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Muhammad Hifzhuddin bin Yusri

Pb - Lead
Electronic Configuration : [Xe] 6s²4f¹⁴5d¹⁰6p2
Extraction :
2PbS + 2O₂ ---> 2PbO + 2SO₂
PbO + C ---> Pb(l) + CO(g)

Physicochemical properties :
- high density
- low boiling point
- high luster, ductile, highly malleable
- resists corrosion

Compounds of Pb :
1. Oxide (PbO, PbO₂, Pb₃O₄)
i) Lead oxide (PbO) (+2)
Preparation :
* Direct reaction between elements
Pb + O2 ---> PbO

*Thermal decomposition of Pb(NO₃)₂
or PbCO3
2Pb(NO₃)₂ ---> 2PbO + 4NO₂ + O₂
PbCO3 ---> PbO + CO2

- PbO is a yellow solid and has a
characteristic of amphoteric oxide

ii) Lead dioxide (PbO2) (+4)
Preparation :
*Heating Pb(II) solution with sodium
chlorate
Pb²⁺ + H₂O + ClO ---> PbO₂ + Cl⁻ +
2H+

*Red lead with nitric acids
Pb₃O₄ + 4HNO₃ ---> PbO₂ +
2Pb(NO₃)₂ + 2H₂O

Properties :
- dark brownish solid or black powder
- ionic compound
- strong oxidizing agent
- decompose when heating
- dissolves in acid such as H₂SO₄, HF
and HCl
- amphoteric oxide
- uses mainly as cathode in lead acid
battery

iii) Trilead tetraoxide (Pb₃O₄)
-Red lead
Preparation :
3Pb + O₂ ---> Pb₃O₄
PbO2 ---> Pb₃O₄ + O2

*contain mixture of PbO and PbO2
*have same properties like PbO and
PbO2

2. Halide (PbX₄ & PbX₂)
*PbX₂ is more stable than PbX4

i) Lead(IV) halide (PbX₄)
- only PbF₄ and PbCl₄ exist
- PbBr₄ and PbI₄ does not exist due to
Br and I are not strong oxidizing
agents

ii) Lead(II) halide (PbX₂)
- All of the halides exist as ionic form
- PbF₂, PbCl₂, PbBr₂ - white solid
- PbI₂ - yellow solid

3. Sulphide (PbS)
- only form PbS
- as black precipitate forms when H₂S is
passed through lead(II) solution
Pb²⁺(aq) +H₂S(g) ---> PbS(s) + 2H⁺

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SUMMARY OF GROUP IVA (LEAD , Pb) MUHAMMAD AFIQ A21HP0072

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SUMMARY OF GROUP IVA (LEAD , Pb) MUHAMMAD AFIQ A21HP0072

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General Information (Lead , Pb)
-existence : mineral-galena Pbs.
-Lead is innert pair effect.
-The electron configuration : [Xe] 6s²4f¹⁴5d¹⁰
-Physicochemical properties :
*high density but soft with low boiling point
*high luster, ductile and highly malleable
*resists corrosion

General reactions of Pb
- Pb + O₂ -> PbO further reaction with O₂ produce Pb₃O4
- Pb + H₂SO₄ -> PbSO₂ insoluble
- Pb + HNO₃ -> Pb(NO₃)2
- Pb + air/moisture → Oxy carbonate Pb

Compound of Pb (Oxide)
1) PbO (lead oxide)
preparation :
-direct reaction between elements
Pb + O₂ -> PbO
-thermal decomposition of Pb(NO₃)₂ or PbCO₃
2Pb(NO₃)₂ -> 2PbO + 4NO₂ + O2
PbCO₃ -> PbO + CO₂
-Properties of PbO
*yellow solid

2) PbO₂ (lead dioxide)
preparation :
-heating Pb(II) solution with sodium chlorate
Pb²⁺(aq) + H2O + ClO⁻(aq) -> PbO2 + Cl⁻(aq) + 2H+(aq)
-red lead with nitric acids
Pb₃O₄ (s) + 4HNO₃(aq) -> PbO₂ + 2Pb(NO₃)₂ (aq) + 2H₂O(l)
-Properties of PbO₂ :
*dark brownish solid / black powder
*ionic compound
*strong oxidizing agent
*decompose when heating
*dissolves in acid

3) Pb₃O4 ( Trilead tetraoxide)
Preparation:
3Pb(s) + O₂ -> Pb₃O2
PbO₂ (s) heat->Pb₃O₄ + O2
-Properties of Pb₃O₄ :
*read lead
*mixture of 2PbO.PbO2

Halide of lead
Lead Halides (PbX₄ & PbX₂)
-Pb(ll) halide is more stable than Pb(lV) halide.
1.Lead(lV), PbX4
*PbF₄ & PbCl₄ exists
*PbBr₄ & Pbl₄ do not exists-because Br₂ and l₂ are not strong oxidizing agents thus unable to oxidize Pb(ll) ->Pb(lV)

2.Lead(ll) halide,PbX2
All halide exixts in ionic form:
*PbF₂ : white solid
*PbCl2 : white solid
*PbBr2 : white solid
*Pbl2 : yellow solid

Lead Sulphide (PbS)
-only form PbS
-As black precipitate forms when H2S is passes through lead(ll) solution
-eq:Pb²⁺ +H₂S(g)--->PbS(s) + 2H⁺ (aq)

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Summary of Group IV ( Tin, Sn ) - UZAIR LATIF HADI BIN ABDUL RAHMAN ( A21HP0206)

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Summary of Group IV ( Tin, Sn ) - UZAIR LATIF HADI BIN ABDUL RAHMAN ( A21HP0206)

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1. General information :
[Kr] 4d¹⁰ 5s² 5p²

2. Tin Allotrope :

α-Sn = grey tin in powder form, diamond lattice structure, 5.75 g/cm³ of density.
β-Sn: white tin in metallic solid form, tetragonal / distorted octahedral lattice structure, 7.31 g/cm³ of density.
Tin-Plague: can change from (β-Sn) to (α-Sn) below 13.2 °C, causes an increase in volume and the tin metallic appearance becomes pock-marked.

3. Physicochemical Properties :
- Physical properties : soft metal, not very ductile, brittle (heat), crackles when bent
- Chemical Properties :

Sn + O2 → SnO₂

Sn + 2H₂O → SnO2 + 2H₂

Sn + Cl₂→ SnCl₂

Sn + 2HCl → SnO2 + 2H₂

4. Oxides :

i) SnO ₂ :-

Sn + O₂ → SnO₂

pure ionic oxide

does not dissolve in HCl, HNO₃ or aqua regia.

SnO₂ + H₂SO4 → Sn(SO₄)₂ + 2H₂O

SnO₂ + 2OH⁻ → SnO₃ ²⁻ + H₂O

ii) SnO :-

Black tin

Sn²⁺ → SnO + CO + CO₂

More base than SnO₂ because it has more electrons.

SnO + 2OH⁻ → SnO₂ ²⁻ + H₂O

SnO + 2H⁺ → Sn²⁺ + H₂O

5. Halides :
i) SnCl ₄

Sn + Cl₂→ SnCl₄

Colourless liquid

Covalent compound with tetrahedral structure

SnCl₄ + 2H₂O → SnO₂ + 4HCl

SnCl₄ + 2HCl → H₂SnCl₆

ii) SnCl ₂

Covalent compound

Soluble in water and organic solvents

Sn (s) hot + 2HCl → SnCl₂ + H₂

Sn + HCl conc. → SnCl₂ + H₂

SnO + HCl dil. → SnCl₂ + H₂O

dissolved in water to give cloudy solution due to formation by hydrolysis of basic chlorides

Strong reduce agent.

6. Sulfide :
i) SnS

Sn²⁺ + H₂S → SnS + H²⁺

Dark brown unstable solid

Easily oxidize to SnS₂

ii) SnS ₂

SnS + S → SnS₂

yellow solid → more stable

SnS₂ + (NH₄)₂S → (NH₄)₂SnS₃

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MUHAMMAD AMIRUL  BIN KHAIRUL NIZAM (A21HP0080)

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MUHAMMAD AMIRUL  BIN KHAIRUL NIZAM (A21HP0080)

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TIN (SN)
Electron Configuration :[kr]4d105s25p2

EXTRATION>
1-from (SnO2) undergo roasting to remove the impurities ( S, As)
2- then (SnO2) pure tin undergo  reduction using anthracite to remove slag so the final product is Sn

TIN ALLOTROPE
a- Tin
color : grey tin
structure :  diamond lattice
density : 5.75 g/cm3
Physical : Powder

b- Tin
color : white tin
structure :  tetragonal / distorted octahedral lattice
density : 7.31 g/cm3
Physical : metallic solid

physicochemical PROPERTIES

- Soft metal, malleable , but not very ductile, become brittle on heating , crackles when bent.

COMPOUNDS OF SN

1-OXIDES
SnO2
preparation :
Sn + O2 -> SnO2
pure ionic oxide
does not dissolve in HCL, HNO3 and aqua regia
Amphoteric oxide with H2SO4 and OH-

SnO ( black tin)
Preparation : heating tin oxalate
Amphoteric oxide (more than SnO2)
in acid :
SnO + 2H+ -> Sn2+ + H2O
in akali:
SnO + 2OH-  -> SnO₂ 2- + H20

2- HALIDES
SnCl4
preparation :
Sn + Cl4 -> SnCl4
colorless liquid
covalent compound with tetrahedral structure

SnCl2
Preparation :
Sn( s) + 2 HCl( aq) → SnCl₂(aq) + H₂(g)
dissolve in water to give cloudy solution due to formation by hydrolysis of basic chlorides
strong reducing agent

3-SULFIDE
SnS
Preparation :
Sn2+ + H2S -> SnS + H+
Dark Brown unstable solid
easily oxidize

SnS2
preparation :
SnS + S -> SnS2
yellow solid
dissolve in excess of (NH4)2SnSx
SnS2 + (Nh4)2S -> (NH4)2SnS3

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NUR ANIS SYAFIQA BINTI ABDUL RASHID | A21HP0132 (Carbon)

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NUR ANIS SYAFIQA BINTI ABDUL RASHID | A21HP0132 (Carbon)

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SUMMARY OF GROUP IVA (Lead, Pb) - YASMIN BINTI AZMAN (A21HP0214)

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SUMMARY OF GROUP IVA (Lead, Pb) - YASMIN BINTI AZMAN (A21HP0214)

