Final Exam. OFB Chapter 16 & 17 1
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1 Final Exam Monday, April 26, :50-5:40PM Chem Annex Room 16 Final 25% of Overall grade Multiple Choice, no partial credit, no extra credit Chapters covered Part A Chapters 1-6 Part B Chapters 7-10 Part C Chapters Part D Chapters Crib Sheets allowed 4 pages A-D above single sided, handwritten Grade Improvement Plan If Part A > Exam 1, Part A score replaces Exam 1 If Part B > Exam 2, Part B score replaces Exam 2 If Part C > Exam 3, Part C score replaces Exam 3 Will use Final Exam total, as sum Parts A+B+C+D OFB Chapter 16 & 17 1
2 Chapter 16 Quantum Mechanics and the Hydrogen Atom 16-1 Waves and Light 16-2 (skip) Paradoxes in Classical Physics 16-3 Planck, Einstein and Bohr 16-4 Waves, Particles and the Schrödinger Equation only Schrödinger equation 16-5 The Hydrogen Atom OFB Chapter 16 & 17 2
3 16-1 Waves and Light A Light Version Electromagnetic Radiation Energy travels through space by electromagnetic radiation Examples, sunlight, microwave ovens, cell phones, X-rays, radiant heat forma fireplace, AM/FM radio, colors from fireworks All travel as waves All travel as the speed of light OFB Chapter 16 & 17 3
4 OFB Chapter 16 & 17 4
5 XXXXXXXXXXXXXXXXXXXXx The electro magnetic spectrum. The frequency doubles 80 times from right to left in the top diagram The wavelength doubles 80 times from left to right in the top diagram Visible light is confined within a single doubling near the middle OFB Chapter 16 & 17 5
6 OFB Chapter 16 & 17 6
7 Important Equations c = 3 x 10 8 m per second λ = wavelength ν = frequency h = Planck s constant h = 6.62 x Js or h = 6.62 x kg m 2 s -1 OFB Chapter 16 & 17 7
8 AM 890 khz Radio Waves c = λν 890,000 waves per second Wavelength is 337 meters (about 1/5 mile) FM 99.1 MHz 99,100,000 waves per second Wavelength is 3 meters (about 10 feet) OFB Chapter 16 & 17 8
9 Problems: General given two values, calculate the third, c is constant 3 X10 8 m/s Problem The laser in an audio compact disc (CD) player uses light with a wavelength of 780 nm. What is the frequency of the light emitted from the laser? OFB Chapter 16 & 17 9
10 Problem The brilliant red color seen in fireworks displays is due to 4.62 x s -1 strontium emission. Calculate the wavelength of the light emitted. c = λν λ = = 8 c 3x10 m/s = 14 ν 4.62x10 s 7 6.5x10 m m = 1nm λ = 650nm OFB Chapter 16 & 17 10
11 16-2 (skip) Paradoxes in Classical Physics OFB Chapter 16 & 17 11
12 16-3 Planck, Einstein, and Bohr 1901 Max Planck found that light (or energy) was quantized Quite a surprise as light was thought to be continuous Energy can be gained or lost only in integer multiples of hν. n are whole numbers (1,2,3, ) H is Planck s constant Determined experimentally h = 6.628X10-34 J s Each unit of size hν is called a packet or quantum OFB Chapter 16 & 17 12
13 Problem Blue fireworks (typically CuCl) emit light of 450 nm. What is the energy of the light emitted at 450 nm c = λν E = hν Rearrange and combine E = h c λ = 6.67x10 34 J 8 3x10 m/s s 450x10 9 m = 4.41x10 19 J OFB Chapter 16 & 17 13
14 1905 Einstein suggested that electromagnetic radiation can be viewed as a stream of particles called photons About the same time, Einstein derived his famous equation E = mc 2 The main significance is that energy has mass OFB Chapter 16 & 17 14
15 OFB Chapter 16 & E = mc 2 Rearrange = = = λ c h hν E c E m where 2 λc h c λ c h m c E m a photon mass of 2 2 = = =
16 Atomic Spectra of Hydrogen 1.) H 2.)H 2 High Energy Spark H * Radiative Decay (Excited State) hν emission E n = E E E hc λ 3 = 2 = 1 = n hc λ hc λ λ 3 2 hc OFB Chapter 16 & * (Excited State) quantized energy n is excited state orbitals N = 1, 2, 3, blue emission green emission red emission
17 n=4 E n e r g y n=3 n=2 E 3 = hc λ 3 blue emission E 2 = hc λ 2 green emission GS n=1 Quantized Emissions E 1 = hc λ 3 red emission OFB Chapter 16 & 17 17
18 The Bohr Model electron nucleus called a Planetary Model E E hc 3 = λ 3 blue emission n=3 n=2 n=1 E hc 2 = λ 2 green emission E hc 1 = λ 3 red emission Orbital Transition Diagram OFB Chapter 16 & 17 18
