[{"data":1,"prerenderedAt":146},["ShallowReactive",2],{"cheatsheet-molecular-geometry-and-bonding-theories":3},{"sheet":4},{"sheetSlug":5,"topicSlugs":6,"primaryTopic":7,"title":8,"subtitle":9,"sections":10},"molecular-geometry-and-bonding-theories",[5],15,"Molecular Geometry & Bonding Theories","VSEPR shapes, bond angles, polarity, hybridization, sigma/pi bonds, and molecular-orbital basics.",[11,23,31,63,71,79,87,95,114,122,130,138],{"heading":12,"kind":13,"items":14},"Bond polarity","rules",[15],{"ref":16,"mode":19,"provenance":20,"text":21,"source_hash":22},{"type":17,"topic":7,"id":18,"field":17},"rule","MS-R001","transform","owned_workbook","Identical atoms → nonpolar bond; different electronegativity → polar bond. A small nonzero ΔEN (e.g. Cl–Br) still gives a real bond dipole even though the ΔEN classification bin calls it 'nonpolar covalent'.","eadad636932fcf3b0bc5ae82985145317a4c3e5783b843e31fd315e600b0c967",{"heading":24,"kind":13,"items":25},"Count electron domains",[26],{"ref":27,"mode":19,"provenance":20,"text":29,"source_hash":30},{"type":17,"topic":7,"id":28,"field":17},"MS-R002","On the central atom, count domains = bonding pairs (a single, double, or triple bond is ONE domain each) + lone pairs + any single-electron radical.","da5338a3c39295fe9163aaecff4ae3c9488debde6fed9543c3dc59a1e5a680ea",{"heading":32,"kind":33,"columns":34,"items":37},"Electron geometry","data",[35,32,36],"Domains","Ideal angles",[38],{"ref":39,"mode":19,"provenance":20,"rows":41,"source_hash":62},{"type":17,"topic":7,"id":40,"field":17},"MS-R003",[42,46,50,54,58],[43,44,45],"2","linear","180°",[47,48,49],"3","trigonal planar","120°",[51,52,53],"4","tetrahedral","109.5°",[55,56,57],"5","trigonal bipyramidal","90° / 120° / 180°",[59,60,61],"6","octahedral","90° / 180°","3fbaac68d2d4646822095b939e492bb286a1174ae98316044b6cf19acdad7e6a",{"heading":64,"kind":13,"items":65},"Molecular geometry",[66],{"ref":67,"mode":19,"provenance":20,"text":69,"source_hash":70},{"type":17,"topic":7,"id":68,"field":17},"MS-R004","Names the arrangement of BONDS only (lone pairs are invisible to the shape). Drop lone-pair domains from the parent electron geometry: e.g. bent, trigonal pyramidal, see-saw, T-shaped, square planar, square pyramidal.","6843ec8c8c1b5be3bfee2f331b8a2aaa37df91c98fc2eaa702ab1cc8211c676a",{"heading":72,"kind":13,"items":73},"Lone-pair repulsion",[74],{"ref":75,"mode":19,"provenance":20,"text":77,"source_hash":78},{"type":17,"topic":7,"id":76,"field":17},"MS-R005","Lone pairs repel more than bonding pairs, compressing angles below ideal: H₂O 104.5° and NH₃ 107° (vs 109.5°). More lone pairs → more compression.","ab5359636f6c0c6566c824f45af425689d757cfdf7508fa56812874fadf38029",{"heading":80,"kind":13,"items":81},"Lone-pair placement",[82],{"ref":83,"mode":19,"provenance":20,"text":85,"source_hash":86},{"type":17,"topic":7,"id":84,"field":17},"MS-R006","Trigonal bipyramidal: lone pairs take equatorial sites (fewer 90° neighbours) → see-saw, T-shaped, linear. Octahedral: two lone pairs go trans (opposite) → square planar.","08fbb39a0185ea4afc691d2667d63f901b564984441b710aa55bd19efbd94378",{"heading":88,"kind":13,"items":89},"Molecular polarity",[90],{"ref":91,"mode":19,"provenance":20,"text":93,"source_hash":94},{"type":17,"topic":7,"id":92,"field":17},"MS-R007","Symmetric arrangement of identical polar bonds → dipoles cancel → nonpolar (CO₂, BF₃, CH₄, PF₅, SF₆). Asymmetric (usually a lone pair on the central atom) → polar (H₂O, NH₃, SO₂, SCl₄).","e617c49762f02d5730bdcd1b313dd7afe0feae39fee7881d73e005cf0d613192",{"heading":96,"kind":33,"columns":97,"items":98},"Hybridization",[35,96],[99],{"ref":100,"mode":19,"provenance":20,"rows":102,"source_hash":113},{"type":17,"topic":7,"id":101,"field":17},"MS-R009",[103,105,107,109,111],[43,104],"sp",[47,106],"sp²",[51,108],"sp³",[55,110],"sp³d",[59,112],"sp³d²","726f0fcb4d850bc5a8f49176f3431212e80a4d8a5f5699fa25a9917d1d7c3069",{"heading":115,"kind":13,"items":116},"Sigma & pi bonds",[117],{"ref":118,"mode":19,"provenance":20,"text":120,"source_hash":121},{"type":17,"topic":7,"id":119,"field":17},"MS-R010","Single = 1 σ; double = 1 σ + 1 π; triple = 1 σ + 2 π. Every bonded connection (including each C–H) is one σ; π count comes only from double and triple bonds.","d293d3cb269e3be6a2dfb0ed5c1887377477ccf6ad984c0e83c6c0baa14b41cc",{"heading":123,"kind":13,"items":124},"MO bond order",[125],{"ref":126,"mode":19,"provenance":20,"text":128,"source_hash":129},{"type":17,"topic":7,"id":127,"field":17},"MS-R013","Bond order = (bonding e⁻ − antibonding e⁻) / 2. Zero means no stable bond (Ne₂). Half-integers occur for odd species: O₂⁻ = 1.5, O₂⁺ = 2.5.","8f3f8ecd8fa1d39152718c349e7a7281af912c7d9f0ceacf981927df12bdf136",{"heading":131,"kind":13,"items":132},"MO 2p ordering",[133],{"ref":134,"mode":19,"provenance":20,"text":136,"source_hash":137},{"type":17,"topic":7,"id":135,"field":17},"MS-R014","For B₂, C₂, N₂ (and CO), s-p mixing puts π₂p BELOW σ₂p. For O₂, F₂, Ne₂ the order is conventional: σ₂p below π₂p.","b976fa01d95f00b72faa5257797cda7d254013a9a662bcd8143b47bcb7ac66a0",{"heading":139,"kind":13,"items":140},"Magnetism",[141],{"ref":142,"mode":19,"provenance":20,"text":144,"source_hash":145},{"type":17,"topic":7,"id":143,"field":17},"MS-R015","All electrons paired → diamagnetic (weakly repelled). Any unpaired electron → paramagnetic (attracted). O₂ has 2 unpaired electrons in π*₂p → paramagnetic.","15359ab52a904b0cd4ac1989b32a044f71065b0302b7d47b9d8b0f4f09b15593",1787246033217]