Period 3 elements and oxides - part 2

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35 Terms

1
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Draw the trend in first ionisation across period 3

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2
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Explain the decrease in first ionisation energy from Mg to Al

Jump to 3p sub shell which is further from nucleus

3
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Explain the decrease in first ionisation energy from P to S

3p3 to 3p4, electron must pair up in orbital so light repulsion makes easier to remove

4
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Draw the trend in melting and boiling points across period 3

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5
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Explain the increase in melting point from Na to Al

Cations increase in charge, cations decrease in size, more delocalised electrons means stronger electrostatic forces

6
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Explain the high melting point of Si

Strong covalent bonds between atoms requires a lot of energy to overcome

7
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Explain the trend in melting point from P to Ar

Slight increase from P to S as molecules contain more electrons so stronger Van der Waals forces, decrease from S to Ar as number of electrons decreases

8
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Which period 3 elements conduct electricity, and what is the trend in those that do?

Na, Mg and Al only, Al3+ has more delocalised electrons so is best

9
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Metal and water —> ?

Metal hydroxide + hydrogen

10
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Metal + steam —> ?

Metal oxide + hydrogen

11
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Flame test for Na

Yellow

12
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Flame test for Mg, Al, Si

Bright white

13
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Flame test for P4

Very white

14
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Flame test for S8

Blue

15
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Reaction of Na2O with water + equation

Dissolves, Na2O + H2O —> 2NaOH

16
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pH of solution formed when Na2O dissolves in water

13

17
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Nature of sodium oxide

Basic

18
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Reaction of MgO with water + equation

Slightly soluble, MgO + H2O —> Mg(OH)2

19
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pH of solution formed when MgO reacts with water

9

20
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Nature of magnesium oxide

Weakly basic

21
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Reaction of Al2O3 with water + equation

Insoluble

22
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Reaction of SiO2 with water + equation

Insoluble

23
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Describe the difference observed when SO2 vs SO3 reacts with water

SO2 dissolves while SO3 dissolves and reacts violently

24
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pH of solution when P4O10 or SO2 reacts with water

3

25
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pH of solution formed when SO3 reacts with water

0/1

26
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Reaction of Na2O with acid

Na2O + 2H+ —> 2Na+ + H2O

27
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Reaction of MgO with acid

MgO + 2H+ —> Mg2+ + H2O

28
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Reaction of Al2O3 with acid

Al2O3 + 6H+ —> 2Al3+ + 3H2O

29
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Reaction of Al2O3 with alkali

Al2O3 + 2OH- + 3H2O —> 2Al(OH)4 -

30
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Nature of aluminium oxide

Amphoteric

31
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Reaction of SiO2 with alkali

SiO2 + OH- —> SiO3 2- + H2O

32
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Conditions needed for SiO2 to react with alkali

Hot and conc NaOH

33
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Reaction of P4O10 with alkali

P4O10 + 12OH- —> 4PO4 3- + 6H2O

34
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Reaction of SO2 with alkali

SO2 + 2OH- —> SO3 2- + H2O

35
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Reaction of SO3 with alkali

SO3 + 2OH- —> SO4 2- + H2O