Unit 2: Atomic Theory & Quantum Mechanics Flashcards
As effective nuclear charge increases, atomic radius ______________
decreases
largest energy gap is between n=_ and n=_
1, 2
how to convert from nm to m
multiply nm by 10^-9
l = 0
s orbital
l = 1
p orbital
l = 2
d orbital
l = 3
f orbital
visible light is only from energy gaps n=_ to n=_
2, 6
wavelength is the ____________ from peak to peak
distance
each element has an ______________ spectrum unique from all others
emission
bohr model and rydberg equation only works for atoms with only ________ electron
one
the work function of a metal….
is the amount of energy required to remove an electron from the metal’s surface in a vacuum
hv < work function
no electrons ejected
hv > work function
electrons ejected
light is a form of energy that can behave sometimes like a ____________ and sometimes like a _____________
wave, particle
(wave-particle duality)
short wavelength = _________ energy
high
DeBroglie equation formula
wavelength = h/mv
Pauli Exclusion Principle
In a given atom, no two electrons can have the same quantum numbers.
An orbital can hold a maximum of two electrons and they must have opposite spin.
all subshells in an energy level are ______________
degenerate
Aufbau principle
electrons fill from lowest energy to highest energy orbitals
Hund’s rule
electrons fill degenerate orbitals singly before pairing up
diamagnetic
all paired electrons
paramagnetic
some unpaired electrons
effective nuclear charge (Zeff)
attraction to the nucleus felt by the outermost electrons in an atom
effective nuclear charge formula
atomic # - # of inner shell electrons
ionization energy
the amount of energy required to remove the first electron from a neutral atom in the gaseous state
electron affinity
the change in energy when an electron is added to a gaseous atom to form an anion
electronegativity
how strongly an atom pulls electrons when bonded to another atom
Aufbau exceptions
Au, Ag, Cu, Cr, Mo
