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Chemistry OCR A A level > Reactivity Trends > Flashcards

Reactivity Trends Flashcards

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1
Q

What are group 2 metals called?

A

Alkaline Earth Metals

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2
Q

What are group 2 metals found as on Earth?

A

Stable compounds such as calcium carbonate

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3
Q

How does the electron configuration of Group 2 metals differ from that of a noble gas?

A

Two more electrons than the nearest noble gas

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4
Q

What is the most common type of reaction of group 2 elements?

A

Redox

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5
Q

What happens to a group 2 metal during a redox reaction?

A

Oxidised
Loses 2 electrons
Becomes a 2+ ion

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6
Q

Is group 2 an oxidising agent or reducing agent? Why?

A

Reducing agent- reduces another species by being oxidised

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7
Q

What is the reaction of a group 2 metal and oxygen?

A

Group 2 metal + oxygen = Metal Oxide

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8
Q

What happens when magnesium burns?

A

Magnesium burns with a bright light

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9
Q

What happens when a group 2 metal reacts with water?

A

Metal + Water = Metal hydroxide + Hydrogen

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10
Q

What happens to reactivity of group 2 metals with water down the group?

A

Reactivity increases down the group

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11
Q

What happens when a group 2 metal reacts with acid?

A

Metal + Acid = Salt + Hydrogen

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12
Q

What happens to reactivity in group 2 metals? Why?

A

Increases
Requires 2 ionisation energies.
Ionisation energy decreases because of greater shielding and atomic radii.

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13
Q

What is the reaction of group 2 oxides with water?

A

Group 2 oxide + water= metal hydroxide

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14
Q

Explain trend in solubility of hydroxides

A

Increases down the group

Resulting solutions contain more OH- ions

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15
Q

Explain trend in alkalinity of hydroxides

A

Solubility increases
More OH- ions
Increase in pH
Increase in alkalinity

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16
Q

What is the pH of magnesium hydroxide?

A

10

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17
Q

What is the pH of barium hydroxide?

A

13

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18
Q

How are group 2 compounds used in agriculture?

A

Ca(OH)2 are added to fields as lime to increase pH of acidic sols

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19
Q

What is the equation of group 2 compounds in agriculture?

A

Ca(OH)2 (s) + 2H+(aq) = Ca 2+(aq) + 2H20(l)

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20
Q

Which 2 group 2 compounds are used in medicine?

A

CaCO3

Mg(OH)2

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21
Q

Give the 2 equations of group 2 compound s in medicine

A

Mg(OH)2 +2HCl = MgCl2 + 2H20

CaCO3+ 2HCl = CaCl2 +H20 + CO2

22
Q

Where are halogens found?

A

Sea Water

Potassium and Sodium deposits

23
Q

What is the appearance and state of fluorine at room temperature and pressure?

A

Pale yellow gas

24
Q

What is the appearance and state of chlorine at room temperature and pressure?

A

Pale green gas

25
Q

What is the appearance and state of bromine at room temperature and pressure?

A

Red brown liquid

26
Q

What is the appearance and state of iodine at room temperature and pressure?

A

Shiny grey-black solid

27
Q

What is the appearance and state of astatine at room temperature and pressure?

A

Never been seen

28
Q

Explain the trend in boiling points of halogens

A

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

29
Q

How does the electron configuration of halogens link to that of a noble gas?

A

One less electron than the nearest noble gas

30
Q

Is a halogen a reducing or oxidising agent?

A

Oxidising agent, induces oxidation in another species by being reduced

31
Q

What do displacement reactions show?

A

Reactivity of halogens decreases down the group

32
Q

What colour are chlorine, iodine and bromine in water?

A

Chlorine- pale green
Bromine- orange
Iodine- brown

33
Q

What colour are chlorine, iodine and bromine in cyclohexane?

A

Chlorine- pale green
Bromine- orange
Iodine- violet

34
Q

Explain the trend in reactivity of halogens

A

Atomic Radii increases
Greater Shielding
Less nuclear attraction to capture electron from another species
Reactivity decreases

35
Q

What is a disproportionation reaction?

A

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

36
Q

What are 2 examples of disproportionation reactions?

A

Chlorine with water

Chlorine with cold, dilute sodium hydroxide

37
Q

Write reaction of chlorine with water

A

Cl2 (aq) +H20 (l) = HClO (aq) + HCl

38
Q

Write reaction of chlorine with cold dilute sodium hydroxide

A

Cl2 (aq) +2NaOH (aq) = NaClO +NaCl + H20

39
Q

What are the negatives to using chlorine?

A

Toxic gas
Respiratory irritant
Can be chlorinated hydrocarbons- which are cancer causing

40
Q

Describe process of carbonate test

A

Add dilute nitric acid to test tube

See bubbles = carbonate

41
Q

How do you test for CO2?

A

Add saturated aqueous solution of calcium hydroxide

42
Q

Describe sulfate test

A

Add Ba2+ ions in the form of barium chloride or nitrate

Barium Sulfate forms which is an insoluble white precipitate if sulfate is present

43
Q

Describe halide test

A

Add aqueous silver nitrate

Different colour precipitates form

44
Q

What is the equation for the halide test?

A

Ag +(aq) + X-(aq) = AgX(s)

45
Q

What colours are the halide precipitates?

A

Chloride- white precipitate
Bromide- cream precipitate
Iodide- yellow precipitate

46
Q

How does solubility of the halides vary with aqueous ammonia?

A

Chloride- soluble in dilute NH3
Bromide- soluble in conc. NH3
Iodide- insoluble in conc. NH3

47
Q

What is the correct order of test for anions?

A

Carbonates
Sulfates
Halides

48
Q

Why do carbonates have to be tested for before sulfates?

A

BaCO3 also forms a solid white precipitate

49
Q

How do you test a mixture of chemicals?

A

Carry out tests in same sequence and on the same solution

50
Q

How do you test for the ammonium ion?

A

Add aqueous sodium hydroxide
Ammonia gas produced
Warm
Test gas with indicator paper

Chemistry OCR A A level (20 decks)

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