The Periodic Table Reactions Flashcards

1
Q

How does NaCl react in water + and pH (for all of these flashcards)

A

Dissolves readily in water to form hydrated ions in a neutral solution

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2
Q

NaCl reaction

A

NaCl(s) -> Na+(aq) + Cl-(aq)

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3
Q

MgCl2 in water reaction and pH

A

Dissolves in water with partial hydrolysis (due to the high polarising power of Mg2+ ions) to give a slightly acidic solution.
pH 6.5

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4
Q

Equation for MgCl2 in water, including that for partial hydrolysis

A

MgCl2 + 6H2O -> [Mg(H2O)6]2+ + 2Cl-

[Mg(H2O)6]2+ + H2O (REVERSIBLE REACTION) [Mg(H2O)5(OH)]+ + H3O+ (hydronium ions to give it its slight acidity)

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5
Q

AlCl3

A

Dissolves in water with partial hydrolysis to give an acidic solution, pH 3

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6
Q

AlCl3 reaction, including partial hydrolysis, and its reaction in limited water

A

AlCl3 + 6H2O -> [Al(H2O)6]3+ + 3Cl-

[Al(H2O)6]3+ + H2O (REVERSIBLE REACTION) [Al(H2O)5(OH)]2+ + H3O+

Limited cold water:
AlCl3 + 3H2O -> Al(OH)3 + 3HCl(g) (white fumes of HCl gas)

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7
Q

SiCl4, PCl5

A

Dissolves in water due to complete hydrolysis to form strongly acidic solutions, pH 2

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8
Q

SiCl4 reaction equation

A

SiCl4 + 2H2O -> SiO2 + 4HCl(aq)

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9
Q

PCl5 reactions (excess water, limited cold water then excess water)

A

Excess water: PCl5 + 4H2O -> H3PO4 + 5HCl

Limited water (1:1 ratio with H2O): PCl5 + H2O -> POCl3(l) + 2HCl(g)
Then Excess water: POCl3 + 3H2O -> H3PO4(aq) + 3HCl(aq)

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10
Q

Why is Al3+ acidic?

A

Al3+ in [Al(H2O)6]3+ has high charge density and can thus polarises the electron clouds of its surrounding water molecules, thereby weakening the O-H bonds in the water molecules which results in the release of protons

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11
Q

Na2O

A

Reacts vigorously to form strongly basic solution NaOH, pH 13

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12
Q

MgO (give equation) and reason

A

Reacts less vigorously to form a weakly alkaline solution due to more exothermic lattice energy. It is sparingly soluble, pH 9.

MgO(s) + H2O(l) (REVERSIBLE REACTION) Mg(OH)2 (aq)

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13
Q

Al2O3 reaction with water

A

Does not react with water due to very high exothermic lattice energy, making it very difficult to break the ionic lattice structure.

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14
Q

SiO2 reaction with water

A

SiO2 does not react with water due to strong and extensive covalent bonds between Si and O atoms in the lattice structure, making SiO2 insoluble in water.

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15
Q

P4O10 reaction with water

A

Covalent non-metal oxides react readily with water to form acidic solution (H3PO4), pH 2

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16
Q

SO3 reaction with water

A

Covalent non-metal oxides react readily with water to form acidic solution (H2SO4), pH 2

17
Q

P4O10 with water equation

A

P4O10 + 6H2O -> H3PO4

18
Q

SO3 with water equation

A

SO3 + H2O -> H2SO4

19
Q

How does the nature of oxides change across a period?

A

Basic to amphoteric to acidic.

20
Q

Reaction of Al2O3 with acids and bases (Amphoteric oxide: Ionic oxide with covalent character)

A

Al2O3(s) + 6HCl -> 2AlCl3(aq) + 3H2O
Al2O3(s) + 2NaOH + 3H2O -> 2NaAl(OH)4

21
Q

Reaction of SiO2 with base

A

SiO2 + 2NaOH (MUST BE CONC.) -> Na2SiO3 + H2O

22
Q

Reaction of P4O10 with base

A

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

23
Q

Reaction of SO3 with base

A

SO3(g) + 2NaOH(aq) -> Na2SO4(aq) + H2O

24
Q

Reaction of Al(OH)3 with acids and bases

A

1) Al(OH)3(s) + 3HCl -> AlCl3 + 3H2O
2) Al(OH)3(s) + NaOH -> NaAl(OH)4 (aq)