Lecture 8 January 28, Silicon crystal surfaces
|
|
- Moses Turner
- 5 years ago
- Views:
Transcription
1 Lecture 8 January 28, 203 Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course number: Ch20a Hours: 2-3pm Monday, Wednesday, Friday William A. Goddard, III, wag@wag.caltech.edu 36 Beckman Institute, x3093 Charles and Mary Ferkel Professor of Chemistry, Materials Science, and Applied Physics, California Institute of Technology Teaching Assistants: Caitlin Scott <cescott@caltech.edu> Hai Xiao xiao@caltech.edu; Fan Liu <fliu@wag.caltech.edu> Silicon crystal surfaces Ch20a-
2 Last time 2
3 Diamond Replacing all H atoms of ethane and with methyls, leads to with a staggered conformation Continuing to replace H with methyl groups forever, leads to the diamond crystal structure, where all C are bonded tetrahedrally to four C and all bonds on adjacent C are staggered A side view is This leads to the diamond crystal structure. An expanded view is on the next slide 3
4 Infinite structure from tetrahedral bonding plus staggered bonds on adjacent centers 2 nd layer 3 st layer nd layer c st layer 2 nd layer Chair configuration st layer of cylcohexane Not shown: zero layer just like 2 nd layer but above layer 3 rd layer just like the st layer but below layer 2 4
5 The unit cell of diamond crystal An alternative view of the diamond structure is in terms of cubes of side a, that can be translated in the x, y, and z directions to fill all space. Note the zig-zag chains c-i-f-i-c and cyclohexane rings (f-i-f)-(i-f-i) There are atoms at all 8 corners (but only /8 inside the cube): (0,0,0) all 6 faces (each with ½ in the cube): (a/2,a/2,0), (a/2,0,a/2), (0,a/2,a/2) plus 4 internal to the cube: (a/4,a/4,a/4), (3a/4,3a/4,a/4), (a/4,3a/4,3a/4), (3a/4,a/4,3a/4), Thus each cube represents 8 atoms. All other atoms of the infinite crystal are obtained by translating this cube by multiples of copyright a in 20 the William x,y,z A. Goddard directions III, all rights reserved c c f i c f c i f f i c f c i f c c 5
6 4 b 2 b Diamond Structure 5 a 3 a a b 4 a 2 a 5 b 3 b c 7 Start with C and make 4 bonds to form a tetrahedron. Now bond one of these atoms, C2, to 3 new C so that the bond are staggered with respect to those of C. Continue this process. Get unique structure: diamond Note: Zig-zag chain b Chair cyclohexane ring: b -7- c 6
7 Properties of diamond crystals 7
8 Properties of group IV molecules (IUPAC group 4).526 There are 4 bonds to each atom, but each bond connects two atoms. Thus to obtain the energy per bond we take the total heat of vaporization and divide by two. Note for Si, that the average copyright 20 bond William is A. much Goddard III, different all rights reserved than for Si H 8
9 Comparisons of successive bond energies SiH n and CH n p lobe lobe p lobe lobe p p 9
10 Miller indices A 3D crystal is characterized by a unit cell with axes, a, b, c that can be translated by integer transations along a, b, c to fill all space. The corresponding points in the translated cells are all equivalent. Passing a plane through any 3 such equivalent points defines a plane denoted as (h,k,l). An equally spaced set of planes parallel to (h,k,l) pass through all equivalent points. Put the origin on a point in one of these parallel planes. The closest one will intersect the unit vectors at a/h, b/k, and c/l. c These are called Miller indices c/l b/k a a/h b 0
11 Examples of special planes c c/l a a/h To denote all equivalent planes we use {h,k,l} so that indicates negative b/k b {,0,0} for cubic includes the 3 cases in the first row) A number with a bar From Wikipedia
12 Crystallographic directions A lattice vector can be written as Rmnp = m a + n b + p c where m,n,p are integers. This is denoted as [m,n,p] The set of equivalent vectors is denoed as <m,n,p> Examples are shown here. From Wikipedia 2
13 The Si Crystal viewed from the [00] direction [00] [00] [0] [00] [00 [00] (00) Surface st Layer RED 2 nd Layer GREEN 3 rd Layer ORANGE 4 th Layer WHITE [,-,0] not show bonds 3 to 5 th layer
14 The Si Crystal (00) surface, unreconstructed Projection of bulk cubic cell Surface unit cell P(x) Surface zig-zag row Every red atom was bonded to two Si that are now removed, thus two dangling bond orbitals (like A state) sticking out of plane (00) VIEW st Layer RED 2 nd Layer GREEN 3 rd Layer ORANGE 4 th Layer WHITE 4
15 Si(00) surface (unreconstructed) viewed (nearly) along the [0] direction Each surface atom has two dangling bond orbitals pointing to left and right, along [,-,0] direction 5
16 The (00) Surface Reconstruction viewed (nearly) along the [0] direction Spin pair dangling bond orbitals of adjacent atoms in [,-,0] direction (originally 2 nd near neighbors Get one strong s bond but leave two dangling bond orbitals on adjacent now bonded atoms (form weak p bond in plane) 6
17 Si(00) surface reconstructed (side view) Surface atoms now bond to form dimers (move from 3.8 to 2.4A) Get row of dimes with doubled surface unit cell One strong s bond, plus weak p bond in plane orginal cell New cell Surface length length bond Lateral 7.6A 3.8A 2.4A displacements 0.7A 0.7A 7
18 Si(00) surface reconstructed (top view) New unit cell reconstructed surface P(2x) Rows of dimer pairs are parallel original unit cell unreconstructed surface P(x) 8
19 Get 2x2 unit cell but atom at center is equivalent to atom at corner, therform c(2x2) 9
20 Two simple patterns for (00) Surface Reconstruction Dimer rows alternate C(2x2), high energy Dimer rows parallel P(2x), low energy 20
21 P(2x) more stable than c(2x2) by ~ kcal/mol The Sisurf-Si2nd-Sisurf bond for c(2x2) opens up to 20º because the Sisurf move opposite directions 20º 0º 20º 0º For P(2x) the Sisurf move the same directions and Sisurf-Si2nd-Sisurf bond remains at 0º 2