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#Electronic configuration :
[Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²

Extraction :
2PbS + 2O2 → 2PbO + 2SO2
PbO + C → Pb(l) + CO(g)

#Physiochemical properties :
-High density
-Low boiling point
-High luster and malleable
-Resists corrosion

#General reactions :
== with O2
Pb--> PbO +O2→Pb3O4

== with Nitric Acid
Pb + HNO3 → Pb(NO3)2

== with Sulphuric Acid
Pb + H2SO4 → PbSO4 (insoluble)

== with air/moisture
Pb + Air/moisture → Oxy carbonate Pb

#Compounds of Pb :

1)Oxide
Exists as PbO, PbO2, Pb3O4

==>PbO (lead oxide)
-oxidation state, +2
-Reaction:
Pb + O2 → PbO  (not like SnO2)

-Thermal decomposition :
2Pb(NO3)2 → 2PbO + 4NO2(brown gas) + O2
PbCO3 → PbO + CO2

-yellow solid (amphoteric oxide)
PbO + 2HCL → PbCl2 + H2O
PbO + 2OH- + H2O → Pb(OH)4^2-
From Pb(OH)4^2-, forms PbO2^2- + 2H2O

==>PbO2 (lead dioxide)
-Preparation :
Pb2+ + H2O + ClO- → PbO2 + Cl- + 2H+
Pb3O4 + 4HNO3 → PbO2 + 2Pb(NO3)2 + 2H2O

Properties :
-Dark brownish solid / black powder
-PbO2, ionic compound (Pb4+ / O2-)
-Strong oxidizing agent
HCl → Cl2
SO2 → SO4^2-
Mn2+ → MnO4-

-Decompose when heating
PbO2 → Pb3O4 + O2

-Dissolves in acid
PbO2 + 2H2SO4 → PbSO4 + 2H2O
PbO2 + 2HF → H2PbF6 + 2H2O
PbO2 + 2HCL → H2PbCl6 + 2H2O

-Amphoteric oxide
PbO2 + 4HCL → PbCl2 + Cl2 + 2H2O
PbO2 + 2OH- → PbO3^2- + H2O

-Used as cathode in Lead Acid Battery

==>Pb3O4 (lead tetraoxide)
-Read lead
-Mixture of 2PbO.PbO2

-Preparation :
3Pb + O2 → Pb3O4
PbO2 → Pb3O4 + O2

2)Halide
-The stability of Pb(II) halide > Pb(IV) halide

==>PbX4
-(PbF5 & PbCl4 exist)
-(PbBr4 and PbI4 do not exist)
-Br2 & I2 are not strong oxidizing agent, unable to oxidize Pb(II) → Pb(IV)

==>PbX2
-Exists in ionic form
PbF2 / PbCl2 / PbBr2 ===> white solid
PbCl2 ===> yellow solid

==>PbS
-Only forms PbS
-Exists as black precipitate, forming H2S, passed through Lead (II) solution
Pb2+ + H2S → PbS + 2H+

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Summary of Group IV (Pb, Lead) - NUR MIRZA AMELIN BT ZAMRI (A21HP0150)

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Summary of Group IV (Pb, Lead) - NUR MIRZA AMELIN BT ZAMRI (A21HP0150)

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1. General information:
a) Electron configuration:
[Xe] 6s2 4f14 5d10

b) Existence: mineral-galena, PbS

c) Extraction:
2PbS + 2O2 -> (roast) 2PbO + 2SO2
PbO + C -> Pb (l)+ CO (g)

d) Physicochemical properties:
- high density but soft with low boiling point.
-high luster, ductile & highly malleable
- resist corrosion

- obtained by oxidation of SnS using ammonium polysulfides (NH4)2Sx

SnS (s) + S (s) -> SnS2 (S)
- yellow solid
- dissolves in excess of (NH4)2Sx
SnS2 (s) + (NH4)2S -> (NH4)2SnS3

2. General reactions:
a) Pb (air, moisture) ---> oxy carbonate Pb
b) Pb + O2 (heat) --> PbO +O2 --> PbO34
c) Pb + H2SO4 --> PbSO4 (insoluble)
d) Pb + HNO3 --> Pb(NO3)2

3. Compounds of Pb:
- Oxide
- exist as PbO, PbO2 & Pb3O4
a) PbO : lead oxide (oxidation state: +2)
*Preparation
i) direct reaction between elements
Pb + O2 -> PbO

ii) thermal decomposition of Pb(NO3)2 / PbCO3
2Pb(NO3)2 -> 2PbO + 4NO2 +O2
PbCO3 -> PbO +CO2

- PbO: yellow solid
- amphoteric oxide
PbO (s) + 2HCl -> PbCl (aq) + H2O
PbO (s) + 2OH- (aq) + H2O -> Pb(OH)4 2- (aq) -> PbO2 2- + 2H2O

b) PbO2: lead dioxide
- Preparation
i) heating Pb(II) solution with Sodium chlorate
ii) red lead with nitric acid

- properties
i) dark brownish solid/ black powder
ii) ionic compound: Pb4+ & O2-
iii) strong oxidizing agent: +4 --> +2
iv) decompose when heating
v) dissolves in acids

- amphoteric oxide
PbO2 + 4HCl -> PbCl2 + Cl2 + 2H2O
PbO2 + 2OH- -> PbO3 2- (aq) + H2O

c) Pb3O4: Trilead tetraoxide
- red lead
- mixture of 2PbO . PbO2
- preparation:
3Pb (s) + O2 -> Pb3O4
PbO2 (s) (heat) -> Pb3O4 + O2
- shows properties like PbO & PbO2

4. Uses of lead compounds as pigment for paint:
i) Red colour
- red lead (Pb3O4)
- red lead commonly used to protect iron & steel from rusting
ii) White colour
- white lead (2PbCO3. Pb(OH)2)
- 75% PbSO4, 20% PbO, 5% ZnO

5. Halide of Lead:
- lead halide: PbX4 & PbX2
- Pb(II) more stable than Pb(IV)
a) Lead (IV) halide, PbX4
* PbF4 & PbCl4 exists
* PbBr4 & PbI4 not exist because Br2 & I2 are not strong oxidizing agents

b) Lead (II) halide, PbX2
* all halides exist in ionic form
PbF2 - white solid
PbCl2 - white solid
PbBr4 - white solid
PbI2 - yellow solid

6. Lead sulphide (PbS):
- only forms PbS
- black precipitate form when H2S is passed through lead (II) solution
- Pb2+(aq) + H2S (g) -> PbS (s) + 2H+ (aq)

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Summary of Group IVA (Silicon,Si)- Noor Khairiyah binti Hasnul Hadi (A21HP0115)

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Summary of Group IVA (Silicon,Si)- Noor Khairiyah binti Hasnul Hadi (A21HP0115)

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Silicon (Si)

Silicon exists as Silicon dioxide (SiO2) and silicate substances on earth.

We can extract Si and obtain pure Si by:

-Reducing SiO2 by coke through electrical furnace.

-Reducing SiCl4 by using Na

-Zone refining process that yields (99.999% pure Si)

Characteristics:

-Has metallic luster and grayish colour for crystalline Si.

-Has diamond lattice

-High melting point

-An inert element but attack by halogen

-Dissolve in base

-Does not dissolve in any acids except for HF.

Silicon Compounds

1.Oxides

Oxide compound of silicon is an inert at low temperature but becoming reactive as the temperature increases plus turned to strong acidic oxide. It dissolves I alkali and HF only.

-Silicon dioxide/ silica (SiO2)

-Exists in a polymeric tetrahedral of SiO2

- Overall molecule is a covalent macromolecule with the formation of polymorph.

Preparation of SiO2

-Hydrolysis of SiCl4 (Silicon tetrachloride)

-Acidification of water glass@ Sodium silicate (Na2SiO3)

2.Silicate (SiO4)4-

-SiO2+ metal X, X=oxides, sulphate, carbonate

-A polymorph (SiO4)4- structured that consist of tetrahedral SiO4 connected through Si-O-Si   bonds.

Aluminosilicate (3-D Silicate)

It occurs when Al atom substitutes Si in the silicate framework.

Examples: Feldspar, Zeolite

Focusing on Zeolite which is a hydrated aluminosilicate.

-As a molecular sieves since it has regular size of pores and channels to separate different sizes of  molecule.

-As an ion exchanger in water softening

-Becoming a strong acidic solid catalyst if the ion is exchanged with H+.

Silicate glass (sand+metal, alumminosilicate, borosilicate)

-          Not a true solid( a supercooled liquid having a very high viscosity that impossible for a free flow liquid.

-          It is amorphus.

-          Inert but attacked by F2, HF and alkali.

Types: Soft glass, hard glass, crooke’s glass, jena glass, flint glass, pyrex glass, ground and reinforced glass. ( These glasses have different uses)

3.Silicones

-An organosilicon compounds (heterocatenated Si-O-Si-O bonds in chains,rings and branches).

-Prepared by hydrolysis of alkyl/aryl silicon halides followed with condensation.

-Types: Disilicone, chain silicone, branched silicone.

-A thermally stable up to (500-700K)

-Low viscosity

-At low temperature silicone rubbers still elastic

-Inert towards chemical attack& oxidation,

Uses: as a makeup primer, breast implant shell, low temperature hydraulic fluids.

4.Silicon Halides (SiX4)

-SiCl4, a series of chlorides up to Si6Cl14 are known.

- All halides are unstable except for SiF4 and undergo hydrolysis in water plus SiF4 undergoes a partial hydrolysis.

-Hydrolysis occurs by the formation of dative bonding from O atom of water to the Si of SiX4 where X= halogen.

Hydrolysis: SiX4+ 2H2O à SiO2 +4HX

X= Cl,Br,I

Partial hydrolysis: 2SiF4 + 2H2O à SiO2 (s)  + H2SiF6 (aq)  + 2HF(aq)

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Summary of Group IV Element ( Tin, Sn) [TAN SOK JING A21HP0225]

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Summary of Group IV Element ( Tin, Sn) [TAN SOK JING A21HP0225]

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General Information

Tin (Sn)
- Metal
-Electron configuration: [Kr]4d¹⁰ 5s² 5p2

Allotropes of Tin

·       3 Types :* alpha (most unstable, lower temperature),* beta (most common, at higher temperatures), gamma (only at very high temperatures)

·       Alpha tin (α-Sn)- Grey tin, loses the metallic properties, turns powdery, can used to plate iron food cans to prevent them from rusting.