19 r Bohr calculated the angular momentum, radius and energy of the electrons traveling in discrete orbits Angular Momentum = m vr n n n h = n n = 1,2,3,... 2π 2 n = a0 = radius of each orbital Z a called the bohr radius, a constant 0 = orbitals, excited states = 1,2,3,... n = 1 called ground state Z is the postive charge on the nucleus (1of E n H, 2 for He, etc.) = Z n 2 2 OFB Chapter 16 & e (2.18x10 18 Calculated levels match those on the photographic plate shown earlier J)
20 Schrödinger Equation Ĥψ = Eψ Results in many solutions, each solution consists of a wave function, ψ (n, l, m l ) called quantum numbers ψ = a wave function which defines an electrons position in 3D space (x, y, z), called an orbital ψ 2 = the probability that an electron is in a certain region of space This defines the shape of the orbital (s, p, d, f) OFB Chapter 16 & 17 20
21 Solutions to the Schrödinger Equation ψ (n, l, m l ) n = principal quantum number n = 1, 2, 3, n is related to the size and energy of the orbital l = azimuthal quantum number l = 0, 1,. (n-1) l is related to the shape of the orbital l = 0 is called an s orbital l = 1 is called a p orbital l = 2 is called a d orbital l = 3 is called an f orbital l = 4 is called a g orbital OFB Chapter 16 & 17 21
22 Solutions to the Schrödinger Equation m l = magnetic quantum number m l = -l,, 0,.+l m l relates to the orientation of the orbital Although not a solution to the Schrödinger Equation, a 4th quantum number is m s = electron spin quantum number m s = +1/2, -1/2 denoted by OFB Chapter 16 & 17 22
23 First four levels of Orbitals in hydrogen n l orbital designation m l # of orbitals 1 0 1s s p -1, 0, s p -1, 0, d -2, -1, 0, +1, s p -1, 0, d -2, -1, 0, +1, f -3, -2, -1, 0, +1, +2, +3 7 n n is related to the size and energy of the N vs orbital l l is related to the shape of the orbital m l relates to the orientation of the orbital l OFB Chapter 16 & 17 23
24 OFB Chapter 16 & 17 24
25 N vs l n l orbital designation m l # of orbitals 1 0 1s s p -1, 0, s p -1, 0, d -2, -1, 0, +1, s p -1, 0, d -2, -1, 0, +1, f -3, -2, -1, 0, +1, +2, +3 7 n is related to the size and energy of the orbital l is related to the shape of the orbital m l relates to the orientation of the orbital OFB Chapter 16 & 17 25
26 n l orbital designation m l # of orbitals 1 0 1s s p -1, 0, s p -1, 0, d -2, -1, 0, +1, s p -1, 0, d -2, -1, 0, +1, f -3, -2, -1, 0, +1, +2, +3 7 n is related to the size and energy of the orbital l is related to the shape of the orbital m OFB Chapter 16 & l relates to the orientation of the orbital
27 F- Orbitals G-Orbitals OFB Chapter 16 & 17 27
28 Chapter 16 Quantum Mechanics and the Hydrogen Atom Example / exercise 16-1, 16-5 Problems 14, 16, 22, 28, 34, 41 OFB Chapter 16 & 17 28
29 Chapter 17 Many-Electron Atoms and Chemical Bonding 17-1 Many-Electron Atoms and the Periodic Table 17-2 Experimental Measures of Orbital Energies 17-3 Sizes of Atoms and Ions 17-4 Properties of the Chemical Bond 17-5 Ionic and Covalent Bonds 17-6 Oxidation States and Chemical Bonding OFB Chapter 16 & 17 29
30 Chapter 17 Many Electron Atoms and Chemical Bonding ψ (n, l, m l ) called quantum numbers n is related to the size and energy of the orbital l is related to the shape of the orbital m l relates to the orientation of the orbital m s is electron spin quantum number Aufbau Principle (building up) Pauli Exclusion Principle No 2 electrons in an atom can have the same set of quantum numbers n, l m l, m s OFB Chapter 16 & 17 30
31 Chapter 17 Many Electron Atoms and Chemical Bonding Aufbau Principle (building up) Pauli Exclusion Principle No 2 electrons in an atom can have the same set of quantum numbers Hund s Rule n, l m l, m s When several orbitals are of equal energy, a single electron enters each orbital before a second electrons. In addition, the spins remain parallel until the second orbital enters the orbital. OFB Chapter 16 & 17 31
32 OFB Chapter 16 & 17 32
33 Hund s Rule When several orbitals are of equal energy, a single electron enters each orbital before a second electrons. In addition, the spins remain parallel until the second orbital enters the orbital. OFB Chapter 16 & 17 33
34 Paramagnetic: Attracted into a magnetic field Have one or more un-paired electrons Diamagnetic: Pushed out of a magnetic field Have paired electrons Carbon (Z = 6) paramagnetic Beryllium (Z = 4) diamagnetic xxx Xxxx xxxxx OFB Chapter 16 & 17 34
