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According to both ab initio calculations and the experimental X-ray structure, the cation is planar, symmetric, and approximately V-shaped, with bond angles 111° at the central atom (angle N2–N3–N4) and 168° at the second and fourth atoms (angles N1–N2–N3 and N3–N4–N5). The bond lengths for N1–N2 and N4–N5 are 1.10 Å and the ...
The 15 N: 14 N ratio is commonly used in stable isotope analysis in the fields of geochemistry, hydrology, paleoclimatology and paleoceanography, where it is called δ 15 N. [40] Of the thirteen other isotopes produced synthetically, ranging from 9 N to 23 N, 13 N has a half-life of ten minutes and the remaining isotopes have half-lives less ...
In chemistry, azide (/ ˈ eɪ z aɪ d /, AY-zyd) is a linear, polyatomic anion with the formula N − 3 and structure − N=N + =N −. It is the conjugate base of hydrazoic acid HN 3. Organic azides are organic compounds with the formula RN 3, containing the azide functional group. [1] The dominant application of azides is as a propellant in ...
Many stoichiometric phases are usually present for most elements (e.g. MnN, Mn 6 N 5, Mn 3 N 2, Mn 2 N, Mn 4 N, and Mn x N for 9.2 < x < 25.3). They may be classified as "salt-like" (mostly ionic), covalent, "diamond-like", and metallic (or interstitial ), although this classification has limitations generally stemming from the continuity of ...
In the NO − 3 anion, the oxidation state of the central nitrogen atom is V (+5). This corresponds to the highest possible oxidation number of nitrogen. Nitrate is a potentially powerful oxidizer as evidenced by its explosive behaviour at high temperature when it is detonated in ammonium nitrate (NH 4 NO 3), or black powder, ignited by the shock wave of a primary explosive.
Oxidation numbers are assigned to elements in a molecule such that the overall sum is zero in a neutral molecule. The number indicates the degree of oxidation of each element caused by molecular bonding. In ionic compounds, the oxidation numbers are the same as the element's ionic charge.
An example of the difference is the empirical formula for glucose, which is CH 2 O (ratio 1:2:1), while its molecular formula is C 6 H 12 O 6 (number of atoms 6:12:6). For water, both formulae are H 2 O. A molecular formula provides more information about a molecule than its empirical formula, but is more difficult to establish.
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.