The group 13 elements or group 3A are also called the boron family. The elements of group 13 of the periodic table consisting of boron, aluminum, gallium, indium, and thallium.
General Trend of Group 13 Elements
The general trend of group 13 elements are given below:
- The metallic character of group 3A increases down the group.
- P-orbital is in the process of filling.
- All the elements show a +3 oxidation state.
- All the elements give MX3 halides.
- Boron is a non-metal but other elements are metal.
- The elements of group 13 give normal oxide.
- Ga, In, and Ti are rare elements.
Properties of Group 13 Elements
Boron
- Atomic number: 5
- Atomic symbol: B
- Atomic mass: 10.811
- Density: 2.34
- Melting point: 2300°C
- Boiling point: 2550°C
- Atomic radius: 87
- Covalent radius: 82
- Electronegativity: 2.04
- Electron affinity: 26.7 KJ/mol
- Magnetic type: Diamagnetic
- Electrical type: Insulator
- Year discovered: 1808
Aluminum
- Atomic number: 13
- Atomic symbol: Al
- Atomic mass: 26.98
- Density: 2.698
- Melting point: 660°C
- Boiling point: 2467°C
- Atomic radius: 118
- Covalent radius: 118
- Electronegativity: 1.61
- Electron affinity: 42.5 KJ/mol
- Magnetic type: Paramagnetic
- Electrical type: Conductor
- Year discovered: 1825
Gallium
- Atomic number: 31
- Atomic symbol: Ga
- Atomic mass: 69.723
- Density: 5.907
- Melting point: 30°C
- Boiling point: 2403°C
- Atomic radius: 136
- Covalent radius: 126
- Electronegativity: 1.81
- Electron affinity: 28.9 KJ/mol
- Magnetic type: Diamagnetic
- Electrical type: Conductor
- Year discovered: 1875
Indium
- Atomic number: 49
- Atomic symbol: In
- Atomic mass: 114.8
- Density: 7.31
- Melting point: 157°C
- Boiling point: 2000°C
- Atomic radius: 156
- Covalent radius: 144
- Electronegativity: 1.78
- Electron affinity: 28.9 KJ/mol
- Magnetic type: Diamagnetic
- Electrical type: Conductor
- Year discovered: 1863
Thallium
- Atomic number: 81
- Atomic symbol: Ti
- Atomic mass: 204.38
- Density: 11.85
- Melting point: 303°C
- Boiling point: 1457°C
- Atomic radius: 156
- Covalent radius: 148
- Electronegativity: 1.62
- Electron affinity: 19.2 KJ/mol
- Magnetic type: Diamagnetic
- Electrical type: Conductor
- Year discovered: 1861
Boron | Overview, Properties, Uses
Peculiar Behavior of Boron
| Boron | Other Group 13 Elements |
|---|---|
| Boron is a metal. | Other elements are non-metal. |
| Boron show +3, -3 oxidation state. | Al, Ga, In, and Ti show only a +3 oxidation state. |
| Boron does not form ionic compounds. | Other elements form ionic compounds. |
| Forms acidic oxide. | Amphoteric oxide except thallium. |
| It can form acids like H3BO3, HBO2, etc. | Do not form acids. |
| It forms molecular addition compounds. | Do not form molecular addition compounds. |
What is Inert Pair Effect In Group 13 Elements?
B5 = [He]2, 2s2, 2p1
Al13 = [Ne]10, 3s2, 3p1
Ga31 = [Ar]18, 3d10, 4s2, 4p1
In49 = [Kr]36, 4d10, 5s2, 5p1
Ti81 = [Xe]54, 4f14, 5d10, 6s2, 6p1
First of all, to know the reason for the inert pair effect, we will know the term shielding effect.
The valence electron of aluminum is attracted by the nucleus but the valence electron of aluminum show repulsion toward the inert electron of Al. So, the valence electron of the aluminum shows both attraction (towards the nucleus) and repulsion (toward the inert electron). The repulsion force of the inert electron of an atom towards the valence electron is called the shielding effect. The order of shielding effect is:
s > p > d > f
Does Gallium Show Inert Pair Effect?
