- Written bySahana Soma Kodarkar
- Last change 01/24/2023
We all know the periodic table. Isn't it difficult to remember all the properties of elements? There are \(18\) groups and \(7\) periods in the periodic table to study the properties of each element. You've probably heard of boron. Boron is used in the manufacture of popular fiberglass. In this article we will learn more about theGroup 13 elements: The boron family, from the periodic table.
Introduction to Group 13 elements
The group \(13\) represents the boron family and the elements that \({\rm{n}}{{\rm{s}}^{\rm{2}}}{\rm{n}} { { \rm{p}}^{\rm{1}}}\) configuration. Contains boron \(\left( {\rm{B}} \right)\) aluminum \(\left( {{\rm{Al}}} \right)\), gallium \(\left( {{\ rm {Ga}}} \right)\), indium \(\left( {{\rm{In}}} \right)\) thallium \(\left( {{\rm{Tl}}} \right) \ ) and the newly discovered element Ununtrium \(\left( {{\rm{uut}}} \right)\), which is radioactive. With the exception of boron, which is not a metal, all elements in this group have metallic properties. The nonmetallic character of B may be due to its small size, high ionization enthalpy, and relatively high electronegativity.
boron deposits
Boron is a relatively rare element known for its occurrence in borax deposits. Aluminum is the third most common element \(\left( {8.3\% } \right)\) in the earth's crust after oxygen \(\left( {46.0\% } \right)\) and silicon\( \left( { 27.7\ % } \right).\) The remaining three elements (Ga, In, and TI) are found in minor amounts as sulfides in lead and zinc sulfide ores.
The important minerals of boron are the following:
- Borax: \({\rm{N}}{{\rm{a}}_2}\left[ {\;{{\rm{B}}_4}{{\rm{O}}_5}{{( {\rm{OH}})}_4}} \right] \cdot 8{{\rm{H}}_2}{\rm{O}}\)
- Kernita: \({\rm{N}}{{\rm{a}}_2}\left[ {\;{{\rm{B}}_4}{{\rm{O}}_5}{{( {\rm{OH}})}_4}} \right]\)
- Colemanita: \({\rm{Ca}}\left[ {{{\rm{B}}_3}{{\rm{O}}_4}{{({\rm{OH}})}_3}} \derecha].{{\rm{H}}_2}{\rm{O}}\)
- Orthoborsäure: \({{\rm{H}}_3}{\rm{B}}{{\rm{O}}_3}\)
The main minerals of aluminum are the following:
- Bauxita: \({\rm{A}}{{\rm{l}}_2}{{\rm{O}}_3} \cdot {\rm{x}}{{\rm{H}}_2} {\rm{O}}\)
- Caolinita: \({\rm{A}}{{\rm{l}}_2}{({\rm{OH}})_4} \cdot {\rm{S}}{{\rm{i}} _2}{{\rm{O}}_5}\)
- Kriolita: \({\rm{N}}{{\rm{a}}_3}{\rm{Al}}{{\rm{F}}_6}\)
Electronic configuration of Group 13 elements
The general electronic configuration of the valence shell of the elements of group \(13\) is \({\rm{n}}{{\rm{s}}^{\rm{2}}}{\rm{ n }}{ { \rm{p}}^{\rm{1}}}{\rm{,}}\) where \(\mathrm{n}=2-7\) While boron and aluminum have noble gas nuclei, gallium and indium have Noble gas plus \(10\) d-electrons and thallium has noble gas plus \(14\,{\rm{f}}\)-plus \(10 \,{\rm{d}) }\)- nuclei of electrons .
