Lecture outline: Chapter 6 Electronic structure of atoms
|
|
- Antony Harrell
- 6 years ago
- Views:
Transcription
1 Lecture outline: Chapter 6 Electronic structure of atoms 1. Radiant energy 2. Quantum effects 3. The Bohr atom, orbitals 4. Many electron systems 1
2 Electronic structure of atoms Understanding the arrangement of electrons in atoms is the key to understanding ng the reactivity ty of atoms and molecules Total number of electrons in atom Locations of electrons in space Energy states of electrons 2
3 The atom is mostly empty space! Nucleus (proton(s) and neutron(s) ~10-18 cm electron: orbits the nucleus multielectron atoms have more than one e- orbiting the nucleus ~10-13 cm Diameter of atom ~ 10-8 cm (~1-5 Å) 3
4 The superstars of chemical physics Max Planck Albert Einstein Niels Bohr Werner Heisenberg Erwin Schrodinger 4
5 Electromagnetic radiation Carries energy Many types Moves Wavelike character 5
6 Properties of waves Regular rise and fall pattern Repeating periodicity Peak maxima and peak minima Wavelength (λ, lambda): the distance from one peak maximum to the next Frequency (ν, nu): the number of peak maxima that are passed per unit time Amplitude: the height of the peak maxima and minima from the central axis λ Amplitude 6
7 Some waves with different wavelengths λ 1 and amplitudes λ 2 λ 3 7
8 Electromagnetic waves Carry energy Electrical and magnetic components Classified based on wavelength Move at a constant speed (c) No propagating medium needed 8
9 1 7/8 1/8 3/4 1/4 1.0 sec/turn 5/8 3/8 1/2 Frequency (ν, nu): the number of peak maxima that are passed per unit time as the wave propagates ν = 16 maxima /second = 16s -1 = 16 hz 3.0 x 10 8 m ν = 8 maxima /second = 8s -1 =8hz 3.0 x 10 8 m ν = 4 maxima /second = 4s -1 = 4 hz 9
10 Proportionality Two variables are proportional if a change in the value of one results in a change in the value of the other, and if the two values are related mathematically by a constant t ( k ) Directly proportional: y x y = k x Inversely proportional: x y 1 x y = k x 1 y x = k 1 y 10
11 What is the difference between AM and FM radio? 11
12 Electromagnetic Spectrum This file is licensed under the Creative Commons Attribution-Share Alike 3.0 Unported license. 12
13 Author Inductiveload, NASA GNU Free Documentation License, Version
14 Unit commonly used for wavelengths Unit Symbol Meaning Radiation (10 n ) type meter m 1 TV, radio centimeter cm 10-2 microwave millimeter mm 10-3 infrared micrometer μm 10-6 infrared nanometer nm 10-9 UV, visible Angstrom Å X-ray, gamma ray Author: Victor Blacus, licensed under the Creative Commons Attribution-Share Alike 3.0 Unported license 14
15 How many peak maxima does red light with a wavelength of 649 nm pass in one second? In other words, what is the frequency of 649 nm light? c = λν 15
16 What is the wavelength of Q92.1 FM radiowaves? c=λν 16
17 Quantum effects: Planck 1900: Max Planck Energy is released/absorbed only in discrete units, packets, or quanta A quantum is the smallest quantity or packet of a given form of electromagnetic radiation Energy is quantized E = hν 17
18 Quantum analogies 18
19 What is the energy associated with 1 quantum of: (1) () 649 nm red light (ν = 4.62 x Hz) (2) a Q92.1 radiowave (ν = 92.1 MHz) (3) a medical x-ray (ν = 9.55 x Hz) E = hν 19
20 Photons: Einstein An explanation for a phenomenon known as the photoelectric effect e - Red light e - e - Blue light e - Light energy absorbed e - Sodium metal Sodium metal 20
21 Photons: Einstein An explanation for a phenomenon known as the photoelectron effect Electromagnetic radiation behaves as if composed of a stream of particles, or photons The energy of one photon = the energy of one quantum 21
22 The dual nature of electromagnetic radiation Light behaving as a wave: Light behaving as a particle: Light behaving as both a wave and a particle: 3.0 x 10 8 m in one second 22
23 The dual nature of light for three wavelengths λ 1 ν = 16 maxima /second = 16s -1 = 16 hz λ 2 ν = 8 maxima /second = 8s -1 = 8h hz λ 3 ν = 4 maxima /second = 4s -1 =4hz 1 second 23
24 Both matter and energy are quantized (exist only in discrete units) Matter: 1 H atom 1.5 H atoms 2 H atoms 2.3 H atoms 3 H atoms 3.7 H atoms Energy: 1 photon 1.5 photons 2 photons 3 photons 2.3 photons 3.7 photons 24
25 What is the energy associated with 1 mol of photons of: (1) 649 nm red light (ν = 4.62 x Hz) E = nhν (2) a Q92.1 radiowave (ν = 92.1 MHz) (3) a medical x-ray (ν = 9.55 x Hz) 25
26 Niels Bohr: a model for the hydrogen atom Based on a phenomenon of atoms and light known as line spectra 26
27 Monochromatic vs. polychromatic light Monochromatic light: light (radiation) of a single wavelength (ex.: laser light) Visible light: composed of light (radiation) of many different wavelengths 27
28 Scattering of visible light through a prism commons.wikimedia.org/wiki/file:arcoiris_high_contrasted_and_filtere d.jpg This work has been released into the public domain by its author, I, Alfredo55. Credit: D-Kuru/Wikimedia Commons, licensed under the Creative Commons Attribution-Share Alike 3.0 Austria license. 28
29 Attribution: User Kieff, Released into public domain 29
30 What would happen to the light of a laser if you shined it through a prism? Author Netweb, Creative Commons Attribution-Share Alike 3.0 Unported license. 30
31 Electron excitation and relaxation gives rise to all of the color that we observe! Source light Reflected light How does it work???? 31
32 The heat of the flame excites an electron to a higher energy state. When the electron relaxes back to the ground state, energy is released as visible light. Li Na K Cu Pb 32
33 Scattering of the light emitted by an + excited atom through a prism H 2 Emitted light E = hν = hc λ - Prism Line spectra: 410 nm 486 nm 656 nm 434 nm 33
34 Bohr s postulates 1. Only electron orbits of certain energies are allowed (the energy of an e - is quantized) 2. An electron in a permitted orbit has a specific energy (an allowed energy state ) 3. An electron in an allowed state is stable and will not radiate energy 34
