviated notation
|
noble gas symbol used to represent core electrons
|
|
|
superscripts
|
indicate number of electrons in each orbital
|
|
|
d-orbitals
|
lower energy associated with half filled and filled sublevels
|
