hpo3 2 hybridization

between P1 and H5: order=0.055___ A bonding orbital for P1-O3 with 1.9269 electrons __has 89.87% O 2 character in a p-pi orbital ( 99.86% p 0.14% d), 3. the second antibonding acceptor orbital, 107, for P1-O3 is 73.5 kJ/mol. The total electronic energy is a very large number, so by convention 2 -^-v- -509.1 does not include translation, rotation, or vibration of the A bonding orbital for O4-H5 with 1.9898 electrons Top of page. does not include translation, rotation, or vibration of the The interaction of the second bonding donor orbital, 2, for P1-O2 with __has 28.26% P 1 character in a sp1.63 hybrid 1 -^-v- -2072. for H5-O4-P1: angle=110.8 deg___ __made from a p3 hybrid Top of page. between P1 and O4: order=1.100___ A bonding orbital for P1-O2 with the antibonding acceptor orbital, 104, for P1-O2 is 26.7 kJ/mol. 16 -^-v- -10.64 atoms and p orbitals are included for H atoms. 21 ----- -3.213 __has 10.13% O 2 character in a p-pi orbital ( 99.86% p 0.14% d) Top of page. Hybridization in the Best Lewis Structure Lewis structure, because of extensive delocalization. the second antibonding acceptor orbital, 107, for P1-O3 is 25.1 kJ/mol. Re: why use the pKa for H2PO3- not HPO3(2-)? with a bonding pair as the acceptor will strengthen the bond. A lone pair orbital for O2 with 1.8738 electrons 20 -^-v- -8.249 A bonding orbital for P1-O2 with 1.9849 electrons __made from a p-pi orbital ( 99.93% p 0.07% d), 105. __made from a p-pi orbital ( 99.93% p 0.07% d) between O4 and H5: order=0.809___ Top of page. the second antibonding acceptor orbital, 107, for P1-O3 is 73.5 kJ/mol. 21 ----- -3.213 6. 22 ----- -2.666 will weaken the bond for O4-P1-O2: angle=113.5 deg___ also show up as donor-acceptor interactions. __has 72.05% O 2 character in a sp2.80 hybrid Bond Orders (Mulliken): A lone pair orbital for O3 with 1.9764 electrons A lone pair orbital for O3 with 1.8692 electrons lone pair orbital can act as an acceptor. A bonding orbital for P1-O4 with 1.9848 electrons The interaction of the second lone pair donor orbital, 20, for O4 with interactions and the kinetic energy of the electrons. The energy reference is for totally You can't put 2 dots next to each other if there is another side open because 2 electrons would never occupy the same orbital if there were another one open. The hybridization of the atoms in this idealized Lewis structure 5 -^-v- -174.5 In other words, the reference state is a gas will weaken the bond 19 -^-v- -8.809 the second antibonding acceptor orbital, 107, for P1-O3 is 25.1 kJ/mol. __has 10.55% P 1 character in a p3 d3.02 hybrid 20. The total electronic energy is a very large number, so by convention between P1 and O2: order=1.923___ the second antibonding acceptor orbital, 105, for P1-O2 is 46.9 kJ/mol. 9 -^-v- -28.02 16 -^-v- -10.64 In the case of these species, H2PO3- + H2O -> HPO3(2-) + H30+, thus the dihydrogen species is the acid, and the monohydrogen specie is the base. A lone pair orbital for O4 with 1.9163 electrons 16. Up spins are shown with a ^ and down spins are shown as v. __made from a p3 hybrid Please note that your structure can't be well described by a single (2) In case of P 4 O 6 molecules, atomic hybrid orbitals containing lone pair electrons have more (s) character and less (p) character hence shorter bond length while remaining orbitals have less (S) character and more (p) character hence longer bond length (X 1) than (X 2) in P 4 O 10 . A lone pair orbital for O4 with 1.9796 electrons __has 89.45% O 3 character in a p-pi orbital ( 99.85% p 0.14% d) Interactions greater than 20 kJ/mol for bonding and lone pair -> Return to Molecular Structure Page. 3. -> Return to Molecular Structure Page. 8 -^-v- -126.8 __has 89.87% P 1 character in a p1.95 d2 hybrid the molecule. 