Boron Number Of Electrons

Article
• General properties of the group
• Compounds of the boron group elements

Because boron and nitrogen together contain the same number of valence electrons (eight) as two bonded carbon atoms, boron nitride is said to be isoelectronic with elemental carbon. Boron nitride exists in two structural forms, which are analogous to two forms of carbon—graphite. To discover the amount of protons and neutrons in boron-11, one must look at its atomic number and atomic mass. Boron-11's atomic number is five, which means it always has five protons. To discover how many electrons boron-11 has, one should subtract the amount of known protons from its atomic mass of 11. It is not a very difficult task to remember the valence electrons as the Valency is decided by the number of electrons that are there in the outer shell. There are certain shells, namely, K, L, M, and N. On the basis of these shells the electrons are distributed accordingly. Boron Number of Valence Electrons.

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Boron Number Of Electron Shells

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Boron has 3 valence electrons. The number of valence electrons within an atom of an element simply corresponds to an element's group (column) on the. The fluorine that shares a double bond with boron has six electrons around it (four from its two lone pairs of electrons and one each from its two bonds with boron). This is one less electron than the number of valence electrons it would have naturally (Group Seven elements have seven valence electrons), so it has a formal charge of +1.

Alan Gibbs MasseySee All Contributors
Reader in Inorganic Chemistry, Loughborough University of Technology, England. Coauthor of Inorganic Chemistry in Non-aqueous Solvents.
Alternative Titles: Group 13 element, Group IIIa element, aluminum group element

Boron group element, any of the six chemical elementsconstituting Group 13 (IIIa) of the periodic table. The elements are boron (B), aluminum (Al), gallium (Ga), indium (In), thallium (Tl), and nihonium (Nh). They are characterized as a group by having three electrons in the outermost parts of their atomic structure. Boron, the lightest of these elements, is a metalloid. Aluminum, gallium, indium, and thallium are silvery white metals. Nihonium has only been produced as individual atoms in particle accelerators.

Periodic Table of the Elements
Test your bond with the periodic table of elements in this quiz on all 118 chemical elements and their symbols. You may be familiar with the chemical symbols for hydrogen and oxygen, but can you match such lower-profile elements as gadolinium and erbium with their corresponding symbols?

None of these elements was known in a pure state before modern chemistry isolated them. Very soon after a method had been found to produce it in commercial quantities, aluminum revolutionized industry. With further development of science and technology, specifically in nanotechnology, boron gained significant attention in industrial sectors as well. The other members of the group still have little commercial value. Some of the compounds of boron and aluminum, however, are indispensable in modern technology and have been widely used in many parts of the world throughout recorded history.

History

The use of a boron compound known as borax (sodium tetraborate, Na2B4O7∙10H2O) can be traced back to the ancient Egyptians, who used it as a metallurgical flux (a substance that aids the heat joining or soldering of metals), in medicine, and in mummification. During the 13th century Marco Polo introduced borax into Europe, but not until the mid-19th century, when vast deposits of borates were discovered in the Mojave Desert, did borax become relatively common. The ancient Egyptians, Greeks, and Romans used a compound of aluminum known as alum (the compound potassium aluminum sulfate) in dyeing as a mordant—i.e., a substance that fixes dye molecules to the fabric. Lapis lazuli, a rare dark blue mineral (the compound sodium aluminum silicate containing sulfur), has been widely used as a semiprecious stone throughout history. The metal aluminum was first isolated early in the 19th century, but it was not until a modern electrolytic process based on the use of bauxite ore had been developed that commercial production of aluminum became economically feasible. Three other boron group elements—gallium, indium, and thallium—were first detected spectroscopically (i.e., by analysis of the light emitted by or passed through substances containing the element) in the late 19th century. The existence and properties of gallium were predicted by a Russian chemist, Dmitry Ivanovich Mendeleyev, on the basis of the periodic table of the elements that he had developed; the ultimate discovery of gallium and the accuracy of his description of the properties of the then unknown element convinced scientists of the theoretical soundness of the table. Gallium is one of two metals (the other is cesium) whose melting points are low enough for them to turn to liquid when held in the hand. Nihonium was artificially produced in a particle accelerator in 2004.

Ionization energies

Every element in the boron group has three electrons in its outermost shell (so-called valence electrons), and for each element there is a sharp jump in the amount of energy required to remove the fourth electron, reflecting the fact that this electron must be removed from an inner shell. Consequently, the elements of the group have maximum oxidation numbers of three, corresponding to loss of the first three electrons, and form ions with three positive charges.

The apparently erratic way in which ionization energies vary among the elements of the group is due to the presence of the filled inner d orbitals in gallium, indium, and thallium, and the f orbital in thallium, which do not shield the outermost electrons from the pull of the nuclear charge as efficiently as do the inner s and p electrons. In Groups 1 and 2 (Ia and IIa), in contrast to the boron group, outer shell (always referred to as n) electrons are shielded in every case by a constant inner set of electrons, in the (n-1)s2(n-1)p6 orbitals, and the ionization energies of these Group-1 and Group-2 elements decrease smoothly down the group. The ionization energies of gallium, indium, and thallium are thus higher than expected from their Group 2 counterparts because their outer electrons, being poorly shielded by the inner d and f electrons, are more strongly bound to the nucleus. This shielding effect also makes the atoms of gallium, indium, and thallium smaller than the atoms of their Group 1 and 2 neighbours by causing the outer electrons to be pulled closer toward the nucleus.

The M3+ state for gallium, indium, and thallium is energetically less favourable than Al3+ because the high ionization energies of these three elements cannot always be balanced by the crystal energies of possible reaction products. For example, of the simple, anhydrous compounds of thallium in its +3 oxidation state, only the trifluoride, TlF3, is ionic. For the group as a whole, therefore, the M3+ ionic state is the exception rather than the rule. More commonly the elements of the group form covalent bonds and achieve an oxidation state of three by promoting one electron from the s orbital in the outer shell (designated ns orbital) to an np orbital, the shift permitting the formation of hybrid, or combination, orbitals (of the variety designated as sp2). Increasingly down the group there is a tendency toward the formation of M+ ions, and at thallium the +1 oxidation state is the more stable one. The basicity (a property of metals) of the elements also increases in proceeding down the group, as shown by the oxides they form: boric oxide (formula B2O3) is acidic; the next three oxides, of aluminum, gallium, and indium (formulas Al2O3, Ga2O3, and In2O3) are either acidic or basic depending on the environment (a property called amphoterism); and thallic oxide (Tl2O3) is wholly basic.

Quick Facts
related topics

How many electrons does boron have?

Boron atomic number 5 has five electrons in its ground state.
Commonly Boron will lose 3 electrons leaving 2 electrons in its most common ionic form.

Explanation:

The atomic number gives the number of protons. Protons which have a positive charge are balanced by an equal number of electrons in a neutral atom.

Boron number 5 has five protons and therefore as a neutral atom also has five electrons.

Boron has an electron configuration of $1 {s}^{2} 2 {s}^{2} 2 {p}^{1}$

The most stable electron configuration for Boron is

$1 {s}^{2}$ + 3 charge. By losing three electrons Boron can achieve the stable electron structure of Helium

Explanation:

Boron is element number 5 in the Periodic Table.

That means it contains five protons and five electrons.

Boron Number Of Electrons Gained Or Lost

They are arranged with two electrons in the first energy shell and three in the second.

Valence Electrons In Boron

A chemist would say that the electron configuration of boron is

$' 1 s {'}^{2} ' 2 s {'}^{2} ' 2 p '$