Solid nitrogen

Solid nitrogen on the plains of Sputnik Planitia on Pluto next to water ice mountains.

Solid nitrogen is a number of solid forms of the element nitrogen, first observed in 1884. Solid nitrogen is mainly the subject of academic research, but low-temperature, low-pressure solid nitrogen is a substantial component of bodies in the outer Solar System and high-temperature, high-pressure solid nitrogen is a powerful explosive, with higher energy density than any other non-nuclear material.

Generation

Karol Olszewski first observed solid nitrogen in 1884, by first liquefying hydrogen with evaporating liquid nitrogen, and then allowing the liquid hydrogen to freeze the nitrogen. By evaporating vapour from the solid nitrogen, Olszewski also generated the extremely low temperature of Template:Val, at the time a world record.

Modern techniques usually take a similar approach: solid nitrogen is normally made in a laboratory by evaporating liquid nitrogen in a vacuum. The solid produced is porous.

Occurrence in nature

Solid nitrogen forms a large part of the surface of Pluto (where it mixes with solid carbon monoxide and methane) and the Neptunian moon Triton. On Pluto it was directly observed for the first time in July 2015 by the New Horizons space probe and on Triton it was directly observed by the Voyager 2 space probe in August 1989.

Much of the surface of Triton is covered in the hexagonal form of solid nitrogen (the β crystal phase), which can be seen as a bluish green band around the equator in this synthetic color photomosaic.

Even at the low temperatures of solid nitrogen it is fairly volatile and can sublime to form an atmosphere, or condense back into nitrogen frost. Compared to other materials, solid nitrogen loses cohesion at low pressures and flows in the form of glaciers when amassed. Yet its density is higher than that of water ice, so the forces of buoyancy will naturally transport blocks of water ice towards the surface. Indeed, New Horizons observed "floating" water ice atop nitrogen ice on the surface of Pluto.

On Triton, solid nitrogen takes the form of frost crystals and a transparent sheet layer of annealed nitrogen ice, often referred to as a "glaze". Eruptions of nitrogen gas were observed by Voyager 2 to spew from the subpolar regions around Triton's southern polar ice cap. A possible explanation of this observed phenomenon is that the Sun shines through the transparent layer of nitrogen ice, heating the layers beneath. Nitrogen sublimes and eventually erupts through holes in the upper layer, carrying dust along with it and creating dark streaks.

Transitions to fluid allotropes

Melting

At standard atmospheric pressure, the melting point of N₂ is Template:Val.

Like most substances, nitrogen melts at a higher temperature with increasing ambient pressure until Template:Val, when liquid nitrogen is predicted to polymerize. Within that region, melting point increases at a rate of approximately Template:Val. Above Template:Val, the melting point drops.

Observed melting points of Template:Chem2

Pressure (GPa)	Temperature (K)
2.8	308
4	368
7	484
50	1920
71	1400

Sublimation

Nitrogen has a triple point at Template:Val and Template:Val; below this pressure, solid nitrogen sublimes directly to gas. At these low pressures, nitrogen exists in only two known allotropes: α-nitrogen (below Template:Val) and β-nitrogen (Template:Val). Measurements of the vapour pressure from Template:Val suggest the following empirical formulae:

$\ln \left(\frac{P_{\text{subl}}}{1\text{ bar}}\right)=12.40-\frac{807.4\text{ K}}{T}-\frac{3926{\text{ K}}^2}{T^2}+\frac{6.297\cdot 10^4{\text{ K}}^3}{T^3}-\frac{4.633\cdot 10^5{\text{ K}}^4}{T^4}+\frac{1.325\cdot 10^6{\text{ K}}^5}{T^5}(\alpha )$$\ln \left(\frac{P_{\text{subl}}}{1\text{ bar}}\right)=8.514-\frac{458.4\text{ K}}{T}-\frac{19870{\text{ K}}^2}{T^2}+\frac{4.800\cdot 10^5{\text{ K}}^3}{T^3}-\frac{4.524\cdot 10^6{\text{ K}}^4}{T^4}(\beta )$

