Presentation is loading. Please wait.

Presentation is loading. Please wait.

Periodic Relationship among the Oxides of the Elements Li to Cl

Published byElwin McKinney Modified over 9 years ago

Similar presentations

Presentation on theme: "Periodic Relationship among the Oxides of the Elements Li to Cl"— Presentation transcript:

1 Periodic Relationship among the Oxides of the Elements Li to Cl
39 39.1 Bonding of the Oxides of Periods 2 and 3 Elements 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis

2 Bonding of the Oxides of Periods 2 and 3 Elements
39.1 Bonding of the Oxides of Periods 2 and 3 Elements

3 Introduction The electronegativity value of oxygen is 3.5
39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.19) Introduction The electronegativity value of oxygen is 3.5

4 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.19)
Introduction When oxygen combines with elements having low electronegativity values (e.g. metals)  the oxygen atoms would gain the electrons from the elements  to form oxide ions

5 Introduction The compounds formed consist of
39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.19) Introduction The compounds formed consist of  positive ions formed the electropositive elements  negative oxide ions These oxides are ionic oxides

6 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.19)
Introduction When oxygen combines with elements of similar electronegativity values  the oxygen atoms would share electrons with these elements  to form covalent oxides

7 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.19)
Nature of Bonding The oxides of Periods 2 and 3 elements can be classified into  ionic oxides  ionic oxides with high covalent character  covalent oxides

8 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.20)
Periodicity in nature of bonding of the oxides of Periods 2 and 3 elements Oxide of Period 2 element Li2O BeO B2O3 CO CO2 N2O NO NO2 N2O4 N2O5 O2 O3 OF2 Nature of bonding in the oxides Ionic Ionic with covalent character Covalent Oxide of Period 3 element Na2O Na2O2 MgO Al2O3 SiO2 P4O6 P4O10 SO2 SO3 Cl2O Cl2O7

9 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.20)
Nature of Bonding Going across a period from left to right, the nature of bonding of the oxides changes from  ionic bonding  ionic bonding with covalent character  covalent bonding

10 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.20)
Nature of Bonding A number of elements in Periods 2 and 3 form more than one oxide with oxygen Example: Sodium is a reactive metal  can form the normal oxide and peroxide with oxygen

11 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.20)
Nature of Bonding Elements with electronegativity values similar to oxygen also form a variety of oxides

12 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.20)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Lithium Lithium oxide Li2O Beryllium Beryllium oxide BeO Boron Boron oxide B2O3

13 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.20 – 21 )
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Carbon Carbon monoxide CO Carbon dioxide CO2 Nitrogen Dinitrogen oxide N2O Nitrogen monoxide NO

14 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.21)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Nitrogen Nitrogen dioxide NO2 Dinitrogen tetraoxide N2O4 Dinitrogen pentaoxide N2O5

15 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.21)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Oxygen O2 Ozone O3 Fluorine Oxygen difluoride OF2 Sodium Sodium monoxide Na2O Sodium peroxide Na2O2

16 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.21)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Magnesium Magnesium oxide MgO Aluminium Aluminium oxide Al2O3 Silicon Silicon(IV) oxide SiO2

17 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.22)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Phosphorus Phosphorus(III) oxide P4O6 Phosphorus(V) oxide P4O10

18 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.22)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Sulphur Sulphur dioxide SO2 Sulphur trioxide SO3

19 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.22)
Names, stoichiometric composition and electronic structures of oxides of Periods 2 and 3 elements Element Name of oxide of element Stoichiometric composition of oxide of element Electronic structure of oxide of element Chlorine Chlorine(I) oxide (dichlorine oxide) Cl2O Chlorine(VII) oxide (dichlorine heptaoxide) Cl2O7 Check Point 39-1

20 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis

21 Ionic Oxides Generally react with water to form hydroxides
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides Generally react with water to form hydroxides As hydroxides are basic oxides  they neutralize with dilute acids to form salts Do not react with dilute alkalis

22 Ionic Oxides Lithium oxide
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides Lithium oxide  reacts vigorously with water to form lithium hydroxide Li2O(s) + H2O(l)  2LiOH(aq)

23 Ionic Oxides Sodium monoxide
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides Sodium monoxide  reacts vigorously with water to form sodium hydroxide Na2O(s) + H2O(l)  2NaOH(aq)

