In chemistry, a nonmetal or non-metal is a chemical element that mostly lacks metallic
attributes.
Physically, nonmetals tend to be highly volatile, have low elasticity, and are good insulators
of heat and electricity; chemically, they tend to have high ionisation energy and electronegativity
values, and gain or share electrons when they react with other elements or compounds.
Seventeen elements are generally classified as nonmetals; most are gases; one is a liquid;
and a few are solids.
Moving rightward across the standard form of periodic table, nonmetals adopt structures
that have progressively fewer nearest neighbours.
Polyatomic nonmetals have structures with either three nearest neighbours, as is the
case with carbon, or two nearest neighbours in the case of sulfur.
Diatomic metals, such as hydrogen, have one nearest neighbour, and the monatomic noble
gases, such as helium, have none.
This gradual fall in the number of nearest neighbours is associated with a reduction
in metallic character and an increase in nonmetallic character.
The distinction between the three categories of nonmetals, in terms of receding metallicity
is not absolute.
Boundary overlaps occur as outlying elements in each category show less-distinct, hybrid-like
or atypical properties.
Although five times more elements are metals than nonmetals, two of the nonmetals—hydrogen
and helium—make up over 99 per cent of the observable Universe, and one—oxygen—makes
up close to half of the Earth's crust, oceans and atmosphere.
Living organisms are also composed almost entirely of nonmetals, and nonmetals form
many more compounds than metals.
Definition and properties
There is no rigorous definition of a nonmetal.
They show more variability in their properties than do metals.
The following are some of the chief characteristics of nonmetals.
Physically, they largely exist as monatomic gases, with a few having more substantial
diatomic or polyatomic forms, unlike metals which are nearly all solid and close-packed;
if solid, they generally have a submetallic or dull appearance and are brittle, as opposed
to metals, which are lustrous, ductile or malleable; they usually have lower densities
than metals; are poor conductors of heat and electricity when compared to metals; and have
significantly lower melting points and boiling points than those of metals.
Chemically, the nonmetals have relatively high ionisation energy and high electronegativity;
they usually exist as anions or oxyanions in aqueous solution; generally form ionic
or interstitial compounds when mixed with metals, unlike metals which form alloys; and
have acidic oxides whereas the common oxides of the metals are basic.
Applicable elements
The elements generally classified as nonmetals comprise one element each in group 1 and group
14: hydrogen and carbon; two elements in group 15: nitrogen and phosphorus; three elements
in group 16: oxygen, sulfur and selenium; most elements in group 17: fluorine, chlorine,
bromine and iodine; and all elements in group 18, with the possible exception of ununoctium.
The distinction between nonmetals and metals is by no means clear.
The result is that a few borderline elements lacking a preponderance of either nonmetallic
or metallic properties are classified as metalloids; and some elements classified as nonmetals
are instead sometimes classified as metalloids, or vice versa.
For example, selenium, a nonmetal, is sometimes classified instead as a metalloid, particularly
in environmental chemistry; and astatine, which is a metalloid and a halogen, is sometimes
classified instead as a nonmetal.
Categories
Nonmetals have structures in which each atom usually forms bonds with nearest neighbours,
where N is the number of valence electrons.
Each atom is thereby able to complete its valence shell and attain a stable noble gas
configuration.
Exceptions to the rule occur with hydrogen, carbon, nitrogen and oxygen.
Atoms of the latter three elements are sufficiently small such that they are able to form alternative
bonding structures, with fewer nearest neighbours.
Thus, carbon is able to form its layered graphite structure, and nitrogen and oxygen are able
to form diatomic molecules having triple and double bonds, respectively.
The larger size of the remaining non-noble nonmetals weakens their capacity to form multiple
bonds and they instead form two or more single bonds to two or more different atoms.
Sulfur, for example, forms an eight-membered molecule in which the atoms are arranged in
a ring, with each atom forming two single bonds to different atoms.
From left to right across the standard form of periodic table, as metallic character decreases,
nonmetals therefore adopt structures that show a gradual reduction in the numbers of
nearest neighbours—three or two for the polyatomic nonmetals, through one for the
diatomic nonmetals, to zero for the monatomic noble gases.
A similar pattern occurs more generally, at the level of the entire periodic table, in
comparing metals and nonmetals.
There is a transition from metallic bonding amongst the metals on the left of the table
through to covalent or Van der Waals bonding amongst the nonmetals on the right of the
table.
Metallic bonding tends to involve close-packed centrosymmetric structures with a high number
of nearest neighbours.
Other metals and metalloids, sandwiched between the true metals and the nonmetals, tend to
have more complex structures with an intermediate number of nearest neighbours.
Nonmetallic bonding, towards the right of the table, features open-packed directional
structures with fewer or zero nearest neighbours.
As noted, this steady reduction in the number of nearest neighbours, as metallic character
decreases and nonmetallic character increases, is mirrored among the nonmetals, the structures
of which gradually change from polyatomic, to diatomic, to monatomic.