22 Construct () surface using cubic unit cell Start at diagonal atom #0 Go straight down to atom # Atom # bonded to 3 atoms #2 Each #2 is bonded to 3 atoms # in top layer. Get hexagonal double layer Each #2 is bonded straight down to an atom#3 Each atom #3 is bonded to 3 atom# c
23 Si() surface (alternate construction) Start with red atom on top, bond to 3 green atoms in 2 nd layer Each green atom is bonded to 2 other st layer atoms plus a 3 rd atom straight down (not shown) The 3 rd layer atoms bond to 3 4 th layer atoms in orange (now white) Surface unit cell P(x) 23
24 Reconstruction of Si() surface Each surface atom has a single dangling bond electron, might guess that there would be some pairing of this with an adjacent atom to form a 2x unit cell. Indeed freshly cleaved Si() at low temperature does show 2x Surface unit cell P(x) 24
25 LEED experiments (Schlier and Farnsworth, 959) observed 7th Order Spots 7x7 unit cell (49 x cells) From 959 to 98 many models proposed to fit various experiments or calculations. Binnig et al., 98 did first STM image of Si (7x7) and saw 2 bright spots in 7x7 cell, showed that every previous model was incorrect Takayanagi et al., 985, proposed the DAS Model that explained the experiments 25
26 two 7x7 cells What kind of interactions can go over a 7x7 region, with cell size 26.6 by 26.6 A? 26
27 New material 27
28 Origin of complex reconstruction of Si() In 49 surface unit cells have 49 dangling bonds. Since cohesive energy of Si crystal is 08 kcal/mol expect average bond energy must be 08/2 = 54 kcal/mol (each atom has 4 bonds, but double count the bonds) (H3Si-SiH3 bond energy is 74 kcal/mol) Thus each dangling bond represents ~ 27 kcal/mol of surface energy =. ev per surface atom Calculated value =.224 ev snap and.200 ev relaxed. 28
29 Consider bonding an atom on top of 3 dangling bonds T 4 H 3 T 4 T 4 H 3 T 4 Get 3x2 unit cell By adding a cap of one adatom Si per 3 top layer Si, can tie off all original dangling bonds. Thus
30 Consider bonding an atom on top of 3 dangling bonds Two ways to do this. T 4 and H 3 T 4 (observed) H 3 (not observed) Stabilize by 0. ev per site Destabilize by 0.5 ev per site 30
31 T4 versus H3 site bonding to dangling bonds Energy increases by 0.5 ev per original surface atom or 0.45 ev per new adatom Angle between bond A and bond B is 80º bad overlap orthog Energy decreases by 0.0 ev per original surface atom or 0.30 ev per new adatom Angle between bond A and bond B is 00º ok overlap no orthog 3
32 0 2 H3 reconstruction 0 Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds. Surface energy increases by 0.3 ev Because 0--2 is linear Unit cell
33 H3 reconstruction, 3 x Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds. Surface energy increases by 0.3 ev
34 T4 reconstruction 3 x 3 2 Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds. Surface energy decreases by 0.0 ev Because 0--2 ~ 00º Unit cell 34
35 T4 reconstruction 2x2 2 Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds, leave dangling bond orbital Surface energy decreases by 0.08 ev Per 2x2 cell Unit cell 35
36 36
37 The () 7x7 DAS Surface 37
38 The () 7x7 DAS Surface Layers (purple, brown and blue atoms have one dangling bond) Adatoms on Top layer These adatoms protrude from the surface so that they show up prominently in STM 38
39 The () 7x7 DAS Surface Layers (purple, brown and blue atoms have one dangling bond) st 2 nd red atoms, all bonded to st layer 3 rd 4 th First unreconstructed layer 39
40 The () 7x7 DAS Surface 2-membered ring at corner of cell 40
41 The () 7x7 DAS Surface Side view 4
42 The () 7x7 DAS Surface Cornerhole 42
43 Si() 7x7 43
44 The () 7x7 DAS Layer Positions REF REF REF 47
45 The () 3x3 DAS Surface Unit Cell Side view Top view 2-membered rings 48
46 The () 5x5 DAS Surface Unit Cell Side view 49
47 The () 5x5 DAS Surface Unit Cell Top view 2- and 8-membered rings 50
48 The () 9x9 DAS Surface Unit Cell Side view 5
49 The () 9x9 DAS Surface Unit Cell Top view 2- and 8-membered rings 52
50 Energy, ev/x Cell DAS Surface Energies (PBE DFT) Regression Ab Initio DAS Cell Size Unreconstructed relaxed surface:.200 ev/x cell Infinite DAS model:.07 ev/x cell 53
51 DAS Reconstruction Driving Force 49 unpaired electrons (/2 Si-Si bond) per 7x7 ev = 58.8 ev/cell DAS 7x7 Surface energy = 5.2 ev/cell (9 unpaired electrons) Energy reduction due to reconstruction = 7.6 ev Difference is due to strain Bond length range = Å (equilibrium 2.35 Å) Bond angle range = 9 7º (Equilibrium 09.4 ) 54
52 Energy, ev/x Cell DAS Surface Energy Contributions (DAS Model Cell Size) - x T4 8R 2R F D TOTAL 55
53 Energy, ev/6x6 Cell DAS Surface Energies: Sequential Size Change Model SSC Irregular-odd and even SSC regular-odd -20 SSC Cell Size Real-time STM by Shimada & Tochihara,
54 Energy, ev/x Cell DAS Surface Energies: Origin of a finite cell size.4.3 SSC Irregular-odd and even SSC regular-odd DFT Cell Size 57
55 The (0) plane (outlined in green, layer ) [00] c [-,,0] [00] [00] [0] 58
56 Si(0) surface (top view) Cut through cubic unit cell surface unit cell P(x) Surface atoms red 59
57 Si(0) surface (viewed nearly along [-,,0] direction) One dangling bond electron per surface atom Surface atoms red bulk atoms orange [,,0] [00] 60
58 Reconstruction of (0) surface, surface atoms only side view (along [-,,0]) Showing just 2 dangling bond orbitals 54.7º 54.7º Top view (from [-,-,0]) [00] [,,0] [-,,0] [00] 6
59 Reconstruction of (0) surface, surface atoms only We have a chain of dangling bond orbitals along the [-,,0] direction, each tilted by 35.3º from the [0] (vertical) axis They will want to tilt toward the vertical axis, reducing their angle from 35.3º). This leads to moving the surface atoms toward the bulk. There could be 2 by 2 pairing to double the surface unit cell in the [-,,0] direction [0] side view (along [-,,0]) Showing just 2 dangling bond orbitals 54.7º 54.7º 54.7º [00] 62
