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Group 13 Flashcards

1
Q

Name elements of Group 13

A

Boron - Aluminum - Gallium - Indium - Thallium - Nihonium

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2
Q

Discuss occurrence of Boron

A
  1. Borax
  2. Orthoboric acid
  3. Kernite
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3
Q

Give formula of borax

A

Na2B4O7.10H2O

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4
Q

Give formula of orthoboric acid

A

H3BO3

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5
Q

Give formula of kernite

A

Na2B4O7.4H2O

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6
Q

Where is borax found in India

A

Sambhar Lake in Rajasthan and Puga Valley in Ladakh

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7
Q

Does boron have isotopes? Discuss

A

Yes, two - B(10) and B(11)

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8
Q

Which isotope of Boron is more abundant

A

B(11) - 81%

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9
Q

Discuss abundancy of Aluminum

A

Most abundant metal

Third most abundant element on the Earth’s crust after oxygen and silicon

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10
Q

Discuss occurrence of Aluminum

A
  1. In Bauxite
  2. In Cryolite
  3. In mica
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11
Q

Give formula of Bauxite

A

Al2O3.2H2O

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12
Q

Give formula of Cryolite

A

Na3AlF6

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13
Q

Where is aluminum found in India

A

As Mica in Madhya Pradesh, Karnataka, Odisha and Jammu

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14
Q

What is the atomic number and mass of Nihonium

A

Nh has atomic number - 113 and atomic mass - 286 g/mol

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15
Q

Is Nh natural? Give its half life

A

Nh is synthetically prepared and radioactive

Its more stable isotope has a half life of 20 seconds

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16
Q

Electronic configuration of group 13

A

ns2np1

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17
Q

Discuss atomic size trend

A

Atomic size increases on going down the group due to increase in number of shells

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18
Q

Discuss exception wrt atomic size

A

Ga has smaller size than Al because Ga has 10 d electrons which provide very small shielding effect for outer electrons and hence attracts the electrons closer to the nucleus

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19
Q

Discuss ionization enthalpy size trend

A

It decreases down the group as with increase in number of shells, the screening effect increases which makes it more and more easier to remove an electron

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20
Q

Discuss exception wrt ionization enthalpy

A

Ga > Al and Tl > In due to presence of d and f electrons

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21
Q

Discuss electronegativity size trend

A

It decreases from B to Al and then increases marginally

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22
Q

Discuss density size trend

A

Density increases down the group

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23
Q

Discuss physical properties of Boron

A
  1. Boron is non metallic
  2. It is hard and black colored
  3. It has many allotropic forms
  4. It has unusually high MP because of strong crystalline lattice
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24
Q