·       Beta tin (β-Sn)- White tin, often used in alloy

·       Tin Plague/ Tin-pest (crystalline structure is broken)

- β-Sn→ α-Sn (causes deterioration of tin at low temperature)

Physicochemical Properties

·       Physical properties: soft metal, not very ductile, brittles (heating)

·       Chemical Properties:

1. Reaction of tin with oxygen:

Sn (s) + O2 (g)→ SnO2 (s) [Tin(IV) oxide]

2. Reaction of tin with water(steam)

Sn (s) + 2H₂O (g)→ SnO₂(s)+ 2H₂ (g)

3. Reaction of tin with chloride

Sn + Cl₂→ SnCl₂

4. Reaction of tin with HCI

Sn (s) + 2HCl (g)→ SnO₂(s)+ 2H₂ (g)

Oxides

· 2 oxidation states: +2 and +4

· Tin(IV) oxide is more stable than Tin(II) oxide.

· Both are amphoteric oxide as can react with both acid and bases.

1. SnO₂ [ Tin(IV) oxide]

· Pure ionic oxide.

· Does not dissolve in HCl, HNO₃ and aqua regia.

· Direct heating of metal in air: Sn + O₂→ SnO₂

2. SnO [Tin(II) oxide]

· Black tin

· More base than SnO₂

·Heating of oxalate : Sn²⁺→ SnO +CO +CO2

Halides

SnCl₂ (dichloride)  is more stable than SnCI4

· Direct heating of the elements: Sn + Cl₂→ SnCl₄

· Colorless liquid

· Covalent compound with tetrahedral structure

·SnCl₄ rapidly hydrolyzed and fuming in moist air:

SnCl₄ + 2H₂O → SnO₂ + 4HCI

· With conc. HCI / NH₄CI form complex SnCI₆ ²⁻

SnCI₄ + 2HCl → H₂SnCI₆

SnCI ₂ (dichloride)

·  Covalent compound

·  Soluble in water and organic solvents

·  Preparation:

a) Anhydrous SnCl2 : Sn (s) hot + 2HCl → SnCI₂ + H₂

b) Hydrated SnCl₂.2H2O :
Sn + HCl conc. → SnCl₂ + H₂

SnO + HCI dil. → SnCl₂ + H₂O

·  Dissolved in water : give cloudy solution

[Sn (OH)2 . SnCl₂]

·  Strong reducing agent, undergo oxidation.

Sulfide [SnS – mono (+2) , SnS ₂ – disulphide (+4)]

SnS

· Preparation :

1.  By passing through the H₂S gas in Sn(II) solution

Sn²⁺ + H₂S → SnS + H²⁺

·  Dark brown unstable solid as it prefers to form SnS2

SnS 2

· Preparation:

1. Oxidation of SnS using ammonium polysulfides (NH₄)₂Sx (mixture of (NH₄)₂S and S)

SnS + S → SnS₂

·  Yellow solid

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SUMMARY OF Group IV ELEMENT (Sn) - LAI LI YIE (A21HP0049)

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SUMMARY OF Group IV ELEMENT (Sn) - LAI LI YIE (A21HP0049)

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1. Electron configuration : [Kr] 4d10 5s2

2. Sn can be purified by :
a. Electrolysis
b. Melting

3.Tin allotrope
a.Alpha- Sn (grey)
b.Beta-Sn (white)
c. Gamma-Sn

4.

Structure of alpha-Sn : Diamond lattice

Physical appearance of alpha-Sn : Powder

Structure of Beta-Sn: Powder

Physical appearance of Beta-Sn : Metallic solid

White Beta-Sn change to grey Alpha-Sn below 13.2 degree celcius. This cause volume increases and tin metallic appearance becomes pock-marked.

5. Physicochemical properties of Sn
a. soft metal
b. malleable
c.brittle on heating
d. crackles when bent

6.  Oxide (SnO2, SnO)
I. Oxidation number of Sn is +4 in SnO2.

Sn(s) + O₂(g) → SnO₂(s)

- Pure ionic oxide

- Does not dissolve in HCl, HNO₃ or aqua regia
-Amphoteric Oxide
i. WITH H₂SO₄  (ACID)

SnO₂(s) + H₂SO₄→  Sn(SO₄)₂(s) + 2H₂O

ii.WITH OH⁻ (ALKALI)

SnO₂(s) + 2OH- →  SnO₃ ²⁻(aq) + H₂O

II. Oxidation number of Sn is +2 in SnO.
-Sn
-  Black tin

-  Preparation: heating tin oxalate

-  Amphoteric oxide is more base than SnO₂ and more Lewis basic because it has more electrons than tin(IV)

i) In acid:

SnO(s) + 2H⁺(aq) → Sn²⁺(aq) + H₂O

ii) In alkali:

SnO(s) + 2OH- (aq) → SnO₂ ²⁻(aq) + H₂O

7. Halides (SnCl ₄, SnCl ₂)

a. SnCl ₄

- Preparation: direct heating of the elements

Sn(s) + Cl₂(g) → SnCl₄(s)

- Colourless liquid

- Covalent compound with tetrahedral structure

i） In moist air, rapidly hydrolyzed and fuming

SnCl₄(l) + 2H₂O(l) →  SnO₂(s) + 4HCl(g)

ii） With conc.HCl/NH₄Cl → complex SnCl₆ ²⁻

SnCl₄(l) + 2HCl(aq) →  H₂SnCl₆(aq)

b. SnCl ₂

- Covalent compound

- Soluble in water and organic solvent

-  Preparation:

i) Anhydrous SnCl2

Sn(s) hot + 2HCl(g) → SnCl₂ + H2

ii) Hydrated SnCl 2. H ₂ O

Sn(s)  + HCl conc. → SnCl₂ + H₂

Sn(s)  + HCl(aq) dil → SnCl₂ + H₂O

- Cloudy solution formed when dissolved in water

SnCl₂(s) + 2H₂O (l) → Sn(OH)2.SnCl₂(s) + HCl(aq)

- Heating SnCl 2. H ₂ O form basic chlorides

SnCl2.H₂O → Sn(OH)2.SnCl₂(s) + HCl(aq) + 2H₂O

- Strong reducing agent

- reduce Mecury(I) chloride to Mecury

Sn²⁺(aq) + Hg₂Cl₂→ Hg(l) + Sn⁴⁺(aq) +2Cl⁻(aq)

8.Sulfide (SnS, SnS ₂)

a) SnS

- Exists as mono

- Obtained by passing through the H₂S gas in Sn(II) solution

Sn²⁺(aq) + H₂S → SnS (s) +H⁺(aq)

- Dark brown solid

- Easily oxidize to SnS₂

b) SnS ₂

- Exists as disulphide

- Obtained by undergies oxidation of SnS using (NH₄)₂SX (mixture of (NH₄)₂S and S)

SnS(s) + S(s) → SnS₂ (s)

- Yellow solid

- Dissolves in excess of (NH₄)₂SX

SnS₂ (s) + (NH₄)₂S → (NH₄)₂SnS₃

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SITI NURFARIESHAH BINTI SUBOH (A21HP0199) - Sn(Tin) 

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SITI NURFARIESHAH BINTI SUBOH (A21HP0199) - Sn(Tin) 

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Sn (Tin/Timah)4d¹⁰5s²5p²

#Extraction:
1.  Cassitserite (SnO2 ) go through roasting to get Pure Tin Ore (pure SnO2) with some impurities (S,As).
2. Pure tin Ore SnO2 go through reduction with  C (anthracite) and get Sn (slag)
SnO2 (s) + 2C(p) → 2Sn(l) + 2CO(g)
3. Sn undergo purification : melting and electrolysis
electrolysis :  H2SiF6 , H2SO4 SnSO4 -electrolytes
anode : SnO2 (impure Sn)
cathode : Sn (pure)

# Tin Allotrope
α-Sn⇆β-Sn⇆γ-Sn⇆liquid Sn

13.2°C   161°C   232°C
Properties:
α-Sn: grey tin in powder form & diamond lattice structure
β-Sn: white tin in metallic dolid form & tetragonal/disorted octahedral lattice structure
Tin-Plagu/Tin pest: can change from (β-Sn  white tin) to (α-Sn grey tin) below 13.2 °C, causes an increase in volume and the tin metallic appearance becomes pock-marked

# Physicochemical Properties
soft metal, malleable, but not very ductile, becomes brittle on heating, crackles when bent
# Chemical properties
Oxygen Forms on heating Sn + O2 → SnO2 No Sn3O4 oxide (this happens for Pb )

# Compound of Sn
Tin exists in two oxidation states, +4 and +2
1.Oxides (SnO2,SnO)
i) SnO2 (+4)
-> Preparation : direct heating on Sn on air/ oxygen
Sn(s) + O₂(g) → SnO₂(s)

-> Pure ionic oxide

-> Does not dissolve in HCl, HNO₃ or aqua regia

-> Amphoteric oxide

i) With H₂SO₄ (acid):
SnO₂(s) + H₂SO₄→  Sn(SO₄)₂(s) + 2H₂O

ii) With OH⁻ (alkali)
SnO₂(s) + 2OH- →  SnO₃ ²⁻(aq) + H₂O

ii) SnO(+2)

-> Black tin

-> Preparation: heating tin oxalate

-> Amphoteric oxide: Lewis basic then SnO2 because it has more electrons than tin(IV)

i) with acid:
SnO(s) + 2H⁺(aq) → Sn²⁺(aq) + H₂O

ii) with alkali:

SnO(s) + 2OH- (aq)

----------SnO₂ is more stable than SnO-------

2. Halides (SnCl ₄, SnCl ₂)

i) SnCl₄

-> Preparation: direct heating
Sn(s) + Cl₂(g) → SnCl₄(s)

ii) SnCl₂

-> Covalent compound

-> Soluble in water and organic solvent

->  Preparation:

1) Anhydrous SnCl₂

Sn(s) hot + 2HCl(g) → SnCl₂ + H₂

2) Hydrated SnCl2.H₂O

Sn(s)  + HCl conc. → SnCl₂ + H₂

Sn(s)  + HCl(aq) dil → SnCl₂ + H₂O

-----SnX₂ is more stable than SnX4-------
3)Sulfide
-> SnS(exist as mono) SnS2(exist as disulphide)

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Summary of Group IVA element Lead (Pb) - Irene Michelle Anak Dony (A21HP0040)

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Summary of Group IVA element Lead (Pb) - Irene Michelle Anak Dony (A21HP0040)