60 The zincblende or sphalerite structure Replacing each C atom of the diamond structure alternately with Ga and As so that each Ga is bonded to four As and each As is bonded to four Ga leads to the zincblende or sphalerite structure (actually zincblende is the cubic form of ZnS and the mineral sphalerite is cubic ZnS with some Fe) As at corners: (0,0,0) As at face centers: (a/2,a/2,0), (a/2,0,a/2), (0,a/2,a/2) Ga 4 internal sites: (a/4,a/4,a/4), (3a/4,3a/4,a/4), (a/4,3a/4,3a/4), (3a/4,a/4,3a/4), Thus each cube has 4 As and 4 Ga. 63
61 Bonding in GaAs Making a covalent bond between to each atoms, one might have expected tetrahedral As to make 3 bonds with a left over lone pair pointing away from the 3 bonds, while Ga might be expected to make 3 covalent bonds, with an empty sp 3 orbital point away from the 3 bonds, as indicated here, where the 3 covalent bonds are shown with lines, and the donor acceptor (DA) or Lewis acid- Lewis base bond as an As lone pair coordinated with and empty orbital on Ga Of course the four bonds to each atom will adjust to be equivalent, but we can still think of the bond as an average of ¾ covalent and ¼ DA 64
62 Other compounds Similar zincblende or sphalerite compounds can be formed with Ga replaced by B, Al,In and /or As replaced by N, P, Sb, or Bi. They are call III-V compounds from the older names of the columns of the periodic table (new UIPAC name 3-5 compounds). In addition a hexagonal crystal, called Wurtzite, also with tetrahedral bonding (but with some eclipsed bonds) is exhibited by most of these compounds. In addition there are a variety of similar II-VI systems, ZnS, ZnSe, CdTe, HgTe, etc 65
63 Last time 66
64 T4 versus H3 site bonding to dangling bonds Energy increases by 0.5 ev per original surface atom or 0.45 ev per new adatom Angle between bond A and bond B is 80º bad overlap orthog Energy decreases by 0.0 ev per original surface atom or 0.30 ev per new adatom Angle between bond A and bond B is 00º ok overlap no orthog 67
65 0 2 H3 reconstruction 0 Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds. Surface energy increases by 0.3 ev Because 0--2 is linear Unit cell
66 H3 reconstruction, 3 x Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds. Surface energy increases by 0.3 ev
67 T4 reconstruction 3 x 3 2 Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds. Surface energy decreases by 0.0 ev Because 0--2 ~ 00º Unit cell 70
68 T4 reconstruction 2x2 2 Top layer labeled 2 nd layer green Addon layer 0, blue Need just /3 Monolayer to tie up bonds, leave dangling bond orbital Surface energy decreases by 0.08 ev Per 2x2 cell Unit cell 7
69 The () 7x7 DAS Surface Layers (purple, brown and blue atoms have one dangling bond) Adatoms on Top layer These adatoms protrude from the surface so that they show up prominently in STM 72
70 The () 7x7 DAS Surface Layers (purple, brown and blue atoms have one dangling bond) st 2 nd red atoms, all bonded to st layer 3 rd 4 th First unreconstructed layer 73
71 The () 7x7 DAS Surface 2-membered ring at corner of cell 74
72 The () 7x7 DAS Surface Cornerhole 75
73 Si() 7x7 76
74 The (0) plane (outlined in green, layer ) [00] c [-,,0] [00] [00] [0] 80
75 Si(0) surface (viewed nearly along [-,,0] direction) One dangling bond electron per surface atom Surface atoms red bulk atoms orange [,,0] [00] 8
76 Reconstruction of (0) surface, surface atoms only We have a chain of dangling bond orbitals along the [-,,0] direction, each tilted by 35.3º from the [0] (vertical) axis They will want to tilt toward the vertical axis, reducing their angle from 35.3º). This leads to moving the surface atoms toward the bulk. There could be 2 by 2 pairing to double the surface unit cell in the [-,,0] direction [0] side view (along [-,,0]) Showing just 2 dangling bond orbitals 54.7º 54.7º 54.7º [00] 82
77 The zincblende or sphalerite structure Replacing each C atom of the diamond structure alternately with Ga and As so that each Ga is bonded to four As and each As is bonded to four Ga leads to the zincblende or sphalerite structure (actually zincblende is the cubic form of ZnS and the mineral sphalerite is cubic ZnS with some Fe) As at corners: (0,0,0) As at face centers: (a/2,a/2,0), (a/2,0,a/2), (0,a/2,a/2) Ga 4 internal sites: (a/4,a/4,a/4), (3a/4,3a/4,a/4), (a/4,3a/4,3a/4), (3a/4,a/4,3a/4), Thus each cube has 4 As and 4 Ga. 83
78 Bonding in GaAs Making a covalent bond between to each atoms, one might have expected tetrahedral As to make 3 bonds with a left over lone pair pointing away from the 3 bonds, while Ga might be expected to make 3 covalent bonds, with an empty sp 3 orbital point away from the 3 bonds, as indicated here, where the 3 covalent bonds are shown with lines, and the donor acceptor (DA) or Lewis acid- Lewis base bond as an As lone pair coordinated with and empty orbital on Ga Of course the four bonds to each atom will adjust to be equivalent, but we can still think of the bond as an average of ¾ covalent and ¼ DA 84
79 Other compounds Similar zincblende or sphalerite compounds can be formed with Ga replaced by B, Al,In and /or As replaced by N, P, Sb, or Bi. They are call III-V compounds from the older names of the columns of the periodic table (new UIPAC name 3-5 compounds). In addition a hexagonal crystal, called Wurtzite, also with tetrahedral bonding (but with some eclipsed bonds) is exhibited by most of these compounds. In addition there are a variety of similar II-VI systems, ZnS, ZnSe, CdTe, HgTe, etc 85
80 New material 86
81 [00] 2 The (0) plane (outlined in green, layer ) [00] c [0] [-,,0] [00] Cut through cubic unit cell surface unit cell P(x) As atoms top layer Ga atoms top layer [00] [-,,0] 87