35 Some simple models to illustrate the idea of quantized orbits and electron energies n = 3 hνν n=4 E = = hc λ electron absorbs radiant energy nucleus n = 1 n=2 E in n = 1 is the ground state allowed orbit n > 1 is an excited state allowed orbit n = 1 n = 2 electron absorbs radiant energy n = 3 n=4 35
36 Some simple models to illustrate the idea of quantized orbits and electron energies n = 3 E hνν n=4 E = = hc λ electron emits radiant energy nucleus n = 1 n=2 n = 1 is the ground state allowed orbit n > 1 is an excited state allowed orbit n = 3 E out n = 2 electron emits radiant n = 1 energy n=4 36
37 The energy of an orbit is referenced relative to the electrons zero point energy, the point where the electron has been completely removed from the atom ΔE = E final E initial Increasing E ΔE 2 3 Zero point E = 0 n = 6 n = 5 n = 4 ΔE 3 4 n = 3 n = 2 First excited state n = n = 8 n = 7 ΔE (+) for removing an electron from the atom s ground state orbit ΔE 1 2 n = 1 Ground state E = (-) 37
38 An electron can jump (or relax) from any one orbit to another ΔE = E final E initial Increasing E ΔE 1 4 Zero point E = 0 n = 2 n = 6 n = 5 n = 4 n = 3 First excited state n = n = 8 n = 7 ΔE (+) for removing an electron from the atom s ground state orbit n = 1 Ground state E = (-) 38
39 The energy of an orbit is referenced relative to the electrons zero point energy, the point where the electron has been completely removed from the atom ΔE = E final E initial Increasing E ΔE 2 3 Zero point E = 0 n = 6 n = 5 n = 4 ΔE 3 4 n = 3 n = 2 First excited state n = n = 8 n = 7 ΔE (-) for placing an external electron in the atom s ground state orbit ΔE 1 2 n = 1 Ground state E = (-) 39
40 Energy levels in the Bohr atom nucleus n = 1 n = 2 n = 3 n = 4 E = (-R )( 1 n H 2 n R = 218x10-18 H J ) ΔE =E final E initial n = 4 n = 2 n = (R )( ) = H 2 n n ΔE E = 2 i f hν n = 1 40
41 When an excited electron in the n=4 orbit relaxes directly to the ground state orbit (n = 1), what wavelength of energy is released? Zero point E = 0 n = 6 Increasing E n = 5 n = 4 ΔE 1 4 n = 3 n = 2 n = 8 n = 7 λ = c ν 1 1 ΔE = (RH )( ) = 2 2 n n i f n = hν n = 1 Ground state E = (-) 41
42 When an excited electron in the n=4 orbit relaxes directly to the ground state orbit (n = 1), what wavelength of energy is released? 1 1 ΔE = (RH )( ) = hν c λ = En = (-RH )( ) 2 n n n i f ν 42
43 Electron excitation and relaxation gives rise to all of the color that we observe! Source light Reflected light What is the difference between a normal incandescent lightbulb and a halogen lightbulb? 43
44 Summary of energy and matter Radiant energy has wavelike properties Radiant energy is quantized (can only exist in discrete packets) Radiant energy has particle like properties Matter (sp., the e-) has particle like properties The energies/orbits of matter are quantized Does matter have wavelike properties? 44
45 The debroglie wavelength of matter h λ = mv velocity Note: lower case v is velocity The greek letter nu is ν, which is frequency Don t confuse the two! 45
46 What is the wavelength of a baseball (120 g) travelling at a speed of 100 mph (44.7 m/s)? λ = h mv 46
47 Heisenberg The dual nature of matter (a particle and a wave) places limitations on the preciseness with which we can know both the location and the momentum (mass x velocity) of an object Know location precisely, then momentum is uncertain Know momentum precisely, then location is uncertain How does this apply to the electron? 47
48 Compare the sizes and wavelengths of the following moving obects: λ = h mv object mass velocity diameter λ ratio λ to diameter baseball 0.12 kg 45 m/s 0.08 m 1.24 x m 1.5 x earth 6.0 x kg 2.98 x 10 4 m/s x 10 7 m 3.71 x m 2.9 x electron 9.11 x kg 1 x 10 6 m/s m 1.22 x m 1.2 x
49 What does all of this mean for electronic structure??!? Schrodinger: The behavior of the electron is better described by focusing on it s wavelike properties p An orbit: a defined, known pathway An orbital: a probability function; the probability that an electron will be found in a given location A description of the distribution of electron density in space Orbitals have a characteristic shape and energy 49
50 The n = 1 orbital Each dot represents a position where an electron may be found at any given moment with respect to the nucleus, which is at the center of the axes 50
51 An overview of the quantum mechanical model of the atom Electrons reside in areas of space called orbitals Orbitals have defined energies, shapes and sizes n = principal p quantum number = shell Subshells are energy levels within shells that have defined shapes (s, p, d, f) Orbitals of a given shape (within a subshell) have a specific orientation in space 51
52 Orbital quantum numbers n (principal) describes the energy of the orbital n = 1,2,3,4 shells l (azimuthal) describes the 3-dimensional i shape of fthe orbital (subshells) l values for a given n n are integers from 0 to n-1 m l (magnetic) describes the orientation of an orbital in space m l values for a given subshell are integers from -l to +l (2l + 1 possible orbitals for each subshell) A specific orbital is defined by specific and unique values for n, l, and m l 52
53 The n = 1 orbital n Allowed values for l: integers from 0 to n-11 Allowed values for m l : integers from -l to +l n = 2 n = 3 = 4 Shell Subshell Orbital Orbital Orbital Orbital # (n) # (l) # (m l ) name shape orientation n= s spherical symmetric z y x s n = 1 l = 0 m l = 0 There is only one orbital in n = 1 (1,0,0) 53
54 The n = 2 orbitals n Allowed values for l: integers from 0 to n-11 Allowed values for m l : integers from -l to +l n = 2 n = 3 = 4 Shell # (n) Subshell # (l) Orbital # (m l ) Orbital name Orbital shape p n=1 Orbital orientation s spherical Symmetric with a wave node p y Dumbbell/ elipsoid about node centered on y axis p z Dumbbell/ about node centered on z axis elipsoid p x Dumbbell/ elipsoid about node centered on x axis There are four orbitals in n = 2 (2,0,0; 2,1,-1; 2,1,0; 2,1,1 ) 54
