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A Level Chemistry > Period 3 > Flashcards

Period 3 Flashcards

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1
Q

Which is more reactive, sodium or magnesium? Why?

A

Sodium is more reactive because it takes more energy to remove 2 electrons from magnesium to form Mg2+ than it does to remove one electron from sodium to form Na+

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2
Q

Describe how sodium reacts with cold water?

A

Sodium reacts vigorously with cold water forming a ball and fizzing. The gas produced is hydrogen, and an allkaline solution of NaOH is produced aswell.

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3
Q

Give the equation for the reaction between sodium and water:

A

2Na(s) + 2H2O(l) –> 2NaOH(aq) + H2(g)

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4
Q

Describe how magnesium reacts with cold water?

A

Magnesium reacts slowly with cold water forming a weak alkaline solution of Mg(OH)2 . It is weak because magnesium hudroxide is sparingly soluble so there are little OH- ions in solution.

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5
Q

Give the equation for the reaction between magnesium and cold water:

A

Mg(s) + 2H2O(l) –> Mg(OH)2(aq) + H2(g)

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6
Q

What does magnesium react much faster with? And what does it form?

A

Steam –> forms magnesium oxide

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7
Q

Give the equation for the reaction between magnesium and steam:

A

Mg(s) + H20(g) –> MgO(s) + H2(g)

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8
Q

What do period 3 elements react with to form oxides?

A

Oxygen

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9
Q

Which two period 3 elements don’t react directly with oxygen?

A

Argon and chlorine

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10
Q

Why is sulphur an exception to the rule that ‘period 3 elements form oxides?’

A

Because its forms SO2 (oxidation state +4) and with a higher temperature and catalyst can form SO3 (oxidation state of +6)

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11
Q

Give the equation between sodium and oxygen:

A

2Na(s) + 1/2O2(g) –> Na2O(s)

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12
Q

Give the equation between magnesium and oxygen:

A

Mg(s) + 1/2O2(g) –> MgO(s)

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13
Q

Give the equation between aluminium and oxygen:

A

2Al(s) + 1 1/2O2(g) –> Al203(s)

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14
Q

Give the equation between silicon and oxygen:

A

Si(s) + O2(g) –> SiO2(s)

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15
Q

Give the equation between phosphorus and oxygen:

A

P4(s) + 5O2(g) –> P4O10(s)

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16
Q

Give the equation between sulphur and oxygen:

A

S(s) + O2(g) –> SO2(g)

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17
Q

Describe sodiums reaction with air? And give the formula of its oxide:

A

Very fast, Na2O

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18
Q

Describe magnesiums reaction with air? And give the formula of its oxide:

A

Very fast, MgO

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19
Q

Describe aluminiums reaction with air? And give the formula of its oxide:

A

Slow but fast if powdered, Al2O3

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20
Q

Describe silicons reaction with air? And give the formula of its oxide:

A

slow, SiO2

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21
Q

Describe phosphorus’s reaction with air? And give the formula of its oxide:

A

spontaneously combusts, P4O10

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22
Q

Describe sulphurs reaction with air? And give the formula of its oxide:

A

Steadily burns, SO2

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23
Q

List the order of period 3 oxides in order of their melting points, highest to lowest:

A

MgO, Al2O3, SiO2, Na2O, P4O10, SO2

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24
Q

Describe the structure and bonding of MgO?

A

Forms a giant ionic lattice, with strong electrostatic forces of attraction, has a high MP than Na2O because the Mg2+ ions are more strongly attracted to the oxygen than the Na+ ions.

25
Q

Describe the structure and bonding of Al2O3?

A

Forms a giant ionic lattice, with strong electrostatic forces of attraction. However, Al2O3 falls lower than MgO because the Al3+ ions distort the electron cloud of oxygen so Al2O3 has some covalent character as well as the expected ionic interactions so less energy is required to break the bonds. The melting point of Al2O3 is lower than expected because the difference in electronegativity between Al and O is not as big as it is between Mg and and O. This means that the O2- ions cannot attract the electrons in the bond in Al2O3 as strongly as it can in MgO.

26
Q

Describe the structure and bonding of Na2O?

A

Forms a giant ionic lattice, with strong electrostatic forces of attraction

27
Q

Describe the structure and bonding of SiO2?

A

It’s melting point is higher than the other non-metal oxides because it forms a macromolecular structure with many stong covalent bonds which require lots of energy to break

28
Q

Describe the strcutre and bonding of P4O10 and SO2?

A

They both have simple molecular structures with weaker intermolecular forces (dipole-dipole and VDW) which do not require as much energy to overcome.

