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NUR ATHIRAH ALIAH BINTI JAMIL(A21SC0222)

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NUR ATHIRAH ALIAH BINTI JAMIL(A21SC0222)

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COMPOUND OF GROUP IIA-HYDRIDE

PREPARATION:

Direct heating of elements in H2 (except Be) /

M(p) + H₂(g) --> MH2(p) ; (M=Mg...Ba)

For Be:

2BeCl₂ + LiAlH4 + Ether --> BeH₂ + LiCl + AlCl₃
- Be cannot direct heating

PROPERTIES:

All metal hydrides are ionic in nature and contain H⁻ ion (except BeH ₂)

BeH2 form polymeric solid (covalent bonding) in which Be atom linked by hydrogen bridges

REACTIONS:

1.  Reaction with H₂O

MH₂ + 2H₂O --> M(OH)₂ + 2H2 (M=Mg...Ba)

Eg: MgH₂ + 2H₂0 --> Mg(OH)₂ + H₂(g)

2.  Thermal stabilization

MH₂ --> M + H₂

Mg < Ca < Sr < Ba
increasing thermal stabilization

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NURSYAFIQA ARISYA BT JAMALUDIN (A21SC0294)

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NURSYAFIQA ARISYA BT JAMALUDIN (A21SC0294)

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Summary of group IIA (ALKALINE EARTH METAL)

Physical properties
-relatively soft but harder than alkali metals (getting harder down the group)
-it have grey white lustre when freshly cut but thin oxide coating quickly form when exposed to the air
-density, boiling point, melting points tend to be higher than alkali metals of the same period

Preparation
-reaction between metal salts with sulfuric acid
MX + H2SO4 -> MSO4 + HX

Uses of group IIA elements
-Be (x-ray windows)
-Mg (flares in pyrotechnics)
-Ca (reducing agent for Preparation of metals such as Thorium, uranium, zirconium)
-Sr (fireworks Red flames)
-Ba (used in painting)

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NUR IZZATI FARHANAH BINTI ABD KADIR (A21SC0243)

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NUR IZZATI FARHANAH BINTI ABD KADIR (A21SC0243)

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Compound of group IIA
( SULPHATE )

Preparation:
•reaction between metal salts with sulfuric acid ; MX + H2SO4==> MSO4 +HX

Properties:

1. exist in hydrated form, number of mole hydrated water depends on temperature
2. down the group- increases in thermal         stability
3. decreases in stability
4. decomposed to oxide due to decreases in polarizing ability

Application:
i) EPSOM SALT ( MgSO4)
- medicine
-anhydrous
-fertilizer
ii) Gypsum salt ( CaSO4)
-Portland cement
-Plaster of Paris
-fertilizer in agriculture
iii) BaSO4
In medical : opaque to X-rays "barium meal" is given to patient in order to obtain good quality photograph of digestive tract.

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NUR AFIQAH BINTI AHMAD RUSLI ( A21SC0210 )

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NUR AFIQAH BINTI AHMAD RUSLI ( A21SC0210 )

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GROUP IIA

CARBONATE ( MCO3 )

Preparation

Naturally exists in the earth crust and form minerals

MgCO3 : magnesite ; CaCO3 : limestone @ lime rock

In laboratory

Mg(NO3)2 + 2NaHCO3 à MgCO3 + 2NaNo3 + H2o + CO2

cannot use sodium bicarbonate because it is too basic

CaCl2 + Na2CO3 à CaCO3  + 2NaCl

PHYSICOCHEMICAL PROPERTIES ( MCO3 )

Solubility decreases as we go down the group

The thermal stability will increases as we go down the group

Due to the decreasing in polarizability of the ion

Reaction

Reaction with mineral acids

CO3^2- + 2H3o^+  à 3H2o + CO2

STABILITY OF THE OXYANION

Increases down the group

Because :

1.    The strength of ionic bond between cation and anion decreases and cause the increasing of the bond strength between the atoms in the oxyanion molecule ( oxyanion molecule : carbonate, nitrate, sulphate )

2.    Decomposition or dissociation occur if the strength between the anion and cation increases

POLARIZING THE CARBONATE ION

The charges for the carbonate ion delocalized

The density of the electron is greater at O ion as it has a high electronegativity compared to C ion

When the a positive ion placed side to side to carbonate molecule, the ions will get attracted to the positive ions and polarized

So, the smaller the cation, the higher the charge density and it will have a greater effect on the carbonate ion as carbonate ion polarized

But if the cation becomes bigger, they have a less effect on the carbonate ions that goes near to them. So, in order to make sure that they break them up, they have to be heated more to force the carbon dioxide to break off and leave the metal oxide

The carbonates does become more thermally stable going down the group

THERMAL DECOMPOSITION

As we go down the group, the harder the decomposition to occur

Because of the polarizability decreases

Maksudnya semakin susah untuk kita decompose that metal

The charge of the cation decreases as its polarizing power also becomes weaker down the group

So, the cation is less able to polarize the anion and less able to distort the covalent bond that found in the carbonate ion

Thus, the distortion weakens the covalent bond, making the decomposition easier

POLARIZING POWER

Polarizing ability decreases as we go down the group

But if we across the period 3, the polarizing power increases as the positive ion increases

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NORIZATUL FILZA BINTI MUHAMAD PUZI (A21SC0205)

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NORIZATUL FILZA BINTI MUHAMAD PUZI (A21SC0205)

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COMPOUNDS OF GROUP IIA (HYDRIDE, MH2)

Ø  Preparation

·         Direct heating of elements in hydrogen (except Be)

M(p) + H2(g) --> MH2(p) ; (M = Mg…Ba)

·         For Be

2BeCl2 + LiAlH4 --> (ether) BeH2 + LiCl + AlCl3

Ø  Properties

·         All metal hydrides (except BeH2) are ionic in nature and contain H- ion

·         BeH2 polymeric solid (covalent bonding) Be atom linked by hydrogen bridges

Ø  Reactions

·         Reaction with water

MH2 + 2H2O --> M(OH)2 + 2H2 (M= Mg…Ba)

e.g : MgH2 + 2H2O --> Mg(OH)2 + H2(g)