55 The four n = 2 orbitals n = 4 n = 3 2s 2p y 2p z 2p x n = 2 1s n = 1 55
56 The four n = 2 orbitals 2s 2p y 2p z 2p x z z y y z y z y x x x x 2s spherical n = 2 l = 0 m l = 0 2p y 2p z 2p x Dumbbell (elipsoid) n = 2 n = 2 n = 2 l = 1 l = 1 l = 1 m l = -1 m l = 0 m l = 1 56
57 2p orbitals n energy shell l shape subshell m l orientation orbital n = 2 n = 2 n = 2 l = 1 l = 1 l = 1 m l = 1 z y m l = 0 z y m l = -1 z y x x x p x p z p y 57
58 Compare the 1s and 2s orbitals z z y node y x x 1s 2s node 58
59 The n = 3 orbitals n Allowed values for l: integers from 0 to n-11 Allowed values for m l : integers from -l to +l n = 2 n = 3 = 4 Shell Subshell Orbital Orbital Orbital Orbital orientation # (n) # (l) # (m l ) name shape s spherical Symmetric with 2 wave nodes p y Dumbbell about node centered on y axis p y p z Dumbbell about node centered on z axis p x Dumbbell about node centered on x axis n= d xy 4 pears four quadrants of xy plane d yz 4 pears four quadrants of yz plane d z2 2 pears to one torus 2 pears in z axis, torus to pears d xz 4 pears Centered about and on x and y axes d x2-y2 4 pears four quadrants of xy plane 59
60 The nine n = 3 orbitals 3s, 3p y, 3p z, 3p x, 3d xy, 3d yz, 3d z2, 3d xz, 3d x2-y2 l = 0 l = 1 l = 2 n=4 n = 3 n = 2 n = 1 60
61 The nine n = 3 orbitals 3s, 3p y, 3p z, 3p x, 3d xy, 3d yz, 3d z2, 3d xz, 3d x2-y2 l = 0 l = 1 l = 2 3s (cutaway 3p y 3p z 3p x view) 3d xy 3d yz 3d z2 3d xz 3d x2-y261
62 The five 3d orbitals y x z y x x z y z 3dxz 3dxy 3dyz x z x y 3dx2-y2 y z 3dz2 62
63 The 1s, 2s, and 3s orbitals n = 1 n = 2 n = 3 l = 0 l = 0 l = 0 m l = 0 m l = 0 m l = 0 63
64 s radial pro obability s 0.1 3s Distance from nucleus 64
65 The n = 4 orbitals n Allowed values for l: integers from 0 to n-11 Allowed values for m l : integers from -l to +l n = 2 n = 3 = 4 Shell # (n) Subshell # (l) Orbital # (m l ) Orbital name Orbital shape n=1 Orbital orientation s spherical Symmetric with 3 wave nodes 4 1-1, 0, 1 4p y, 4p z, 4p x Dumbbell Centered about and on x, y and z axes 4 2-2, -1, 4d xy,, 4d yz,, 4 pears and As for 3d orbitals 0, 1, 2 4d z2, 4d xz, 2 pears to 4d x2-y2 one torus 4 3-3, -2, - 1, 0, 1, 2, 3 4f z3, 4f xz2, 4f yz, 4f xyz, 4f 2 2 z(x y ), 4f x(x 3y ), 4f ( ) Pretty complicated! Pretty complicated! 4f y(3x 2 y 2 ) 65
66 The sixteen n = 4 orbitals 4s, 4p y, 4p z, 4p x, 4d xy, 4d yz, 4d z2, 4d xz, 4d x2-y2 4f x 7 l = 0 l = 1 l = 2 l = 3 n = 4 n = 3 n = 2 n = 1 66
67 The seven f orbitals: difficult to draw, rarely encountered in your daily life 67
68 0 to n-1 allowed values -l to +l allowed values for each value of l n l Subshell m l value # of orbitals #oforbitals orbitals value value name in subshell in shell 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,
69 Principal quantum Number of subshells (l) Subshell name (type of number n (shell) orbital) m l 1 1 s 2 2 s, p 3 3 s, p, d 4 4 s, p, d, f 5 5 s, p, d, f, g Type of subshell Number of orbitals in that subshell s 1 p 3 d 5 f 7 69
70 Atomic orbitals summary n = 1: One orbital 1s n = 2: Four orbitals: 2s 2p x, 2p y, 2p z n = 3: nine orbitals: 3s 3p x, 3p y, 3p z 3d xy, 3d yz, 3d z2, 3d xz, 3d x2-y2 n=4:sixteenorbitals: 4s 4p x, 4p y, 4 pz 4d xy, 4d yz, 4d z2, 4d xz, 4d x2-y2 4f x 7 70
71 Orbitals for the 1 st four energy levels of the H atom Zero point E = 0 n = Increasing E 4s 4p 4d 4f n = 4 3s 3p 3d n = 3 2s 2p n = 2 1s n = 1 Ground state E = (-) 71
72 Energies of the orbitals in n=1 to 4 for the H atom n = n = 4 n = 3 4s 3s 4p 4d 4f 3p 3d creasing E n = 2 2s 2p In n = 1 1s 72
73 Energies of the orbitals in n=1 to 4 for the H atom creasing E n = n = 4 n = 3 n = 2 Shells (energies) In 4s 3s 2s 4p 4d 4f 3p 3d subshells 2p Specific orbitals: defined orientations in space (orbital shapes) subshells (orbital shapes) n = 1 1s 73
74 Multielectron atoms All of the considerations to now were developed for the H atom with a single electron How does the quantum mechanical model apply to multielectron atoms? Same quantum numbers, shapes, orbitals Maximum of 2 electrons can occupy each orbital Energies of orbitals are affected by presence of other electrons in other orbitals 74
75 Principle energies are lower in multielectron atom Energies of subshells are split in multielectron atoms Some crossover of energy levels in multielectron atoms results in certain subshells having lower energies than subshells with lower n values Increasing E n = n = 4 n = 3 n =2 4s 3s 2s 4p 4d 4f 3p 3d 2p ΔE 1 2 ncreasing E I 6s 5s 4s 3s 5p 4p 3p 2p 4d 3d 4f 2s ΔE 1 2 n =1 1s 1s Energy levels of the single electron atom Energy levels of the multielectron atom, where additional electrons occupy higher energy orbitals in succession 75
76 Electrostatic interactions are responsible for the differences in energies for the single- and multielectron atoms Zp+ n = 1 n = 4 n = 3 n = 2 76
77 The spin quantum number, m s N S S N m s = +1/2 m s = -1/2 77
78 How do electrons populate orbitals in a multielectron atom? The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n energy shell l shape subshell m l orientation orbital m s electron spin clockwise (CW) or CCW 78
79 Populating orbitals in a multielectron atom 6s 5s 5p 4p 4d 4f 4s 3d Increas sing E 3s 2s 3p 2p The Pauli exclusion principle: p No two electrons in an atom can have the same set of four quantum numbers Electrons want to occupy the lowest energy orbital available 1s
80 4p Increa asing E 4s 3s 2s 3p 2p 3d The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n energy shell l shape subshell m l orientation orbital l m s electron spin clockwise (CW) or CCW Electrons want to occupy the lowest energy orbital available Represent an electron by a single sided arrow: and 1s 80
81 4p Increa asing E 4s 3s 2s 3p 2p n = 1 3d The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n energy shell l shape subshell m l orientation orbital m s electron spin clockwise (CW) or CCW Electrons want to occupy the lowest energy orbital available l = 0 The H atom: one e- 1s m l = 0 m s = +1/2 81
