Algemene Chemie
Inhoud
Hoofdstuk 1: experimenteren en meten ................................................................ 5
-> 1.1 Metrologie ................................................................................................... 5
-> 1.2 Belangrijke begrippen:.................................................................................. 6
-> 1.3 Beduidende cijfers ....................................................................................... 6
Hoofdstuk 2: Atomen, moleculen en ionen ........................................................... 7
-> 2.1 Elementen en Periodiek tabel van Mendeljev ................................................. 7
-> 2.2 Atoomtheorie van Dalton.............................................................................. 9
-> 2.3 Atomische structuren .................................................................................. 9
-> 2.4 Atoomnummer .......................................................................................... 10
-> 2.4 Chemische vs Nucleaire reacties ................................................................ 10
-> 2.5 Radioactiviteit ........................................................................................... 11
-> 2.6 Covalente vs ionaire bindingen ................................................................... 12
-> 2.7 Naamgeving .............................................................................................. 12
Hoofdstuk 3: Massaverhouding in chemische reacties ........................................ 13
-> 3.1 Chemie voorstellen op verschillende levels ................................................. 13
-> 3.2 Stoichiometrie ........................................................................................... 13
Hoofdstuk 4: Reacties in waterig milieu .............................................................. 15
-> 4.1 Concentraties............................................................................................ 15
-> 4.2 Elektrolyten in waterige oplossing ............................................................... 15
-> 4.3 Soorten reactiestypes ................................................................................ 17
Hoofdstuk 5: De elektronische structuur van atomen .......................................... 20
-> 5.1 Elektromagnetisch spectrm ........................................................................ 20
-> 5.2 Waaruit bestaat elektromagnetische golven? ............................................... 21
-> 5.3 Atoommodellen ......................................................................................... 21
Hoofdstuk 6: Ionaire verbindingen en periodiciteit .............................................. 24
-> 6.1 Elektronenconfiguraties ............................................................................. 24
-> 6.2 Ionenstralen .............................................................................................. 24
-> 6.3 Elektronenaffiniteit .................................................................................... 25
,Hoofdstuk 7: Covalente bindingen en Lewisstructuur .......................................... 26
-> 7.1 Covalente bindingen .................................................................................. 26
-> 7.2 Elektonegativiteit ....................................................................................... 27
-> 7.4 Lewisstructuur: ......................................................................................... 28
HFST 8: Covalente Bindingen en Moleculaire Structuur ....................................... 31
-> 8.1 VSEPR-model ............................................................................................ 31
-> 8.2 Valence bond theorie ................................................................................. 32
-> 8.3 Polariteit en dipool ..................................................................................... 33
-> 8.4 INTERMOLECULAIRE KRACHTEN ................................................................ 34
HFST 9 Thermochemie: chemische energie......................................................... 36
-> 9.1 Soorten energie ......................................................................................... 36
-> 9.2 ENERGIE EN ENTHALPIE ............................................................................ 37
-> 9.3 Enthalpieveranderingen in chemische processen:........................................ 37
-> 9.4 Entropie .................................................................................................... 39
Hoofdstuk 10: Gassen, eigenschappen en gedrag................................................ 40
-> 10.1 Gassen en druk ........................................................................................ 40
-> 10.2 De gaswetten ........................................................................................... 40
-> 10.2.2 De ideale gas-wet.................................................................................. 41
-> 10.3 Partieeldruk ............................................................................................. 41
Hoofdstuk 11: Vloeistoffen, vaste stoffen en faseovergangen .............................. 42
-> 11.1 Faseovergangen ....................................................................................... 42
-> 11.2 Verdampen en koken ................................................................................ 43
-> 11.3 Vaste stoffen ........................................................................................... 44
-> 11.4 Fasediagrammen ..................................................................................... 46
Hoofdstuk 12: Oplossingen en hun eigenschappen! ............................................ 47
-> 12.1 oplossingen ............................................................................................. 47
-> 12.2 Oplossen................................................................................................. 47
-> 12.3 oplosbaarheid ......................................................................................... 49
-> 12.4 Vier colligatieve eigenschappen ................................................................ 49
,Hoofdstuk 13: Kinetiek ....................................................................................... 52
-> 13.1 Reactiesnelheid ....................................................................................... 52
-> 13.2 Reactie-orde ........................................................................................... 52
-> 13.3 Halfwaardetijd ......................................................................................... 53
-> 13.4 Arrheniusvergelijking ................................................................................ 53
-> 13.5 Katalyse .................................................................................................. 54
Hoofdstuk 14: Chemisch evenwicht ................................................................... 56
-> 14.1 Evenwicht ............................................................................................... 56
-> 14.2 Evenwichtconstante ................................................................................ 57
-> 14.3 Het principe van Le Chatelier .................................................................... 60
-> 14.4 Snelheid vs evenwicht .............................................................................. 61