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Electronic Configuration : [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²

Physicochemical Properties
-High Density as it is heaviest common element, Low Boiling Point
-High Luster, ductile & highly malleable
-Resists corrosion

Compounds of Pb :
OXIDE
Exists as PbO, PbO2 & Pb3O4
i) PbO (Lead Oxide)
Oxidation state :+2
Preparation :
1. Direct reaction between elements
Pb + O2 --> PbO
2. Thermal Decomposition of Pb(NO3)2 or PbCO3
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
PbCO3 --> PbO + CO2

ii) PbO2 (Lead Dioxide)
Preparation
1. Heating Pb(II) solution with sodium chlorate
Pb+2   + H2O + ClO⁻ --> PbO2 + Cl⁻ + 2H+
2. Red Lead with Nitric Acids
Pb3O4 + 4HNO3 --> PbO2 + 2Pb(NO3)2    + 2H2O
Properties
- Dark Brownish solid or black powder
- PbO2 is an ionic compound
- Strong oxidizing agent (+4 --> +2)
-Decomposes when heating form Pb3O4 and O2
- Dissolves in acids
Uses
- Mainly as cathode in Lead Acid Battery

iii) Pb3O4 ( Trilead Tetraoxide)
-Red lead
-Mixture of 2PbO.PbO2
Preparation
3Pb + O2 --> Pb3O4
PbO2 --> Pb3O4 + O2
Uses
-Red lead (red pigment) is commonly used to protect iron and steel from rusting

HALIDE
PbX4 & PbX2
Pb(II)halide more stable than Pb(IV) halide

i)Lead(IV) halide, PbX4
- PbF4 & PbCl4 exist but PbBr4 & PbI4 do not exist due to weak oxidizing agents so that unable to oxidize Pb(II) --> Pb(IV)
ii)Lead(II) halide, PbX2
-Exist in ionic form
-White solid ( PbF2, PbCl2 & PbBr2)
-Yellow solid (PbI2)

LEAD SULPHIDE
-only forms PbS
-Black precipitate forms when H2S is passed through lead(II) solution
Pb2⁺ + H2S --> PbS + 2H⁺

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Summary of Group IV Element Lead(Pb) - NUR SYIDAH BINTI SALIM

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Summary of Group IV Element Lead(Pb) - NUR SYIDAH BINTI SALIM

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Electronic configuration: [Xe]6s¹4f¹⁴5d10

Extraction:
1) 2PbS + 2O₂ -->  2PbO + 2SO2
2) PbO + C --> Pb(l) + CO (g)

Physiochemical of Lead:
- High density since it is heaviest common element but soft
- low boiling point
- high luster, ductile, and highly malleable
- Resist corrosion

Compounds of Lead:
1) OXIDE (PbO, PbO₂, Pb₃O₄)

a) PbO (Oxidation state:+2)

Preparation:
i - Direct reaction between elements
Pb + O₂ --> PbO
ii - Thermal decomposition of Pb(NO₃)₂ or PbCO3
2Pb(NO₃)₂ --> 2PbO + 4NO₂ +O₂
PbCO₃ --> PbO + CO2
- Yellow solid

b) PbO 2 (Oxidation state:+4)
Preparation:
i - Heating Pb(II) solution with sodium chlorate
Pb2+ (aq) + H²O + ClO⁻(aq) --> PbO₂(s) + Cl⁻(aq)+ 2H⁺(aq)
ii - Red lead with nitric acid
Pb₃O₄(s) + 4HNO₃(aq) --> PbO₂(s) + 2Pb(NO₃)₂(aq) + 2H₂O(l)

Properties

- Dark brownish solid or black powder
- PbO₂ is an ionic compound
- Strong oxidizing agent
- Decompose to Pb₃O₄ and O₂ when heating
- Dissolves in acids

Uses

As cathode in Lead Acid Battery

c) Pb ₃ O 4 (Mixture of 2PbO.PbO₂) Red Lead

Preparation

i - 3Pb(s) + O₂ --> Pb₃O₄
ii - PbO₂(s) --> Pb₃O₄ + O₂

Uses

Red Lead - Used in paint industry to give the red pigment. Paint made with red lead is commonly used to protect Iron and Steel from rusting.

2) HALIDE (PbX₄ and PbX₂)
Pb(II) halide is more stable than Pb(IV) halide

a) Lead(IV) halide, PbX4
- PbF ₄ and PbCl ₄ but PbBr4 & PbI₄ do not exist because Br₂ and I₂ are not strong oxidizing agent thus unable to oxidize Pb(ii) to Pb(IV)

b) Lead(II) halide, PbX ₂
- All halides exist in ionic form
- White solid: PbF₂, PbCl₂, PbBr₂
- Yellow solid: PbI2

c) Lead Sulphide (PbS)
- Only forms PbS
- As black precipitate forms when H2S passed through lead(II) solution
Pb²⁺(aq) + H₂S(g) --> PbS(s) + 2H⁺(aq)

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Summary of Group IVA element (Pb)- Iman Adlina

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Summary of Group IVA element (Pb)- Iman Adlina

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LEAD,Pb

Electronic configuration=6s²f¹⁴5d¹⁰

Properties= high density, low BP, ductile, high malleable and resist corrosion

Used=major in paint pigment(Pb₃O₄ and 2PbCO3.Pb(OH)₂)

Extraction=

i)2PbS+2CO₂ →2PbO+2SO₂

ii)2PbO+C →Pb+CO

OXIDE

1)      PbO (oxidation state=+2, , amphoteric acid, lead(II) yellow solid)

Preparation:

i) Pb+O₂ →PbO (not PbO2 like SnO₂)

ii) Thermal decomposition PB(NO₃)₂ or PbCO3
2Pb(NO₃)₂ →2PbO+4NO₂+O₂

2)      PbO 2 (oxidation state=+4, strong oxidizing agent(sbb dia always nk direduced since Pb(II) more stable than Pb(IV),black solid)

Preparation:

i)Heating Pb(II) with ClO⁻; Pb²⁺+2H₂O+ClO⁻ →PbO₂+Cl⁻+2H⁺

ii)Red Lead with HNO₃;
PbO₃O₄+4HNO₃ →PbO₂+2Pb(NO₃)₂+2H₂O

-decompose when heating(into Pb₃O₄)

-dissolves in acid;
(eg: PbO₂+2h₂SO₄ →PbSO₄+2H₂O)

-act as amphoteric acid

-mainly used as cathode in lead acid battery

3)      Pb ₃ O 4 (trilead tetraoxide, red lead)

Preparation:

i)3Pb+O₂ →Pb₃O₄

ii)PbO₂ →Pb₃O₄₊O₂

HALIDE

-Pb(II) halide is more stable than Pb(IV) halide

-PbF4  and PbCl₄ exist but PbBr4 and PbI₄ not exist bcs it is weak oxidizing agent

- PbF2, PbCl2a and PbBr2 are white solid while PbI2 is yellow solid

SULPHIDE

-Only form PbS(black precipitation)

-Pb²⁺+H₂S →PbS+2H+

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Summary of Group IVA Element Tin (Sn) - ONG SHI TING A21HP0181

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Summary of Group IVA Element Tin (Sn) - ONG SHI TING A21HP0181

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Electronic configuration: [Kr]4d¹⁰5s²5p2

Extraction:

1. Cassiterite (SnO₂) undergo roasting to get the pure SnO₂ (some impurities S, As)

2. Pure SnO₂ undergo reduction with anthracite (C) to get Sn (Slag is produced)

3. Purification: Sn undergo electrolysis- H₂SiF₆, H₂SO₄, SnO4 act as electrolytes

4. SnO₂ (as anode), pure Sn (as cathode)

Tin Allotrope:
α-Sn⇆β-Sn⇆γ-Sn⇆liquid Sn

13.2°C   161°C   232°C

a) α-Sn

- Grey tin

- Diamond lattice structure

- In powder form

b) β-Sn

- White tin

- Tetragonal/ distorted octahedral lattice structure

- Metallic solid

Tin-plague

- Also known as tin pest

- Change from white (β-Sn) to grey tin (α-Sn)

- Increase in volume and the metallic appearance become pock-marked

Physicochemical Properties:

a) Soft metal, become brittle on heating, crackles when bent

b) Chemical properties:

- Sn react with O₂ form SnO2 on heating (No Sn₃O₄ oxide, this happens for Pb)

- Sn react with Cl₂ form SnCl₄ on heating

- Sn react with conc. HCl form hydrated SnCl₂

Compound of Sn

1. Oxides (SnO₂, SnO)

a) SnO₂

- Preparation: direct heating of the Sn
Sn(s) + O₂(g) → SnO₂(s)

- Pure ionic oxide

- Does not dissolve in HCl, HNO₃ or aqua regia

- Amphoteric oxide

i) With H₂SO₄ (acid):
SnO₂(s) + H₂SO₄→  Sn(SO₄)₂(s) + 2H₂O

ii) With OH⁻ (alkali)
SnO₂(s) + 2OH- →  SnO₃ ²⁻(aq) + H₂O

b) SnO

-  Black tin

-  Preparation: heating tin oxalate

-  Amphoteric oxide: more base than SnO₂ and more Lewis basic because it has more electrons than tin(IV)

i) In acid:
SnO(s) + 2H⁺(aq) → Sn²⁺(aq) + H₂O

ii) In alkali:

SnO(s) + 2OH- (aq) → SnO₂ ²⁻(aq) + H₂O

**SnO ₂ is more stable than SnO

2. Halides (SnCl₄, SnCl₂)

a) SnCl₄

- Preparation: direct heating of the elements
Sn(s) + Cl₂(g) → SnCl₄(s)

- Colourless liquid

- Covalent compound with tetrahedral structure

- In moist air, rapidly hydrolyzed and fuming
SnCl₄(l) + 2H₂O(l) →  SnO₂(s) + 4HCl(g)

- With conc.HCl/NH₄Cl → complex SnCl₆ 2-
SnCl₄(l) + 2HCl(aq) →  H₂SnCl₆(aq)

b) SnCl₂

- Covalent compound

- Soluble in water and organic solvent

-  Preparation:

i) Anhydrous SnCl2  (transparent crystalline solid)

Sn(s) hot + 2HCl(g) → SnCl₂ + H₂

ii) Hydrated SnCl 2. H ₂ O

Sn(s)  + HCl conc. → SnCl₂ + H₂

Sn(s)  + HCl(aq) dil → SnCl₂ + H₂O

- Dissolved in water- cloudy solution (formation by hydrolysis of basic chlorides)

