Mock revision Flashcards
What is the meaning of aliphatic
an organic compound which carbon atoms form open chains single, double and triple bonds
What is alicyclic
both aliphatic and cyclic( go round and carbon atoms join)
what is aromatic?
a unsaturated ring of one or more atoms
2 bonding pairs
linear(180d)
3 bonding pairs
trigonal planr(180d)
2 bonding pair one lone pair
bent or non linear (117.5)
4 bond pairs
tetrahedral (109.5)
3 bond pairs 1 lone pair
trigonal pyramidal( 107)
2 bonding pairs to lone pairs
bent (104.5)
5 bonding pairs
trigonal bipyramidal(120, 90)
6 bonding pairs
octahedral 90d
pv=nrt
pressure=pa
v=m3
n=moles
r=8.134
t=k = c+273
moles?
moles = mass(g)/mr
relative atomic mass
(isotopic mass * percentage abundance)/ 100
concentration?
concentration = moles(n)/ volume (dm3)
moles(gas)
moles = volume(dm3)/ 24
nitrate ion
No3-
carbonate ion
No3 -2
Sulfate ion
So4 2-
Hydroxide
OH-
ammonium
NH4+
Zinc ion
Zn2+
Silver ion
Ag+
ionisation energy down the group
decreases beacause there are larger atoms more shielding easier for electrons to be removed from the atom
ionisation energy across a period
Increases, the shielding stays the same but the atomic number(proton increase) more nuclear charge so electrons are pulled in more so smaller atomic radii
What are the exceptions to increase in ionisation energy
groups 2-3 and 5-6
Why are they the exception
group 2-3 are going into a new orbital(p orbital) higher energy than s orbital so easier to remove
group 5-6 because when adding an electron to in group 6 the orbital is now paired so there is repulsion between the two electrons
What type of atoms form covalent bonds
non metals
what type of atomic form ionic bonds
metals and non metals
what is the trend of ionisation in group 2
going down the group ionisation energy decreases ( easier to remove electrons)
Group 2 reacting with dilute acid
forms salt and hydrogen
M + HCL -> MCL + H2
Oxides of group 2 with water
Makes metal hydroxides which is very soluble and makes the solution alkaline
What are Group 2 elements used for
To neutralise acids
- in soil
- antacids in the stomach
How does the boiling point act going down the group in halogens
boiling point increases going down the group because there are larger molecules, more electrons so more induced dipole dipole interactions
Halogen reactivity down the group
less reactive down the group, larger atom more shielding less pull from the nucleus so harder to gain an electron
How do halogens react with each other
A more reactive halogen will displace a less reactive one in its own solution
What is the test for halide
Add dilute nitric acid then add silver nitrate positive test should show a precipitate forming
What are the colours of the precipitates
Chlorine- white
bromine- cream
iodine- yellow
How do the halides dissolve in ammonia solution
chlorine- dissolves in dilute ammonia
bromine dissolves in conc ammonia
iodine does not dissolve in conc ammonia
What is disproportionation
when an atom undergoes oxidation and reduction at the same time
How do halogens undergo disproportionations
with alkali solutions
How to make bleach
NaOH + Cl2 -> NaClO + NaCl2 + H20
Cl2 + water
Cl2+ H20 -> HCL + HClO
Chloric acid
HClO+ H20 -> ClO- + H3O++
Test for carbonates
Add a dilute acid , if carbonate present then Co2 will be released(bubbly)
Co3- + H+ -> Co2 + H20
Whats the test for Co2
Bubble the gas through lime water positive if it goes cloudy
What’s the test for sulphates
add dilute hcl then barium chloride solution if there is a white ppt then it it is barium sulphate
Ba + So4 -> BaSo4
Ammonia gas test
damp red litmus paper turns blue
Ammonium ion test
Add sodium hydroxide and warm mixture should turn red litmus paper blue as it is just ammonia
NH4+ OH -> NH3 + H2O
What should be the order for ion tests
add dilute acid to all
test for carbonate then sulphates then halide
alkene + hydrogen
makes alkane
150degrees and an nickel catalyst
alkene and halogens
dihaloalkanes
How to test for double bonds
add bromine water should go from orange to colourless
Alkene + steam
Makes alcohol
600d 60-70 atm and acid catalyst(phosphoric acid)
Alkene + hydrogen halide
Haloalkanes
primary oxidation of alcohols
distil aldehyde reflux carboxylic acid
secondary oxidation of alcohols
aldehyde
tertiary oxidation of alcohols
NA(burned instead)
heterolytic fission
both electrons go to one atom
