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Samenvatting Anorganische Chemie Theorie

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Course
Anorganische Chemie (V3A726)

Institution
Katholieke Hogeschool VIVES (VIVES)

Anorganische chemie 1ste jaar Bachelor Agro - en Biotechnologie deel theorie is een vak op zich. Hiervan is een samenvatting gemaakt van alle theorie die wordt behandeld in het eerste semester. Het eerste deel van Anorganische chemie is zeer algemeen. Met behulp van deze samenvatting was ik gesla...

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anorganische chemie
chemie
2019
2020
biotechnologie
vives

Institution
Katholieke Hogeschool VIVES (VIVES)
Education
Agro-en Biotechnologie
Course
Anorganische Chemie (V3A726)

matissem

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ANORGANISCHE CHEMIE
INHOUD

Hoofdstuk 1: Structuuraspecten van de materie ........................................................................................................... 6
1. Atomen en moleculen ......................................................................................................................................... 6
1.1 Samenstelling van een atoom ............................................................................................................................. 6
1.2 Atoomnummer (Z) en Massanummer (A) ........................................................................................................... 7
1.3 Isotopen .............................................................................................................................................................. 9
1.4 Relatieve atoommassa (RAM) ........................................................................................................................... 10
1.5 Relatieve molecuulmassa (RMM) ..................................................................................................................... 10
1.6 Mol en Molaire massa ....................................................................................................................................... 10
2. Elektronen in schillen en orbitalen ....................................................................................................................... 11
2.1 Visie van Bohr.................................................................................................................................................... 11
2.2 Moderne atoomtheorie .................................................................................................................................... 11
2.3 Elektronenconfiguratie ..................................................................................................................................... 14
Voorstelling elektronenconfiguratie ........................................................................................................................ 15
2.4 Inversie 15
2.5 Elektronenconfiguratie en periodiek systeem .................................................................................................. 16
Hoofdstuk 3: Chemische binding ................................................................................................................................. 17
1) Ionbinding ......................................................................................................................................................... 17
3.1 Definitie van een ionbinding ............................................................................................................................. 18
3.2 Schrijven ionbinding .......................................................................................................................................... 18
Kationen, positief geladen iongroepen .................................................................................................................... 18
Anionen en negatief geladen iongroepen ................................................................................................................ 19
2.6 Stoichiometrische of samengestelde namen .................................................................................................... 20
2.7 Mechanisme van de vorming van een ionbinding ............................................................................................ 21
1ste ionisatie – energie .............................................................................................................................................. 22
2de ionisatie – energie ............................................................................................................................................. 22
3de ionisatie – energie ............................................................................................................................................. 22
Elektronenaffiniteit (stap 4) ..................................................................................................................................... 23
2) Covalente binding ................................................................................................................................................. 24
Voorstelling covalente binding ................................................................................................................................. 25
Soorten covalente bindingen ................................................................................................................................... 25
Formele lading (goed kennen) ................................................................................................................................. 26
Bepaling Lewisformule ............................................................................................................................................. 27
Stappenplan voor Lewis formule.......................................................................................................................... 27
Resonantie (mesomerie) .......................................................................................................................................... 28

, Elektronennegativiteit (EN) – Polariteit van covalente binding ............................................................................... 29
Het begrip Elektronennegativiteit (examen) ........................................................................................................ 29
V.S.E.P.R. – theorie ................................................................................................................................................... 30
Voorbeelden: ........................................................................................................................................................... 33
Hybridisatie .................................................................................................................................................................. 35
Sp - Sp2 – Sp3 ................................................................................................................................................................. 36
Sp3d – sp3d2 .................................................................................................................................................................. 37
Hybridisatie dubbele en driedubbele binding .............................................................................................................. 39
Polariteit van covalente moleculen .............................................................................................................................. 40
Radicalen ...................................................................................................................................................................... 41
Stappen van radicaal reacties .................................................................................................................................. 41
Toepassingen radicalen ............................................................................................................................................ 41
Metaalbinding .............................................................................................................................................................. 42
Krachten en bindingen tussen en in moleculen ........................................................................................................... 42
In een molecule: intermoleculaire krachten ............................................................................................................ 42
Tussen moleculen: intermoleculaire krachten ............................................................................................................. 43
Hoofdstuk 4: Chemische functies ................................................................................................................................. 44
Zuurfunctie (zuren) .................................................................................................................................................. 44
Binaire zuren ........................................................................................................................................................ 44
Oxozuren of ternaire zuren .................................................................................................................................. 44
Toepassingen van zuren ....................................................................................................................................... 45
Basenfunctie (basen) ................................................................................................................................................ 45
Hydroxidebasen ................................................................................................................................................... 45
Aminebasen.......................................................................................................................................................... 45
Toepassingen van basen ...................................................................................................................................... 45
Zoutfunctie ............................................................................................................................................................... 46
Toepassingen zouten............................................................................................................................................ 46
Oxiden ...................................................................................................................................................................... 46
Zure oxiden........................................................................................................................................................... 46
Basische oxiden .................................................................................................................................................... 46
Amfotere oxiden .................................................................................................................................................. 47
Toepassingen oxiden ............................................................................................................................................ 47
Belangrijke kenmerken van verbindingen ................................................................................................................ 47
Sterke elektrolyten ............................................................................................................................................... 47
Zwakke elektrolyten ............................................................................................................................................. 48
Ionisatiegraad ....................................................................................................................................................... 48
Lijst met belangrijkste zuren en afgeleide zuurresten ............................................................................................. 49