24 Ionic Oxides Sodium peroxide
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides Sodium peroxide  reacts with water to give sodium hydroxide and hydrogen peroxide Na2O2(s) + 2H2O(l)  2NaOH(aq) + H2O2(aq)

25 Ionic Oxides Magnesium oxide  less basic
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides Magnesium oxide  less basic  reacts slightly with cold water and moderately with hot water to form magnesium hydroxide, which is very slightly soluble

26 Ionic Oxides Magnesium oxide
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides Magnesium oxide  Magnesium hydroxide solution is a weakly alkaline solution MgO(s) + H2O(l)  Mg(OH)2(s)

27 Ionic Oxides All ionic oxides react with dilute acids to form salts
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides All ionic oxides react with dilute acids to form salts

28 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides The reactions can be summarized by the following ionic equations: Li2O(s) + 2H+(aq)  2Li+(aq) + H2O(l) Na2O(s) + 2H+(aq)  2Na+(aq) + H2O(l) Na2O2(s) + 2H+(aq)  2Na+(aq) + H2O2(aq) MgO(s) + 2H+(aq)  Mg2+(aq) + H2O(l)

29 Ionic Oxides with High Covalent Character
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides with High Covalent Character Beryllium oxide and aluminium oxide  ionic oxides with high covalent character  not soluble in water

30 Ionic Oxides with High Covalent Character
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides with High Covalent Character Beryllium oxide and aluminium oxide  react with both dilute acids and dilute alkalis to form soluble compounds  amphoteric oxides

31 Ionic Oxides with High Covalent Character
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides with High Covalent Character Beryllium oxide and aluminium oxide BeO(s) + 2H+(aq)  Be2+(aq) + H2O(l) BeO(s) + 2OH–(aq) + H2O(l)  [Be(OH) 4]2–(aq) beryllate ion

32 Ionic Oxides with High Covalent Character
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.23) Ionic Oxides with High Covalent Character Beryllium oxide and aluminium oxide Al2O3(s) + 6H+(aq)  2Al3+(aq) + 3H2O(l) Al2O3(s) + 2OH–(aq) + 3H2O(l)  2[Al(OH)4]–(aq) aluminate ion

33 Covalent Oxides Some covalent oxides that are soluble in water
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) Covalent Oxides Some covalent oxides that are soluble in water  react with water to form acids  react with dilute alkalis  do not react with dilute acids

34 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Boron(III) oxide  reacts with water to form boric(III) acid B2O3(s) + 3H2O(l)  2H3BO3(s)

35 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Carbon monoxide  neutral  insoluble in water

36 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Carbon dioxide  moderately soluble in cold water  the solution formed is slightly acidic CO2(g) + H2O(l)  H2CO3(aq)

37 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Dinitrogen oxide and nitrogen monoxide  neutral  insoluble in water

38 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Nitrogen dioxide  reacts rapidly with cold water to give a mixture of nitric(III) acid and nitric(V) acid 2NO2(g) + H2O(l)  HNO2(aq) + HNO3(aq) nitric(III) acid nitric(V)acid

39 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Dinitrogen tetraoxide  reacts with water to form nitric(III) acid and nitric(V) acid N2O4(g) + H2O(l)  HNO2(aq) + HNO3(aq)

40 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Dinitrogen pentaoxide  reacts with cold water to form nitric(V) acid N2O5(s) + H2O(l)  2HNO3(aq)

41 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Oxygen  neutral  very slightly soluble in water

42 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis Oxygen difluoride  colourless gas  hydrolyzes slowly to form oxygen gas and hydrogen fluoride OF2(g) + H2O(l)  2HF(aq) + O2(g)

43 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis The reactions can be summarized by the following ionic equations: B2O3(s) + 6OH–(aq)  2BO33–(aq) + 3H2O(l) CO2(g) + 2OH–(aq)  CO32–(aq) + H2O(l)

44 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis The reactions can be summarized by the following ionic equations: 2NO2(g) + 2OH–(aq)  NO2–(aq) + NO3–(aq) + H2O(l) N2O4(g) + 2OH–(aq)  NO2–(aq) + NO3–(aq) + H2O(l)

45 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.24) 1. Behaviour of Covalent Oxides of Period 2 Elements in Water and Dilute Alkalis The reactions can be summarized by the following ionic equations: N2O5(s) + 2OH–(aq)  2NO3–(aq) + H2O(l) OF2(g) + 2OH–(aq)  2F–(aq) + O2(g) + H2O(l)