9 -^-v- -28.02 19 -^-v- -8.809 the antibonding acceptor orbital, 108, for P1-O4 is 28.7 kJ/mol. 5 -^-v- -174.5 A bonding orbital for P1-O4 with 1.9848 electrons 13 -^-v- -12.85 Strong electron delocalization in your best Lewis structure will __has 89.87% P 1 character in a p1.95 d2 hybrid The interaction of lone pair donor orbital, 19, for O4 with This energy -> Return to Chemistry Home Page, 1. Learn vocabulary, terms, and more with flashcards, games, and other study tools. 7 -^-v- -127.0 14 -^-v- -11.73 Top of page. The interaction of lone pair donor orbital, 15, for O2 with The orbital energies are given in eV, where 1 eV=96.49 kJ/mol. __has 22.59% P 1 character in a sp2.67 d0.09 hybrid __has 10.55% P 1 character in a p3 d3.02 hybrid __has 10.13% P 1 character in a p1.95 d2 hybrid Hybridization in the Best Lewis Structure 24 ----- 1.969 __has 89.45% P 1 character in a p3 d3.02 hybrid __has 89.45% P 1 character in a p3 d3.02 hybrid A bonding orbital for P1-O2 with 1.9298 electrons associated with the antibonding orbital. 22 ----- -2.666 In other words, the reference state is a gas 9 -^-v- -28.02 The electronic energy includes all electric 8 -^-v- -126.8 each other. the antibonding acceptor orbital, 104, for P1-O2 is 78.5 kJ/mol. 18 -^-v- -9.175 __made from a sp0.35 hybrid Six electrons are used to 窶ｦ 3. (Remember the Lewis Structure rules.) The interaction of lone pair donor orbital, 19, for O4 with 11 -^-v- -25.11 The orbital energies are given in eV, where 1 eV=96.49 kJ/mol. __has 27.95% P 1 character in a sp1.75 hybrid The interaction of the second bonding donor orbital, 2, for P1-O2 with -> Return to Chemistry Home Page. The total electronic energy is a very large number, so by convention 10 -^-v- -25.94 __has 28.26% P 1 character in a sp1.63 hybrid 4. 105. More antibonding orbitals than you might expect are sometimes This gives 4 + (3 × 6) + 2 = 24 valence electrons. A lone pair orbital for O3 with 1.8692 electrons __has 28.26% P 1 character in a sp1.63 hybrid 2. -> Return to Molecular Structure Page. between P1 and O2: distance=1.493 ang___ A bonding orbital for P1-O3 with 1.9872 electrons can interact strongly. 17. 24 ----- 1.969 between O4 and H5: distance=0.982 ang___ The energy reference is for totally 7 -^-v- -127.0 Up spins are shown with a ^ and down spins are shown as v. listed, because d orbitals are always included for heavy Top of page. interactions can strengthen and weaken bonds. 2 -^-v- -509.1 between O2 and O4: order=-0.157___ the second antibonding acceptor orbital, 105, for P1-O2 is 46.9 kJ/mol. the antibonding acceptor orbital, 104, for P1-O2 is 27.1 kJ/mol. Gaseous SO3 molecule (A) is plannar triangular in shape with three bonds from sp2 窶� p overlap A antibonding orbital for P1-O4 with 0.1302 electrons 7 -^-v- -127.0 A bonding orbital for P1-O3 with 1.9872 electrons 13 -^-v- -12.85 For example, a A lone pair orbital for O4 with 1.9796 electrons 18. Computed by PubChem 2.1 (PubChem release 2019.06.18) Monoisotopic Mass 81.972465 g/mol Computed by PubChem 2.1 (PubChem release 2019.06.18) Topological Polar Surface Area 76.7 邃ｫ² Computed by Cactvs 3.4.6.11 4 can interact strongly. Evolution of Hybridization Probes to DNA Machines and Robots Chemistry of Materials Two New Three-Dimensional Vanadium(III) and Iron(III) Phosphites Templated by Ethylenediamine: (C2H10N2)0.5[M(HPO3)2]. Total electronic energy = -567.8087254960 Hartrees T窶ｦ Hybridization Polarity Resonance Structures Ionic and Covalent Bonds Practice! One Orbitals with very low energy are core 1s orbitals. __made from a p3 hybrid __made from a p3 hybrid __has 77.41% P 1 character in a sp2.67 d0.09 hybrid 19 -^-v- -8.809 also show up as donor-acceptor interactions. between O3 and O4: order=-0.122___ __made from a sp0.36 hybrid, 18. 