82 n value l value Subshell name m l value # of orbitals in subshell # of orbitals in shell Increa asing E 4p 3d 4s 3p 3s 2p 2s n = 1 n =1 l = 0 l = 0 m l = 0 m l = 0 m s = +1/2 m s = -1/ s 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 The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n energy shell l shape subshell m l orientation orbital m s electron spin clockwise (CW) or CCW Electrons want to occupy the lowest energy orbital available 1s The He atom: two e- 82
83 4p Increa asing E 4s 3s 2s 3p 2p n = 2 l = 0 m l = 0 3d The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n energy shell l shape subshell m l orientation orbital m s electron spin clockwise (CW) or CCW 0 Electrons want to occupy the lowest energy orbital available m s = +1/2 1s n = 1 n = 1 l = 0 l = 0 m l = 0 m l = 0 m s = +1/2 m s = -1/2 The Li atom: 3 e- 83
84 4p Increa asing E 4s 3s 2s 3p 2p n = 2 l = 0 m l = 0 m s = +1/2 n = 2 l = 0 m l = 0 3d The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n energy shell l shape subshell m l orientation orbital m s electron spin clockwise (CW) or CCW 0 Electrons want to occupy the lowest energy orbital available m s = -1/2 1s n = 1 n = 1 l = 0 l = 0 m l = 0 m l = 0 m s = +1/2 m s = -1/2 The Be atom: 4 e- 84
85 4p Increa asing E 4s 3s 2s 3p 2p n = 2 l = 0 m l = 0 m s = +1/2 3d n = 2 l = 0 m l = 0 m s = -1/2 The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers n = 2 l = 1 m l = 1 m s = +1/2 Electrons want to occupy the lowest energy orbital available 1s n = 1 n = 1 l = 0 l = 0 m l = 0 m l = 0 m s = +1/2 m s = -1/2 The B atom: 5 e- 85
86 Thegistofallthis: this: An electron will occupy the lowest energy orbital that is available A maximum of two electrons can occupy any given orbital (Pauli exclusion principle) 86
87 4p The B atom: 5 e- Increa asing E 4s 3s 3p 2p 3d An electron will occupy the lowest energy orbital that is available A maximum of two electrons can occupy any given orbital (Pauli exclusion principle) 2s 1s 87
88 Hund s rule For degenerate orbitals (orbitals of the same energy), the lowest energy is attained when the number of electrons with the same spin is maximized Two e- with different spins Two e- with same spins 88
89 Increa asing E 4s 3s 2s 4p The C atom: 6 e- 3d An electron will occupy the lowest 3p energy orbital that is available A maximum of two electrons can occupy any given orbital (Pauli exclusion principle) 2p For degenerate orbitals (orbitals of the same energy), the lowest energy is attained when the number of electrons with the same spin is maximized 1s 89
90 Increa asing E 4s 3s 2s 4p The N atom: 7 e- 3d An electron will occupy the lowest 3p energy orbital that is available A maximum of two electrons can occupy any given orbital (Pauli exclusion principle) 2p For degenerate orbitals (orbitals of the same energy), the lowest energy is attained when the number of electrons with the same spin is maximized 1s 90
91 4p The O atom: 8 e- 4s 3d Increa asing E 3s 2s 1s 3p An electron will occupy the lowest energy orbital that is available 2p A maximum of two electrons can occupy any given orbital (Pauli exclusion principle) For degenerate orbitals (orbitals of the same energy), the lowest energy is attained when the number of electrons with the same spin is maximized 91
92 4p The O atom: 8 e- Increa asing E 4s 3s 2s 3p 2p 3d A faster way to draw orbital filling: 1s 1s 2s 2p 3s 3p 4s 92
93 Electron configuration for the O atom 1s 2s 2p 3s 3p 4s Electron configuration: 1s 2 2s 2 2p 4 4p 4s 3d Incr reasing E 3s 2s 3p 2p 1s 93
94 Write electron configurations for n = 2 and n = 3 elements 4p Increasing E 4s 3s 2s 3p 2p 3d 1s 1s 2s 2p 3s 3p 4s 3d 4p 94
95 Write electron configurations for n = 4 elements 4p Increasing E 4s 3s 2s 3p 2p 3d 1s 1s 2s 2p 3s 3p 4s 3d 4p 95
96 Rules for adding electrons to orbitals Electrons go into the lowest energy orbital available For a given n shell, s orbitals are lower in energy than p which are lower in energy than d which are lower than f Only two electrons can occupy a given orbital For orbitals of the same energy, one electron will occupy each orbital before they start pairing up Some energy level crossovers occur due to electrostatic effects 96
97 Two easy ways to keep track of the order of orbital filling in multielectron atoms Use the periodic table to guide you The principle quantum number of d block elements is one less than that of the adjacent s and p block elements The principle quantum number of f block elements is two less than that of the adjacent s and p block elements, and one less than the adjacent d block Even easier: use the Auf-Bau principle 97
98 The periodic table color coded by the type of subshell being filled 1s 1s 2s 2p 3s 4s 5s 6s 7s 3d 4d 5d 6d 3p 4p 5p 6p 7p 4f 5f 98
99 The periodic table color coded by principle quantum number of the orbital being filled 1s2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 99
100 The periodic table color coded by principle quantum number of the orbital being filled 1s2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p
101 The Auf-Bau Rule : The Order in which the Orbitals Fill in Polyelectronic Atoms 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 14 5s 2 5p 6 5d 10 5f 14 6s 2 6p 6 6d 10 6f 14 7s 2 7p 6 Follow this rule and you can t go wrong!! 1s2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 101
102 Write electron configurations for n = 5 elements Increasing E 6s 5p 5s 4d 4p 3d 4s 3p 3s 2p 2s 4f 1s 2 2s 2 2p 6 1s 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 14 5s 2 5p 6 5d 10 5f 14 6s 2 6p 6 6d 10 6f 14 7s 2 7p 6 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 102
103 Write electron configurations for n = 6 elements Increasing E 6s 5p 5s 4d 4p 3d 4s 3p 3s 2p 2s 4f 1s 2 2s 2 2p 6 1s 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 14 5s 2 5p 6 5d 10 5f 14 6s 2 6p 6 6d 10 6f 14 7s 2 7p 6 1s2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 103
104 Electron configurations of the elements Anomolous electron configurations are in red 104