46 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Silicon(IV) oxide  does not react with water  weakly acidic  reacts with hot alkalis to form silicates(IV) SiO2(s) + 2NaOH(aq)  Na2SiO3(aq) + H2O(l)

47 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Phosphorus(III) oxide  reacts slowly with cold water to form phosphoric(III) acid P4O6(s) + 6H2O(l)  4H3PO3(aq)

48 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Phosphorus(V) oxide  reacts vigorously with cold water to form phosphoric(V) acid P4O10(s) + 6H2O(l)  4H3PO4(aq)

49 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Sulphur dioxide  react with water to form sulphuric(IV) acid SO2(g) + H2O(l)  H2SO3(aq) sulphuric(IV) acid

50 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Sulphur trioxide  react with water to form sulphuric(VI) acid SO3(g) + H2O(l)  H2SO4(aq) sulphuric(VI) acid

51 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Chlorine(I) oxide  dissolves in water to form chloric(I) acid (also known as hypochlorus acid) Cl2O(g) + H2O(l)  2HOCl(aq) chloric(I) acid

52 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Chlorine(VII) oxide  dissolves in water to form a very strong acid called chloric(VII) acid (also known as perchloric acid) Cl2O7(l) + H2O(l)  2HClO4(aq) chloric(VII) acid

53 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Ionic equations: P4O6(s) + 12OH–(aq)  4PO43–(aq) + 6H2O(l) P4O10(s) + 12OH–(aq)  4PO43–(aq) + 6H2O(l)

54 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Ionic equations: SO2(g) + 2OH–(aq)  SO32–(aq) + H2O(l) SO3(g) + 2OH–(aq)  SO42–(aq) + H2O(l)

55 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.25) 2. Behaviour of Covalent Oxides of Period 3 Elements in Water and Dilute Alkalis Ionic equations: Cl2O(g) + 2OH–(aq)  2OCl–(aq) + H2O(l) Cl2O7(l) + 2OH–(aq)  2ClO4–(aq) + H2O(l)

56 Oxide of Period 2 element Behaviour of oxides in water
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.26) Periodicity in the behaviour of oxides of Periods 2 elements in water, dilute acids and dilute alkalis Oxide of Period 2 element Li2O BeO B2O3 CO CO2 N2O NO NO2 N2O4 N2O5 O2 OF2 Behaviour of oxides in water Reacts vigorously with water to form LiOH Does not react with water Reacts with water to form H3BO3, which is a very weak acid CO: Insoluble in water CO2: Moderately soluble in water to form H2CO3, which is a very weak acid N2O and NO: Insoluble in water NO2 and N2O4: React with water to form HNO2 and HNO3 N2O5: Reacts with cold water to form HNO3 Very slightly soluble in water, does not react with water Hydrolyzes slowly to form O2 and an acidic solution of HF

57 Oxide of Period 2 element Behaviour of oxides in dilute acids
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.26) Periodicity in the behaviour of oxides of Periods 2 elements in water, dilute acids and dilute alkalis Oxide of Period 2 element Li2O BeO B2O3 CO CO2 N2O NO NO2 N2O4 N2O5 O2 OF2 Behaviour of oxides in dilute acids Reacts to form Li+ Reacts to form Be2+ Does not react with dilute acids Do not react with dilute acids

58 Oxide of Period 2 element Behaviour of oxides in alkalis
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.26) Periodicity in the behaviour of oxides of Periods 2 elements in water, dilute acids and dilute alkalis Oxide of Period 2 element Li2O BeO B2O3 CO CO2 N2O NO NO2 N2O4 N2O5 O2 OF2 Behaviour of oxides in alkalis Does not react with dilute alkalis Reacts to form [Be(OH)4]2– Reacts to form BO33– CO: Does not react with dilute alkalis CO2: Reacts to form CO32– N2O and NO: Do not react with dilute alkalis NO2 and N2O4: React to form NO2– and NO3– N2O5: Reacts to form NO3– Reacts to form F– and O2

59 Oxide of Period 2 element Acidic/ basic nature of oxides
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.26) Periodicity in the behaviour of oxides of Periods 2 elements in water, dilute acids and dilute alkalis Oxide of Period 2 element Li2O BeO B2O3 CO CO2 N2O NO NO2 N2O4 N2O5 O2 OF2 Acidic/ basic nature of oxides Alkaline Amphoteric Acidic Neutral