SnCl₂(s) + 2H₂O (l) →  Sn(OH)2.SnCl₂(s) + HCl(aq)

- Heating SnCl2.H₂O form basic chlorides

SnCl2.H₂O → Sn(OH)2.SnCl₂(s) + HCl(aq) + 2H₂O

- Strong reducing agent

e.g. reduce Mecury(I) chloride → Mecury

Sn²⁺(aq) + Hg₂Cl₂→ Hg(l) + Sn⁴⁺(aq) +2Cl⁻(aq)

**SnX ₂ is more stable than SnX ₄

3. Sulfide (SnS, SnS₂)

a) SnS

- Exists as mono

- Preparation: passing through the H₂S gas in Sn(II) solution

Sn²⁺(aq) + H₂S → SnS (s) +H⁺(aq)

- Dark brown solid

- Unstable- easily oxidize to SnS₂

b) SnS₂

- Exists as disulphide

- Preparation: oxidation of SnS using (NH₄)₂SX (mixture of (NH₄)₂S and S)

SnS(s) + S(s) → SnS₂ (s)

- Yellow solid

- Dissolves in excess of (NH₄)₂SX

SnS₂ (s) + (NH₄)₂S → (NH₄)₂SnS₃

**SnS ₂ is more stable than SnS

# data[].attributes.headline
Summary of an element of Group IVA (Tin)- Norsyafiqa Madlan (A21HP0120)

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Summary of an element of Group IVA (Tin)- Norsyafiqa Madlan (A21HP0120)

# data[].attributes.body
Electronic Configuration : [Kr]4d¹⁰5s²5p²

Allotropes (different physical form) :

1) α-Sn
Properties = Grey Tin
Structure = Diamond lattice
Density = 5.75 g/cm3
Physical appearance = Powder

2) β-Sn
Properties = White Tin
Structure = Tetragonal / Distorted octahedral lattice
Density = 7.31 g/cm3
Physical appearance = Metallic solid

3)  γ-Sn

4) Tin-Plague or Tin-Pest
-The conversion from β-Sn to α-Sn below 13.2 ° C causes an increase in the volume and appearance of tin metal.

Physiochemical Properties

-Soft metal
-Malleable
-not very ductile
-becomes brittle on heating
-crackles when bent

Compound of Sn

1) Oxides (SnO₂,SnO)
SnO₂ (Tin (IV) Oxide)
*We can get SnO₂  by direct heating of the metal in air or oxygen.
Sn(s) + O₂(g) = SnO₂
*Pure ionic oxide
* SnO₂ does not dissolve in HCL,HNO₃ and aqua regia (mixtures of concentrated HNO₃ and concentrated HCL)
*Amphoteric oxide
-with H₂SO4 (Acid)
SnO2(S) + H2SO4 -> SN(SO4)2(s) + 2H20
-With OH- (Alkali)
SN02(s) + 2OH- -> SNO3^2-(aq) + H20
SnO(Tin(II) Oxide)
*Referred to as a black tin
*We can get SnO by heating the tin oxalate
*Sno is aamphoteric oxide too but more basic than SnO2 and more lewis basic because it has more electrons than tin (IV).
-In acid
SnO(s) + 2H+(aq) -> Sn^2+(aq) + H20
-In alkali
SnO(s) + 2OH-(aq) -> SnO2^2-(aq) + H20

2) Halides (SnCl4,SnCl2)
SnCl4
*Prepared by direct heating of the elements
-Sn(s)+CL2(g) -> SnCl4(l)
*Colourless liquid
*Covalent Compund with tetrahedral structure.
* SnCl4 will rapidly hydrolyzed and funing in moist air.
-SnCl4(l) + 2H2O(l) -> SnO2(s) + 4HCL (g)
SnCl2
*Predominantly covalent compound
*Soluble in water and organic solvents
*Preparation of anhydrous SnCl2
-Sn(s)hot + 2HCl(g) -> SnCl2 + H2
*Dissolved in water to give cloudy solution due to formation by hydrolysis of basic chlorides.
*Heating SnCl2.2H2O also form basic chlorides.
*Strong reducing agent ( will go oxidation).

SnCl2 is more stable than SnCl4

3)Sulfide
SnS(exist as mono)
*Obatained by passing through the H2S gas in Sn(ll)solution.
-Sn^2+(aq) + H2S -> SnS + H+(aq)
*Dark brown unstable solid
*Easy oxidize to SnS2

SnS2(exist as disulphide)
*Obatained by oxidation of SnS by using ammonium polysulfides.
-SnS (s) + S(s) -> SnS2(s)
* Yellow solid
* Dissolves in excess of (NH4)2Sx

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Summary on Group IV (Lead,Pb) - NUR SUHAILA BINTI SHUKOR 

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Summary on Group IV (Lead,Pb) - NUR SUHAILA BINTI SHUKOR 

# data[].attributes.body
Lead has electronic conf : [Xe]6s24f145d106p2

Lead can be extract by :
- roasting it with O2
2Pbs + 2O2 ->2PbO + 2SO2
- lead oxide with carbon
PbO + C ->Pb(l) + CO (g)

Properties of lead :
-high density, soft with low bp
- high luster
- resist corrosion

Reaction of lead :
1. Pb with air/moisture will form oxy carbonate Pb ( PbCO3)
2. Pb + HNO3 -> Pb(NO3)2
3. Pb + O2 with heating -> PbO , further react with O2 form Pb3O4
4. Pb + H2SO4 -> PbSO4

COMPOUND OF LEAD
1. Oxide - PbO, PbO2 & Pb3O4

- PbO (+2)
preparation:

direct reaction between elements:
Pb +O2 -> PbO

thermal decomposition of Pb(NO3)2 or PbCO3 :
2Pb(NO3)2 -> 2PbO + 4NO2 +O2
PbCO3 -> PbO +CO2

PbO is yellow solid and an amphoteric acid

- PbO2 ( +4)
preparation :

heating Pb(ll) solution with NaCl :
Pb2+ (aq) + H2O +ClO-(aq) -> PbO2(s) + Cl-(aq) + 2H+(aq)

red lead with nitric acids :
Pb3O4 (s) + 4HNO3 (aq) -> PbO2 (s) + 2Pb(NO3)2 (aq) + 2H2O (l)

PbO2 is dark brown solid / black powder, ionic compound, strong oxidizing agent, dissolves in acids and an amphoteric oxide. Mainly use as cathode in lead acid battery.

- Pb3O4 ( trilead tetraoxide)
preparation:
a mixture of 2PbO and PbO2
3Pb (s) + O2 -> Pb3O4
PbO2 (s) -> Pb3O4 + O2

red lead and show properties like PbO and PbO2. Use in paint with red pigment to protect iron and steel from rusting.

2. Halides - PbX4 & PbX2

- Pb(ll) halide more stable than Pb(iv) halide

PbX4 :
exists in Group 17 as PbF4 and PbCl4 ; PbBr4 and PbI4 does not exist due to not strong oxidizing agent.

PbX2 :
All halides exist in ionic form
PbF2, PbCl2, PbBr2, ( white solid )
PbI2 ( yellow solid )

3. Sulphide - PbS

Formed black precipitate when H2S is passed through lead(II) solution.

Pb2+ (aq) + H2S(g) ->PbS (s) + 2H+ (aq)

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Summary On Group IVA (Pb)- Mohamad Faris Aiman Mohd Azahri

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Summary On Group IVA (Pb)- Mohamad Faris Aiman Mohd Azahri

# data[].attributes.body
Pb Electron configuration:
[Xe]6s²4f¹⁴5d¹⁰6p²

- Exist as mineral-galena(PbS)
To get Pb, PbS have to extract by roasting it with Oxygen.

2PbS + 2O₂ -> 2PbO + 2SO₂
PbO + C -> Pb(l) + CO₂(g)

Physicochemical Properties:
- High density
- Soft metal
- Low boiling point
- Resists corrosion

Compound of Pb

1. Oxide (PbO, PbO ₂, Pb ₃ O ₄)

i) PbO (Lead Oxide)(+2)
Preparation:

- Direct reaction between elements
Pb + O₂ -> PbO

- Thermal decomposition of Pb(NO₃)₂ or PbCO₃

2Pb(NO₃)₂ -> 2PbO + 4N0₂ + O₂
PbCO₃ -> PbO + CO₂

- Yellow solid
- Amphoteric Oxide

ii) PbO2 (Plumbum Dioxide) (+4)
Preparation:

- Heating Pb(ll) solution with NaCl.
Pb²⁺ + H₂O + CLO⁻ -> PbO2 + Cl⁻ + 2H+

- Red lead with nitric acids
Pb₃O₄ + 4HNO₃ ->PbO₂ + 2Pb(NO₃)₂ + 2H₂O

Properties:
- Dark brownish solid/ black powder.
- Ionic compound
- Strong oxidizing agent(reduction occur): +4 -> +2
- Decompose when heating
PbO₂ -> Pb₃O₄ + O2

- Dissolve in acid:
PbO + 2HCl -> H₂PbCl₆ + 2H₂O

- Amphoteric Oxide
- Commonly use as cathode in Lead Acid Battery.

iii) Pb ₃ O ₄ (Trilead tetraoxide)

- Red lead
- Mixture of 2PbO.PbO2

Preparation:

3Pb + O₂ -> Pb₃O₄
PbO₂ -> Pb₃O₄ + O₂

- Properties similar as PbO and PbO₂

2. Halide (PbX4 & PbX2)

Pb(ll)halide more stable than Pb(iv)halide.

Lead(iv) halide, PbX4:
Only PbF4 and PbCl4 exists.
Br and I is not strong oxidizing agent, hence cannot produce Lead halide.

Lead(ll) halide, PbX2
- All halide exists as ionic form
- PbF₂ - White solid
- PbCl₂ - White solid
- PbBr₂ - White solid
- Pbl₂ - Yellow solid

3) Sulphide

-Only form PbS.
- H₂S pass through Lead(ll) solution to form black precipitate(PbS).