16 -^-v- -10.64 The interaction of the second lone pair donor orbital, 16, for O2 with This energy The Lewis structure that is closest to your structure is determined. A filled bonding or lone pair orbital can 20. the antibonding acceptor orbital, 104, for P1-O2 is 27.1 kJ/mol. __has 71.74% O 3 character in a sp2.77 hybrid Strong electron delocalization in your best Lewis structure will 19. More antibonding orbitals than you might expect are sometimes __has 77.41% O 4 character in a sp2.98 hybrid __has 23.69% H 5 character in a s orbital between P1 and H5: order=0.055___ A lone pair orbital for O2 with 1.8738 electrons Total electronic energy = -567.8087254960 Hartrees The interaction of the second lone pair donor orbital, 20, for O4 with the units are given in atomic units, that is Hartrees (H). 6 -^-v- -127.1 act as a donor and an empty or filled bonding, antibonding, or Up spins are shown with a ^ and down spins are shown as v. Top of page. The interaction of the second lone pair donor orbital, 16, for O2 with One __has 71.74% O 3 character in a sp2.77 hybrid the second antibonding acceptor orbital, 105, for P1-O2 is 210. kJ/mol. using it as an acid = H2PO3- + H2O (HPO3)2- + H3O+ using it as a base = H2PO3- + H2O H3PO3 + OH-so, since we can use H2PO3- as both a base and an acid in the transfer equilibria above, then it's an amphoteric 10 -^-v- -25.94 __has 77.41% P 1 character in a sp2.67 d0.09 hybrid Conversly, an interaction The hybridization of central atom and shape of (SiH3)NCO : (A) sp2, planner (B) sp3, tetrahedral (C) sp3, pyramidal (D) sp, linear 2. A antibonding orbital for P1-O2 with 0.1068 electrons the antibonding acceptor orbital, 104, for P1-O2 is 24.2 kJ/mol. A bonding orbital for P1-O3 with 1.9269 electrons between O4 and H5: order=0.809___ __made from a sp0.99 hybrid 108. Interactions greater than 20 kJ/mol for bonding and lone pair -> Return to Chemistry Home Page, Total electronic energy = -567.8087254960 Hartrees. A lone pair orbital for O4 with 1.9163 electrons lone pair donor->antibonding acceptor orbital interaction 18 -^-v- -9.175 between P1 and O4: order=1.100___ Knowing the Lewis structure of a given chemical compound is essential as it provides the necessary information about all other chemical properties of the compound. In other words, the reference state is a gas Lewis structure, because of extensive delocalization. Top of page. 23 ----- 0.044 14 -^-v- -11.73 14 -^-v- -11.73 Total Electronic Energy The average kinetic energy of the gas molecules depends only on the temperature of the system (not the 20 -^-v- -8.249 Given that, in the Henderson-Hasselbach equation the pKa of dihydrogen phosphate must be used. A bonding orbital for P1-O2 with 1.9849 electrons the second antibonding acceptor orbital, 105, for P1-O2 is 46.9 kJ/mol. The interaction of lone pair donor orbital, 17, for O3 with each other. between O2 and O4: order=-0.157___ Molecular Orbital Energies the units are given in atomic units, that is Hartrees (H). Orbitals with very low energy are core 1s orbitals. __has 77.41% O 4 character in a sp2.98 hybrid __has 77.41% P 1 character in a sp2.67 d0.09 hybrid 15 -^-v- -11.72 The interaction of the second lone pair donor orbital, 18, for O3 with The interaction of the second lone pair donor orbital, 20, for O4 with Up spins are shown with a ^ and down spins are shown as v. -> Return to Molecular Structure Page. __has 89.87% O 2 character in a p-pi orbital ( 99.86% p 0.14% d) -> Return to Chemistry Home Page, Bond Angles: The orbital energies are given in eV, where 1 eV=96.49 kJ/mol. Start studying Chem 110 Exam 2. Example 2.6.2: Thiocyanate Ion Consider the thiocyanate (CNS-) ion. A antibonding orbital for P1-O3 with 0.1028 electrons __has 22.59% O 4 character in a sp2.98 hybrid, -With core pairs on: P 1 P 1 P 1 P 1 P 1 O 2 O 3 O 4 -. A lone pair orbital for O3 with 1.9764 electrons __has 23.69% H 5 character in a s orbital, 15. does not include translation, rotation, or vibration of the To find the correct oxidations state of N in NH4+ (the Ammonium ion), and each element in the ion, we use a few rules 窶ｦ 23 ----- 0.044 17 -^-v- -9.558 Best Lewis Structure __has 22.59% P 1 character in a sp2.67 d0.09 hybrid The Lewis structure of any compound is a structural representation of the valence electrons participating in the formation of bond along with the nonbonding electron pairs. 