As a result, the electronic configurations of the elements in group \(13\) are more complex than those in groups \(1\) and \(2.\). Therefore, the chemistry of all elements in this group is affected by this difference. in electronic configurations. The table shows the overall electronic configuration of these elements.
| Element | atomic number | Electronic configuration | with noble gas core |
| Boro \(\left( {\rm{B}} \right)\) | \(5\) | \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}} {\rm{2}}{{\rm{p}}^{\rm{1}}}\) | \([{\rm{Él}}]2\;{{\rm{s}}^2}2{{\rm{p}}^1}\) |
| Aluminium \(\left( {{\rm{Al}}} \right)\) | \(13\) | \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}} {\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\ rm{3}}{{\rm{p}}^{\rm{1}}}\) | \([{\rm{Ne}}]3\;{{\rm{s}}^2}3{{\rm{p}}^1}\) |
| Galio \(\left( {{\rm{Ga}}} \right)\) | \(31\) | \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}} {\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\ rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\ rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{1}}}\) | \([{\rm{Ar}}]3\;{{\rm{d}}^{10}}4\;{{\rm{s}}^2}4{{\rm{p}} ^1}\) |
| Indio \(\left( {{\rm{In}}} \right)\) | \(49\) | \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}} {\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\ rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\ rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}{\rm{ 4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}{\rm{ 5}}{{\rm{p}}^{\rm{1}}}\) | \([{\rm{Kr}}]4\;{{\rm{d}}^{10}}5\;{{\rm{s}}^2}5{{\rm{p}} ^1}\) |
| Talio \(\left( {{\rm{Tl}}} \right)\) | \(81\) | \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}} {\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\ rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\ rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}{\rm{ 4}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{f}}^{{\rm{14}}}}{\ rm{5}}{{\rm{s}}^{\rm{2}}}{\rm{5}}{{\rm{p}}^{\rm{6}}}{\rm{ 5}}{{\rm{d}}^{{\rm{10}}}}{\rm{6}}{{\rm{s}}^{\rm{2}}}{\rm{ 6}}{{\rm{p}}^{\rm{1}}}\) | \([{\rm{Xe}}]4{{\rm{f}}^{14}}5\;{{\rm{d}}^{10}}6\;{{\rm{s }}^2}6{{\rm{p}}^1}\) |
Physical Properties of the Boron Family (Group 13 Elements)
The physical characteristics of the born family are explained below.
1.atomic and ionic radii:
The atomic and ionic radii of the group \(13\) elements are smaller than those of the group \(2\). Both atomic and ionic radii are expected to increase as one moves down the group, as a new electron shell is added with each successive element. However, there are some deviations if we go from \({\rm{Al}}\) to \({\rm{GA}}\). For example, the atomic radius of \({\rm{Ga(135\,pm)}}\) is slightly smaller than that of \({\rm{Al(143\,pm)}}\)
2.Ionisationsenthalpien:
The first ionization enthalpies \(\left( {{{\rm{\Delta }}_{\rm{i}}}{{\rm{H}}_{\rm{1}}}} \right) \ ) of the element group \(13\) are lower than those of the element group \(2\), i.e. the alkaline earth metals. The downward movement of the \(13\) group from B to Al leads to a strong decrease in the enthalpy of the first ionization \(\left( {{{\rm{\Delta }}_{\rm{i}}}{ { \rm {H}}_{\rm{1}}}} \right)\) of Al due to an increase in atomic size and shielding effect (from \({\rm{2s}}}\) and \( {\ rm {2p}}\) electrons), which offsets the effect of the increased nuclear charge. However, the \(\left( {{{\rm{\Delta }}_{\rm{i}}}{{\rm{H}}_{\rm{1}}}} \right)\ ) of Ga is only slightly higher \(\left( {{\rm{2\;kJ\;mo}}{{\rm{l}}^{{\rm{ – 1}}}}} \ right)\ ) than that of Al, while that of Tl is much higher than that of Al, Ga, and In.
3.electronegativity
Elements of the boron family (group \(13)\) are more electronegative than the alkali metals (group \(1)\) and alkaline earth metals (group \(2).\) The electronegativity decreases from B to Al and then increases just behind the Group.
4.Electropositive character-metallic character
The group \(13\) elements are less electropositive or metallic than the alkali metals (group \(1)\) and the alkaline earth metals (group \(2).\) The electropositive character of the elements increases from boron to aluminum and increases then from aluminum to thallium as you go down the group.