82 Reconstruction of (0) surface, side view along [-,,0] Si has dangling bond electron at each surface atom 54.7º 54.7º Surface As has 3 covalent bonds to Ga, with 2 e in 3s lone pair, relaxes upward until average bond angle is 95º Surface Ga has 3 covalent bonds leaving 0 e in 4th orbital, relaxes downward until average bond angle is 9º. GaAs angle 0º 26º 54.7º Ga As [0] Si (0) GaAs (0) [00] 88
83 Top view (from [-,-,0]) Reconstruction of GaAs(0) surface As has 3 covalent bonds, leaving 2 electrons in 3s lone pair, Ga has 3 covalent bonds leaving 0 eletrons in 4 th orbital Ga As 54.7º 54.7º [00] [,,0] [-,,0] [00] side view (along [-,,0]) 89
84 Reconstruction of (0) GaAs 90
85 III-V reconstruction 9
86 92
87 Reconstruction of GaAs(0) surface, discussion We consider that bulk GaAs has an average of 3 covalent bonds and one donor acceptor (DA) bond. But at the surface can only make 3 bonds so the weaker DA bond is the one broken to form the surface. The result is that GaAs cleaves very easily compared to Si. No covalent bonds to break. As has 3 covalent bonds, leaving 2 electrons in 3s lone pair. AsH3 has average bond angle of 92º. At the GaAs surface As relaxes upward until has average bond angle of 95º Ga has 3 covalent bonds leaving 0 eletrons in 4th orbital. GaH3 has average bond angle of 20º. At the GaAs surface Ga relaxes downward until has average bond angle of 9º. This changes the surface Ga-As bond from 0º (parallel to surface to 26º. Observed in LEED experiments and QM calculations 95
88 Analysis of charges Bulk structure: each As has 3 covalent bonds and one Donoraccepter bond(lewis base Lewis acid). This requires 3+2=5 electrons from As and 3+0=3 electrons from Ga. We consider that each bulk GaAs bond has 5/4 e from As and ¾ e form Ga. Each surface As has 5/4+++2 = 5.25e for a net charge of each surface Ga has ¾+++0= 2.75 e for a net charge of Thus considering both surface Ga and As, the (0) is neutral 5.25e 2.75e Net Q = Ga As Ga As Ga As 3/4 5/4 3/4 5/4 3/4 5/4 5/4 3/4 5/4 3/4 5/4 3/4 5/4 3/4 5/4 3/4 5/4 3/4 a g a g a g 3/4 5/4 3/4 5/4 3/4 5/4 3/4 5/4 3/4 5/4 3/4 96
89 The GaAs (00) surface, unreconstructed Every red surface atom is As bonded to two green 2 nd layer Ga atoms, but the other two bonds were to two Ga that are now removed. This leaves three non bonding electrons to distribute among the two dangling bond orbitals sticking out of plane (like AsH 2 ) st Layer RED 2 nd Layer GREEN 3 rd Layer ORANGE 4 th Layer WHITE 97
90 GaAs(00) surface reconstructed (side view) For the perfect surface, As in top layer, Ga in 2 nd layer, As in 3 rd layer, Ga in 4 th layer etc. For the unreconstructed surface each As has two bonds and hence three electrons in two nonbonding orbitals. Expect As atoms to dimerize to form a 3 rd bond leaving 2 electrons in nonbonding orbitals. Surface As-As bonds As As Ga As Ga Ga As 98
91 Charges for 2x GaAs(00) 2 nd layer ga has 3 e 2e As-ga bond 2e As LP st layer As has 5.5 e 3/4 3/ /4 5/4 3/4 3/4 3/4 5/4 5/ /4 3/4 5/4 3/4 5/4 3/4 5/4 2e As-As bond 3/4 3/4 3/4 3/4 3/4 3/4 Top layer, As 2 nd layer, ga 3 rd layer, as Each surface As has extra 0.5 e dimer has extra e Not stable 99
92 Now consider a missing row of As for GaAs(00) Top layer, As ga empty LP st layer As has 5.5 e 3/4 3/4 3/4 5/4 3/ /4 2 nd layer ga has 2.25e 3/4 5/4 3/4 3/4 3/4 3/4 3/4 3/4 0 2 nd layer, ga 3 rd layer, as Each 2 nd layer ga next to missing As is deficient by 0.75e extra 0.5 e 4 ga are missing 3e 00
93 Consider missing As row out of =0 net charge Extra e missing 3e Extra e Thus based on electron counting expect simplest surface reconstruction to be 4x2. This is observed Extra e Extra e missing 3e 0
94 Different views of GaAs(00)4x2 reconstruction -.0e Previous page, 3 As dimer rows then one missing +.5e Two missing As row plus missing Ga row Exposes 3 rd row As Agrees with experiment Hashizume et al Phys Rev B 5, 4200 (995) 02
95 summary Postulate of surface electro-neutrality Terminating the bulk charges onto the surface layer and considering the lone pairs and broken bonds on the surface should lead to: the atomic valence configuration on each surface atom. For example As with 3 covalent bonds and a lone pair and Ga with 3 covalent bonds and an empty fourth orbital A neutral surface This leads to the permissible surface reconstructions 03
96 Intrinsic semiconductors
97 Excitation energy 05
98 To be added band states 06
99 To be added band states 07
100 Semiconducting properties 08
101 Semiconducting properties 09
102 0
103
104 2
105 3
106 4
107 5
108 To be added band states IP(P)=4.05 ev ev Remove e from P, add to conduction band = = ev Thus P leads to donor state just 0.045eV below LUMO or CBM 6
109 7
110 8
111 To be added band states EA(Al)=5.033 ev ev Add e to Al, from valence band = = ev Al leads to acceptor state just 0.067eV above HOMO or VBM 9
112 20
113 Stopped Feb. 5 2
114 22
115 23
Lecture February 13-15, Silicon crystal surfaces
Lecture 18-19 February 13-15, 2012 Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course number: Ch120a
More informationCh125a-1. copyright 2015 William A. Goddard III, all rights reserved
Lecture, October 28, 205: Si, Ga crystal surfaces Ch 25a: Elements of Quantum Chemistry with Applications to Chemical Bonding and Properties of Molecules and Solids Ch 20a:Nature of the Chemical bond Room
More informationLecture 8 January 24, 2013 GaAs crystal surfaces, n-p dopants Si
Lecture 8 January 24, 2013 Ga crystal surfaces, n-p dopants Si Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinornic chemistry, and
More informationLecture 9 January 26, 2011 Si, GaAs surfaces
Lecture 9 January 26, 20 Si, GaAs surfaces Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy William A.
