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AQA A level Chemistry > Period 3 Oxides > Flashcards

Period 3 Oxides Flashcards

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1
Q

Why is Na more reactive than Mg

A

Na needs less energy to remove 1 electron compared to Mg who needs more to remove two

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2
Q

How does Na react with water

A
  • sodium reacts vigorously with cold water, forms a ball and fizzes
  • gas produced is h2
  • produces alkaline solution of NaOH

2Na +2H20 -> 2NaOH +H2

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3
Q

How does magnesium react with water

A

Reacts slowly
Forms weak alkaline solution of Mg(OH)2
-it’s weak because magnesium hydroxide is sparingly soluble

Mg + H20 -> Mg(OH)2 + H2

When it reacts with steam
It’s fast and it makes Mgo and H2

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4
Q

Which element in period three does not form an oxide

A

Sulphur forms sulphur dioxide

With higher temps and a catalyst can form so3

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5
Q

What is the equation of sodium forming an oxide and how does it react with

  1. Air
A

2Na + 1/2 o2 —> 2Na2o

Oxide: sodium oxide
Reacts very fast
White/yellow solid
yellow or orange flame

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6
Q

What is the equation of magnesium forming an oxide and what are the observations

  1. Air
A

Mg + 1/2 o2 —> Mgo

Oxide: MgO
Reaction: very fast

White solid
bright white light

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7
Q

What is the equation of aluminium forming an oxide and how does it react with

  1. Air
A

2Al + 1/2 o2 —> Al203

Oxide: Al2o3
Reaction: slow generally (fast if a powder)

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8
Q

What is the equation of silicon forming an oxide and how does it react with

  1. Air
A

Si + o2 —> Sio2

Reaction is slow

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9
Q

What is the equation of a phosphorus forming an oxide and how does it react with

  1. Air
A

P4 + 5o2 —> P4o10

Oxide: P4o10
Reaction: spontaneously combusts

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10
Q

What is the equation of sulphur forming an oxide and how does it react with

  1. Air
A

S + o2 —> SO2

Oxide: SO2
Reaction: steadily burns

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11
Q

Why does Magnesium oxide have a higher melting point that sodium oxide

A

Mg forms 2+ ions whereas Na forms 1+, so 2+ ions are attracted more strongly to the oxygen

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12
Q

Why does aluminium oxide have a lower melting point that magnesium oxide

A

Al 3+ ions distort election cloud of oxygen, pull electrons from oxygen towards it
So aluminium oxide has some covalent character as well as ionic interactions
This means less energy is required to break the bond

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13
Q

What kind of structure and bonding is there in silicon dioxide

A

Forms a macromolecular structure

Has many strong covalent bonds so lots of energy is retired to break then

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14
Q

What kind of structure and bonding do p4010 and SO2 form

A

Structure: simple molecular

Bonding: van der waals,

Less energy is required to break them compared to silicon dioxide

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15
Q

Ionic oxides

What kind of solution do Na and Mg form in water
What kind of ph is there and why

A

Both form alkaline solutions

Na2O creates alkaline solution of 12-14 as it dissolves readily (strong base)

MgO creates an alkaline solution of 9-10 as it dissolves sparingly in water

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16
Q

Simple Covalent oxides

What kind of solution does P4O10 and So2 form in water
What kind of ph is there

What is the equation for Sulphur dioxide reacting with water

A

Solution: acidic

pH: is 1-2

Phosphore dioxide forms phosphoric acid which can dissociate to form H+ ions

H3PO4 —> 3H+ + Po4 3-

Equation
So2 + H20 —> H2So3 (sulphuric IV acid or sulphurous acid)

To make sulphuric acid
Sulphur trioxide needs to react with water

17
Q

What happens to silicon dioxide in water

A

Insoluble in water
Silicon dioxide is sand by the way
As there are many covalent bonds
Will react with a base to form salt so it’s classed as an acid

18
Q

How does silicon dioxide react with water

A

It’s amphoteric, as it has both covalent and ionic characters

Insoluble in water
But will react with both acids and bases to form salts

19
Q

What happens when aluminium oxide acts as an acid

1:2:3

A

Produces no water

2NaoH + Al2o3 +3H20 —> 2NaAl(OH)4

20
Q

What happens aluminium oxide acts as an alkali

A

3H2SO4 + Al2O3 -> Al2(SO4)3+ 3H20

AQA A level Chemistry (26 decks)

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