Pb²⁺ + H₂S -> PbS + 2H⁺

# data[].attributes.headline
Summary Group IV Element (Sn)- Miza Faiqah binti Suhaimi (A21HP0059)

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Summary Group IV Element (Sn)- Miza Faiqah binti Suhaimi (A21HP0059)

# data[].attributes.body
Electron Configuration: [Kr]4d105s2

Extraction

· Cassiterite (SnO2) – (Tin Ore-impurities: S, As) to SnO2 (pure Tin Ore) by roasting then from SnO2 (pure Tin Ore) to Sn (pure) by reduction with anthracite

· Sn also undergoes electrolysis to get pure Sn at cathode

Tin Allotrope

· Alpha tin (grey tin)

Structure: diamond lattice

Density: 5.75 g/cm3

Physical appearance: powder

· Beta tin (white tin)

Structure: tetragonal/ distorted octahedral lattice

Density: 7.31 g/cm3

Physical appearance: metallic solid

· Gamma tin

· Tin-plague/ tin pest

- Change from white tin to grey tin due to increase in volume and the tin metallic appearance becomes pock-marked and eventually powdered.

Physicochemical properties

1.    Soft metal

2.    Malleable but not very ductile

3.    Brittle on heating

4.    Crackles when bent

Compound of Sn

Oxide (SnO2, Sno)

· SnO2 oxidation number is Sn +4

- Direct heating of the metal in air or oxygen

Sn(s) + O2(g) -> SnO2(s)

-  Pure ionic oxide

- Does not dissolve in HCl, HNO3 or  even aqua regja

- Amphoteric oxide

o   With H2SO4 (acid)

SnO2(s) + H2SO4 -> Sn(SO4)2(s) + 2H2O

o   With OH- (alkali)

SnO2(s) + 2OH- -> SnO3 2-(aq) +H2O

·  SnO oxidation number is Sn +2

- as black tin

·  Preparation

Heating tin oxalate

·  Amphoteric oxide

§ More lewis basic than SnO2 due to has more electron

In acid

SnO(s) + 2H+(aq) -> Sn2+(aq) +H2O

In alkali

SnO(s) + 2OH-(aq) -> SnO2 2-(aq) + H2O

Halides

· SnX2 more stable than SnX4

SnCl4

· Preparation

Direct heating elements

Sn(s) +Cl2(g) -> SnCl4(l)

· Colorless liquid

· Covalent compound with tetrahedral structure

· Rapidly hydrolyzed and fuming as a result in moist air.

SnCl4(l) +2H2O(l) -> SnO2(s) + 4HCl(g)

· With conc. HCl/NH4Cl form complex SnCl6 2-

SnCl4(l) +2HCl(aq) -> H2SnCl6 (aq)

SnCl4

· Predominantly covalent compound

· Soluble in water and organic solvents

· Preparation

Sn(s)hot + 2HCl(g) -> SnCl2 + H2

Anhydrous salt is a transparent crystalline solid

Hydrated SnCl2.2H2O

Sn(s) + HCl conc. -> SnCl2 + H2

SnO(s) + HCl(aq) dil -> SnCl2 +H2O

· Dissolved in water to give cloudy solution due to formation by hydrolysis of basic chlorides

2SnCl2(s) + 2H2O(l) -> Sn(OH)2.SnCl2(s) + HCl(aq)

· Heating SnCl2.2H2O also form basic chlorides

SnCl2.2H2O -> Sn(OH)2.SnCl2(s) +HCl(aq) + 2H2O

· Strong reducing agent

Reduce Mercury(l) chloride -> Mercury
Sn2+(aq) + Hg2Cl2 -> Hg(l) + Sn4+(aq) +2Cl-(aq)

Iron(lll) -> iron(ll)

Sn2+(aq) + 2Fe3+(aq) -> 2Fe2+ + Sn4+(aq)

Nitrobenzene -> phenylamine(analine)

Sulfide

· Exist as (SnS) and disulphide (SnS2)

SnS

· Obtained by passing through the H2S gas in Sn(lll) solution

Sn2+(aq) + H2S(g) -> SnS(s) + H+(aq)

· Dark brown unstable solid

· Easily oxidize to SnS2

SnS2

· Obtained by oxidation of SnS using ammonium polysulfides (NH4)2Sx (mixture of (NH4)2S and S)

SnS(s) + S(s) -> SnS2(s)

· Yellow solid

· Dissolves n excess of (NH4)2SnS3

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Summary Group IVA Element Tin,Sn - Muhammad Afkar

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Summary Group IVA Element Tin,Sn - Muhammad Afkar

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Sn= stannum
Electronic Configuration: [Kr]4d105s2
Extraction:
1) roasting the cassitserite (SnO2) to get pure tin ore
2) Pure tin ore undergoes reduction with anthracite to get Sn
3) Sn can undergo electrolysis to get pure Sn at cathode

3 tin allotropes
- alpha tin (white tin)
structure: diamond lattice
physical appearance: powder
- beta tin (grey tin)
structure:  tetragonal / distorted octahedral lattice
physical appearance: metallic solid
- gamma tin

Tin plague/tin pest
- the change of white tin to grey tin as the increasing of volume and the tin metallic become pork-marked.
Physicochemical:
soft metal, malleable but not very ductile, brittle when heating and crackles when bend.

Compound of Sn
1) Oxides (SnO2,SnO)
SnO2 is Sn +4
SnO is Sn +2
i)SnO2
Preparation:
Direct heating of tin in air or oxygen
Sn + O2 -> SnO2
Properties:
- pure ionic oxide
- not dissolve in HCl,HNO3 and aqua regia
- amphoteric oxide
with acid
SnO2 (s) + H2SO4 → Sn(SO4 )2 (s) + 2H2O
with alkali
SnO2 (s) + 2OH− → SnO3 2− (aq) + H2O

ii) SnO (black tin)
Preparation:
Heating tin oxalate
Properties:
amphoteric oxide (more basic than SnO2 because more lewis base, have more electron than tin(iv))
In acid
SnO(s) + 2H+ (aq) → Sn2+(aq) + H2O
In base
SnO(s) + 2OH− (aq) → SnO2 2− (aq) + H2O

2) Halides (SnX2,SnX4)
SnX2 is Sn +2
SnX4 is Sn +4
SnX2 is more stable than SnX4
i)SnCl4
Preparation:
Direct heating of Sn with Cl2 gas
Sn(s) + (g) → SnCl4 (l)
Properties:
Colourless liquid
covalent compound with tetrahedral structure
Rapidly hydrolyzed and fuming in moist air
SnCl4 (l) + 2H2O(l) → SnO2 (s) + 4HCl(g)
With concentrated HCl/NH4Cl, form complex SnCl6 2-

ii) SnCl2
Predominantly covalent compound
Soluble in water and organic solvents
Preparation:
anhydrous SnCl2:
Sn(s) hot + 2HCl(g) → SnCl2 + H2
hydrated SnCl2:
Sn(s) + HCl conc. → SnCl2 + H2
SnO(s) + HCl(aq) dil → SnCl2 + H2O
Properties:
dissolved in water to give cloudy solution
heating  SnCl2 .2H2O -> basic chloride
strong reducing agents
-reduce Mercury(I) chloride -> Mercury
-reduce Iron(III) -> Iron(II)
-reduce nitrobenzene → phenylamine

3) Sulfide
SnS - mono
SnS2 - disulphide

i) SnS
Preparation:
passing through the H2S gas in Sn(II) solution
Sn2+(aq) + H2S(g) → SnS(s) + H+ (aq)
Properties:
dark brown colour
unstable solid
easily oxidizes to SnS2

ii) SnS2
Preparation:
oxidation of SnS using ammonium polysulfides (NH4 )2Sx (mixture of (NH4 )2S and S)
SnS(s) + S(s) → SnS2 (s)
Properties:
yellow solid
dissolve in excess of (NH4)2S

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MUHD SABRI

Lead (Pb)
1. electronic configuration-[Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²
2. existence in mineral-galena, Pbs
3.can be extract by :
* 2PbS + 2O2 → 2PbO + 2SO2
* PbO + → Pb(l) + CO(g)

Physicochemical properties:
-high density, soft, low bp
-high luster, ductile, highly malleable
-resists corrosion

General reaction
*Pb + O2 → PbO further reaction with 02 prodece Pb3O4
* Pb + H2SO4 → PbSO2 (insoluble)
*Pb + HNO3 → Pb(NO3)2
* Pb + air/moisture → Oxy carbonate Pb

Oxide of Pb (PbO, PbO2, Pb3O4)
i)Lead Oxide (PbO) (+2)
-can be prepared by direct reaction between elements and thermal decomposition of Pb(NO3)2 or PbCO3
-yellow solid in color and has characteristic as amphoteric oxide
ii)Lead dioxide (PbO2)
-can be prepared by heating Pb(ii) with sodium chlorate and reaction between red lead with nitric acid
-dark brownish solid or black powder
-ionic compound
-strong oxidizing agent
-decompose when heating
-dissolves in acid such as sulfuric acid, HF and and HCL
-also amphoteric oxide
-uses mainly as cathode in lead acid battery

iii)Trilead tetraoxide (Pb3O4)
-also know as red lead
-contain mixture of Pb0 and PbO2
-can be prepared by reaction Pb and O2 or heating od PbO2
-shows properties like PbO and Pb02
-uses in paint made with red lead

Halide of Lead (PbX4 & PbX2)
-Pb(ii) halide more stable than Pb(iv) halide

i)Lead(iv) halide (PbX4)
-exists in PbF4 and PbCl4 only
-PbBr4 and PbI4 do not exist due to Br and I are not strong oxidizing agent and unable to oxidize Pb(ii) to Pb(iv)

ii)Lead(ii) halide (PbX2)
-all halide exist in ionic form

Lead Sulphide (PbS)
-only form PbS
-as black precipitate forms when H2S is passed through lead(ii) solution
-Pb²⁺ (aq)+ H₂S(g) → PbS(s) + 2H⁺

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Summary Group IV Element (Lead Pb)-Balqis Binti Mohd Azman

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Summary Group IV Element (Lead Pb)-Balqis Binti Mohd Azman

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Lead (Pb)

-exist in mineral-galena,Pbs.
-The electronic configuration of Lead,Pb is [Xe]6s ² 4f ¹⁴ 5d ¹⁰ 6p ²

Extraction of Pb:

2Pbs + 2O₂ roast----> 2PbO + 2SO₂

PbO + C -----> Pb(l) + CO (g)

Physicochemical properties of Pb:

High density

soft with low boiling point

high luster,ductile,highly malleable

resists corrosion

General reaction of Pb

Pb (air& moisture)-->oxy carbonate Pb

Pb (O₂&heat)---> PbO ---> Pb₃O₄

Pb (H₂SO₄) ---> PbSO₄

Pb (HNO₃) ---> Pb(NO₃)₂

compound of Pb (oxide)
exist as:
1.PbO (lead oxide)

preparation:

direct reaction between elements

- Pb + O₂ ---> PbO

thermal decomposition of Pb(NO₃)2 or PbCO₃

- 2Pb(NO₃)₂ -->2PbO + 4NO₂ + O2
- PbCO₃ --> PbO + CO2

Properties of PbO:

yellow solid

2.PbO ₂ (lead dioxide)
preparation:

heating Pb(II) solution with sodium chlorate

Pb²⁺(aq) + H₂O + ClO-  (aq) --->PbO₂ + Cl⁻ (aq) + 2H⁺ (aq)

red lead with nitric acids

Pb₃O₄ (s) + 4HNO₃(aq)---> PbO₂ + 2Pb(NO₃)₂ (aq) + 2H₂O(l)

properties of PbO₂:

dark brownish solid / black powder

ionic compound

strong oxidizing agent

decompose when heating

dissolves in acid

3.Pb ₃ O 4 ( Trilead tetraoxide)
Preparation:

3Pb(s) + O₂ ---> Pb₃O₂

PbO₂ (s) heat---->Pb₃O₄ + O₂

Properties of Pb₃O4:

read lead

mixture of 2PbO.PbO₂

Halide of lead

Lead Halides (PbX₄ & PbX₂)
-Pb(ll) halide is more stable than Pb(lV) halide.

