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Inorganic Chemistry > 3.2.4 Properties of period 3 elements and their oxides > Flashcards

3.2.4 Properties of period 3 elements and their oxides Flashcards

1
Q

Is sodium or magnesium more reactive?

A

Sodium (G1) is more reactive than magnesium (G2).
When they react they lose electrons to form Na+ and Mg2+.

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2
Q

Why is sodium more reactive than magnesium?

A

The amount of energy required to remove an outer electron from sodium is lower than it is to remove 2 electrons from magnesium. More energy is required for magnesium to react.

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3
Q

Explain the reaction between Sodium + water

A

reacts vigorously with cold water.
Forms a ball and fizzing
Gas produced is hydrogen (H2) and alkaline solution (NaOH).

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4
Q

Write out an equation to show the reaction of sodium with water.

A

2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)

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5
Q

Explain the reaction between magnesium and water.

A

reacts slowly with cold water, weak alkaline solution of Mg(OH)2 is formed = due to Mg(OH)2 being sparingly soluble = little OH- ions in solution.

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6
Q

Write an eqaution to show the reaction between magnesium and water.

A

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

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7
Q

Explain the reaction between magnesium and steam.

A

reacts more faster forming MgO

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8
Q

Write an equation to show the reaction between magnesium and steam.

A

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

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9
Q
A
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10
Q

When period 3 elements react with oxygen what do they form?

A

Oxides.

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11
Q

What element in period 3 is excepted with their reaction with oxygen and why?

A

Sulfur forms SO2 (oxidation state = +4).
With higher temperature and catalyst = oxidation state = +6

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12
Q

Sodium + oxygen

A

2Na(s) + 1/2O2(g) -> 2Na2O(s)
sodium oxide
Reaction with air: very fast

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13
Q

Magnesium and oxygen

A

Mg(s) + 1/2O2(g) -> MgO(s)
magenisum oxide
Reaction with air: Very fast

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14
Q

Aluminium and oxygen

A

2Al(s) + 1/2O2(g) -> Al2O3(s)
Aluminium oxide
Reaction with air: Slow (fast if powered as larger SA)

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15
Q

Silicon and oxygen

A

Si(s) + O2(g) -> SiO2(s)
Silicon dioxide
Reaction with air: slow

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16
Q

Phosphate and oxygen

A

P4(s) + 5O2(g) -> P4O10(s)
Phosphorous (v) oxide.
Reaction with air: Spontaneously combusts.

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17
Q

Sulfur and oxygen

A

S(s) + O2(g) -> SO2(g)
sulfur dioxide
Reaction with air: Steadily burns.

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18
Q

What affects the melting point of period 3 oxides?

A

Their structure and bonding.

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19
Q

Explain the structure and bonding of Na2O, MgO and Al2O3 compared to their melting points.

A

High melting points Na2O, MgO and Al2O3 as they form giant ionic lattices, strong electrostatic forces between oppositely charged ions, lots of energy required to overcome these bonds.

20
Q

Why does MgO have a higher melting point than Na2O?

A

Mg forms 2+ ions and Na forms 1+ ions.
2+ ions are strongly attracted to oxygen.
Less energy needed for Na to lose 1 electron than it does for Mg to lose 2 electrons.

21
Q

Why does Al2O3 have a lower melting point than MgO?

A

The Al3+ ions distort the electron cloud of oxygen.
Some covalent character = 3+ charge means that electrons from oxygen are pulled towards Al2.
Less energy is required to break the bonds.

22
Q

Explain the structure and bonding of SiO2 compared to its melting point.

A

Non-metal.
Macro molecular structure = giant covalent structure formed.
Many covalent bonds.
Lots of energy required to break these bonds.

23
Q

Why do P4O10 and SO2 have a lower melting point than SiO2?

A

They form simple molecular structures
weaker intermolecular forces
Less energy is required to break these bonds.

24
Q

What are ionic oxides?

A

Na and Mg form alkaline solutions when added to water.
Contain O2- ion which accepts protons from the water molecule when dissolved in solution.

