Inorganic⚗️ Chemistry

Front 1

Periodicity.

Unit 2: Section 1;

Back 1

:)

Front 2

How can we split the periodic table into blocks?

Back 2

s,p,d,f depending on the last sub-shell in their electronic structure.

Front 3

Why does atomic radius decrease across a period?

Back 3

)higher nuclear charge pulls the electrons closer (as they are added to the same outer energy level).

Front 4

How does ionisation energy change across a period?

Back 4

general increase with a few blips due to sub-shells/orbitals.

Front 5

How do melting points change across a period and why?

Back 5

Erratic due to it being linked to bond strength and structure.

Front 6

How melting points change across period 3?

Back 6

starts off with increasing metallic bonds then silicon has macromolecular spike and then decreases with the simple molecular decreasing with respect to the size as more electrons more van der waals.

Front 7

Group 2, the Alkaline Earth Metals.

Unit 2: Section 2;

Back 7

:)

Front 8

Hoe does reactivity change down group 2 and why?

Back 8

Increases, as, they lose electrons and first ionisation energies decrease.

Front 9

How do melting points change down group 2?

Back 9

Decrease, as, the metal ions get bigger but the charge on the ion remains at 2+

Front 10

What is the exception to how the melting points change down group 2, and why?

Back 10

Magnesium has a big downwards blip as it has a different crystal structure(arrangement of metallic ions).

Front 11

When group elements react, they are:

Back 11

oxidised from a state of 0 to +2, forming

e.g. Ca -> Ca2+ +2e-

Front 12

group 2 metals react with water to give:

Back 12

metal hydroxide and hydrogen.

Front 13

How does groups 2 elements readiness to react with water change down group 2 and why?

Back 13

Be, doesn't react -Ca, reacts steadily -Ba, reacts rapidly. Because ionisation energies decrease down the group so they can be more easily oxidised.

Front 14

How do solubility trends down group 2 change & why?

Back 14

Depend on compound ion, but, generally single charge negative ions(e.g. OH-,hydroxide)increase & doubly charged ions(e.g. SO42-,sulfate) decrease.

Front 15

Sparingly soluble means?

Back 15

Very low solubility

Front 16

barium sulfate (BaSO4), solubility:

Back 16

Insoluble

Front 17

magnesium hydroxide Mg(OH)2, solubility:

Back 17

Sparingly soluble

Front 18

Test for sulfate ions?

Back 18

If acidified barium chloride (BaCl2) is added to a solution containing sulfate ions then a white precipitate of barium sulfate is formed.

Front 19

Why does a solution need to be acidified for a test for sulfate ions & how?

Back 19

with hydrochloric acid(HCl) to get rid of any lurking sulfites(SO32-) or carbonates(CO2−), which also produce a white precipitate.

Front 20

Calcium hydroxide use:

Back 20

Slaked lime, used in agriculture to neutralise acid soils.

Front 21

Magnesium hydroxide use:

Back 21

Milk of magnesium, use in some indigestion tablets as an antacid - this is a substance which neutralises excess stomach acid.

Front 22

Barium sulfate use:

Back 22

Barium meals, line soft tissue and are opaque to x-rays so show them up when normally it would pass through.

Front 23

Magnesium use:

Back 23

Extraction of titanium, TiO2 is converted to TiCl4 by heating it with carbon in a steam of chlorine gas and purified in fractional distillation before being reduced by magnesium in a furnace at nearly 1000C to form Ti

Front 24

Calcium oxide and calcium carbonate use:

Back 24

Wet scrubbing, removes sulfur dioxide from flue gases by reacting them with a slurry made of said alkali and water and produces solid waste product calcium sulfite.

Front 25

Group 7[17], the Halogens.

Unit 2: Section 3;

Back 25

;)

Front 26

Difference between halogen & halide.

Back 26

Halogen describes X or x2, halide describes X-

Front 27

colour change down the halogens:

Back 27

F2-Pale yellow

Cl2-Green

Br2-Red-brown

I2-Grey

Front 28

Halogen displacement reactions & rule:

Back 28

e.g. with KX, the less electronegative element will be displaced, premise chlorine water is colourless, bromine water is orange & iodine solution is brown;

Front 29

How to make bleach and show it's a disproportionation reaction.