In the case of Gallium, 3d10 is present and 10 electrons in the 3d subshell which is poorly shielded toward 4s2 and 4p1 subshell electrons. It means that 3d10 subshell electrons poorly Shield the 4s2 and 4p1 electrons.
So due to the poor shielding effect, 4s2 subshell electrons are attracted toward the nucleus strongly. That’s why 4s2 not easily loses electrons and does not take part in bond formation and gallium easily loses one electron of 4p1 and forms Ga1+, but if three electrons are removed and form Ga3+, more and more energy is required to form Ga3+. So, the inertness of 4s2 subshell electrons is called the inert pair effect.
Does Indium Show Inert Pair Effect?
In the case of Indium, 4d10 subshell electrons are present and before 4d10, 3d10 is also present. The electrons of 3d and 4d subshell poorly shield toward 5s2 and 5p1 subshell electrons. Due to the poor shielding effect of 3d10 and 4d10 on 5s2 and 5p1, the 5s2 attracted toward the nucleus strongly. That’s why 5s2 does not easily lose electrons and does not take part in bond formation. That’s why indium easily forms In1+ but not In3+. So, the inertness of 5s2 subshell electrons is called the inert pair effect.
Does Thallium Show Inert Pair Effect?
In the case of Thallium, 4f14 and 5d10 subshell electrons are present, and as we know the f-subshell has a very poor shielding effect toward the valance electrons. The electrons of 4f and 5d are very poorly shielded by the 6s2 and 6p1 electrons, and 6s2 show a stronger force of attraction toward the nucleus. That’s why thallium 6s2 valance electrons do not take part in bond formation. Thallium easily forms a +1 oxidation state but not +3 and we can say that Ti1+ is more stable than Ti3+. So, the inertness of 6s2 subshell electrons is called the inert pair effect.
As we move from top to bottom in a group, the inert pair effect increase. The order of inert pair effect of group-13 is:
Ti > In > Ga
Chemical Properties of Group 13 Elements
Reactions of Boron
React with Acid
Boron reacts with strong oxidizing acids such as nitric acid or hot concentrated sulfuric acid to form boric acid.
B + 3HNO3 → H3BO3 + 3NO2
2B + 3H2SO4 → 2H3BO3 + 3SO2
React with Alkalies
Boron reacts with boiling concentrated sodium hydroxide to form sodium metaborate and hydrogen gas is also evolved.
2B + 2NaOH + 2H2O → 2NaBO2 + 3H2
React with Water
2B + 6H2O → 2H3BO3 + 3H2
React with Oxygen
Oxides are formed by the direct reaction of boron with oxygen.
2B + 3O2 → B2O3
React with Sulfur
Boron directly reacts with sulfur at high temperatures and forms sulfides.
2B + 3S → B2S3
The boron sulfides are hydrolyzed by water.
B2S3 + 6H2O → 2H3BO3 + 3H2S
React with Nitrogen
Boron directly reacts with nitrogen and forms boron nitride.
2B + N2 → 2BN
Reactions of Aluminium
React with Water
At room temperature, Aluminium does not react with H2O but reacts with stream-evolving hydrogen gas.
2Al + 6H2O → 2Al(OH)3 + 3H2
React with Hydrogen
Aluminum combine with hydrogen gas and forms aluminum hydride.
2Al + 3H2 → 2AlH3
React with Oxygen
Oxides of aluminum are formed by the reaction of aluminum with oxygen. Aluminum oxides are used in flashlight photography.
4Al + 3O2 → 2Al2O3
React with Halides
Aluminum reacts with halogens X2 and forms 2AlX3. This reaction is exothermic in nature.
2Al + 3X2 → 2AlX3
2Al + 3Cl2 → 2AlCl3
React with Acids
2Al + 6HCl → 2AlCl3 + 3H2
2Al + 6H2SO4 → Al2(SO4)3 + 3SO2 + 6H2O
Al + HNO3 → NO Reaction
React with Alkali
It reacts with alkali and forms soluble sodium aluminate and liberates hydrogen gas.
2Al + 2NaOH + 6H2O → 2NaAl(OH)4 + 3H2
2Al + 2NaOH + 2H2O → 2NaAlO2 + 3H2
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