Discuss physical properties of all other elements

A
  1. They are soft metals
  2. They have low MP
  3. High electrical conductivity
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25
Discuss exception in Gallium's MP and BP
It is extremely low MP to the point where it melts in summer. It also has an incredibly high BP which makes it useful for measuring high temperatures
26
Oxidation State in Boron
Because of its small size, the sum of first 2 IEs is high and hence +3 ionic bonds are not formed. Instead, covalent bonds are formed.
27
Oxidation States observed in other elements
They show +1 and +3 oxidation states
28
Which OS is more stable and why
As we go down the group, due to poor shielding, the increased nuclear charge increases considerably and holds ns electrons tightly. This makes +1 OS more stable as we go down the group
29
Comparison of OS states
1. +1 is predominant in Ga, In, Tl 2. +3 is very oxidizing 3. Compounds formed with +1 state are much more ionic than +3 compounds
30
Discuss stability of +3 metals
They have only 6 electrons in their outermost orbital making them electron deficient They accept a pair of electrons, behaving as Lewis acids Tendency to behave as LA increases with size Al3+ compounds achieve stability by forming dimers
31
Discuss hydrolysis of +3 compounds
1. Most of them get hydrolyzed to [M(OH)4]- which is tetrahedral and the hybridization of M is sp3 2. Aluminum gets hydrolyzed to [Al(H2O)6]3+ which is octahedral and the hybridization of Al is sp3d2
32
Discuss reactivity in air
Boron is unreactive in crystalline form Aluminum forms a very thin oxide layer which prevents further attack on the metal All form oxides and nitrides
33
Oxides formation
M + O2 = M2O3
34
Nitrides formation
M + N2 = MN
35
Nature of oxides formed
Boron trioxide is acidic and reacts with metallic oxides to give metal borates Aluminum and Gallium oxides are amphoteric Indium and Thallium oxides are predominantly basic
36
Reactivity of boron with acids/alkalis
Boron does not react with either even at moderate temperatures
37
Reactivity of aluminum with acids/alkalis
Aluminum reacts with dil. HCl to release H2 gas However with conc HNO3, it becomes passive due to formation of passive oxide layer Aluminum also reacts with NaOH to release H2 gas
38
Reactivity with halogens
M + X2 = MX3
39
What anomalies can be seen in Boron
1. Unlike other metal trihalides, BX3 is insoluble in water 2. Other hydrolyzed compounds are also soluble in water except Boron 3. BF3 (Lewis acid) reacts with NH3 (Lewis base) to complete its octet 4. Other elements dimerize to attain stability but boron does not as its covalency cannot go beyond 4 due to absence of d orbitals
40
Correct formula of Borax
Na2 [B4O5{OH}4] 8H2O
41
Borax + water
Borax dissolves in water to give alkaline solution | Borax + water = NaOH + H3BO3 (weak acid)
42
Borax + heat
Initially, borax loses water and swells up (Na2B4O7) On further heating, it forms a transparent liquid which solidifies into a glass like material (B2O3 - boric anhydride/borax bead)
43
Explain the borax bead test
Metaborates of many transition elements give different colored borax beads eg: CoO on heating with a loop of platinum wire gives Co(BO2)2 which is a blue borax bead
44
Structure of Borax
White crystalline solid
45
Structure of H3BO3
White crystalline solid with soapy touch | Layer structure where planar BO3 units are joined by hydrogen bonds
46
Solubility of H3BO3
Sparingly soluble in water but solubility increases with heat
47
How is orthoboric acid prepared
By acidifying an aqueous solution of borax | By hydrolysis of any boron compounds
48
Discuss acidity of orthoboric acid
Weak monobasic acid | Acts as a Lewis acid by accepting electrons from a hydroxyl ion
49
Heating orthoboric acid
H3BO3 + heat = H2BO3 (metaboric acid) | H2BO3 + heat = B2O3
50
How is diborane prepared
``` BF3 + LiAlH4 = B2H6 + LiF + AlF3 In a laboratory, NaBH4 + I2 = NaI + B2H6 + H2 Industrially, BF3 + NaH = B2H6 + NaF ```
51
Physical properties of diborane
Colorless, highly toxic gas | Catches fire spontaneously in air ( most higher boranes are spontaneously flammable)
52
Hydrolysis of diboranes
B2H6 + H2O = B(OH)3 + H2
53
Diborane + Lewis Acid
Adducts are formed with the Lewis acid | eg: B2H6 + CO = BH3.CO
54
What is borazine
Inorganic benzene | B3N3H6
55
How is borazine formed?
B2H6 + NH3 = [BH2(NH3)2]+ [BH4]- | [BH2(NH3)2]+ [BH4]- + heat = B3N3H6 + H2
56
Structure of B2H6
Four terminal hydrogens + two boron atoms are all in one plane connected by single bonds The remaining two hydrogens are bridge atoms above and below this plane with B-H-B bonds
57
Hydridoborates
Boron forms a series of hydridoborates, the most important one being [BH4]- Lithium and sodium tetraborates are formed using this ion
58
What does -ve electrode potential mean
High tendency to perform reaction, makes stable product
59
What does +ve electrode potential mean
Low tendency to perform, very unstable
60
White fumes appear around the bottle of anhydrous aluminum chloride. Give reason
Anhydrous AlCl3 is partially hydrolyzed with atmospheric moisture to liberate HCl gas. Moist HCl appears white in color
61
Why is Boric acid considered weak
Because it cannot liberate H+ ions on its own. It receives OH- ions from water, completes its octet and then releases H+ ion

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