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Chemistry A level > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

Why is Sodium more reactive than Magnesium?

A

As the amount of energy required to remove an electron from sodium is lower than it is to remove 2 with magnesium.

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2
Q

State the equation for Sodium reacting with water

A

2Na (s) + 2H2O (l)  2NaOH (aq) + H2 (g)

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3
Q

What observations can be made when sodium reacts with water?

A

It reacts vigorously forming a ball and fizzing, forming a strong alkaline solution (pH = 12 – 14)

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4
Q

State the equation for Magnesium reacting with water

A

Mg (s) + 2H2O (l)  Mg(OH)2 (s) + H2 (g)

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5
Q

State the equation when Magnesium reacts with steam

A

Mg (s) + H2O (l)  MgO (s) + H2 (g)

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6
Q

What observations can be made when magnesium reacts with water/steam?

A

Few bubbles and reacts slowly with water forming a weak alkaline solution as its not very soluble (pH = 9) Much faster with steam to form magnesium oxide

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7
Q

Why does magnesium react slowly in water?

A

This is because it requires more energy to lose 2 electrons

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8
Q

State the equation for Sodium reacting with Oxygen

A

4Na + O2 –> 2Na2O

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9
Q

What observations can be made when sodium reacts with oxygen?

A

Burns with yellow-orange flame to produce white powder

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10
Q

State the equation for Magnesium reacting with Oxygen

A

2Mg + O2  2MgO

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11
Q

What observations can be made when Magnesium reacts with oxygen?

A

Burns with white flame to produce white powder

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12
Q

State the equation for Aluminium reacting with Oxygen

A

4Al + 3O2  2Al2O3

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13
Q

What observations can be made when Aluminium reacts with oxygen?

A

Burns with white flame to produce white powder

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14
Q

State the equation for Silicon reacting with Oxygen

A

Si + O2  SiO2

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15
Q

What observations can be made when silicon reacts with oxygen?

A

Burns with white flame to produce white powder

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16
Q

State the equation for Phosphorus reacting with Oxygen

A

P4 + 5O2  P4O10

17
Q

What observations can be made when Phosphorus reacts with oxygen?

A

Burns with very bright white flame to produce white powder

18
Q

State the equation for Silicon reacting with Oxygen

A

S + O2  SO2

19
Q

What observations can be made when silicon reacts with oxygen?

A

Burns with blue flame & gives off choking gas

20
Q

Explain the trends in the Melting Points of Period 3 oxides

A
  • First 3 have high melting points as they form giant ionic lattices which have lots of strong attractive forces requiring a lot of energy to break.
  • MgO has a higher m.p than Na2O as Mg forms 2+ ions and Na forms 1+ ions. 2+ ions more strongly to the oxygen
  • Al2O3 lower as it has more covalent character therefore requires less energy to break bonds
  • SiO2 has a higher melting point than the other non metal oxides and this is because it forms a giant covalent structure with many strong covalent bonds requiring a lot of energy to break
  • P4O10 & SO2 have lower melting points as they form simple molecular structures with weaker intermolecular forces requiring less energy to break the bonds.
21
Q

State the equation for Sodium Oxide reacting with water? What happens?

A

Na2O + H2O  2NaOH (aq), dissolves and forms a solution

22
Q

State the equation for Magnesium Oxide reacting with water? What happens?

A

MgO (s) + H2O (l)  Mg(OH)2 (aq), slightly soluble, some dissolves forming a solution, less soluble than Na2O due to higher lattice enthalpy

23
Q

State the equation for Aluminium Oxide reacting with water? What happens?

A

Insoluble due to high lattice enthalpy

24
Q

State the equation for Silicon Oxide reacting with water? What happens?

A

Insoluble due to lattice being held together by strong covalent bonds

25
Q

State the equation for Phosphorus Oxide reacting with water? What happens?

A

P4O10 + 6H2O  4H3PO4, reacts violently

26
Q

State the equation for Sulfur dioxide reacting with water? What happens?

A

SO2 + H2O  H2SO3, dissolves and reacts with water to form a solution

27
Q

State the equation for Sodium trioxide reacting with water? What happens?

A

SO3 + H2O  H2SO4, reacts violently

28
Q

State the equation for Sodium Oxide reacting with acids

A

Na2O + 2HCl  2NaCl + H2O

29
Q

State the equation for Magnesium Oxide reacting with acids

A

MgO + 2HCl  MgCl2 + H2O

30
Q

State the equation for Aluminium Oxide reacting with acids

A

Al2O3 + 3H3SO4  Al2(SO4)3 + 3H2O

31
Q

State the equation for Aluminium Oxide reacting with alkalis

A

Al2O3 + 2NaOH + 3H2O  2NaAl(OH)4

32
Q

State the equation for Sulphur dioxide reacting with alkalis

A

SO2 + 3NaOH  Na2SO3 + H2O

33
Q

State the equation for Sulphur trioxide reacting with alkalis

A

SO3 + 2NaOH  Na2SO4 + H2O

Chemistry A level (10 decks)

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