LAST BIT OF REVISION!!! Flashcards
Why is Aluminium titanium harder than pure Aluminium
Titanium ions distort the regular arrangement of atoms
Size of atoms greater/smaller
Layers slide over each other
Why is the Ionic Radius greater in non metals ions
More e - –> more repelled
–> valence e- further from the nucleus
Pv = nRT (symbols)
P = Kpa
V = dm^3
Why is the Atomic Radius of Aluminium is greater than Silicon
Silicon greater number of protons
Causes stronger pull on the outer e- valence shells
–> Same number of shells
Why is the Ionic Radius of Na greater than Na
Na -> Na+
- –> Lower Energy Levels
–> Less shielding
–> Greater effective nuclear charge
How does volume affect equilibrium?
High volume –> Low pressure
Hydrogenation of Alkenes Equation and what is neeeded
H2 + C2H4 –> C2H6
High Pressure + Temp
Catalyst: Nickel
Hydration of Alkenes
C2H4 + H2O –> C2H5OH
Catalyst: H2SO4
How volatiles are esters?
Very volatile
Equation for Esterification
Ethanoic Acid + Ethanol –> H2O + Ethyl Ehanoate
Initiation Equation
Cl2 –> 2Cl’
Propagation Equation
CH3’ + CH4 –> ‘CH3 + HCl
‘CH3 + Cl2 –> CH3Cl + Cl’
Termination
Cl’ + Cl’ –> Cl2
‘CH3 + ‘CH3 –> C2H6
Explain the general increasing trend in the first ionization energies of the period 3elements, Na to Ar.
increasing number of protons
OR
increasing nuclear charge
«atomic» radius/size decreases
OR
same number of shells
OR
similar shielding «by inner electrons»
«greater energy needed to overcome increased attraction between nucleus andelectrons»
IHD equation
IHD = 2X + 2-Y/2
What is an electrophile
Species that are electron deficient + positive charge
Why does Benzene not do addition reactions
Decline in stability as Delocalised e- become unstable
What is the purpose of the ozone layer
Absorbs harmful Uv radiation from the sun
How are ozone levels maintained
By a continuous cycle of synthesis and breakdown reactions by the action of energy from UVC and UVB
Outline, giving a reason, how the bond polarity changes going down group 17.
Repeating Units
see
Graphite Structure
each carbon atom is covalently bonded to three other carbon atoms
layered structure consisting of carbon atoms arranged in fused hexagonal rings
The layers are held together by relatively weak London dispersion forces.
Fullerene structure
Like graphite, each carbon atom is covalently bonded to 3 other carbon atoms.
C60 does have delocalised electrons but the electrons cannot jump between individual fullerenes, therefore, it is a poorer electrical conductor than graphite.
