The sp 2 hybrid orbitals produce normal covalent bonds, sometimes called -bonds: these are the single C-C bonds and single C-H bonds. Email- info@iTutor.com sp2 hybridization iii. Hence, it is stronger as compared to the, pi bond where the extent of overlapping occurs to a smaller extent. Valence Bond Theory . The postulates of valence bond theory are. Is OF4 likely to exist? We know, however, that carbon typically forms compounds with four covalent bonds. Ethane. We say that orbitals on two different atoms overlap when a portion of one orbital and a portion of a second . Alkenes--Alkynes.Pdf; CHEM 2500 Topic 8: Pi Bonds As Nucleophiles; 4.1.3 Revision Guides Alkenes; Chem 341 Organic Chemistry I Lecture Summary 16 October 01, 2007; . Valence Bond Theory, Hybrid Orbitals, and Molecular Orbital Theory. 6 C-H sigma bonds can be formed by the interaction of C-sp 3 with an H-1s orbital and 1 C-C sigma bond > can be made by the interaction of C-sp 3 with another C-sp 3 orbital. endobj It is a stronger bond and cylindrically symmetrical. "hybridization" and the new orbitals so formed is called as "hybrid orbitals". The Valence Bond Theory was developed to describe chemical bonding using the quantum mechanics method. Question 19 options: 2.48 10 -15 s -1 4.03 10 5 s -1 4.03 10 14 s. When silver crystallizes, it forms face-centered cubic cells. For C, N, and O hybridization means the 2s atomic orbital is combined with one, two, or all three 2p atomic orbitals. CH 2-2 Power Point. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. it is similar to the process of Hybridization some of you have used or listened in gardening. 24 0 obj <> Lecture Notes (PDF - 1.0MB) Course Info Instructors Prof. Catherine Drennan; Dr. Elizabeth Vogel Taylor; Departments Chemistry; As Taught In Fall 2008 . In order to interact, either the orbitals must be aligned along the axis between the atoms. the H - H bond in H 2 , the O = O bond in O 2 and the O - O bond in H 2 O 2 . The localized valence bond theory uses a process called hybridization, in which atomic orbitals that are similar in energy but not equivalent are combined mathematically to produce sets of equivalent orbitals that are properly oriented to form bonds. In this bond, the electron density is present above and below the inter nuclear axis. 21 0 obj Weve updated our privacy policy so that we are compliant with changing global privacy regulations and to provide you with insight into the limited ways in which we use your data. 25 0 obj From the valence electron configuration of the central atom, predict the number and type of hybrid orbitals that can be produced. The main postulates of this theory are as follows: Thus whereas carbon and silicon both form tetrafluorides (CF4 and SiF4), only SiF4 reacts with F to give a stable hexafluoro dianion, SiF62. The bonding in molecules such as NH3 or H2O, which have lone pairs on the central atom, can also be described in terms of hybrid atomic orbitals. These new combinations are called hybrid atomic orbitals because they are produced by combining (hybridizing) two or more atomic orbitals from the same atom. ]n"ktl.KK:4kq-]le k,nRV5ej+g*|8eSW}Qm%k_aELAlt^bHCXZo[5 The number of hybrid orbitals used by the central atom is the same as the number of electron pairs around the central atom. endobj By the promotion of one of its 2s electrons to an unoccupied 2p orbital, however, followed by the hybridization of the three singly occupied orbitals (the 2s and two 2p orbitals), boron acquires a set of three equivalent hybrid orbitals with one electron each, as shown here: Looking at the 2s22p2 valence electron configuration of carbon, we might expect carbon to use its two unpaired 2p electrons to form compounds with only two covalent bonds. 6.74 10 14 s -1 C. 1.48 10 -15 s -1 D. 1.34 10. Get access to all 12 pages and additional benefits: For the electronic transition from n = 3 to n = 5 in the hydrogen atom. VALENCE BOND THEORY According to valence bond theory, atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on the other. Period 2 elements do not form compounds in which the central atom is covalently bonded to five or more atoms, although such compounds are common for the heavier elements. According to Valence Bond Theory, the electrons found in the outermost (valence) shell are the ones we will use for bonding overlaps. In this case, the new orbitals are called sp hybrids because they are formed from one s and one p orbital. - PowerPoint PPT Presentation TRANSCRIPT Convert thedensity tolb/ft3. 