25
Q

Sodium oxide + water

A

Na2O(s) +H2O(l) -> 2NaOH(aq)

sodium oxide readily dissolves in water to form alkaline solution = NaOH. pH 12-14.

26
Q

Magnesium oxide + water

A

MgO(s) + H2O(l) -> Mg(OH)2(aq)

Magnesium oxide dissolves sparingly in water so alkaline solution formed (pH = 9-10) is not as strong as sodium oxide (pH = 12-14)

27
Q

What are simple covalent oxides?

A

form acidic solutions when added to water. (P and S)
Form solutions with a pH of 0-2 (assuming minimum concentration of 1moldm-3)

28
Q

Phosphorous oxide + water

A

P4O10(s) + 6H2O(l) ->4H3PO4(aq)
H3PO4(aq) -> 3H+ + PO4^2-
Phosphoric acid

29
Q

sulfur dioxide + water

A

SO2(g)+ H2O(l) -> H2SO3(aq)
H2SO3(aq) -> 2H+(aq) + SO3^2- (aq)
sulfuric acid / sulfurous acid

30
Q

Sulfur trioxide and water

A

SO3(l) + H2O(l) -> H2SO4(aq)
H2SO4(aq) -> 2H+ + SO4^2-(aq)
sulfuric (VI) acid
OS of sulphur = +6

31
Q

Silicon dioxide and water

A

Insoluble

Have giant covalent structures = strong covalent bonds = large amount of energy to overcome bonds = why silicion dioxide is insoluble in water.

Will react with base to form salt = so classed as acid.

32
Q

Aluminium oxide and water

A

Insoluble
Amphoteric will react with both acid and base to form salt
Has both covalent and ionic character.

33
Q

What does an acid + base form?

A

Salt + water.

34
Q

MgO(s) + H2SO4(aq) ->

A

MgSO4(aq) + H2O (l)

35
Q

Reaction with basic oxides

2HCl (aq) + MgO (s) ->

A

MgCl2(aq) + H2O (l)

36
Q

Reaction with basic oxides

H2SO4(aq) + NaO2(s) ->

A

Na2SO4(aq) + H2O (l)

37
Q

Na2O(s) + 2HCl (aq) ->

A

2NaCl(aq) + H2O (l)

38
Q

Reactions with acid oxides

2NaOH(aq) + SiO2(s) ->

A

Na2SiO3(aq) + H2O(l)

sodium silicate

39
Q

Reactions with acidic oxides

12NaOH(aq) + P4O10(s) ->

A

4Na3PO4(aq) + 6H2O(l)

salt will always be phosphate and metal
if it was Potassium it would be 4K3Po4 + 6H2O

40
Q
  1. What is phospohric acid.
  2. How many H+ ions can it donate?
  3. Outline the reaction with sodium hydroxide.
A
  1. Tribasic
  2. 3H+ions
  3. H3PO4(aq) + NaOH (aq) -> NaH2PO4(aq) + H2O (l)
    * NaH2PO4 (aq) + NaOH (aq) -> Na2HPO4(aq) + H2O (l)
    * Na2HPO4 (aq) + NaOH (aq) -> Na3PO4(aq) + H2O (l)
  4. Overall Reaction: 3NaOH(aq) + H3PO4(aq) -> Na3PO4(aq) + 3H2O(l)
41
Q

Reactions with acidic oxides

2NaOH(aq) + SO2(g) ->

A

Na2SO3(aq) + H2O (l)

42
Q

Reaction with acidic oxides

2NaOH(aq) + SO2(g) ->

A

Na2SO3(aq) + H2O(l)
sodium sulfate

43
Q

Reactions with acidic oxides.

2NaOH(aq) +SO3(g) ->

A

Na2SO4(aq) + H2O (l)
sodium sulfate.

44
Q

Reaction with acidic oxides

2NaOH(aq) + Al2O3(s) + 3H2O(l) ->

A

2NaAl(OH)4 (aq)

Aluminium oxide acts as your acid.
No water produced.
Reacts with hot conc. NaOH

45
Q

3H2SO4(aq) + Al2O3(s) ->

A

Al2(SO4)3(aq) + 3H2O(l)

Inorganic Chemistry (6 decks)

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