lap 3 chemistry Flashcards
light has characteristics of both
particles and waves
electromagnetic moves likes a
wave(repetitive motion)
particle
emission of particles when in contact with certain materials
electrons exist only in
very specific energy states for every atom of each element such as the ground and excited states
bohrs model of the hydrogen illustrates
electron transition states
electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space; a type of radiation that carries energy through space
list electromagnetic spectrum (from low to high frequency)
radio waves, microwaves, infrared, visible light, ultraviolet, x-rays, gamma
blackbody radiation
the emission of light from heated objects
planks constant
6.626 x 10 to the -34 js
to solve for a quantum of energy, use the equation
E=hv
ephoton is equal to
the difference between the atoms initial state and its final state
when the excited electron relaxes back to its ground state,
the energy is released as electromagnetic radiation
bohrs model of a hydrogen states
- electrons are in specified orbit; never in between
2.when energy is put in, the electrons absorb the energy and become excited moving to a new energy level - when the excited electron relaxes and releases(emits) the energy, it will either fall back to its ground state or to a lower energy state
- when the electrons fall to the lower energy level, it releases energy in the form of light color
- perfectly explains hydrogen’s one electron
- assumed to work out for all atoms
Heisenberg uncertainty principle
it is impossible to determine simultaneously both the position and velocity of an electron or any other particle
principle quantum number is represented by
n (energy levels)
number of electrons per energy level is determined by the formula
2(n^2)
angular momentum quantum is represented by
l (sublevels)
magnetic quantum number is represented by
m sub l (number of orbitals)
s orbital is shaped like a
sphere
p orbital is shaped like a
dumbbell
magnetic spin number is represented by
m sub s (up and down spin)
aufbau principle
an electron occupies the lowest-energy orbital that can receive it
pauli exclusion principle
no two electrons of the same atom can have the same set of four quantum numbers
hunds principle
orbitals of equal energy are each occupied by one electron before any orbit is occupied by a second electron and all electrons b
how to find speed of light
c= wavelength times frequency
how to find wavelength
speed of light/ frequency
how to find frequency
speed of light/wavelength
as the frequency increases,
the wavelength decreases
diamagnetic
does not have unpaired electrons and is not attracted to a magnetic field
frequency is expressed in
hertz
wavelength is expressed in
m/s
n equals
the period
m/s goes with
speed of light (3.00 x 10^8)
J x S goes with
planks constant
hz goes with
frequency
m goes with
wavelength
what are sub levels
s,p,d,f
aufbau
lowest energy orbitals are filled first
pauli
orbitals can only have 2 electrons with opposite spins
hunds rule
when orbitals of the same energy are available they are single put out before the paired ones (don’t leave any blank)
if the configuration forgot something, it is
aufbau violation
if the configuration has too many in one it is
pauli violation
if the configuration has 2 up in one and 2 down in one, it is
pauli violation(supposed to be one up and one down per “box”)
electron affinity increases from
down up and from left to right
atomic radius increases from
up down and from right to left
ionization energy increases from
left to right to and down up
electronegativity increases from
left to right and down up
