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Question 1: Elemental fluorine is a dangerously powerful oxidant, reflecting the extreme ________ of fluorine.
HalogenNoble gasElectronegativityPeriodic table

Question 2: In 1886, the isolation of elemental fluorine was reported by ________ after almost 74 years of effort by other chemists.
Svante ArrheniusHenri MoissanAdolf von BaeyerAlfred Werner

Question 3: It is found in the -1 ________, except when bonded to another fluorine in F2 which gives it an oxidation number of 0.
HydrogenOxygenOxideOxidation state

Question 4: Hydrofluoric acid is extremely dangerous, whereas in synthetic drugs incorporating an ________ (e.g.
NaphthaleneBenzeneAromatic hydrocarbonAromaticity

Question 5: Along with some of its compounds, fluorine is used in the production of pure ________ from uranium hexafluoride and in the synthesis of numerous commercial fluorochemicals, including vitally important pharmaceuticals, agrochemical compounds, lubricants, and textiles.
CuriumTechnetiumPlutoniumUranium

Question 6: Naturally occurring organofluorine compounds are rare, the most notable example is ________, which functions as a plant defence against herbivores in at least 40 plants in Australia, Brazil and Africa.
Barium carbonateStrychnineSodium fluoroacetateAluminium phosphide

Question 7: The carbon-fluoride bond is ________ and very stable.
Metallic bondAromaticityChemical bondCovalent bond

Question 8: For example, it will readily "burn" hydrocarbons at room temperature, in contrast to the ________ of hydrocarbons by oxygen, which requires an input of energy with a spark.
CombustionFireFlameInternal combustion engine

Question 9: ________ antidepressants, except in a few instances, are fluorinated molecules.
MirtazapineTricyclic antidepressantSelective serotonin reuptake inhibitorSerotonin reuptake inhibitor

Question 10: In 1670 Schwanhard found that glass was etched when it was exposed to fluorspar that had been treated with ________.
AcidAcid–base reactionAcid dissociation constantOxygen
















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