From the number of electron pairs around O in OF. Sri Ramakrishna Mission Vidyalaya College of Arts and Science,Coimbatore-20. With suitably optimized hybrids a few structures are capable of giving results close to those obtained at the full-CI limit, while even a single structure (the . Now customize the name of a clipboard to store your clips. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. <>
He said that unpaired . 1 lb = 454.55 g 1 ft = 12 in 1 in = 2.54 cm, What is the frequency of electromagnetic radiation with a wavelength of 445 nm appears as blue light to the human eye? 6.6 Strengths of Ionic and Covalent Bonds 6.7 . Table of Contents Features of Valence Bond theory Hybridization and Geometry of Complexes Hybridization is a concept used in organic chemistry to explain the chemical bonding in cases where the valence bond theory does not provide satisfactory clarification. 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. CH 1-3 Power Point . This confers. Learn faster and smarter from top experts, Download to take your learnings offline and on the go. By accepting, you agree to the updated privacy policy. 15 0 obj
According to the view-point of the C-Me segregating theory in solid alloys, it can be deduced that the hybridization and consequently accept electron pairs from the ligands as under: It can be seen that the d orbitals used in the hybridization are the inner d orbitals (3d) endobj
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 . 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. <>
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(b) For octahedral complexes, using VB theory, hybridization occurs to achieve the most stable angular overlap and therefore the strongest coordinate bonds between the central metal cation and ligands; using this information answer the following questions: (i) For 1st series transition metals, list down the four (4) sets of orbitals that are . As a result, the OF4 molecule is unlikely to exist. Valence Bond Theory and Hybridization Explain the difference between a bond and bond. The theory says that electrons fill the atomic orbitals of an atom within a molecule. 7.1 Introduction 7.2 Valence Bond Theory 7.3 Hybrid Atomic Orbitals 7.4 Multiple Bonds 8 Composition of Substances and Solutions 8.1 Introduction 8.2 Formula Mass and . 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. Each N atom is sp3 hybridized and uses one sp3 hybrid orbital to form the NN bond, two to form NH bonds, and one to accommodate a lone pair. Simply put, this means. 18 0 obj
Furthermore, the two electrons shared by the bonded atoms must have opposite spins. In this case, the new orbitals are called sp hybrids because they are formed from one s and one p orbital. Practice: Bond hybridization. Carbon does form compounds with only two covalent bonds (such as CH2 or CF2), but these species are highly reactive, unstable intermediates that only form in certain chemical reactions. Valence Bond Theory and Hybridization Explain the difference between a bond and bond. Asked for: hybridization of the central atom. In answer to these questions scientists proposed the phenomenon of Hybridization. Worked examples: Finding the hybridization of atoms in organic molecules. !PY pawgdNE,sd1+QSGk=(E(J$hJHU@ P:{tB"(PA(JUib-6}Z(TV;$Z.ok6T4 VQM&cxT
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z=V6'*7aXLmSxr`` /a`"@p Unfortunately, however, recent experimental evidence indicates that in NH3 and H2O, the hybridized orbitals are not entirely equivalent in energy, making this bonding model an active area of research. This theory is especially useful to explain the covalent bonds in organic molecules. - PowerPoint PPT Presentation TRANSCRIPT Get access to all 12 pages and additional benefits: For the electronic transition from n = 3 to n = 5 in the hydrogen atom. 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 endobj
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T- 1-855-694-8886 Furthermore, VSEPR does not provide an explanation of chemical bonding. 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 Is this ion likely to exist? In NH3, for example, N, with a 2s22p3 valence electron configuration, can hybridize its 2s and 2p orbitals to produce four sp3 hybrid orbitals. In fact, it has not been detected. To obtain a measure of the con-tribution of dierent atomic states in the band . Using the VSEPR approach to determine the number of electron pairs and the molecular geometry of the molecule. <>
