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Molecular nitrogen is ${\mathrm{N}}_2$, the dominant molecular component of ordinary dry air. Its strong triple bond makes it comparatively resistant to many reactions under ordinary conditions.

Converting it into more reactive nitrogen compounds requires a pathway that activates that bond, as in biological nitrogen fixation or industrial ammonia synthesis. The molecule is homonuclear and has no permanent electric dipole, so its ordinary pure rotational spectrum differs from that of a polar diatomic molecule.

Nitrogen is the chemical element with atomic number 7 and symbol $\mathrm{N}$. Its familiar elemental form is molecular nitrogen, ${\mathrm{N}}_2$, whose strong triple bond contributes to its low reactivity under many ordinary conditions. Nitrogen in ammonia, nitrate, and biological molecules occupies chemically different forms.^[ref]

Nitrogen–ammonia quenching occurs when transport preserves a nonequilibrium partition between molecular nitrogen and Ammonia. Their net conversion may be writtenbut its actual relaxation time depends on a multistep reaction network. Near a chemical quench level, that time exceeds the eddy mixing time, so the abundance can retain a deeper value instead of following local thermochemical equilibrium.

Coupled diffusion and chemistry models illustrate ammonia enhancement by transport and destruction at high altitudes by atmospheric photochemistry.^[ref] Interpreting an ammonia feature therefore requires an atmospheric pressure-temperature profile and a transport model, not only a molecular identification.

A molecular nitrogen experiment used a $0.5\mathrm{mm}$ pulsed nozzle and two skimmers. A $5\mathrm{cm}$ tube raised the rotational temperature. Opposed vacuum-ultraviolet laser pulses excited selected molecular levels and, about $10\mathrm{ns}$ later, selectively ionized excited nitrogen fragments. A microchannel plate detector, phosphor screen and camera recorded radii.^[ref]

The measured squared radii were fitted against molecular excitation energies, referenced to the parent ground state:The intercept at zero radius gave the excited-product threshold; the fitted slope absorbed the detector scale. A wavemeter monitored the excitation source; scanning the probe covered the recoil Doppler shift. Subtracting the atomic excitation energies converted the intercept to ground-product $D_0$.^[ref]

An apertured grounded plate and detector timing rejected faster competing channels. Selecting fragment electronic states distinguished nearby thresholds. Agreement of $D_e$ across isotopes after zero-point energy correction tested consistency. The method still requires correctly assigned levels, adequate near-threshold signal and stable imaging; a signal drop alone can reflect another channel or a barrier.^[ref]

This measurement determines a state-resolved ground-state dissociation energy. Obtaining a finite-temperature bond-dissociation enthalpy requires the thermal increments above; obtaining a bond potential-well depth requires the zero-point energy correction. The three quantities describe different starting conditions for the same specified separation.

Conversion of molecular nitrogen into biologically accessible reduced nitrogen. Symbiotic fixation costs energy and must be distinguished from nitrate uptake.

An intense band near $2088\mathrm{c}{\mathrm{m}}^{-1}$ is consistent with the high-frequency coupled C–N–N stretching motion of a diazo group, with substantial N–N multiple-bond character. It lies above a typical isolated C=N double-bond stretch, and supports contributions with a strong N–N connection. It does not establish that the molecule is a literal localized C–N single bond plus an unperturbed N≡N triple bond: a normal mode moves the coupled framework, and the resonance contributors describe one electronic structure.

Protonation at the nucleophilic carbon gives methyldiazonium, $\mathrm{C}{\mathrm{H}}_3-{\mathrm{N}}^{+}\equiv \mathrm{N}$. The carbon-rich highest occupied molecular orbital and the carbon-negative resonance contributor rationalize this site. Subsequent displacement of molecular nitrogen can be strongly favourable; the initial protonation product still contains both nitrogens.

First, proton transfer from acetic acid to the carbon of diazomethane gives methyldiazonium and an acetate ion:Draw an electron-pair arrow from carbon, using the carbon-negative resonance contributor, to the acidic hydrogen, and another from the acid O–H bond to oxygen. Second, an acetate oxygen attacks the diazonium methyl carbon by an SN2 reaction; an arrow from the C–N bond to nitrogen expels neutral ${\mathrm{N}}_2$:The acid's hydroxyl hydrogen has become the third hydrogen of the newly installed methyl group. This is a methyl-transfer sequence driven by formation of molecular nitrogen, without forming a free methyl carbocation or invoking Fischer esterification.

