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Inorganic Chemistry > Period Three Oxides > Flashcards

Period Three Oxides Flashcards

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1
Q

Predict the pH of the solution when phosphorus oxide reacts with water and write an equation (2)

A

P₄O₁₀(s) + 6H₂O(l) -> 4H₃PO₄(aq)
Acidic (0-2)

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2
Q

Explain why excess MgO can be used to neutralise acidic compounds. (1)

A

Weakly ionising

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3
Q

Describe the observations and give the equation for the reaction of magnesium with water at a high temperature. (3)

A

Mg(s) + H₂O(l) -> MgO(s) + H₂(g)
-White precipitate
-White flame

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4
Q

Give the formula, structure and bonding shown in phosphorus oxide. (4)

A

-P₄O₁₀
-simple molecular structure
-covalent bonding
-VDWs between molecules

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5
Q

Write an equation for the reaction between sulphur dioxide and water. (1)

A

SO₂(g) + H₂O(l) -> H₂SO₃(aq)

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6
Q

Write an equation for the reaction between aluminium oxide and hydrochloric acid.(1)

A

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

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7
Q

Write an equation for the reaction between Na₂O and HCl. (1)

A

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

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8
Q

Write two equations to show the amphoteric nature of aluminium oxide (2)

A

Al₂O₃(aq) + 6HCl(aq) -> 2AlCl₃(aq)
+ 3H₂O(l)

Al₂O₃ + 2NaOH + 3H₂O -> 2Na⁺ + 2[Al(OH)₄]⁻

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9
Q

Explain why phosphorus oxide has a higher melting point than sulfur oxide. (2)

A

P₄O₁₀ is a bigger molecule
Therefore, VDWs between molecules are stronger

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10
Q

State the type of bonding in sodium oxide and explain why it reacts to form an alkaline solution in water. (3)

A

ionic
O²⁻ reacts with water (accepts protons)
forming OH⁻ ions

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11
Q

Compare and explain the melting points of phosphorus oxide and sulphur dioxide. (3)

A

lower melting point
molecular with covalent bonding
weak van der Waals between molecules

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12
Q

Write an equation for the reaction between aluminium and oxygen. (1)

A

2Al(s) + 3/2O₂(g) + Al₂O₃(aq)

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13
Q

Explain why sodium oxide has a high melting point. (2)

A

Ionic lattice
strong forces of attraction between oppositely charged ions

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14
Q

Write the equation for the reaction between phosphorus oxide and magnesium oxide. (1)

A

P₄O₁₀(s) + 6MgO(s) -> 2Mg₃(PO₄)₂(s)

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15
Q

Predict the pH of the solution when sodium oxide reacts with water and write an equation. (2)

A

Na₂O(s) + H₂O(l) -> 2Na(OH)
pH 14

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16
Q

Give the equation for phosphoric acid with magnesium oxide. (1)

A

MgO(s) + H₃PO₄(aq) -> MgHPO₄(aq) + H₂O(l)

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17
Q

Write an equation for the reaction between silicon dioxide and sodium hydroxide. (1)

A

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

18
Q

Explain why sodium oxide has a high melting point. (2)

A

ionic lattice
strong attraction between oppositely charged ions

19
Q

Explain why the melting point of silicon dioxide is high (2)

A

giant covalent structure
strong covalent bonds

20
Q

Write an equation for the reaction of phosphorus oxide with sodium hydroxide

A

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

21
Q

Write an equation for the acid-base reaction that occurs between sodium oxide and phosphorus oxide. (1)

A

6Na₂O(s) + P₄O₁₀(s) -> 4Na₃PO₄(s)

22
Q

Outline an experiment that could be used to show that aluminium oxide contains ions. (2)

A

-heat until molten
-if its conducts electricity then the compound contains ions

23
Q

Explain why sulphur trioxide has a higher melting point than sulphur dioxide. (2)

A

-sulphur trioxide is a larger molecule
-so van der Waals forces between molecules are stronger

24
Q

Explain why the melting point of phosphorus oxide is higher than the melting point of sulphur dioxide. (2)

A

-phosphorus oxide is a bigger molecule
-stronger van der Waals between molecules

25
Q

Write an equation for the reaction of sulfur oxide with water and give the pH of the solution formed. (2)

A

SO₂(g) + H₂O(l) -> H₂SO₄(aq)
pH 1

26
Q

Write an equation to show MgO acting as a base with another reagent. (2)

A

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

27
Q

Explain, with the aid of an equation, why silicon oxide is an acidic oxide. (2)

A

-reacts with bases
-SiO₂ + 2NaOH -> Na₂SiO₃ + H₂O

28
Q

Write an ionic equation to show how aluminium oxide reacts with hydrochloric acid. (1)

A

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

29
Q

Explain why the melting point of phosphorus oxide is low. (1)

A

weak van der Waals between molecules

30
Q

Describe observations when sulfur burns in oxygen. Write an equation for the reaction that occurs and state the type of bonding in the oxide formed. (4)

A

-blue flame
-choking gas
-S + O₂ -> SO
-covalent

31
Q

Write an equation for the reaction between sodium and oxygen. State the observations observed. (3)

A

2Na + ½O₂ -> Na₂O
-white ash
-yellow flame

32
Q

Explain why sodium oxide and phosphorus oxide have different melting points. (6)

A

-sodium oxide forms an ionic lattice
- strong forces of attraction
-big difference in electronegativity between sodium and phosphorus
-P₄O₁₀ simple molecular covalent
-weak van der Waals between molecules
-melting point of sodium oxide is greater than phosphorus oxide

33
Q

State the structure and bonding in sulfur dioxide and 2 properties. (4)

A

-simple molecular structure
-covalent bonding
-hard
-insoluble

34
Q

Suggest why SO₂ is insoluble in water. (3)

A

-simple molecular structure
-covalent
-water doesn’t supply sufficient energy to break the strong bonds

35
Q

State the meaning of the term amphoteric. (1)

A

reacts with acids and bases

36
Q

Write an equation for the reaction between phosphorus oxide and water. (1)

A

P₄O₁₀ + 6H₂O -> 4H₃PO₄

37
Q

Write an ionic equation to show how aluminium oxide reacts with aqueous sodium hydroxide. (1)

A

Al₂O₃ + 2OH⁻ + 3H₂O -> 2Al(OH)₄⁻

38
Q

Write an equation for the reaction between sodium and water. (1)

A

2Na + 2H₂O -> 2NaOH+ H₂

39
Q

Write an equation for the reaction between sodium oxide and phosphorus oxide. State the general type of reaction shown. (2)

A

6Na₂O + P₄O₁₀ -> 4Na₃PO₄
acid-base

40
Q

Suggest why silicon dioxide does not react with HCl. (1)

A

it is acidic

Inorganic Chemistry (1 decks)

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