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A-LEVEL CHEMISTRY > A3 Inorganic Chemistry > Flashcards

A3 Inorganic Chemistry Flashcards

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1
Q

How do all electronic configurations of Group 2 elements end

A

S (^2)

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2
Q

What happens to all group 2 elements in redox reactions

A

Oxidised to form 2+ ions

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3
Q

General symbol equation for Group 2 elements reacting with dilute acid

A
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4
Q

General symbol equation for Group 2 elements reacting with water

A
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5
Q

General symbol equation for Group 2 elements reacting with oxygen

A
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6
Q

State and explain the reactivity of Group 2 elements

A
  • Reactivity increases down group
  • More shells
  • More sheilding
  • Nuclur attraction decreases
  • Ionisation energy decreases
  • Less energy required to remove outer-shell electron
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7
Q

Down Group 2, what happens to elements reducing power

A

Strong reducing agents

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8
Q

State how solubility changes down the group and so the effect this has on the solution produced

A
  • Solubility increases
  • More alkaline solutions form
  • Solutions have higher pH
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9
Q

General symbol equation for metal oxide reacting with water

A
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10
Q

What property of group 2 compounds make them useful

A

They are basic

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11
Q

What is the use of calcium hydroxide in commerce, and what is the equation

A
  • Neutralise soil acids in agriculture
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12
Q

What is the use of magnesium hydroxide and calcium carbonate in commerce, and what are their equations

A
  • Antacids to treat indigestion
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13
Q

What electronic configurations do all group 7 elements end with

A

s(^2)p(^5)

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14
Q

What happens to all group 7 elements in redox reactions

A

Reduced to form 1- ions

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15
Q

How do all group 7 elements exist

A

Diatomic molecules

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16
Q

Why does the boiling point of group 7 elements decrease down the group

A
  • London forces become stronger
  • More energy needed to break London forces
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17
Q

State and explain the trend in reactivity down the group 7

A
  • Reactivity decreases
  • More shells
  • Atomic radius increases
  • More sheilding
  • Nuclear attraction decreases
  • Ionisation energy decreases
  • More energy required to attract outer-shell electron
18
Q

Colour of chlorine regular

A

Colourless

19
Q

Colour of chlorine aqueous

A

Colourless

20
Q

Colour of chlorine organic

A

Colourless

21
Q

Colour of bromine regular

A

Red-Brown

22
Q

Colour of bromine aqueous

A

Orange

23
Q

Colour of bromine organic

A

Brown

24
Q

Colour of iodine regular

A

Dark grey

25
Q

Colour of iodine aqueous

A

Orange

26
Q

Colour of iodine organic

A

Violet

27
Q

Define Disproportionation

A

The reduction and oxidation of the same element in the same reaction

28
Q

Equation for chlorine reacting with cold, dilute aqeous sodium hydroxide, to form bleach

A
29
Q

Chemical formula and name for bleach

A
  • NaClO
  • Sodium Chlorate (I)
30
Q

When chlorine is used to form bleach, what are the conditions required for sodium hydroxide

A
  • Cold
  • Dilute
31
Q

Equation for chlorine used for water treatment

A
32
Q

Formula and name of acid created when chlorine is used for water treatment (not HCl)

A
  • Chloric (I) acied
  • HClO
33
Q

Benefits of using chlorine for sterelising drinking water

A

Kills bacteria

34
Q

Risks with using chlorine for sterelising drinking water

A
  • Chlorine gas is toxic
  • Chlorinated hydrocarbons formed which are carcinogenic
35
Q

How to test for halide ions and result

A
  • Add HNO3
  • Add AgNO3
  • Add ammonia
  • Chloride ppt dissolved in dilute ammonia
  • Bromide ppt dissolved in concentrated ammonia
  • Iodide ppt insoluble in concentrated ammonia
36
Q

Equation for halide ion test

A
37
Q

How to test for carbonate ions, and result

A
  • Add HCl
  • Bubble gas through limewater
  • Limewater turns cloudy
38
Q

Equation for carbonate ion test

A
39
Q

How to test for sulfate ions

A
  • Add HCl to remove any carbonates
  • Add BaCl2
  • White ppt will form
40
Q

Equation for sulfate ion test

A
41
Q

How to test for ammonium ions and result

A
  • Add NaOH
  • Gently heat
  • Ammonia gas produced
  • Turns damp litmus blue
42
Q

Equation for ammonium ion test

A

A-LEVEL CHEMISTRY (11 decks)

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