105 Electron configurations of the elements, color coded by subshell type 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 14 5s 2 5p 6 5d 10 5f 14 Anomolous electron configurations are in red 6s 2 6p 6 6d 10 6f 14 7s 2 7p 6 105
Lecture outline: Chapter 6 Electronic structure of atoms. Electronic structure of atoms
Lecture outline: Chapter 6 Electronic structure of atoms 1. Radiant energ 2. Quantum effects 3. The Bohr atom, orbitals 4. Man electron sstems Electronic structure of atoms Understanding the arrangement
More informationElectronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
Chemistry: The Central Science Chapter 6: Electronic Structure of Atoms Electronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
More informationChapter 6 Electronic Structure of Atoms. 許富銀 ( Hsu Fu-Yin)
Chapter 6 Electronic Structure of Atoms 許富銀 ( Hsu Fu-Yin) 1 The Wave Nature of Light The light we see with our eyes, visible light, is one type of electromagnetic radiation. electromagnetic radiation carries
More informationChapter 5. The Electromagnetic Spectrum. What is visible light? What is visible light? Which of the following would you consider dangerous?
Which of the following would you consider dangerous? X-rays Radio waves Gamma rays UV radiation Visible light Microwaves Infrared radiation Chapter 5 Periodicity and Atomic Structure 2 The Electromagnetic
More informationChapter 6 - Electronic Structure of Atoms
Chapter 6 - Electronic Structure of Atoms 6.1 The Wave Nature of Light To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation Visible light is an example
More informationElectromagnetic Radiation All electromagnetic radiation travels at the same velocity: the speed of light (c), m/s.
Chapter 6 Electronic Structure of Atoms Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance between corresponding points on
More informationChapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum. All EM radiation travels at the speed of light, c = 3 x 10 8 m/s
Chapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum V I B G Y O R All EM radiation travels at the speed of light, c = 3 x 10 8 m/s Electromagnetic radiation is a wave with a wavelength
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change Chapter 5: Electrons in Atoms 5 Section 5.1 Section Section 5.3 Table Of Contents Light and Quantized Energy Electron Configuration Compare the wave and particle natures of
More informationChapter 6 Electronic structure of atoms
Chapter 6 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 6.1 The wave nature of light Visible light is
More informationLight. October 16, Chapter 5: Electrons in Atoms Honors Chemistry. Bohr Model
Chapter 5: Electrons in Atoms Honors Chemistry Bohr Model Niels Bohr, a young Danish physicist and a student of Rutherford improved Rutherford's model. Bohr proposed that an electron is found only in specific
More informationElectronic structure of atoms
Chapter 1 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 1.1 The wave nature of light Much of our understanding
More informationUnit 4. Electrons in Atoms
Unit 4 Electrons in Atoms When were most of the subatomic particles discovered? Who discovered densely packed nucleus surrounded by fast moving electrons? Rutherford s Model Major development Lacked detail
More informationDevelopment of the Periodic Table. Chapter 5. Light and the EM Spectrum. Light
Chapter 5 Periodic Table Song Periodicity and Atomic Structure Development of the Periodic Table Mid-1800 s, several scientists placed known elements in order based on different criteria. Mendeleev s and
More informationEnergy and the Quantum Theory
Energy and the Quantum Theory Light electrons are understood by comparing them to light 1. radiant energy 2. travels through space 3. makes you feel warm Light has properties of waves and particles Amplitude:
More informationChapter 6: Electronic Structure of Atoms
Chapter 6: Electronic Structure of Atoms Learning Outcomes: Calculate the wavelength of electromagnetic radiation given its frequency or its frequency given its wavelength. Order the common kinds of radiation
More informationThe Atom & Unanswered Questions:
The Atom & Unanswered Questions: 1) Recall-Rutherford s model, that atom s mass is concentrated in the nucleus & electrons move around it. a) Doesn t explain how the electrons were arranged around the
More informationChapter 7. The Quantum Mechanical Model of the Atom
Chapter 7 The Quantum Mechanical Model of the Atom Quantum Mechanics The Behavior of the Very Small Electrons are incredibly small. Electron behavior determines much of the behavior of atoms. Directly
More information2) The energy of a photon of light is proportional to its frequency and proportional to its wavelength.
Advanced Chemistry Chapter 13 Review Name Per Show all work Wave Properties 1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c 2) The energy of a photon of
More informationChapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
More informationChapter 8: Electrons in Atoms Electromagnetic Radiation
Chapter 8: Electrons in Atoms Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy transmission modeled as waves moving through space. (see below left) Electromagnetic Radiation
More informationI. Multiple Choice Questions (Type-I)
I. Multiple Choice Questions (Type-I) 1. Which of the following conclusions could not be derived from Rutherford s α -particle scattering experiement? (i) Most of the space in the atom is empty. (ii) The
More informationAtomic Structure. Standing Waves x10 8 m/s. (or Hz or 1/s) λ Node
Atomic Structure Topics: 7.1 Electromagnetic Radiation 7.2 Planck, Einstein, Energy, and Photons 7.3 Atomic Line Spectra and Niels Bohr 7.4 The Wave Properties of the Electron 7.5 Quantum Mechanical View
More informationElectron Arrangement - Part 1
Brad Collins Electron Arrangement - Part 1 Chapter 8 Some images Copyright The McGraw-Hill Companies, Inc. Properties of Waves Wavelength (λ) is the distance between identical points on successive waves.
