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AQA A Level Chemistry > Inorganic Chapter 2: Group 2 & Group 7 > Flashcards

Inorganic Chapter 2: Group 2 & Group 7 Flashcards

1
Q

What is group 2 called?

A

Alkaline Earth metals

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2
Q

What is trend in Atomic Radius down group 2?

A

It increases - no. of shells increases

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3
Q

What is the trend in first ionisation energy down group 2?

A

It decreases - electrons get further away from the nucleus - easier to remove

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4
Q

What is the trend in reactivity down group 2?

A

It increases - electrons are easier to remove due to distance from nucleus

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5
Q

What is the trend in melting points down group 2?

A

Generally decreases - Metal ions get bigger, nuclei get further away from the delocalised electrons, easier to break bonds

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6
Q

What ions do group 2 elements form?

A

2+ ions

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7
Q

What do group 2 elements produce when reacting with water?

A

A metal hydroxide & Hydrogen

E.g. Ca + 2H2O -> Ca(OH) + H2

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8
Q

What happens to the oxidation state of group 2 elements when they react?

A

They are oxidised from a state of 0 to +2

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9
Q

What are the two factors that decrease first ionisation energy down group 2?

A

Increased shielding
Increased atomic radius

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10
Q

What do solubility trends with group 2 elements depend on?

A

The compound anion (OH, SO4, etc)

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11
Q

What is the trend down group 2 of solubility with singly charged anions?

A

Increases

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12
Q

What is the trend down group 2 of solubility with doubly charged anions?

A

Decreases

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13
Q

How can you test for sulfate ions?

A

Add acidified barium chloride, see a white ppt on a positive result

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14
Q

What are group 2 elements used for?

A

Neutralising acidity - often in agriculture or antacids
Magnesium is used to extract Titanium
Calcium compounds used to remove SO2
‘Barium meals’ for X-rays

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15
Q

How is Magnesium used to extract titanium?

A

It reduces the Ti

TiCl4 + 2Mg -> Ti + 2MgCl

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16
Q

How are calcium compounds used to remove SO2?

A

Flue gas desulfurisation - Mix the compound (CaO or CaCO3) with water, then sprayed it onto the flue gases.

CaO + 2H2O + SO2 -> CaSO3 + 2H2O
CaCO3 + 2H2O + SO2 -> CaSO3 + 2H2O + CO2

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17
Q

What is a ‘Barium meal’ and how does it work?

A

People eat small amount of barium sulfate, which is opaque to X-rays, and will coat the tissue of the digestive tract, showing it on X-rays to diagnose issues.

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18
Q

What is Group 7 called?

A

The Halogens

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19
Q

What ions do group 7 form?

A

1- ions

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20
Q

What is the trend of boiling points down group 7?

A

They increase - increasing strength of VdW forces as size increases

21
Q

What is the trend in electronegativity down group 7?

A

It decreases - larger atoms have less attracting power than smaller atoms

22
Q

What happens when you add a halogen to a halide solution formed with a less reactive halogen?

A

The less reactive halogen will be displaced & a new halide will be formed

23
Q

What is the general rule for halide displacement?

A

The halogen will displace a halide if it’s made from a halogen below it in the periodic table.

24
Q

How can we use displacement reactions of halides?

A

To determine which halide is present in a solution

25
Q

What are some uses of Halogens?

A

Bleach
Cleaning swimming pools

26
Q

How do you make bleach?

A

Sodium Hydroxide & Chlorine

2NaOH + Cl2 -> NaClO + NaCl + H2O

27
Q

How does chlorine kill bacteria in water?

A

It undergoes disproportionation, and the chlorate (I) ions that are formed kill bacteria.

Cl2 + H2O <-> 2H+ + Cl- + ClO-

28
Q

What are some risks associated with chlorine water treatment?

A

Chlorine gas is toxic if you breathe it in
Organic compounds within water can form carcinogenic chlorinated hydrocarbons when reacting with chlorine

29
Q

What is the trend of reducing power going down group 7?

A

It increases - electrons are further away from the nucleus & there is greater shielding effect.

30
Q

What is the reaction of flouride or chloride with sulfuric acid?

A

Produces HF or HCl - reaction stops there

e.g. NaF + H2SO4 -> NaHSO4 + HF

31
Q

What is the reaction of Bromide with sulfuric acid?

A

Produces HBr, which then produces sulfur dioxide, bromine, and water with the sulfuric acid

NaBr + H2SO4 -> NaHSO4 + HBr
HBr + H2SO4 -> Br2 + SO2 + H2O

32
Q

What is the reaction of Iodide with sulfuric acid?

A

Produces HI, which will then reduce H2SO4 and then further reduces the produced SO2 to H2S.
(Equations same as Br)

6HI + SO2 -> H2S + 3I2 + 2H2O

33
Q

What solution is used to test for halides?

A

Silver Nitrate - forms a different colour precipitate depending on the ion.
Next, add Ammonia to identify possibility of Chlorine.

34
Q

What colour ppt does silver nitrate form with Flourine?

A

No ppt

35
Q

What colour ppt does silver nitrate form with Chlorine?

A

White

36
Q

What colour ppt does silver nitrate form with Bromine?

A

Cream

37
Q

What colour ppt does silver nitrate form with Iodine?

A

Yellow

38
Q

What is the result of adding ammonia after a silver nitrate test?

A

Chlorine will form a white ppt
Bromine will form a cream ppt
Iodine will form a yellow ppt

39
Q

What tests can you use to identify group 2 ions?

A

Flame tests
NaOH tests

40
Q

What colour ppt does Mg form with NaOH?

A

white ppt

41
Q

What colour ppt does Ca form with NaOH?

A

Slight white ppt

42
Q

What colour ppt does Sr form with NaOH?

A

Slight white ppt

43
Q

What colour ppt does Ba form with NaOH?

A

None

44
Q

What colour does Ca go in a flame test?

A

Brick red

45
Q

What colour does Sr go in a flame test?

A

red

46
Q

What colour does Ba go in a flame test?

A

Green

47
Q

What is a good test for ammonium ions?

A

Red litmus paper & NaOH - add NaOH to an ammonium solution, it’ll form ammonia gas, which will turn the litmus paper blue due to being alkaline.

48
Q

How do you test for hydroxides?

A

Use a pH indicator, an alkaline result will form if the solution has hydroxides

49
Q

How can you test for carbonates?

A

Add dilute hydrochloric acid, the solution will begin to fizz. Bubble this gas through limewater, and if the limewater goes cloudy, the solution contained carbonate ions.

AQA A Level Chemistry (25 decks)

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