As is the case with the major categories of metals, metalloids and nonmetals, there is
some variation and overlapping of properties within and across each category of nonmetal.
Among the polyatomic nonmetals, carbon, phosphorus and selenium—which border the metalloids—begin
to show some metallic character.
Sulfur, is the least metallic of the polyatomic nonmetals but even here shows some discernible
metal-like character.
Of the diatomic nonmetals, iodine is the most metallic.
Its number of nearest neighbours is sometimes described as 1+2 hence it is almost a polyatomic
nonmetal.
Within the iodine molecule, significant electronic interactions occur with the two next nearest
neighbours of each atom, and these interactions give rise, in bulk iodine, to a shiny appearance
and semiconducting properties.
Of the monatomic nometals, radon is the most metallic and begins to show some cationic
behaviour, which is unusual for a nonmetal.
Polyatomic nonmetals
Four nonmetals are distinguished by polyatomic bonding in their standard states, in either
discrete or extended molecular forms: carbon; phosphorus; sulfur; and selenium.
Consistent with their higher coordination numbers, the polyatomic nonmetals show more
metallic character than the neighbouring diatomic nonmetals; they are all solid, mostly semi-lustrous
semiconductors with electronegativity values that are intermediate to moderately high.
Sulfur is the least metallic of the polyatomic nonmetals given its dull appearance, brittle
comportment, and low conductivity—attributes common to all sulfur allotropes.
It nevertheless shows some metallic character, either intrinsically or in its compounds with
other nonmetals.
Examples include the malleability of plastic sulfur and the lustrous-bronze appearance
and metallic conductivity of polysulfur nitride.
The polyatomic nonmetals are distinguished from the diatomic nonmetals by virtue of having
higher coordination numbers, higher melting points, and higher boiling points; and having
wider liquid ranges and lower room temperature volatility.
More generally they show a marked tendency to exist in allotropic forms, and a stronger
inclination to catenate; and have a weaker ability to form hydrogen bonds.
The ability of carbon to catenate, in particular, is fundamental to the field of organic chemistry
and life on Earth.
All of the polyatomic nonmetals are solids, and all are known in either malleable, pliable
or ductile forms; most also have lower ionisation energies and electronegativities than those
of the diatomic nonmetals.
Diatomic nonmetals
Seven nonmetals exist as diatomic molecules in their standard states: hydrogen; nitrogen;
oxygen; fluorine; chlorine; bromine; and iodine.
They are generally highly insulating, highly electronegative, non-reflective gases, noting
that bromine, a liquid, and iodine, a solid, are both volatile at room temperature.
Exceptions to this generalised description occur at the boundaries of the category: hydrogen
has a comparatively low electronegativity due to its unique atomic structure; iodine,
in crystalline form, is semi-lustrous, and a semiconductor in the direction of its layers,
both of these attributes being consistent with incipient metallic character.
The diatomic nonmetals are distinguished from the polyatomic nonmetals by virtue of having
lower coordination numbers, lower melting points, and lower boiling points; and having
narrower liquid ranges and greater room temperature volatility.
More generally, they show less inclination to exist in allotropic forms, and to catenate;
and have a stronger ability to form hydrogen bonds.
Most are also gases, and have higher ionisation energies and higher electronegativities than
those of the polyatomic nonmetals.
Noble gases
Six nonmetals occur naturally as monatomic noble gases: helium, neon, argon, krypton,
xenon, and the radioactive radon.
They comprise a group of chemical elements with very similar properties.
In their standard states they are all colorless, odourless, nonflammable gases with characteristically
very low chemical reactivity.
With their closed valence shells, the noble gases have the highest first ionization potentials
in each of their periods, and feeble interatomic forces of attraction, with the latter property
resulting in very low melting and boiling points.
That is why they are all gases under standard conditions, even those with atomic masses
larger than many normally solid elements.
The status of the period 7 congener of the noble gases, element 118 is not known—it
may or may not be a noble gas.
It was originally predicted to be a noble gas but may instead be a fairly reactive solid
with an anomalously low first ionisation potential, due to relativistic effects.
On the other hand, if relativistic effects peak in period 7 at element 112, element 118
may turn out to be a noble gas after all albeit more reactive than either xenon or radon.
Elemental gases Hydrogen, nitrogen, oxygen, fluorine, chlorine,
plus the noble gases are collectively referred to as the elemental gases.
They are distinguished by having the lowest densities, lowest melting and boiling points,
strongest insulating properties, and highest electronegativity and ionization energy values
in the periodic table.
It is not scientifically proven if any synthetic elements with atomic number above 108 are
gases.
If it transpires that copernicium and flerovium are gaseous metals at or near room temperature,
as some calculations have suggested, the category of elemental gases may need to be sub-divided
into nonmetallic gases and metallic gases.
