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By contrast, ammonia is basic and highly polar (1.47 D). [12] This contrast reflects the differing electronegativities of H vs F. Similar to dioxygen, NF 3 is a potent yet sluggish oxidizer. [6] It oxidizes hydrogen chloride to chlorine: [citation needed] 2 NF 3 + 6 HCl → 6 HF + N 2 + 3 Cl 2
When comparing a polar and nonpolar molecule with similar molar masses, the polar molecule in general has a higher boiling point, because the dipole–dipole interaction between polar molecules results in stronger intermolecular attractions. One common form of polar interaction is the hydrogen bond, which is also known as the H-bond.
The F 2 molecule is commonly described as having exactly one bond (in other words, a bond order of 1) provided by one p electron per atom, as are other halogen X 2 molecules. However, the heavier halogens' p electron orbitals partly mix with those of d orbitals, which results in an increased effective bond order; for example, chlorine has a ...
Attempted deprotonation results in defluorination to generate F − and difluorocarbene (CF 2). Some organocopper and organocadmium compounds have been developed as trifluoromethylation reagents. [7] Fluoroform is a precursor of the Ruppert-Prakash reagent CF 3 Si(CH 3) 3, which is a source of the nucleophilic CF − 3 anion. [8] [9]
Nitrosyl fluoride is typically produced by direct reaction of nitric oxide and fluorine, although halogenation with a perfluorinated metal salt is also possible.The compound is a highly reactive fluorinating agent that converts many metals to their fluorides, releasing nitric oxide in the process:
NF3 may refer to: Nitrogen trifluoride (NF 3), a colorless gas used as an etchant; Zukertort Opening, an opening move in chess (1. Nf3) This page was last edited on 3 ...
It is moderately polar with a dipole moment of 0.6 D. 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. [citation needed] 2 NCl 3 → N 2 + 3 Cl 2
Specifically, the dipole can cause electrostatic attraction or repulsion of the electrons from the non-polar molecule, depending on orientation of the incoming dipole. [13] Atoms with larger atomic radii are considered more "polarizable" and therefore experience greater attractions as a result of the Debye force. [citation needed]