Section 3 - Period 3 Elements Flashcards
Is Na or Mg more reactive?
Sodium - it takes less energy to lose one electron than to lose two.
How does sodium react with cold water?
- vigorously
- forms alkaline solution
- forms a molten ball on surface
- fizzes and produces H2 gas
Complete the equation:
2Na(s) + 2H2O(l) –>
2NaOH(aq) + H2(g)
What is the pH of NaOH?
Strongly alkaline - pH 12-14
How does magnesium react with cold water?
- Very slowly
- Alkaline solution is formed
- Thin coating of magnesium hydroxide forms on surface of metal
What is the pH of magnesium hydroxide and why?
Weakly alkaline - pH 9-10
It is not very soluble in water so very few hydroxide ions are produced.
Complete the equation:
Mg(s) + 2H2O(l) –>
Mg(OH)2(aq) + H2(g)
What is a faster way to react magnesium with water and what does it produce?
React it with steam
Magnesium Oxide
Complete the equation:
Mg(s) + H2O(g) –>
MgO(s) + H2(g)
What do period 3 elements form when they react with oxygen?
Oxides
What is the general pattern for oxidation states of elements in oxides? (and what is the exception?)
Usually oxidised to their highest oxidation state (the same as their group numbers).
Sulfur is the exception - it forms SO2 which has an oxidation state of +4. A catalyst and high temp are needed to create SO3.
Give the equation for:
Sodium and Oxygen
2Na(s) + 1/2O2(g) –> Na2O(s)
Give the equation for:
Magnesium and Oxygen
Mg(s) + 1/2O(g) –> MgO(s)
Give the equation for:
Aluminium and Oxygen
2Al(s) + 3/2O2(g) –> Al2O3(s)
Give the equation for:
Silicon and Oxygen
Si(s) + O2(g) –> SiO2(s)
Give the equation for:
Phosphorous and Oxygen
P4(s) +5O2(g) –> P4O10(s)
Give the equation for:
Sulfur and Oxygen
S(s) + O2(g) –> SO2(g)
How does Na react in air?
Vigorously
How does Mg react in air?
Vigorously
How does Al react in air?
Slow (faster if powdered)
How does Si react with air?
Slowly
How does P react in air?
Spontaneously combusts
How does S react in air?
Burns steadily
What does the graph of period 3 oxides mpts look like?
(ignore chlorine)

Why do the metal oxides (sodium, magnesium and aluminium) have high mpts?
They form giant ionic lattices
Strong forces of attraction between each ion
A lot of energy required to break the bonds
Why does MgO have a higher mpt than Na2O?
Mg forms 2+ ions so it bonds more strongly than the 1+ Na ions.
Why does Al2O3 have a lower mpt?
The highly charged Al3+ ions distort the oxygen’s electron cloud making the bonds partially covalent.
Why does SiO2 have the highest non-metal oxide mpt?
It has a giant macromolecular structure
The strong covalent bonds must be broken
This requires a lot of energy
Why do the phosphorous and sulfur oxides have relatively low mpts?
They form simple molecular structures
Weak intermolecular forces (dipole-dipole and VdWs) are easy to break
How do you determine if an oxide is acidic or alkaline?
Ionic oxides are alkaline, covalent oxides are acidic.
Why do ionic oxides form alkaline solutions when dissolved in water?
The oxide ions (O2-) accept protons from the water molecules to form hydroxide ions.
Give the equation for the reaction of:
sodium oxide with water
Na2O(s) + H2O –> 2NaOH(aq)
Give the equation for the reaction of:
magnesium oxide and water
MgO(s) + H2O(l) –> Mg(OH)2(aq)
What type of solutions do the simple covalent oxides of phosphorus and sulfur form?
Strong acidic
Give the equation for the reaction of:
phosphorus (V) oxide and water
P4O10(s) + 6H2O(l) –> 4H3PO4(aq)
Give the equation for the reaction of:
sulfur dioxide and water
SO2(g) + H2O(l) –> H2SO3(aq)
Give the equation for the reaction of:
sulfur trioxide and water
SO3(l) + H2O(l) –> H2SO4(aq)
Give the equation for the disassociation of phosphoric (V) acid:
H3PO4(aq) –> 3H+(aq) + PO43-(aq)
Give the equation for the disassociation of sulfurous acid:
H2SO3(aq) –> 2H+(aq) + SO32-(aq)
Give the equation for the disassociation of sulfuric acid:
H2SO4(aq) –> 2H+(aq) + SO42-(aq)
What happens when you react silicon dioxide with water?
Nothing - it is insoluble in water
Is silicon dioxide classed as acidic or basic?
acidic - it reacts with bases.
What happens when you react aluminium oxide with water?
Nothing - it is insoluble
Is aluminium oxide classed as acidic or basic?
Both - it is amphoteric
Due to its partially ionic and partially covalent bonding
Give the equation of the neutralisation reaction between sodium oxide and hydrochloric acid:
Na2O(s) + 2HCl(aq) –> 2NaCl(aq) + H2O(l)
Give the equation of the neutralisation reaction between magnesium oxide and sulfuric acid:
MgO(s) + H2SO4(aq) –> MgSO4(aq) + H2O(l)
Give the equation of the neutralisation reaction between silicon dioxide and sodium hydroxide:
SiO2(s) + 2NaOH(aq) –> Na2SiO3(aq) + H2O(l)
Give the equation of the neutralisation reaction between phosphorous oxide and sodium hydroxide:
P4O10(s) + 12NaOH(aq) –> 4Na3PO4(aq) + 6H2O(l)
Give the equation of the neutralisation reaction between sulfur dioxide and sodium hydroxide:
SO2(g) + 2NaOH(aq) –> Na2SO3(aq) + H2O(l)
Give the equation of the neutralisation reaction between sulfur trioxide and sodium hydroxide:
SO3(g) +2NaOH(aq) –> Na2SO4(aq) + H2O(l)
Give the equation of the neutralisation reaction between aluminium oxide and sulfuric acid:
(aluminium oxide as a base)
Al2O3(s) + 3H2SO4(aq) –> Al2(SO4)3(aq) + 3H2O(l)
Give the equation of the neutralisation reaction between aluminium oxide and sodium hydroxide:
(aluminium oxide as an acid)
Al2O3(s) + 2NaOH(aq) + 3H2O(l) –> 2NaAl(OH)4(aq)