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Chemistry preparation Cap1 > Period 3 > Flashcards

Period 3 Flashcards

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1
Q

What happens to atomic radius across a period

A

Decreases: Increase in nuclear charge, same shielding, electron shells held closer to the nucleus

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2
Q

What happens to electronegativity across the period

A

Increases: Increase in nuclear charge, same amount of shielding, elements have an increased capability to withdraw electron density from a covalent bond

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3
Q

Why does melting point increase from Na to Al

A

The charge of the metal ion increases
The size of the metal ion decreases across the row
Increase in the strength of attraction between metal ions and delocalised electrons

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4
Q

Which P3 element has the highest melting point

A

Silicon- has a macromolecular structure with lots of covalent bonds which are very strong

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5
Q

What IMF do period 3 non-metals have

A

P4,S8 and Cl2 have simple molecule structures with IDD
Argon has the weakest IDD

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6
Q

Which P3 element has the highest boiling point and why

A

Once silicon has been melted most of its strong covalent bonds have been broken so boiling requires little energy. In the liquid state, Al has strong electrostatic attraction between ions and delocalised electrons and so requires a large amount of energy

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7
Q

Equation and PH for Sodium with water

A

2Na + 2H2O —> 2NaOH + H2
Ph- 13-14
Vigorous reaction- the metal fizzes rapidly and melts due to the heat released. A strong alkaline solution is formed

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8
Q

Magnesium with water

A

Mg + 2H2O —> Mg(OH)2 + H2
Slow reaction at room temp. Bubbles of gas are produced, only a weak alkali as magnesium hydroxide is only sparingly soluble
PH= 9-10

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9
Q

Magnesium with steam

A

Mg + H2O —> MgO + H2
occurs a lot faster due to the temperatures needed to generate the steam

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10
Q

Chlorine’s two reactions with water

A

1: Cl2 + H2O [reversible symbol] —> HClO + HCl
Ph= 2-3
2. In the prescence of bright sunlight
2Cl2 + 2H2O —> 4HCl + O2
PH= 2-3

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11
Q

Reaction of Sodium with Oxygen

A

For simple oxide: 2Na + 0.5O2 —> Na2O
For peroxide: 2Na + O2 —> Na2O2
Burns brightly in O2 to form a characteristic yellow flame and a white solid

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12
Q

magnesium with oxygen

A

2Mg + O2 —> 2MgO
burns brightly with a white flame that forms a white solid

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13
Q

Aluminium with oxygen

A

4Al + 3O2 —> 2Al2O3
Burns with a bright white flame to produce aluminium oxide.
Ph= 7

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14
Q

Silicon and oxygen

A

Si + O2 —> SiO2
PH- 7

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15
Q

Phosphorous and oxygen

A

Two different forms of phosphorous: red phosphorous with chains of P4 tetrahedrons
White phosphorous which is single P4 tetrahedral molecules
P4+5O2–> P4O10

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16
Q

Sulfur and oxygen

A

S + O2 —> SO2

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17
Q

Why does MgO have the highest melting point

A

MgO has ionic bonds where strong electrostatic attraction between oppositely charged ions, these require a lot of energy to overcome

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18
Q

Why does Al2O3 have more covalent character than MgO

A

Al3+ is smaller than Mg2+, meaning it is more polarising which distorts the electron cloud around the o2- ion more so that there is more electron density shared between the two ions

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19
Q

Sodium oxide with water

A

Na2O + H2O —> 2Na+ + 2OH-
Ph= 13-14

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20
Q

Magnesium oxide with watee

A

MgO + H2O —> Mg(OH)2

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21
Q

Aluminium and silicon oxide are both insoluble in water so what is there ph?

