What Are Group 13 Elements?
The group 13 elements are the first group in the p-block of the periodic table. All the elements of group 13 are also called the boron family. The periodic table is segregated into s, p, d and f-blocks. This segregation is done based on the valence electron; if the valence electron falls on the p subshell, it comes in the p-block and so on.
The members of Group 13 elements are as follows:
The general electronic configuration for the group 13 elements is ns2 np1.
Table of Contents
- Oxidation States
- Covalent Character
- Anomalous Behaviour of Boron
- Chemical Properties
- Physical Properties
- Compounds of Group 13 Elements
Oxidation States and Inert Pair Effect
The general oxidation state exhibited by the group 13 elements in the group are +3 and +1. As we go down the group of the Boron family, the tendency to form +1 ion increases. This is due to the inert pair effect.
To elucidate, consider B3+ and B+. It is shown experimentally that B3+ is more stable than B+. Now, consider, Tl3+ and Tl+. It was seen that Tl+ is more stable than Tl3+.
This can be explained using the inert pair effect. It is the non-participation of the s-orbital during chemical bonding due to the poor shielding of the intervening electrons.
Simply put, for elements like Indium and Thallium, d and f orbitals are filled with electrons. Since the shielding ability of d and f orbitals are very poor, the nuclear charge that seeps through attracts the s orbital closer to the nucleus. This makes the s orbital reluctant to bond, thereby, only the p electrons are involved in bonding.
Covalent Character of Group 13 Elements
There are three reasons for the formation of covalent compounds by group 13 elements.
- Fajan’s rule may be applied. The smaller the cation, the more is the covalence.
- They have very high ionisation enthalpies ( IE1+IE2+IE3), which makes the formation of ionic compounds hard.
- They have relatively higher electronegativities, and hence the formation of compounds would not result in a higher electronegativity difference.
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Reasons Behind the Anomalous Behaviour of Boron
Boron behaves differently from the rest of the elements present in group 13 because of the following reasons:
- It has a very small size
- It has very high ionisation enthalpy
- It has high electronegativity owing to its small size
- The absence of d-orbital in the valence shell
⇒ Check: List of all periodic table elements
Chemical Properties of Group 13 Elements
Reactivity of Group 13 towards Oxygen
All of the elements of group 13 react at high temperatures forming trioxides, M2O3.
4M(s) + O2 (g) → 2M2O3(s)
Tl, besides forming Tl2O3, forms Tl2O.
The reactivity of group 13 elements towards oxygen increases down the group.
Boron is unreactive towards oxygen in its crystalline form. Finely divided amorphous boron reacts with oxygen on heating to form B2O3.
Thermodynamically, aluminium should react with air, but it is stable. This is because Al2O3 forms as a protective layer on the surface of the metal, thereby making it inert.
Reactivity of Group 13 towards Acids and Alkalis
Boron does not react with non-oxidising acids like HCl, but at higher temperatures, it reacts with strong oxidizing acids like a mixture of hot concentrated H2SO4 and HNO3 to give boric acid.
B(s) + 3HNO3 (aq) → H3BO3 (aq) + 3NO2 (g)
Boron resists the action of alkalis (NaOH and KOH) up to 773 K, above which they form borates.
2B(s) + 6KOH(s) → 2K3BO3(s) + 3H2(g)
All the other elements of group 13 react both with non-oxidising and oxidising acids, liberating hydrogen gas.
Note: The action of concentrated HNO3 renders Aluminium and Gallium passive by forming a protective layer of oxide.
Aluminium and Gallium can also react with alkalis liberating hydrogen gas.
2Al(s) + 2NaOH (aq) + 6H2O (l) → 2Na [Al (OH) 4] (aq) + H2 (g)
Reactivity of Group 13 towards Halogens
They react with halogens at high temperatures to form trihalides MX3.
2M(s) + 3X2 (g) → 2MX3 (where X=F,Cl,Br,I)
Tl, however, only forms TlF3 and TlCl3.
Note: Tl also forms mono-halides.
Reactivity of Group 13 towards Water and Metals
Reactivity towards Water :
Boron does not react with water or steam; however, at very high temperatures, it reacts with steam.
2B + 3H2O → B2O3 + 3H2
If the oxide layer is absent, Aluminium decomposes in cold water to yield hydrogen gas. Gallium and Indium do not react with water unless oxygen gas is present. Thallium forms TlOH in moist air.
4Tl + 2H2O + O2 → 4TlOH
Reactivity towards Metals:
Only boron combines with metals to form borides. The rest of the elements of group 13 are reluctant to combine with metals. This portrays the non-metallic character of Boron.
3Mg + 2B → Mg3B2
Complex Forming Tendency
Group 13 elements have more tendency to form complexes than s-block elements due to their smaller size and more polarising power.
Boron can form many complexes like [BF4]–. It has sp3 hybridized orbitals and tetrahedral geometry. Other elements also form complex compounds like Li[AlH4], [GaCl6]3-.
Physical Properties of Group 13 Elements
Atomic and Ionic Radii
The atomic radii of group 13 elements are lesser than their corresponding group 2 elements. This is because the effective nuclear charge increases which makes the size of the atom smaller.
The atomic and ionic radii down the group increase due to the addition of a new shell. There is a deviation, however, on moving from Aluminium (143 pm) to Gallium (135 pm). This arises due to the poor shielding of the intervening d-orbitals in Gallium, making the size smaller than Aluminium.
Boron< Aluminium > Gallium < Indium< Thallium
Down the group, the values of Ionization Enthalpy do not decrease smoothly. From Boron to Aluminium, the Ionization Enthalpy increases as expected. But from Aluminium to Gallium, the Ionization Enthalpy increase slightly. The first Ionization Enthalpy of Thallium is greater than Aluminium.
