exam 2 Flashcards
(34 cards)
hess’s law
the overall enthalpy change of a process is the sum of the enthalpy change of each step of the process
frequency
the number of cycles per seconds (s-1)(Hz)
wavelength
the distance between any point on a wave and the same point on a corresponding crest (m or nm)
1 nm
10^-9 meters
speed
distance per unit of time (meters/second)
speed of light
3.00 x 10^8
amplitude
the height of the radiation wave (intensity and color)
electromagnetic spectrum (greatest to least)
gamma x-ray UV visible infared microwave radio
bohr model
one works for one electron models
rydberg equation is used for…
position of a wavelength give n values
ground state
lowest e energy level (n-1)
excited state
(n>1) orbit farther from the nucleus
principle quantum number
(n) the SIZE, relative distance to the nucleus. also specifies energy level
angular momentum quantum #
(l) integer from 0 to (n-1). tells us the SHAPE
the possible # of l values is = to the n value
magnetic quantum #
(-1 to +1)(m) tells us the ORIENTATION of the orbital
quantum #s and energy level
energy level/shells = n
sub-level/sub-shells= l
molarity
concentration of a solute in a solution (moles of solute / 1 liter of solution)
paulis exclusion principle
no two electrons in the same atom can have the same 4 quantum #s
ex. baseball stadium seating
shielding
electrons feel not only attraction to the nucleus but also repulsion’s from other electrons
REDUCES full nuclear charge to Zeff
Zeff
the nuclear charge an e- actually experienced.
lower Zeff makes it easier to move
order of sub level energies
lowest to highest
S P D F
aufbau principle
to build up: must fill the lower sub level before filling a higher one
hunds rule
the electron configuration of the lowest energy has the max # of unpaired electrons with parallel spins
highest in the top right corner
Zeff
Ionization energy
Electron affinity