Solubility in common cryogens

Solid nitrogen is slightly soluble in liquid hydrogen. Based on solubility in Template:Val gaseous hydrogen, Seidal et al. estimated that liquid hydrogen at Template:Val can dissolve Template:Val. At the boiling point of hydrogen with excess solid nitrogen, the dissolved molar fraction is 10⁻⁸. At Template:Val (just below the boiling point of Template:Chem2) and Template:Val, the maximum molar concentration of dissolved N₂ is Template:Val. Nitrogen and oxygen are miscible in liquid phase but separate in solid phase. Thus excess nitrogen (melting at 63 K) or oxygen (melting at 55 K) freeze out first, and the eutectic liquid air freezes at 50 K.

Crystal structure

Dinitrogen crystals

At ambient and moderate pressures, nitrogen forms [[dinitrogen|Template:Chem2]] molecules; at low temperature London dispersion forces suffice to solidify these molecules.

α and β

Solid nitrogen admits two phases at ambient pressure: α- and β-nitrogen.

Below Template:Val, nitrogen adopts a cubic structure with space group Pa3; the Template:Chem2 molecules are located on the body diagonals of the unit cell cube. At low temperatures the α-phase can be compressed to Template:Val before it changes (to γ), and as the temperature rises above Template:Val, this pressure rises to about Template:Val. At Template:Val, the unit cell dimension is Template:Val, decreasing to Template:Val under Template:Val.

Above Template:Val (until it melts), nitrogen adopts a hexagonal close packed structure, with unit cell ratio Template:Math. The nitrogen molecules are randomly tipped at an angle of Template:Val, due to strong quadrupole-quadrupole interaction. At Template:Val the unit cell has Template:Math and Template:Math, but these shrink at Template:Val and Template:Val to Template:Math and Template:Math. At higher pressures, the Template:Math displays practically no variation.

γ

The tetragonal γ form exists at low temperatures below Template:Val and pressures around Template:Val. The α/β/γ₂ triple point occurs at Template:Val and Template:Val. Formation of γ-dinitrogen exhibits a substantial isotope effect: at Template:Val, the isotope ¹⁵N converts to the γ form at a pressure Template:Cvt lower than natural nitrogen.

The space group of the γ phase is P4₂/mnm. At Template:Val and Template:Val, the unit cell has lattice constants Template:Math and Template:Math.

The nitrogen molecules themselves are arranged in P4₂/mnm pattern f and take the shape of a prolate spheroid with long dimension Template:Val and diameter Template:Val. The molecules can vibrate up to Template:Value on the Template:Math plane, and up to Template:Value in the direction of the Template:Mvar axis.

δ, δ_loc, and ε

At high pressure (but ambient temperature), dinitrogen adopts the cubic δ form, with space group pm3n and eight molecules per unit cell. This phase admits a lattice constant of Template:Value (at Template:Val and Template:Value). δ-Template:Chem2 admits two triple points. The (δ-Template:Chem2, β-Template:Chem2, liquid) triple point occurs somewhere around Template:Val and Template:Val. The (δ-Template:Chem2, β-Template:Chem2, γ-Template:Chem2) triple point occurs at Template:Val and Template:Val.

Within the lattice cells, the molecules themselves have disordered orientation, but increases in pressure causes a phase transition to a slightly different phase, δ_loc, in which the molecular orientations progressively order, a distinction that is only visible via Raman spectroscopy. At high pressure (roughly Template:Val) and low temperature,Template:Refn the dinitrogen molecule orientations fully order into the rhombohedral ε phase, which follows space group RTemplate:Overlinec. Cell dimensions are Template:Math, Template:Math, Template:Math, Template:Math, Template:Math, volume Template:Val, Template:Math.

Dissolved Template:Chem2 can stabilize ε-Template:Chem2 at higher temperatures or lower pressures from transforming into δ-Template:Chem2 (see Template:Slink).