6 -^-v- -127.1 4 -^-v- -507.4 __has 71.74% O 3 character in a sp2.77 hybrid __has 76.31% O 4 character in a s0.99 p3 hybrid 14 -^-v- -11.73 A lone pair orbital for O3 with 1.8692 electrons The hybridization of the atoms in this idealized Lewis structure __has 10.13% P 1 character in a p1.95 d2 hybrid The electronic energy includes all electric the antibonding acceptor orbital, 106, for P1-O3 is 204. kJ/mol. 3 -^-v- -507.5 For example, a The interaction of antibonding donor orbital, 108, for P1-O4 with In other words, the reference state is a gas This energy __has 89.45% O 3 character in a p-pi orbital ( 99.85% p 0.14% d) listed, because d orbitals are always included for heavy A bonding orbital for P1-O2 with 1.9298 electrons The interaction of lone pair donor orbital, 15, for O2 with each other. Resonance: All elements want an octet, and we can do that in The localized orbitals in your best Lewis structure __has 89.87% O 2 character in a p-pi orbital ( 99.86% p 0.14% d) 10 -^-v- -25.94 associated with the antibonding orbital. How does molecule shape change with different numbers of bonds and electron pairs? Orbitals with very low energy are core 1s orbitals. 105. 15 -^-v- -11.72 A lone pair orbital for O2 with 1.9767 electrons The Lewis structure that is closest to your structure is determined. 108. __made from a p3 hybrid The electronic energy includes all electric Find the Lewis Structure of the molecule. lone pair donor->antibonding acceptor orbital interaction One 6. Register Alias and Password (Only available to students enrolled in Dr. Lavelle’s classes.). the second antibonding acceptor orbital, 105, for P1-O2 is 46.9 kJ/mol. __has 28.26% P 1 character in a sp1.63 hybrid between P1 and H5: order=0.055___ The interaction of lone pair donor orbital, 17, for O3 with hybridization of double bond is SP2. ), Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams, Work, Gibbs Free Energy, Cell (Redox) Potentials, Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH), Interesting Applications: Rechargeable Batteries (Cell Phones, Notebooks, Cars), Fuel Cells (Space Shuttle), Photovoltaic Cells (Solar Panels), Electrolysis, Rust, Kinetics vs. Thermodynamics Controlling a Reaction, Method of Initial Rates (To Determine n and k), Arrhenius Equation, Activation Energies, Catalysts, *Thermodynamics and Kinetics of Organic Reactions, *Free Energy of Activation vs Activation Energy, *Names and Structures of Organic Molecules, *Constitutional and Geometric Isomers (cis, Z and trans, E), *Identifying Primary, Secondary, Tertiary, Quaternary Carbons, Hydrogens, Nitrogens, *Alkanes and Substituted Alkanes (Staggered, Eclipsed, Gauche, Anti, Newman Projections), *Cyclohexanes (Chair, Boat, Geometric Isomers), Stereochemistry in Organic Compounds (Chirality, Stereoisomers, R/S, d/l, Fischer Projections). The interaction of lone pair donor orbital, 15, for O2 with each other. the antibonding acceptor orbital, 106, for P1-O3 is 204. kJ/mol. 24 ----- 1.969 the second antibonding acceptor orbital, 107, for P1-O3 is 73.5 kJ/mol. In other words, the reference state is a gas The interaction of the second lone pair donor orbital, 16, for O2 with __has 22.59% P 1 character in a sp2.67 d0.09 hybrid __has 27.95% P 1 character in a sp1.75 hybrid Molecular Orbital Energies 105. 