Chemistry:The central science, plus MasteringChemistry with Pearson eText
Samenvatting levende chemie (cursus over atomen, lewisstructuren, 3D vorm van moleculen, isomeren en conformaties, polariteit, intermoleculaire krachten, koolwaterstoffen en hun naamgeving, bi0moleculen, zure en basische eigenschappen, en groene chemie)
Inhoud
Atoom...............................................................................................................................................3
Atoommodel en isotopen...................................................................................................................3
Atoomnotatie.....................................................................................................................................3
Ionen en lading...................................................................................................................................3
Valentie-elektronen............................................................................................................................4
Hoe zwaar is een atoom.....................................................................................................................4
Benaming groepen periodiek systeem en belangrijkste atomen........................................................4
Edelgasconfiguratie en octetregel......................................................................................................4
Covalente binding en ionogene binding.............................................................................................4
Standaardkleuren elementen.............................................................................................................5
Lewisstructuur...................................................................................................................................5
Wat is een lewisstructuur...................................................................................................................5
Vrije elektronen..................................................................................................................................5
Gebruik van de octetregel om lewisstructuren te maken:.................................................................5
3D vorm van moleculen.....................................................................................................................5
Elektrondomeinen..............................................................................................................................5
Elektrondomein geometrie vs moleculaire geometrie.......................................................................5
Bindingshoek bepalen........................................................................................................................6
Verschillende weergaves van molecule.............................................................................................6
Molecuulformule................................................................................................................................6
Condensed..........................................................................................................................................6
Fully displayed lewisstructuur............................................................................................................6
Condesed and skeletal Space-filling model (water)............................................................................6
Primair, secundair tertiair...................................................................................................................6
Isomeren en conformaties.................................................................................................................7
Conformaties......................................................................................................................................7
Structuurisomeren..............................................................................................................................7
Stereo-isomeren.................................................................................................................................7
Polariteit...........................................................................................................................................8
Dipoolmoment...................................................................................................................................8
Vuistregel polariteit............................................................................................................................8
Netto- dipoolmoment.........................................................................................................................8
Bepalen of een molecuul polair is: aanpak.........................................................................................9
Log P...................................................................................................................................................9
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,Intermoleculaire krachten.................................................................................................................9
London dispersiekrachten..................................................................................................................9
Dipool-dipoolinteracties...................................................................................................................10
Waterstofbruggen............................................................................................................................10
Koolwaterstoffen en hun naamgeving.............................................................................................10
Alkanen, alkenen en alkynen............................................................................................................10
Onvertakte alkanen..........................................................................................................................10
Naamgeving......................................................................................................................................10
Belangrijkste eigenschappen verbindingen/groepen:......................................................................12
Zure en basische eigenschappen.....................................................................................................12
Biomoleculen...................................................................................................................................14
Waarom de biomoleculen RNA, DNA, eiwitten, (fosfo)lipiden, sachariden een specifieke
macromoleculaire structuur aannemen...........................................................................................14
Structuurformules biomoleculen......................................................................................................14
Reactievergelijking fotosynthese etc................................................................................................15
Samenstelling van aardolie en biomassa..........................................................................................15
Bijlage belangrijke moleculen..........................................................................................................16
Groene chemie................................................................................................................................18
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, Samenvatting levende chemie
Atoom
Atoommodel en isotopen
Elektronen zitten in gekwantificeerde banen (orbits) om de kern (nucleus) heen. Hoe verder een
elektron is verwijderd van de kern, des te meer energie dit elektron heeft. Het massagetal is het
aantal protonen + het aantal neutronen
Lading Massa Plaats in atoom Berekenen/ zien in
periodiek systeem
Proton +1 1 Kern Atoomnummer
Neutron 0 1 Kern Massagetal- p
Elektron -1 0 Orbits/ elektronenschillen p- lading
Isotopen: hebben evenveel protonen maar een verschillend aantal neutronen. Dit betekent dat de
molaire massa van een element in het periodiek systeem een gemiddelde is van alle isotopen.
Isotopen gedragen zich chemisch identiek.
Atoomnotatie
Ionen en lading
- Positief geladen ion (kation) meer protonen dan elektronen ( voorbeeld: H +). Hebben
elektronen afgestaan
- Negatief geladen ion (anion) meer elektronen dan protonen (voorbeeld: Cl -). Hebben
elektronen opgenomen
Lading
De ion ladingen van de elementen kunnen in het periodiek systeem worden afgelezen: rechts boven
in de hokjes staat de lading. Om de lading van een ion te kunnen voorspellen dien je de plek in het
periodieksysteem te weten. Vanuit hier kijk je naar hoeveel plekken deze is verwijderd van de
dichtstbijzijnde edelgas. Het verschil in positie is de lading. Als een ion een metaal is, is de lading
positief en als het een niet-metaal is, is de lading negatief.
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