Section 3 - Period 3 Elements Flashcards

1
Q

Is Na or Mg more reactive?

A

Sodium - it takes less energy to lose one electron than to lose two.

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2
Q

How does sodium react with cold water?

A
  • vigorously
  • forms alkaline solution
  • forms a molten ball on surface
  • fizzes and produces H2 gas
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3
Q

Complete the equation:

2Na(s) + 2H2O(l) –>

A

2NaOH(aq) + H2(g)

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4
Q

What is the pH of NaOH?

A

Strongly alkaline - pH 12-14

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5
Q

How does magnesium react with cold water?

A
  • Very slowly
  • Alkaline solution is formed
  • Thin coating of magnesium hydroxide forms on surface of metal
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6
Q

What is the pH of magnesium hydroxide and why?

A

Weakly alkaline - pH 9-10

It is not very soluble in water so very few hydroxide ions are produced.

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7
Q

Complete the equation:

Mg(s) + 2H2O(l) –>

A

Mg(OH)2(aq) + H2(g)

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8
Q

What is a faster way to react magnesium with water and what does it produce?

A

React it with steam

Magnesium Oxide

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9
Q

Complete the equation:

Mg(s) + H2O(g) –>

A

MgO(s) + H2(g)

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10
Q

What do period 3 elements form when they react with oxygen?

A

Oxides

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11
Q

What is the general pattern for oxidation states of elements in oxides? (and what is the exception?)

A

Usually oxidised to their highest oxidation state (the same as their group numbers).

Sulfur is the exception - it forms SO2 which has an oxidation state of +4. A catalyst and high temp are needed to create SO3.

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12
Q

Give the equation for:

Sodium and Oxygen

A

2Na(s) + 1/2O2(g) –> Na2O(s)

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13
Q

Give the equation for:

Magnesium and Oxygen

A

Mg(s) + 1/2O(g) –> MgO(s)

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14
Q

Give the equation for:

Aluminium and Oxygen

A

2Al(s) + 3/2O2(g) –> Al2O3(s)

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15
Q

Give the equation for:

Silicon and Oxygen

A

Si(s) + O2(g) –> SiO2(s)

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16
Q

Give the equation for:

Phosphorous and Oxygen

A

P4(s) +5O2(g) –> P4O10(s)

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17
Q

Give the equation for:

Sulfur and Oxygen

A

S(s) + O2(g) –> SO2(g)

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18
Q

How does Na react in air?

A

Vigorously

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19
Q

How does Mg react in air?

A

Vigorously

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20
Q

How does Al react in air?

A

Slow (faster if powdered)

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21
Q

How does Si react with air?

A

Slowly

22
Q

How does P react in air?

A

Spontaneously combusts

23
Q

How does S react in air?

A

Burns steadily

24
Q

What does the graph of period 3 oxides mpts look like?

A

(ignore chlorine)

25
Q

Why do the metal oxides (sodium, magnesium and aluminium) have high mpts?

A

They form giant ionic lattices

Strong forces of attraction between each ion

A lot of energy required to break the bonds

26
Q

Why does MgO have a higher mpt than Na2O?

A

Mg forms 2+ ions so it bonds more strongly than the 1+ Na ions.

27
Q

Why does Al2O3 have a lower mpt?

A

The highly charged Al3+ ions distort the oxygen’s electron cloud making the bonds partially covalent.

28
Q

Why does SiO2 have the highest non-metal oxide mpt?

A

It has a giant macromolecular structure

The strong covalent bonds must be broken

This requires a lot of energy

29
Q

Why do the phosphorous and sulfur oxides have relatively low mpts?

A

They form simple molecular structures

Weak intermolecular forces (dipole-dipole and VdWs) are easy to break

30
Q

How do you determine if an oxide is acidic or alkaline?

A

Ionic oxides are alkaline, covalent oxides are acidic.

31
Q

Why do ionic oxides form alkaline solutions when dissolved in water?

A

The oxide ions (O2-) accept protons from the water molecules to form hydroxide ions.

32
Q

Give the equation for the reaction of:

sodium oxide with water

A

Na2O(s) + H2O –> 2NaOH(aq)

33
Q

Give the equation for the reaction of:

magnesium oxide and water

A

MgO(s) + H2O(l) –> Mg(OH)2(aq)

34
Q

What type of solutions do the simple covalent oxides of phosphorus and sulfur form?

A

Strong acidic

35
Q

Give the equation for the reaction of:

phosphorus (V) oxide and water

A

P4O10(s) + 6H2O(l) –> 4H3PO4(aq)

36
Q

Give the equation for the reaction of:

sulfur dioxide and water

A

SO2(g) + H2O(l) –> H2SO3(aq)

37
Q

Give the equation for the reaction of:

sulfur trioxide and water

A

SO3(l) + H2O(l) –> H2SO4(aq)

38
Q

Give the equation for the disassociation of phosphoric (V) acid:

A

H3PO4(aq) –> 3H+(aq) + PO43-(aq)

39
Q

Give the equation for the disassociation of sulfurous acid:

A

H2SO3(aq) –> 2H+(aq) + SO32-(aq)

40
Q

Give the equation for the disassociation of sulfuric acid:

A

H2SO4(aq) –> 2H+(aq) + SO42-(aq)

41
Q

What happens when you react silicon dioxide with water?

A

Nothing - it is insoluble in water

42
Q

Is silicon dioxide classed as acidic or basic?

A

acidic - it reacts with bases.

43
Q

What happens when you react aluminium oxide with water?

A

Nothing - it is insoluble

44
Q

Is aluminium oxide classed as acidic or basic?

A

Both - it is amphoteric

Due to its partially ionic and partially covalent bonding

45
Q

Give the equation of the neutralisation reaction between sodium oxide and hydrochloric acid:

A

Na2O(s) + 2HCl(aq) –> 2NaCl(aq) + H2O(l)

46
Q

Give the equation of the neutralisation reaction between magnesium oxide and sulfuric acid:

A

MgO(s) + H2SO4(aq) –> MgSO4(aq) + H2O(l)

47
Q

Give the equation of the neutralisation reaction between silicon dioxide and sodium hydroxide:

A

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

48
Q

Give the equation of the neutralisation reaction between phosphorous oxide and sodium hydroxide:

A

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

49
Q

Give the equation of the neutralisation reaction between sulfur dioxide and sodium hydroxide:

A

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

50
Q

Give the equation of the neutralisation reaction between sulfur trioxide and sodium hydroxide:

A

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

51
Q

Give the equation of the neutralisation reaction between aluminium oxide and sulfuric acid:

(aluminium oxide as a base)

A

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

52
Q

Give the equation of the neutralisation reaction between aluminium oxide and sodium hydroxide:

(aluminium oxide as an acid)

A

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