5 Kinds of EM waves There are many different l and n Radio waves, microwaves, x rays and gamma rays are all examples.Light is only the part our eyes can detect.GammaRadioRayswaves
6 The speed of light in a vacuum is 2.998 x 108 m/s = c c = ln What is the wavelength of light with a frequency 5.89 x 105 Hz?What is the frequency of blue light with a wavelength of 484 nm?
7 In 1900Matter and energy were seen as different from each other in fundamental ways.Matter was particles.Energy could come in waves, with any frequency.Max Planck found that as the cooling of hot objects couldn’t be explained by viewing energy as a wave.
8 Hot Objects and the Quantization of Energy Planck found DE came in chunks with size hnDE = nhnwhere n is an integer.and h is Planck’s constanth = x J-sthese packets of hn are called quantum
9 The Photoelectric Effect - Einstein is next Light shining on a clean metal surface causes the surface to emit electrons.Said electromagnetic radiation is quantized in particles called photons.Each photon has energy = hn = hc/lCombine this with E = mc2You get the apparent mass of a photon.m = h / (lc)
10 You Try It…Calculate the energy of one photon of yellow light whose wavelength is 589 nm.
11 Which is it? Is energy a wave like light, or a particle? Yes Concept is called the Wave -Particle duality.What about the other way, is matter a wave?
12 Matter as a waveUsing the velocity v instead of the frequency n we get.De Broglie’s equation l = h/mvCan calculate the wavelength of an object.The quantity mv for any object is called its momentumDe Broglie used the term matter waves.
13 You Try It…What is the wavelength of an electron moving with a speed of 5.97 x 106 m/s? The mass of an electron is 9.11 x g.
14 DiffractionWhen light passes through, or reflects off, a series of thinly spaced line, it creates a rainbow effectbecause the waves interfere with each other.
23 Several wavesSeveral wavesSeveral CurvesInterference Pattern
24 What will an electron do? It has mass, so it is matter.A particle can only go through one hole.A wave through both holes.An electron does go through both, and makes an interference pattern.It behaves like a wave.Other matter has wavelengths too short to notice.
25 Spectrum The range of frequencies present in light. White light has a continuous spectrum.All the colors are possible.A rainbow.
26 Hydrogen spectrum 656 nm 434 nm 410 nm 486 nm Emission spectrum because these are the colors it gives off or emits.Called a line spectrum.There are just a few discrete lines showing656 nm434 nm410 nm486 nm
27 What this meansOnly certain energies are allowed for the hydrogen atom.Can only give off certain energies.Use DE = hn = hc / lEnergy in the in the atom is quantized.
28 Niels Bohr Developed the quantum model of the hydrogen atom. He said the atom was like a solar system.The electrons were attracted to the nucleus because of opposite charges.Didn’t fall in to the nucleus because it was moving around.
29 The Bohr Ring AtomHe didn’t know why but only certain energies were allowed.He called these allowed energies energy levels.Putting Energy into the atom moved the electron away from the nucleus.From ground state to excited state.When it returns to ground state it gives off light of a certain energy.
31 Give it some thought…As the electron in a hydrogen atom bumps from n=3 orbit to the n=7 orbit, does it absorb energy or emit energy?
32 The Bohr Model Doesn’t work for all atoms. Only works for hydrogen atoms.Electrons don’t move in circles.The quantization of energy is right, but not because they are circling like planets.
33 Limitations to the Bohr Model Bohr model offers an explanation for the line spectrum of the hydrogen atom, it cannot explain the spectra of the other atoms.Important step along the way toward the development of a more comprehensive model1. Electrons exist only in certain discrete energy levels, described by quantum numbers2. Energy is involved in moving an electron from one level to another.
34 The Quantum Mechanical Model A totally new approach.De Broglie said matter could be like a wave.De Broglie said they were like standing waves.The vibrations of a stringed instrument.
36 What’s possible?You can only have a standing wave if you have complete waves.There are only certain allowed waves.In the atom there are certain allowed waves called electrons.1925 Erwin Schroedinger described the wave function of the electron.Much math but what is important is the solution.
37 Schroedinger’s Equation The wave function is a F(x, y, z)Solutions to the equation are called orbitals.These are not Bohr orbits.Each solution is tied to a certain energy.These are the energy levels.
38 There is a limit to what we can know German physicist Werner Heisenberg proposed that the dual nature of matter places a fundamental limitation on how precisely we can know both the location and the momentum of any object.The Heisenberg Uncertainty Principle.
39 What does Schroedinger’s Wave Function mean? nothing.it is not possible to visually map it.The square of the function is the probability of finding an electron near a particular spot.best way to visualize it is by mapping the places where the electron is likely to be found.
40 Defining the size The nodal surface. The size that encloses 90% to the total electron probability.NOT at a certain distance, but a most likely distance.For the first solution it is a sphere.
47 Quantum Numbers There are many solutions to Schroedinger’s equation Each solution can be described with 4 quantum numbers that describe some aspect of the solution.1. Principal quantum number (n) size and energy of an orbital.Has integer values >0
48 Quantum numbers 2. Angular momentum quantum number l . shape of the orbital.integer values from 0 to n-1l = 0 is called sl = 1 is called pl =2 is called dl =3 is called fl =4 is called g
49 Values of l123Letter usedsSharppPrinci-paldDiffusefFunda-mental
50 Quantum numbers 3. Magnetic quantum number (m l) integer values between - l and + l, including zero.Describes the orientation of the orbital in space.4. Electron spin quantum number (m s)Can have 2 values.either +1/2 or -1/2
51 Give it some thought…What is the difference between an ORBIT in the Bohr model and an ORBITAL in the quantum mechanical model?
52 Terms…Electron shell – the collection of orbitals with the same value of nSubshell – the set of orbitals that have the same n and l valuesFor example, the orbitals that have n=3, l=2 are called 3d orbitals and are in the 3d subshell.
53 Electron Configurations Pauli Exclusion Principal – no 2 electrons can have the same set of 4 quantum numbers.at most there can only be 2 electrons in a single orbital.Aufbau Principal – electrons will fill the lowest energy level firstHund’s Rule – for orbitals with equal energy, electrons will occupy singly to the maximum extent possible with parallel spin before pairing up.
54 Increasing energy He with 2 electrons 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 3d4d5d7p6d4f5fHe with 2 electrons
55 Fill from the bottom up following the arrows 2s 2p3s 3p 3d4s 4p 4d 4f5s 5p 5d 5f6s 6p 6d 6f7s 7p 7d 7f1s22s22p63s23p64s23d104p65s24d105p66s2
56 DetailsElements in the same column have the same electron configuration.Put in columns because of similar properties.Similar properties because of electron configuration.Noble gases have filled energy levels.Transition metals are filling the d orbitals
57 Exceptions Cr = [Ar] 4s1 3d5 Half filled orbitals. Scientists aren’t sure of why it happenssame for Cu [Ar] 4s1 3d10
58 More exceptions Lanthanum La: [Xe] 6s2 5d1 Cerium Ce: [Xe] 6s2 4f1 5d1 Promethium Pr: [Xe] 6s2 4f3 5d0Gadolinium Gd: [Xe] 6s2 4f7 5d1Lutetium Pr: [Xe] 6s2 4f14 5d1We’ll just pretend that all except Cu and Cr follow the rules.
59 Writing Electron Configurations Write the electron configuration and orbital diagram for IronWrite the electron configuration and orbital diagram using the short-hand method for Barium.