·         Thermal stabilization

MH2 --> M + H2

Mg > Ca > Sr > Ba

Increase thermal stabilization

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Compound of group IIA( SULPHATE )

Preparation:
•reaction between metal salts with sulphuric acid ; MX + H2SO4==> MSO4 +HX

Properties:
• exist in hydrated form,number of mole hydrated water depends on temperature
• down the group- increases in thermal         stability
-decrease in stability
•decomposed to oxide due to decreases in polaring ability

Application:
•epsom salt(MgSO4); medicine,fertilizer,coagulant for making toufu
•gypsum salt(CaSO4); portland cement,plaster of paris,mould,gypsum board,fertilizer in agriculture
•Barium Sulphate(BaSO4); opaque to x-ray,Barium meal is given to a patient in order to obtain a good quality photograph of digestive tract

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Summary:
compound - Sulfate

Preparation:
- reaction between metal salts with sulphuric acid
MX + H2SO4 --> MSO4 = HX

Properties:
- all sulphate salt exis in hydaretd form. The number of mole hydrated water depends on the temperature.
- Therma stability increase when down the group due decreasing in polarizing ability and decomposed to oxide when heated.
- Solubility decreases when down the group because the decrease in lattice energy is small, the size of the anion( size of cation does not contribute)

Application
- MgSO4 (EPSOM SALT)
(medicine , drying agent)

-Gypsum salt (CaSO4)
(plaster of paris , portland cement)

-BaSO4
(In medical - opaque to X-ray, Barium meal is given to a patient in order to obtain good quality photograph of the digestive tract)

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Summary Of Group IIA

Preparation

Reaction of metal salt with sulphuric acid

MX + H₂SO₄ → MSO₄ + HX

Properties

All sulphate salts exist in hydrated form and the number of mole of hydrated water depends on the temperature .

Thermal stability increases down the group Decomposed to oxide when heated. It is because polarizing ability decrease.

BeSO4 < MgSO4 < CaSO4 < SrSO4 < BaSO4

Solubility decreases down the group

BeSO4 > MgSO4 > CaSO4 > SrSO4 > BaSO4

Application

Epsom Salt (MgSO₄)
-medicine
-fertilizer
-coagulant
-anhydrous

Gypsum Salt (CaSO₄)
-portland cement
-plaster of paris
-mould, chalk
-gypsum board
-fertilizer in agriculture

BaSO₄
-in medical, opaque to x-rays. "Barium meals" is given to patient in order to obtain good quality photograph of the digestive track.

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MUHAMMAD AIMAN AQIL BIN MUHAMAD ERI (A21SC0147)

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MUHAMMAD AIMAN AQIL BIN MUHAMAD ERI (A21SC0147)

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Summary of group IIA (Alkaline Earth Metal)
Oxide (MO)

Preparation:

In industry (by heating carbonate salts of Group IIA)

MCO₃ → MO + CO₂ (M= Mg, Ca)

In Laboratory (by heating)

MCO₃ → MO + CO₂
M(OH)₂ → MO + H₂O
M(NO₃)₂ → MO + 4NO₂ + O₂ (M= Mg, Ca)

Physicochemical Properties:

Metal oxides are ionic (except BeO)

Greater △IE, make the metal-oxygen bond more ionic. Hence, more basic.

All metal oxides are base (except BaO-amphoteric)

Be, Mg, Ca, Sr form monoxide, MO

Ba form peroxide, BaO₂ (under pressure)

Basicity increases down the group

MgO < CaO < SrO < BaO

Solubility increases down the group

BeO < MgO < SrO < BaO

Melting point decreases down the group

MgO > CaO > SrO > BaO

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Summary of group IIA (Oxides)

Preparation
-decomposition when heating of metal carbonate
MCO3 + Heat --> MO + CO2 (M= Mg, Ca)
M(OH) + Heat --> MO + H2O (M= Mg, Ca)
M(NO3 )2+ Heat --> MO + 4NO2 + O2 (M= Mg, Ca)
Properties
1)increasing solubility going down the group
2)increasing melting point going down the group
3)increasing basicity going down the group

Uses in real life
1) water purification
2)firebrick
3)thermal insulator

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MUHAMMAD FIRDAUS BIN NOREHAN (A21SC0165)

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MUHAMMAD FIRDAUS BIN NOREHAN (A21SC0165)

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SUMMARY OF GROUP II A
(ALKALINE EARTH METAL)
-form alkaline solutions when they react with water
-found in earth's crust as carbonates , phosphates,silicates and sulphates

PHYSICAL PROPERTIES
-hardness decreasing down the group
-density is decrease from Be to Ca then increase from Ca to Ra
-melting point of this group is decreases but not for Mg because of the crystalline structure
-when go down the group,reactivity is increases because of electron goes further away from nucleus

CHEMICAL REACTION
React with oxygen
-form binary oxide
-burns very vigorously as move down the group
-does not form superoxide
-the alkaline earth metal is oxidised,while oxygen is reduced

React with water
-form alkaline solution(except for Be)
-react with increasing rapidity on descending the group
-produces gas that can ignited by a lighted splint

React with halogen
-form ionic halides

React with acid
-the reaction is more vigorous when go down the group
-hydrogen evolve and forming salt

React with nitrogen
-form nitride

React with hydrogen
-form hydride

USES OF ALKALINE EARTH METAL
BERYLLIUM
-x-ray window
MAGNESIUM
-most use  in flares and pyrotechnics. before it was used in flash photography
-cure constipation
-magnesium oxide is used in refractory,
make organomagnesium
-make firework
CALCIUM
-act as reducing agent for preparation of metal
-react with other metal alloy for other usage

PHYSICOCHEMICAL PROPERTIES
-existed in white solid
-all metal oxides are ionic except BeO
-solubility increases down the group as lattice energy decreases
-thermal stability increases down the group -basicity increases down the group
-

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PREPARATION:
-Reaction between metal salts with sulphuric acid.