More informationCHAPTER 4 10/11/2016. Properties of Light. Anatomy of a Wave. Components of a Wave. Components of a Wave
Properties of Light CHAPTER 4 Light is a form of Electromagnetic Radiation Electromagnetic Radiation (EMR) Form of energy that exhibits wavelike behavior and travels at the speed of light. Together, all
More informationChapter 6. Electronic Structure of Atoms. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 6 John D. Bookstaver St. Charles Community College Cottleville, MO Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic
More informationChapter 4 Electron Configurations
Chapter 4 Electron Configurations Waves Today scientists recognize light has properties of waves and particles Waves: light is electromagnetic radiation and travels in electromagnetic waves. 4 Characteristics
More informationThe Bohr Model of the Atom
Unit 4: The Bohr Model of the Atom Properties of light Before the 1900 s, light was thought to behave only as a wave. Light is a type of electromagnetic radiation - a form of energy that exhibits wave
More informationCVB102 Lecture 1 - Chemical Structure and Reactivity. Contact Information: Dr. Bill Lot Electronic Structure of Atoms
CVB102 Lecture 1 - Chemical Structure and Reactivity Contact Information: Dr. Bill Lot b.lott@qut.edu.au Electronic Structure of Atoms Text: Blackman, et al Pp. 127-147 (Pp. 148-159 recommended) The periodic
More informationChapter 6. of Atoms. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 6 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall,
More informationChapter 6. of Atoms. Waves. Waves 1/15/2013
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 6 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall,
More informationChapter 4 Arrangement of Electrons in Atoms. 4.1 The Development of a New Atomic Model
Chapter 4 Arrangement of Electrons in Atoms 4.1 The Development of a New Atomic Model Properties of Light Electromagnetic Radiation: EM radiation are forms of energy which move through space as waves There
More informationElectrons in Atoms. Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration
Electrons in Atoms Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration Click a hyperlink or folder tab to view the corresponding slides. Exit
More informationCHEMISTRY - TRO 4E CH.7 - THE QUANTUM-MECHANICAL MODEL OF THE ATOM
!! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of
More informationAP Chemistry. Chapter 6 Electronic Structure of Atoms
AP Chemistry Chapter 6 Electronic Structure of Atoms Section 6.1 Wave Nature of Light When we say "light," we generally are referring to visible light a type of electromagnetic radiation But actually Visible
More informationChapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
More informationWavelength (λ)- Frequency (ν)- Which of the following has a higher frequency?
Name: Unit 5- Light and Energy Electromagnetic Spectrum Notes Electromagnetic radiation is a form of energy that emits wave-like behavior as it travels through space. Amplitude (a)- Wavelength (λ)- Which
More informationThe Electron Cloud. Here is what we know about the electron cloud:
The Electron Cloud Here is what we know about the electron cloud: It contains the subatomic particles called electrons This area accounts for most of the volume of the atom ( empty space) These electrons
More informationChapter 7 Atomic Structure -1 Quantum Model of Atom. Dr. Sapna Gupta
Chapter 7 Atomic Structure -1 Quantum Model of Atom Dr. Sapna Gupta The Electromagnetic Spectrum The electromagnetic spectrum includes many different types of radiation which travel in waves. Visible light
More informationNovember 06, Chapter 7 Atomic Struture. CHAPTER 7 Atomic Structure. Oct 27 9:34 AM ATOMIC STRUCTURE. Oct 27 9:34 AM
CHAPTER 7 Atomic Structure ATOMIC STRUCTURE 1 The Wave Nature of Light Most subatomic particles behave as PARTICLES and obey the physics of waves. Visible light Ultravioletlight Wavelength Frequency (Hertz
More informationElectromagnetic Radiation. is a form of energy that exhibits wavelike behavior as it travels through space.
Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through space. What are the 7 forms of electromagnetic radiation, in order of INCREASING wavelength? gamma rays
More informationChapter 7 QUANTUM THEORY & ATOMIC STRUCTURE Brooks/Cole - Thomson
Chapter 7 QUANTUM THEORY & ATOMIC STRUCTURE 1 7.1 The Nature of Light 2 Most subatomic particles behave as PARTICLES and obey the physics of waves. Light is a type of electromagnetic radiation Light consists
More informationElectrons hold the key to understanding why substances behave as they do. When atoms react it is their outer pars, their electrons, that interact.
Electronic Structure of Atoms The Wave Nature of Light Electrons hold the key to understanding why substances behave as they do. When atoms react it is their outer pars, their electrons, that interact.
More informationUNIT 4 Electrons in Atoms. Advanced Chemistry 235 Lanphier High School Mr. David Peeler
UNIT 4 Electrons in Atoms Advanced Chemistry 235 Lanphier High School Mr. David Peeler Section 4.1 Models of the Atom OBJECTIVES: Identify the inadequacies in the Rutherford atomic model. Section 4.1 Models
More informationChapter 6. Electronic. Electronic Structure of Atoms Pearson Education
Chapter 6 Laser: step-like energy transition 6.1 The Wave Nature of Light 6.2 Quantized Energy and Photons 6.3 Line Spectra and the Bohr Model 6.4 The Wave Behavior of Matter 6.5 Quantum Mechanics and
More informationChapter 7. Characteristics of Atoms. 7.1 Electromagnetic Radiation. Chapter 7 1. The Quantum Mechanical Atom. Atoms: How do we study atoms?
Chapter 7 The Quantum Mechanical Atom 1 Characteristics of Atoms Atoms: possess mass contain positive nuclei contain electrons occupy volume have various properties attract one another combine to form
More informationElectronic Structure of Atoms. Chapter 6
Electronic Structure of Atoms Chapter 6 Electronic Structure of Atoms 1. The Wave Nature of Light All waves have: a) characteristic wavelength, λ b) amplitude, A Electronic Structure of Atoms 1. The Wave
More information5.1 Light & Quantized Energy
5.1 Light & Quantized Energy Objectives: 1. Describe electromagnetic (EM) wave properties & measures 2. Relate visible light to areas of the EM spectrum with higher & lower energy 3. Know the relationship
More informationCh 7 Quantum Theory of the Atom (light and atomic structure)
Ch 7 Quantum Theory of the Atom (light and atomic structure) Electromagnetic Radiation - Electromagnetic radiation consists of oscillations in electric and magnetic fields. The oscillations can be described
More informationBecause light behaves like a wave, we can describe it in one of two ways by its wavelength or by its frequency.
