A-level Chemistry: 3.2.4 Properties of Period 3 Elements Part 2
This flashcard set compares the reactivity of sodium and magnesium, explaining why sodium is more reactive and how each metal behaves when reacting with cold water. It includes observations, explanations, and relevant chemical equations.
State the equation for when sulfur dioxide reacts with water. Include pH.
SO₂ + H₂O → H₂SO₃
pH ≈ 3
Key Terms
State the equation for when sulfur dioxide reacts with water. Include pH.
SO₂ + H₂O → H₂SO₃
pH ≈ 3
State the equation for when sulfur trioxide reacts with water. Include pH.
SO₃ + H₂O → H₂SO₄
pH ≈ 0
State the equation for the dissociation of phosphoric(V) acid
H₃PO₄ ⇌ H⁺ + H₂PO₄⁻
State the equation for the dissociation of sulfurous acid (or sulfuric(IV) acid)
H₂SO₃ ⇌ H⁺ + HSO₃⁻
State the equation for the dissociation of sulfuric(VI) acid
H₂SO₄ → H⁺ + HSO₄⁻
HSO₄⁻ ⇌ H⁺ + SO₄²⁻
State which Period 3 oxides are insoluble in water
Aluminium oxide
Silicon dioxide
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| Term | Definition |
|---|---|
State the equation for when sulfur dioxide reacts with water. Include pH. | SO₂ + H₂O → H₂SO₃ |
State the equation for when sulfur trioxide reacts with water. Include pH. | SO₃ + H₂O → H₂SO₄ |
State the equation for the dissociation of phosphoric(V) acid | H₃PO₄ ⇌ H⁺ + H₂PO₄⁻ |
State the equation for the dissociation of sulfurous acid (or sulfuric(IV) acid) | H₂SO₃ ⇌ H⁺ + HSO₃⁻ |
State the equation for the dissociation of sulfuric(VI) acid | H₂SO₄ → H⁺ + HSO₄⁻ |
State which Period 3 oxides are insoluble in water |
|
Silicon dioxide is because it… | Silicon dioxide is acidic because it reacts with bases to form salts |
Explain why Al2O3 and SiO2 do not dissolve in water |
|
Aluminium oxide is because it…. | amphoteric ∵ reacts with acids and bases to form salts |
Basic oxides netutralise _____ | acids |
Basic oxides netutralise acids: Na2O(s) + 2HCl(aq) → …. | Na2O(s) + 2HCl(aq) → 2NaCl(aq) + H2O(I) |
Basic oxides netutralise acids: MgO(s) + H2SO4(aq) → …. | MgO(s) + H2SO4(aq) → MgSO4(aq) + H2O(l) |
SiO₂ + 2NaOH → Na₂SiO₃ + H₂O | |
P₄O₁₀ + 12NaOH → 4Na₃PO₄ + 6H₂O | |
SO₂ + 2NaOH → Na₂SO₃ + H₂O | |
SO₂₍g₎ + 2NaOH₍aq₎ → Na₂SO₃₍aq₎ + H₂O₍l₎ | |
Al2O3+3H2SO4→Al2(SO4)3+3H2O | |
Al2(SO4)3+3H2O | |
State what you would observe when sodium reacts with oxygen (excluding its speed e.g. vigorous) | Sodium burns with a yellow flame to produce a white solid |
State what you would observe when Mg, Al, Si and P reacts with oxygen (excluding its speed) | Mg, Al, Si and P burn with a white flame to give white powder (Mg & Al) / smoke |
State what you would observe when sulfur reacts with oxygen (excluding its speed) | S burns with a blue flame to form an acidic choking gas |
Explain why aluminium metal appears unreactive |
|
All elements from Na to S, react directly with chlorine if _ to form chlorides | heated |
From Na to S, why does the bonding change from ionic to covalent? | Bonding is due to decrease in electronegativity from Na to S |
Describe how sodium chloride and magnesium chloride reacts with water |
|
Why is the solution produced from aluminium chloride reacting with water acidic? | Al3+ ion pull electrons towards it from Al---O bonds = loss of H+ ion = acidic solution |
State the equation for when aluminium chloride reacts with (a little bit of) water | AlCl3(s) + 3H2O(l) → Al(OH)3(s) + 3H+(aq) + 3Cl-(aq) |
Describe how silicon tetrachloride reacts with water | It reacts violently with cold water to form a strongly acidic solution & colourless 'silica' gel |
State the equation for when silicon tetrachloride reacts with water | SiCl4(l) + 2H2O(l) → SiO2(s) + 4H+(aq) + 4Cl-(aq) |
Describe what happens when phosphorus pentachloride reacts with water | It reacts with boiling water to produce phosphoric acid and hydrochloric acid |
State the equation for when phosphorus pentachloride reacts with water | PCl5(s) + 4H2O(l) → H3PO4(aq) + 5H+(aq) + 5Cl-(aq) |
Suggest why the melting point of magnesium oxide is much higher than the melting point of magnesium chloride (2) |
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Na2O + H2O & P4O10 + H2O are _ _______ reactions | Na2O + H2O & P4O10 + H2O are vigorous exothermic reactions |
Aluminium oxide is partially and partially _ bonded | Aluminium oxide is partially ionic and partially covalently bonded |
Aluminum chlorides are with ________ | Aluminum chlorides are largely ionic with lots of covalent character |
AlCl3 and Al2Cl6 form in the ___ phase | gas |
Describe the bonding in AlCl3 | Has 6 outer electrons & forms a dimer - co-ordinate covalent bonds form between lone pairs of electrons in chlorine atoms and (electron-deficient) aluminium atoms |
Draw Al2Cl6 | |
Draw [Al(H2O)6]3+ | |
State the equation for when aluminium chloride reacts with excess water and state the pH of the solution (2) | AlCl3 + 6H2O → [Al(H2O)6]3+ + 3Cl- Below 6.9 |
Write an ionic equation to show how aluminium oxide reacts with aqueous sodium hydroxide (1) | Al2O3 + 2OH– +3H2O → 2Al(OH)4– |
State why NaCl forms a neutral solution | no reaction or no hydrolysis or only dissolving occurs |
Suggest why sulfur dioxide forms a weakly acidic solution (1) | Reaction is an equilibrium / reversible reaction displaced mainly to the left / partially ionised / dissociated |
Write an ionic equation for the reaction of phosphorus(V) oxide with an excess of sodium hydroxide solution (1) | P4O10 + 12OH– → 4PO43- + 6H2O |