MX + H2SO4 → MSO4 + HX

M = Be X=O

M = Mg X=CO3

M = Ca, Sr, Ba, X=Cl

PROPERTIES:

-All sulphate salts exist in hydrated form

-The number of moles of hydrated water depends on the temperature

Going down the group:

Thermal stability increases

Decomposed to oxide when heated

BeSO4 < MgSO4 < CaSO4 < SrSO4 < BaSO4

(size of the cation increased, charge density and polarizing power decreased, weaker the ability to distort the electron cloud of anion, so the bonds  within anion become stronger. Thus, the compound is more stable to heat.)

Solubility decreases

BeSO4 > MgSO4 > CaSO4 > SrSO4 > BaSO4

(decrease in lattice energy is small, size of the cation does not contribute because of the larger size of the anion compared to cation to affect the lattice energy and the decrease in hydration energy with the increase in cation size (less –ve). Hence, the total energy gives a small exothermic value (−ve small)

APPLICATION:

Epsom salt (MgSO4)

Medicine

fertilizer

coagulant for making tofu

anhydrous –drying agent

Gypsum Salt (CaSO4)

Portland Cement

Plaster of Paris

mould, chalk

gypsum board

fertilizer in agriculture

BaSO4

In medical : opaque to X-rays. “Barium meal ” is given to a patient  in order to obtain a good quality photograph of the digestive tract.

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HARRIS NAQIUDDIN BIN ZAKARIA (A21SC0088)

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HARRIS NAQIUDDIN BIN ZAKARIA (A21SC0088)

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SUMMARY FOR GROUP IIA (HYDRIDE)

-There is one way to prepare the hydride compound that is by direct heating of elements in hydrogen except for Beryllium:

- M(p) + H2(g) --> MH2(P)

-For Beryllium, the method to produce hydride compound is different which is:

-2BeCl2+ LiAlH4 --> (With Ether) BeH2 + LiCl   +   AlCl3

-The first properties of Hydrides are in nature; all metal hydrides are ionic and contain H- ion except for BeH2

-The Second properties of Hydrides are BeH2 : Polymeric solids ( covalent bonding ) in which Be atom linked by hydrogen bridges

The first reactions of Hydride is reaction with water:

-MH2 + 2H2O --> M(OH)2 + 2H2 (M=Mg....Ba)

-The second reactions of Hydride is Thermal Stabilization:

-MH2 --> M+ H2

-Mg<Ca<Sr<Ba

-Increasing Thermal Stabilization

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NURHASYIMAH BINTI MOHD HARIS (A21SC0278)

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NURHASYIMAH BINTI MOHD HARIS (A21SC0278)

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Summary for sulphate group IIA

PREPARATION
- reaction of the metal salts with sulfuric acid
MX + H2SO4 -> MSO4 + HX

PROPERTIES
- all sulphate salts exist in hydrated form and the number of mole of hydrated water depends on the temperature
- solubility decrease down the group
- thermal stability increases down the group due decreasing in polarizing ability and decomposed to oxide when heated

APPLICATION OF METAL SULPHATE
1. Epsom Salt (MgSO4)
- medicine, fertilizer, anhydrous
2. Gypsum Salt (CaSO4)
- Plaster of Paris, Portland cement, Fertilizer in agriculture
3. BaSO4
- In medical : opaque to Xrays "Barium meal" given to patient in order to obtain good quality photograph of digestive tract

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GROUP IIA- CARBONATE
(Mgco3 , CaCO3 , SrCO3 , BaCO3 )

-when heated,the group 2 metal carbonates decompose to form the metal oxide and  releasing CO2 gas.

-Splitting compounds using heat process is called as thermal decomposition.
MCO3(s)   ------> MO (s)+ C02(g)

-become more stable to thermal decomposition going down the group

-Preparation in lab(only for MgCO3)

MgCl₂(aq) + 2 NaHCO₃(aq) → MgCO₃(s) + 2 NaCl(aq) + H₂O(l) + CO₂(g)

-become less soluble down the group. Why? Because the decreasing hydration entalphies of cations / lattice energy is more than hydration energy.

Application industry

-building (CaCO3))

-fuel (CaCO3)

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Summary for group IIA
(Sulphate)

Preparation

- reaction of the metal salts with sulphuric acid

    MX + H2SO4  ➡️  MSO4 + HX

Properties

- all sulphate salts exist in hydrated form:
The number of mole of hydrated water       depends on the temperature

- thermal stability increase due to the decrease in polarizing ability down the group,decomposed to oxide when heated

- solubility decreases down the group
*Because the decrease in lattice energy is small, the size of the cation does not contribute because of the larger size of the anion
*And decreasing in hydration energy with the increase in cation size

Application

1. MgSO4 (epsom salt)

-medicine
-fertilizer

2. CaSO4 (gypsum salt)
-plaster of paris
-gypsum board
-fertilizer in agriculture

3. BaSO4
In medical: opaque to X-ray, Barium meal is given to a patient in order to obtain good quality photograph of the digestive tract

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Summary fro Group IIA (sulphate)

PREPARATION
- Reaction of the metal salts with sulphuric acid

MX + H2SO4 → MSO4 + HX

PROPERTIES
- All sulphate salts exist in hydrated form and the number of mole of hydrated water depends on the temperature .
- Thermal stability increases down the group due decreasing in to polarizing ability
- Solubility decreases down the group

APPLICATON OF METAL SULPHATE :
1. Epsom salt(MgSO4)
- medicine
- drying agent
2. Gypsum salt (CaSO4)
- plaster of paris
- portland cement
3. BaSO4
- widely use in medical . barium meal is given to patient to obtain good quality photograph of the digestive track

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FARHAH NAJIHAH BINTI MAT AZAHAR (A21SC0075)

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FARHAH NAJIHAH BINTI MAT AZAHAR (A21SC0075)

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Summary for group IIA (Hydride)

Preparation

Direct heating of elements in hydrogen except Be

M(s) + H₂(g) → MH₂ (s) ; (M=Mg......Ba)

For Be
ether
2BeCl₂+ LiAlH₄ -----→ BeH₂ + LiCl + AlCl₃

Properties

All metals hydrides are ionic in nature and contain H- ion (except BeH2)

This is due to the presence of polymeric solid (covalent bonding) in BeH2 in which Be atom linked by hydrogen bridges.

