2. waves

4. speed of light(c) = 3.0 x 108 m/s or 186,000 miles/s
λ = wavelength
ν = frequency
ν inversely related to λ

5. The Ionosphere and Radio Wave Propagation
the D layer is good at absorbing AM radio waves
D layer dissapears at night.... the E and F layers bounce the waves back to the earth
this explains why radio stations adjust their power output at sunset and sunrise

10. Niels Bohr only works for hydrogen
no other spectral lines match the energy of the electrons
doesn’t explain why electrons don’t fall in to nucleus
electrons give off energy and move toward nucleus, yet they never fall in to the nucleus
if e- fell in to the nucleus, matter would not exist
quantum mechanic video

12. Max Planck (1858-1947) founder of quantum theory
studied electromagnetic radiation emitted from objects
determined the radiation was given off in specific amounts
quanta
separated physics
classical physics - study of particles, forces
quantum physics – study of wave/energy and particle interaction
video

13. Albert Einstein (1879-1955) evaluated photoelectric effect
Showed that electrons could be ejected from a metal surface by shining a specific frequency of light on that surface
mathematically proved the frequency of light contained quanta of energy
referred to these as particles of energy
photons – particles/bundles of energy
light(energy) is a wave(classical)
light(energy) is a particle? (quantum)

14. Erwin Schroedinger (1887-1961)
mathematically derived an equation that proved an electron has wave-like properties
electron is a particle (classical physics)
behaves as particles should
affected by forces
has mass
electron is a wave (quantum physics)
has wave properties
double slit experiment
wavelength and frequency can be measured

15. Louis de Broglie ( )
derived an equation that could explain the wavelength characteristics of all matter
λ = h/mv
λ = wavelength
h = Planck’s constant (6.626 x jxs)
m = mass of particle
v = velocity of particle
the wavelength of an electron matches the distance electrons are found from the nucleus

16. Thomas Young double slit experiment video

17. Wave-Particle Duality theory
Double Slit Experiment with Light

18. The observer in double slit experiment (youtube video)

19. Wave-Particle Duality theory

20. Wave-Particle Duality theory
waves exhibit particle-like properties
photons
photoelectric effect
particles exhibit wave-like properties
frequency and wavelength of particles
dual slit experiment
waves and particles are interchangeable
video

21. Quantum Mechanical Model
Schroedingers Cat-Thought Experiment

22. Heisenberg Uncertainty Principle
the exact position and momentum/speed of a particle cannot be simultaneously known
large particles have little uncertainty
baseball
due to the baseballs large mass the amount of uncertainty of where the ball is or how fast the ball is traveling is very small(not measurable)
small particles have high uncertainty
electron
due to the electrons small mass the amount of uncertainty of where the electron is or how fast the electron is traveling is very large(can’t know position if momentum is known, can’t know momentum if position is known)
video

23. Quantum Mechanical Model
visual example
bees around a hive
bees are electrons
currently accepted model of atom
most probable location of electrons described with quantum numbers
can’t know exact position or path
predict most probable location of locating an electron in a specific region around the nucleus
similar to predicting Mr. Andresen’s location in the school at any given moment
video

24. Quantum Numbers Principal Quantum number
quantum numbers describe most probable location of electrons around the nucleus(3-D model)
Principal Quantum number
denotes distance electrons are from the nucleus
similar to the number of floors in a building
NRG levels
whole numbers 1 - ∞(7)
1st nrg level is closest to nucleus
7th nrg level is farthest from nucleus

25. Quantum Numbers Orbital(angular momentum) Quantum number
indicates the shape of where the electron is most probably located within the NRG level
similar to the shape of a room in a building
denoted by letters s, p, d, f, (g, h, i, j…)
s-orbital smallest
lowest NRG orbital
f-orbitals largest, most complex
highest NRG orbital

26. Quantum Numbers s-sublevel p-sublevel d-sublevel f-sublevel
1 - spherical shaped orbital
only 1 orbital/NRG level
p-sublevel
3 - peanut shaped orbitals
start on 2nd NRG level
d-sublevel
4 - four leaf clover shaped + unique shape
5 orbitals/NRG level(starting with 3rd NRG level)
f-sublevel
7 very complex shapes(flower petals)
7 orbitals/NRG level(starting with 4th NRG level)

27. Quantum Numbers Magnetic quantum number
indicates the position of each orbital in the nrg level with regard to the three axis(x, y, z) in space
s-orbital only has one position
sxyz – sphere is positioned on all three axis equally

28. p-orbital has three positions
px, py, pz = p sublevel

30. d-orbital has five positions
dxy, dxz, dyz, dx2-y2, dz2 = d sublevel
too complex for us

31. f-orbital has seven positions
7 orbitals = f sublevel
way too complex for us

32. Quantum Numbers Spin Quantum number
indicates the spin/magnetic field orientation of the electron
according to classical physics, a charged object that is spinning creates a magnetic field
electrons have a magnetic field, i.e. they are “spinning”
denoted with +1/2 and -1/2
also denoted with , 
each orbital position can hold a maximum of 2 electrons but they must have opposite spin(Pauli’s Exclusion Principle)
s-sublevel(1 orbital) = 2 electrons
p-sublevel(3 orbitals) = 6 electrons
d-sublevel(5 orbitals) = 10 electrons
f-sublevel(7 orbitals) = 14 electrons

33. NASA and Google team up to create a quantum computer(click here)
diagramming e- in an atom
orbital notation
e- configuration
e- dot diagram