29
Q

What do ionic oxides form when added to water?

A

Alkaline solutions

30
Q

How do ionic oxides form alkaline solutions?

A

The ionic oxides contain the O2- ion which accepts protons from the water molecule.

31
Q

Give two example of ionic oxides that form alkaline solutions when added to water?

A

Na2O and MgO (sodium and magnesium oxide)

32
Q

What is the equation for the reaction between sodium oxide and water?

A

Na2O(s) + H2O(l) –> 2NaOH(aq)

33
Q

What is the equation for the reaction between magnesium oxide and water?

A

MgO(s) + H2O(l) –> Mg(OH)2(aq)

34
Q

What is formed when Na2O dissolves in water?

A

An alkaline solution of pH 12-14

35
Q

Describe the readiness of Na2O dissolving?

A

Na2O dissolves readily

36
Q

What is formed when MgO dissolves in water?

A

A weak alkaline solution of pH 9-10

37
Q

Describe the readiness of MgO dissolving?

A

MgO dissolves sparingly in H2O

38
Q

List the two simple covalent oxides?

A

Phosphorus oxide and sulphur oxide

39
Q

What do the simple covalent oxides form when they are added to water?

A

Acidic solutions

40
Q

Describe the pH of the solution formed from the acid which was formed from the simple covalent oxide? What is this assuming?

A

pH 0-2 assuming a minimum concentration of 1moldm-3

41
Q

Show the equation between phosphorus oxide and water: forming phosphoric (V) acid

A

P4O10(s) + 6H2O(l) –> 4H3PO4(aq)

42
Q

Show the equation for the dissociation of phosphoric (V) acid forming H+ ions and its conjugate base.

A

H3PO4(aq) –> 3H+(aq) + PO42-(aq)

43
Q

Show the equation between sulphur dioxide and water forming sulphuric (IV) acid:

A

SO2(g) + H20(l) –> H2SO3(aq)

44
Q

Show the equation for the dissociation of sulphuric (IV) acid:

A

H2SO3(aq) –> 2H+(aq) + SO32- (aq)

45
Q

Show the equation between sulphur trioxide and water forming sulphuric (VI) acid:

A

SO3(l) + H2O(l) –> H2SO4(aq)

46
Q

Show the equation for the dissociation of sulphuric (VI) acid:

A

H2SO4(aq) –> 2H+(aq) + SO42-(aq)

47
Q

How does silicon dioxide behave when it is added to water?

A

Because silicon dioxide forms a giant covalent structure (macromolecular), it has many strong covalent bonds which require lots of energy to overcome. Because of this, silicon dioxide is insoluble in water.

48
Q

How does aluminium oxide behave when it is added to water?

A

Aluminium oxide is amphoteric because it has both ionic and covalent character and it is insoluble in water. It will react with both acids and bases to form salts which is why it is amphoteric.

49
Q

Is silicon dioxide an acid or a base and why?

A

It will react with a base to form a salt so it is classified as an acid.

50
Q

Acid + base –>

A

Salt + water

51
Q

What is the acid-base reaction involving the basic oxide, MgO?

A

2HCl(aq) + MgO(s) –> MgCl2(aq) + H2O(l)

52
Q

What is the acid-base reaction involving the basic oxide, Na2O?

A

H2SO4(aq) + Na2O(s) –> Na2SO4(aq) + H2O(l)

53
Q

What is the acid-base reaction involving the acidic oxide, SiO2?

A

2NaOH(aq) + SiO2(g) –> Na2SiO3 (aq) + H2O(l)

54
Q

What is the acid-base reaction involving the acidic oxide, P4O10?

A

12NaOH (aq) + P4O10(s) –> 4Na3PO4 (aq) + 6H2O(l)

55
Q

What is the acid-base reaction involving the acidic oxide, SO2?

A

2NaOH (aq) + SO2(g) –> Na2SO3(aq) –> H2O(l)

56
Q

What is the acid-base reaction involving the acidic oxide, SO3?

A

2NaOH (aq) + SO3 (g) –> Na2SO4(aq) + H2O(l)

57
Q

Give the acid-base equation of aluminium oxide acting as a base:

A

3H2SO4(aq) + Al2O3(s) –> Al2(SO4)3 (aq) + 3H2O(l)

58
Q

Give the acid-base equation of aluminium oxide acting as an acid:

A

2NaOH(aq) + Al2O3(s) + 3H2O(l) –> 2NaAl(OH)4 (aq)

A Level Chemistry (17 decks)

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