,Chemische reacties ...................................................................................................................................................... 50
Zuurbasereacties ...................................................................................................................................................... 50
Reactie van een zuur met een base ..................................................................................................................... 50
Reactie van een zuur oxide met een base ............................................................................................................ 51
Reactie van een basisch oxide met een zuur ....................................................................................................... 51
Reactie met amfotere oxiden met zuren of basen............................................................................................... 51
Sterkzuur verdrijft een zwakzuur uit zijn zout...................................................................................................... 52
Sterke base verdrijft een zwakke base uit haar zout ........................................................................................... 52
Neerslagreactie ........................................................................................................................................................ 52
Oxidatiereductiereacties .......................................................................................................................................... 53
Oxidatiegetal ........................................................................................................................................................ 53
Hoe een oxidatie reductie reactie neerschrijven? ................................................................................................... 54
1. Oxidatiegetal veranderingen ......................................................................................................................... 54
2. Vereenvoudigde reactievergelijking ............................................................................................................. 54
3. Elektronentransfer ........................................................................................................................................ 54
4. Elektronenbalans .......................................................................................................................................... 54
5. Ladingsbalans ................................................................................................................................................ 55
6. Zuurstof – en waterstofbalans ...................................................................................................................... 55
7. Molecuulbalans ............................................................................................................................................. 55
Stoichiometrie .............................................................................................................................................................. 56
Uitdrukken van concentratie.................................................................................................................................... 56
Massa /Volume procent ....................................................................................................................................... 56
Molariteit (CN) ......................................................................................................................................................... 56
Normaliteit ............................................................................................................................................................... 57
Gramequivalent in zuur – basereacties ................................................................................................................ 57
Gramequivalent in redoxreacties ......................................................................................................................... 58
Volume / volume procent ........................................................................................................................................ 58
Concentratie uitdrukken in mol-eenheden .............................................................................................................. 58
Kwantitatieve oefeningen reactievergelijkingen.................................................................................................. 58
Reacties in oplossing ................................................................................................................................................ 59
Redoxreacties ....................................................................................................................................................... 59
Chemisch evenwicht .................................................................................................................................................... 60
Kc – waarde .............................................................................................................................................................. 60
Algemeen ............................................................................................................................................................. 60
Factoren die chemisch evenwicht beïnvloeden ....................................................................................................... 60
Toevoegen of wegnemen een van de reactiepartners ........................................................................................ 60
Verdunning van een oplossing ............................................................................................................................. 61

