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Chemistry > Inorganic Chemistry and the Periodic Table > Flashcards

Inorganic Chemistry and the Periodic Table Flashcards

1
Q

Explain the trend in Ionisation Energies down Group 2

A
  • Ionisation Energies Decreases
  • Down the group number of shells increase
  • The positive charge nucleus is increased as you go down the Group but is counter affected by increase shielding
  • Overall This will lead to a greater distance from a nucleus weakening electrostatic attraction
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2
Q

Explain the trend in Reactivity down Group 2

A

Reactivity increases
Ionisation Energy decreases as you go down the group
Lower activation energies
Outer two electrons can form +2 ions more easily/quicker in reactions

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3
Q

What is formed if a Group 2 metal reacts with oxygen

A

Solid white Metal oxide

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4
Q

What is formed if a Group 2 metal reacts with water

A

Metal hydroxide
Hydrogen

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5
Q

What is formed if a Group 2 metal reacts with chlorine

A

White Solid Chloride

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6
Q

What is the flame colour for lithium

A

Red

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7
Q

What is the flame colour for sodium

A

Yellow

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8
Q

What is the flame colour for potassium

A

Lilac

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9
Q

What is the flame colour for beryllium

A

No flame colour

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10
Q

What is the flame colour for calcium

A

Brick Red

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11
Q

What is the flame colour for Strontium

A

Red

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12
Q

What is the flame colour for Barium

A

Apple Green

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13
Q

What is formed if a Group 2 metal oxide reacts with water

A

Metal hydroxides which dissolve making strongly alkaline solutions
Except Beryllium oxide

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14
Q

What is formed if a Group 2 metal hydroxide reacts with oxygen

A

Metal hydroxides

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15
Q

What is formed if a Group 2 metal oxide reacts with a dilute acid

A

Salt
Water

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16
Q

What is formed if a Group 2 metal hydroxide reacts with a dilute acid

A

Salt
Water

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17
Q

Describe the trend in solubility of hydroxides

A

Solubility increases as you go down the group

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18
Q

Describe the trend in solubility of sulphates

A

Solubility decreases as you go down the group

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19
Q

Define ‘Thermal Decomposition’

A

Thermal Decomposition is when a substance breaks down when it is heated

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20
Q

Define ‘Thermal Stability’

A

An indication of how easily a compound thermally decomposes.

21
Q

Explain the thermal stability of Group 1 Nitrates and Carbonates com[pared with Group 2

A

Group 1 Nitrates and Carbonates more more thermally stable than Group 2
- Smaller ionic charge
- Less distortion
- Weaker polarising power

22
Q

Explain the trend in thermal stability of Group 2 Nitrates and Carbonates

A

Thermal Stability increases down Group 2
- Size of Charge remains the same but Ionic radius increases so charge density decreases
- leading to lower polarising power
- distorts the anions(nitrate/carbonate ion) less resulting in in strong bond
- requires more energy to break

23
Q

What is formed when a Group 2 carbonate is thermally decomposed

A
  • Metal Oxide
  • Carbon Dioxide
24
Q

What is formed when a Group 2 nitrate is thermally decomposed

A
  • Metal Oxide(white solid)
  • Nitrogen Dioxide(brown gas)
  • Oxygen(colourless gas)
25
Q

What is formed when a Group 1 carbonate is thermally decomposed

A

Group 1 compounds are thermally stable
Except Lithium Carbonate which forms a metal oxide and carbonate

26
Q

What is formed when a Group 1 nitrate is thermally decomposed

A

Metal Nitrite
Oxygen
except

27
Q

Describe the trends of melting and boiling points of the halogens

A

Boiling and Melting points increase down group 7
More electron shells resulting in more electrons
Increase strength of London Dispersion Forces

28
Q

Describe the trend in electronegativity of the halogens

A

Decreases down group 7
More electron shells (increase shielding)
Greater distance from nucleus between bonding pair of electron Reducing electrostatic attraction

29
Q

State the physical states of halogens at R.T

A

Cl - gas
Br- liquid
I - solid

30
Q

Describe the trend in reactivity of the halogens

A

Decreases down group 7
More electron shells greater shielding, greater distance from the nucleus
Weaker electrostatic attraction for an additional electron to bond with

31
Q

What happens when you react a halogen with a halide ion in an aqueous solution

A

The more reactive halogen will oxide the halide
For example Chorine oxidises bromide and iodide ions making it the greatest oxidising agent out of the three
Bromine oxidises iodide ions but not chlorine
Iodine cant do any except theoretically astatide
This all means that oxidising ability falls as you go down the Group.

32
Q

What are the colours are the halogens in an aqueous solution?

A

Cl2 - Palest Green
Br2 - Yellow
I2 - Brown

33
Q

What are the colours are the halogens in an organic solution?

A

Cl2 - Palest Green
Br2 - Red
I2 - Violet

34
Q

State the reaction between chlorine and water and why is it useful

A

Disproportionate
Cl2 + H20 –>(reversible) HCl + HOCl(chloric acid)
Use in swimming pools/water treatment

35
Q

State the reaction between chlorine and cold, dilute alkali and why is it useful

A

Cl2 + 2NaOH –> NaCl + NaClO+ H20
Sodium chlorate is used for killing bacteria in bleach

36
Q

State the reaction between chlorine and hot concentrated alkali and why is it useful

A

Cl2 + 6NaOH –> 5NaCl + NaClO3 + 3H20

37
Q

Describe the trend of reducing power of the halides by the reaction between sulphuric acid and a halide

A

Reducing Power Increases as you move down the group
Fluoride ions aren’t a strong enough reducing agent to reduce H2SO4
Chloride ions reduce H2SO4 to HCL(steamy fumes)
Bromide ions reduce to SO2(acidic chocking gas)
Iodide ions reduce to S(yellow solid) or H2S(rotten eggs)

37
Q

State the colour of the precipitates of the halide with silver nitrate solution

A

Chloride - White
Bromide - Cream
Iodide - Yellow

37
Q

State the colour of the precipitates of the halide with silver nitrate solution followed by aqueous ammonia solution

A

AgCl - precipitate dissolves to give a colourless solution
AgBr - precipitate is almost unchanged using dilute ammonia solution, but dissolves in concentrated ammonia solution to give a colourless solution
AgI - precipitate is insoluble in ammonia solution of any concentration

38
Q

Why is there no observation between silver nitrate solution and fluoride ions?

A

Silver Fluoride Dissolves in water

39
Q

State the reaction between Hydrogen Halide and water

A

H2O + HCl —> H3O+ + Cl-

40
Q

State the reaction between Hydrogen Halide and ammonia

A

NH3(g) + HCl(g) → NH4Cl(s)

41
Q

How do you test for carbonate ions?

A

Add an aqueous acid (HCL) to form CO2
Bubble it through limewater which should change from clear to cloudy

42
Q

How do you test for sulphate ions

A

First add HCl to remove any impurities
Add barium chloride to form barium sulphate
Barium sulphate is insoluble and will form a precipitate

43
Q

How do you test for ammonium ions?

A

Add sodium hydroxide and the ammonium compound together then heat it to produce ammonia gas
Use damp red litmus paper and it should change from red to blue

44
Q

State the half equation for the test of carbonate ions

A

2H+ + C03 –> C02 + H20

45
Q

State the half equation for the test of sulphate

A

Ba2+ + S04(2-) —> BaS04

46
Q

State the ionic/half equation for ammonium ions

A

OH- + NH4+ –> NH3 + H20

Chemistry (10 decks)

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