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AS Chemistry (AQA) > IC1 & IC2 > Flashcards

IC1 & IC2 Flashcards

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1
Q

How do you know if an element is s, p, d or f block?

A

According to its position in the Periodic Table, which is determined by its proton number

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2
Q

How is the periodic table arranged?

A

Periods (rows) and groups (columns), by atomic (proton) number.

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3
Q

Elements within a period have the same number of what?

A

The same number of electron shells (if you ignore the s and p sub-shells).

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4
Q

All elements within a group have the same number of what in their outer shell - hence they have similar properties.

A

Electrons.

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5
Q

What does the group number tell you?

A

The number of electrons in the outer shell.

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6
Q

So, does group 0 have 0 electrons on its outer shell? Tip: Hit Alt-F4 if you think this is correct.

A

No. Group 0 elements all have full outer shells – that’s two electrons for helium, and eight electrons for all the others.

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7
Q

Why do we split the periodic table into s, p, d, f?

A

It shows you which sub-shells all the electrons go to

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8
Q

Across a period (vertically), what happens to atomic radius?

A

It decreases across a period

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9
Q

As the number of protons increases, what happens to the nucleus’s charge?

A

It increases.

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10
Q

If the nucleus charge is higher, what happens?

A

Electrons are pulled closer to the radius, making the overall atomic radius smaller.

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11
Q

As you go across a period, an electron is added. Why does this have no effect on the overall radius?

A

Because the electron is on the outermost shell, so it doesn’t really have much of a shielding effect.

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12
Q

Across a period, the energy for ionisation GENERALLY….

A

Increases.

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13
Q

Why does the energy for ionisation generally increase?

A

There are more protons, meaning a bigger positive charge at the nucleus, meaning there is an increasing attraction.

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14
Q

So, we’ve established as you go across a period, ionisation generally increases.

But there are a few blips.

Group 2 and 3 are one such case.

What does the drop in ionisation between Group 2 and 3 show?

A

The sub-shell structure.

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15
Q

Group 5 and 6 also show this “blip”. Why?

A

Electron repulsion.

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16
Q

Melting points in metals vary across the period. Why?

A

They depend on the structure of elements and the bonding within them.

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17
Q

Sodium, magnesium and aluminium are metals. Why does aluminium have the highest boiling and melting point?

A

The metal bonds are stronger. This is because the metal ions have an increasing positive charge, an increasing number of delocalised electrons and a decreasing radius as you go along the period.

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18
Q

What kind of structure is silicon? Tip: It’s YUGE.

A

Silicon is macromolecular.

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19
Q

What kind of shape does silicon have? Tip: It’s like a retarded square.

A

Silicon is tetrahedral.

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20
Q

How is silicon held together?

A

Strong covalent bonds between silicon atoms hold it together.

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21
Q

Why does silicon need a lot of energy to reach melting or boiling point?

A

It has a lot of bonds, so lots of energy is needed to break ‘em all.

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22
Q

Phosphorus, Sulfur and chlorine. Other than being useful to Al Qaeda, what do these things have in common?

A

They’re molecular. And they have van der Waals forces. This means melting point is dependant on the strength of the vDW forces. And vDW forces are completely shite, so these elements all easily melt.

23
Q

Why is it harder to knock over Jermain than Liam?

A

Because although Liam is stronger, there is less of him to push over.

24
Q

Why was that relevant to Chemistry?

A

DAVID I FUCKING GET IT, ITS NOT IN THE SPEC BUT PLEASE APPRECIATE THE METHOD.

25
Q

Why does sulfur have a higher melting point than potassium? Potassium is a metal, it has metal-metal bonding.

A

Although potassium has those metal-metal bonds, sulfur has MORE shite bonds, so more energy is needed to melt it down. Sometimes, more bonds (even if they’re vDW) beats having STRONGER bonds.

26
Q

How many electrons does a Group 2 element have on its outer shell?

A
  1. It has 2.
27
Q

What gets larger as you go down? Tip: Huehuehue

A

The atomic radius.

28
Q

First ionisation energy does what down the group?

A

Decrease.

29
Q

As you go down group 2, what is added to each element?

A

An electron shell.

30
Q

Why is the attraction of the nucleus shielded as you go further down Group 2?

A

There are more inner electron shells. It also means that the outer electrons are further away from the nucleus, which greatly reduces the nucleus’ attraction.

31
Q

As you go down group 2, what happens to the charge of the nucleus?

A

It increases. However, this is negligible due to the extra shells.

32
Q

What does the extra shell mean for the atom?

A

The outer electrons are further from the nucleus, reducing the nucleus’ attraction.

33
Q

The more electron shells, the what ionisation is?

A

Easier. Less energy is required for first ionisation if there are more shells.

34
Q

As you go down the period, why does reactivity go up?

A

The first ionisation energy decreases as you go down, meaning the easier it is to lose electrons, the more reactive the element, so reactivity increases down the group.

35
Q

As you go down Group 2, what happens to melting point?

A

It decreases.

36
Q

What type of structure do Group 2 elements have?

A

Metallic structures.

37
Q

Group 2 positive ions, how are they configured?

A

Positive ions are configured in a crystal structure surrounded by delocalised electrons.

38
Q

Where are the delocalised electrons found in Group 2?

A

The outer electron shell.

39
Q

In Group 2, what is the number of delocalised electrons?

A

2.

40
Q

When a Group 2 metal reacts with water, what does it produce?

A

Metal hydroxide and hydrogen.

41
Q

Why does Caesium explode but Calcium just go “pssshth” when placed in water?

A

The further down Group 2 the metal is, the more readily it reacts with water. This is because IONISATION ENERGY decreases.

42
Q

How is titanium refined?

A

Titanium ore is converted to Titanium chloride by heating it with carbon in chlorine gas. Then the titanium chloride is purified by fractional distillation, and then reduced by MAGNESIUM at 1000C.

43
Q

Which Group 2 compounds are more soluble than others?

A

Group 2 compounds with a singly charged negative ion have the most solubility, and double charged have less solubility.

44
Q

What is barium meal used for?

A

Diagnosing problems with the stomach or intestine. This is because it comes up in X-Rays.

45
Q

Acidified Barium Chloride does what when added to a solution containing sulfate ions?

A

It turns white.

46
Q

Why must hydrochloric acid be added to the solution before testing?

A

Carbonates will produce a white preciptate, but we aren’t testing for those. Adding the hydrochloric effectively eliminates them.

47
Q

Where do we use Mg(OH)2?

A

Magnesium hydroxide (Mg(OH)₂) is used in some indigestion tablets as an antacid – this is a substance which neutralises excess stomach acid.

48
Q

Where do we use Ca(OH)2?

A

Calcium hydroxide (slaked lime, Ca(OH)₂) is used in agriculture to neutralise acid solids.

49
Q

What is the ionic equation for neutralisation?

A

Oh, cmon David, this is common sense.

〖𝐻^+〗((𝑎𝑞))+〖〖𝑂𝐻〗^−〗((𝑎𝑞))→𝐻_2 𝑂_((𝑙))

50
Q

How do we remove flue gases?

A

CaO or CaCO3.

51
Q

Why are fossil fuels bad?

A

When burning, they release sulfur dioxide.

52
Q

How can we deal with the acidic sulfur dioxide?

A

By reacting it with an alkali (wet scrubbing).

53
Q

How is powered calcium oxide useful to us?

A

It is mixed with water and then sprayed onto flue gases. The sulfur dioxide reacts with the mixture to produce… CALCIUM SULFITE.

AS Chemistry (AQA) (2 decks)

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