, Verandering van druk ........................................................................................................................................... 61
Invloed van temperatuur op het evenwicht ........................................................................................................ 61
Invloed van katalysator ........................................................................................................................................ 61
Homogene evenwichten in water ................................................................................................................................ 62
Waterconstante Kw.................................................................................................................................................. 62
Waterstof exponent pH............................................................................................................................................ 62
Protolysereacties met water .................................................................................................................................... 63
Zuur base reacties ................................................................................................................................................ 63
Zuurconstante .......................................................................................................................................................... 64
Baseconstante .......................................................................................................................................................... 65
Richting van zuur – base reactie........................................................................................................................... 65
Buffermengsels ........................................................................................................................................................ 65
Zuur base titratie ...................................................................................................................................................... 67
Heterogene evenwichten in water............................................................................................................................... 67
Oplosbaarheid .......................................................................................................................................................... 67
Oplosbaarheidsproduct ............................................................................................................................................ 67
Toepassingen homogene en heterogene evenwichten in grotten .......................................................................... 69
Reactiesnelheid ............................................................................................................................................................ 70
Nulde orde reactie ................................................................................................................................................... 70
Eerste orde reactie ................................................................................................................................................... 71
Activatie – energie ................................................................................................................................................... 72
Snelheid en temperatuur ..................................................................................................................................... 72
Katalyse ................................................................................................................................................................ 73
Kernchemie .................................................................................................................................................................. 74
Aard en eigenschappen van radioactieve straling ................................................................................................... 74
Soorten ladingen .................................................................................................................................................. 74
Alfa straling .......................................................................................................................................................... 75
Bèta straling ......................................................................................................................................................... 75
Gamma straling .................................................................................................................................................... 75
Neutrino’s............................................................................................................................................................. 75
Desintegratiesnelheid – halveringstijd ..................................................................................................................... 76
Atoomkernen eigenschappen .................................................................................................................................. 78
Isotopenverdeling ................................................................................................................................................ 78
Stabiliteit .............................................................................................................................................................. 78
Kernsplijting en kernversmelting ............................................................................................................................. 79
Splijting of fissie ................................................................................................................................................... 79
Versmelting of fusie ............................................................................................................................................. 79

, Dosisequivalent (Sievert) ..................................................................................................................................... 80
Detectie en meting radioactiviteit ........................................................................................................................... 80
Ionisatie van gassen: Geiger Muller teller ............................................................................................................ 80
Toepassingen............................................................................................................................................................ 81
Splijtingsbommen ................................................................................................................................................. 81
Elektrische centrales ............................................................................................................................................ 81
Ouderdomsbepaling Koolstof 14 – methode ....................................................................................................... 82
Toepassingen in natuurwetenschappen .................................................................................................................. 82
Activeringsanalyse ................................................................................................................................................ 82
sterilisatie ............................................................................................................................................................. 82
Toepassingen in geneeskunde ................................................................................................................................. 82
Radiodiagnostiek .................................................................................................................................................. 82
Nucleaire geneeskunde ........................................................................................................................................ 82
Elektrochemie .............................................................................................................................................................. 83
Galvanische cellen of elektrische cel ........................................................................................................................ 83
Vergelijking van Nernst ............................................................................................................................................ 84
Complexe ionen ........................................................................................................................................................... 84
Bidentaten ............................................................................................................................................................ 85
Chelaten ............................................................................................................................................................... 85
Toepassingen............................................................................................................................................................ 86

,HOOFDSTUK 1: STRUCTUURASPECTEN VAN DE MATERIE

1. ATOMEN EN MOLECULEN
1.1 SAMENSTELLING VAN EEN ATOOM

➔ Atoom komt van het Griekse: a-tomos = ondeelbaar
o = het kleinste deeltje waaruit een stof is opgebouwd.

Atoom:
• Elektrisch neutraal
• Voorgesteld als een kern met een grote ‘wolk’
• In de kern zitten kerndeeltjes of nucleonen
o Protonen (positief geladen +)
o Neutronen (neutraal geladen)
• Rond de kern zitten elektronen (negatief geladen -) in een ‘wolk’
• Aantal protonen = aantal elektronen

Subatomair deeltje Symbool Lading

Elektron e -1

Proton p +1

Neutron n 0

, ➔ De massa zit hoofdzakelijk in de kern
➔ Bepaalde C-atomen hebben 12 kerndeeltjes
o Eenheid van de massa= 1/12 deel van de absolute massa van koolstofatoom met 12
nucleonen
-24
o Werkelijke massa= 1,66.10 = 1/12 van C-atoom = 1unit (1u)

Subatomair Symbool Massa Massa (u)
deeltje afgerond

Elektron e 0,005 0

Proton p 1,0073 1

Neutron n 1,0087 1

1.2 ATOOMNUMMER (Z) EN MASSANUMMER (A)

➔ Atoomnummer = Aantal protonen
➔ Massanummer = Atoomnummer + aantal neutronen

Opgelet: Protonen blijven steeds gelijk. Verander je de protonen -> dan verander je van element!

