S-block (Group 2) Flashcards

1
Q

The first element …………. differs from the rest of the elements in the group and shows diagonal relationship with ………

A

Beryllium

Aluminum

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2
Q

Ionization energy order

A

Be > Mg > Ca > Sr > Ra > Ba

Due to poor shielding of 4f electrons

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3
Q

Hydration Energies G1 G2 comparison

A

Decreases down the group

HE: G1 < G2

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4
Q

Melting point order

A

Be > Ca > Sr > Ba > Mg

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5
Q

Boiling point order

A

Be > Ba > Ca > Sr > Mg

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6
Q

Density order

A

Ba > Sr > Be > Mg > Cr

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7
Q

Melting and boiling point comparision in G1 and G2

A

G1 < G2

Due to better metallic bonding in G2

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8
Q

Alkali earth metal hardness

A

These are comparatively softer than d-block elements because in d-block in addition to ns electrons (n-1)d electrons also take part in metallic bonding

But these are harder than alkali metals

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9
Q

Flame test

A

Calcium - brick red
Strontium - crimson
Barium - apple green

Due to high ionization energy of Be and Mg electrons do not get excited

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10
Q

G1 G2 reactivity comparison

A

G1 > G2

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11
Q

Reaction of Be and Mg towards oxygen and water

A

Be and Mg are inert to oxygen and water due to formation of oxide film on their surface

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12
Q

Powdered form of Be burns brilliantly in air to give

A

BeO and Be3N2

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13
Q

Magnesium burns in air

A

with dazzling brilliance to give MgO and Mg3N2

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14
Q

Ca, Sr, and Ba are readily attacked by air to form

A

their oxides and nitrides

(no peroxides and super oxides are formed)

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15
Q

Reaction with Water (rates)

A

Be neither reacts with hot water nor with steam of cold water

Mg decomposed hot water
Mg + 2H2O —> Mg(OH)2 + H2 [hot water]
Mg + H2O —> MgO + H2 [Cold water}

Ca, Sr, and Ba react with increasing vigor even with cold water to form hydroxide.

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16
Q

Reaction With Halogens

A

@ high temperature

M + X2 —> MX2

17
Q

Reactivity towards hydrogen

A

All elements except Be react with hydrogen to form their hydrides (MH2)

BeH2 can however be prepared by the reaction of BeCl2 and LiAlH4.

2BeCl2 + LiAlH4 —> 2 BeH2 + LiCl + AlCl3

18
Q

BeH2 and MgH2 Structure

A

Polymeric

19
Q

Reactivity towards acid

A

M + 2HCl —> MCl2 + H2

Generally dil. HCl and dil. H2SO4 are taken.

20
Q

Reactivity nature
Standard oxidizing and reduction potential order

A
  • EM/M2+
    BE 1.97
    Mg 2.36
    Ca 2.84
    Sr 2.89
    Ba 2.92

Thus Ba is the best reducing agent and Be is the worst reducing agent in group 2

21
Q

Why is Be the worst reducing agent?

A

The reaction
BE(s) —> Be2+(aq) + 2e-
takes place in two steps.

Step 1:
Sublimation of BE solid to Be gas. This process requires energy to proceed

Step 2:
Ionization. This process requires a lot of energy due to the small size .

Step 3:
Be2+ (g) –H2O–> Be2+ (aq)
In this process energy is released which is much less than the energy required

hence it is worst reducing agent

22
Q

Solution in liquid ammonia

A

Like alkali metals the alkaline earth metals dissolve in liquid ammonia to give deep blue black solution ammoniated ions.

M+ (x+y) NH3 —> [M(NH3)x 2+ + 2e(NH3)y]

From these solutions the ammoniates [M(NH3)6]2+ can be recovered by evaporation of ammonia from the solution.

M(NH3)6 —> M(NH3)2 + 4NH3 + H2

23
Q

Concentrated solution of metals in ammonia are …………. colored

A

Bronze colored due to the formation of metal ion clusters.

24
Q

Structure of alkaline earth metal oxides

A

Rock salt structures

25
Q

Alkaline earth metal oxides react with water to form

A

Metal hydroxides

except BeO

MO + H2O —> M(OH)2

26
Q

Thermal stability and basic character of hydroxides

A

increase from Mg(OH)2 to Ba(OH)2

The G2 hydroxides are however less basic and less stable than the G1 hydroxides

27
Q

Be is ….. in nature and reacts with

A

Be is amphoteric in nature and reacts with both acid and alkali.

Be(OH) + 2OH- —> [Be(OH)4]2- Beryllate ion

Be(OH)2 + 2HCl + 2H2O —> [Be(OH2)4]Cl

28
Q

Carbonates in water

A

Carbonates of G2 are insoluble in water.

They can be precipitated by addition of sodium or ammonium carbonate to the solution of soluble salts of these metals.

Solubility of carbonates in water decreases as atomic number increases.

29
Q

Thermal stability of Carbonates

A

increases from BeCO3 to BaCO3.

MCO3(s) —> MO+(s) + CO2

BeCO3 is very unstable and can kept in CO2 atmosphere

30
Q

Solubility of Sulphates

A

BeSO4 and MgSO4 are readily soluble in water and the solubility decreases from CaSO4 to BaSO4

31
Q

Solubility of nitrates

A

Nitrates of all elements are soluble in water.

2M(NO3)2 –heat–> 2MO + 2NO2 + O2

32
Q

Nature of halides

A

Except for Be halides all other alkaline earth metal halides are ionic in nature

BeX2 is covalent and soluble in organic solvents

BeCl2 is polymeric

33
Q

Heating hydrated halides

A

CaX2 + yH2O —> CaX2 + yH2O
SrX2 + zH2O —> SrX2 + zH2O
BaX2 + zH2O —> BaX2 + zH2O

In case of Be and Mg halides on heating hydrolysis occurs.

MgCl2.6H2O –heat–> Mg(OH)2 + 2HCl + 4H2O
Mg(OH)2 –heat–> MgO + H2O

34
Q

Preparation of anhydrous BeX2

A

BeO + C + Cl <—600-900K—> BeCl2 + CO

(NH4)2 BeF4 –heat–> 2NH3 + 2HF + BeF2

35
Q

Hydrolysis of Nitrides

A

Be3N2 + 6H2O —> 2NH3 + 3Be(OH)2

Mg3N2 + 6H2O —> 2NH3 + 3Mg(OH)2

36
Q

Hydrolysis of Carbides

A

BeC2 + 2H2O —> C2H2 + Be(OH)2 [Acetylides]

CaC2 + 2H2O —> C2H2 + Ca(OH)2 [Acetylides]

Mg2C3 + 4 H2O —> C3H4 + 2Mg(OH)2 [Sesquioxide]

Be2C + 4H2O —> CH4 + 2Be(OH)2 [Methanoids]