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Inorganic Chemistry > Period 3 > Flashcards

Period 3 Flashcards

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1
Q

Explain why sodium is more reactive than magnesium.

A

→ Na has a lower nuclear charge
→ weaker attraction between nucleus & outer electron
→ ∴ outer e- is lost more easily than in Mg

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2
Q

Describe the reaction between sodium and cold water. Give the equation.

A

→ reacts vigorously, forms a ball + fizzes
2Na + 2H₂O → 2NaOH + H₂

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3
Q

Describe the reaction between magnesium and cold water. Give the equation.

A

→ reacts slowly, forms weak alkaline solution
Mg + 2H₂O → Mg(OH)₂ + H₂

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4
Q

Describe the reaction between magnesium and steam. Give the equation.

A

→ fast reaction
Mg (s) + H₂O (g) → MgO (s) + H₂ (g)

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5
Q

Explain why the reaction between magnesium and water produces a weak alkaline solution.

A

→ Mg(OH)₂ is produced which is sparingly soluble
→ ∴ low concentration of OH- in solution

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6
Q

State the formulas of the compounds formed when period 3 elements react with oxygen.

A

→ Na₂O
→ MgO
→ Al₂O₃
→ SiO₂
→ P₄O₁₀
→ SO₂

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7
Q

How is SO₃ made?

A

→ reaction between sulfur & oxygen
→ at high temperature
→ with a catalyst

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8
Q

Explain why MgO has a higher melting point than Na₂O.

A

→ MgO lattice consists of 2+ ions which are more strongly attracted to oxygen ions
→ stronger ionic bonding ∴ more energy required

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9
Q

Explain why Al₂O₃ has a lower melting point than MgO.

A
  • Al³⁺ ions distort oxygen’s electron cloud
  • this means there is some covalent character
  • ∴ less energy required to break the bonds
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10
Q

Explain why silicon dioxide has a high melting point (compared to other non-metal oxides).

A

→ macromolecular structure
→ with many strong covalent bonds
→ requires high amounts of energy to breaks

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11
Q

Explain why P₄O₁₀ and SO₂ have low melting points.

A

→ simple molecular structures
→ so weak intermolecular forces (VDW)
→ less energy required

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11
Q

How do period 3 oxides react with water?

A

ionic oxides → form hydroxides
non-metal oxides → form acids

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12
Q

Give the equation for the reaction between sodium oxide and water. State the pH of the solution formed.

A

Na₂O + H₂O → 2NaOH
pH 13

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13
Q

Give the equation for the reaction between magnesium oxide and water. State the pH of the solution formed.

A

MgO + H₂O → Mg(OH)₂
pH 9

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14
Q

Give the equation for the reaction between phosphurus oxide and water. State the pH of the solution formed.

A

P₄O₁₀ + 6H₂O → 4H₃PO₄
pH 0

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15
Q

Give the equation for the reaction between sulfur dioxide and water. State the pH of the solution formed.

A

SO₂ + H₂O → H₂SO₃
pH 3

16
Q

Give the equation for the reaction between sulfur trioxide and water. State the pH of the solution formed.

A

SO₃ + H₂O → H₂SO₄
pH 0

17
Q

State why silicon dioxide and aluminium oxide do not react with water.

A

insoluble in water due to their structures

18
Q

Explain what is meant by the term amphoteric.

A

acts as both a base and an acid

19
Q

State which period 3 oxide is classified as amphoteric.

A

aluminium oxide

20
Q

Reaction between magnesium oxide and hydrochloric acid.

A

MgO + 2HCl → MgCl₂+ H₂O

21
Q

Reaction between sodium oxide and hydrochloric acid.

A

Na₂O + 2HCl → 2NaCl + H₂O

22
Q

Reaction between sodium oxide and sulfuric acid.

A

Na₂O + H₂SO₄ → Na₂SO₄ + H₂O

23
Q

Reaction between phosphurus oxide and sodium hydroxide.

A

P₄O₁₀ + 12NaOH → 4Na₃PO₄ + 6H₂O

24
Q

Reaction between phosphurus oxide and sodium oxide.

A

P₄O₁₀ + 6Na₂O → 4Na₃PO₄

25
Q

Reaction between sulfur dioxide and sodium hydroxide.

A

SO₂ + 2NaOH → Na₂SO₃ + H₂O

26
Q

Reaction between sulfur trioxide and sodium hydroxide.

A

SO₃ + 2NaOH → Na₂SO₄ + H₂O

27
Q

Reaction between silicon dioxide and sodium hydroxide.

A

SiO₂ + 2NaOH → Na₂SiO₃ + H₂O

28
Q

Give the equation for the reaction of aluminium oxide as an acid.

A

Al₂O₃ + 2NaOH + 3H₂O → 2NaAl(OH)₄

29
Q

Give the equation for the reaction of aluminium oxide as a base with sulfuric acid.

A

3H₂SO₄ + Al₂O₃ → Al₂(SO₄)₃ + 3H₂O

30
Q

Give the equation for the reaction of aluminium oxide as a base with hydrochloric acid.

A

Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O

31
Q

Describe the appearance of the reaction between sodium and oxygen.

A

→ yellow flame
→ produces a white solid

32
Q

Describe the appearance of the reaction between sulfur and oxygen.

A

→ burns with a blue flame
→ forms an acidic choking gas

33
Q

Describe the appearance of the reaction between the elements oxygen and Mg, Al, Si, P respectively.

A

→ white flame
→ white solid smoke

34
Q

Explain, using an equation, why silicon(IV) oxide is classified as an acidic oxide.

A

Reacts with bases
SiO2 + 2NaOH → Na2SiO3 + H2O

Inorganic Chemistry (13 decks)

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