ζ

Above Template:Val, ε-Template:Chem2 transforms to an orthorhombic phase designated by ζ-Template:Chem2. There is no measurable discontinuity in the volume per molecule between ε-Template:Chem2 and ζ-Template:Chem2. The structure of ζ-Template:Chem2 is very similar to that of ε-Template:Chem2, with only small differences in the orientation of the molecules. ζ-Template:Chem2 adopts the monoclinic space group C2/c, and has lattice constants of Template:Math, Template:Math, Template:Math and Template:Math with sixteen molecules per unit cell.

θ and ι

Further compression and heating produces two crystalline phases of nitrogen with surprising metastability.

A ζ-Template:Chem2 phase compressed to Template:Val and then heated to over Template:Val produces a uniformly translucent structure called θ-nitrogen.

The ι phase can be accessed by isobarically heating ε-Template:Chem2 to Template:Val at Template:Val or isothermal decompression of θ-Template:Chem2 to Template:Val at Template:Val. The ι-Template:Chem2 crystal structure is characterised by primitive monoclinic lattice with unit-cell dimensions of: Template:Math, Template:Math, Template:Math and Template:Math at Template:Val and ambient temperature. The space group is P2₁/c and the unit cell contains 48 Template:Chem2 molecules arranged into a layered structure.

Upon pressure release, θ-Template:Chem2 does not return to ε-Template:Chem2 until around Template:Val; ι-Template:Chem2 transforms to ε-Template:Chem2 until around Template:Val.

"Black phosphorus" nitrogen

When compressing nitrogen to pressures Template:Val and temperatures above Template:Val, nitrogen adopts a crystal structure ("bp-N") identical to that of black phosphorus (orthorhombic, Cmce space group). Like black phosphorus, bp-N is an electrical conductor. The existence of bp-N structure matches the behavior of heavier pnictogens, and reaffirms the trend that elements at high pressure adopt the same structures as heavier congeners at lower pressures.

Oligomer crystals

Hexagonal layered polymeric nitrogen

Hexagonal layered polymeric nitrogen (HLP-N) was experimentally synthesized at Template:Val and Template:Val. It adopts a tetragonal unit cell (P4₂bc) in which the single-bonded nitrogen atoms form two layers of interconnected Template:Chem2 hexagons. HPL-N is metastable to at least 66 GPa.

Linear forms (N₆ and N₈)

Linear N₈, EEE isomer (trans; EZE isomer – not shown – is cis) after Hirschberg et al. (2014)

The decomposition of hydrazinium azide at high pressure and low temperature produces a molecular solid made of linear chains of 8 nitrogen atoms (Template:Chem2). Simulations suggest that Template:Chem2 is stable at low temperatures and pressures (< 20 GPa); in practice, the reported Template:Chem2 decomposes to the ε allotrope below 25 GPa but a residue remains at pressure as low as 3 GPa.

Linear N₆ after Hirschberg et al. (2014)

Grechner et al. predicted in 2016 that an analogous allotrope with six nitrogens should exist at ambient conditions.

Amorphous and network allotropes

Non-molecular forms of solid nitrogen exhibit the highest known non-nuclear energy density.

μ

When the ζ-N₂ phase is compressed at room temperature over Template:Val an amorphous form is produced. This is a narrow gap semiconductor, and designated the μ-phase. The μ-phase has been brought to atmospheric pressure by first cooling it to Template:Val.

η

η-N is a semiconducting amorphous form of nitrogen. It forms at pressures around Template:Val and temperatures Template:Val. In reflected light it appears black, but does transmit some red or yellow light. In the infrared there is an absorption band around Template:Val. Under even higher pressure of approximately Template:Val, the band gap closes and η-nitrogen metallizes.