Four possible molecular signatures of disequilibrium chemistry in an exoplanet atmosphere, measured through an exoplanet transmission spectrum or exoplanet emission spectrum, are:

The first two signatures can be consequences of the same process and are not independent evidence for two mechanisms. Changes in atmospheric carbon-to-oxygen ratio, atmospheric metallicity of a giant planet, exoplanet cloud coverage, and the atmospheric pressure-temperature profile can mimic abundance changes. A convincing inference compares several molecular bands with a chemically consistent equilibrium model rather than identifying one unusual band alone.

For solar elemental abundances, take a molecular hydrogen- and helium-dominated atmosphere with atmospheric carbon-to-oxygen ratio near $0.55$. The principal oxygen-bearing molecule is generally water; the carbon and nitrogen carriers depend on both temperature and pressure.

At the cool $500\mathrm{K}$ observable upper layers, methane is the expected main carbon reservoir under chemical equilibrium, with abundant water and much less carbon monoxide. At the hotter layers approaching $1400\mathrm{K}$, carbon monoxide becomes the main carbon carrier and water contains much of the oxygen not bound in it. The relevant law of mass action follows fromLower temperature favors the exothermic methane-forming direction, while increasing pressure favors the side with fewer molecules. This explains why the change of dominant carrier cannot be specified by temperature alone.

Nitrogen is distributed between molecular nitrogen and Ammonia. Cooling favors Ammonia, but low pressure favors molecular nitrogen; it is therefore unsafe to call Ammonia dominant throughout the $500\mathrm{K}$ low-pressure region. The exact partition requires the equilibrium constant for ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$.

Carbon dioxide is usually a minor constituent at solar composition; hydrogen cyanide and acetylene are much less abundant than the principal carbon carriers in this oxygen-rich equilibrium case. Condensation can remove refractory species where a condensation curve is crossed. The robust cool-atmosphere expectation is a molecular hydrogen–helium background with methane and water, changing toward carbon monoxide in hotter layers. Precise mixing ratios require thermodynamic data and an explicitly specified elemental inventory after rainout.

Take the logarithm to base ten and write pressure in units of $1\mathrm{bar}$, so its argument is dimensionless. Continuity of the atmospheric pressure-temperature profile givesThusIf the logarithm means $\ln$, the equivalent constant is $C=900/\ln 100\simeq 195.4\mathrm{K}$. A plot of temperature against logarithmic pressure is vertical in each isothermal region and straight between the two endpoints.

The processes can be organized by the supplied pressure ranges, although the exact boundaries require reaction rates, irradiation and mixing information:

The profile identifies plausible chemical regimes, but does not fix their transition pressures by itself. In particular, cloud formation depends on the species-specific condensation curve, and ultraviolet processing depends on shielding.

Plants generally incorporate combined nitrogen into organic compounds, whereas animals eliminate the surplus nitrogen of metabolized compounds chiefly as Ammonia, urea or uric acid. The two processes connect nitrogen chemistry to the organism's carbon supply, water economy and environment.

Roots take up nitrate and ammonium from their surroundings. Nitrate must be reduced before its nitrogen can be incorporated in the usual amino form: nitrate reductase produces nitrite, and nitrite reductase produces ammonium. The balanced reduction, written without implying a single elementary reaction, isReducing equivalents and energy must be supplied by metabolism; nitrate is not simply deposited unchanged inside every protein.

