C5 - Chemical Change Flashcards

1
Q

List the order of the reactivity series including carbon.

A

Potassium , sodium , lithium , calcium , magnesium , aluminium , carbon , zinc , iron , tin , lead , hydrogen , copper , silver , gold , platinum .

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2
Q

What is oxidisation in terms of oxygen?

A

The gain of oxygen.

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3
Q

What is reduction in terms of oxygen?

A

The loss of oxygen

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4
Q

What is the definition of a displacement reaction?

A

A chemical reaction where a more reactive metal displaces a less reactive metal.

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5
Q

Why does a displacement reaction occur?

A

A displacement reaction occurs because a more reactive metal pushes out(displaces) a less reactive metal from it’s compound.

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6
Q

What does oxidisation mean in terms of electrons?

A

The loss of electrons.

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7
Q

What does reduction mean in terms of electrons?

A

The gain of electrons.

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8
Q

Describe displacement reactions using an ionic equation between calcium and copper sulfate

A

Ca^2+ + CuSO_4 —–> CaSO_4 + Cu^2+

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9
Q

Explain how carbon is used to reduce an ore.

A

The carbon displaces the metal from the compound, and removes the oxygen from the oxide, this leaves the metal by itself.

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10
Q

Explain how hydrogen is used to reduce an ore.

A

The ore is heated with hydrogen, the hydrogen displaces the less reactive metal from its compound and leaves the metal on its own.

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11
Q

Describe how metals can be extracted.

A

Metals are extracted from their ore by using displacement reactions with carbon and hydrogen (and electrolysis).

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12
Q

Explain why some metals are found uncombined in the Earth’s crust.

A

Some metals are found uncombined (in a compound) in the earth’s crust because the metal is very unreactive or inert.

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13
Q

What is the definition of a salt?

A

A compound formed when some or all of the hydrogen in an acid is replaced by a metal.

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14
Q

Describe how to make a salt.

A

By reacting a metal with an acid.

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15
Q

Explain ionically the reaction between a metal and an acid.

A

For a metal to react with an acid it must be more reactive than hydrogen; if this condition is met the metal will displace the hydrogen and form an ionic compound with the non metal part of the acid.

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16
Q

Describe a method to prepare a pure, dry sample of a soluble salt from an insoluble substance and a dilute acid.

A
  • Place base into acid.
  • Speed up reaction via heat and shaking.
  • Wait for reaction to end.
  • Filter out any excess base.
  • Leave to evaporate in an evaporating basin at room temperature to get best quality crystals.
17
Q

Why is a reaction between a base and a dilute acid a neutralisation reaction?

A

This is because a base is alkali and the acid is acidic. So these two substances practically ‘cancel’ each other out.

18
Q

Explain how alkalis are a subgroup of bases.

A

Because alkalis are soluble bases.

19
Q

What is the general equation for metal carbonate + acid?

A

Metal carbonate + acid –> salt + water + carbon dioxide

20
Q

What is the method for making salt from metal carbonate + acid?

A
  • Place metal carbonate in acid
  • Place either pH meter or universal indicator in solution.
  • Wait for pH to be 7.
  • Filter out left over carbonate.
  • Leave to evaporate in an evaporating basin at room temperature for crystals to form.
21
Q

Why is the reaction between ammonium and dilute acids important in agricultural?

A

Because the ammonium forms salts from the non hydrogen ions in the acid and becomes a useful nutrient for plants to grow.

22
Q

How do we tell between acids and alkalis with universal indicator?

A

Acids turn Ul yellow-red and alkalis turn Ul blue-purple.

23
Q

How can we use universal indicator to determine approximate pH?

A

We can use a spectrum of colours with approximate pH values assigned to them and compare them to our solution.

24
Q

Describe the pH scale.

A

A scale used to measure the concentration of H+ ions in a solution and thus how acidic or alkali it is.

25
What is considered alkali and what is considered acid on the pH scale?
Anything below 7 is acidic anything above is alkali.
26
What are examples of acid alkali base, acidic chemicals?
sulphuric acid ,sodium hydroxide copper hydroxide, hyrdochloric acid
27
How does the pH of a solution change as we add acid or alkali?
It goes up or down respectively.
28
What is a strong acid?
One that fully ionises.
29
What is a weak acid?
One that doesn't fully ionise.
30
What is a concentrated acid?
High volume of acid with a low volume of water.
31
What is a dilute acid?
Low volume of acid with a high volume of water.
32
Give an example of a strong acid.
Hydrochloric acid.
33
What is an example of a weak acid?
Ethanoic acid.
34
What is the difference between concentration and strength in terms of acid?
Concentration shows how much acid is in a solution while strength shows how many hydrogen ions ionise.
35
How can we tell if an acid is strong or not via its ionic equation?
We can see how many of its H+ ions broke off from the rest of the molecule.
36
How do you find the pH by using the concentration of hydrogen ions?
-log(H in mol/dm^3)
37
What is the general equation for metal + oxygen?
Metal + oxygen ---> metal oxide
38
What is the general equation fro metal + water?
Metal(more reactive than hydrogen) + water --> metal hydroxide + hyrdogen
39
What is the general equation for a metal + acid?
Metal + acid --> salt + hydrogen