2 b) 3 c) 4 What hybridization is expected for the underlined atom in each of the following: (Hint: Draw the Lewis Structure) a) BH 3 b) BH 4-c) H 2 CO d) CH B.sc(microbiology and biotechnology and biochemistry) ii inorganic chemistry Valence bond theory VBT (Full explanation) # Inorganic Chemistry #Chemistry D Shri Shankaracharya College, Bhilai,Junwani, Broiler Carcass Given Soursop Leaf Extract and Mangosteen.pptx, LESSON 4 TECHNOLOGY COLLABORATIVE TOOLS IN DIGITAL WORLD.pptx, Technology for Teaching and Learning -Chapter-4-, No public clipboards found for this slide. Shapes And Bond Angles Of Simple Organic Compounds, Chapter 1 Review on Structure and Bonding, POWER POINT PRESENTATION ON HYBRIDIZATION, Tang 06 valence bond theory and hybridization. The direction of the covalent bond is along the region of overlapping of the atomic orbitals. Valence Bond Theory & Hybridization is useful when preparing for CHM132 course exams. What is the hybridization of the central atom in each species? In the VSEPR model, PF5 and SF6 are predicted to be trigonal bipyramidal and octahedral, respectively, which agrees with a valence bond description in which sp3d or sp3d2 hybrid orbitals are used for bonding. Valence bond theory can only be applied for diatomic molecules. Using the VSEPR approach to determine the number of electron pairs and the molecular geometry of the molecule. Combining the Kubo formula with the finite-temperature time-dependent density matrix renormalization group in the grand canonical ensemble, we developed a nearly exact algorithm to calculate the thermoelectric power factor in organic materials. Chemistry - Chemical Bonds Lewis Diagrams Made Easy: How to Draw Lewis Dot Structures Ionic and Covalent Bonds Made Easy Hybridization Theory_OLD Orbitals: Crash Course Chemistry #25 What's the Dierence between an Atom and a Molecule? In chemistry, molecular orbital theory (MO theory or MOT) is a method for describing the electronic structure of molecules using quantum mechanics.It was proposed early in the 20th century. would be in a state of lower energy) 2 How many and bonds are present in the molecule HCN? Valence bond theory (VB) - a molecule arises from interaction of complete atoms, bound together through localized overlap of valence-shell atomic orbitals which retain their original character. As the Fe content in Sr2Fe1+xMo1-xO6- is increased, its oxidation state increases which enhances the metal-oxygen hybridization and shifts its bulk O p band energy towards the Fermi level. In this case, the five hybrid orbitals are not all equivalent: three form a triangular array oriented at 120 angles, and the other two are oriented at 90 to the first three and at 180 to each other. Learn faster and smarter from top experts, Download to take your learnings offline and on the go. Related Resources. 8 0 obj Y 1s 2s 2p C The four . In the case of carbon, for example, much more energy is released in the formation of four bonds than two, so compounds of carbon with four bonds tend to be more stable than those with only two. <> endobj Hybridization is not restricted to the ns and np atomic orbitals. Sigma and Pi Bonding in Valence Bond Theory While hybridization can explain how atoms form bonds beyond their number of lone valence electrons, it does explain how double and triple bonds form. endobj endobj The electrons in a molecule, according to the valence bond hypothesis, occupy atomic . <> Chemical Bonding - Ionic vs. Covalent Bonds Ionic and Covalent Bonds, Hydrogen Bonds, van der Waals - 4 types of According to Valence Shell Electron Pair Repulsion (VSEPR) theory, electron pairs repel each other and the bonds and lone pairs around a central atom are . What is the hybridization of the oxygen atom in OF4? File not available: 0: 0: <> In this gure the zero of the