In the modern biochemical account, glutamine synthetase incorporates ammonium into glutamine, using ATP; glutamate synthase transfers that nitrogen to a carbon skeleton derived from 2-Oxoglutarate, producing glutamate. Further transfer and synthesis distribute nitrogen into other amino acids, proteins, nucleotides and other cell constituents. Carbon metabolism therefore provides both energy and skeletons for nitrogen assimilation. These named enzymes and reactions explain the process today; they were not a completed molecular scheme in 1864.^[ref]

Ordinary higher-plant cells do not themselves reduce atmospheric molecular nitrogen merely because the gas surrounds the leaves. Biological nitrogen fixation is performed by particular microorganisms; symbiotic associations can supply fixed nitrogen to a host plant. The later elucidation of root-nodule symbiosis should be distinguished from what the examiner could have expected. Organic nitrogen can also be taken up in suitable circumstances, so nitrate and ammonium are important routes rather than an exhaustive prohibition on every other source.^[ref]

A useful assimilation experiment grows comparable seedlings in a defined medium containing all required minerals except combined nitrogen, with parallel nitrate- or ammonium-supplied cultures. Initial seed reserves, contaminating nitrogen, water and microbial growth must be allowed for. Growth and final nitrogen content are more informative than green appearance alone. A plant initially growing in a nitrogen-free solution may simply be consuming seed reserves; that observation does not demonstrate fixation of atmospheric nitrogen.

Animals obtain most of their nitrogen from organic food. Amino acid metabolism separates nitrogen handling from oxidation or reuse of the carbon skeleton. Free Ammonia is toxic at high concentrations, and mammals convert much of their waste nitrogen into urea in the liver; the kidneys then eliminate it in urine. Uric acid is also produced from purine breakdown. Renal ammonium excretion has a separate important connection with acid-base balance. Urea formation and urinary excretion are different processes in different organs.^[ref]

Many aquatic animals can release Ammonia directly into abundant surrounding water. Birds, many reptiles and many insects eliminate much nitrogen as relatively insoluble uric acid, conserving water; mammals generally depend more on soluble urea. These are broad physiological strategies with exceptions, not a rule that all animals have human urine. Faecal nitrogen includes unabsorbed food as well as endogenous material, while smaller losses can occur through skin and secretions. For a stated interval the accounting identity isPositive retention during growth and negative balance during tissue loss need not be errors of excretion. Nitrogen is redistributed or lost in compounds; it is not simply breathed out as all the atmospheric nitrogen passing through the lungs.

Purified coal gas is mainly molecular hydrogen, methane and carbon monoxide, with smaller quantities of other hydrocarbons and diluent gases. It is made by heating coal in retorts with little or no admitted air, not by completely burning the coal.

The hot products include permanent gases, condensable organic vapours and water vapour, leaving coke in the retort. Cooling removes much of the coal tar and condenses water, which captures Ammonia as ammoniacal liquor. Further washing and purification remove much of the remaining Ammonia, hydrogen sulfide and other objectionable constituents before the gas is distributed. A crude retort product and purified household coal gas therefore have different compositions.

Molecular hydrogen is commonly the largest component by volume. Methane is another major combustible constituent, while carbon monoxide contributes fuel value and serious toxicity. Ethylene and other unsaturated hydrocarbons, together with vapours such as benzene, contribute strongly to the luminous flame. Their thermal breakdown can produce incandescent soot, explaining why a small fraction of heavier hydrocarbons can disproportionately affect lighting quality. Smaller or variable quantities of carbon dioxide and molecular nitrogen dilute the combustible mixture. Molecular oxygen is not an intended major constituent; air ingress can change the mixture.

There is no single balanced chemical equation for making coal gas: coal is a complex feed and produces many products simultaneously. Nor is one exact percentage composition universal; it depends on the coal, retort temperature, operating conditions and purification. The main distinction is between the light combustible gases, the smaller illuminating hydrocarbon fraction, and contaminants or diluents. Modern natural gas, usually rich in methane, should not be used as a synonym for historical coal gas.

A solvent is the component designated as the medium of a chemical solution, commonly the component present in greatest proportion. Water is a common solvent, not a necessary one. A mixture of mostly ethanol with a little water can designate ethanol as solvent and water as solute. Chemical solutions can also be gas or solid mixtures; molecular nitrogen is the principal medium of ordinary well-mixed air. When proportions are comparable, state the convention explicitly.^[ref]

The solvent is part of the final sample. Choosing it influences solubility and solvation; measuring its added volume alone does not determine the final chemical solution volume. Solvent and solute masses add in a closed account, whereas the final volume should be measured rather than inferred by adding pre-mixing volumes.