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NSFC Chemistry AQA A level Y13 > Group 2 and Group 7 > Flashcards

Group 2 and Group 7 Flashcards

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1
Q

Atomic Radius
group 2

A

Increases. Trend in atomic radius down the group. This trend is due to more orbitals and a weaker nuclear charge as the charge is offset by the shielding that has come about from more orbitals

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2
Q

First ionisation energy group 2

A

Decreases. Trend in first ionisation energies down the group. This is because the electrons get further from the nucleus so has a weaker pull from the nucleus

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3
Q

Reactivity
group 2

A

Increases. Trend in reactivity down the group. This is due to the electrons being further from the nucleus allowing the interaction with other molecules

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4
Q

Melting point
group 2

A

Decreases. Trend in melting point down the group. This is because the delocalised electrons are further from the nucleus as the atomic radius increases

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5
Q

Equation for when an element from group 2 reacts with liquid water:

A

X + 2H2O -> X(OH)2 + H2

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6
Q

Reactivity with water down group 2

A

Increases. This is because the ionisation energy decreases so there are more molecules with enough energy for a successful reaction due to increased successful collisions

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7
Q

Trend in solubility of group 2 hydroxides

A

Increases going down the group.

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8
Q

Trend in solubility of sulphates going down group 2

A

Decreases

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9
Q

Uses of Mg(OH)2

A

Treats indigestion

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10
Q

Use of Ca(OH)2

A

Neutralise Soil

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11
Q

Titanium Extraction Equation

A

TiCl4 + 2Mg -> Ti + 2MgCl2

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12
Q

How to test for sulphate ions

A

HCl and BaCl2, look for a white precipitate

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13
Q

Equation for testing for sulphate example

A

BaCl2 + Na2SO4 -> 2NaCl + BaSO4

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14
Q

Why is acid added to the sulfate/halide ion tests

A

To remove interfering impurities that can give false positives.

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15
Q

Solubility of BaSO4

A

Insoluble

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16
Q

Solubility of Mg(OH)2

A

Sparingly soluble

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17
Q

Define sparingly soluble

A

Only a very small amount

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18
Q

Use of BaSO4 and why it is safe to use it for this?

A

Use - X-Rays/Barium meals
This can be safe because barium sulfate is insoluble even though it is toxic.

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19
Q

Uses for CaO and CaCO3

A

Used to remove acidic gases from chimney flews via wet scrubbing

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20
Q

Equation for Wet Scrubbing with CaO

A

CaO(s) + 2H2O(l) + SO2(g) -> CaSO3(s) + 2H2O(l)

21
Q

Equation for Wet Scrubbing with CaCO3

A

CaCO3(s) + 2H2O(l) + SO2(g) -> CaSO3(s) + 2H2O(l) + CO2(g)

22
Q

Reaction of magnesium with steam

A

Mg(s) + H2O(g) -> MgO(s) + H2(g)

23
Q

What’s the use of Ca(OH)2?

A

Neutralises acidic soil

24
Q

Explain the trend in atomic radius down group 7

A

-Increases down group
-More shells + shielding so e- further from nucleus.

25
Q

Explain the trend in melting points down group 7

A

-Increases down group.
-Molecules become larger, more e- + stronger van der waal’s forces between molecules
-More energy required to overcome van der waal’s forces between molecules.

26
Q

Explain the trend in 1st ionisation energies down group 7

A

-Decreases down group.
- larger atomic radius
-More shielding so weaker attraction from electrons to the nucleus.

27
Q

Explain the trend in electronegativity down group 7

A

-Decreases down group.
-Atomic radii and shielding increases so nucleus less able to attract electrons.

28
Q

What is an oxidising agent?

A

An electron acceptor.

29
Q

What is a reducing agent?

A

An electron donor.

30
Q

Is Cl2 a strong or weak oxidising agent? Why?

A

Strong, small atomic radius so excellent at attracting electrons

31
Q

Is I- a strong or weak reducing agent? Why?

A

Strong, large ionic radius so good at giving away electrons to other compounds.

32
Q

Show the equations for the reaction between Br- and Cl2 and state observations.

