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Ammonium chloride reacts with a strong base, like sodium hydroxide, to release ammonia gas: NH 4 Cl + NaOH → NH 3 + NaCl + H 2 O. Similarly, ammonium chloride also reacts with alkali-metal carbonates at elevated temperatures, giving ammonia and alkali-metal chloride: 2 NH 4 Cl + Na 2 CO 3 → 2 NaCl + CO 2 + H 2 O + 2 NH 3
Lewis structure of a water molecule. Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.
An example of a dative covalent bond is provided by the interaction between a molecule of ammonia, a Lewis base with a lone pair of electrons on the nitrogen atom, and boron trifluoride, a Lewis acid by virtue of the boron atom having an incomplete octet of electrons. In forming the adduct, the boron atom attains an octet configuration.
In another comparison of Lewis and Brønsted–Lowry acidity by Brown and Kanner, [19] 2,6-di-t-butylpyridine reacts to form the hydrochloride salt with HCl but does not react with BF 3. This example demonstrates that steric factors, in addition to electron configuration factors, play a role in determining the strength of the interaction ...
The nitrogen centres of hexachlorophosphazene are weakly basic, and this Lewis base behaviour has been suggested to play a role in the polymerisation mechanism. [7] Specifically, hexachlorophosphazene has been reported to form adducts of various stoichiometries with Lewis acids AlCl 3 , AlBr 3 , GaCl 3 , SO 3 , TaCl 5 , VOCl 3 , but no isolable ...
Mild heating results in production of hydrogen chloride, nitrogen, oxygen, and water. 4 NH 4 ClO 4 → 4 HCl + 2 N 2 + 5 O 2 + 6 H 2 O. The combustion of AP is quite complex and is widely studied. AP crystals decompose before melting, even though a thin liquid layer has been observed on crystal surfaces during high-pressure combustion processes ...
The nitrogen center is basic but much less so than ammonia. It is hydrolyzed by hot water to release ammonia and hypochlorous acid. NCl 3 + 3 H 2 O → NH 3 + 3 HOCl. Concentrated samples of NCl 3 can explode to give N 2 and chlorine gas. 2 NCl 3 → N 2 + 3 Cl 2. NCl 3 can react with certain organic compounds to produce amines. [2]
Liquid nitrogen is a compact and readily transported source of dry nitrogen gas, as it does not require pressurization. Further, its ability to maintain temperatures far below the freezing point of water, specific heat of 1040 J ⋅kg -1 ⋅K -1 and heat of vaporization of 200 kJ⋅kg -1 makes it extremely useful in a wide range of applications ...