Paper 2- Inorganic Chemistry Flashcards

1
Q

Explain the process of titration in detail. (using hydrochloric acid and sodium hydroxide as an example)

A
  • Using pipette & pipette filler add some alkali (about 25cm3) to conical flask with 2/3 drops of indicator
  • Fill a burette with acid & do this below eye level
  • Using burette add acid to alkali a bit at a time & give conical flask a regular swirl
  • Indicator changes colour when all alkali has been neutralised (e.g phenolphthalein = pink in alkalis but colourless in acids)
  • record volume of acid used to neutralise alkali
  • repeat process for reliable results
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2
Q

Titration calculation formula

A

mol

vol x conc

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3
Q

Give the steps taken in a titration calculation when you need to find the concentration of an acid

A

1) work out the moles of the known substance

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4
Q

Name the elements in the reactivity series

A
Potassium 
Sodium 
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper
Silver
Gold
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5
Q

Name the 4 most reactive elements in the reactivity series

A

Potassium
Sodium
Lithium
Calcium

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6
Q

Name the 3 fairly reactive elements in the reactivity series

A

Magnesium
Aluminium
Zinc

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7
Q

Name the 3 not very reactive elements in the reactivity series

A

Iron
Copper
Silver

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8
Q

Name the not reactive element in the reactivity series

A

Gold

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9
Q

How does metals reacting with dilute acids tell you how reactive they are

A

-the more reactive the metal the faster the reaction will go

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10
Q

acid + metal –>

A

salt + hydrogen

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11
Q

Describe the steps you would take in the practical to investigate the differences in reactivity of a variety of metals by using their reaction with acids

A

1) set up 3 boiling tubes and fill with equal volumes of dilute hydrochloric acid/ dilute sulfuric acid
2) place pieces of magnesium, zinc, iron in separate test tubes
- speed of reaction is indicated by the rate of hydrogen bubbles given off
- hydrogen is confirmed by burning splint test

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12
Q

give the word equation for metals reacting with water

A

metal + water –>

metal hydroxide + hydrogen

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13
Q

how do very reactive metals react with water

A
  • react vigorously with water:

- produce bubbles of hydrogen gas

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14
Q

how do less reactive metals react with water

A

-won’t react much with cold water

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15
Q

why do more reactive metals displace less reactive metals

A
  • as more reactive metals react more strongly than less reactive metals
  • meaning more reactive metals displace a less reactive metal from its oxide as it will bond more strongly to the oxygen
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16
Q

iron oxide + aluminium –>

-which element is being displaced in this reaction

A

aluminium oxide + iron

-iron would be displaced from iron oxide by the more reactive aluminium

17
Q

what occurs if you put a reactive metal into a solution of a less reactive metal

A

-reactive metal replaces the less reactive metal in the salt

18
Q

copper sulfate + iron –>

A

iron sulfate + copper

19
Q

what happens if a piece of silver metal is put into copper sulfate solution

A

-nothing happens as the more reactive metal (copper) is already in the salt

20
Q

What conditions are needed for iron to rust?

A

Oxygen and Water

21
Q

What is the name of the chemical reaction that occurs when iron rusts

A

-oxidation reaction

22
Q

What is the chemical name of rust?

A

Hydrated iron(III) oxide

23
Q

How can barrier methods prevent rust

A

-barrier methods coat the iron with a barrier keeping out the water and oxygen

24
Q

Name some barrier method to prevent rust

A
  • paint
  • oil
  • grease
25
Q

Name another way of preventing iron rusting other than barrier methods

-what does this method involve

A
  • sacrificial method
  • involved placing a more reactive metal (zinc) with the iron.
  • The water and oxygen then react with the sacrifical metal instead of iron
26
Q

Rusting can be prevented by spraying iron in zinc, this is called …

A

Galvanising

27
Q

Meaning of Oxidation

A
  • Gain of oxygen

- Lose of electrons

28
Q

Meaning of Reduction

A
  • Loss of oxygen

- Gain of electrons

29
Q

Meaning of Redox reactions

A

Reduction and Oxidation reactions.

30
Q

Oxidising agent

A

-substance that oxidises the metal

-and gets reduced:
Gains electrons
Loses oxygen

31
Q

Reducing agent

A

-substance that reduces metal

  • and gets oxidised
  • Loses electrons
  • Gains oxygen
32
Q

magnesium + oxygen –> magnesium oxide

-what is being oxidised in this freaction

A

-magnesium is oxidised to magnesium oxide