IB Chemistry on Chemical Properties, Oxides and Chlorides of period 3

1. Periodicity
Predicted pattern/trend in physical/chemical property across period.
Physical properties Chemical properties
Physical change - without change in molecular composition.
– appearance change
- composition remain unchanged.
Chemical change – diff composition from original substances
- chemical bonds broken/ formed
- new products formed
Element properties Atomic properties
• Color, texture, odor
• Density, hardness, ductility
• Brittleness, Malleability
• Melting /boiling point
• Solubility, polarity
• Ionization energy
• Atomic radii
• Ionic radii
• Electronegativity
Periodic Trends
• Across period 2/3
• Down group 1/17
Gp 1 Gp 17
period 3
period 2
Ionization
energy
Atomic/ionic
radii
Melting
point
Electronegativity
Group 1 (Alkali Metal)
Water
Group 17 (Halogen)
HalogenOxygen
Chemical reaction Chemical reaction
Water AgNO3 Displacement
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Physical Properties Chemical Properties
Gp 17
Gp 1

2. 2Li + CI2 -> 2LiCI
2Na + CI2 -> 2NaCI
2K + CI2 -> 2KCI
Chemical Properties Group 1
Size increase
Reaction with water
4Li + O2 -> 2Li2O
4Na + O2 -> 2Na2O
4K + O2 -> 2K2O
Click here video potassium in water
shell
2.1
2.8.1
2.8.8.1
2.8.8.18.1
Na
Li
K
Rb
lose electron easily
electropositive
Reactivity increase
Group 1 (Alkali Metal)
Chemical reaction
2Li + 2H2O -> 2LiOH + H2
2Na + 2H2O -> 2NaOH + H2
2K + 2H2O -> 2KOH + H2
Reaction with oxygen Reaction with halogen
Lithium – move slowly surface water – red flame
Sodium – move fast, hissing sound – yellow flame
Potassium – move fast, ignite - lilac flame
Turn red litmus blue- produce hydrogen gas
Solution of metal hydroxide/alkaline produced
Click here video sodium in water
Similar chemical property but diff reactivity
Lithium –burn slowly , red flame
Sodium – burn brightly, yellow flame
Potassium –burn very brightly, lilac flame
Kept in paraffin oil
Strong reducing agent
Reduce H+ ion to H2 gas
(losing e to H+)

3. F2 + 2KCI -> 2KF + CI2
CI2 + 2KBr -> 2KCI + Br2
Br2 + 2KI -> 2KBr + I2
Ag+ + CI- -> AgCI
Ag+ + Br- -> AgBr
Ag+ + I- -> AgI
Chemical Properties Group 17
Size increase
Reaction with water
Click here video fluorine chemistry
shell
2.7
2.8.7
2.8.8.7
2.8.18.18.7
CI
F
Br
I
Ability attract electron
decrease/EN lower
Reactivity decrease
Group 17 (Halogen)
Chemical reaction
CI2 + H2O -> HCI + HOCI
Br2 + H2O -> HBr + HOBr
I2 + H2O -> HI + HOI
Reaction with AgNO3
Adding AgNO3
AgCI – white ppt
AgBr - yellow cream ppt
AgI – yellow ppt
Kept in seal, reactive
Fluorine – yellow gas
Chlorine – greenish gas
Bromine – brown liquid
Iodine – violet solid
Click here video on chlorine chemistry
Similar chemical property - decrease reactivity
Chlorine – dissolve quickly –yellowish HOCI
Bromine – dissolve slowly – brown HOBr
Iodine – slightly soluble- brown HOI
Displacement Reaction
Reactive halogen displace less reactive
halogen from its halide solution
Click here video displacement reaction

4. Add NaBrAdd NaCIAdd NaIAdd NaCIAdd NaIAdd NaBr
violet solid
brown liquid
yellow gas
Click here video displacement rxn
Click here video displacement rxn
CI2 + 2NaBr -> 2NaCI + Br2 ✓
CI2 + 2NaI -> 2NaCI + I2 ✓
Br2 + NaCI -> ✗
Br2 + 2NaI -> 2NaBr + I2 ✓
I2 + NaCI -> ✗
I2 + NaBr -> ✗
Chemical Properties Group 17
Group 17 (Halogen)
greenish gas
Displacement Reaction
Reactive halogen displace
less reactive halogen from
its halide solution
CI2 in hexane Br2 in hexane
I2 in hexane
Br2 in
hexane
I2 in
hexane
I2 in
hexane
CI2 + 2NaBr -> 2NaCI + Br2 CI2 + 2NaI -> 2NaCI + I2 ✗ Br2 + 2NaI -> 2NaBr + I2 ✗ ✗

