Reactivity Trends Flashcards

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
What is the appearance and state of bromine at room temperature and pressure?
Red brown liquid
26
What is the appearance and state of iodine at room temperature and pressure?
Shiny grey-black solid
27
What is the appearance and state of astatine at room temperature and pressure?
Never been seen
28
Explain the trend in boiling points of halogens
More electrons Stronger London forces More energy required to break intermolecular forces Boiling point increases
29
How does the electron configuration of halogens link to that of a noble gas?
One less electron than the nearest noble gas
30
Is a halogen a reducing or oxidising agent?
Oxidising agent, induces oxidation in another species by being reduced
31
What do displacement reactions show?
Reactivity of halogens decreases down the group
32
What colour are chlorine, iodine and bromine in water?
Chlorine- pale green Bromine- orange Iodine- brown
33
What colour are chlorine, iodine and bromine in cyclohexane?
Chlorine- pale green Bromine- orange Iodine- violet
34
Explain the trend in reactivity of halogens
Atomic Radii increases Greater Shielding Less nuclear attraction to capture electron from another species Reactivity decreases
35
What is a disproportionation reaction?
A redox reaction in which the same element is both oxidised and reduced
36
What are 2 examples of disproportionation reactions?
Chlorine with water | Chlorine with cold, dilute sodium hydroxide
37
Write reaction of chlorine with water
Cl2 (aq) +H20 (l) = HClO (aq) + HCl
38
Write reaction of chlorine with cold dilute sodium hydroxide
Cl2 (aq) +2NaOH (aq) = NaClO +NaCl + H20
39
What are the negatives to using chlorine?
Toxic gas Respiratory irritant Can be chlorinated hydrocarbons- which are cancer causing
40
Describe process of carbonate test
Add dilute nitric acid to test tube | See bubbles = carbonate
41
How do you test for CO2?
Add saturated aqueous solution of calcium hydroxide
42
Describe sulfate test
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
Describe halide test
Add aqueous silver nitrate | Different colour precipitates form
44
What is the equation for the halide test?
Ag +(aq) + X-(aq) = AgX(s)
45
What colours are the halide precipitates?
Chloride- white precipitate Bromide- cream precipitate Iodide- yellow precipitate
46
How does solubility of the halides vary with aqueous ammonia?
Chloride- soluble in dilute NH3 Bromide- soluble in conc. NH3 Iodide- insoluble in conc. NH3
47
What is the correct order of test for anions?
Carbonates Sulfates Halides
48
Why do carbonates have to be tested for before sulfates?
BaCO3 also forms a solid white precipitate
49
How do you test a mixture of chemicals?
Carry out tests in same sequence and on the same solution
50
How do you test for the ammonium ion?
Add aqueous sodium hydroxide Ammonia gas produced Warm Test gas with indicator paper