[{"data":1,"prerenderedAt":167},["ShallowReactive",2],{"cheatsheet-intermolecular-forces-and-phase-changes":3},{"sheet":4},{"sheetSlug":5,"topicSlugs":6,"primaryTopic":7,"title":8,"subtitle":9,"sections":10},"intermolecular-forces-and-phase-changes",[5],18,"Intermolecular Forces & Phase Changes","Identifying IMFs, their trends, phase transitions and diagrams, heating curves, and crystalline solids.",[11,23,33,66,74,82,91,99,127,135,159],{"heading":12,"kind":13,"items":14},"Identify the main IMF","steps",[15],{"ref":16,"mode":19,"provenance":20,"text":21,"source_hash":22},{"type":17,"topic":7,"id":18,"field":17},"rule","LS-R006","transform","owned_workbook","Ionic solid → ionic attraction; ionic dissolved → ion-dipole. Polar molecule with H on F/O/N → hydrogen bonding; other polar → dipole-dipole; nonpolar → London dispersion (present in all). Geometry sets polarity: symmetric polar bonds cancel (nonpolar); a lone pair on the central atom breaks symmetry (polar).","501f0759253aaa0a3ee59397ca4011b922372bf4d3528b0133aad1fcadb6c19e",{"heading":24,"kind":25,"items":26},"IMF strength & properties","rules",[27],{"ref":28,"mode":19,"provenance":30,"text":31,"source_hash":32},{"type":17,"topic":7,"id":29,"field":17},"LS-R008","original","Ionic > hydrogen bonding > dipole-dipole > dispersion (at similar size). But a big polarizable nonpolar molecule can beat a small polar one (I₂ > HCl). Stronger IMF → higher boiling point, viscosity, surface tension; lower vapor pressure.","29ead18ff97cb81835545129cf23d2e0d77060fd7ba3b67ca1d6cee5aeeed4a6",{"heading":34,"kind":35,"columns":36,"items":40},"Phase transitions","data",[37,38,39],"Transition","Name","Heat",[41],{"ref":42,"mode":19,"provenance":20,"rows":44,"source_hash":65},{"type":17,"topic":7,"id":43,"field":17},"LS-R010",[45,49,53,56,59,62],[46,47,48],"solid → liquid","melting","endo",[50,51,52],"liquid → solid","freezing","exo",[54,55,48],"liquid → gas","vaporization",[57,58,52],"gas → liquid","condensation",[60,61,48],"solid → gas","sublimation",[63,64,52],"gas → solid","deposition","dbaedfc71bd7d7ff18916494ad65c0b84f7979aa311332c63734cbaddcedc0d4",{"heading":67,"kind":25,"items":68},"Temperature is flat during a phase change",[69],{"ref":70,"mode":19,"provenance":20,"text":72,"source_hash":73},{"type":17,"topic":7,"id":71,"field":17},"LS-R005","During a phase change T stays constant: heat changes potential energy (breaking/forming IMFs), not kinetic. Phase change: Q = ΔH × moles (ΔH_fus or ΔH_vap). Within one phase: Q = m·s·ΔT.","6f1659330c6417a795dc95db88e8ae2070d8322c634bb7b512124d3089153759",{"heading":75,"kind":13,"items":76},"Water heating curve (per mole/gram)",[77],{"ref":78,"mode":19,"provenance":20,"text":80,"source_hash":81},{"type":17,"topic":7,"id":79,"field":17},"LS-R004","Up to 5 steps: warm ice (s = 2.09 J/g·°C) → melt at 0 °C (6.02 kJ/mol) → warm water (4.18) → boil at 100 °C (40.7 kJ/mol) → warm steam (1.84). Sum only the segments the path crosses; convert mass → moles (÷ 18.015) for the ΔH steps.","291ece69d5c0f8d914338285a758b73499b860a1feacc710e22eaed05eef6208",{"heading":83,"kind":84,"items":85},"Non-water substances","pitfalls",[86],{"ref":87,"mode":19,"provenance":30,"text":89,"source_hash":90},{"type":17,"topic":7,"id":88,"field":17},"LS-R013","Use the water defaults (ΔH_fus 6.02, ΔH_vap 40.7 kJ/mol) ONLY for water. For any other substance, take its own ΔH_fus, ΔH_vap, and specific heats from the problem; all constants must match the named substance.","f882ade116e81ddd6bdf713b4e2a9038e22e6d8baa7f3032a40a770886722db4",{"heading":92,"kind":25,"items":93},"Phase diagram",[94],{"ref":95,"mode":19,"provenance":20,"text":97,"source_hash":98},{"type":17,"topic":7,"id":96,"field":17},"LS-R009","Regions: solid (low T, high P), liquid (middle), gas (high T, low P). Lines = two phases coexist. Triple point: all three coexist. Critical point: end of the liquid-gas line (supercritical beyond). Normal boiling point: liquid-gas line at 1 atm.","35f037ce840b60181ed31fdd4ad657aa111a384f70df81970b7b9005ad80a0c5",{"heading":100,"kind":35,"columns":101,"items":105},"Crystalline solids",[102,103,104],"Type","Bonding","Properties",[106],{"ref":107,"mode":19,"provenance":30,"rows":109,"source_hash":126},{"type":17,"topic":7,"id":108,"field":17},"LS-R011",[110,114,118,122],[111,112,113],"Ionic","ion attractions","hard, brittle; conducts only molten/dissolved; high MP",[115,116,117],"Metallic","electron sea","shiny, malleable; conducts; variable MP",[119,120,121],"Covalent network","3D covalent","very hard; insulator; very high MP",[123,124,125],"Molecular","IMFs","soft; insulator; low MP","7bb376fdbbb293fae8445e737df486fa89d364f148875c153c33e1e661b7c6a4",{"heading":128,"kind":25,"items":129},"Unit-cell density",[130],{"ref":131,"mode":19,"provenance":20,"text":133,"source_hash":134},{"type":17,"topic":7,"id":132,"field":17},"LS-R001","ρ = n·M / (N_A·a³), n = atoms per cell (SC 1, BCC 2, FCC 4). Convert edge a from pm to cm first (1 pm = 10⁻¹⁰ cm) for ρ in g/cm³. Rearrange to solve for a, M, or n.","02b401bfab7e4931ccd058cc025419d8108df7ea51bb715a5295294b0a5ae132",{"heading":136,"kind":35,"columns":137,"items":141},"Atomic radius by cell type",[138,139,140],"Cell","Atoms/cell","Radius",[142],{"ref":143,"mode":19,"provenance":20,"rows":145,"source_hash":158},{"type":17,"topic":7,"id":144,"field":17},"LS-R003",[146,150,154],[147,148,149],"SC","1","r = a/2",[151,152,153],"BCC","2","r = a√3/4",[155,156,157],"FCC","4","r = a√2/4","6a178515f7881c39f0f93e4ed85e3dd3b033f83028a7b4488b0c8271b2f47d48",{"heading":160,"kind":25,"items":161},"Identify the element",[162],{"ref":163,"mode":19,"provenance":20,"text":165,"source_hash":166},{"type":17,"topic":7,"id":164,"field":17},"LS-R014","After computing M from density + cell data, match within ±0.5 g/mol of the tabulated mass AND confirm the crystal structure. Near-mass elements need the cell-type check: Co (58.93, hcp) and Ni (58.69, fcc) differ by only ~0.24 g/mol, so structure is what distinguishes them.","b29481ae1f4e7e1660d4815849ba813b960a0e5298fd18af6af2f2f202b9328f",1787246033490]