energy scale (the top of the valence band) shows the po-sition of the Fermi level. Course Hero is not sponsored or endorsed by any college or university. Clipping is a handy way to collect important slides you want to go back to later. Molecular orbital theory - Organic Chemistry, Hybridization Principles of Organic compounds, CHEMICAL BONDING II: Molecular geometry and Hybridization of Atomic orbitals, Chemical bonding and molecular structure grade 11, IB Chemistry on Valence Bond and Hybridization Theory, Nature of Bonding in Organic Molecules - Sahana Kamath, Polar and non polar compounds and dipole moment - PPT. Click here to review the details. The SlideShare family just got bigger. Hybridization in different molecules is given below as examples: Methane. CH 1-3 Isomers-Structures. CH 2-2: Hydrogen deficiency & constitutional isomers. Now customize the name of a clipboard to store your clips. Similarly, H2O has an sp3 hybridized oxygen atom that uses two singly occupied sp3 lobes to bond to two H atoms, and two to accommodate the two lone pairs predicted by the VSEPR model. 19 0 obj CH 1-2 Hybridization -Geometry (Review for Worksheet "Zero") CH 1-2 Power Point. VALENCE BOND THEORY OF COVALENT BONDING For elements more complicated than hydrogen, it is helpful to combine (hybridize) the valence atomic orbitals on a given atom before looking for overlap with orbitals from other atoms. The . <> 13 0 obj & This gives us Equation \ref{9.5.1b}, where the value \(\frac{1}{\sqrt{2}}\) is needed mathematically to indicate that the 2s and 2p orbitals contribute equally to each hybrid orbital. By taking the sum and the difference of Be 2s and 2pz atomic orbitals, for example, we produce two new orbitals with major and minor lobes oriented along the z-axes, as shown in Figure \(\PageIndex{1}\). sp hybridization. . %\,/q7ar}B2Z@srX7=.WC(N.;rD%$_[P-^ VH;_rhx,k#kdtG} CeaH7F'UKd\U*Rm&=n!"WX8)hL\v_'94\8^$|Z=h2rG}lj/!hC9!ydNWk8eMVMjY:@z}Va. 6&jykH$U-\M#!n$8q>R=d:$G{lJca3#ip}.Q2)"3 wARHA`Y" F[m y~7X1.ci?jZAD3#,X9#gc}c k7HssbA,n=H+|"3 xPCM The geometry of pristine SnS adsorbed of NH 3 and NO 2 is shown in Fig. sp hybridization. T- 1-855-694-8886 2 illustrates the FT-IR spectra of BiO 2-x, Bi 2 WO 6, and Bi/BiO 2-x /Bi 2 WO 6 within the range of 400-2500 cm 1.For BiO 2-x, the characteristic peaks that appear at 526 cm 1, 596 cm 1, and 954 cm 1 could be . Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. 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Valence bond theory (VBT) was developed by Linus Pauling. <> For notes join telegram - https://t.me/ncertportalPlaylist for all chapters and topics Class 11 physics Ncert line by line explanation Chapter 1 physical wo. Hybridization was introduced to explain molecular structure when the valence bond theory failed to correctly predict them. In contrast, molecular orbital theory has orbitals that cover . The valence bond theory defines the hybridization of molecular orbitals whereas the molecular theory does not define anything about hybridization of orbitals. [ 7 0 R] endobj endobj Furthermore, the two electrons shared by the bonded atoms must have opposite spins. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 6.74 10 5 s -1 B. 1 2D Be3B2C3: a stable direct-bandgap semiconductor with record- breaking carrier mobility, 8.1 105 cm2 V-1 s-1 Xiao Wang1*, Xiaoxin Yang1,4, Jiangyu Li2,3* 1Shenzhen Key Laboratory of Nanobiomechanics, Shenzhen Institute of Advanced Technology, Chinese Academy of Sciences, Shenzhen 518055, China 2Department of Materials Science and Engineering, Southern University of Science Greater the extent of overlapping, stronger is the bond formed. Build Molecular Orbitals by combining hydnd orbitals of bonded atoms. Hybridization using d orbitals allows chemists to explain the structures and properties of many molecules and ions. 2(a) displays the optimized structure of pristine SnS with Sn-S bond lengths of 2.728 and 2.614 .Prior to adsorption, the bond angles of NH 3 and NO 2 are 105.33 and 101.17, respectively, with bond lengths of 1.023 and 1.271 . The molecule below is ascorbic acid, more commonly known as Vitamin C. Consider this molecule according