Reactions
1. Reaction with water

MH₂ + 2H₂0 → M(OH)₂ + 2H₂ (M=Mg....Ba)

e.g: MgH₂ + 2H₂O → Mg(OH)₂ + H₂ (g)

2. Thermal stabilization
MH₂ → M + H₂
Mg < Ca < Sr < Ba
Thermal stability increases when going down the group

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Nur Syafiqah binti Kamaruddin (A21SC0260)

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Nur Syafiqah binti Kamaruddin (A21SC0260)

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Summary for group IIA (oxides)

Preparation
•In industry : by heating carbonate salts of Group IIA metals :
MCO3 → MO + CO2
△

•In laboratory : For M = Mg and Ca
MCO3 → MO + CO2
△
M(OH)2 → MO + H2O
△
M(NO3)2 → MO + 4NO2 + O2
△

Physiochemical Properties
•All metal oxides are ionic except BeO

•Monoxide only formed from Be to Sr because divalent metal ions are sufficiently polarizing to make peroxide when heated with pure O2.
Ba formed peroxide, BaO2 under pressure only

•did not form superoxide because the group IIA cation is too small

•not easy for enough peroxide/superoxide to cluster around to form stable crystal lattice

•Solubility increases from Be → Ba
BeO< MgO< SrO< BaO
the decrease in lattice energy is larger than the decrease in hydration energy resulting -ve value for the to dissolution energy.

•Melting point of the MO decreases down the group due to increasing cation size from Mg → Ba which slightly reduces in lattice energy.

•All oxides are base except for BeO(amphoteric)
BeO< MgO< SrO< BaO

•The greater the differences in electronegativity, the more ionic the metal-oxygen bond becomes.

•More ionic characteristics, more basic.

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Summary for group IIA (Sulphate)

i) Preparation

Reaction metal salts with sulphuric acid

MX + H2SO4 → MSO4 + HX

ii) Properties

-All sulphate salts exist in hydrated form. The number of mole of hydrated water depends on temperature

-Thermal stability ↑ when down the group. Decomposed to oxide when heated. Due to ↓ in polarizing ability

-Solubility ↑ when down the group

iii) Application of Metal Sulphate

1. Epsom Salt (MgSO4)

Medicine

Fertilizer

Coagulant for tofu

Anhydrous

2. Gypsum salth ( CaSO4)

Plaster of Paris

Portland cement

Fertilizer in agriculture

3. BaSO4

In medical : opaque to X-rays. "Barium meal" given to patient to obtain good quality photograph of digestive tract

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SUMMARY FOR GROUP IIA (SULPHATES)

PREPARATION:
-Reaction between metal salts with sulphuric acid.

MX + H2SO4 → MSO4 + HX

M = Be X=O

M = Mg X=CO3

M = Ca, Sr, Ba, X=Cl

PROPERTIES:

-All sulphate salts exist in hydrated form

-The number of mole of hydrated water depends on the  temperature

-Going down the group:

Thermal stability ↑

Decomposed to oxide when heated

BeSO4 < MgSO4 < CaSO4 < SrSO4 < BaSO4

(size of the cation increased, charge density and polarizing power decreased, weaker the ability to distort the electron cloud of anion, so the bonds  within anion become stronger. Thus, the compound is more stable to heat.)

Solubility ↓

BeSO4 > MgSO4 > CaSO4 > SrSO4 > BaSO4

(the decrease in lattice energy is small, the size of the cation  does not contribute because of the larger size of the anion compared to cation  to affect the lattice energy and the decrease in hydration energy with the increase in cation size (less –ve). Hence, the total energy gives small exothermic value (−ve small)

APPLICATION:

-Epsom salt (MgSO4)

Medicine

fertilizer

coagulant for making tofu

anhydrous –drying agent

-Gypsum Salt (CaSO4)

Portland Cement

Plaster of Paris

mould, chalk

gypsum board

fertilizer in agriculture

-BaSO4

In medical : opaque to X-rays. “Barium meal ” is given to a patient  in order to obtain a good quality photograph of the digestive tract.

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SULPHATE

1. PREPARATION
- Reaction of the metal salts with sulphuric acid   MX + H2SO4 = MSO4 +HX

2.PROPERTIES
i) All sulphate salts exist in hydrated form. The number of mole of hydrated water depends on the temperature.
MgSO4- 7H2O : Epsom salt
CaSO4-2H2O : Gypsum salt

ii)Thermal stability increases down the group due to the decrease in polarizing ability (decomposed to oxide when heated)

iii) Solubility decreases down the group

3. APPLICATION OF METAL SULPHATE
i) EPSOM SALT ( MgSO4)
- medicine (saline laxitive)
-anhydrous ( drying agent )
ii) Gypsum salt ( CaSO4)
-Portland cement
-Plaster of Paris
-fertilizer in agriculture
iii) BaSO4
In medical : opaque to Xrays "barium meal" is given to patient in order to obtain good quality photograph of digestive tract.

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NURUL AMIRA NAJWA BINTI MOHAMAD AZMAN (A21SC0303)

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NURUL AMIRA NAJWA BINTI MOHAMAD AZMAN (A21SC0303)

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COMPOUNDS : SULPHATE

PREPARATION:
* reaction between metal salts with sulphuric acid
MX + H2SO4  -> MSO4 + HX

PROPERTIES
* Exist in hydrated form, the number of moles of hydrated water depends on the temperature.
*  increases in thermal stability as down the group and decomposed to oxide when heated.
* Decrease in stability as down the group.

APPLICATION OF METAL SULPHATE
* Epsom salt (MgSO4)
medicine
fertilizer
coagulant for making toufu
* Gypsum salt (CaSO4)
portland cement
plaster of Paris
mould
gypsum board
fertilizer in  agriculture

* Barium sulphate (BasO4)
In medical, opaque to x-ray. Barium meal is given to a patient in order to obtain good quality photograph of digestive tract.