5.density
Group \(13\) elements have higher densities than group \(2\) elements due to smaller atomic and ionic radii. The densities increase as you go down the group. This is due to an increase in the atomic mass of the elements, which offsets the effect of increasing atomic size. However, the boron and aluminum densities are much lower than those of the other members.
6.melting and boiling points
The melting points of the \(13\) elements do not follow a regular pattern, as do those of the \(1\) and \(2\) elements. This is most likely due to the peculiar crystal structures of B and Ga. As you go down the group from B to Ga, the melting points actually fall sharply and then rise from Ga to Tl. Therefore, Ga has the lowest melting point \((303 \mathrm{~ K})\) of the elements of group \(13\) and can exist as a liquid at room temperature in summer.
Chemical Properties of the Boron Family (Group 13 Elements)
1.oxidation state: The elements of the group \(13\) have two electrons in the s orbital and one electron in the p orbital. As a result, these elements should have a uniform oxidation state of \(+3.\). This is true for boron and aluminum, which have an oxidation state of \(+3,\), but gallium, indium, and thallium have oxidation. States of \(+1\) and \(+3\) due to the inert pair effect.
2.reduce nature:The first element, boron, is not a reducing agent as it does not tend to donate valence electrons. A reducing agent is aluminum. As the hydration energy released compensates for the ionization energy required to lose electrons in an aqueous solution. In general, the reducing character reduces the group in the order \(\mathrm{Al}>\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}\)
3.hydride formation: Group \(13\) elements (boron family) do not combine directly with hydrogen to form hydrides. However, some of the hydrides of these elements have been produced indirectly.
4.halide formation: The elements of group \(13\) react with halogens at high temperatures to form trihalides of the general formula \(\mathrm{MX}_{3}\) thallium(III) iodide \(\left( {{ \ rm{ However, Tl}}{{\rm{l}}_{\rm{3}}}} \right)\) is unknown.
\(2{\rm{M(s) + 3}}{{\rm{X}}_{\rm{2}}}{\rm{(g)}}\mahop \a \límites^{{ \rm{ Calor }}} 2{\rm{M}}{{\rm{X}}_3}({\rm{X}} = {\rm{F}},{\rm{Cl}}, {\rm{Br}},{\rm{I}})\)
5.Oxide formation (reactivity to air): All metals of group \(13\) react with dioxygen at high temperatures to form trioxides of the formula \({{\rm{M}}_2}{{\rm{O}}_3}\)
6.hydroxide formation: Hydroxide, \({\rm{M}}{({\rm{OH}})_3}\) is formed by dissolving metal oxides, \({{\rm{M}}}_2}{{\ rm { O }}_3}\), in water.
\(\mahop {{{\rm{M}}_2}{{\rm{O}}_3}}\limits_{{\rm{Metal}}\,\,{\rm{óxido}}} + 3 {{\rm{H}}_2}{\rm{O}} \to \mahop {2{\rm{M}}{{({\rm{OH}})}_3}}\limits_{{\ rm{Metall}}\,\,{\rm{hidróxido}}} \)
Hydroxides behave similarly to oxides, i.e. \({\rm{B}}{({\rm{OH}})_3}\) or boric acid is a typical acid, \({ \rm { Al}}{({ \rm{OH}})_3}\) and \({\rm{Ga}}{({\rm{OH}})_3}\) are both amphoteric, while \ (\ln { ({\rm{ OH}})_3}\) and \({\rm{Tl}}}{({\rm{OH}})_3}\) are basic in nature.
7.Reactivity to acids and alkalis:
A.The Effect of Acids: Boron does not react with non-oxidizing acids such as hydrochloric acid. However, high temperatures are caused by strong oxidizing acids, e.g. B. a hot concentrated mixture. \({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\) and \({\rm{HN}}{{\rm{O}}_3 }(2:1)\) formation of boric acid \(\left( {{{\rm{H}}_3}{\rm{B}}{{\rm{O}}_3}} \right)\)
All other elements react with oxidizing and non-oxidizing acids. For example, aluminum reacts with dilute hydrochloric acid to release hydrogen gas.
