Mock revision

Question 1

What is the meaning of aliphatic

Answer 1

an organic compound which carbon atoms form open chains single, double and triple bonds

Question 2

What is alicyclic

Answer 2

both aliphatic and cyclic( go round and carbon atoms join)

Question 3

what is aromatic?

Answer 3

a unsaturated ring of one or more atoms

Question 4

2 bonding pairs

Answer 4

linear(180d)

Question 5

3 bonding pairs

Answer 5

trigonal planr(180d)

Question 6

2 bonding pair one lone pair

Answer 6

bent or non linear (117.5)

Question 7

4 bond pairs

Answer 7

tetrahedral (109.5)

Question 8

3 bond pairs 1 lone pair

Answer 8

trigonal pyramidal( 107)

Question 9

2 bonding pairs to lone pairs

Answer 9

bent (104.5)

Question 10

5 bonding pairs

Answer 10

trigonal bipyramidal(120, 90)

Question 11

6 bonding pairs

Answer 11

octahedral 90d

Question 12

pv=nrt

Answer 12

pressure=pa
v=m3
n=moles
r=8.134
t=k = c+273

Question 13

moles?

Answer 13

moles = mass(g)/mr

Question 14

relative atomic mass

Answer 14

(isotopic mass * percentage abundance)/ 100

Question 15

concentration?

Answer 15

concentration = moles(n)/ volume (dm3)

Question 16

moles(gas)

Answer 16

moles = volume(dm3)/ 24

Question 17

nitrate ion

Answer 17

No3-

Question 18

carbonate ion

Answer 18

No3 -2

Question 19

Sulfate ion

Answer 19

So4 2-

Question 20

Hydroxide

Answer 20

OH-

Question 21

ammonium

Answer 21

NH4+

Question 22

Zinc ion

Answer 22

Zn2+

Question 23

Silver ion

Answer 23

Ag+

Question 24

ionisation energy down the group

Answer 24

decreases beacause there are larger atoms more shielding easier for electrons to be removed from the atom

Question 25

ionisation energy across a period

Answer 25

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

Question 26

What are the exceptions to increase in ionisation energy

Answer 26

groups 2-3 and 5-6

Question 27

Why are they the exception

Answer 27

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

Question 28

What type of atoms form covalent bonds

Answer 28

non metals

Question 29

what type of atomic form ionic bonds

Answer 29

metals and non metals

Question 30

what is the trend of ionisation in group 2

Answer 30

going down the group ionisation energy decreases ( easier to remove electrons)

Question 31

Group 2 reacting with dilute acid

Answer 31

forms salt and hydrogen M + HCL -> MCL + H2

Question 32

Oxides of group 2 with water

Answer 32

Makes metal hydroxides which is very soluble and makes the solution alkaline

Question 33

What are Group 2 elements used for

Answer 33

To neutralise acids - in soil - antacids in the stomach

Question 34

How does the boiling point act going down the group in halogens

Answer 34

boiling point increases going down the group because there are larger molecules, more electrons so more induced dipole dipole interactions

Question 35

Halogen reactivity down the group

Answer 35

less reactive down the group, larger atom more shielding less pull from the nucleus so harder to gain an electron

Question 36

How do halogens react with each other

Answer 36

A more reactive halogen will displace a less reactive one in its own solution

Question 37

What is the test for halide

Answer 37

Add dilute nitric acid then add silver nitrate positive test should show a precipitate forming

Question 38

What are the colours of the precipitates

Answer 38

Chlorine- white bromine- cream iodine- yellow

Question 39

How do the halides dissolve in ammonia solution

Answer 39

chlorine- dissolves in dilute ammonia bromine dissolves in conc ammonia iodine does not dissolve in conc ammonia

Question 40

What is disproportionation

Answer 40

when an atom undergoes oxidation and reduction at the same time

Question 41

How do halogens undergo disproportionations

Answer 41

with alkali solutions

Question 42

How to make bleach

Answer 42

NaOH + Cl2 -> NaClO + NaCl2 + H20

Question 43

Cl2 + water

Answer 43

Cl2+ H20 -> HCL + HClO

Question 44

Chloric acid

Answer 44

HClO+ H20 -> ClO- + H3O++

Question 45

Test for carbonates

Answer 45

Add a dilute acid , if carbonate present then Co2 will be released(bubbly) Co3- + H+ -> Co2 + H20

Question 46

Whats the test for Co2

Answer 46

Bubble the gas through lime water positive if it goes cloudy

Question 47

What's the test for sulphates

Answer 47

add dilute hcl then barium chloride solution if there is a white ppt then it it is barium sulphate Ba + So4 -> BaSo4

Question 48

Ammonia gas test

Answer 48

damp red litmus paper turns blue

Question 49

Ammonium ion test

Answer 49

Add sodium hydroxide and warm mixture should turn red litmus paper blue as it is just ammonia NH4+ OH -> NH3 + H2O

Question 50

What should be the order for ion tests

Answer 50

add dilute acid to all test for carbonate then sulphates then halide

Question 51

alkene + hydrogen

Answer 51

makes alkane 150degrees and an nickel catalyst

Question 52

alkene and halogens

Answer 52

dihaloalkanes

Question 53

How to test for double bonds

Answer 53

add bromine water should go from orange to colourless

Question 54

Alkene + steam

Answer 54

Makes alcohol 600d 60-70 atm and acid catalyst(phosphoric acid)

Question 55

Alkene + hydrogen halide

Answer 55

Haloalkanes

Question 56

primary oxidation of alcohols

Answer 56

distil aldehyde reflux carboxylic acid

Question 57

secondary oxidation of alcohols

Answer 57

aldehyde

Question 58

tertiary oxidation of alcohols

Answer 58

NA(burned instead)

Question 59

heterolytic fission

Answer 59

both electrons go to one atom