Comparison of properties Characteristic and other properties of polyatomic
nonmetals, diatomic nonmetals, and the monatomic noble gases are summarized in the following
table.
Physical properties are listed in loose order of ease of determination; chemical properties
run from general to specific, and then to descriptive.
Allotropes
Many nonmetals have less stable allotropes, with either nonmetallic or metallic properties.
Graphite, the standard state of carbon, has a lustrous appearance and is a fairly good
electrical conductor.
The diamond allotrope of carbon is clearly nonmetallic however, being translucent and
having a relatively poor electrical conductivity.
Carbon is also known in several other allotropic forms, including semiconducting buckminsterfullerene.
Nitrogen can form gaseous tetranitrogen, an unstable polyatomic molecule with a lifetime
of about one microsecond.
Oxygen is a diatomic molecule in its standard state; it also exists as ozone, an unstable
polyatomic nonmetallic allotrope with a half-life of around half an hour.
Phosphorus, uniquely, exists in several allotropic forms that are more stable than that of its
standard state as white phosphorus.
The red and black allotropes are probably the best known; both are semiconductors; black
phosphorus, in addition, has a lustrous appearance.
Phosphorus is also known as diphosphorus, an unstable diatomic allotrope.
Sulfur has more allotropes than any other element; all of these, bar plastic sulfur
which is malleable, have nonmetallic properties.
Selenium has several nonmetallic allotropes, all of which are much less electrically conducting
than its standard state of grey 'metallic' selenium.
Iodine is also known in a semiconducting amorphous form.
Under sufficiently high pressures, just over half of the nonmetals, starting with phosphorus
at 1.7 GPa, have been observed to form metallic allotropes.
Abundance and extraction
Hydrogen and helium are estimated to make up approximately 99 per cent of all ordinary
matter in the universe.
Less than five per cent of the Universe is believed to be made of ordinary matter, represented
by stars, planets and living beings.
The balance is made of dark energy and dark matter, both of which are poorly understood
at present.
Hydrogen, carbon, nitrogen, oxygen and constitute the great bulk of the Earth's atmosphere,
oceans, crust, and biosphere; the remaining nonmetals have abundances of 0.5 per cent
or less.
In comparison, 35 per cent of the crust is made up of the metals sodium, magnesium, aluminium,
potassium and iron; together with a metalloid, silicon.
All other metals and metalloids have abundances within the crust, oceans or biosphere of 0.2
per cent or less.
Nonmetals, in their elemental forms, are extracted from: brine: Cl, Br, I; liquid air: N, O,
Ne, Ar, Kr, Xe; minerals: C; F; P; I; natural gas: H, He, S; and from ores, as processing
byproducts: Se; and Rn.
Applications in common For prevalent and speciality applications
of individual nonmetals see the main article for each element.
Nonmetals do not have any universal or near-universal applications.
This is not the case with metals, most of which have structural uses; nor the metalloids,
the typical uses of which extend to oxide glasses, alloying components, and semiconductors.
Shared applications of different subsets of the nonmetals instead encompass their presence
in, or specific uses in the fields of: cryogenics and refrigerants: H, He, N, O, F and Ne; fertilisers:
H, N, P, S, Cl and Se; household accoutrements: H, He, C, N, O, F, Ne, P, S, Cl, Ar, Se, Br,
Kr, I, Xe and Rn; industrial acids: C, N, F, P, S and Cl; inert air replacements: N,
Ne, S, Ar, Kr and Xe; lasers and lighting: He, C, N, O, F, Ne, S, Ar, Kr and Xe; and
medicine and pharmaceuticals: He, O, F, Cl, Br, I, Xe and Rn.
The number of compounds formed by nonmetals is vast.
The first nine places in a "top 20" table of elements most frequently encountered in
8,427,300 compounds, as listed in the Chemical Abstracts Service register for July 1987,
were occupied by nonmetals.
Hydrogen, carbon, oxygen and nitrogen were found in the majority of compounds.
The highest rated metal, with an occurrence frequency of 2.3 per cent, was iron, in 11th
place.
Notes
Citations
References
Monographs Emsley J 1971, The inorganic chemistry of
the non-metals, Methuen Educational, London, ISBN 0423861204
Johnson RC 1966, Introductory descriptive chemistry: selected nonmetals, their properties,
and behavior, WA Benjamin, New York Jolly WL 1966, The chemistry of the non-metals,
Prentice-Hall, Englewood Cliffs, New Jersey Powell P & Timms PL 1974, The chemistry of
the non-metals, Chapman & Hall, London, ISBN 0470695706
Sherwin E & Weston GJ 1966, Chemistry of the non-metallic elements, Pergamon Press, Oxford
Steudel R 1977, Chemistry of the non-metals: with an introduction to atomic structure and
chemical bonding, English edition by FC Nachod & JJ Zuckerman, Berlin, Walter de Gruyter,
ISBN 3110048825