Reason: This trend is observed due to the poor shielding of d and f orbitals. Gallium is smaller than Aluminium due to poor d shielding; therefore, IE1 of Aluminium < IE1 of Gallium. Similarly, Thallium has intervening f orbitals, which are very poor at shielding, thereby increasing the IE1 of Thallium.
The electronegativity first decreases from B to Al, then it increases slightly from Aluminium to Tl. This can be attributed to the poor shielding of the intervening d and f orbitals.
The trend expected should be the exact opposite of electronegativity. The metallic character first increases from B to Al, then it decreases slightly from Aluminium to Tl.
This is due to the fact that Group 13 has a very high Ionization Enthalpy. Also, the larger the size of the ion, the lesser is its Ionization Enthalpy. Therefore, Aluminium is the most metallic. This can further be explained using the standard reduction potentials.
This shows that Aluminium is the most metallic and that Tl3+ isn’t that stable, as the potential is positive, making Gibb’s free energy positive. (∆G = -nFE).
The elements of group 13 have higher densities than group 2 elements. This is because they have smaller sizes, and hence small volumes. The density increases from B to Tl.
The acidic character of oxides of group 13 elements decreases down the group, and the basic character increases.
Note: Both Al and Gallium are amphoteric in nature.
H3BO3 is a monobasic acid in water. This is because water acts as a Lewis base, and H3BO3 acts as a Lewis acid. This results in the release of a proton,
B (OH) 3 + H2O ↔ [B (OH) 4] – + H+
Compounds of Group 13 Elements
All the elements of group 13 form sesquioxides (sesqui means one and a half). The formula of the oxide formed is MO3/2 or M2O3.
B2O3 is formed by heating amorphous boron in air,
4B + 3O2 → 2B2O3
Boron suboxide (BO) 2 is formed by heating B2O3 with boron at 1050°C.
B + B2O3 → (BO) 2
The oxides of the other elements can be prepared by the thermal decomposition of their nitrates or their hydroxides.
2Al (OH) 3 → Al2O3 + 3H2O
Boron forms trihalides with Fluorine, Chlorine, and Iodine. All of the trihalides formed are planar molecules and sp2 hybridized.
Since all the elements of group 13 possess only 6 electrons in their valance shell, they act as Lewis acids.
The order of the Lewis acid character exhibited by the trihalides is,
Reason: This is not in accordance with the normal trend observed; surely, we can claim that BF3 is the most acidic as F is the most electronegative.
The reason for the above trend is back bonding, specifically, pπ-pπ back bonding. The lone pair on F is given to the empty p-orbital of B, making it less electropositive and, thereby, reducing the acidic character.
The overlap of B and F is maximum as their sizes are compatible. Boron cannot form effective back bonding with Cl or Br as they are bigger than B. The halides of Al, Gallium, In and Tl are largely covalent.
Borates are compounds of group 13 containing discrete [BO3]3- units. Each unit is sp2 hybridized. They are classified according to the way the individual units are linked.
- Orthoborates: They contain discrete BO33- units. For example, Mg3(BO3)2.
- Pyroborates: Two units of BO33- are linked via a common oxygen atom. The formula is B2O54-. For example, Mg2B2O5.
- Metaborates: They have a structure where each unit shares two oxygen atoms. Therefore, they are either in the form of chains or cyclic. The general formula is (BO2)nn-.
- Sheet borate: The two-dimensional network of borates where all three oxygen atoms are shared.
The binary compounds formed by boron and hydrogen are called boranes. The simplest borane known is B2H6. They are classified into three major types,
- Closo-boranes ( BnH2n+2)
- Nido-boranes (BnH2n+4)
- Arachno-boranes (BnH2n+6)
It can be prepared by reacting BCl3 with hydrogen gas over a Cu-Al catalyst at 450°C.
2BCl3 + 6H2 → B2H6 + 6HCl
Diborane on heating alone or in the presence of hydrogen, higher boranes are obtained.
Structure of Diborane
The total number of valence electrons present in diborane = 3 × 2 + 1 × 6 = 12 electrons.
The number of valence electrons in ethane (C2H6) = 4 × 2 + 1 × 6 = 14 electrons.
Therefore, we can see that diborane is electron deficient, and hence should be unstable.
From the data obtained from electron diffraction studies, we were able to elucidate the structure of diborane.
It has two types of hydrogen atoms, terminal and bridged. The four terminal B-H bonds have the same bond length, and they are normal covalent bonds.
The two bridged hydrogen atoms, however, the H-B-H bond, are much longer than the terminal B-H bond. The H-B-H bond is unusual as the two bridges involve only one electron from each hydrogen atom giving a total of four electrons. That is, each H-B-H bond has two electrons delocalized over three centres, giving rise to a three-centred two-electron bond.
Boron-Nitrogen species that carry only one substituent on each atom and exist as trimers are called Borazine (B3N3H6).
It is prepared by heating diborane and ammonia in a 1:2 molar ratio at -120°C, which gives ionic species which, on heating, give borazine.
B2H6 + 2NH3 → [H2B(NH3)2]+[BH4]– → B3N3H6 + 6H2
Similarities of Borazine with Benzene
- Borazine is isoelectric with benzene, i.e., the total number of electrons in benzene = 6 × 6 + 1 × 6 = 42 electrons and the total number of electrons in borazine = 3 × 5 + 3 × 7 + 6 × 1 = 42 electrons.
- Borazine is isosteric with benzene. That is, the total number of atoms are the same.
- Borazine possesses a cyclic structure of alternating boron and nitrogen atoms.
- Both N and B are sp2 hybridized.
Properties of Borazine
- It readily undergoes an addition reaction. This is because the B-N bond is polar, unlike the covalent C-C bond, and hence addition reactions happen easily.
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