Chemistry Section 12

---

• Phosphoric acid can be produced by the reaction of PCI5, P2O3, and P2O5 with water.
• “Phosphorus” is derived from a Greek word meaning “Light bearing.”
• The poisonous allotropic form of phosphorus is “White phosphorus.”
• Acetic anhydride can be obtained by treating ethyl alcohol with P2O5 and H2SO4.
• Thermal decomposition of phosphorous acid yields phosphoric acid and “Phosphine.”
• P2O5 is a hygroscopic powder that sublimes at 360°C.
• Phosphoric acid is a weak acid with a basicity of “3.”
• All elements in group VIA are “polymeric” in nature.
• The most stable allotropic form of phosphorus is “black phosphorus.”
• The chemical composition of cinnabar is “HgS.”
• Oxygen and sulfur show the same oxidation state, but not the same electronic configuration of valence shell electrons.
• Arsenic oxides are removed by passing through “Ferric hydroxide.”
• When sulfuric acid is treated with ethanol, sulfuric acid acts as a “dehydrating agent.”
• Nitrogen has the lowest melting point among the given elements.
• The most electronegative element among the given options is “Nitrogen.”
• Phosphene gas is produced if phosphorous acid undergoes “decomposition.”
• Pure quartz is not a “colored solid.”
• Steel does not contain “phosphorus.”
• Graphite is not used as an “abrasive.”
• The brown ring in the nitrate test is formed by “FeSO4.NO.”
• Oxygen and sulfur resemble each other in “showing same oxidation state.”
• The element in group VIA which is a “non-metal” is sulfur.
• All elements in group VIA, like sulfur, are “polymeric” in nature.
• The most stable allotropic form of phosphorous is “black phosphorus.”
• Nitrogen is the most electronegative element among the options given.
• Phosphine gas is produced when phosphorous acid is subjected to “oxidation” and “decomposition.”
• The oxide of chlorine produced in the given reaction is “ClO2.”
• The given reaction is a “disproportionation reaction.”
• Fluorine is the rarest halogen element, “Astatine” is the rare element.
• Vander Waals forces are strongest in “I2.”
• The most powerful oxidizing agent among the halogens is “F2.”
• Chlorine spontaneously reacts with gold (Au) to form Au+3, making “Cl2” the correct answer.
• Iodine reacts very slowly with halogen and is “Iodine.”
• The halogen with the highest electron affinity is “Chlorine.”
• Bromine can be liberated from KBr solution by the action of “Chlorine.”
• The brown ring test in the nitrate test involves the formation of “FeSO4.NO.”
• The element present in Teflon is “Fluorine.”
• Fluorine does not react with “Metals.”
• The halogen used for artificial fruit ripening is “Ethene.”
• The oxide of iodine used for quantitative analysis of CO is “I2O5.”
• Chlorine gas has a “greenish yellow” color.
• The reactivity of fluorine is due to the “polarity of C-Mg bond.”
• The reaction of ethyl magnesium bromide with acetone forms a “tertiary alcohol.”
• In primary alkyl halides, the halogen atom is attached to a carbon connected to “one” other carbon atom.
• Alkyl halides are best prepared by the reaction of alcohols with “SOCl2/Pyridine.”
• The general formula for alkynes is “CnH2n-2.”
• An alkyne with a triple bond at the second carbon is named using the suffix “-2-yne.”
• The reaction of alkynes with two equivalents of HCl forms “cis-dihaloalkanes.”
• Sodium alkynides are used to prepare alkynes with the addition of “water.”
• Alkynes can be reduced to alkanes using “sodium in liquid ammonia” as a reducing agent.
• Alkynes are more acidic than “alkanes” and “alkenes.”
• The reaction of alkynes with water in the presence of mercury(II) sulfate forms “ketones.”
• Alkynes can be hydrated to form “ketones” using dilute sulfuric acid as a catalyst.
• The polymerization of alkynes under high pressure and temperature forms “polyacetylene.”
• Alkynes readily undergo addition reactions with “H2” in the presence of catalysts like “Pd/C.”
• Addition of hydrogen to alkynes produces “alkanes.”
• The reaction of alkynes with hydrogen in the presence of a catalyst forms “alkanes.”
• The reaction of alkynes with “H2” over “Pd/C” catalyst forms alkanes.
• Alkynes react with halogens to form “tetrahaloalkanes.”
• Alkynes react with hydrogen in the presence of a “Pd/C” catalyst to form alkanes.
• The reaction of alkynes with hydrogen in the presence of a “Pd/C” catalyst reduces them to alkanes.
• The reaction of alkynes with “H2” over “Pd/C” catalyst leads to the formation of alkanes.
• Alkynes react with “HCl” and “HBr” to give “haloalkenes.”
• Alkynes react with hydrogen halides to form “vinyl halides.”
• Alkynes react with “HCl” and “HBr” to form “vinyl halides.”
• Alkynes react with hydrogen halides to form “haloalkenes.”
• Alkynes react with “H2O/H2SO4” to form “aldehydes” and “ketones.”
• The reaction of alkynes with “H2O/H2SO4” produces “aldehydes” and “ketones.”
• The reaction of alkynes with “HgSO4/H2SO4” followed by “NaBH4” produces “alkenes.”
• Alkynes react with “HgSO4/H2SO4” followed by “NaBH4” to form “alkenes.”