More informationLecture 6 January 18, 2012 CC Bonds diamond, ΔHf, Group additivity
Lecture 6 January 18, 2012 CC Bonds diamond, ΔHf, Group additivity Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry,
More informationLecture 7,8 January 24, 2011 CC Bonds
Lecture 7,8 January 24, 2011 CC Bonds Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy William A. Goddard,
More informationLecture 16, February 25, 2015 Metallic bonding
Lecture 16, February 25, 2015 Metallic bonding Elements of Quantum Chemistry with Applications to Chemical Bonding and Properties of Molecules and Solids Course number: Ch125a; Room 115 BI Hours: 11-11:50am
More informationLecture 11 January 30, Transition metals, Pd and Pt
Lecture 11 January 30, 2011 Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course number: Ch120a Hours:
More informationLecture 16 February 20 Transition metals, Pd and Pt
Lecture 16 February 20 Transition metals, Pd and Pt Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course
More informationLecture 15 February 15, 2013 Transition metals
Lecture 15 February 15, 2013 Transition metals Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course
More informationLecture 13 February 1, 2011 Pd and Pt, MH + bonding, metathesis
Lecture 13 February 1, 2011 Pd and Pt, MH + bonding, metathesis Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and
More informationLecture 9-10 January 25-27, 2012 Rules for Chem. React. - Woodward-Hoffmann
Lecture 9-10 January 25-27, 2012 Rules for Chem. React. - Woodward-Hoffmann Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic
More informationLecture February 8-10, NiCHx
Lecture 16-17 February 8-10, 2011 Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course number: Ch120a
More informationNature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
Lecture 13, October 31, 2016 Transition metals, Pd and Pt Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
More informationDensity Functional Theory Study of the Geometry, Energetics, and Reconstruction Process of Si(111) Surfaces
12404 Langmuir 2005, 21, 12404-12414 Density Functional Theory Study of the Geometry, Energetics, and Reconstruction Process of Si(111) Surfaces Santiago D. Solares, Siddharth Dasgupta,, Peter A. Schultz,
More informationNature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
Lecture 12, October 21, 2016 Transition metals Heme-Fe Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
More informationLecture 18, March 2, 2015 graphene, bucky balls, bucky tubes
Lecture 18, March 2, 2015 graphene, bucky balls, bucky tubes Elements of Quantum Chemistry with Applications to Chemical Bonding and Properties of Molecules and Solids Course number: Ch125a; Room 115 BI
More informationNature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
Lecture 22, November 16, 2016 Graphite, graphene, bucky balls, bucky tubes Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry,
More informationEnergetics and Reconstruction Process of Si(111) Surfaces
Density Functional Theory Study of the Geometry, Energetics and Reconstruction Process of Si(111) Surfaces Santiago D. Solares a, Siddharth Dasgupta a,b, Peter A. Schultz c, Yong-Hoon Kim,a,d, Charles
More informationChapter 10 Chemical Bonding II
Chapter 10 Chemical Bonding II Valence Bond Theory Valence Bond Theory: A quantum mechanical model which shows how electron pairs are shared in a covalent bond. Bond forms between two atoms when the following
More informationCarbon and Its Compounds
Chapter 1 Carbon and Its Compounds Copyright 2018 by Nelson Education Limited 1 1.2 Organic Molecules from the Inside Out I: The Modelling of Atoms Copyright 2018 by Nelson Education Limited 2 s orbitals:
More informationCHAPTER TEN MOLECULAR GEOMETRY MOLECULAR GEOMETRY V S E P R CHEMICAL BONDING II: MOLECULAR GEOMETRY AND HYBRIDIZATION OF ATOMIC ORBITALS
CHAPTER TEN CHEMICAL BONDING II: AND HYBRIDIZATION O ATOMIC ORBITALS V S E P R VSEPR Theory In VSEPR theory, multiple bonds behave like a single electron pair Valence shell electron pair repulsion (VSEPR)
More informationLecture 17 February 14, 2013 MH + bonding, metathesis
Lecture 17 February 14, 2013 MH + bonding, metathesis Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
More informationLecture 9 January 30, Ionic bonding and crystals
Lecture 9 January 30, 2013 Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course number: Ch120a Hours:
More informationChemical bonds. In some minerals, other (less important) bond types include:
Chemical bonds Chemical bond: force of attraction between two or more atoms/ions Types of bonds in crystals: Ionic bond: electrostatic attraction between two oppositely charged ions. This type of bond
More informationLecture 14 February 3, 2014 Rules for Chem. React. - Woodward-Hoffmann
Lecture 14 February 3, 2014 Rules for Chem. React. - Woodward-Hoffmann Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry,
More informationELEMENTARY BAND THEORY
ELEMENTARY BAND THEORY PHYSICIST Solid state band Valence band, VB Conduction band, CB Fermi energy, E F Bloch orbital, delocalized n-doping p-doping Band gap, E g Direct band gap Indirect band gap Phonon
More informationEECS143 Microfabrication Technology
EECS143 Microfabrication Technology Professor Ali Javey Introduction to Materials Lecture 1 Evolution of Devices Yesterday s Transistor (1947) Today s Transistor (2006) Why Semiconductors? Conductors e.g
More informationProperties of Individual Nanoparticles
TIGP Introduction technology (I) October 15, 2007 Properties of Individual Nanoparticles Clusters 1. Very small -- difficult to image individual nanoparticles. 2. New physical and/or chemical properties
More informationMolecular Orbital Theory This means that the coefficients in the MO will not be the same!