1.Lead(lV), PbX₄

PbF₄ & PbCl₄ exists

PbBr₄ & Pbl₄ do not exists-because Br₂ and l₂ are not strong oxidizing agents thus unable to oxidize Pb(ll) -->Pb(lV)

2.Lead(ll) halide,PbX2
All halide exixts in ionic form:

PbF₂=white solid

PbCl₂=white solid

PbBr₂= white solid

Pbl₂=yellow solid

Lead Sulphide (PbS)

only form PbS

As black precipitate forms when H2S is passes through lead(ll) solution

eq:Pb²⁺ +H₂S(g)--->PbS(s) + 2H⁺ (aq)

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Aisyah Binti Nazeri(A21HP0012)

1. Electronic configuration: [Xe] 6s24f145d10

2. Exist in Minarel-Galane (Pbs)

3. Physicochemical properties:
- high density
- high luster,ductile
- resist corrosion

4. Compound of Pb
OXIDE (PbO,PbO2&Pb3O4)
i) lead oxide(PbO)
preparation PbO(Yellow solid)
1. Direct reaction between element
Pb + O2 --> PbO
2. Thermal decomposition of Pb(NO3)2 or PbCO3
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
PbCO3 --> PbO + CO2
3. PbO (Amphoteric oxide)
PbO + 2HCl --> PbCl2 + H2O
PbO + 2OH- + H2O --> Pb(OH4)2-
ii) lead dioxide(PbO2)
Preparation PbO2(dark Brownish solid/black powder)
1. Heating Pb(II) solution with sodium chlorate
Pb2 + H2O + ClO- --> PbO2 + Cl- + 2H+
2. Red lead with nitric acids
Pb3O4 + 4HNO3 --> PbO2 + 2Pb(NO3)2 + 2H2O
Properties:
- ionic compound
- strong oxidizing agent
- decompose when heating
PbO2 --> Pb3O4 + O2
- Dissolves in acids
PbO2 + 2H2SO4 --> PbSO4 + 2H2O
PbO2 + 2HF --> H2PbF6 + 2H2O
PbO2 + 2HCl --> H2PbCl5 + 2H2O
- amphoteric oxide
PbO2 + 4HCl --> PbO3 2- + H2O
PbO2 + 2OH- --> PbO3 2- + H2O
iii) trilead tetraoxide(Pb3O4)
- red lead
- mixture of 2PbO&PbO2
- properties same as PbO&PbO2
Preparation
3Pb + O2 --> Pb3O4
PbO2 --> Pb3O4 + O2 (heated)

HALIDE(PbX4&PbX2)
- PbX2 more stable than PbX4

1. Lead(IV) Halide
- PbF4&PbF4, & PbCl4 exists
- PbBr4 & PbI4 do not exists
(Br2 and I2 not strong oxidizing agent)
2. Lead(II) Halide
- all halide exist in ionic compound
PbF2,PbCl2,PbBr2- white solid
PbI2-yellow solid

SULPHIDE (PbS)
-Only form PbS, (+2 exist but +4 did not)
- As black precipitate forms when H2S is passes through lead(II) solution
- Pb2+ + H2S --> PbS + 2H+

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Summary of element Group IVA (Carbon) – Alya

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Summary of element Group IVA (Carbon) – Alya

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CHE NURUL ALYA FATNIN BINTI CHE SUHAIMI

Carbon has oxidation number +4 and the electronic configuration is 2s²2p².

Carbon existence in air (0.03% CO₂), igneous rock, anthracite (100% C), bituminous coal (85% C) and lignite (60%).

8 allotropes of carbon :

Diamond

Graphite

lonsdaleite

C₆₀ (buckminsterfullerene or buckyball)

C₅₄₀

C₇₀

Amorphous carbon

Single-walled carbon nanotube or buckytube

Allotropes of carbon (detail):

1. Diamond
- produce from crystallization of molten magna in the earth crust.
- can be synthesized from graphite.
- structure made of carbon atoms  bonded together by covalent bonds.
- has a very high melting point (~4000 c).
- each C atom is bonded to 4 other C atoms having sp³ hybridization.
- cannot conduct electricity because there is no free electrons.
- application: jewelry and making cutting tool.

2. Graphite
- prepared by Acheson Process (in high temperature electrical furnace).
SiO₂ + C -> SiC + CO
SiC -> Si + C
- structure made up of stacked of two-dimensional carbon sheets.
- each C atom is bonded covalently to 3 other C atoms (sp² hybridization).
- can conduct electricity, act as oxidizing agent, used in pencils, lubricant.

3. Fullerene
- consist of big C framework consisting of even numbers of C atoms.
-structure the most symmetry fullerene, also called “bucky ball” or “buckmisterfullerene”.
- having sp2 hybridization.
- can conduct electricity and used as superconductor wire.

Carbon compound:

1. Oxides ( exist as CO and CO ₂)

a. Carbon Monoxide, CO
- colourless gas, does not smell.
- burned with blue flame.
- bind strongly with hemoglobin causes the cell received less oxygen for respiration leads to death.
- strong reducing agent.

Fe₂O₃ + 3CO -> Fe + 3CO2
NiO + CO -> Ni + CO2
- act as ligand in the formation of carbonyl complexes by donating electron pair to transition metal.
- application: production of pure Ni, gas in synthesis gas, reagent to produce phosgene.

b. CO ₂
- colourless gas and does not smell.
- solid CO₂ is called dry ice.
- prepared by heating limestone or the reaction of acid with CaCO₃.
- dissolve in water to form carbonic acid, CO₂ is an anhydride.
- react with base to form carbonate.
- act as ligant: molecule donating electron.
- application: dry ice, fire retardant, producing or carbonated drink and baking soda.

2. Carbonate
- Only Group IA and Group IIA (barely) carbonates can dissolve in water.
- Geometry trigonal planar.
- Has hybridization sp2
- It exist as resonance structure.

3. Halides (CX ₄)
- As C has no d-orbital, it cannot receive electron pair from water molecule and CX₄ does not undergo hydrolysis.
- CCl₄ can be used as organic solvent.
- CCl4 can be prepared by reacting CS₂ with Cl₂.
- CF₄ is inert, non-toxic and non-corrosive. It cannot dissolve in water, alcohols and HF, but can dissolve on chlorocarbons.
- Bond energy of CF₄ very high, thus have high stability.
- Application: CF₄ can be used s refrigerating gas (freon), non-stick cooking utensil (polytetrafluoroethene), and monomer for making plastic (perfluorovinylchloride).

4. Carbides
- Compound of C+ metal.
- Ionic carbide formed from C+ Group IA,IIa,IIA metal.
- They are easily hydrolyze.
- Covalent carbide formed from C+ Si/Ba. They are giant molecule which held by covalent bonding.
- They are very inert and hard substances that can be used to make cutting tool.
- Interstitial carbide formed from C+ transition metals.
- Carbon atoms are adsorbed into metallic lattices interstices and ocupy at the holes of interstices.
- Extremely hard solid but brittle.

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CARBON

Carbon exist as CO₂, igneous rock, anthracite, bituminous coal and lignite.

Allotropes of carbon include:

a. Diamond

- can be synthesize from graphite

- carbon atoms bonded together by covalent bonds.

- high melting point.

- having sp3 hybridization, which each C atom bonded to 4 other C atoms.

- cannot conduct electricity because there is no free electrons.

- application: jewelry, making cutting tool.

b. Graphite

- prepared by Acheson Process

SiO₂ + C → SiC + CO

SiC → Si + C

- made up of stacked of 2D carbon sheets.

- having sp2 hybridization, which each C atom bonded to 3 other C atoms.

- carbon atoms bonded by covalent bond.

- can conduct electricity, act as oxidizing agent, used in pencils, lubricant.

c. Fullerene

- known as ‘bucky ball’.

- having sp² hybridization.

- can conduct electricity, so used as superconductor wire.

Carbon compounds consist of:

a. Oxides (CO ₂, CO)

i. CO

- colourless gas with no smell.

- burned with blue flame.

- bind strongly with hemoglobin causes the cell received less oxygen for respiration leads to death.

- prepared from dehydration of formic acid by concentrated H₂SO₄ and reduction of CO2.

- strong reducing agent (itself will be oxidized)

- act as ligand (carbonyl complexes) in the formation of carbonyl complexes by donating electron pair to transition metal.

- application: production of pure Ni, gas in synthesis gas, hydroformylation, reagent to produce phosgene.

ii. CO ₂

- colourless gas with no smell.

- prepared by heating limestone or the reaction of acid with CaCO₃

- dissolve in water to form carbonic acid.

- react with base to form carbonate.

- act as ligant.

- application: dry ice, fire retardant, reactant for the producing of Na₂CO₃, producing or carbonated drink and baking soda, carbon cycle.

b. Carbonate

- only Group IA and Group IIA (barely) carbonates can dissolve in water.

- geometry: trigonal planar.

- hybridization: sp².

- exist as resonance.

c. Halides (CX ₄)

- As C has no d-orbital, it cannot receive electron pair from water molecule, and thus, CX₄ does not undergo hydrolysis.