Hoofdstuk 15: Zuren en Basen ............................................................................ 63
-> 15.1 Zuren en basen ........................................................................................ 63
-> 15.2 Gehydrateerde protonen........................................................................... 65
-> 15.3 Dissociatie van water ............................................................................... 66
-> 15.4 De pH-schaal .......................................................................................... 66
-> 15.6 Verband tussen Ka en Kb ............................................................................ 70
-> 15.7 Zouten .................................................................................................... 70
Hoofdstuk 16: Evenwichten in waterige oplossingen ........................................... 72
-> 16.1 Gemeenschappelijk ion ............................................................................ 72
-> 16.2 Buffers .................................................................................................... 72
-> 16.3 Henderson-Hasselbalch........................................................................... 73
-> 16.4 Titraties ................................................................................................... 73
-> 16.5 Titratie sterk zuur + sterke base ................................................................. 74
-> 16.6 Titratie van zwak zuur met sterke base ....................................................... 75
-> 16.7 Titratie van zwakke base met sterk zuur ..................................................... 77
-> 16.8 Titratie van polyprotisch zuur met sterk base.............................................. 77
-> 16.9 Oplosbaarheidproduct ............................................................................. 79
Hoofdstuk 17 Thermodynamica: Entropie, Vrije Energie en Evenwicht .................. 81
-> 17.1 Spontane processen ................................................................................ 81
-> 17.2 Entropie .................................................................................................. 82
-> 17.3 Vrije energie G ......................................................................................... 84
, -> 17.4 Evenwicht................................................................................................ 85
Hoofdstuk 18: Elektrochemie ............................................................................. 87
-> 18.1 Redox-reacties ........................................................................................ 87
-> 18.2 Elektrochemie ......................................................................................... 88
-> 18.3 Galvanische cel ....................................................................................... 89
-> 18.4 Celpotentiaal........................................................................................... 91
-> 18.5 Reductiepotentiaal .................................................................................. 92
-> 18.6 Nernst-vergelijking ................................................................................... 93
-> 18.7 Evenwicht................................................................................................ 94
! belangrijke dingen die terug komen !
• l = vloeistof
• s = vaste stof
• g = gas
R=8,314 J/(mol·K)
R=0,0821 L·atm/(mol·K)
amfolyt = zuur en base
° = standaardomstandigheden
• = Temperatuur van 25°
• = concentratie van 1M
• = Druk van 1atm
• = vloeistoffen en vaste stoffen in hun pure vorm
pH op 2 decimalen
bijna alle reacties zijn evenwichtreacties (evenwichtpijl gebruiken) buiten sommige
redox-reacties die heel groot zijn
Inhoud
Hoofdstuk 1: experimenteren en meten ................................................................ 5
-> 1.1 Metrologie ................................................................................................... 5
-> 1.2 Belangrijke begrippen:.................................................................................. 6
-> 1.3 Beduidende cijfers ....................................................................................... 6
Hoofdstuk 2: Atomen, moleculen en ionen ........................................................... 7
-> 2.1 Elementen en Periodiek tabel van Mendeljev ................................................. 7
-> 2.2 Atoomtheorie van Dalton.............................................................................. 9
-> 2.3 Atomische structuren .................................................................................. 9
-> 2.4 Atoomnummer .......................................................................................... 10
-> 2.4 Chemische vs Nucleaire reacties ................................................................ 10
-> 2.5 Radioactiviteit ........................................................................................... 11
-> 2.6 Covalente vs ionaire bindingen ................................................................... 12
-> 2.7 Naamgeving .............................................................................................. 12
Hoofdstuk 3: Massaverhouding in chemische reacties ........................................ 13
-> 3.1 Chemie voorstellen op verschillende levels ................................................. 13
-> 3.2 Stoichiometrie ........................................................................................... 13
Hoofdstuk 4: Reacties in waterig milieu .............................................................. 15
-> 4.1 Concentraties............................................................................................ 15
-> 4.2 Elektrolyten in waterige oplossing ............................................................... 15
-> 4.3 Soorten reactiestypes ................................................................................ 17
Hoofdstuk 5: De elektronische structuur van atomen .......................................... 20
-> 5.1 Elektromagnetisch spectrm ........................................................................ 20
-> 5.2 Waaruit bestaat elektromagnetische golven? ............................................... 21
-> 5.3 Atoommodellen ......................................................................................... 21
Hoofdstuk 6: Ionaire verbindingen en periodiciteit .............................................. 24
-> 6.1 Elektronenconfiguraties ............................................................................. 24
-> 6.2 Ionenstralen .............................................................................................. 24
-> 6.3 Elektronenaffiniteit .................................................................................... 25
,Hoofdstuk 7: Covalente bindingen en Lewisstructuur .......................................... 26
-> 7.1 Covalente bindingen .................................................................................. 26
-> 7.2 Elektonegativiteit ....................................................................................... 27
-> 7.4 Lewisstructuur: ......................................................................................... 28
HFST 8: Covalente Bindingen en Moleculaire Structuur ....................................... 31
-> 8.1 VSEPR-model ............................................................................................ 31