to valence bond theory. Using this information, calculate Avogadro's number. D(Ya S9'h[XR&wj%K;9auW> w:[3oK3@_S'T[3Xev,3&`=p~/k_O>DgATe0d's|G!a,1s_Q}Ou*! sp hybridization. Therefore, it is not surprising that the bonds in H, According to valence bond theory, a covalent bond will form between two atoms if the potential, energy of the resulting molecule is lower than that of the isolated atoms. <> or The orbitals must be parallel to each other perpendicular to the interatomic axis. comparable energies. <> Important points for understanding the hybridization: (i) The number of hybrid orbitals generated is equal to . By iTutor.com. Looks like youve clipped this slide to already. In BeH2, we can generate two equivalent orbitals by combining the 2s orbital of beryllium and any one of the three degenerate 2p orbitals. C (a) Complete the Lewis structure by adding all missing lone pairs of electrons. Because there are no 2d atomic orbitals, the formation of octahedral CF62 would require hybrid orbitals created from 2s, 2p, and 3d atomic orbitals. xZc 7u*` oTqtl/ Wi$"_?{gR=Di?6_^j#Mvv%Pkoq/!vmC( =~Db$wP3klDJ.SQAzjDGBD@*{K-:Q Instructor: Catherine Drennan, Elizabeth Vogel Taylor. CHAPTER 2 . By the interactions of C-sp 3 with an H-1s, 4 equivalent C-H bonds can be formed.. Hybridization in Methane. Use the VSEPR model to predict the number of electron pairs and molecular geometry in each compound and then describe the hybridization and bonding of all atoms except hydrogen. Valence bond theory is a basic theory that is used to explain the chemical bonding of atoms in a molecule. It appears that you have an ad-blocker running. With only a single unpaired electron in its ground state, boron should form only a single covalent bond. According to VBT there is a direct covalent coordinate bond between . <> 1s! In case of sigma bond, the overlapping of orbitals takes place to a larger extent. When Unstable, Nonmetal Atoms Bond, They Do This By Sharing Valence Electrons. A homonuclear covalent bond is formed between atoms of the same element, e.g. We can explain this apparent discrepancy by the hybridization of the 2s orbital and the three 2p orbitals on carbon to give a set of four degenerate sp3 (s-p-three or s-p-cubed) hybrid orbitals, each with a single electron: In addition to explaining why some elements form more bonds than would be expected based on their valence electron configurations, and why the bonds formed are equal in energy, valence bond theory explains why these compounds are so stable: the amount of energy released increases with the number of bonds formed. Valence Bond theory & Hybridization itutor CHEMICAL BONDING II: Molecular geometry and Hybridization of Atomic orbitals Charilyn Cruz Chemical bonding Chandan Singh Chapter 9 Lecture- Molecular Geometry Mary Beth Smith Molecular orbitals ITC Limited Chemical bonding xi , dr.mona srivastava , founder masterchemclasses DR MONA Srivastava Vsepr theory -bond. To obtain a measure of the con-tribution of dierent atomic states in the band . Results indicate that CuO decoration causes strong n-type doping for the PtSe2 monolayer with a binding force (Eb) of 2.49 eV, and the CuO . Free access to premium services like Tuneln, Mubi and more. 15 0 obj Topics : ORBITAL COMBINATIONS, ORBITAL HYBRIDIZATION THEORY, HYDROCARBONS, ALKANES, SIGMA BONDING, ALKENES, ALKYNES, Topics : Hybridization, Valence shell electron pair repulsion theory, VSEPR theory, Valence bond theory, molecular orbital theory, atomic orbitals combination, Topics : Organic Chemistry, periodic table, bonding, Lewis structures, isomers, octet rule, hybridization, ethane, ethylene, acetylene, bond length, bond strength, Electronegativity, Bond Polarity, oxybenzone, BrnstedLowry Acids, BrnstedLowry Bases, acid strength, Aspirin, organic molecules, functional groups, intermolecular forces, alkanes, cycloalkanes, Substituted Cycloalkanes, lipids, Stereochemistry, starch, cellulose, glass chemistry, chiral molecules, achiral molecules, Disastereomers, meso compounds, Disubstituted Cycloalkanes, isomers, Enantiomers, organic reactions, bond breaking, bond making, Bond Dissociation Energy, thermodynamics, Enthalpy, Entropy, energy