Dit is een samenvatting van het partim algemene chemie, Cel I van prof Klaartje De Buysser.
In deze samenvatting staat alle leerstof goed uitgelegd en verwerkt, ook met genoeg afbeeldingen.
Cel I: Algemene chemie
INHOUD
1 Atomen en moleculen: basis van biologische systemen ................................................................. 4
1.1 Chemische elementen ............................................................................................................. 4
1.2 Ionen en moleculen ................................................................................................................. 5
1.3 De dipolaire binding ................................................................................................................ 5
1.3.1 Coördinatiecomplexen .................................................................................................... 5
1.3.2 Geometrie van coördinatieverbindingen ....................................................................... 6
1.3.3 complexvorming in biologische systemen ...................................................................... 6
2 Intermoleculaire krachten en gecondenseerde fasen .................................................................... 7
2.1 Types intermoleculaire krachten............................................................................................. 7
2.1.1 Dipool – dipool krachten ................................................................................................. 7
2.1.2 Londonkrachten (dispersiekrachten) .............................................................................. 7
2.1.3 Waterstofbrug ................................................................................................................. 7
2.2 Intra- en intermoleculaire interacties in biologische macromoleculen .................................. 8
2.3 Aggregatietoestanden en hun specifieke eigenschappen....................................................... 9
2.3.1 Vaste toestand................................................................................................................. 9
2.3.2 Vloeibare toestand .......................................................................................................... 9
2.3.3 Gassen ............................................................................................................................. 9
3 Oplossingen: oplosbaarheid en concentratie................................................................................ 10
3.1 Water als oplosmiddel........................................................................................................... 10
3.2 Het oplosproces..................................................................................................................... 10
3.3 Lichaamsvocht ....................................................................................................................... 10
3.4 Oplosbaarheid ....................................................................................................................... 11
3.4.1 Oplosbaarheidsproduct Ks ............................................................................................. 11
3.4.2 De oplosbaarheid S........................................................................................................ 11
3.4.3 Invloed van druk en temperatuur op oplosbaarheid .................................................... 11
3.4.4 Invloed van hydrolyse en zuurtegraad van de oplossing .............................................. 12
3.4.5 Invloed van complexvormers ........................................................................................ 12
3.4.6 Biomedische aspecten van oplosbaarheid .................................................................... 12
3.5 Concentratiegrootheden ....................................................................................................... 12
3.6 concentratie en giftigheid ..................................................................................................... 13
3.7 Essentiele elementen in het menselijk lichaam .................................................................... 13
4 Oplossing: osmose......................................................................................................................... 13
4.1 Begrip osmose ....................................................................................................................... 13
4.2 Iso-, hyper- en hypotonisch ................................................................................................... 14
4.3 Het bereiden van een fysiologische oplossing ...................................................................... 14
4.4 Osmotische eigenschappen van elektrolytoplossingen ........................................................ 14
4.5 Gibbs-Donnanevenwicht ....................................................................................................... 15
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Cel I: Algemene Chemie
4.6 Colloïden of colloïdale mengsels ........................................................................................... 15
5 Biochemische kinetiek ................................................................................................................... 16
5.1 Reactiesnelheid voor (bio)chemische deeltjes ...................................................................... 16
5.2 Invloed van de concentratie op de snelheid ......................................................................... 17
5.3 Verandering van de concentratie met de tijd ....................................................................... 17
5.4 moleculaire verklaring van de reactiesnelheid ..................................................................... 18
5.5 Invloed van temperatuur op reactiesnelheid ........................................................................ 19
5.6 Invloed van een katalysator .................................................................................................. 19
5.6.1 Natuurlijke katalysatoren of “enzymen” ....................................................................... 19
5.7 Reactiekinetiek en reactie-evenwicht ................................................................................... 20
6 Chemische reacties: energie en evenwicht ................................................................................... 20
6.1 Energie en warmte ................................................................................................................ 20
6.2 Cellen zetten één type van energie om in het andere .......................................................... 20
6.3 Calorimetrie ........................................................................................................................... 21
6.4 Wet van behoud van energie ................................................................................................ 21