-> 8.2 Valence bond theorie ................................................................................. 32
-> 8.3 Polariteit en dipool ..................................................................................... 33
-> 8.4 INTERMOLECULAIRE KRACHTEN ................................................................ 34
HFST 9 Thermochemie: chemische energie......................................................... 36
-> 9.1 Soorten energie ......................................................................................... 36
-> 9.2 ENERGIE EN ENTHALPIE ............................................................................ 37
-> 9.3 Enthalpieveranderingen in chemische processen:........................................ 37
-> 9.4 Entropie .................................................................................................... 39
Hoofdstuk 10: Gassen, eigenschappen en gedrag................................................ 40
-> 10.1 Gassen en druk ........................................................................................ 40
-> 10.2 De gaswetten ........................................................................................... 40
-> 10.2.2 De ideale gas-wet.................................................................................. 41
-> 10.3 Partieeldruk ............................................................................................. 41
Hoofdstuk 11: Vloeistoffen, vaste stoffen en faseovergangen .............................. 42
-> 11.1 Faseovergangen ....................................................................................... 42
-> 11.2 Verdampen en koken ................................................................................ 43
-> 11.3 Vaste stoffen ........................................................................................... 44
-> 11.4 Fasediagrammen ..................................................................................... 46
Hoofdstuk 12: Oplossingen en hun eigenschappen! ............................................ 47
-> 12.1 oplossingen ............................................................................................. 47
-> 12.2 Oplossen................................................................................................. 47
-> 12.3 oplosbaarheid ......................................................................................... 49
-> 12.4 Vier colligatieve eigenschappen ................................................................ 49
,Hoofdstuk 13: Kinetiek ....................................................................................... 52
-> 13.1 Reactiesnelheid ....................................................................................... 52
-> 13.2 Reactie-orde ........................................................................................... 52
-> 13.3 Halfwaardetijd ......................................................................................... 53
-> 13.4 Arrheniusvergelijking ................................................................................ 53
-> 13.5 Katalyse .................................................................................................. 54
Hoofdstuk 14: Chemisch evenwicht ................................................................... 56
-> 14.1 Evenwicht ............................................................................................... 56
-> 14.2 Evenwichtconstante ................................................................................ 57
-> 14.3 Het principe van Le Chatelier .................................................................... 60
-> 14.4 Snelheid vs evenwicht .............................................................................. 61
Hoofdstuk 15: Zuren en Basen ............................................................................ 63
-> 15.1 Zuren en basen ........................................................................................ 63
-> 15.2 Gehydrateerde protonen........................................................................... 65
-> 15.3 Dissociatie van water ............................................................................... 66
-> 15.4 De pH-schaal .......................................................................................... 66
-> 15.6 Verband tussen Ka en Kb ............................................................................ 70
-> 15.7 Zouten .................................................................................................... 70
Hoofdstuk 16: Evenwichten in waterige oplossingen ........................................... 72
-> 16.1 Gemeenschappelijk ion ............................................................................ 72
-> 16.2 Buffers .................................................................................................... 72
-> 16.3 Henderson-Hasselbalch........................................................................... 73
-> 16.4 Titraties ................................................................................................... 73
-> 16.5 Titratie sterk zuur + sterke base ................................................................. 74
-> 16.6 Titratie van zwak zuur met sterke base ....................................................... 75
-> 16.7 Titratie van zwakke base met sterk zuur ..................................................... 77
-> 16.8 Titratie van polyprotisch zuur met sterk base.............................................. 77
-> 16.9 Oplosbaarheidproduct ............................................................................. 79
Hoofdstuk 17 Thermodynamica: Entropie, Vrije Energie en Evenwicht .................. 81
-> 17.1 Spontane processen ................................................................................ 81
-> 17.2 Entropie .................................................................................................. 82
-> 17.3 Vrije energie G ......................................................................................... 84
, -> 17.4 Evenwicht................................................................................................ 85
Hoofdstuk 18: Elektrochemie ............................................................................. 87
-> 18.1 Redox-reacties ........................................................................................ 87
-> 18.2 Elektrochemie ......................................................................................... 88
-> 18.3 Galvanische cel ....................................................................................... 89
-> 18.4 Celpotentiaal........................................................................................... 91
-> 18.5 Reductiepotentiaal .................................................................................. 92
-> 18.6 Nernst-vergelijking ................................................................................... 93
-> 18.7 Evenwicht................................................................................................ 94
! belangrijke dingen die terug komen !
• l = vloeistof
• s = vaste stof
• g = gas
R=8,314 J/(mol·K)
R=0,0821 L·atm/(mol·K)
amfolyt = zuur en base
° = standaardomstandigheden
• = Temperatuur van 25°
• = concentratie van 1M
• = Druk van 1atm
• = vloeistoffen en vaste stoffen in hun pure vorm
pH op 2 decimalen
bijna alle reacties zijn evenwichtreacties (evenwichtpijl gebruiken) buiten sommige
redox-reacties die heel groot zijn