• Atoom slechts gekend indien zowel aantal protonen als neutronen in de kern bekend zijn
= nuclide

Toepassing zware metalen (1, max 2 kennen)

, - Komen voor in de natuur onder de vorm van:
o Ionen
o Gebonden aan andere stof
o Opgelost in water
o Damp in atmosfeer
o Mineraal in gesteente en bodem
- Definitie: verwijst naar atoommassa of densiteit of beide
o Praktijk: blootstelling levert mogelijk gevaar op.

Naam Symbool Schadelijke effecten
Koper Cu Acute long- leverschade bij
inademing

Kwik Hg Aantasting long en
zenuwstelsel bij
inademing

Lood Lb Schade aan maag en
ingewanden,
bloedarmoede

Zink Zn Koorts bij inademen
metaaldamp
Welke symbolen te kennen?

Ac Actinum Co Kobalt P Fosfor
Al Aluminium C Koolstof Ge Germanium
Sb Antimoon Cu Koper Au Goud
Ar Argon Hg Kwik Mg Magnesium
As Arseen Li Lithium Mn Mangaan
Ba Barium Pb Lood Mo Molybdeen
Be Beryllium Ra Radium Na Natrium
Bi Bismut Rn Radon Ne Neon
B Boor Sc Scandium Ni Nikkel
Br Broom Se Seleen Pt Platina
Cd Cadmium Si Silicium Pu Plutonium
Ca Calcium N Stikstof Po Polonium
He Helium Sr Strontium Sn Tin

, Fe IJzer Cs Cesium Ti Titaan
In Indium Cl Chloor U Uranium
I Jood Cr Chroom V Vanadium
K Kalium F Fluor H Waterstof
W Wolfraam Xe Xenon Ag Zilver
Zn Zink Zr Zirkonium O Zuurstof
S Zwavel

1.3 ISOTOPEN

Isotoop = een atoom van éénzelfde en hetzelfde element, die van elkaar verschillen door het aantal neutronen.

• Isotoop afkomstig van Griekse isos (gelijk) en topos (plaats)
• Gekenmerkt door dezelfde chemische eigenschappen
• Verschillen in fysische eigenschappen

Toepassingen
1. Originefraude in plantaardige voeding opsporen
• Koolstof bij C4 planten (mais) is anders dan bij C3 planten (95% van de planten)
o Op deze manier kan men honing onderscheiden van maisstroop

2. C-14 methode voor bepaling ouderdom voorwerpen die koolstof bevatten
• C-14 methode gebruikt bij
ouderdomsbepaling
o Bepalen via massaspectrometer
• C14 onstabiel isotoop en zal terugvallen tot
N14
• De halveringstijd om C-14 tot de helft laten
terugvallen bedraagt 5730 jaar.

, 3. Uit isotopen weten wat je eet
• Door fotosynthese CO2 opgenomen uit de lucht
• Omgezet in andere stoffen (glucose)
• Planten nemen C12 meer op dan het zwaardere C13
• Mate van N15 geeft een idee over hoeveelheid van consumptie van plantaardig en dierlijk voedsel

1.4 RELATIEVE ATOOMMASSA (RAM)

• Hoeveel de massa van een bepaald atoom groter is dan de eenheid u (1.66.10-24)

Vb. Silicium (Si)

Relatieve atoommassa = 28.08

Werkelijke atoommassa = 28,08 . 1.66.10-24g

1.5 RELATIEVE MOLECUULMASSA (RMM)

• Hoeveel de massa van een molecuul groter is dan de eenheid u

Vb. Molecule H2O bestaat uit 2 atomen H en 1 atoom O

RMM (H2O) = 2 x RAM (H) + RAM (O) = (2 x 1) + 16 = 18

RMM (H2SO4) = 2 x RAM (H) + RAM (S) + 4 x RAM (O) = 2 + 32.06 + 64= 98.06

Werkelijk massa = 18 x 1.66.10-24g

1.6 MOL EN MOLAIRE MASSA

• Mol verwijst naar de hoeveelheid van een stof =
o 6.02.1023 = Getal van Avogadro

Vb. 1 Mol H2SO4 = 6.02.1023 moleculen H2SO4

Molaire massa (M)

• Stelt het aantal gram voor dat de stof bevat in 1 mol (6.02.1023 deeltjes).
o Eenheid : g/mol

Vb. Water (H2O)

RMM (H2O) = 18

Molaire massa = 18 g/mol

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Samenvatting Anorganische Chemie Theorie

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