A

-Cl displaces Br:
2e- + Cl2 -> 2 Cl-
2Br- -> Br2 + 2e-
-Yellow solution

33
Q

Show the equations for the reaction between I- and Cl2 and state observations.

A

-Cl displaces I:
2e - + Cl2 -> 2Cl- + 2e-
2I- -> I2 + 2e-
-Brown solution

34
Q

Show the equations for the reaction between I- and Br2 and state observations.

A

-Br displaces I:
2e- + Br2 -> 2Br -
2I- -> I2 + 2e-
-Brown solution

35
Q

Write the equation to show the displacement reaction between NaCl and H2SO4 and state any observations.

A

-NaCl(s) + H2SO4(l) -> HCl(g) + NaHSO4(s)
-White steamy fumes.

36
Q

Write the equation to show the displacement reaction between NaF and H2SO4 and state any observations.

A

-NaF(s) + H2SO4(l) -> HF(g) +NaHSO4(s)
-White steamy fumes

37
Q

Write the equation to show the redox reaction between NaBr and H2SO4 and state any observations.

A

Red: 2H+ + H2SO4 + 2e- -> SO2 + 2H2O
Ox: 2Br- -> Br2 + 2e-
Redox:
2H+ + H2SO4 + 2Br- -> SO2 + 2H2O + Br2
-brown liquid/orangey brown fumes(Br2)
-Colourless acidic gas (SO2)

38
Q

Write the equation to show the redox reaction between NaI and H2SO4 and state any observations.

A

Red: 2H+ + H2SO4 + 2e- -> SO2 + 2H2O
6H+ + H2SO4 + 6e- -> S + 4H2O
8H+ + H2SO4 + 8e- -> H2S + 4H2O
Ox: I2- -> I2 + 2e-
Redox: 6H+ + H2SO4 + 6I- -> S + 4H2O + 3I2
8H+ + H2SO4 + 8I- -> H2S + 4H2O + 4I2
-Yellow solid (S)
-Rotten egg smell (H2S)
-Grey/black solid (I2)

39
Q

Write the equation to show the redox reaction between Ag+ and Cl- and state any observations.

A

-Ag+(aq) + Cl-(aq) -> AgCl(s)
-White ppt

40
Q

Does silver chloride dissolve in dilute or conc. ammonia?
(equation)

A

Dilute ammonia or conc ammonia to form a complex ion.
AgCl + 2NH3 –> [Ag(NH3)2]+ + Cl-

41
Q

Does silver bromide dissolve in dilute or conc. ammonia?
(equation)

A

conc ammonia to form a complex ion.
AgBr + NH3 –> [Ag(NH3)2] + Br-

42
Q

Write the equation to show the redox reaction between Ag+ and Br- and state any observations.

A

Ag+(aq) + Br-(aq) -> AgBr(s)
-Cream ppt

43
Q

Does silver bromide dissolve in dilute or conc. ammonia?

A

Conc. ammonia to form a complex ion.

44
Q

Write the equation to show the redox reaction between Ag+ and I- and state any observations.

A

-Ag+(aq) + I-(aq) -> AgI(s)
-Pale yellow ppt

45
Q

Does silver iodine dissolve in dilute or conc. ammonia?

A

Neither, it is insoluble in ammonia.

46
Q

Write the equation to show the disproportionation reaction between Cl2 and H2O and state any observations.

A

-Cl2(g) + H2O(l) = HClO(aq) + HCl(aq)
-Cl2 greenish colour
-HClO is bleach

47
Q

Write the equation to show the disproportionation reaction between Cl2 and H2O in UV and state any observations.

A

2Cl2 + 2H2O -> 4H+ + 4Cl- + O2

48
Q

Write the equation to show the disproportionation reaction between Cl2 and cold dilute NaOH and state any observations.

A

Cl2(aq) + 2NaOH(aq) -> NaCl(aq) + NaClO(aq) + H2O(l)
-Cl2 (+Br2, I2) reacts and the colour fades to colourless.
-NaCl + NaClO used as bleach.

NSFC Chemistry AQA A level Y13 (41 decks)

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