Loading presentation...

Present Remotely

Send the link below via email or IM

Copy

Present to your audience

Start remote presentation

  • Invited audience members will follow you as you navigate and present
  • People invited to a presentation do not need a Prezi account
  • This link expires 10 minutes after you close the presentation
  • A maximum of 30 users can follow your presentation
  • Learn more about this feature in our knowledge base article

Do you really want to delete this prezi?

Neither you, nor the coeditors you shared it with will be able to recover it again.

DeleteCancel

Make your likes visible on Facebook?

Connect your Facebook account to Prezi and let your likes appear on your timeline.
You can change this under Settings & Account at any time.

No, thanks

CHEMISTRY

Ox. No. of Oxides & Hydroxides of Period 3 Elements
by

Nicholas Ng

on 13 May 2013

Comments (0)

Please log in to add your comment.

Report abuse

Transcript of CHEMISTRY

Recap: Basic oxides:
Oxides which react with water to form bases.


Amphoteric oxides:
Oxides which display both basic AND acidic properties.


Acidic oxides:
Oxides which react with water to form acids.


Argon is a noble gas & does not
form an oxide. Going Across Period 3 Oxides of Period 3 - Maximum oxidation no. of Period 3 element increases

-Oxidation no. of Period 3 element is always +ve (O, which has Ox. No. -2, is more electronegative than ALL Period 3 elements)

-Oxides of elements go from Basic Amphoteric Acidic Basic Oxides -Sodium & Magnesium Amphoteric Oxide -Aluminium Acidic Oxides -Silicon, Phosphorus, Sulfur & Chlorine THANK YOU
FOR VIEWING ;) Common oxides: Silicon: Silicon dioxide Phosphorus: Phosphorus(V) oxide,
Phosphorus(III) oxide Sulfur: Sulfur dioxide,
Sulfur trioxide Chlorine: Dichlorine Heptoxide,
Chlorine(I) Oxide Common oxides: Sodium: Sodium oxide Magnesium: Magnesium oxide Common oxide: Aluminium(III) oxide Na, Mg, Al, Si, P, S, Cl, Ar Oxides and Water Hydroxides of Na & Mg -Aluminium oxide DOES NOT react or dissolve in water at room temperature.

-It reacts with both alkaline and acidic solutions.

-It displays both basic and acidic properties.

-It behaves as a base when reacted with an acid & forms salt + water.

-It behaves as an acid when reacted with an alkali & forms salt. Reaction with an acid: Reaction with Hot, Concentrated alkali: Oxides and Water Acids of P & S Oxidation No. of Elements Na₂O Na Al MgO Al₂O₃ Mg SiO₂ Si P₄O P SO₂ S +1 +2 +3 +4 +5 SO₃ +4 +6 Cl Cl₂O +7 -Phosphorus reacts vigorously and dissolves in water to form an acidic solution of phosphoric(V)acid.

P₄O₁ ₀(s) + 6H₂O(l) →----> 4H₃PO₄(aq) 0 -The oxides of sulfur, SO₂ and SO₃ both react and dissolve in water forming acidic solutions, forming sulfuric(IV) acid & sulfuric(VI) acid.

SO₂(g) + H₂O(l) ----> H₂SO₃(aq)
SO₂(g) + H₂O(l) ---->→ H₂SO₄(aq) -Silicon dioxide has no reaction with water. -Phosphorus(III)oxide forms Phosphoric(V) acid when reacted with water.
H₃PO₄

-Sulfur dioxide & sulfur trioxide forms sulfuric(IV) acid & sulfuric(VI) acid respectively when reacted with water.

H₂SO₃
H₂SO₄ Al₂O₃(s) + 6HCl(aq) ----> 2AlCl₃(aq) + 3H₂O(l) Al₂O₃(s) + 2NaOH(aq) + 3H₂O(l) ---> 2Na[Al(OH)₄](aq) -Sodium oxide reacts with water to form sodium hydroxide.

Na₂O(s) + H₂O(l) ---> 2NaOH(aq) -Magnesium oxide reacts with water to form magnesium hydroxide.

MgO(s) + H₂O(l) ---> Mg(OH)₂(aq) Sodium Hydroxide (strongly alkaline solution)

NaOH Magnesium Hydroxide (weakly alkaline solution)

Mg(OH)₂ 10 7 P₄O₆ 6 +3
Full transcript