A

7

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22
Q

Potassium oxide with water

A

P4O10 + 6H2O —> 4H3PO4
Ph- 1-2

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23
Q

Sulfur dioxide with water

A

SO2 + H2O —> H2SO3
Ph- 2-3

24
Q

Sulfur trioxide with water

A

SO3 + H2O —> H2SO4
Ph- 0-1

25
Q

Sodium oxide and H2SO4

A

Na2O + H2SO4 —> Na2SO4 + H2O

26
Q

Magnesium oxide with HCl

A

MgO + 2HCl —> MgCl2 + H2O

27
Q

Amphoteric oxides, HCl and NaOH : Al2O3

A

Al2O3 + 6HCl —> 2AlCl3 + 3H2O

al2O3 + 2NaOH + 3H2O —> 2NaAl

28
Q

Phosphoric acid and NaOH and phosphorus oxide

A

H3PO4 + 3NaOH —> Na3PO4 + 3H2O
P4O10 + 12NaOH —> 4Na3PO4 + 6H2O

29
Q

Reaction of sulfur dioxide in solution

A

SO2 + 2NaOH —> Na2SO3 + H2O

30
Q

P4O10 + 6Na2O

A

4Na3PO4

31
Q

P4O10 + 6MgO —>

A

2Mg3(PO4)2

32
Q

Explain why magnesium has a higher melting point than sodium

A

Mg has a greater charge of 2+, meaning there is a stronger electrostatic attraction between positive metal ions and delocalized electrons

33
Q

A sample of the highest oxide of phosphorous was prepared in a laboratory. describe a method for determining the melting point of the sample- state how the result could be obtained to evaluate its purity

A

sample in a suitable melting point apparatus- heat slowly to establish the boiling point- lower melting point indicates impurities

34
Q

state the structure of and bonding in silicone dioxide, other than high melting point, give 2 physical properties

A

Structure: Macromolecular
Bonding: Covalent
property: Brittle, doesn’t conduct

35
Q

give the formula of the species in a sample of solid phosphorous oxide. state the structure and bonding

A

formula:P4O10
structure: molecular
Bonding: Shared paired of electrons/bonding

36
Q

Equation for the reaction between SO2 and H2O

A

SO2 + H2O –> H+ + HSO3

37
Q

state the type of bonding in magnesium oxide, outline a simple experiment to demonstrate that magnesium oxide has this type of bonding

A

melt it and see if it can conduct electricity

38
Q

Why is silicon dioxide insoluble in water

A

macromolecular structure with strong covalent bonds between molecules- water cannot break hydrogen bonding

39
Q

the melting point of P4O10 compared to silicon dioxide

A

lower- is a simple molecule with weak covalent bonds between molecules, covalent bonds are stronger in SiO2 so requires less energy to overcome in P4O10- doesn’t require much energy to break the IDD

40
Q

Equation for magnesium oxide acting as a base

A

MgO + 2HCl –> MgCl2 + H2O

41
Q

phosphorous oxide with sodium hydroxide

A

P4O10 + 12NaOH –> 4Na3PO4 + 6H2O

42
Q

state the type of bonding in these basic oxides, explain why this causes them to have basic properties

A

Ionic- Contains O2- which can form OH- in water

43
Q

sulfur dioxide and water

A

SO2 + H2O –> HSO3- + H+

44
Q

suggest why sulfur dioxide forms a weakly acidic solution

A

Reaction is in equilibrium- it is a reversible reaction

45
Q

explain why siO2 is described as an acidic oxide even though it is insoluble in water

A

SiO2 reacts with bases

46
Q

explain why phosphorous oxide has a higher melting point than sulfur oxide

A

P4O10 is a larger molecule, more electrons

47
Q

phosphoric acid and magnesium oxide

A

3H3PO4 + 2MgO –> Mg3(PO4)2 + 3H2O

48
Q

why does SO2 have a low melting point

A

weak induced dipole dipoles between molecules

49
Q

Na2O and P4O10

A

6P4O10 + Na2O –> 4Na3PO4

50
Q

observation when su;fur burns in oxygen

A

pale blue fame and fumy gas- has covalent bonding

51
Q

Al2O3 and HCl

A

Al2O3 + 6HCl –> 2Al2+ + 3H2O

52
Q

Al2O3 and sodium hydroxide

A

Al2o3 + 2OH- __. 3H2O + 2Al(OH)4

53
Q

lithium melting point higher or lower than sodium oxide

A

lower- stronger attraction to O2-

54
Q

Na2O and P4)10 - what reaction

A

6Na2O + P4O10 –> 4Na3PO4
acid base

55
Q

property of aluminum oxide coating that causes aluminum to resist the corrosion of water

A

insoluble

56
Q

why does silicon dioxide not react with HCl but does with sodium hydroxide

A

SiO2 + 2NaOH –> Na2SiO3 + H2O

57
Q

two equations to show how vanadium oxide acts as a catalyst in this process

A

1: V2O5 + SO2 –> V2O4 + SO3
2: V2O4 + 1/2O2 –> V2O5

Chemistry preparation Cap1 (16 decks)

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