Light We can use different terms to describe light: Color Wavelength Frequency Light is composed of electromagnetic waves that travel through some medium. The properties of the medium determine how light
More informationYellow. Strontium red white. green. yellow violet. green. red. Chapter 4. Arrangement of Electrons in Atoms. Table of Contents
Chapter 4 Arrangement of Electrons in Atoms Table of Contents Section 1 Section 2 Section 3 The Development of a New Atomic Model The Quantum Model of the Atom Electron Configurations Sodium Yellow Strontium
More information2) The number of cycles that pass through a stationary point is called A) wavelength. B) amplitude. C) frequency. D) area. E) median.
Chemistry Structure and Properties 2nd Edition Tro Test Bank Full Download: http://testbanklive.com/download/chemistry-structure-and-properties-2nd-edition-tro-test-bank/ Chemistry: Structure & Properties,
More informationLight. Light (con t.) 2/28/11. Examples
Light We can use different terms to describe light: Color Wavelength Frequency Light is composed of electromagnetic waves that travel through some medium. The properties of the medium determine how light
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More informationChemistry 111 Dr. Kevin Moore
Chemistry 111 Dr. Kevin Moore Black Body Radiation Heated objects emit radiation based on its temperature Higher temperatures produce higher frequencies PhotoElectric Effect Light on a clean metal surface
More informationArrangement of Electrons. Chapter 4
Arrangement of Electrons Chapter 4 Properties of Light -Light s interaction with matter helps to understand how electrons behave in atoms -Light travels through space & is a form of electromagnetic radiation
More informationElectrons in Atoms. Section 5.1 Light and Quantized Energy
Name Date Class 5 Electrons in Atoms Section 5.1 Light and Quantized Energy In your textbook, read about the wave nature of light. Use each of the terms below just once to complete the passage. amplitude
More informationRecall the Goal. What IS the structure of an atom? What are the properties of atoms?
Recall the Goal What IS the structure of an atom? What are the properties of atoms? REMEMBER: structure affects function! Important questions: Where are the electrons? What is the energy of an electron?
More informationPeriodicity and the Electronic Structure of Atoms 國防醫學院生化學科王明芳老師
Periodicity and the Electronic Structure of Atoms 國防醫學院生化學科王明芳老師 2018-10-2 1 2 Light and the Electromagnetic Spectrum Electromagnetic energy ( light ) is characterized by wavelength, frequency, and amplitude.
More informationChapter 6 Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms What is the origin of color in matter? Demo: flame tests What does this have to do with the atom? Why are atomic properties periodic? 6.1 The Wave Nature of Light
More informationLecture 11 Atomic Structure
Lecture 11 Atomic Structure Earlier in the semester, you read about the discoveries that lead to the proposal of the nuclear atom, an atom of atomic number Z, composed of a positively charged nucleus surrounded
More informationAtoms, Electrons and Light MS. MOORE CHEMISTRY
Atoms, Electrons and Light MS. MOORE CHEMISTRY Atoms Remember Rutherford??? What did he discover with his gold foil experiment. A: Atoms contain a dense nucleus where the protons and neutrons reside. ATOMS
More informationSample Exercise 6.1 Concepts of Wavelength and Frequency
Sample Exercise 6.1 Concepts of Wavelength and Frequency Two electromagnetic waves are represented in the margin. (a) Which wave has the higher frequency? (b) If one wave represents visible light and the
More informationChapter 6. Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms 6.1 The Wave Nature of Light Made up of electromagnetic radiation. Waves of electric and magnetic fields at right angles to each other. Parts of a wave Wavelength
More informationAtomic Structure 11/21/2011
Atomic Structure Topics: 7.1 Electromagnetic Radiation 7.2 Planck, Einstein, Energy, and Photons 7.3 Atomic Line Spectra and Niels Bohr 7.4 The Wave Properties of the Electron 7.5 Quantum Mechanical View
More informationTo review Rutherford s model of the atom To explore the nature of electromagnetic radiation To see how atoms emit light
Objectives To review Rutherford s model of the atom To explore the nature of electromagnetic radiation To see how atoms emit light 1 A. Rutherford s Atom.but there is a problem here!! 2 Using Rutherford
More informationIntroduction. Electromagnetic Waves. Electromagnetic Waves
Introduction Much of the information we know about electrons comes from studies of interactions of light and matter. In the early 1900 s, scientists discovered that light has properties of both a wave
More informationAtomic Structure and the Periodic Table
Atomic Structure and the Periodic Table The electronic structure of an atom determines its characteristics Studying atoms by analyzing light emissions/absorptions Spectroscopy: analysis of light emitted
More informationChapter 7. The Quantum- Mechanical Model of the Atom. Chapter 7 Lecture Lecture Presentation. Sherril Soman Grand Valley State University
Chapter 7 Lecture Lecture Presentation Chapter 7 The Quantum- Mechanical Model of the Atom Sherril Soman Grand Valley State University The Beginnings of Quantum Mechanics Until the beginning of the twentieth
More informationThe Structure of the Atom Review
The Structure of the Atom Review Atoms are composed of PROTONS + positively charged mass = 1.6726 x 10 27 kg NEUTRONS neutral mass = 1.6750 x 10 27 kg ELECTRONS negatively charged mass = 9.1096 x 10 31
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More informationCh. 5 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 5 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 5.1 Notes I. Light and Quantized Energy A. The Wave Nature of Light 1) the wave
More informationCHAPTER 4. Arrangement of Electrons in Atoms
CHAPTER 4 Arrangement of Electrons in Atoms 4.1 Part I Development of a New Atomic Model 4.1 Objectives 1. Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic
More informationPart One: Light Waves, Photons, and Bohr Theory. 2. Beyond that, nothing was known of arrangement of the electrons.