60 Oxide of Period 3 element Behaviour of oxides in water
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) Periodicity in the behaviour of oxides of Periods 3 elements in water, dilute acids and dilute alkalis Oxide of Period 3 element Na2O Na2O2 MgO Al2O3 SiO2 P4O6 P4O10 SO2 SO3 Cl2O Cl2O7 Behaviour of oxides in water Na2O: Reacts vigorously with water to form NaOH Na2O2: Reacts with water to form NaOH and H2O2 Reacts slightly with cold water and moderately with hot water to form a weakly alkaline solution of Mg(OH)2 Does not react with water P4O6: Reacts slowly with cold water to form H3PO3 P4O10: Reacts vigorously with cold water to form H3PO4 SO2: Reacts with water to form H2SO3 SO3: Reacts with water to form H2SO4 Cl2O: Dissolves in water to form HOCl Cl2O7: Dissolves in water to form HClO4

61 Oxide of Period 3 element Behaviour of oxides in dilute acids
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) Periodicity in the behaviour of oxides of Periods 3 elements in water, dilute acids and dilute alkalis Oxide of Period 3 element Na2O Na2O2 MgO Al2O3 SiO2 P4O6 P4O10 SO2 SO3 Cl2O Cl2O7 Behaviour of oxides in dilute acids React to form Na+ Reacts to form Mg2+ Reacts to form Al3+ Does not react with dilute acids Do not react with dilute acids

62 Oxide of Period 3 element Behaviour of oxides in dilute alkalis
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) Periodicity in the behaviour of oxides of Periods 3 elements in water, dilute acids and dilute alkalis Oxide of Period 3 element Na2O Na2O2 MgO Al2O3 SiO2 P4O6 P4O10 SO2 SO3 Cl2O Cl2O7 Behaviour of oxides in dilute alkalis Do not react with dilute alkalis Does not react with dilute alkalis Reacts to form [Al(OH)4]– Reacts with hot alkalis to form SiO32– P4O6: Reacts slowly with cold water to form H3PO3 P4O10: Reacts vigorously with cold water to form H3PO4 SO2: Reacts to form SO32– SO3: Reacts to form SO42– Cl2O: Reacts to form OCl– Cl2O7: Reacts to form ClO4–

63 Oxide of Period 3 element Acidic/ basic nature of oxides
39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) Periodicity in the behaviour of oxides of Periods 3 elements in water, dilute acids and dilute alkalis Oxide of Period 3 element Na2O Na2O2 MgO Al2O3 SiO2 P4O6 P4O10 SO2 SO3 Cl2O Cl2O7 Acidic/ basic nature of oxides Alkaline Weakly acidic Amphoteric Acidic Neutral Check Point 39-2

64 The END

65 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.22)
Check Point 39-1 (a) To which type of oxide does each of the following oxides belong? (i) Magnesium oxide (ii) Nitrogen monoxide (iii) Silicon dioxide (iv) Aluminium oxide Answer (a) (i) Ionic oxide (ii) Covalent oxide (iii) Covalent oxide (iv) Ionic oxide with covalent character

66 39.1 Bonding of the Oxides of Periods 2 and 3 Elements (SB p.22)
Check Point 39-1 (b) Carbon can form two oxides. Name the two oxides and draw their electronic structures. Answer (b) Carbon monoxide (CO): Carbon dioxide (CO2): Back

67 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) Check Point 39-2 (a) Why does silicon(IV) oxide not react with water? (a) Silicon(IV) oxide does not react with water because the electronegativity values of silicon and oxygen are very similar. The Si — O bond can be considered as nonpolar, so there is no positive centre for the lone pair electrons of the water molecule to attack. Answer

68 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) Check Point 39-2 (b) Complete and balance the following equations: (i) K2O(s) + H2O(l)  (ii) Na2O2(s) + HCl(aq)  (iii) Al2O3(s) + H2SO4(aq)  (iv) P4O10(s) + NaOH(aq)  (v) SO3(g) + NaOH(aq)  Answer

69 39.2 Behaviour of Oxides of Periods 2 and 3 Elements in Water, Dilute Acids and Dilute Alkalis (SB p.27) (b) (i) K2O(s) + H2O(l)  2KOH(aq) (ii) Na2O2(s) + 2HCl(aq)  2NaCl(aq) + H2O2(aq) (iii) Al2O3(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2O(l ) (iv) P4O10(s) + 12NaOH(aq)  4Na3PO4(aq) + 6H2O(l) (v) SO3(g) + 2NaOH(aq)  Na2SO4(aq) + H2O(l) Back

Download ppt "Periodic Relationship among the Oxides of the Elements Li to Cl"

Similar presentations

Year 12 What you should know already

Year 12 What you should know already
Periodic Trends in Chemical Properties

Periodic Trends in Chemical Properties
Chemical Properties 3.3.1 HL3-3.ppt.

