Absorbtion, light, unit 2 chem

Wavelength equation

speed of light/ frequency

c/v

inversly related to frequency

speed of light

3.00 × 10^8 m/s

why is light a wave?

diffraction (double slit experiment)

interference (destructive (out of phase) and constructive(inphase)

photelectric effect

light shines on metal and electrons are emmitted

light transfers its energy directlt to electrons on the metal surface

part of energy breaks the attracion forces and leftover emits th eloectron

frequency threshold

Lighy is also a particle because

carries energy in little packets (photons)

energy of photon depends on its frequency

energy of photon equation

Ep = h x v

h= planks constant (6.626 × 10^-34)

v = frequency

OR h x c/ wavelength

increasing light intensity on photoelectric effect

more elctrons emmitted (w the same velocity)

bhors model

electrons move w defined energy from a defined distance from the nucleus

energy of electrons are quantized

energy of photon equals the differnce between energy levels

why does matter have wave like properties

x ray diffraction observed

double split experiment w electrons

wave particle duality

wavelength of a matter wave

wavelength = h/(m)(v)

m= mass (kg)

v = velocity (m/s)

schrodingers equation

calculates the energy levels available for electrons and the probability of finding them there

the solutions: atomic orbitals

nodes

where the wave of the energy of an electron amplitude is zero

separate nodes

where energy is zero

s orbital

sphere shaped

one per a given n (energy level)

size increases as n increases

radial nodes only

p orbital

dumbell shaped

3 p orbitals in a subshell

planar and radial nodes

d orbitals

clover shaped

5 orbitals in a subshell

planar and radial nodes

hierchy of shells, subshells and orbitals

a group of atomic orbitals make up a : subshell

a group of subhells make up a shell or principal energy level

shell contains n² orbitals

pauli exclusion principle

electrons can share the same orbital if they have opposite spins

aufbau principle

electrons fill teh lowest energy level first

hunds rule

ups fill first then pairs

valence electrons

fill the outermost energy level, loosely bound

participate in interactions

atomic radius trends in periodic table

doewn a group: increases

left to right: dercreases

what determines the size of the atom

inward and outward push of energys ebetween electrons and nucleas

coulombs law

effective nuclear charge

the net postive charge experienced by valence electrons

slightly shielded by core electrons

Zeff= Z - S

z= actual nuclear charge (atomic number/protons)

S= charged screened by core electrons