CHAPTER SEVEN: QUANTUM THEORY AND THE ATOM Part One: Light Waves, Photons, and Bohr Theory A. The Wave Nature of Light (Section 7.1) 1. Structure of atom had been established as cloud of electrons around
More informationElectromagnetic Radiation
Chapter 6: The Periodic Table and Atomic Structure Electromagnetic Radiation Atomic Spectra The Bohr Atom Quantum Mechanical Model of the Atom Wave Mechanics Quantum Numbers and Electron Orbitals Interpreting
More informationQuantum Theory of the Atom
The Wave Nature of Light Quantum Theory of the Atom Electromagnetic radiation carries energy = radiant energy some forms are visible light, x rays, and radio waves Wavelength ( λ) is the distance between
More informationDemocritus and Leucippus Matter is made up of indivisible particles Dalton - one type of atom for each element. Greek Idea
Electrons in Atoms Democritus and Leucippus Matter is made up of indivisible particles Dalton - one type of atom for each element Greek Idea Thomson s Model Discovered electrons Atoms were made of positive
More informationQuantum Theory & Electronic Structure of Atoms. It s Unreal!! Check your intuition at the door.
Quantum Theory & Electronic Structure of Atoms It s Unreal!! Check your intuition at the door. 1 Quantum Theory of the Atom Description of the atom and subatomic particles. We will focus on the electronic
More informationAP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity
AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 10-1 10-10 10-8 4 to 7x10-7 10-4 10-1 10 10 4 gamma
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE The Electromagnetic Spectrum The Wave
More informationQUANTUM THEORY & ATOMIC STRUCTURE. GENERAL CHEMISTRY by Dr. Istadi
QUANTUM THEORY & ATOMIC STRUCTURE GENERAL CHEMISTRY by Dr. Istadi 1 THE NATURE OF LIGHT Visible light is one type of electromagnetic radiation ( radiation (electromagnetic The electromagnetic radiation
More informationThe Bohr Model Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
5.1 The Development of Atomic Models Rutherford s atomic model could not explain the chemical properties of elements. Rutherford s atomic model could not explain why objects change color when heated. The
More informationElectronic Structure and the Periodic Table. Unit 6 Honors Chemistry
Electronic Structure and the Periodic Table Unit 6 Honors Chemistry Wave Theory of Light James Clerk Maxwell Electromagnetic waves a form of energy that exhibits wavelike behavior as it travels through
More informationI understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited
NCCS 1.1.2 & 1.1.3 I understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited state I will describe how an electron
More informationAtomic Structure Part II. Electrons in Atoms
Atomic Structure Part II Electrons in Atoms Radiant energy travels in the form of waves that have both electrical and magnetic properties. These electromagnetic waves can travel through empty space, as
More informationAtomic Structure Part II Electrons in Atoms
Atomic Structure Part II Electrons in Atoms Radiant energy travels in the form of waves that have both electrical and magnetic properties. These electromagnetic waves can travel through empty space, as
More informationCh. 4 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 4 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Light and Quantized Energy A. The Wave Nature of Light 1) the wave nature of
More informationThe Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol λ.
CHAPTER 7 Atomic Structure Chapter 8 Atomic Electron Configurations and Periodicity 1 The Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol
More informationChapter 4. Table of Contents. Section 1 The Development of a New Atomic Model. Section 2 The Quantum Model of the Atom
Arrangement of Electrons in Atoms Table of Contents Section 1 The Development of a New Atomic Model Section 2 The Quantum Model of the Atom Section 3 Electron Configurations Section 1 The Development of
More informationChapter 2. Atomic Structure and Periodicity
Chapter 2 Atomic Structure and Periodicity Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) (2.9) Electromagnetic radiation The nature of matter The atomic spectrum of hydrogen
More informationQuantum Theory of the Atom
Quantum Theory of the Atom The Wave Nature of Light A wave is a continuously repeating change or oscillation in matter or in a physical field. Light is also a wave. It consists of oscillations in electric
More informationGeneral Chemistry by Ebbing and Gammon, 8th Edition
Chem 1045 General Chemistry by Ebbing and Gammon, 8th Edition George W.J. Kenney, Jr Last Update: 26-Mar-2009 Chapter 7: Quantum Theory of the Atom These Notes are to SUPPLIMENT the Text, They do NOT Replace
More informationChapter 9. Blimps, Balloons, and Models for the Atom. Electrons in Atoms and the Periodic Table. Hindenburg. Properties of Elements Hydrogen Atoms
Chapter 9 Electrons in Atoms and the Periodic Table Blimps, Balloons, and Models for the Atom Hindenburg Blimps, Balloons, and Models for the Atom Properties of Elements Hydrogen Atoms Helium Atoms 1 Blimps,
More informationCHEMISTRY - ZUMDAHL 8E CH.7 - ATOMIC STRUCTURE & PERIODICITY.
!! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of
More informationWhite Light. Chapter 7 Electron Structure of the Atom
Chapter 7 Electron Structure of the Atom Electromagnetic Radiation and Energy The Bohr Model of the Hydrogen Atom The Modern Model of the Atom Periodicity of Electron Configurations Valence Electrons for
More informationQuantum Mechanics & Atomic Structure (Chapter 11)
Quantum Mechanics & Atomic Structure (Chapter 11) Quantum mechanics: Microscopic theory of light & matter at molecular scale and smaller. Atoms and radiation (light) have both wave-like and particlelike
More informationGeorgia Institute of Technology CHEM 1310 revised 10/8/09 Spring The Development of Quantum Mechanics. ν (nu) = frequency (in s -1 or hertz)
The Development of Quantum Mechanics Early physicists used the properties of electromagnetic radiation to develop fundamental ideas about the structure of the atom. A fundamental assumption for their work
More informationThe Quantum Mechanical Atom
The Quantum Mechanical Atom CHAPTER 7 Chemistry: The Molecular Nature of Matter, 6 th edition By Jesperson, Brady, & Hyslop CHAPTER 8: Quantum Mechanical Atom Learning Objectives q Light as Waves, Wavelength
More informationWAVE NATURE OF LIGHT
WAVE NATURE OF LIGHT Light is electromagnetic radiation, a type of energy composed of oscillating electric and magnetic fields. The fields oscillate perpendicular to each other. In vacuum, these waves
More informationChapter 7. Quantum Theory and the Electronic Structure of Atoms
Chapter 7 Quantum Theory and the Electronic Structure of Atoms This chapter introduces the student to quantum theory and the importance of this theory in describing electronic behavior. Upon completion
More informationA Much Closer Look at Atomic Structure
Ideas We Will Clear Up Before You Graduate: WRONG IDEAS 1. The electron always behaves as a particle. BETTER SUPPORTED BY EXPERIMENTS 1. There s a wavelength associated with very small particles like the
More information