Inorganic Chemistry And Periodic Table Flashcards by Lucy Broderick

trend in ionisation in group 2

decrease down the group
outer electron distance from the nucleus increases
shielding also increases
attraction to the nucleus decreases

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trend in reactivity in group 2

as you go down, increases
can lose electron easier
as increased shielding
increase atomic radii

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reaction of group 2 with oxygen

2M + O2 → 2MO
except barium forms a peroxide
Ba + O2 → 2BaO2

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flame colour of Mg

bright white

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flame colour of Ca

brick red

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flame colour of Sr

crimson

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flame colour of Ba

apple green

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reaction of group 2 with water

less reactive than group 1
Ca + 2H2O → Ca(OH)2 + H2
steam Mg + H2O → MgO + H2

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reaction of group 2 with chlorine

when heated

Mg + Cl2 → MgCl2

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reaction of group 2 oxides with water

CaO + H2O → Ca(OH)2

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reaction of group 2 oxides with dilute acid

MgO + H2SO4 → MgSO4 + H2O
CaO + 2HNO3 → Ca(NO3)2 + H2O
BaO + 2HCl → BaCl2 + H2O

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reaction of group 2 hydroxides with dilute acid

Ca(OH)2 + 2HNO3 → Ca(NO3)2 + 2H2O

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trend in the solubilities of group 2 sulphates

decreases down the group
Ba2+(aq) + SO42-(aq) → BaSO4(s)
ca=slightly soluble
Sr+Ba=insoluble

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trend in the solubilities of group 2 hydroxides

increases down the group

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trend in thermal decomposition of group 1 carbonates

Li2CO3 Li2O + CO2
more thermally stable down the group
atomic radius increases
decreased charged density
decreased polarising power
aren’t able to distort the carbonate as much
Bonds in the carbonate aren’t weakened as much

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trend in thermal decomposition of group 2 carbonates

MgCO3 MgO + CO2
less thermally stable than group 1
higher charge density
more thermally stable down the group
raduis incr, less charge dense
decreased polarising power
Bonds in the carbonate aren’t weakened as much

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trend in thermal decomposition of group 1+2 nitrates

Li+G2 less thermally stable
2M(NO3)2 → 2MO + 4NO2 + O2
4LiNO3 → 2Li2O + 4NO2 + O2
G1 more stable break apart less
NaNO3 → 2NaNO2 + O2

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reasons for flame tests colours

placed in a flame, their electrons are pushed to a higher energy level
electrons drop back to a lower level again, give out energy in the form of light
The light is characteristic of each particular metal and gives the flame a certain colour

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flame test for Li

red

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flame test for Na

yellow

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flame test for K

lilac

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states and colours of chlorine

Room temp= green gas
Aq=pale green
hydrocarbon solution=pale green

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states and colours of Bromine

Room temp=red/brown liquid
Aq=orange/yellow
hydrocarbon=red

states and colours of iodine

room temp=grey/black solid
Aq=brown
hydrocarbon=violet

trend in bp+mp of group 7

increases down the group have more electrons stronger london forces more energy need to overcome intermolecular forces

electronegativity of group 7

decreases down the group larger atomic radius shared bonding pair of e- is further from nucleus increased shielding

trend in reactivity of group 7

``` decreases down the group increased shielding increased atomic radius decreased attraction to the nucleus harder to gain electrons ```

example of halogen displacement reaction

Cl2 + 2KBr → Br2 + 2KCl

when an organic solvent is added to displacement reactions

forms two layers | eg cyclohexane on the top layer

colours of the two layers of bromine water in displacement

dissolves more easily in organic so dark orange top layer light less concentrated bottom layer

colours of the two layers of iodine water in displacement

purple top layer pale green bottom layer

halogen oxidizing power

``` decreases down the group increasing shielding increasing atomic radius decreasing attraction to the nucleus electron gained less easily ```

oxidation reactions of group 1+2 metals

2Na + Cl2 → 2NaCl | Mg + Br2 → MgBr2

disproportionation reaction of chlorine with water

Cl2 + H2O ⇌ HOCl + HCl

use of chlorine in water treatment

chloric(I) acid, HOCl, contains the chlorate(I) ion which has a strong anti-bacterial action, so sterilises the water

disproportionation reaction of chlorine with cold, dilute aqueous sodium hydroxide to form bleach

Cl2 + NaOH → NaOCl + NaCl + H2O | produces a much higher concentration of chlorate(I)

the disproportionation reaction of chlorine with hot alkali

3Cl2 + 6NaOH → NaClO3 + 5NaCl +3H2O

halide reducing power

increases down the group ion increases in size more able to lose an electron and return to the Halogen. halide ion transfers its electron to another substance substance is reduced

Concentrated sulfuric acid with chloride

KCl + H2SO4 → KHSO4 + HCl | white steamy fumes produced

Concentrated sulfuric acid with bromide

2HBr + H2SO4 → Br2 + 2H2O + SO2 | orange-brown steamy fumes

Concentrated sulfuric acid with iodide

2HI + H2SO4 → I2 + 2H2O + SO2

halide test

Ag+(aq) + X-(aq) → AgX(s) dissolved in water, acidified with dilute nitric acid silver nitrate solution is added. A precipitate of silver halide forms

halide test to further determine

add dilute ammonia solution concentrated ammonia solution or sunlight

order of halide test with the colour gradient

CBI

test for chloride

White precipitate purple/grey in sunlight dissolves in dilute ammonia

test for bromide

cream precipitate green/yellow is sunlight partially dissolves in dilute fully dissolves in conc

test for iodide

yellow precipitate no effect in sunlight doesn't dissolve

hydrogen halides with water

HX(aq) → H+(aq) + X-(aq) | soluble in water, and when dissolved in they split up (dissociate) into ions forming an acidic solution

hydrogen halides with ammonia

HX(g) + NH3(g) → NH4X(s) | gaseous hydrogen halides come into contact with gaseous ammonia, dense white smoke of ammonium halide is produced

assumptions of fluorine properties (too reactive to test)

strongest oxidising agent in the group, but fluoride ions would be the weakest reducing agent

assumptions of astatine properties (too radioactive, has a short half-life)

weakest oxidising agent in the group, but astatide ions would be the strongest reducing agent

test for Carbonate, hydrogencarbonate

CO32-(aq) + 2H+(aq) → H2O(l) + CO2(g) HCO3-(aq) + H+(aq) → H2O(l) + CO2(g) Add dilute HCl test gas given off with limewater

test for Sulfate

Ba2+(aq) + SO42-(aq) → BaSO4(s) | Add dilute hydrochloric acid to a solution of X, followed by barium chloride solution, White precipitate forms

test for Ammonium

NH4+(aq) + OH-(aq) → H2O(l) + NH3(g) | Warm X with sodium hydroxide solution, Hold damp red litmus to the mouth of the tube, Red litmus goes blue

limewater test

Ca(OH)2(aq) + CO2(g) → CaCO3(s) + H2O(l) | colourless to cloudy