Studied by 3 peoplethe product of the frequency and wavelength equals
speed of the wave
because C, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is
inversely proportional to wavelength
according to the photo electric effect, certain kinds of light cannot eject electrons from metals due to the energy of light being too low
true
if electromagntic radiation A has a lower frequency then electromagnetic radiation b, then compared to b wavelength a is
longer
distance between two sucessive peaks in waves
wavelngth
quantum of electromagnetic energy is
photon
energy of photon is related to its
frequency
the emission of electrons from metals that have absorbed photons is called
photoelectric effect
a line spectrum is produced when an electron moves from one energy level to another
to a lower energy level (thing weird shaped ladder)
for an electron in an atom to change from the ground state to an excited state
energy must be absorbed
where do electrons circle the nucleus
in speicific allowed orbitals
emitting energy
go down energy levels (e.g 4 to 1)
absorbing energy
go up energy levels (e.g 2 to 3)
the electron in a hydrogen atom has its lowest total energy when the electron is in its
ground state
french scientist louis broglie theorized that
electrons could have a dual wave particle nature
three dimensional region around a nucleus where an electron may be found is called an electron path
false
according to the quantum theory of an atom, in an orbital
an electrons position cannot be known exaclty (think the rat and flashlight anaology)
main energy levels of an atom are indicated by the
principal quantum theory
number of sublevels within each energy level of an atom is equal to the value of
principal quantum theory
an electron for which n=4 has more energy than an electron that has n=2
true
the spin quantum number indicates that the number of possible spin states for an electron is an orbital is
2
the set of orbtil that are speherical shaped are directed along the x,y,and z axes are called
s orbitals
the major differences between a 1s orbital and a 2s orbital is that
the 2s orbital is at a higher energy level
the p orbital shape
dumbell
for s sublevel, number of orbital is
7
how many electrons can occupy the p orbital at each energy level
6 if they have opposite spins
if n is the principal quantum number of the main energy level, the max number of electrons of that energy level is
2n^2
how many electrons are needed to completly fill the fourth energy level
2n^2=2(4)^2=32
at n=1 the total number of electrons that can be found
2
the main energy level that can hold only two electrons is the
first
which of the following rules requires that each o the p orbitals at a paticular energy level recieve one electron before any of them can have two electrons
hunds rule
two electrons in the 1s orbital must have different spin quantum numbrs to satisfy
the pauli's exclusion principle
the sequence in which enregy sublevels are filled is specified by
the aufbau principle (bottom-top)
the aufbau principle states that an electron
occupies the lowest available energy level
what is the electron configuration for nitrogen atomic number 7
1s^22s^22p^3
the electron for aluminum atomic number 13 is
1s^22s^22p^63s^23p^1
according to bohr electrons cannot reside
in-between orbitals
with a wavelegnth of 170 nm what is the frequency in hertz of this particular wavelength of uv light
c=(wavelength)(v)=1.76x10^-14 hz
the electron configuration for nitrogen is 1s^22s^22p^3 what does the 3 in 2p^3 mean
electron
what is the relationship between wavelength and frequency
inversely proportional
Note 
Flashcard (41)