5. Na
(metal)
Mg
(metal)
AI
(Metal)
Si
Non
Metal
P
Non Metal
S
Non
Metal
CI
Non
Metal
m/p (/C) 98 650 660 1423 44 120 -101
Conductivity Good
Free e
Good
Free e
Good
Free e
Moderate
Semi
Poor
Molecular
Poor
Molecular
Poor
Molecular
Bonding metallic metallic metallic Giant
covalent
Simple
covalent
Simple
covalent
Simple
covalent
Period 3
Across period 3 (Metal – Non metallic )
Na2O MgO AI2O3 SiO2 P4O10
P4O6
SO3
SO2
CI2O7
CI2O
State Solid Solid Solid Solid Solid Solid Liquid
Bonding Ionic Ionic Ionic Giant covalent Simple covalent Simple covalent Simple covalent
m/p
(C)
High
(1274)
High
(2852)
High
(2020)
High
(1610)
Low
(24)
Low
(17)
Low
(-92)
Nature of
Oxide
Metal oxide
Basic oxide
Metal oxide
Basic oxide
Metal oxide
Amphoteric
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Reaction
with
water
Form
NaOH
(Alkaline)
Form
Mg(OH)2
(Alkaline)
No reaction
✗
No reaction
✗
Form
H3PO4
(Acidic)
Form
H2SO4
(Acidic)
Form
HCIO4
(Acidic)
Oxides period 3 (Metal – Non metallic oxide )
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Water hydrolysis is chemical rxn
Dissolving NOT a chemical rxn
NaCI MgCI2 AI2CI6 SiCI4 PCI3 S2CI2 CI2
State Solid Solid Solid Liquid Liquid/Solid Liquid Gas
Bonding Ionic Ionic Covalent Simple covalent Simple covalent Simple covalent Simple covalent
m/p
(C)
High
(801)
High
(714)
Low
(178)
Low
(-70)
Low
(-112)
Low
(-80)
Low
(-101)
Conductivity Good
Ions
Good
Ions
Poor Poor Poor Poor Poor
Reaction
with
water
No reaction
Dissolve
✗
No reaction
Dissolve
✗
Water
hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Click here video chloride period 3
Chloride period 3 (Metal – Non metallic chloride )

6. Hydrogen ion ((H+) produced
Oxides period 3 (Metal – Non metallic )
Na2O MgO AI2O3 SiO2 P4O10
P4O6
SO3
SO2
CI2O7
CI2O
Bonding Ionic Ionic Ionic Giant covalent Simple covalent Simple covalent Simple covalent
Nature of
Oxide
Metal oxide
Basic oxide
Metal oxide
Basic oxide
Metal oxide
Amphoteric
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Reaction
with
water
Form
NaOH
(Alkaline)
Form
Mg(OH)2
(Alkaline)
No reaction
✗
No reaction
✗
Form
H3PO3
(Acidic)
Form
H2SO4
(Acidic)
Form
HCIO4
(Acidic)
Chemical reaction - Water hydrolysis
Breaking bond presence of water
Na2O + H2O -> 2NaOH -> 2Na+ + 2OH-
Metal /Basic oxide
Ionic
bonding
Hydroxide ion ((OH-) produced
Na2O -> 2Na+ + O2-
Oxide ion
:O:2- + H2O -> 2OH-
H
O
H
+
-
lone pair electron
attract to H+
+
H
O
H
O
2-
-
:
:
Bond break
pair electron move to oxygen
-
O
O2- produce OH- become alkaline
Water hydrolysis
Non Metal /Acidic oxide
covalent
bonding
Chemical reaction - Water hydrolysis
Breaking bond presence of water
SO2 + H2O -> H2SO3
Reaction mechanism
Reaction mechanism
O
O
S
-
-
+
Lone pair electron
attract to S+
Bond polarity of SO2
cause hydrolysis H2O
O
H
H
S
O
O
O
H
H
Bond break
O
O
O
H
S
H
H2SO3
H2SO3 -> 2H+ + SO3
2- - H+ makes it acidic