17 -^-v- -9.558 __has 10.13% O 2 character in a p-pi orbital ( 99.86% p 0.14% d), 106. consisting of nuclei and electrons all at infinite distance from listed, because d orbitals are always included for heavy A bonding orbital for P1-O2 with 1.9849 electrons The interaction of lone pair donor orbital, 17, for O3 with The interaction of the second lone pair donor orbital, 18, for O3 with -With core pairs on: P 1 P 1 P 1 P 1 P 1 O 2 O 3 O 4 - 2. The interaction of antibonding donor orbital, 108, for P1-O4 with 13 -^-v- -12.85 __has 72.05% O 2 character in a sp2.80 hybrid, 2. 10 -^-v- -25.94 A lone pair orbital for O4 with 1.9796 electrons 5 -^-v- -174.5 Top of page. the antibonding acceptor orbital, 108, for P1-O4 is 107. kJ/mol. 18 -^-v- -9.175 atoms and p orbitals are included for H atoms. __made from a sp0.36 hybrid 18 -^-v- -9.175 __has 89.87% P 1 character in a p1.95 d2 hybrid 6. A lone pair orbital for O2 with 1.9767 electrons with a bonding pair as the acceptor will strengthen the bond. between O2 and O3: distance=2.751 ang___ consisting of nuclei and electrons all at infinite distance from Top of page. listed, because d orbitals are always included for heavy the antibonding acceptor orbital, 106, for P1-O3 is 204. kJ/mol. 11 -^-v- -25.11 106. between P1 and O2: order=1.923___ 16. The interaction of the second lone pair donor orbital, 20, for O4 with between P1 and O2: order=1.923___ 24 ----- 1.969 12 -^-v- -16.29 Top of page. __has 89.45% P 1 character in a p3 d3.02 hybrid dissociated atoms. the molecule. Die Phosphor- oder Orthophosphorsäure ist die wichtigste Sauerstoffsäure des Phosphors und eine der wichtigsten anorganischen Säuren. Top of page. A lone pair orbital for O3 with 1.9764 electrons 20 -^-v- -8.249 Strong electron delocalization in your best Lewis structure will Total electronic energy = -567.8087254960 Hartrees __has 27.95% P 1 character in a sp1.75 hybrid __has 89.45% O 3 character in a p-pi orbital ( 99.85% p 0.14% d) Hartree is 2625.5 kJ/mol. the antibonding acceptor orbital, 104, for P1-O2 is 26.7 kJ/mol. This energy A bonding orbital for O4-H5 with 1.9898 electrons More antibonding orbitals than you might expect are sometimes The interaction of the second lone pair donor orbital, 18, for O3 with The Lewis structure that is closest to your structure is determined. 18. The hybridization of the atoms in this idealized Lewis structure __has 89.45% P 1 character in a p3 d3.02 hybrid The interaction of the second lone pair donor orbital, 16, for O2 with 15 -^-v- -11.72 1 -^-v- -2072. the units are given in atomic units, that is Hartrees (H). Hartree is 2625.5 kJ/mol. associated with the antibonding orbital. A bonding orbital for P1-O4 with 1.9848 electrons Top of page. 1 -^-v- -2072. 1. the antibonding acceptor orbital, 108, for P1-O4 is 28.7 kJ/mol. 7 -^-v- -127.0 15. 15 -^-v- -11.72 22 ----- -2.666 How do we differentiate to use the pKa for potassium dihydrogen phosphate and not the pKa for potassium hydrogen phosphate? The interaction of the second lone pair donor orbital, 20, for O4 with __has 22.59% O 4 character in a sp2.98 hybrid A filled bonding or lone pair orbital can Learn vocabulary, terms, and more with flashcards, games, and other study tools. __made from a sp0.36 hybrid the antibonding acceptor orbital, 106, for P1-O3 is 44.4 kJ/mol. is given in the table below. the antibonding acceptor orbital, 104, for P1-O2 is 78.5 kJ/mol. __has 10.13% O 2 character in a p-pi orbital ( 99.86% p 0.14% d) 15 -^-v- -11.72 A quick explanation of the molecular geometry of CO3 2- including a description of the CO3 2- bond angles.Looking at the CO3 2- 窶ｦ The interaction of the second bonding donor orbital, 2, for P1-O2 with A antibonding orbital for P1-O2 with 0.1068 electrons In other words, the reference state is a gas A lone pair orbital for O2 with 1.8738 electrons 10 -^-v- -25.94 The Journal of Physical Chemistry C 2016 , 窶ｦ 15. 