35 Electron Configuration Nomenclature 10 Ne: 1s 2 2s 2 2p x2 2p y2 2p z 2 1s 2 2s 2 2p 6 [He]2s 2 2p 6 [Ne] OFB Chapter 16 & 17 35
36 OFB Chapter 16 & 17 36
37 OFB Chapter 16 & 17 37
38 Exercise (pg 730): The ground-state electron configuration of an atom is 1s 2 2s 2 2p 6 3s 2 3p 3. Name the atom. Is it paramagnetic? If so, state how many unpaired electrons it has. 15-electron atom; Phosphorus 1s 2s 2p x 2p y 2p z 3s 3p x 3p y 3p z This is paramagnetic with three unpaired electrons. OFB Chapter 16 & 17 38
39 Valence Electrons Are electrons that can become directly involved in chemical bonding They occupy the outermost (highest energy) shell of an atom Beyond the immediately preceding noble-gas configuration Among the s-block and p-block elements, the valence electrons include electrons in s and p sub shells only OFB Chapter 16 & 17 39
40 Valence Electrons Among the s-block and p-block elements, the valence electrons include electrons in s and p sub shells only Among d-block and f-block (transition elements), valence electrons usually consist of electrons in s orbitals plus electrons in unfilled d and f sub shells OFB Chapter 16 & 17 40
41 Problem: Write the valance-electron configuration and state the number of valence electrons in each of the following atoms and ions: (a) Y, (b) Lu, (c) Mg 2+ (a) Y (Yttrium): atomic number Z = 39 [Kr] 5s 2 4d 1 3 valence electrons (b) Lu (Lutetium): Z = 71 [Xe] 6s 2 4f 14 5d 1 Note filled 4f sub shell 3 valence electrons (c) Mg 2+ (Magnesium (II) ion): Z = 12 This is the 2+ ion, thus 10 electrons [Ne] configuration or 1s 2 2s 2 2p 6 0 valence electrons OFB Chapter 16 & 17 41
42 The filling sub shells and the structure of the periodic table. Anomalous ground-state electron configurations are indicated explicitly All others can be derived from the position of the element in the table OFB Chapter 16 & 17 42
43 PRS transmitters Turn in your transmitters Chem Annex Stockroom Before the end of Finals week, no extensions. Make sure someone signs your form indicating that they received the transmitter Otherwise, a $42 charge will be sent to the Bursar. OFB Chapter 16 & 17 43
44 Chapter 17 Many-Electron Atoms and Chemical Bonding Example / exercise 17-1, 17-2 HW problems 1, 3, 5, 7 OFB Chapter 16 & 17 44
45 Ionization energy of an atom is the minimum amount of energy necessary to detach an electron form an atom that is in its ground state. X X + + e - E = IE 1 X+ X 2+ + e - E = IE 2 OFB Chapter 16 & 17 45
46 Ionization energy first ionization energies IE tends to decrease in a group E.g., Li to Na to K to Rb to Cs E.g., F to Cl to Br to I OFB Chapter 16 & 17 46
47 Electron Affinity of an atom equals the negative energy change of the system when a neutral atom in its ground state gains an electron X + e - X - energy E = electron attachment Electron Affinity = - E = electron attachment energy OFB Chapter 16 & 17 47
48 Electron Affinity X + e - X - energy E = electron attachment EA tends to parallel IE, but shifted one atomic number lower E.g., Halogens much higher EA than noble gases E.g., F to Cl to Br to I OFB Chapter 16 & 17 48
49 Sizes of Atoms and Ions Atomic size generally increases moving down a group Among s-block and p-block elements, atomic size generally decreases moving from left to right OFB Chapter 16 & 17 49
50 Sizes of Atoms and Ions Ionic Radii vs Atomic Number Each line connects a set of atoms or ions having the same charge; all species have noble gas configuration -2>-1>+1>+2>+3>+4 OFB Chapter 16 & 17 50
51 Properties of the Chemical Bond As Bond length increases, bond enthalpy decreases OFB Chapter 16 & 17 51
52 Bond Order and Bond Enthalpies OFB Chapter 16 & 17 52
53 Ionic and Covalent Bonds Electronegativity of an atom is a measure of its ability in a molecule to attract electrons to itself O C H 3 C CH 3 δ- δ+ O C Ohasapartial negative C has a partial positive charge OFB H 3 CChapter 16 CH & Acetone Acetone
54 Ionic and Covalent Bonds Percent Ionic Character OFB Chapter 16 & 17 54
55 Oxidation State and Chemical Bonding OFB Chapter 16 & 17 55
56 Oxidation State and Chemical Bonding OFB Chapter 16 & 17 56
57 Oxidation State and Chemical Bonding Transition Elements OFB Chapter 16 & 17 57
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