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;
32 Cards in this Set
- Front
- Back
|
electromagnetic spectrum
|
the range of different kinds of electromagnetic energy
|
|
|
wavelength
|
(lambda - looks likes upside-down y)
distance between peaks |
|
|
frequency
|
(nu - looks like v)
# of peaks that pass a given point per unit time usually expressed in s^-1 or Hz |
|
|
amplitude
|
height of the wave max from center
larger amplitude = higher intensity |
|
|
visible light wavelengths?
|
380 to 780 nm
|
|
|
speed of light
|
c = 3.00 x 10^8 m/s
c = wavelength-lambda x frequency-nu |
|
|
line spectrum
|
the wavelengths of light emitted by an energetically excited atom
|
|
|
What different sets of m indicate with the Balmer-Rydberg equation?
|
m=1 UV series results
m=2 visible light results m=3 infrared series results |
|
|
1 J = ?
|
1 ( kg*m^2 / s^2 )
|
|
|
E = ?
|
hv where h = Planck's constant & v = amplitude
(measured in Joules/photon) |
|
|
Avogadro's number
|
6.022 x 10^23
|
|
|
quantum
|
the smallest possible amount of radiant energy, a.k.a. a photon
|
|
|
Wavelength = ?
(de Broglie equation) |
h / mv
Planck's constant divided by mass times velocity |
|
|
quantum mechanical model
|
says it's best to focus an electron's wavelike properties in movement around an atom
|
|
|
Heisenberg uncertainty principle
|
says it's impossible to know precisely where an electron is and what path it's following
|
|
|
wave functions
orbitals |
represented by Greek psy (looks like Triton's staff)
|
|
|
principal quantum number
|
n is a positive integer.
Represents number of allowed orbitals/shells. |
|
|
angular-momentum quantum number
|
l defines the three dimensional shape of the orbital = 0 to n-1.
Represents subshells in order of s, p, d, f, g |
|
|
magnetic quantum number
|
m of l defines the spatial orientation = -l to +l.
|
|
|
node
|
zero probability area of where an electron may be found
|
|
|
p orbital shape
|
look like dumbbells
|
|
|
s orbital shape
|
spherical
|
|
|
spin quantum number
|
m of s = -1/2 or +1/2
|
|
|
effective nuclear charge
a.k.a. the Z effective |
the nuclear charge actually felt by an electron
|
|
|
ground-state electron configuration
|
the lowest-energy configuration of an atom
|
|
|
degenerate
|
description for orbitals that have the same energy level
|
|
|
Rules of the aufbau principle
|
1. Lower-energy orbitals fill first
2. An orbital can only hold 2 e- with opposite spins 3. (Hund's rule) One electron goes into each degenerate orbital until they're half-full |
|
|
valence shell
|
outermost shell
|
|
|
measuring atomic radii
|
ideally you measure the distance between two identical bonded atoms and divide by 2
|
|
|
As you go across the periodic table, atoms get ...
As you go down the periodic table, atoms get... |
smaller.
larger. |
|
|
pH = ?
|
-log [H3O+]
only ever 2 sig figs |
|
|
[H3O+] = ?
|
antilog (-pH) = 10^-pH
|