- CCl₄ can be used as organic solvent and it can be prepared by reacting CS₂ with Cl₂.

- CF₄ is inert, non-toxic and non-corrosive. It cannot dissolve in water, alcohols and HF, but can dissolve in chlorocarbons. Bond energy of CF4 is very high and resulting it to have high stability.

- application: CF₄ can be used as refrigerating gas (freon), monomer for making plastic (perfluorovinylchlride), and non stick cooking utensil (polytetrafluoroethene).

d. Carbides

- compounds of C + metal.

- Ionic carbide formed from C + Group IA/ IIA/ IIIA metal. They are easily hydrolyze.

- Covalent carbide formed from C + Si/Ba. They are giant molecule, which held by covalent bonding. They are very inert and hard substances that can be used to make cutting tool, discs, and drillers.

- Interstitial carbide formed from C + transition metals. Carbon atoms are adsorbed into metallic lattices interstices. They are inert, hard but brittle solid, and have high melting points.

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Summary an element of Group IVA ( Silicon) - Maizurah Nazri- 

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Summary an element of Group IVA ( Silicon) - Maizurah Nazri- 

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After oxygen, silicon is the second abundant element in the earth. There are two for the existence of silicon, like as silicon dioxide also known as silica, SiO2 and as silicate substances. Next, to extract element silicon, there are two ways.
1) Reducing SiO2 by coke
- electrical furnace
coke is actually fuel used mainly in blast furnace. It contains carbon.
Eg: SiO2 + C --> Si + 2CO
Then by using excess silica, it will prevent the formation of SiC known as silicon carbide
Eg: SiO2 + 2C --> SiC + 2CO
2SiC + SiO2 --> 3Si + 2CO
2) for obtain pure Si, it have 2 steps:
i) Reducing SiCl4 by Na
SiCl4 + 4Na --> Si + 4NaCl
ii) Zone refining process to remove the impurities Si that has been formed in (i).

Characteristics of Silicon,Si
- crystalline Si has metallic luster and grayish colour.
- diamond lattice
- High melting point
-Inert element but attack by hydrogen
- HF the only one acid that Si can be dissolve, Eg: Si + 6HF --> H2SiF6 + 2H2
-But in base, Si can be dissolve
Si + 2OH- + H2O --> SiO32- + H2

Silicon Compounds
1) Oxides
Silica or silicon dioxide. It exists as polymeric tetrahedral.
In oxides, it have only 50% ionic due to difference in electronegativity for Si-O. But as for whole molecule, it is covalent macromolecule.

Preparation of SiO2
1) Hydrolysis of SiCl4
SiCl4 + 4H2O --> 4HCl + H4SiO4
H4SiO4 will be decompose at 1270 K temperature to yield SiO2.
2) Acidification of water glass, Na2SiO3.
Na2SiO3 + 2HCl --> 2NaCl + H2SiO3
H2SiO3 will be heating at 1270 K temperature to yield SiO2.

Properties of SiO2.
-Inert at low temperature but become reactive at elevated temperature.
- Strong acidic oxide at elevated temp.
-Dissolve in HF only
SiO2 + 6HF --> H2SiF6 + 2H2O
-Dissolve in alkali
SiO2 + 2NaOH --> Na2SiO3 + H2O

2) Silicate, (SiO4)4-
Example of silicate is water glass or known as sodium silicate, Na2SiO3 . To prepare sodium silicate, Silica react with sodium carbonate, Eg: SiO2 + Na2CO3 --> Na2SiO3 + CO2 . Structure of silicate  is polymorph which contains of tetrahedral SiO4 join through Si-O-Si bonds.

3) Aluminosilicate
- Al atom substitutes Si in the silicate framework, [(SiO4)n(AlO4)m] m-
- Cations from group 1A and IIA or transition metals will balance the excess charge.
-Eg: - Feldspar : - KAISi3O8, orthoclase
- NaAlSi3O8 , albite
- Zeolite: Hydrated aluminosilicate
Zeolite have regular size of pores and channels and molecular ranges size is (4-12 A). Next, cation balancing framework zeolite can be exchangeable; ion exchanger. It needed zeolite process where Ca2+ and Mg2+ akan dimendapkan dan dibuang. Then, once H+ has exchanged the cation, zeolite becomes strong acidic solid catalyst.

4) Silicate Glass
To produce for example like soda glass, it need mixture of CaSiO3 and Na2SiO3.
Type of glasses: soft glass, Hard glass, Flint glass, Jena glass, Pyrex or corning glass, Crooke's glass, Quartz glass, Ground glass, Reinforced glass

5) Silicones
Bonds in chain, rings, and branches of silicones  is like Si-O-Si-O with alkyl / aryl group bonded to Si atom. To prepare silicones, hydrolysis of alkyl / aryl silicon halides first is needed then followed by condensation.

Types of silicones consists of three:
1) Disilicone - Initial R3SiX
2) Chain Silicone- Initial R2SiX2
3) Branced Silicone- Initial RSiX3

Properties of silicone:
- thermally stable up to 500-600 K.
-low viscosity which changes with temperature.
- Silicone rubbers remain elastic
- Hydrophobic (ia takkan melekat-lekat kerana bersifat as water repellent)
- Inert towards chemical attack or oxidation.

Uses: As lubricants, in comestic, breast implant shell, and silicone wax.

5) Silicon Halides, SiX4
X can be halide such as F, Cl, Br, I .
Halides unstable (Cl, Br, I) will undergo hydrolysis in water,
Eg: SiX4 + 2H2O --> SiO2 +4HX
While halide stable (F) undergo partial hydrolysis,
Eg: 2SiF4 + 2H2O --> SiO2 + H2SiF6 + 2HF

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Tin Allotrope:
alpha-Sn, beta-Sn, gama-Sn, liquid-Sn
Physiochemical properties:
-soft metal
-malleable but not very ductile
-crackles when bent
-brittle when heating

Compound of Sn:
1)Oxides (SnO2, SnO)
i) Preparation of SnO2:
direct heating of Sn in oxygen/air:
Sn + O2 -->SnO2
Physical Properties:
- does not dissolve in HCl/aqua regia.
-pure ionic oxide
-Amphoteric oxide :
with acid (H2SO4):
SnO2+H2SO4-->Sn(SO4)2+2H2O
with alkali(OH):
SnO2+ 2OH -->SnO3 +H2O

ii) Preparation of SnO: Heating tin oxalate.
Physical Properties:
-Amphoteric oxide.
with acid (H+) :
SnO + 2H^+ --> Sn^2+ + H2O
with alkali (OH-):
SnO +2OH- --> SnO2 +H2O

2) Halides (SnX2, SnX4) X=Cl,Br,I
i) Preparation SnX4: Direct heating
Sn + X2(X=Cl,Br,I) --> SnX4
Physical Properties:
-Colorless liquid
-covalent compound with tetrahedral structure

ii) Preparation of SnCl2 (X=Cl,Br,I)
Sn (hot)+ 2HCl --> SnCl2 + H2
Physical properties:
-soluble in water and organic solvents
-strong reducing agent

3) Sulfide (SnS, SnS2)
i) SnS : Prepared through H2S gas in Sn(II) solution.
Sn^2+ + H2S --> SnS + H^+
Physical properties:
-Dark brown unstable solid
-Easily oxidized to SnS2.

ii) SnS2 : Prepared by oxidation of SnS using ammonium polysulfides
SnS + S --> SnS2
Physical properties :
-Yellow solid
-more stable than SnS.
-Dissolves in excess of (NH4)2Sx
SnS2 + (NH4)2S --> (NH4)2SnS3

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Darshiny Muralitharan
Electronic configuration: [Xe] 6s24f15d106p2

Extraction
2PbS + 2O2 ---> PbO + 2SO2
PbO + C ---> Pb(l) + CO(g)

Physicochemical properties:
- High density (heaviest common element) but soft with low boiling point
- High luster, ductile & highly malleable
- Resists corrosion

Compounds of Pb
1) Oxides
Exists as PbO, PbO2 & Pb3O4
PbO: Lead oxide ( yellow)
Preparation:
i) Direct reaction between elements
Pb + O2 ---> PbO
ii) Thermal decomposition of Pb(NO3)2 or PbCO3
2Pb(NO3)2 ---> 2PbO + 4NO2 + O2
PbCO3 ---> PbO + CO2
- PbO is an amphoteric oxide
PbO + 2HCl ---> PbCl2 + H2O
PbO + 2OH- + H2O ---> Pb(OH4)2-

PbO2 : Lead dioxide ( dark brownish solid or balck powder
Preparation:
i) Heating Pb(II) solution with sodium chlorate
Pb2 + H2O + ClO- ---> PbO2 + Cl- +     2H+
ii) Red lead with nitric acids
Pb3O4 + 4HNO3 ---> 2PbO2 + 2Pb(NO3)2 + 2H2O

Properties:-
- PbO2 is a ionic compound - Pb4+ & O2-
- Strong oxidising agent
- Decompose when heating
PbO2 ---> Pb3O4 + O2
- Dissolves in acids
PbO2 + 2H2SO4 ---> PbSO4 + 2H2O
PbO2 + 2HF ---> H2PbF6 + 2H2O
PbO2 + 2HCl ---> H2PbCl5 + 2H2O
- amphoteric oxide
PbO2 + 4HCl ---> PbO3 2- + H2O
PbO2 + 2OH- ---> PbO3 2- + H2O

Pb3O4 : Trilead tetraoxide
Preparation:
3Pb + O2 ---> Pb3O4
PbO2 ---> Pb3O4 + O2 ( must heat)

- Red lead
- A mixture of 2PbO.PbO2
- Shows properties like PbO and PbO2

2) Halide of Lead

Lead Halide (PbX4 & PbX2)
- Pb(II) halide is more soluble than Pb(IV) halide

Lead (IV) halide, PbX4
- PbF4, & PbCl4 exists
-PbBr4 & PbI4 do not exists because Br2 and I2 are not strong oxidising agent thus unable to oxidize Pb(II) --> Pb (IV)

Lead halide, PbX2
- All halides exists in ionic form
PbI2 - white solid
PbCl2 - white solid
PbBr2 - white solid
PbI2 - yellow solid

3) Lead Sulphide ( PbS)
- Only forms PbS
- As black precipitate forms when H2S is passes through lead(II) solution
- Pb2+ + H2S ---> PbS + 2H+