Cubic gauche

At pressures higher than Template:Val and temperatures around Template:Val, nitrogen forms a network solid, bound by covalent bonds in a cubic-gauche structure, abbreviated as cg-N. The cubic-gauche form has space group I2₁3. Each unit cell has edge length Template:Val, and contains eight nitrogen atoms. As a network, cg-N consists of fused rings of nitrogen atoms; at each atom, the bond angles are very close to tetrahedral. The position of the lone pairs of electrons is ranged so that their overlap is minimised.

The cubic-gauche structure for nitrogen is predicted to have bond lengths of 1.40 Å, bond angles of 114.0° and dihedral angles of −106.8°. The term gauche refers to the odd dihedral angles, if it were 0° it would be called cis, and if 180° it would be called trans. The dihedral angle Φ is related to the bond angle θ by sec(Φ) = sec(θ) − 1. The coordinate of one atom in the unit cell at x,x,x also determines the bond angle by cos(θ) = x(x-1/4)/(x²+(x-1/4)²).

All bonds in cg-N have the same length: Template:Val at Template:Val. This suggests that all bonds have the same order: a single bond carrying Template:Val. In contrast, the triple bond in gaseous nitrogen carries only Template:Val, so that relaxation to the gaseous form involves tremendous energy release: more than any other non-nuclear reaction. For this reason, cubic-gauche nitrogen is being investigated for use in explosives and rocket fuel. Estimates of its energy density vary: simulations predict Template:Val is predicted, which is Template:Val the energy density of HMX.

cg-N is also very stiff with a bulk modulus around Template:Val, similar to diamond.

Poly-N

Another network solid nitrogen called poly-N and abbreviated pN was predicted in 2006. pN has space group C2/c and cell dimensions a = 5.49 Å, β = 87.68°. Other higher pressure polymeric forms are predicted in theory, and a metallic form is expected if the pressure is high enough.

Others

Yet other phases of solid dinitrogen are termed ζ'-N₂ and κ-N₂.

Bulk properties

At Template:Val the ultimate compressive strength is 0.24 MPa. Strength increases as temperature lowers becoming 0.54 MPa at 40.6 K. Elastic modulus varies from 161 to 225 MPa over the same range.

The thermal conductivity of solid nitrogen is 0.7 W m⁻¹ K⁻¹. Thermal conductivity varies with temperature and the relation is given by k = 0.1802×T^0.1041  W m⁻¹ K⁻¹. Specific heat is given by 926.91×e^0.0093T joules per kilogram per kelvin. Its appearance at 50 K is transparent, while at 20 K it is white.

Nitrogen frost has a density of 0.85 g cm⁻³. As a bulk material the crystals are pressed together and density is near that of water. It is temperature dependent and given by ρ = 0.0134T² − 0.6981T + 1038.1 kg/m³. The volume coefficient of expansion is given by 2×10⁻⁶T² − 0.0002T + 0.006 K⁻¹.

The index of refraction at 6328 Å is 1.25 and hardly varies with temperature.

The speed of soundTemplate:Clarify in solid nitrogen is 1452 m/s at 20 K and 1222 m/s at 44 K. The longitudinal velocity ranges from 1850 m/s at 5 K to 1700 m/s at 35 K. With temperature rise the nitrogen changes phase and the longitudinal velocity drops rapidly over a small temperature range to below 1600 m/s and then it slowly drops to 1400 m/s near the melting point. The transverse velocity is much lower ranging from 900 to 800 m/s over the same temperature range.

The bulk modulus of s-N₂ is 2.16 GPa at 20 K, and 1.47 GPa at 44 K. At temperatures below 30 K solid nitrogen will undergo brittle failure, particularly if strain is applied quickly. Above this temperature the failure mode is ductile failure. Dropping 10 K makes the solid nitrogen 10 times as stiff.

Related substances

Under pressure nitrogen can form crystalline van der Waals compounds with other molecules. It can form an orthorhombic phase with methane above 5 GPa. With helium He(N₂)₁₁ is formed. N₂ crystallizes with water in nitrogen clathrate and in a mixture with oxygen O₂ and water in air clathrate.