Diatomic molecules: Heteronuclear molecules In heteronuclear diatomic molecules, the relative contribution of atomic orbitals to each MO is not equal. Some MO s will have more contribution from AO s on
More informationLecture 2. Semiconductor Physics. Sunday 4/10/2015 Semiconductor Physics 1-1
Lecture 2 Semiconductor Physics Sunday 4/10/2015 Semiconductor Physics 1-1 Outline Intrinsic bond model: electrons and holes Charge carrier generation and recombination Intrinsic semiconductor Doping:
More informationOrganic Chemistry 1 Lecture 5
CEM 232 Organic Chemistry I Illinois at Chicago Organic Chemistry 1 Lecture 5 Instructor: Prof. Duncan Wardrop Time/Day: T & R, 12:30-1:45 p.m. January 26, 2010 1 Self Test Question Which of the following
More informationThe Solid State. Phase diagrams Crystals and symmetry Unit cells and packing Types of solid
The Solid State Phase diagrams Crystals and symmetry Unit cells and packing Types of solid Learning objectives Apply phase diagrams to prediction of phase behaviour Describe distinguishing features of
More informationMTLE-6120: Advanced Electronic Properties of Materials. Intrinsic and extrinsic semiconductors. Reading: Kasap:
MTLE-6120: Advanced Electronic Properties of Materials 1 Intrinsic and extrinsic semiconductors Reading: Kasap: 5.1-5.6 Band structure and conduction 2 Metals: partially filled band(s) i.e. bands cross
More informationCh. 2: Energy Bands And Charge Carriers In Semiconductors
Ch. 2: Energy Bands And Charge Carriers In Semiconductors Discrete energy levels arise from balance of attraction force between electrons and nucleus and repulsion force between electrons each electron
More informationExperiment 21 Lewis structures and VSEPR Theory
Experiment 21 Lewis structures and VSEPR Theory Introduction 1. Lewis Structures and Formal Charge LG.N. Lewis, at the University of California at Berkeley devised a simple way to understand the nature
More informationSemiconductor Device Physics
1 Semiconductor Device Physics Lecture 1 http://zitompul.wordpress.com 2 0 1 3 2 Semiconductor Device Physics Textbook: Semiconductor Device Fundamentals, Robert F. Pierret, International Edition, Addison
More informationAtoms & Their Interactions
Lecture 2 Atoms & Their Interactions Si: the heart of electronic materials Intel, 300mm Si wafer, 200 μm thick and 48-core CPU ( cloud computing on a chip ) Twin Creeks Technologies, San Jose, Si wafer,
More informationChapter 10. Structure Determines Properties! Molecular Geometry. Chemical Bonding II
Chapter 10 Chemical Bonding II Structure Determines Properties! Properties of molecular substances depend on the structure of the molecule The structure includes many factors, including: the skeletal arrangement
More informationBe H. Delocalized Bonding. Localized Bonding. σ 2. σ 1. Two (sp-1s) Be-H σ bonds. The two σ bonding MO s in BeH 2. MO diagram for BeH 2
The Delocalized Approach to Bonding: The localized models for bonding we have examined (Lewis and VBT) assume that all electrons are restricted to specific bonds between atoms or in lone pairs. In contrast,
More informationCHAPTER 4. Crystal Structure
CHAPTER 4 Crystal Structure We can assume minerals to be made of orderly packing of atoms or rather ions or molecules. Many mineral properties like symmetry, density etc are dependent on how the atoms
More informationCHEMISTRY. Chapter 8 ADVANCED THEORIES OF COVALENT BONDING Kevin Kolack, Ph.D. The Cooper Union HW problems: 6, 7, 12, 21, 27, 29, 41, 47, 49
CHEMISTRY Chapter 8 ADVANCED THEORIES OF COVALENT BONDING Kevin Kolack, Ph.D. The Cooper Union HW problems: 6, 7, 12, 21, 27, 29, 41, 47, 49 2 CH. 8 OUTLINE 8.1 Valence Bond Theory 8.2 Hybrid Atomic Orbitals
More informationCHEM Lecture 4
CEM 494 Special Topics in Chemistry Illinois at Chicago CEM 494 - Prof. Duncan Wardrop October 1, 2012 Course Website http://www.chem.uic.edu/chem494 Syllabus Course Policies Other handouts Announcements
More informationSemiconductor physics I. The Crystal Structure of Solids
Lecture 3 Semiconductor physics I The Crystal Structure of Solids 1 Semiconductor materials Types of solids Space lattices Atomic Bonding Imperfection and doping in SOLIDS 2 Semiconductor Semiconductors
More informationGa and P Atoms to Covalent Solid GaP
Ga and P Atoms to Covalent Solid GaP Band Gaps in Binary Group III-V Semiconductors Mixed Semiconductors Affect of replacing some of the As with P in GaAs Band Gap (ev) (nm) GaAs 1.35 919 (IR) GaP 2.24
More informationWe have arrived to the question: how do molecular bonds determine the band gap? We have discussed that the silicon atom has four outer electrons.
ET3034Tux - 2.2.2 - Band Gap 2 - Electrons in Molecular Bonds We have arrived to the question: how do molecular bonds determine the band gap? We have discussed that the silicon atom has four outer electrons.
More informationScanning Tunneling Microscopy. how does STM work? the quantum mechanical picture example of images how can we understand what we see?
Scanning Tunneling Microscopy how does STM work? the quantum mechanical picture example of images how can we understand what we see? Observation of adatom diffusion with a field ion microscope Scanning
More informationLecture Presentation. Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory
Lecture Presentation Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory Predicting Molecular Geometry 1. Draw the Lewis structure. 2. Determine the number
More informationCLASS 1 & 2 REVISION ON SEMICONDUCTOR PHYSICS. Reference: Electronic Devices by Floyd
CLASS 1 & 2 REVISION ON SEMICONDUCTOR PHYSICS Reference: Electronic Devices by Floyd 1 ELECTRONIC DEVICES Diodes, transistors and integrated circuits (IC) are typical devices in electronic circuits. All
More informationLecture 3b. Bonding Model and Dopants. Reading: (Cont d) Notes and Anderson 2 sections
Lecture 3b Bonding Model and Dopants Reading: (Cont d) Notes and Anderson 2 sections 2.3-2.7 The need for more control over carrier concentration Without help the total number of carriers (electrons and
More informationLecture 6: September 7, 2018
CM 223 Organic Chemistry I Prof. Chad Landrie Lecture 6: September 7, 2018 Ch. 4: Nomenclature of Cylcoalkanes and their Physical and Chemical Properties (4.1-4.3) Conformational Isomers of Cycloalkanes
More informationCHAPTER 2: ENERGY BANDS & CARRIER CONCENTRATION IN THERMAL EQUILIBRIUM. M.N.A. Halif & S.N. Sabki
CHAPTER 2: ENERGY BANDS & CARRIER CONCENTRATION IN THERMAL EQUILIBRIUM OUTLINE 2.1 INTRODUCTION: 2.1.1 Semiconductor Materials 2.1.2 Basic Crystal Structure 2.1.3 Basic Crystal Growth technique 2.1.4 Valence