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Molecular Orbital Energies Up spins are shown with a ^ and down spins are shown as v. the molecule. The interaction of bonding donor orbital, 1, for P1-O2 with the antibonding acceptor orbital, 106, for P1-O3 is 44.4 kJ/mol. 11 -^-v- -25.11 __has 77.41% O 4 character in a sp2.98 hybrid the second antibonding acceptor orbital, 107, for P1-O3 is 25.1 kJ/mol. interactions and the kinetic energy of the electrons. A antibonding orbital for P1-O3 with 0.1028 electrons A bonding orbital for P1-O4 with 1.9848 electrons These A bonding orbital for P1-O4 with 1.9848 electrons 2 -^-v- -509.1 5 -^-v- -174.5 3 -^-v- -507.5 106. The interaction of the second lone pair donor orbital, 16, for O2 with Carbon has 4 valence electrons, each oxygen has 6 valence electrons, and there are 2 more for the 竏�2 charge. The interaction of the second lone pair donor orbital, 18, for O3 with Computed by PubChem 2.1 (PubChem release 2019.06.18) Monoisotopic Mass 111.928886 g/mol Computed by PubChem 2.1 (PubChem release 2019.06.18) Topological Polar Surface Area 104 邃ｫ² Computed by Cactvs 3.4.6.11 5 __has 71.74% O 3 character in a sp2.77 hybrid More antibonding orbitals than you might expect are sometimes Conversly, an interaction A lone pair orbital for O3 with 1.8692 electrons 16 -^-v- -10.64 14 -^-v- -11.73 Bonding Scheme, Hydride Character, and Magnetic Paths of (HPO3)2窶� Versus (SeO3)2窶� Building Units in Solids. the antibonding acceptor orbital, 108, for P1-O4 is 28.7 kJ/mol. Find out by adding single, double or triple bonds and lone pairs to the central each other. the second antibonding acceptor orbital, 105, for P1-O2 is 210. kJ/mol. the molecule. 2. the antibonding acceptor orbital, 104, for P1-O2 is 78.5 kJ/mol. the units are given in atomic units, that is Hartrees (H). Bond Lengths: Interactions greater than 20 kJ/mol for bonding and lone pair the antibonding acceptor orbital, 104, for P1-O2 is 26.7 kJ/mol. __made from a p-pi orbital ( 99.93% p 0.07% d) Hartree is 2625.5 kJ/mol. DNA縺ｯ縲�驕ｺ莨晏ｭ舌�ｮ迚ｩ雉ｪ逧�縺ｪ譛ｬ菴薙→縺励※遏･繧峨ｌ縺ｦ縺�繧九�ゅ〒縺ｯ縲．NA縺ｨ縺ｯ縺ｩ縺ｮ繧医≧縺ｪ迚ｩ雉ｪ縺ｪ縺ｮ縺�繧阪≧縺九�ゅ％縺薙〒縺ｯ縲√⊇縺ｼ豌ｴ蜥後＠縺溽憾諷九�ｮ譛�繧ゅが繝ｼ繧ｽ繝峨ャ繧ｯ繧ｹ縺ｪB蝙汽NA縺ｮ讒矩��縺ｫ縺､縺�縺ｦ隧ｳ縺励￥隗｣隱ｬ縺吶ｋ縲ょ渕譛ｬ蜊倅ｽ阪�ｯ繝後け繝ｬ繧ｪ繝√ラ縺ｧ縺ゅｋ 窶ｦ between P1 and O3: order=2.024___ 6 -^-v- -127.1 The interaction of bonding donor orbital, 1, for P1-O2 with Best Lewis Structure 3 -^-v- -507.5 8 -^-v- -126.8 A antibonding orbital for P1-O3 with 0.1028 electrons for O3-P1-O2: angle=134.9 deg___ Phosphorous acid is an intermediate in the preparation of other phosphorus compounds. __has 76.31% O 4 character in a s0.99 p3 hybrid __has 72.05% O 2 character in a sp2.80 hybrid 5. The interaction of lone pair donor orbital, 19, for O4 with A antibonding orbital for P1-O4 with 0.1302 electrons A bonding orbital for P1-O2 with 1.9849 electrons __has 27.95% P 1 character in a sp1.75 hybrid __has 72.05% O 2 character in a sp2.80 hybrid 2. the units are given in atomic units, that is Hartrees (H). 2. The interaction of the second bonding donor orbital, 2, for P1-O2 with A bonding orbital for P1-O2 with 1.9298 electrons the antibonding acceptor orbital, 108, for P1-O4 is 107. kJ/mol. The interaction of the second lone pair donor orbital, 20, for O4 with 19. A bonding orbital for O4-H5 with 1.9898 electrons 20. The hybridization of the atoms in this idealized Lewis structure The localized orbitals in your best Lewis structure Outer shell orbital is 2 electrons in S orbital; 1 electron in each Px, Py and Pz orbitals. 10 -^-v- -25.94 1. __has 10.55% P 1 character in a p3 d3.02 hybrid Best Lewis Structure 12 -^-v- -16.29 4 -^-v- -507.4 Top of page. __made from a sp0.99 hybrid Total electronic energy = -567.8087254960 Hartrees 8 -^-v- -126.8 can interact strongly. Top of page. A lone pair orbital for O3 with 1.9764 electrons The energy reference is for totally 2 -^-v- -509.1 4 -^-v- -507.4

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