2.5 Hydrocarbons Flashcards
Well if u seem concerned, go see the first few pages if ya want
Okay
What are free radicals?
Atoms/groups of atoms which have a single unpaired electron
How are free radicals formed?
What name for it?
Bond splits evenly - each atom having one of the 2 electrons
Homolytic fission
What are the 3 stages of Homolytic fission?
Stage 1 - Initiation
Stage 2 - Propagation
Stage 3 - Termination
Explain intitiation stage?
UV radiation causing a [chlorine-chlorine] bond to split homolytically
(symbol for radical is that full stop on the top right of it) aka
Cl]-[Cl (U.V)-> Cl˙ + Cl˙ OR Cl2 (UV)-> 2CL˙ (Chlorine radicals)
Explain propagation stage?
Radicals = reactive ∴ take part in a series of propagation reactions
CH4 + Cl˙ -> ˙CH3 + HCl
CH3 + Cl2 -> CH3Cl + ˙Cl
There’s a diagram for dat one too + chain reaction type sh forming radical as a product
Explain termination stage?
Cl˙ + Cl˙ -> Cl2
Cl˙ + ˙CH3 -> CH2Cl
˙CH3 + ˙CH3 -> CH3CH3
Propagation will continue until two radicals meet = termination
How are alkenes more reactive than alkanes?
And ig how alkenes forms bonds or summin?
- Alkenes more electron density
- Due to more as there are 2 electron pairs = 4 electrons
- Centred between carbons either side of double bond
- Can use one electron pair in double bond to react and form new bonds to each carbon atom
What happens to alkanes when their one electron pair is used?
- Sigma bond broken
- Molecule destroyed
U also gotta look at page 6 for them reactivity of alkene n alkane n stuff
Okay
Explain how alkenes give rise to pi bonds?
And ig what that means too?
During carbon bond, as second bond (second pair of electrons) created, overlap of the p-orbitals of the 2 carbon atoms happen, forming pi bonds (area of high electron density) above and below plane of molecule.
This is why it’s a double bond???? idk
Or just go to page 7 for alkenes related bonding thing
Okay
What it mean for carbon-carbon double bonds having restricted rotation?
- No free rotation due to pi-bond
- Therefore even tho it’s the same molecules,
- It’s a different thing due to it’s position
- That’s why carbon-carbon single bonds would still have the same name despite different position of molecules
Define electrophile?
Atom (or group of atoms) attracted to an electron-rich centre/atom. Accepts a pair of electrons to form new covalent bond
E.g. Hbr/HCl/Cl2/Br2/H
Define nucleophile?
Chemical that can donate a pair of electrons with the subsequent formation of a covalent bond
E.g (All molecules except H have 2 dots above em, lone pair type sh)
-OH, Br-, Cl-, -CN/H2O or NH3