Placing five valence electrons in the four hybrid orbitals, we obtain three that are singly occupied and one with a pair of electrons: The three singly occupied sp3 lobes can form bonds with three H atoms, while the fourth orbital accommodates the lone pair of electrons. ns-105-general-chemistry-2-svc-1.63.pdf: Jul 30, 2019: 65.9 MB: Offline ZIP: An offline HTML copy of the content. 1. According to VBT there is a direct covalent coordinate bond between . 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. A covalent bond is formed only when half-filled orbitals of two atoms overlap each other. No, valence bond theory can not be used to determine the molecule's shape. According to Valence Bond Theory, the electrons found in the outermost (valence) shell are the ones we will use for bonding overlaps. The main postulates of this theory are as follows: A covalent bond is formed by the overlapping of two half-filled valence atomic orbitals of, The electrons in the overlapping orbitals get paired and confined between the nuclei of two, The electron density between two bonded atoms increases due to overlapping. What hybridization is expected for atoms that have the following numbers of charge clouds? sp2 hybridization iii. Because the difference A B can also be written as A + (B), in Figure \(\PageIndex{2}\) and subsequent figures we have reversed the phase(s) of the orbital being subtracted, which is the same as multiplying it by 1 and adding. Valence Bond Theory & Hybridization written by CHM132 was published in the year 2009 and uploaded for 100 level Science and Technology students of University of Ilorin (UNILORIN) offering CHM132 course. For C, N, and O hybridization means the 2s atomic orbital is combined with one, two, or all three 2p atomic orbitals. Each of the overlapping atomic orbitals must contain, a single, unpaired electron. As we will see, some compounds are highly unstable or do not exist because the amount of energy required to form hybrid orbitals is greater than the amount of energy that would be released by the formation of additional bonds. CH 1-2 Hybridization -Geometry (Review for Worksheet "Zero") CH 1-2 Power Point. By the interactions of C-sp 3 with an H-1s, 4 equivalent C-H bonds can be formed.. Hybridization in Methane. When they overlap in a fashion that creates a node along this axis, they form a bond. The localized bonding model (called valence bond theory) assumes that covalent bonds are formed when atomic orbitals overlap and that the strength of a covalent bond is proportional to the amount of overlap. Valence bond theory describes the electronic structure of molecules. Furthermore, the two electrons shared by the bonded atoms must have, opposite spins. What is the hybridization of the central atom in each species? Valence Bond Theory, Hybrid Orbitals, and Molecular Orbital Theory. sp3d with three BrF bonds and two lone pairs. 27 related questions found. 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. The Necessary Hybrid Orbitals. The molecular geometry about each N is trigonal pyramidal. 17 0 obj
What is the de Broglie wavelength of an electron (m = 9.11 10-31kg) moving at a velocity of 3.0 107m/s? sp hybridization I. VALENCE BOND THEORY AND HYBRIDIZATION 1s! Related: Valence Bond Theory - Chemical Bonding? Ans: The valence bond theory describes the formation of covalent bonds and the electronic structure of molecules. Consider making a donation by buying points. 16 0 obj
comparable energies. 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 Answer PROBLEM 5.3. What is the hybridization of the oxygen atom in OF4? 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. We know, however, that carbon typically forms compounds with four covalent bonds. a.) When Unstable, Nonmetal Atoms Bond, They Do This By Sharing Valence Electrons. endobj
Valence Bond theory was first proposed by W.Heitler and F.London in 1927. 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. Also includes XML, included media files, and other support files. 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. With only a single unpaired electron in its ground state, boron should form only a single covalent bond. 6.74 10 14 s -1 C. 1.48 10 -15 s -1 D. 1.34 10. Valence bond theory is a basic theory that is used to explain the chemical bonding of atoms in a molecule. 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. 22 0 obj
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View the article. Figure 3 shows the total density of states for the va-lence and conduction band. endobj
