Give the equation for the reaction that occurs when sodium oxide reacts with hydrochloric acid.

Na2O(s) + 2HCl(aq) ➔ 2NaCl(aq) + H2O(l)

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Why is aluminium oxide known as an amphoteric oxide?

Because it reacts with both acids and alkalis.

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Give the equation for the reaction between aluminium oxide and hydrochloric acid?

Al2O3(s) + 6HCl(aq) ➔ 2AlCl3(aq) + 3H2O(l)

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Give the equation for the reaction between aluminium oxide and hot, concentrated sodium hydroxide.

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


NaAl(OH)4 is called sodium aluminate.

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What is the equation for the reaction of phosphoric(V) acid with excess sodium hydroxide?

H3PO4(aq) + 3NaOH(aq) ➔ Na3PO4(aq) + 3H2O(l)


The reaction occurs in three stages, as each hydrogen of H3PO4 in turn reacts with a hydroxide ion and is replaced by a sodium ion.

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What is the equation for the reaction of sulfur dioxide with excess sodium hydroxide?

SO2(aq) + 2NaOH(aq) ➔ Na2SO3(aq) + H2O(l)


Na2SO3 is called sodium sulfite.

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How does the type of bonding in the oxides of period 3 change as you move across the period?

As you move across the period, the oxides of period 3 change from ionic (Na2O, MgO and Al2O3) to covalent (SiO2, P4O10, SO2 and SO3).


Al2O3 is an ionic oxide with a degree of covalent character.

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Describe the bonding and structure of the oxides of period 3 from sodium to sulfur.

Period 3 oxideNa2OMgOAl2O3SiO2P4O10SO2SO3
BondingIonicIonicIonic (with covalent character)CovalentCovalentCovalentCovalent
StructureGiant ionicGiant ionicGiant ionicGiant covalentSimple molecularSimple molecularSimple molecular

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What type of solution is formed when sodium oxide reacts with water? Explain your answer with an equation.

A strongly alkaline solution of sodium hydroxide is formed:

Na2O(s) + H2O(l) ➔ 2NaOH(aq)

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Explain the difference in pH of the solutions formed when magensium oxide and sodium oxide react with water.

Both reactions produce alkaline solutions as the metal hydroxide is formed.

NaOH is soluble and produces a solution with a pH of ≈14.

Mg(OH)2 is only sparingly soluble so produces a solution with a pH of ≈10.

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What type of solution is formed when phosphorus pentoxide reacts with water? Explain your answer with an equation.

An acidic solution of phosphoric(V) acid is formed:

P4O10(s) 6H2O(l) ➔ 4H3PO4(aq)

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What type of solution is formed when sulfur dioxide reacts with water? Explain your answer with an equation.

An acidic solution of sulfurous acid is formed:

SO2(g) + H2O(l) ➔ H2SO3(aq)


Sulfurous acid is also called sulfuric(IV) acid.

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What type of solution is formed when sulfur trioxide reacts with water? Explain your answer with an equation.

An acidic solution of sulfuric acid is formed:

SO3(g) + H2O(l) ➔ H2SO4(aq)

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What type of oxides (metal or non-metal) form alkaline solutions in water?

Metal oxides

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What type of oxides (metal or non-metal) form acidic solutions in water?

Non-metal oxides

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State the trend in the the oxidation state of period 3 elements in their oxides from sodium to phosphorus?

The oxidation states of period 3 elements in their oxides increases from +1 in sodium oxide to +5 in phosphorus pentoxide.

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What is the pH of the resulting solution formed in the reaction of sodium and water?

The reaction produces a strongly alkaline solution with a pH of 12-14.

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What is the pH of the resulting solution formed in the reaction of magnesium and water?

The reaction produces a weakly alkaline solution with a pH of ≈10.

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Describe, and give the equation for, the reaction of sodium with oxygen.

Sodium burns brightly with a yellow flame to form white sodium oxide.

2Na(s) +  1⁄2O2(g) ➔ Na2O(s)

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Describe, and give the equation for, the reaction of magnesium with oxygen.

Magnesium burns with a bright white flame producing white magnesium oxide powder.

2Mg(s) + O2(g) ➔ 2MgO(s)

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Describe, and give the equation for, the reaction of aluminium powder with oxygen.

Aluminium powder burns brightly to produce white aluminium oxide powder.

4Al(s) + 3O2(g) ➔ 2Al2O3(s)

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Give the equation, including state symbols, for the reaction of silicon with oxygen.

Si(s) + O2(g) ➔ SiO2(s)

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Describe, and give the equation for, the reaction of phosphorus with oxygen.

Phosphorus ignites spontaneously in air producing white clouds of phosphorus pentoxide.

4P(s) + 5O2(g) ➔ P4O10(s)

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Describe, and give the equation for, the reaction of sulfur with oxygen at room temperature.

Sulfur burns with a blue flame to produce sulfur dioxide.

S(s) + O2(g) ➔ SO2(g)

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Give the equation for the reaction of magnesium with water at room temperature.

Mg(s) + 2H2O(l) ➔ Mg(OH)2(aq) + H2(g)

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Give the equation for the reaction of sodium with water at room temperature.

2Na(s) + 2H2O(l) ➔ 2NaOH(aq) + H2(g)

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Name the period 3 oxides that are insoluble in water.

Aluminium oxide and silicon dioxide

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Describe, and give the equation for, the reaction of phosphorus(V) oxide with water.

Phosphorus(V) oxide (P4O10) dissolves in water to form a strongly acidic solution of phosphoric(V) acid.

P4O10(s) + 6H2O(l) ➔ 4H3PO4(aq)

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What is the general trend in the pH of the solutions formed by the oxides of period 3 elements as you move across the period?

As you move across period 3, the pH of the solutions formed by the oxides decreases.


The solutions go from alkaline (Na2O and MgO) to acidic (P4O10. SO2 and SO3). 

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Give the equation for the reaction of sulfur trioxide and water.

SO3(g) + H2O(l) ➔ H2SO4(aq)

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Give the equation for the reaction of sulfur dioxide and water.

SO2(g) + H2O(l) ➔ H2SO3(aq)

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