6.5 Enthalpie en enthalpieverandering ∆H ................................................................................. 21
6.6 Berekening van enthalpieveranderingen .............................................................................. 22
6.7 Entropie en spontaneïteit...................................................................................................... 22
6.8 De verandering in Vrije Energie ∆G bepaalt de spontaneïteit .............................................. 22
6.9 vrije energie en chemisch evenwicht .................................................................................... 24
6.10 Chemische potentiaal ............................................................................................................ 24
6.11 Vrije energie en nuttige arbeid.............................................................................................. 24
6.12 Gekoppelde reacties.............................................................................................................. 25
7 Zuren en basen .............................................................................................................................. 25
7.1 pH .......................................................................................................................................... 25
7.1.1 Het ionenproduct van water ......................................................................................... 25
7.2 Intrinsieke zuursterkte en moleculaire structuur.................................................................. 26
7.2.1 Intrinsieke zuursterkte van covalente hydriden, H-X .................................................... 26
7.2.2 Zuursterkte van oxozuren ............................................................................................. 27
7.3 pH van sterke zuren en basen ............................................................................................... 28
7.4 pH van zwakke zuren en basen ............................................................................................. 28
7.5 pH van mengsels van zuren en basen ................................................................................... 29
7.6 pH van meerbasische zuren .................................................................................................. 29
7.7 pH van oplossingen van zouten – hydrolyse ......................................................................... 29
8 Zuurtegraad en levende materie................................................................................................... 30
8.1 Amfolyten (amfotere bestanddelen) .................................................................................... 30
8.1.1 Alkali-hydrogeniumzouten van zwakke polyzuren ........................................................ 30
8.1.2 Zuur-basegedrag van aminozuren................................................................................. 31
8.2 Bufferoplossingen.................................................................................................................. 32
8.2.1 De componenten van een buffer .................................................................................. 32
8.2.2 Werking en pH van een buffer ...................................................................................... 32
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Cel I: Algemene Chemie
8.2.3 Controle op de bufferende werking van een bufferoplossing ...................................... 32
8.2.4 Buffercapaciteit ............................................................................................................. 32
8.2.5 Gebruik van buffers in medische experimenten ........................................................... 34
9 Elektrochemie ............................................................................................................................... 34
9.1 Inleiding ................................................................................................................................. 34
9.2 Galvanisch element – Voltacel .............................................................................................. 34
9.3 Standaardreductiepotentialen – elektromotorische kracht E............................................... 35
9.4 Standaard elektromotorische kracht E° ................................................................................ 35
9.5 Elektromotorische kracht, concentratie en Gibbs vrije energie............................................ 36
9.5.1 Potentiaalbetrekking van Nernst................................................................................... 36
9.5.2 Elektrochemisch evenwicht........................................................................................... 36
9.5.3 Concentratiecellen ........................................................................................................ 36
9.5.4 Biologische concentratiecellen...................................................................................... 37
9.5.5 Standaardreductiepotentialen in biologische systemen (E°’) ....................................... 37
9.5.6 Redoxpotentialen in de mitochondriën ........................................................................ 37
9.6 Elektroforese ......................................................................................................................... 37
9.6.1 Basisprincipes ................................................................................................................ 37
9.6.2 Elektrische variabelen ................................................................................................... 38
9.6.3 Elektrokinetische potentiaal ............................................................................................... 38
9.6.4 Ionsterkte I .................................................................................................................... 38
9.6.5 pH .................................................................................................................................. 39
9.6.6 Temperatuur en viscositeit............................................................................................ 39
9.6.7 Specifieke interacties .................................................................................................... 39
9.6.8 Experimentele aspecten ................................................................................................ 39
9.6.9 Enkele elektroforesemethoden..................................................................................... 39
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, lOMoAR cPSD| 32056276
Cel I: Algemene Chemie
Metalen: hebben spontane neiging om elektronen af te geven ->
vormen kationen
Niet-metalen: nemen makkelijk elektronen op -> vormen anionen
Metalloïden: hebben eigenschappen van zowel kationen en
anionen of ergens daartussen
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