7. H2SO4H2SO4 -> 2H+ + SO4
2- - H+ makes it acidic
Hydrogen ion ((H+) produced
Oxides period 3 (Metal – Non metallic )
Na2O MgO AI2O3 SiO2 P4O10
P4O6
SO3
SO2
CI2O7
CI2O
Bonding Ionic Ionic Ionic Giant covalent Simple covalent Simple covalent Simple covalent
Nature of
Oxide
Metal oxide
Basic oxide
Metal oxide
Basic oxide
Metal oxide
Amphoteric
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Reaction
with
water
Form
NaOH
(Alkaline)
Form
Mg(OH)2
(Alkaline)
No reaction
✗
No reaction
✗
Form
H3PO3
(Acidic)
Form
H2SO4
(Acidic)
Form
HCIO4
(Acidic)
Chemical reaction - Water hydrolysis
Breaking bond presence of water
MgO + H2O -> 2MgOH -> 2Mg+ + 2OH-
Metal /Basic oxide
Ionic
bonding
Hydroxide ion ((OH-) produced
MgO -> Mg2+ + O2-
Oxide ion
:O:2- + H2O -> 2OH-
H
O
H
+
-
lone pair electron
attract to H+
+
H
O
H
O
2-
-
:
:
Bond break
pair electron move to oxygen
-
O
O2- produce OH- become alkaline
Water hydrolysis
Non Metal /Acidic oxide
covalent
bonding
Chemical reaction - Water hydrolysis
Breaking bond presence of water
SO3 + H2O -> H2SO4
Reaction mechanismReaction mechanism
O
O
S
-
-
+
Lone pair electron
attract to S+
Bond polarity of SO3
cause hydrolysis H2O
O
H
H
S
O
O
O
H
H
Bond break
O
O
O
H
S
H
O O O

8. Written in two waysWritten in two ways
Na2O MgO AI2O3 SiO2 P4O10
P4O6
SO3
SO2
CI2O7
CI2O
Bonding Ionic Ionic Ionic Giant covalent Simple covalent Simple covalent Simple covalent
Nature of
Oxide
Metal oxide
Basic oxide
Metal oxide
Basic oxide
Metal oxide
Amphoteric
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Reaction
with
water
Form
NaOH
(Alkaline)
Form
Mg(OH)2
(Alkaline)
No reaction
✗
No reaction
✗
Form
H3PO4
(Acidic)
Form
H2SO4
(Acidic)
Form
HCIO4
(Acidic)
Amphoteric oxide
+
OH
-
Act as acid
3+
High charge density AI3+
attract lone pair e of OH-
Act as base
AI2O3 + 3H2O or 2AI(OH)3 AI2O3 + 3H2O or 2AI(OH)3
3+
OH
-
As acid – react with base
AI2O3 + 3H2O + 2OH- -> 2AI(OH)4
-
2AI(OH)3 + 2OH- -> 2AI(OH)4
-
As base – react with acid
Al2O3 + 6HCI -> 2AICI3 + 3H2O
2AI(OH)3 + 6H+ -> 2AI3+ + 6H2O
H
H
H
H
H
H
+
+
+
+
+
+
AI
AI
H2O
H2O
H2O
H2O H2O
H2O
3+
3+
OH- react with H+ form H2O
Water hydrolysis
AI2O3 no reaction with water
BUT
reacts with either acid or base
-
-

9. Strong covalent bonds
H3PO3
P4O6 + 6H2O -> 4H3PO3
Hydrogen ion ((H+) produced
Na2O MgO AI2O3 SiO2 P4O10
P4O6
SO3
SO2
CI2O7
CI2O
Bonding Ionic Ionic Ionic Giant covalent Simple covalent Simple covalent Simple covalent
Nature of
Oxide
Metal oxide
Basic oxide
Metal oxide
Basic oxide
Metal oxide
Amphoteric
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Non metal oxide
Acidic oxide
Reaction
with
water
Form
NaOH
(Alkaline)
Form
Mg(OH)2
(Alkaline)
No reaction
✗
No reaction
✗
Form
H3PO3
(Acidic)
Form
H2SO4
(Acidic)
Form
HCIO4
(Acidic)
No reaction with water ✗
Non metal oxide
Giant macromolecular
structure
SiO2 + 2NaOH -> Na2SiO3 + H2O
SiO2 + 2OH- -> SiO3
2- + H2O
O
O
OSi
Bond break
-
Si
Non Metal/Acidic oxide
covalent
bonding
Chemical reaction - Water hydrolysis
Breaking bond presence of water
Lone pair electron
attract to P+
Bond polarity of P4O6
cause hydrolysis H2O
O
H
H
P
O
O
H
H
Bond break
O
O
H
P
H
H2PO3 -> 3H+ + PO3
2- - H+ makes it acidic
O O
H
As acid – react with base
O
H
Lone pair electron
attract to Si+
O
O
H
O
-
Water hydrolysis
SiO2 react with OH- -> SiO3
2-
H
SiO2 no reaction with water
BUT
reacts with base

