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Strongly Basic oxides: Na2O, MgO ( metals )
Amphoteric oxide: Al2O3 ( metals )

shows both acidic and basic properties

Weakly Acidic oxide: SiO2 ( metalloid )
Strongly Acidic oxides: P4O10, SO3 ( non-metals )

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Sulphur trioxide (acidic)
- reacts violently with water to produce a fog of sulphuric acid droplets H2SO4
- reacts with NaOH to form sodium sulphate salt Na2SO4

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- Phosphorus oxide (acidic) reacts violently with water to form phosphoric acid
- P4O10 reacts with NaOH to for sodium phosphate salt

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Acid-Base Behavior (Shannon)

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Silicon dioxide
- Due to strong covalent bonds in its giant covalent structure, it does not react in water
- Reacts with HOT CONCENTRATED sodium hydroxide solution to form colourless solution of sodium silicate Na2SiO3

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P4O10, SO3 ( non-metals ):

Structure - Simple molecular oxides

Bonding - Weak Van der Waals (Intermolecular bonds) forces of attraction between molecules > less energy needed to break the bonds

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SiO2 ( metalloids ):

Structure - Giant covalent structure

Bonding - Strong Covalent bonding (Intramolecular bonds) between atoms > more energy needed to break the bonds

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Metals conduct electricity because the electrons are delocalized and are free to move throughout the structure.

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Na2O, MgO, Al2O3 ( metals ):

Structure - Giant structures of ionic lattice

Bonding - Strong Ionic bonding (Intramolecular bonds) between cations and anions > more energy needed to break the bonds

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Metals have high melting and boiling point because of the strong metallic bonding between the metal nucleus and the “sea” of electrons. (Intramolecular bonds)

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Properties and reaction of Period 3 chlorides 

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Properties and reaction of Period 3 chlorides 

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Bonding and Structure:
NaCl and MgCl2: giant ionic lattice, strong ionic bonding between cations and anions
AlCl3 and PCl5: simple molecular, but ionic solids at low temperature, converts to molecules at liquid and vapour phases at high temperature, weak intermolecular forces of attraction between molecules
SiCl4: simple molecular, weak intermolecular forces of attraction between molecules

Reaction with H2O:
NaCl: no reaction and dissolves in water
MgCl2: no reaction and dissolves in water to give acidic solution (pH ~ 6)
AlCl3: violent reaction, [Al(H2O)6]3+ formed (known as Hexaaquaaluminium ions), produces steamy fumes of hydrogen chloride gas
SiCl4: violent reaction, produces silicon dioxide and fumes of hydrogen chloride
PCl5:
Cold water:
PCl5 (s) + H2O (l) --> POCl3 (g) + 2HCl (aq)
Warm water:
PCl5 (s) + 4H2O (l) --> H3PO4 (aq) + 5HCl (aq)

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Metalloids are a semiconductor and can only conduct electricity at high temperature. At room temperature, it is a non-electrical conductor as there are no free electrons.

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Metaloids has high melting and boiling point due to the strong covalent bonds between the Si atoms in the giant covalent structure.

(intramolecular bonds)

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Aluminium Oxide
- It does not react with water the intermolecular force is very strong in the lattice structure.
- It is an amphoteric compound meaning it can react with both acid and base
- Reacts with HOT dilute HCL (acid) to produce aluminium chloride solution AlCl3.
- Reacts with HOT CONCENTRATED sodium hydroxide (base) to give colourless tetrahydroxoaluminate [the Al(OH)4 is always a constant]
- diff products formed depending on the temperature and concentration of the NaOH solution.

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They do not conduct electricity as they are simple molecules with no free electrons.

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Non-metals are simple molecules with only Van der Waals attractions between the molecules. Their melting or boiling points will be lower than those of the first four members of the period which have giant structures.
(intermolecular bonds)

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-Simple molecules
-Weak Van der Waals forces between molecules
-Low melting and boiling point
-Do not conduct electricity.

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-Giant covalent structure
-Strong covalent bonds between atoms
-High melting and boiling point
-Do not conduct electricity

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Magnesium Oxide
- slight reaction occurs when MgO reacts with water and forms magnesium hydroxide Mg(OH)2
- when react with dilute HCL, it produces magnesium chloride solution MgCl2

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-Metallic structure
-Strong attraction (metallic bonding) between metal nucleus and “sea” of electrons
-High melting and boiling point
-Conduct electricity (has free moving electrons)

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Sodium Oxides
- Na2O reacts exothermally with cold water and produces 2NaOH solution
- Reacts with dilute HCL and produces sodium chloride solution (NaCl)

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Bonding & Structure (Shannon)

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-Elements include Na, Mg, Al, Si, P, S, Cl to Ar
-Changes from metals (Na, Mg, Al), metalloids (Si) to non-metals (P, S, Cl, Ar)
-They have 3 electron shells
-Atomic number ranges from 11 to 18.

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Properties and reactions of Period 3 chlorides (Zi Yi)

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Properties and reactions of Period 3 chlorides (Zi Yi)

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Properties and reactions of Period 3 oxides (Priya & Shannon)

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Properties and reactions of Period 3 oxides (Priya & Shannon)

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Properties and reaction of Period 3 hydroxides ( Anshaf ) 

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Properties and reaction of Period 3 hydroxides ( Anshaf ) 

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3 types of hydroxide learnt today :
Aluminum hydroxide ( Al(OH)3 ),
Magnesium hydroxide ( Mg(OH)2  ) ,
Sodium hydroxide (NaOH)

All 3 hydroxides able to react with acids to form salts.

Aluminium Hydroxide is
1) amphoteric ( it has both basic and acidic properties.)
2) able to react with Hydrochloric acid to form a colorless solution of aluminum chloride
3) is able to react with sodium hydroxide to produce a colourless solution of sodium tetrahydroxoaluminate.

Sodium Hydroxide is
1) Basic ( hydroxide ions released when dissolved
2) able to react with acids such as HCL and H2SO4 to form salts such as Na2SO4 ( Neutral salt ).

Magnesium hydroxide is
1) Basic
2) Reacts with acids to form salts such as MgCl2 and MgSO4

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Period 3 elements