Helium

Solid nitrogen can dissolve 2 mole % helium under pressure in its disordered phases such as the γ-phase. Under higher pressure 9 mol% helium, He can react with ε-nitrogen to form a hexagonal birefringent crystalline van der Waals compound. The unit cell contains 22 nitrogen atoms and 2 helium atoms. It has a volume of 580 Å³ for a pressure of 11 GPa decreasing to 515 Å³ at 14 GPa. It resembles the ε-phase. At 14.5 GPa and 295 K the unit cell has space group P6₃/m and a=7.936 Å c=9.360 Å. At 28 GPa a transition happens in which the orientation of N₂ molecules becomes more ordered. When the pressure on He(N₂)₁₁ exceeds 135 GPa the substance changes from clear to black, and takes on an amorphous form similar to η-N₂.

Methane

Solid nitrogen can crystallise with some solid methane included. At 55 K the molar percentage can range up to 16.35% CH₄, and at 40 K only 5%. In the complementary situation, solid methane can include some nitrogen in its crystals, up to 17.31% nitrogen. As the temperature drops, less methane can dissolve in solid nitrogen, and in α-N₂ there is a major drop in methane solubility. These mixtures are prevalent in outer Solar System objects such as Pluto that have both nitrogen and methane on their surfaces. At room temperature there is a clathrate of methane and nitrogen in 1:1 ratio formed at pressures over 5.6 GPa.

Carbon monoxide

The carbon monoxide molecule (CO) is very similar to dinitrogen in size, and it can mix in all proportions with solid nitrogen without changing crystal structure. Carbon monoxide is also found on the surfaces of Pluto and Triton at levels below 1%. Variations in the infrared linewidth of carbon monoxide absorption can reveal the concentration.

Noble gases

Neon or xenon atoms can also be included in solid nitrogen in the β and δ phases. Inclusion of neon pushes the β−δ phase boundary to higher pressures. Argon is also very miscible in solid nitrogen. For compositions of argon and nitrogen with 60% to 70% nitrogen, the hexagonal form remains stable to 0 K. A van der Waals compound of xenon and nitrogen exists above 5.3 GPa. A van der Waals compound of neon and nitrogen was shown using Raman spectroscopy. The compound has formula (N₂)₆Ne₇. It has a hexagonal structure, with a=14.400 c=8.0940 at a pressure of 8 GPa. A van der Waals compound with argon is not known.

Hydrogen

With dideuterium, a clathrate (N₂)₁₂D₂ exits around 70 GPa.

Oxygen

Solid nitrogen can take up to a one fifth substitution by oxygen O₂ and still keep the same crystal structure. δ-N₂ can be substituted by up to 95% O₂ and retain the same structure. Solid O₂ can only have a solid solution of 5% or less of N₂.

Use

Solid nitrogen is used in a slush mixture with liquid nitrogen in order to cool faster than with liquid nitrogen alone, useful for applications such as sperm cryopreservation. The semi-solid mixture can also be called slush nitrogen or SN2.

Solid nitrogen is used as a matrix on which to store and study reactive chemical species, such as free radicals or isolated atoms. One use is to study dinitrogen complexes of metals in isolation from other molecules.

Reactions

When solid nitrogen is irradiated by high speed protons or electrons, several reactive radicals are formed, including atomic nitrogen (N), nitrogen cations (N⁺), dinitrogen cation (N₂⁺), trinitrogen radicals (N₃ and N₃⁺), and azide (N₃⁻).Template:Clear

External links

• Template:Commons category-inline
• Jessica Orwig: Freezing Liquid Nitrogen Creates Something Amazing. On: BusinessInsider. Jan 28, 2015 - Videos of nitrogen boiling, freezing, and spontaneously changing crystal form.
• Xiaoli Wang, J. Li, N. Xu et al. (2015): Layered polymeric nitrogen in RbN₃ at high pressures. In: Scientific Reports volume 5, Article number: 16677. doi:10.1038/srep16677.