Back 29

Chlorine gas with cold, dilute, aqueous sodium hydroxide:

2NaOH(aq) + Cl2(g) -> NaClO(aq) + NaCl(aq) + H2O(l)

Ox. state: 0 +1 -1

Front 30

[sodium chlorate(I), NaCl] uses:

Back 30

Used in water treatment, to bleach paper and textiles .. and handy for cleaning toilets

Front 31

Chlorine in water:

Back 31

When you mix chlorine with water, it undergoes disproportionation. You end up with a mixture of chloride ions and chlorate(I) ions.(BTW it's a reversible reaction)

Front 32

Chlorine in water in sunlight what happens:

Back 32

In sunlight, there is an extra step, Chlorine can also decompose water to form Chloride ions and oxygen this is bad as chlorate(I) ions are what we actually wanted.

Front 33

Pros of treating water

Back 33

)Kills diseases-causing microorganisms

)Persists and prevents later infection

)Prevents the growth of algae, eliminating bad tastes and smells, and removes discolouration caused by organic compounds.

Front 34

Cons of treating water

Back 34

)Chlorine is harmful - breathed in irritates lungs & liquid give chemical burns; both can be fatal

)Carcinogenics are created when chlorine forms chlorinated hydrocarbons; this risk is small compared to e.g. cholera = 1000's dead

)Kills useful microorganisms like anerobes that produce B12

Front 35

What happens to reducing power down the halogens and why?

Back 35

Increases, as, the ions get bigger - electrons further from nuclear charge & extra inner shells - more shielding.

Front 36

Reaction of NaF or NaCl with H2SO4(sulfuric acid):

Back 36

1)HF or HCl is formed. You'll see misty fums as the gas comes into contact with moisture in the air. +you get NaHSO4

2)But HF & HCl aren't Strong enough reducing agents so it stops there.

3)Not a redox reaction the halide and sulfur stay the same (-1 & +6)

Front 37

Reaction of NaBr with H2SO4(sulfuric acid):

Back 37

1)First misty fumes of HBr + NaHSO4

2)Strong enough reducing agent so reacts with H2SO4 in a redox reaction.

3)The HBr reacts to form choking fumes of SO2 and orange fumes of Br2 + some water

Front 38

Reaction of NaI with H2SO4(sulfuric acid):

Back 38

1)Same as NaBr

2)But as strong as reducing agents get and the HI reduces SO2

3)forms H2S + water and iodine also

Front 39

H2S

Back 39

Hydrogen sulfide: toxic and smells of bad eggs.

Front 40

Test for halides:

Back 40

First add dilute nitric acid to remove ions which might interfere, then add a few drops of silver nitrate solution (AgNO3(aq)). A precipitate of the silver halide is formed. Then to be extra sure add ammonia solution as each silver halide has a different solubility in it.

Front 41

Halide test for Fluoride F-

Back 41

No precipitate

Front 42

Halide test for Chloride Cl-

Back 42

White precipitate that forms the slowest then dissolves in dilute NH3(aq).

Front 43

Halide test for Bromide Br-

Back 43

Cream precipitate then dissolves in concentrated NH3(aq).

Front 44

Halide test for Iodide I-

Back 44

Yellow precipitate that forms the fastest then is insoluble in concentrated NH3(aq).

Front 45

Test to identify Group 2 ions:

Back 45

1)Dip a nichrome loop in concentrated HCl.

2)Then dip the wire loop into the unknown compound.

3)Hold the loop in the blue part of a Bunsen burner flame.

4)'Observe colour change in flame.

Front 46

Calcium, Ca2+, flame colour:

Back 46

brick red.

Front 47

Strontium, Sr2+,flame colour:

Back 47

Red.

Front 48

Barium, Ba2+,flame colour:

Back 48

Pale green.

Front 49

Test for Ammonium ions(NH4+):

Back 49

Add some dilute sodium hydroxide solution and gently heat NH3 which is an alkaline will be given off, and this will turn damp red litmus paper blue.

Front 50

Test for Sulfates(SO42-):

Back 50

HCl followed by barium chloride , white precipitate of barium sulfate forms.

Front 51

Test for hydroxides:

Back 51

Dip a piece of red litmus paper into a soltion if OH- is present it will turn blue.

Front 52

Test for carbonates(CO32-):

Back 52

add HCl will fizz as CO2 is formed then will turn limewater cloudy if you bubble the CO2 through it.