\({\rm{2Al(s) + 6HCl(ac)}} \to {\rm{2A}}{{\rm{l}}^{{\rm{3 + }}}}}{\rm{ (ac) + 6C}}{{\rm{l}}^{\rm{ – }}}{\rm{(ac) + 3}}{{\rm{H}}_{\rm{2} }}{\rm{(g)}}\)
B.The action of alkalis: Boron is resistant to the action of alkalis \({\rm{(NaOH \;o\;KOH)}}\) up to \({\rm{773\,K}}}\), but above this temperature it is reacts, forming borates and releasing dihydrogen gas.
Summary
The group \(13\) represents the boron family, and the elements have a \({\rm{n}}{{\rm{s}}^{\rm{2}}}{\rm{n }} { {\rm{p}}^{\rm{1}}}\) configuration. Contains boron \(\left( {\rm{B}} \right)\) aluminum \(\left( {{\rm{Al}}} \right)\) gallium \(\left( {{\rm { Ga}}} \right)\), indium \(\left( {{\rm{In}}} \right)\) thallium \(\left( {{\rm{Tl}}} \right)\ ) and the newly discovered element Ununtrium \(\left( {{\rm{uut}}} \right)\), which is radioactive. The atomic and ionic radii of the group \(13\) elements are smaller than those of the group \(2\). The elements of the boron family (group \(13)\) are more electronegative than the group I and group II elements.
Frequently asked questions about group 13 elements
Frequently asked questions about Group 13 elements are answered here:
Q.1. What are the elements of group 13: the boron family?
Answer:The group \(13\) represents the boron family. The elements of the group \(13\) are boron \(\left( {\rm{B}} \right)\) aluminum \(\left( {{\rm{Al}}} \right)\), gallium \ (\left( {{\rm{Ga}}} \right)\), indium \(\left( {{\rm{In}}} \right)\), thallium \(\left( {{\ rm {Tl}}} \right)\) and the newly discovered element Ununtrium \(\left( {{\rm{uut}}} \right)\)
P.2. Why is group 13 called the boron family?
Answer:The group \(13\) is called the boron family because boron is the first element in this group. This group of elements is known as icosages or triels. All elements of this family have almost the same chemical properties.
P.3. Why are Group 13 elements called Icosages?
Answer:Due to the icosahedral structures formed by these elements, elements of group \(13\) are also known as icosagens.
P.4. What are Group 13 elements?
Answer:The elements of the group \(13\) are the following:
| Element |
| Boro \(\left( {\rm{B}} \right)\) |
| Aluminium \(\left( {{\rm{Al}}} \right)\) |
| Galio \(\left( {{\rm{Ga}}} \right)\) |
| Indio \(\left( {{\rm{In}}} \right)\) |
| Talio \(\left( {{\rm{Tl}}} \right)\) |
P.5. What Are the Physical Properties of Group 13 Elements?
Answer:The physical properties of the elements of group \(13\) are as follows:
I.atomic and ionic radii: The atomic and ionic radii of the elements of the group \(13\) are smaller than those of the elements of the group \(2\).
ii.density: Group \(13\) elements have higher densities than group \(2\) elements due to smaller atomic and ionic radii.
iii.melting and boiling points: The melting points of the elements in group \(13\) do not follow a regular pattern, as is the case for elements in groups \(1\) and \(2\).
IV.Electropositive character-metallic character: The elements of group \(13\) are less electropositive or metallic than the alkali metals (group \(1)\) and the alkaline earth metals (group \(2).\)
v.electronegativity: The elements of the boron family (group \(13)\) are more electronegative than those of the alkali metals (group \(1)\) and alkaline earth metals (group \(2).\)
We hope this article on Group 13 Elements, Boro Family has been useful to you. If you have any questions, please leave a comment below and we will get back to you.