Chemical Properties HL3-3.ppt.
Chapter 20 The Representative Elements. Section 20.1 A Survey of the Representative Elements Return to TOC Copyright © Cengage Learning. All rights reserved.

Chapter 20 The Representative Elements. Section 20.1 A Survey of the Representative Elements Return to TOC Copyright © Cengage Learning. All rights reserved.
Title: Lesson 4 Period 3 Oxides

Title: Lesson 4 Period 3 Oxides
Chapter 8 Periodic Properties of the Elements. 1.2s orbital 2.2p orbital 3.3s orbital 4.3p orbital 5.3d orbital In an germanium atom, which electron will.

Chapter 8 Periodic Properties of the Elements. 1.2s orbital 2.2p orbital 3.3s orbital 4.3p orbital 5.3d orbital In an germanium atom, which electron will.
Building Blocks 1d Int 2 1234 567 89 10 111213 14 15 22 23242526 161718192021.

Building Blocks 1d Int
Strength n Acids and Bases are classified acording to the degree to which they ionize in water: –Strong are completely ionized in aqueous solution; this.

Strength n Acids and Bases are classified acording to the degree to which they ionize in water: –Strong are completely ionized in aqueous solution; this.
Standard Grade Revision Units 3 and 4 Answer:- (a) Lithium Q1. The box below shows the names of some elements. neon.lithiumchlorine oxygencopperargon (a)Identify.

Standard Grade Revision Units 3 and 4 Answer:- (a) Lithium Q1. The box below shows the names of some elements. neon.lithiumchlorine oxygencopperargon (a)Identify.
NAMING COMPOUNDS CH. 6.3. We use the word, COMPOUND, when describing an ionic bonded molecule. An example: –NaCl is sodium chloride.

NAMING COMPOUNDS CH We use the word, COMPOUND, when describing an ionic bonded molecule. An example: –NaCl is sodium chloride.
1 Chapter 8 Acids and Bases 8.6 Reactions of Acids and Bases Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.

1 Chapter 8 Acids and Bases 8.6 Reactions of Acids and Bases Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.
Advanced Higher Chemistry Unit 1 The oxides, chlorides and hydrides.

Advanced Higher Chemistry Unit 1 The oxides, chlorides and hydrides.
Chemical Synthesis Lesson 2. Learning objective: To explain the reactions involving acids. Must: Describe the pH scale. Grade D Must: Describe what happens.

Chemical Synthesis Lesson 2. Learning objective: To explain the reactions involving acids. Must: Describe the pH scale. Grade D Must: Describe what happens.
Third Period elements 1 R.B.Mahajan.  The trend  The diagram shows how the atomic radius changes as you go across Period 3.  The increasing number.

Third Period elements 1 R.B.Mahajan.  The trend  The diagram shows how the atomic radius changes as you go across Period 3.  The increasing number.
13.1. Period 3: Oxides and Chlorides

13.1. Period 3: Oxides and Chlorides
Periodic Relationship among the Oxides, Chlorides & Hydrides

Periodic Relationship among the Oxides, Chlorides & Hydrides
MAKING SALTS 27/08/2015. Making Soluble Salts There are 3 types of reaction that can be used to make soluble salts. All 3 involve: An Acid A metal or.

MAKING SALTS 27/08/2015. Making Soluble Salts There are 3 types of reaction that can be used to make soluble salts. All 3 involve: An Acid A metal or.
PRINCIPLES OF CHEMICAL REACTIVITY: CHEMICAL REACTIONS

PRINCIPLES OF CHEMICAL REACTIVITY: CHEMICAL REACTIONS
Types of Reactions I. Synthesis reactions – have only one product. General Form: A + X  AX EX: 2 Na(s) + Cl 2 (g)  2 NaCl(s) 2 H 2 (g) + O 2 (g)  2.

Types of Reactions I. Synthesis reactions – have only one product. General Form: A + X  AX EX: 2 Na(s) + Cl 2 (g)  2 NaCl(s) 2 H 2 (g) + O 2 (g)  2.
The solvent is generally in excess.

The solvent is generally in excess.

Similar presentations

Ads by Google