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WHY NOT? > Chapter 8 - Reactivity Trends > Flashcards

Chapter 8 - Reactivity Trends Flashcards

Group 2, The halogens and Quantitative analysis.

1
Q

What is a reducing agent?

A

A species that donates it’s electrons to another species, thereby reducing that species.

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2
Q

Which group are reducing agents commonly found?

A

Group 2

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3
Q

What is the trend in reactivity down group 2?

A

Reactivity increases.

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4
Q

Explain the trend of reactivity down group 2

A

Increased atomic radius and shielding effect so ionisation energies decrease. Therefore it’s easier to lose electrons.

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5
Q

What are the products of a group 2 element reacting with water?

A

Metal hydroxide and hydrogen

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6
Q

What is the product of a group 2 element reacting with oxygen?

A

Metal oxide

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7
Q

What is the trend of solubility down group 2?

A

Increases

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8
Q

Explain the trend of solubility down group 2

A

Down the group, the solution has a greater concentration of OH-.

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9
Q

Given that group 2 oxides, hydroxides and carbonates neutralise acids, what can they be referred to as?

A

Bases

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10
Q

Given that most group 2 oxides, hydroxides and carbonates are soluble in water, what are they also besides bases?

A

Alkalis

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11
Q

What is the use of calcium hydroxide in agriculture?

A

Increases the pH of acidic soils.

Ca(OH)(2) + 2H+ -> Ca2+ + 2H(2)O

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12
Q

How are group 2 compounds used in medicine?

A

Used in indigestion tablets as antacids, often a suspension of a metal hydroxide in water.

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13
Q

What is another name for group 2?

A

Alkaline Earth Metals

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14
Q

What is another name for group 7?

A

Halogens

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15
Q

What is the trend in boiling point down group 7?

A

Increases

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16
Q

Explain the trend in boiling point down group 7

A

More electrons,
Stronger London forces,
More energy to break intermolecular forces,
Boiling point increases.

17
Q

What is the trend in reactivity down group 7?

A

Reactivity decreases

18
Q

Explain the trend in reactivity down group 7

A 
Atomic radius increases,
More inner shells,
Shielding increases,
Nuclear attraction decreases,
Reactivity decreases.
19
Q

What do more reactive halogens do to less reactive halide ions?

A

Displace them

20
Q

What can displacement reactions be used to identify?

A

Which halide is present in solution.

21
Q

Which compound is used to test for halides?

A

Silver nitrate solution

22
Q

How can the results for a halide test be further tested?

A

Solubility in ammonia solution

23
Q

What is disproportionation?

A

A redox reaction in which the same element is both oxidised and reduced.

24
Q

Describe the test for carbonates

A

Carbonates react with acids to form carbon dioxide gas.
Add dilute nitric acid to testing solution. If bubbles observed could be a carbonate. To prove its CO(2), bubble gas through lime water, a white precipitate will form.

25
Q

Describe the test for sulphates

A

Aqueous barium ions are added to the solution. If a white precipitate forms, there is a sulphate.

26
Q

In the halide tests, what happens to chloride with silver nitrate and then ammonia

A

Silver nitrate - white precipitate

Ammonia - soluble in dilute ammonia

27
Q

In the halide tests, what happens to bromide with silver nitrate and then ammonia

A

Silver nitrate - cream precipitate

Ammonia - soluble in concentrated ammonia

28
Q

In the halide tests, what happens to iodide with silver nitrate and then ammonia

A

Silver nitrate - yellow precipitate

Ammonia - insoluble in concentrated ammonia

29
Q

What is the correct order for these anion tests?

A

Carbonate test, sulphate test, halide test

30
Q

Why is this the correct order for anion tests carbonate, sulphate, halide?

A

Carbonates also form a white precipitate in the sulphate test but not vice versa.
Carbonates and sulphates form precipitates with silver nitrate.

31
Q

Describe the test for ammonium ions

A

Add aqueous NaOH to the solution,
Ammonia gas is produced,
Can be detected with moist indicator paper as it will turn blue.

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