10. Hydrogen ion ((H+) produced
NaCI(s) + H2O -> NaCI (aq)
MgCI2(s) + H2O -> MgCI2 (aq)
Ionic compound
Ionic
bonding
Ions are hydrated by water molecules
Ion attract polar H2O
Simple covalent
covalent
bonding
Chemical reaction - Water hydrolysis
Breaking bond presence of water
SiCI4 + 4H2O -> Si(OH)4 + 4HCI
Reaction mechanism show only ONE H2O
CI
Si
-
-
+
Lone pair electron
attract to Si+
Bond polarity of SiCI4
cause hydrolysis of H2O
O
H
H
Si
CI
O
H
Bond break H+ makes it acidic
NaCI MgCI2 AI2CI6 SiCI4 PCI3 S2CI2 CI2
Bonding Ionic Ionic Covalent Simple covalent Simple covalent Simple covalent Simple covalent
Conductivity Good
Ions
Good
Ions
Poor Poor Poor Poor Poor
Reaction
with
water
No reaction
(Neutral)
✗
No reaction
(Neutral)
✗
Water
hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Dissolving - NO chemical rxn
- NO water hydrolysis
Na+ CI-
Mg2+ CI-
CI-Mg2+
CI
CI
CI
-
-
CI
CI
CI
H
Si
CI
CI
CI
O
H
+ H
+
Water hydrolysis
Chloride period 3 (Metal – Non metallic chloride)
NaCI/MgCI2 no reaction with water

11. AICI3
Bond breaking
AICI3 + 3H2O -> AI(OH)3 + 3HCI
Water hydrolysis
Lone pair electron on
oxygen attract to AI3+
NaCI MgCI2 AI2CI6 SiCI4 PCI3 S2CI2 CI2
Bonding Ionic Ionic Covalent Simple covalent Simple covalent Simple covalent Simple covalent
Conductivity Good
Ions
Good
Ions
Poor Poor Poor Poor Poor
Reaction
with
water
No reaction
(Neutral)
✗
No reaction
(Neutral)
✗
Water
hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
CI
covalent
bonding
AI3+ion - small size, + high charge – high charge density
H
H
O
+
+
AI AI
CI
CI CI CI
CI CI
Covalent and ionic character
AI2CI6
High charge density AI3+
attract lone pair electron
from CI form dative bond
3+ 3+
High charge density AI3+
hydrated by six H2O AI3+
CI
CI
-
-
-
Water hydrolysis -breaking bond presence of water
AICI3 is acidic
Polarise H2O -release of H+ – ACIDIC
AI3+
+
CI
CI
CI
-
-
-
AI3+ :
:
H
H
H
H
H
H
O
O
O
AI3+
H
O
O
H
H
H
+
+
High charge density AI3+
hydrated by six H2O
H+ makes it acidic
Chloride period 3 (Metal – Non metallic chloride)
AICI3 written as AI(H2O)6
3+ + 3CI-

12. NaCI MgCI2 AI2CI6 SiCI4 PCI3 S2CI2 CI2
Bonding Ionic Ionic Covalent Simple covalent Simple covalent Simple covalent Simple covalent
Conductivity Good
Ions
Good
Ions
Poor Poor Poor Poor Poor
Reaction
with
water
No reaction
(Neutral)
✗
No reaction
(Neutral)
✗
Water
hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
Water hydrolysis
(Acidic)
H+ makes it acidic
SiCI4 + 4H2O -> Si(OH)4 + 4HCI
Chemical reaction - Water hydrolysis
Breaking bond presence of water
Hydrogen ion ((H+) produced
Simple covalent
covalent
bonding
Chemical reaction - Water hydrolysis
Breaking bond presence of water
PCI3 + 3H2O -> P(OH)3 /H3PO3 + 3HCI
CI
Si
-
-
+
Lone pair electron
attract to Si+
Bond polarity of SiCI4
cause hydrolysis H2O
O
H
H
Si
CI
O
H
Bond break
H+ makes it acidic
CI
CI
CI
-
-
CI
CI
CI
H
Si
CI
CI
CI
O
H
+ H
+
Simple covalent
covalent
bonding
Hydrogen ion ((H+) produced
P
H
+
CI
CI
CI
O
H
H
P
CI
CI
CI
O
H
H
Bond break
P
O
CI
CI
H
+
+
Chloride period 3 (Metal – Non metallic chloride)
Water hydrolysis
Reaction mechanism show only ONE H2O Reaction mechanism show only ONE H2O

13. Lone pair electron
attract to Si+
Bond polarity of SiCI4
cause hydrolysis H2O
H-
H
H
Bond break
Si
H
+
Reaction mechanism show ONE H2O Reaction mechanism show ONE H2O
Reaction mechanism show FOUR H2O Reaction mechanism show THREE H2O
Si
O
O
O
O
H
H
H
H
H
H
H
CI
CI
CI
CI
O
O
O
O
H
H
H
H
SiCI4 + 4H2O -> Si(OH)4 + 4HCI
-
-
-
P
O
O
O
H
H
H
H
CI
CI
CI
Lone pair electron
attract to P+
Bond polarity of PCI3
cause hydrolysis H2O
Bond break
+
O
O
O
P
H
H
PCI3 + 3H2O -> P(OH)3 /H3PO3 + 3HCI
+ +
CI
CI
CI
CI
CI
CI CI
-
-
-
-
-
- -
-
-
-