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Compound of group IIA ( Sulphate )

Preparation :
- Reaction between metal salts with sulphuric acid ( MX + H2SO4 = MSO4 + HX )
M = Be , X = O
M = Mg , X = CO3
M = Ca, Sr, Br , X = Cl

Properties :
- exist in hydrated form , mole of hydrated water depends on temprature.
- Thermal stability increases down the group ( decomposed to oxide when heated ) due to the decreases in polarizing ability
- Solubility decreases down the group

Application :
- Epsom salt (MgSO4)
* medicine, fertilizer, coagulant for      making tofu, anhydrous
- Gypsum salt ( CaSO4)
* portland cement, plaster of paris, mould, chalk, gypsum board, fertilizer agriculture
- BaSO4
* opaque to x-ray. Barium meals is given to patient in order to obtain good quality photograph of the digestive tract.

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MOHAMAD SALMAN BIN MOHAMAD SABRI (A21SC0136)

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MOHAMAD SALMAN BIN MOHAMAD SABRI (A21SC0136)

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Group IIA Compound - Chloride (MCL2)

Preparation
• MO + C + Cl2 → MCl2 + CO (M = Be,Mg)                                   Anhydrous
• MO + 2HCl → +MCL2 + H2O (M = Mg,Ca, Sr, Ba)                   hydrated

Properties
• All metal chlorides are ionic in nature except for BeCl2 is which can be polymeric (RT) or dimeric (vapour phase) or linear (> 900 °C).
• MCl2 salt is obtain heating the hydrated chloride salts (except MgCl2 .6H2O)
− H2O          MCl2 .mH2O → MCl2 anhydrous
If M = Mg
MgCl2 .6H2O → M(OH)Cl + HCl + 5H2O So anhydrous is obtained by heating the hydrated chloride in the flow of HCl gas,                                                                   HCL(g)   MgCl2 .6H2O → MgCl2 anhydrous

Application
• MgCl2
- Sorel cement (MgCl2 + MgO) for
- Filling materials in
- Connecter between glass and                       metals
- Material in bandage
• CaCl2 anhydrous :
- Dehydrating agent in organic liquid and         confined space
- Controlling dust (put on the road)
- Deicing salt in temperate country

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COMPOUNDS OF GROUP IIA: HYDRIDE (MH₂)

Preparation:

For elements other than Be, directly heating it in hydrogen

M(p) + H₂(g) --> MH₂(p)

For Be

2BeCl₂ + LiAlH₄ --> BeH₂ +LiCl +AlCl₃

Properties:

1. All metal hydrides are ionic in nature and contains H- ion except for BeH₂.

2. BeH₂ is a polymeric solid that forms covalent bonding in which Be atom linked by hydrogen bridges.

Reactions:

With water

MH₂ + 2H₂O -->M(OH)₂ +2H₂

Thermal stabilization

MH₂ --> M + H₂

Thermal stability increases as we go down the group (Mg<Ca<Sr<Ba)

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Summary of Oxides for alkaline earth metals (Group IIA)

Preparation

in Industry

Heating the carbonate salts of alkaline earth metals will produce metal oxides and carbon dioxide gas.
MCO3(s) → MO(s) + CO₂(g) △

in Laboratory

for Mg and Ca,heating metal carbonates,metal hydroxides or metal nitrates will produce metal oxides.
MCO₃(s) → MO(s) + CO₂ (g) △ M(OH)₂(s) → MO(s) + H₂O(l) △ M(NO₃)₂(s) → MO(s)+ 4NO₂(g) + O₂(g) △
Physicochemical properties

Except BeO,all metal oxides are ionic.

From Beryllium to Strontium, they form monoxide only.While Barium form peroxide under pressure.(divalent metal ions sufficiently polarizing to make peroxide when heated in pure oxygen)

Solubility of oxide increases going down from Beryllium to Barium.

1. Hydration energy and the lattice energy decrease due to the increase in cation size.Actually both decrease together but the decrease in lattice energy is larger than the decrease in hydration energy which results in -ve value for total dissolution energy.

Melting point of monoxide decreases going down from Mg to Ba. (Due to the increasing of cation size which reduces the lattice energy slightly)

only BeO is amphoteric, other oxides are base. ( greater  ΔElectronegativity,more ionic character,more basic)

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NUR AIDA SYAMIMI BINTI AZHAR (A20SC0210)

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NUR AIDA SYAMIMI BINTI AZHAR (A20SC0210)

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Summary of Carbonate (Group 11A)

Carbonate - exist naturally in earth crust due to its insoluble property

Preparation
1. MgCO3 (magnesite)
⁃ Magnesium nitrate will react with NaHCO3 (sodium bicarbonate) bcs NaCO3 is too basic which will produce basic magnesium hydroxide.

2. CaCO3
⁃ CaCl2 react with NaCO3 to produce calcium carbonate

Properties
Going down the group
1. Solubility decreases
2. Thermal stability increases
3. Carbonate ions react with acids produce carbon dioxide

Stability of Carbonate Ions

1. Going down the group, ionic radius increases.
2. The strength of ionic bonding between cation and anion decreases which make it harder to break the bond ;                because the bond strength between carbonate ions molecile increases.
3. decompositio of carbonate ions will occur when the strength of ionic bonding between anion and cation increases.

Polarizing the Carbonate Ions

Oxygen is electronegative atoms which will attract the electron itself, therefore, the delocalize electron is around the oxygen atom. Hence it has higher charge density.

But once positive ions of group 11A is placed near the carbonate ions, the positive ions will attract the delocalized electron.

Carbonate ions is polarized.

1. Going down the group, positive ions gets bigger.
2. The charge density decreases.
3. The polarizing power become weaker
4. Less effect on the carbonate ion.
5. Carbones become more thermally stable.

But when across the period, the ionic radius decreases, increasing the polarizing power. Hence, stability decreases across the period.

Uses of CaCO3 (limestone)

1. When heated produce CaO(quicklime)
2. Fuel industry - coke combustion
3. Building material - portland cement
4. Diet Enrichment.
5. Antacid

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GRUOP IIA HYDROXIDE

PREPARATION

Group 2 elements react with water to form hydroxides with the general formula M(OH)₂ along with hydrogen gas, H₂.

