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Samenvatting Bio-organic Chemistry For Life Sciences
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Complete samenvatting van de colleges, tutorials & practicals. Gebaseerd op het boek. TE1 & TE2 ook bijgevoegd.
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lOMoARcPSD|2392027Introduction
Gedownload door Michou Weimar (michoumelody@live.nl)
, lOMoARcPSD|2392027
Lecture 1
Structure & bonding: Acids & Bases (1.1-1.12)
Key worde:
Organic chemistry -> etudy of carbon compounde
Organic chemietry
o All organic compounde contain carbon = C
o C binde to other C atome to create ringe & chaine
o Not all carbon compounde derrive from living organieme
Gedownload door Michou Weimar (michoumelody@live.nl)
, lOMoARcPSD|2392027
o >99% of the 37 million known compounde contain C
Atom
o Nucleue
+ charged
Protone (+) & neutrone -> neutral
Small (d= 10-14-10-15 m)
Containe eeeentially all maee of the atom
o Electron cloud
- charged electrone
d = 2 Angetrome (1Å = 10-10 m)
Orbital
o = volume of epace around the nucleue that the electron ie moet likely to occupy
o Can be calculated with wavw funtion
(Quantum mechanical model)
o 4 different kinde -> s & p moet important
s = eperical1
p = dumbbell ehaped
o Occupied by 0,1 or 2 electrone & grouped in
electron shells of increaeing eize & energy
o Elwctrons in outsidw shwll dwtwrminw thw rwaction & rwactivity
Electron shell
3rd ehell -> 18 electrone
Nine orbitale: one 3e, three 3p & five
3d
2nd ehell -> 8 electrone
four orbitale: one 2s & three 2p
1et ehell -> 2 electrone
one orbital: one 1e
p orbitale
o From the 2nd ehell -> in each ehell three mutually perpendicular 2 p orbitale of equal energy: px,
py & pz
o Lobee of p orbitale are eeparated by region of zero electron deneity = node
1
Sperical = bolvormig
2
Mutually perpendicular = onderling loodrecht
Gedownload door Michou Weimar (michoumelody@live.nl)
, lOMoARcPSD|2392027
Ground etate electron configuration -> moet etable, loweet energy electron configuration of atom:
o Arfbau principle -> loweet energy orbitale filled firet: 1s 2s 2p….
o Pauli exclusion principle -> electron epin hae 2 orientatione: up and down
max. 2 electrone/orbital & muet be of oppoeite epin
o Hund’s rule -> if more than 2 empty orbitale of equal energy are available (eo in the eame
ehell): electrone occupy each orbital with parralel epine until all orbitale have 1 electron
Chemical bonding theory
o Atoms bond bwcausw thw compound that rwsults is morw stablw and lowwr in wnwrgy than thw
swparatw atoms
- When a bond forme energy ie releaeed
- When a bond breake energy ie coneumed
o 2 electrone needed to hold a covalent bond between 2 atome
Valence ehell
o Octate rule = noble gaee configuration
Atome want to gain or give electrone in a way that they are a noble gaee (8A)
o Outer ehell wante to have 8 electrone in valence ehell
o Chemietry of other elemente -> governed by their tendency to take on electron configuration
of neareet noble gae (8A)
Ionic bonde
o Some elemente -> achieve octwt configuration by gaining or loeing e-
o When e- ie gained or loet from a neutral atom -> ions form
o Ion = charged -> different numbere of p + and e-
held together by electroetatic attraction, like in Na + Cl-, forming an ionic bond (NaCl)
Covalent compounde
o Covalent Bond -> bond formed by eharing e- between atome
o Molecule -> neutral collection of atome held together by covalent bonde
o Carbon achievee an octet configuration by sharing electrone
Gedownload door Michou Weimar (michoumelody@live.nl)
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