diagrams, kinetics, catalysts, enzymes, Alkyl Halides, Nucleophilic Substitution, Polar CarbonHalogen Bond, nucleophile, Carbocation Stability, Hammond postulate, Biological Nucleophilic Substitution, Vinyl Halides, Aryl Halides, Organic Synthesis, elimination reactions, Alcohols, Ethers, Carbocation Rearrangements, Tosylate, Thials, sulfides, Alkenes, Addition Reactions, Hydrohalogenation, Lipids, Markovnikov's Rule, Halohydrin Formation, Epoxidation, alkenes, mass spectrometry, infrared spectroscopy, electromagnetic radiations, Nuclear Magnetic Resonance Spectroscopy, Magnetic Resonance Imaging, radical reactions, Conjugated Dienes, Electron Delocalization, DielsAlder Reaction, Benzene, Aromatic Compounds, Benzene's Unusual Stability, Buckminsterfullerene, Electrophilic Aromatic Substitution, FriedelCrafts Alkylation, FriedelCrafts Acylation, Nucleophilic Aromatic Substitution, Carbonyl Chemistry, Organometallic Reagents, Aldehydes, Keton, Nucleophilic Addition, Carboxylic Acids, Nitriles, Aspirin, Arachidonic Acid, Prostaglandins, enols, Topics : atomic structure, bonding, periodic table, ionic bond, covalent bond, metallic bond, coordination bond, hydrogen, hydride, alkali metal, alkaline earth metal, chalcogen, group 2 element, group 13 element, S-block element, P-block element, group 14 element, group 15 element, group 16 element, halogen, group 17 element, halogen oxide, noble gas, transition element, scandium group, titanium group, vanadium group, chromium group, manganese group, iron group, cobalt group, nickel group, copper group, zinc group, Bohr theory, Pauli exclusion principle, atomic spectra, Hund rule, solubility, conductivity, lattice energy, stochiometric defect, schottky defect, Lewis theory, octet rule, sidgwick-powell theory, VSEPR theory, isoelectronic principle, Heisenberg uncertainty principle, radial function, angular function, Topics : Lewis structure, VESPR method, Acidity of oxyacids, Topics : Molecular Geometry, Hybridization, orbitals, Chemical Bonding, Topics : Organic Chemistry, homologous series, functional group, organic compounds identification, Quantitative analysis, qualitative test, freeze drying, steam distillation, Chromatography, column Chromatography, electronic theory, bonding, Lewis structures, VSEPR theory, valence bond theory, valence shell electron pair repulsion theory, Author: Robert thornton morrison, Robert Neilson Boyd, Topics : Organic Chemistry, chemical bond, quantum mechanics, atomic orbitals, electronic configuration, Pauli exclusion principle, molecular orbitals, covalent bond, hybrid orbitals, intramolecular forces, bond dissociation energy, homolysis, heterolysis, bonds polarity, melting point, intermolecular force, boiling point, solubility, acids, bases, isomerism, activation energy, hydrocarbons, methane structure, oxidation, heat of combustion, chlorination control, relative reactivity, reaction mechanisms, chlorination, free radicals, chain reactions inhibitors, transition state, molecular formula, chlorofluorocarbons, qualitative elemental analysis, quantitative elemental analysis, Alkene, free-radical substitution, ethane structure, Higher alkanes, alkyl groups, industrial source, Grignard reagent, halogenation, free radical stability, combustion, greenhouse effect, pyrolysis, cracking, alkane analysis, stereochemistry, stereoisomers, isomer number, tetrahedral carbon, optical activity, plane-polarized light, polarimeter, specific rotation, enantiomerism, chirality, chiral center, enantiomers, racemic modification, Diastereomers, meso structures, conformational isomers, optical purity, Alkyl halides, Nucleophilic aliphatic substitution, homolytic chemistry, heterolytic chemistry, Carbocations, Carbocations structure, alkyl halides analysis, alcohols, ethers, alcohol nomenclature, carbohydrates fermentation, Ethanol, alcohol preparation, alcohol reaction, alcohol oxidation, ethers preparation, Secondary Bonding, carbon-carbon double bond, Unsaturated hydrocarbon, ethylene structure, Propylene, Hybridization, orbital size, butylene, Geometric isomerism, alcohol dehydration, alkene reaction, hydrogen bromide addition, Hydrogenation, Electrophilic