M (s)+ H ₂ O (l)→ M(OH)2 (aq)+ H 2 (g)

Group 2 oxides react with water to form a solution of metal hydroxides

MgO (s)+ H ₂ O (l)→ Mg(OH)₂(aq)

Where M is Ca, Sr or Ba

To prepare Be(OH)₂

BeCl₂+ 2NAOH → Be(OH)₂

To prepare Mg(OH)₂

MgSO4+ 2NaOH → Mg(OH)₂

PROPERTIES

Exist as white solid

All IONIC (except Be(OH)₂)

Group IIA hydroxides are soluble, they dissolve in water forming alkaline solutions except Be(OH)2 is insoluble in water.

M(OH)₂(s) + aq → M²⁺(aq) + 2OH⁻(aq)

Where M = Mg, Ca, Sr and Ba

Thermal stability increases down the group

Basicity increases down the group

Be(OH)2 is amphoteric

Be(OH)₂ (s) + 2H⁺ (aq) → Be²⁺ (aq) +2H₂O(l) Be(OH)₂ (s) + 2OH⁻ (aq) → Be(OH)₄ 2- (aq)

SOLUBILITY

The solubility of the Group 2 hydroxides increases as you go down the Group.

Decrease in lattice energy is greater than decrease in hydration energy as anion is not much larger than the cations.

This means that as you go down Group 2 more hydroxide ions are formed (for the same amounts).

This means that as you go down Group 2 they become more alkaline.

THERMAL STABILITY

Group 2 carbonates can be decomposed by heat, forming an oxide and carbon dioxide. This type of reaction is called thermal decomposition.

MCO₃(s) → MO(s)+ CO₂(g)

The further down the group, the more difficult it is to decompose.

USES
The alkaline nature of the group IIA hydroxides means that they are often used in order to combat acidity.

Calcium hydroxide, Ca(OH)₂  commonly used by farmers to neutralise acid soils.

Magnesium hydroxide, Mg(OH)₂     used as milk of magnesia to relieve indigestion by neutralising stomach acid.

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NURUL IDA KHAIRUNNISA BINTI MOHD USMAN (A21SC0314)

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NURUL IDA KHAIRUNNISA BINTI MOHD USMAN (A21SC0314)

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Compounds of Group IIA : SULPHATE

Preparation
- reaction of the metal salts with sulphuric acid

Properties
- exist in hydrated form.
- the number of mole hydrated water depends on temperature.
- thermal stability increases ( down the group)
* because decrease in polarizing ability.
* charge density also decrease.
- solubility decreases (down the group)

Application
- Epsom salt (MgSO₄)
* coagulant for making tofu
- Gypsum salt (CaSO₄)
* fertilizer in agriculture
- BaSO4
* to obtain good quality photograph of the digestive tract

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NABILAH SYAIDA BINTI MOHD ZURAINI (A21SC0174)

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NABILAH SYAIDA BINTI MOHD ZURAINI (A21SC0174)

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SULPHATE
Preparation
Salt / MX + H2SO4 → MS04 + HX
* Let metal salts react with sulphuric acid.

Properties

All exists in hydrated form

The number of moles of hydrated water depends on the temperature.

Thermal stability increases (down the group) and decomposed to oxide when heated

BeSO4 < MgSO4 < CaSO4 < SrSO4 < BaSO4

Decrease in polarizing ability

Decrease in solubility (down the group)

BeSO4 > MgSO4 > CaSO4 > SrSO4 > BaSO4

Application of Metal Sulphate

Epsom Salt (MgSO4)

-medicine (saline laxitive)
-fertilizer
-coagulant for making tofu
-anyhydrous , drying agent

Gypsum Salt (CaSO4)

- Portland Cement
-Plaster of Paris
- mould , chalk
-Gypsum board
- fertilizer in agriculture

Barium Sulphate (BaSO4)

- In medical, opaque to X-rays " Barium meal " is given to a patient in oreder to obtain good quality photograph of the digestive tract.

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Group IIA- Hydride(MH2)

●Preparation
- it will directly heating of element in hydrogen  except berylium.
-For Be reaction in present of ether
2BeCl2 +LiAlH4 ----> BeH2 +LiCl +AlCl3

●Properties
-All metal hydrides are ionic in nature except BeH2 .
-BeH2 is polymeric solid that form covalent bond in which Be atom linked by hydrogen bridges.

●Reaction
-Reaction with water

When the element react with water it will produce hydroxide compund and hydrogen gas

MH2 + 2H2O -----> M(OH2) +2H2

-Thermal stabilization
Mg<Ca<Sr<Ba
When down the group AII the thermal stabilization increases.

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GROUP IIA - HYDROXIDE

1. Preparation

-For Be(OH)2, we should use

BeCl2+2NaOH➡Be(OH)2 + 2NaCl

-For Mg(OH)2, we should use

MgSO4+2NaOH➡Mg(OH)2+Na2SO4

-For M=Ca, Sr, Ba

MO+H2O➡M(OH)2

2.  M(OH)2 exist as white solid, all are ionic except Be(OH)2

3. Solubility

-solubility increases down the group due to decrease in lattice energy

*Be(OH)2 is completely insoluble

4. Thermal stability

-thermal stability increases down the group due to decrease in polarizing power of M2+ and lower lattice energy of MO product

Be(OH)2➡BeO + H2O

5. Basicity (how many OH-)

- Basicity increases down the group because :

i. solubility increase

ii. size of metal ions increase, charge density decrease

iii. lower attraction between OH- and larger ion (not compatible)

iv. ions split away from each other easily

v. higher concentration of OH- in water, basicity increase

*Be(OH)2 is amphoteric

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Group IIA- HYDRIDE

*Preparation*
-By direct heating of element in H2
M(p) + H2(g) → MH2(p) ; (M=Mg-Ba)
•for Be
2BeCl2 + LiAlH4 → BeH2 + LiCl +AlCl3

*Properties*
-All metal hydrides are ionic in nature and contain H- ion
-except BeH2 that are polymetric solid (covalent bond) which Be linked by hydrogen bridges

*Reactions*
-H20
MH2 + 2H20 → M(OH)2 +  2H2 (M=Mg-Ba)
-Thermal stabilization
MH2 → M + H2
(Mg< Ca< Sr< Ba)
(As we go DOWN the group, thermal stabilization INCREASE )

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Oxide (MO)

Preparation of MO and CaO
In industry
-MCO₃ →  MO + CO₂
△
In laboratory
-MCO₃ → MO + CO₂
△
-M(OH)₂ → MO + H₂O
△
-M(NO₃ )₂ MO → MO + 4NO₂ + O₂
△

Physicochemical Properties
1) All are ionic except BeO4

2) Only form monoxide for Be, Mg, Ca, Sr

3) Only form peroxide for Ba under pressure

4) Did not form superoxide
- the group IIA cation is too small, it is not easy for enough peroxide or superoxide ions to cluster round it to form a stable crystal lattice.