Important points for understanding the hybridization: (i) The number of hybrid orbitals generated is equal to . it is similar to the process of Hybridization some of you have used or listened in gardening. The geometry of pristine SnS adsorbed of NH 3 and NO 2 is shown in Fig. xZc
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Wi$"_?{gR=Di?6_^j#Mvv%Pkoq/!vmC( =~Db$wP3klDJ.SQAzjDGBD@*{K-:Q 12 Bonding with Valence Bond Theory According to valence bond theory, bonding takes place between atoms when their atomic or hybrid orbitals interact. Hence, it is stronger as compared to the, pi bond where the extent of overlapping occurs to a smaller extent. Free access to premium services like Tuneln, Mubi and more. Valence Bond theory & Hybridization 1 of 30 Valence Bond theory & Hybridization Sep. 17, 2013 135 likes 69,557 views Download Now Download to read offline Education Technology Economy & Finance itutor Follow Advertisement Recommended Hybridization Principles of Organic compounds Dr. Rajasekhar reddy Alavala 360 views 55 slides This theory is largely concerned with the production of individual bonds from the atomic orbitals of the atoms involved in the formation of a molecule. lecnotes15 Valence bond theory and hybridization.pdf - Free download as PDF File (.pdf), Text File (.txt) or read online for free. particles of the atom, Atomic structure, Modern electronic theory of atom, Topics : Water potential, osmosis, plasmolysis, root pressure theory, transpiration pull theory, school: Chukwuemeka Odumegwu Ojukwu University, Topics : polypeptide bond, carboxyl group, synthesized RNA, school: Federal University of Technology, Minna, Topics : chemical bond, octet rule, Nuclear chemistry, bonding, Topics : inorganic chemistry, IUPAC, isomers, molecular formula, chemical reaction, separation technique, mole ratio, chemical bond, alicyclic compound, heterocyclic compound, Topics : isotopy, electronic configuration, chemical bond, thermodynamics, electrochemistry. Given the density of silver is 10.5 g/cm3. <>
In case of sigma bond, the overlapping of orbitals takes place to a larger extent. Transcript. <>
What is the hybridization of the central atom in each species? a) Calculatethe energy. In BeH2, we can generate two equivalent orbitals by combining the 2s orbital of beryllium and any one of the three degenerate 2p orbitals. 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. Each overlapping atomic orbital should contain an unpaired electron with an opposite spin. 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. Such descriptions explain the approximately tetrahedral distribution of electron pairs on the central atom in NH3 and H2O. Using the ns orbital, all three np orbitals, and one (n 1)d orbital gives a set of five sp3d hybrid orbitals that point toward the vertices of a trigonal bipyramid (part (a) in Figure \(\PageIndex{7}\)). PDF: PDF file, for viewing content offline and printing. 19 0 obj
The molecular geometry is tetrahedral. xWjfJVkF These new combinations are called hybrid atomic orbitals because they are produced by combining (hybridizing) two or more atomic orbitals from the same atom. endobj
b) Calculate the wavelength (in nm). The valence bond theory is based on covalent interactions between the central metal and the ligands. '(9\/(llMbwn6{%Zx. D(Ya S9'h[XR&wj%K;9auW> w:[3oK3@_S'T[3Xev,3&`=p~/k_O>DgATe0d's|G!a,1s_Q}Ou*! It is a stronger bond and cylindrically symmetrical. endobj
This strong interaction reduces the symmetry of the structure and manifests in the form of dipoles, resulting in dipole-related properties, including piezoelectric properties. ]n"ktl.KK:4kq-]le
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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. information to examine is the hybridization and charge distribution. 11 0 obj
CH 2-1: Hydrocarbons sp3 characterization. Instructor: Catherine Drennan, Elizabeth Vogel Taylor. The combination of an ns and an np orbital gives rise to two equivalent sp hybrids oriented at 180, whereas the combination of an ns and two or three np orbitals produces three equivalent sp2 hybrids or four equivalent sp3 hybrids, respectively. 4. Consider the energy level diagram for a single atom of hydrogen: 1s 1 Hydrogen would be much happier (i.e. J Pharm Pharmaceut Sci (www.cspsCanada.org) 8(3):586-592, 2005 588 Graph theory. 3HF\*_$zvAoNNIxKQym@5j65(Y=rrEjw wu8zG7-ac((`(@nb1o?Ah}lO~Y 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. \[sp = \dfrac{1}{\sqrt{2}} (2s + 2p_z) \label{9.5.1a} \], \[sp = \dfrac{1}{\sqrt{2}} (2s - 2p_z) \label{9.5.1b} \]. endobj
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 . 24 0 obj
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