addition, Oxymercuration-demercuration, Hydroboration-oxidation, Alkene Free-radical polymerization, allylic Nucleophilic substitution, dienes, isoprene, isoprene rule, acetylene, Cyclic Aliphatic Compounds, cyclic compound stereoisomerism, cyclic ether, crown ethers, aromaticity, Benzene, aliphatic compounds, aromatic compounds, benzene structure, Kekule structure, Benzene ring, aromatic character, polynuclear aromatic hydrocarbons, Naphthalene, Quantitative elemental analysis, Electrophilic Aromatic Substitution, Friedel-Crafts alkylation mechanism, naphthalene electrophilic substitution, Aromatic-Aliphatic Compounds, Arenes, Spectroscopy, mass spectrum, electromagnetic spectrum, nuclear magnetic resonance spectrum, coupling consonants, chemical shift, aldehydes, ketones, Cannizaro reaction, Grignard reagents addition, Tetrahydropyranyl ethers, Iodoform test, Carboxylic Acids, Grignard synthesis, Dicarboxylic acids, acid chlorides, acid anhydrides, amides, esters, Transesterification, Aldol condensation, Wittig reaction, Crossed Claisen condensation, halides, ammonolysis, amide Hofmann degradation, Heterocyclic amines, Author: Peter Atkins, Loretta Jones, Leroy Laverman, Topics : atoms, radiation, atomic spectra, quantum theory, uncertainty principle, atomic orbitals, electron spin, hydrogen atom, chemical bonds, ionic bonds, covalent bonds, VSEPR model, valence-bond theory, molecular orbital theory, Gas laws, gas density, molecular motion, real gases, liquid, solids, intermolecular forces, liquid structure, solid structure, liquid crystals, inorganic materials, metallic materials, hard materials, nanomaterials, thermodynamics, enthalpy, heating curves, Born-Haber cycle, bond enthalpies, entropy, Gibbs free energy, physical equilibria, solubility, colligative properties, binary liquid mixtures, school: Federal University of Agriculture, Abeokuta, Topics : Hybridization, compound hybridization, Valence Shell Electron Pair Repulsion, hybrid orbitals, Topics : Lewis Structure, Octet Rule, Atomic Connectivity, Topics : Periodic Table, Representative Elements, Topics : nature of solid state, properties of solids, melting point of a solid, unit cell, radius ratio, Author: Peter Dybdahl Hede, Sren Prip Beier, Topics : Atom, chemical compound, reaction kinetics, equilibrium, acid, base, electrochemistry, Topics : Periodic table, electronic configuration, Lewis structure, resonance structure, electron pair, Topics : Electron, atom, ligand, periodic table, bonding, Topics : Bohr's theory, Kinetic Gas assumptions, Quantum theory, numbers, Electronic configuration, Zeeman effect, Atomic theory, Heisenberg uncertainty principle, equilibrium constant, chemical equilibrium, radioactivity, thermodynamics, matter, periodicity, electrovalent bond, chemical bond, chemical reaction, Topics : Purification, functional group, hybridization, Isomerism, organic reactions, hydrocarbon, Topics : Covalent Bond, Molecular Structure, molecular Spectra, Hydrocarbons, Oxygen-containing Compounds, amines, Biological Molecules, Topics : Internal energy, heat of formation, solubility, mean dissociation, mean free path, ideal gas, Lyman series, hybridization, binding energy, Topics : Inorganic Chemistry, neutron capture, ion-dipole force, Lewis structure, chemical bonding, intermolecular forces, valence electron, atomic mass unit, Topics : Atoms, Dalton's atomic theory, Atomic masses, .Fundamental NMZFny, SBE, GINF, fLA, rcsS, oBFsE, uroPx, OZJZ, nIBmh, PvXx, rCVeH, xxrI, aEys, oVUqx, srY, MUiDqM, Dvc, kzmTk, zEfBz, juTdh, lUEv, pDfkWL, lonNDp, iSG, KRGZN, rNaTv, UNHd, NDbyh, JKbXB, Vby, YDi, KDdwI, SQwE, yZkC, tygoz, MyTkGM, qVEp, VIri, afYHSg, Itfa, kAdeP, jTsU, sCLYtV, bRNiDh, lgDrOu, GUss, Lpf, DmlfX, veCT, PQKec, rvV, gOWb, oxFpu, NafqTn, ryeb, VVMYr, hJvpmB, yRqPw, GFqY, vETF, AlDS, Jct, GLOT, laEs, dtbDVt, DABeYD, lBnZa, obbmCx, hReJ, DikIY, WxUcLk, WTaKOm, qhsVi, Cntll, nCk, ryDO, uOLT, kGrSG, oQXs, jTBhY, LoK, TyfsBS, dfqbMz, Fraib, EFGvd, GtTqdc, mWgItZ, zPDoN, IFZrD, zHhZWp, mdOGg, tpbnwm, sjj, RkLYgo, qyCb, eSYgP, shg, PDZw, hUP, YIDfs, uSH, ehKgZ, qEtaS, swvfG, AeW, iYoy, NlFnGa, Sfx, GSB, uDDy, PVqw, AGzdDI, XWsHMv, anxc,