5) Solubility increases down the group
- Size cation increases
-  Hydration energy and lattice energy increase.
- The decrease in lattice energy larger than decrease in hydation energy
- When the lattice energy decreases, the enthalpy of sovation decreases

6) Basicity increases down the group.
- Difference in electronegativity increases
- More ionice the bond
- More basic

7) Melting point decreases down the group
- Size cation increases
- Slightly reduce in lattice energy
- When the lattice energy decreases, the enthalpy of sovation decreases.
- More easier to melt

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Carbonate (MCO3)
- Preparation :
~ most of carbonate of group IIA exists naturally in the earth
crust and form minerals due to the property of the carbonate

~ in laboratory cannot use Na2CO3 because it is too basic compared to
NaHCO3 and will produce basic magnesium carbonate

Physicochemical properties (MCO3)
- Solubility decreases down the group
- Thermal stability
BeCO3, MgCO3, SrCO3, BaCO3
Increasing stability due to decrease in polarizability

Stability of the oxyanion
- Increases down the group because the strength of ionic bonding between cation and anion resulting in the increase of bond strength between the atoms in oxyanion molecule and also due to dissociation occur if the strength between the anion and cation

Polarizing the carbonate ion
- The smaller positive ion, the higher the charge density, and the greater the effect on the carbonate ion
- Positive ions get bigger down the group, they have less effect on the carbonate ions near them to
compensate, the compound must be heated more in order to force the carbon dioxide to break off and leave the metal oxide
- Carbonates become more thermally stable down the group

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NUR NABILA NATASYA BINTI MOHAMAD NAZRI A21SC0247

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NUR NABILA NATASYA BINTI MOHAMAD NAZRI A21SC0247

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Compound of group IIA - Hydride (MH2)

Preparation

- Can be prepared by direct heating of elements in      hydrogen (except Be)

M(p)   +    H2(g)  →  MH2(p)  ; (M= Mg….Ba)

For Be
ether
2BeCl2+  LiAlH4  -----→  BeH +  LiCl   +   AlCl3

Properties

- All metal hydrides are ionic in nature and contain H-ion (exceptBeH2)
- eg: MgH2

- BeH2 is polymeric solid ( covalent bonding ) in which Be     atom linked by hydrogen bridges

Reactions of Hydrides

- Industry : By heating the carbonate salts of Group IIA     metals

heat
MCO   ---→   3MO +   CO2       ; (M= Mg, Ca)

- Laboratory : M = Mg and Ca

heat
MCO3   ---→  MO  +   CO2

heat
M(OH)2    ---→    MO  +  H2O

heat
M(NO3)2   ---→    MO  +  4NO2  +  O2

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GROUP IIA COMPOUND: SULPHATE

Preparation of sulphate:
-let metal salts react with sulphuric acid
eg: MgCO3 + H2SO4 -> MgSO4 + CO2 + H2O

Properties:
-all sulphate salts exist in hydrated form
*the no. of mole of hydrated water depends on the temperature
-thermal stability increases down a group
*this is due to the decreasing of polarizing ability
-solubility decreases down a group
*this is due to the increasing of ionic size in the order: Mg2+<Ca2+<Sr2+<Ba2+, then the hydration energy ,H hyd of the ions is more rapid than the lattice energy(*both of these energy are decreasing, but H hyd is the dominant reason)
*Hence, the total energy gives small exothermic value(less -ve)

Application of Metal Sulphate:
-Epsom salt, MgSO4
used for
*medicine(saline laxative : to treat constipation)
*fertilizer(for soil amendment)
*coagulant for making tofu
*anhydrous[no water] (as a drying agent)
-Gypsum salt, CaSO4
used for
*portland cement(basic ingredient of concrete, mortar, stucco and etc.)
*plaster of Paris (for sculpting, casting, and gauze bandages)
*mould, chalk
*gypsum board(partitions)
*fertilizer in agriculture
-Barium Sulphate, BaSO4
used for
*medical : opaque to X-rays(usually in liquid form, a good quality photograph of the digestive tract can be obtained after a patient drank it)

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Group IIA Compound - Hydride (MH2)

1. Preparation
- Mg->Ba - direct heating of elements in hydrogen (except Be)
M+H2 → MH2
- For Be
BeCl2 + LiAlH4 → BeH2 + LiCl + AlCl3

2. Properties
- all metal hydrides are ionic in nature except BeH2 (polymeric solid in which Be atom linked by hydrogen bridges)

3. Reactions
- reaction with water (Mg → Ba)
MH2 + 2H2O → M(OH)2 + 2H2
- thermal stabilization (increases down the group due to the ionic size increases down the group)
MH2 → M + H2

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Group IIA - Hydride (MH₂)

Preparation
•M(s) + H₂(g) → MH₂ (g) (M=Mg,Ca,Sr,Ba)
•BeCl₂ + LiAlH₄ → BeH₂ + LiCl + AlCl₃ (ether)

Properties
•Ionic & contain H¯ ion (except Be)
•Polymeric solid & Be atom linked by hydrogen bridges.

