Unit 3 Flashcards
1 meter is equal to
10^9 nanometers
Violet light color frequency
400 x 10^-9 meters
Red light color frequency
700 x 10^-7 meters
frequency symbol
cursive v
wavelength symbol
upside down y
formula to find frequency
v = E/h
formula to find wavelength
y = c/v
frequency and wavelength relationship
inversely proportional
frequency and energy relationship
directly proportional
wavelength and energy relationship
inversely proportional
Planck’s assumption
heated object emits energy in specific amounts (quanta) not continuously
discrete packet of energy emitted by objects
quanta
a quanta of light
a photon
minimum quantity of energy that can be lost or gained by an atom
quantum
according to planck, light has ___ properties
particle-like
according to broglie, electrons have ____ properties
wave-like
bohr model
electrons can only have certain orbits around the nucleus to be able to orbit around the atom
the ground state is
when the electrons are in the lowest energy state possible (closest to the atom) (normal orbital notation)
the excited state is
when the electrons absorb different quanta of energy and jump to the next energy level (not closest to the atom)
first energy level is
closest to the nucleus, lowest amount of energy, most stable
higher energy levels are
father away from the nucleus, higher amounts of energy, less stable
electrons in excited state return to ground state by
emitting specific quanta of energy
electrons in ground state move to excited state by
absorbing specific quanta of energy
how much energy does an electron need to jump
exact amount, no more and no less
emission of light from an atom occurs when
an electron goes from upper to lower energy level
absorption of light from an atom occurs when
an electron goes from lower to higher energy level
the pattern formed when photons are emitted from the electron shifting from higher to lower energy state is called
bright line spectra
bright line spectra are
like a fingerprint for elements
the pattern formed when photons are emitted from the electron shifting from lower to higher energy state is called
dark line spectra
total energy absorbed by electrons when they go from ground to excited state is ____ to the total energy released when electrons go from excited to ground state
exactly equal
each orbital can hold max
2 electrons
principle quantum number
describes the energy level of an electron (2s, 4p, etc)
angular momentum quantum number
describes the type of sublevel (2s, 4p, etc)
s orbital shape
spherical
p orbital shape
peanut/figure 8
d orbital shape
square/double peanut
f orbital shape
flower
s orbital number
1 on each s sublevel
Pauli Exclusion principle
two electrons in the same orbital must have opposite spins