More informationHelpful Hints Lewis Structures Octet Rule For Lewis structures of covalent compounds least electronegative
Helpful Hints Lewis Structures Octet Rule Lewis structures are a basic representation of how atoms are arranged in compounds based on bond formation by the valence electrons. A Lewis dot symbol of an atom
More informationBulk Structures of Crystals
Bulk Structures of Crystals 7 crystal systems can be further subdivided into 32 crystal classes... see Simon Garrett, "Introduction to Surface Analysis CEM924": http://www.cem.msu.edu/~cem924sg/lecturenotes.html
More informationAlicyclic Hydrocarbons can be classified into: Cycloalkanes Cycloalkenes Cycloalkynes
Cycloalkanes Open-chain The carbon atoms are attached to one another to form chains Ex: CH 3 -CH 2 -CH 2 -CH 3 n-butane Cyclic compounds the carbon atoms are arranged to form rings called: cyclic compounds,
More informationCrystal Properties. MS415 Lec. 2. High performance, high current. ZnO. GaN
Crystal Properties Crystal Lattices: Periodic arrangement of atoms Repeated unit cells (solid-state) Stuffing atoms into unit cells Determine mechanical & electrical properties High performance, high current
More informationBasic cell design. Si cell
Basic cell design Si cell 1 Concepts needed to describe photovoltaic device 1. energy bands in semiconductors: from bonds to bands 2. free carriers: holes and electrons, doping 3. electron and hole current:
More informationSTRUCTURAL AND MECHANICAL PROPERTIES OF AMORPHOUS SILICON: AB-INITIO AND CLASSICAL MOLECULAR DYNAMICS STUDY
STRUCTURAL AND MECHANICAL PROPERTIES OF AMORPHOUS SILICON: AB-INITIO AND CLASSICAL MOLECULAR DYNAMICS STUDY S. Hara, T. Kumagai, S. Izumi and S. Sakai Department of mechanical engineering, University of
More informationEE143 Fall 2016 Microfabrication Technologies. Evolution of Devices
EE143 Fall 2016 Microfabrication Technologies Prof. Ming C. Wu wu@eecs.berkeley.edu 511 Sutardja Dai Hall (SDH) 1-1 Evolution of Devices Yesterday s Transistor (1947) Today s Transistor (2006) 1-2 1 Why
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationIntroduction to Semiconductor Physics. Prof.P. Ravindran, Department of Physics, Central University of Tamil Nadu, India
Introduction to Semiconductor Physics 1 Prof.P. Ravindran, Department of Physics, Central University of Tamil Nadu, India http://folk.uio.no/ravi/cmp2013 Review of Semiconductor Physics Semiconductor fundamentals
More informationC PM RESURRECTION
Announcements Final Exam TIME: October 8, 7:30-9:30AM VENUE: CTC 105 65-Multiple Choice Questions 3 Questions Each Chapter 2-5 7 Questions Each Chapter 6-8 30 Questions From Chapter 9-11 Saturday Review
More informationVSEPR Theory. Shapes of Molecules. Molecular Structure or Molecular Geometry
VSEPR Theory VSEPR Theory Shapes of Molecules Molecular Structure or Molecular Geometry The 3-dimensional arrangement of the atoms that make-up a molecule. Determines several properties of a substance,
More information1 Review of semiconductor materials and physics
Part One Devices 1 Review of semiconductor materials and physics 1.1 Executive summary Semiconductor devices are fabricated using specific materials that offer the desired physical properties. There are
More informationCHM1321 Stereochemistry and Molecular Models Assignment. Introduction
CM1321 Stereochemistry and Molecular Models Assignment Note: A significant amount of background information is provided in the following sections. More detail is found in the Mechanistic Patterns textbook
More informationThe wavefunction that describes a bonding pair of electrons:
4.2. Molecular Properties from VB Theory a) Bonding and Bond distances The wavefunction that describes a bonding pair of electrons: Ψ b = a(h 1 ) + b(h 2 ) where h 1 and h 2 are HAOs on adjacent atoms
More informationLecture B2 VSEPR Theory
Lecture B2 VSEPR Theory Covalent Bond Theories 1. VSEPR (valence shell electron pair repulsion model). A set of empirical rules for predicting a molecular geometry using, as input, a correct Lewis Dot
More informationการกำเน ดของ Organic Semiconductors Organic Semiconductors Meet the World
98 SWU Sci. J. Vol. 22 No. 2 (2006) บทความว ชาการ การกำเน ดของ Organic Semiconductors Organic Semiconductors Meet the World พรพ มล ประยงค พ นธ * Pornpimol Prayongpan Introduction Today, semiconductor technologies
More informationSo why is sodium a metal? Tungsten Half-filled 5d band & half-filled 6s band. Insulators. Interaction of metals with light?
Bonding in Solids: Metals, Insulators, & CHEM 107 T. Hughbanks Delocalized bonding in Solids Think of a pure solid as a single, very large molecule. Use our bonding pictures to try to understand properties.
More information* motif: a single or repeated design or color
Chapter 2. Structure A. Electronic structure vs. Geometric structure B. Clean surface vs. Adsorbate covered surface (substrate + overlayer) C. Adsorbate structure - how are the adsorbed molecules bound
More informationOrganic Chemistry Lecture I. Dr. John D. Spence
HEMISTRY 3 Organic hemistry Lecture I Dr. John D. Spence jdspence@scu.edu jspence@csus.eduedu http://www.csus.edu/indiv/s/spencej What is Organic hemistry? 780 s hemistry of compounds from living organisms
More informationSurface Structure and Morphology 2D Crystallography
Surface Structure and Morphology 2D Crystallography Selvage (or selvedge (it. cimosa)): Region in the solid in the vicinity of the mathematical surface Surface = Substrate (3D periodicity) + Selvage (few
More informationChapter 9. Molecular Geometry and Bonding Theories
Chapter 9 Molecular Geometry and Bonding Theories MOLECULAR SHAPES 2 Molecular Shapes Lewis Structures show bonding and lone pairs do not denote shape Use Lewis Structures to determine shapes Molecular
More informationHybridisation of Atomic Orbitals
Lecture 7 CHEM101 Hybridisation of Atomic Orbitals Dr. Noha Osman Learning Outcomes Understand the valence bond theory Understand the concept of hybridization. Understand the different types of orbital
More informationLecture 4: Band theory
Lecture 4: Band theory Very short introduction to modern computational solid state chemistry Band theory of solids Molecules vs. solids Band structures Analysis of chemical bonding in Reciprocal space
More informationChapters 8 and 9. Octet Rule Breakers Shapes
Chapters 8 and 9 Octet Rule Breakers Shapes Bond Energies Bond Energy (review): The energy needed to break one mole of covalent bonds in the gas phase Breaking bonds consumes energy; forming bonds releases
More informationChapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories
Chapter 9 Chemical Bonding II: Molecular Geometry and Bonding Theories Topics Molecular Geometry Molecular Geometry and Polarity Valence Bond Theory Hybridization of Atomic Orbitals Hybridization in Molecules
More informationELEC311( 물리전자, Physical Electronics) Course Outlines:
ELEC311( 물리전자, Physical Electronics) Course Outlines: by Professor Jung-Hee Lee Lecture notes are prepared with PPT and available before the class (http://abeek.knu.ac.kr). The topics in the notes are
More informationNature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
Lecture 20, November 11, 2016 Ionic bonding and crystals Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy
More informationQuantum Condensed Matter Physics Lecture 4
Quantum Condensed Matter Physics Lecture 4 David Ritchie QCMP Lent/Easter 2019 http://www.sp.phy.cam.ac.uk/drp2/home 4.1 Quantum Condensed Matter Physics 1. Classical and Semi-classical models for electrons
More informationCHEM1002 Worksheet 1: Introduction to Carbon Chemistry
CEM1002 Worksheet 1: Introduction to Carbon Chemistry Model 1: Bonding in rganic Molecules ere is a partial periodic table. The shaded elements are the focus of organic chemistry. The number above each
More informationPhotoinduced Water Oxidation at the Aqueous. GaN Interface: Deprotonation Kinetics of. the First Proton-Coupled Electron-Transfer Step
Supporting Information Photoinduced Water Oxidation at the Aqueous Interface: Deprotonation Kinetics of the First Proton-Coupled Electron-Transfer Step Mehmed Z. Ertem,,,* eerav Kharche,,* Victor S. Batista,
More informationBonding and Dynamics. Outline Bonding and Dynamics Water Interactions Self Ionization of Water Homework
Liquid Water Structure In liquid water, most of the water molecules have the same local environment as in ice but the long range structure of ice disappears due to motion of the molecules. Bonds between
More information130 points on 6 pages + a useful page 7
Name KEY Chemistry 350 Spring 2012 Exam #2, March 30, 2012 50 minutes 130 points on 6 pages + a useful page 7 1. Circle the element/compound most likely to have the desired property. Briefly explain your
More informationLecture 2. Unit Cells and Miller Indexes. Reading: (Cont d) Anderson 2 1.8,
Lecture 2 Unit Cells and Miller Indexes Reading: (Cont d) Anderson 2 1.8, 2.1-2.7 Unit Cell Concept The crystal lattice consists of a periodic array of atoms. Unit Cell Concept A building block that can
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. How to get the book of
More informationDiamond. Covalent Insulators and Semiconductors. Silicon, Germanium, Gray Tin. Chem 462 September 24, 2004
Covalent Insulators and Chem 462 September 24, 2004 Diamond Pure sp 3 carbon All bonds staggered- ideal d(c-c) - 1.54 Å, like ethane Silicon, Germanium, Gray Tin Diamond structure Si and Ge: semiconductors
More informationEE130: Integrated Circuit Devices
EE130: Integrated Circuit Devices (online at http://webcast.berkeley.edu) Instructor: Prof. Tsu-Jae King (tking@eecs.berkeley.edu) TA s: Marie Eyoum (meyoum@eecs.berkeley.edu) Alvaro Padilla (apadilla@eecs.berkeley.edu)
More informationELECTRONIC I Lecture 1 Introduction to semiconductor. By Asst. Prof Dr. Jassim K. Hmood
ELECTRONIC I Lecture 1 Introduction to semiconductor By Asst. Prof Dr. Jassim K. Hmood SOLID-STATE ELECTRONIC MATERIALS Electronic materials generally can be divided into three categories: insulators,
More informationLecture 14 February 7, 2014 Symmetry
Lecture 14 February 7, 2014 Symmetry Nature of the Chemical Bond with applications to catalysis, materials science, nanotechnology, surface science, bioinorganic chemistry, and energy Course number: Ch120a
More informationTypes of Covalent Bonds
Types of Covalent Bonds There are two types of covalent bonds (sigma bonds and pi-bonds) depending on which atomic orbitals overlap and how they overlap to form a bond. A sigma bond (σ-bond) is formed
More informationLecture 2: Bonding in solids
Lecture 2: Bonding in solids Electronegativity Van Arkel-Ketalaar Triangles Atomic and ionic radii Band theory of solids Molecules vs. solids Band structures Analysis of chemical bonds in Reciprocal space
More information8.2 Hybrid Atomic Orbitals
420 Chapter 8 Advanced Theories of Covalent Bonding Answer: (a) is a π bond with a node along the axis connecting the nuclei while (b) and (c) are σ bonds that overlap along the axis. 8.2 Hybrid Atomic
More informationAtomic Arrangement. Primer in Materials Spring
Atomic Arrangement Primer in Materials Spring 2017 30.4.2017 1 Levels of atomic arrangements No order In gases, for example the atoms have no order, they are randomly distributed filling the volume to
More informationB. Electron Deficient (less than an octet) H-Be-H. Be does not need an octet Total of 4 valence electrons
B. Electron Deficient (less than an octet) e.g. BeH 2 H-Be-H Be does not need an octet Total of 4 valence electrons Not the same as unsaturated systems that achieve the 8e - (octet) through the formation
More informationLecture 2 Electrons and Holes in Semiconductors
EE 471: Transport Phenomena in Solid State Devices Spring 2018 Lecture 2 Electrons and Holes in Semiconductors Bryan Ackland Department of Electrical and Computer Engineering Stevens Institute of Technology
More informationProperties of Liquids and Solids. Vaporization of Liquids. Vaporization of Liquids. Aims:
Properties of Liquids and Solids Petrucci, Harwood and Herring: Chapter 13 Aims: To use the ideas of intermolecular forces to: Explain the properties of liquids using intermolecular forces Understand the
More informationProperties of Liquids and Solids. Vaporization of Liquids
Properties of Liquids and Solids Petrucci, Harwood and Herring: Chapter 13 Aims: To use the ideas of intermolecular forces to: Explain the properties of liquids using intermolecular forces Understand the
More informationWhat Is Organic Chemistry?
What Is Organic Chemistry? EQ: What is Organic Chemistry? Read: pages 1-3 Answer the questions in your packet Basics of Organic Chem 1 Chapter 1: Structure and Bonding Key terms Organic Chemistry Inorganic
More informationCrystallographic structure Physical vs Chemical bonding in solids
Crystallographic structure Physical vs Chemical bonding in solids Inert gas and molecular crystals: Van der Waals forces (physics) Water and organic chemistry H bonds (physics) Quartz crystal SiO 2 : covalent
More information