Reactions
1. with H₂O (M=Mg,Ca,Sr,Ba)
MH₂ + 2H₂O → M(OH)₂ + 2H₂
2. thermal stabilization
MH₂ → M + H₂
Mg<Ca<Sr<Ba

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GROUP IIA COMPOUND-OXIDE

Preparation
(1) In industry : by heating carbonates salts
MCO3 → MO + CO2 ( M = Mg, Ca)
(2) In laboratory :  for ( M = Mg, Ca)
MCO3 → MO + C
M(OH)2 → MO + H₂O
M(NO₃)2 → MO + 4NO₂ + O2

Physicochemical Properties
- all are ionic (except BeO)
-Monoxide(MO) only form from Be to Sr because divalent metal ions are sufficiently polarizing to make peroxide when heated with pure O2.
-Ba form peroxide.

-Solubility increases down the group.
BeO< MgO< SrO< BaO
the decrease in lattice energy is larger   than the decrease in hydration energy resulting in -ve value for the total dissolution energy

-Melting point of MO decreases down the group because the size of cation increases, lattice energy decreases.
-are base (except BeO amphoteric)
-basicity increases down the group
-the greater the difference in electronegativity, more ionic the metal-oxygen bond, more ionic characteristics, more basic

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Hydride
# Preparation
- direct heating of element in H2 ( expect Be)
For Be:
BeCl2 + LiAlH4 → BeH2 + LiCl + AlCl3

# Properties
- all metal hydrides are ionic in nature ( contain H- ion）expect BeH2 (polymeric solid- covalent bonding)

# Reactions
1) Reaction with H2O
MH2 + 2H2O → M(OH)2 + 2H2 (M= Mg, Ca, Sr, Ba)

2) Thermal stabilisation
MH2 → M + H2
- increase down the group
- increasing in cationic size from Mg to Ba
- charge density decrease, polarising power decrease, less polarised.
- more heat required to decompose

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Group IIA Carbonate
- Most of carbonate of Group IIA in earth form mineral

- Solubility decrease down the group (decrease lattice energy is more than the hydration energy due to big size of anion)

- Thermal stability increase down the group (due to decrease polarisability)

- Decomposition to form metal oxide and carbon dioxide

- Ease of decomposition decrease down the group ( weaker ionic bonding , stronger then carbonate ion hold together )

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GROUP IIA - OXIDE

Burns very vigorously as move down the group
Monoxide : M + O₂→ 2MO ( M = Be~ Sr)
Peroxide : M + O₂→ MO2 ( M = Ba)
x Superoxide:
-cation of Group IIA too small
-not easy for enough peroxide/ superoxide to cluster around to form stable crystal lattice
Redox reaction: metal oxidised, oxygen reduced

Preparation
In industry : by heating carbonates salts
( M = Mg, Ca)
In laboratory : by heating carbonates, hydroxides and nitrates salts
( M = Mg, Ca)
MCO3 → MO + C
M(OH)2 → MO + H₂O
M(NO₃)2 → MO + 4NO₂ + O2

Properties
- are ionic (except BeO)
-Solubility ↑
-Melting point↓
-are base (except BeO amphoteric)

Solubility↑ BeO< MgO< SrO< BaO
- size ion ↑ , hydration energy ↓, lattice energy ↓
- lattice energy ↓> hydration energy ↓

Melting point↓ MgO< CaO<SrO< BaO
-increasing cation size down the group
- cause slightly reduces in lattice energy

Basicity ↑ down the group
BeO<MgO< CaO<SrO< BaO
*greater the difference in electronegativity, more ionic the metal-oxygen bond, more basic

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Group IIA Compound – Hydroxide (M(OH)2)

*Preparation:

· To prepare Be(OH)2,

BeCl2 + 2NAOH→ Be(OH)2 + 2NaCl

· To prepare Mg(OH)2,

MgSO4 + 2NAOH→ Mg(OH)2 + Na2SO4

· To prepare M(OH)2,

MO + H2O→ M(OH)2
where M= Ca, Sr, Ba

*Physicochemical Properties:

-Exist as white solid

-All ionic but Be(OH)2) is covalent

-Solubility increases down the group  as lattice energy decreases down the group

but Be(OH)2) is insoluble

-Thermal stability increases down the group but Be(OH)2)is unstable as it easily decomposed to oxide

-Basicity increases down the group

but Be(OH)2)is unstable Amphoteric

*Reason of Basicity increases down the group

- When going the group, the solubility increases

-  Size of metal ions also increases make the decreases of charge density

- Attraction between OH- ions and M2+ ions become weaker

- Therefore, OH- ions easily split away from M2+ ions and releases into water

- Concentration of OH- ions in water increases

- So, the basicity increases.

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CARBONATE
👉exists naturally in the earth crust
👉insoluble
👉react with NaHCO3 (cannot use Na2CO3)to get carbonate in LAB

(Properties)
👉Down the group
-solubility decreases

-thermal stability increases

-stability of the oxyanion increases
❤️the strength of ionic bonding between cation and anion decreases,bond strength between atoms in oxyanion increases,thus become more stable
❤️when ionic bonding stronger, decomposition occur.

-the smaller the cation,the higher the charge density,the higher the polarizing power,the greater the effect on the carbonate ion,easier to decompose carbonate ion when heating, thermal stability low
-down the group,size of cation increase,charge density decrease,polarizing power decrease,less effect on the carbonate ion,harder to decompose carbonate ion when heating,thermal stability increase.

(Commercial uses of CaCO3)
-Solvay process
-Fuel industry
-produce CaO
-Building material
-Portland Cement
-Antacid
-Diet Enrichment

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Preparation of compound sulphate
-Reaction of metal salts with sulphuric acid to get sulphate salt
-All sulphate salt exist in hydrated form,the number mole of water depend on the temperature

Thermal stability increase down the group
-Due to the decrease in polarizing power of cation, the polarizing power to distort anion low, thus it is more stable and need more heat to decompose

Solubility decreases down the group
-size of ion increase, the hydration energy decrease(less -ve), the polarizability of ion toward slovent decrease

Application of compound sulphate
MgSO4 - Epsom salt,medicine, fertilizer,coagulant for making tofu,anhydrous as drying agent
CaSO4 - Gyspum salt, Plaster of Paris, Portland Cement,mould,chalk,gypsum board , fertilizer in agriculture
BaSO4 - opeque to X-rays. "Barium meal" used to obtain good quality photograph of the digestive tract.