Chemistry Section 11

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• In base-catalyzed carbonyl reaction, catalyst increases nucleophilic character.
• Alkali metals are named due to basic oxide and hydroxides solubility.
• Formula of Chile saltpetre is NaNO3.
• Beryllium oxide (BeO) is amphoteric.
• Li differs due to small size, high charge density, and less electropositivity.
• Carbonates of lithium are unstable due to low electropositivity.
• Radium is not an alkali metal.
• Cesium resembles no other element in its family.
• Downs cell prepares sodium metal.
• Ammonia is prepared by heating ammonium chloride with aqueous sodium hydroxide.
• Crystals of Na2CO3.10H2O lose water when exposed to air.
• Na2CO3 gives a white precipitate with aqueous BaCl2.
• Deliquescence is when a solid absorbs moisture and becomes liquid.
• In a diaphragm cell, higher brine level prevents hydroxide ions from reaching the anode.
• Alkali and alkaline earth metals exhibit colors when heated due to de-excitation of electrons.
• First ionization potential of alkaline earth metals is greater due to smaller atomic sizes.
• NaOH is called caustic soda due to its corrosion of organic tissues.
• Carnalite has the chemical formula KCI.MgCl2.6H2O.
• Electrolysis of dilute NaCl solution results in oxygen at the anode.
• Cs+ ion has the maximum heat of hydration.
• Natron is Na2CO3.H2O.
• LiOH is least ionic, decomposing on heating.
• Alkali derives from the Arabic term for ashes.
• Normal leaf development requires calcium (Ca).
• Nitrates of Li and Na give different products on thermal decomposition.
• BaSO4 is the least soluble sulfate in water.
• H2O is gypsum’s chemical formula.
• Molten sodium chloride conducts electricity due to ion movement.
• CaCO3 is insoluble among the listed carbonates.
• In a diaphragm cell, hydrogen is discharged by the reduction of water.
• Gypsum is applied to soil as a source of Ca and S.
• Lithium forms only normal oxide on reacting with O2.
• Lithium and magnesium show diagonal relationship in the periodic table.
• Sodium doesn’t exist in the +2 oxidation state due to high second ionization potential.
• Magnesium metal doesn’t burn in neon gas.
• Alkali metal’s second ionization potential is high due to inert gas configurations.
• Lithium can form a complex.
• Gypsum prevents rapid hardening of cement.
• Phenanthrene contains three benzene rings.
• Benzene has six electrons forming a delocalized electron cloud.
• Iodine is given the number one position in naming when substituting benzene.
• Michael Faraday discovered benzene in the gas produced by destructive distillation without oxygen.
• Benzene reacts with three moles of H2 when heated with hydrogen and a platinum catalyst.
• Resonance energy of benzene is 150.5 kJ/mol.
• Organo-nickel is employed as a catalyst when benzene is prepared from acetylene.
• Chlorobenzene with NaOH at 360°C & 150atm. produces benzene.
• Benzene doesn’t undergo addition reactions with bromine in the presence of sunlight.
• Benzene doesn’t undergo addition reactions with bromine in the presence of sunlight.
• Aniline is a derivative of benzene with an amino group.
• Resonance energy of benzene is not 150.5 K Cal/mole.
• Friedel & Craft alkylation uses catalysts Cr2O3 + A?2O3 + SiO2.
• Toluene reacts with hydrogen in the presence of a platinum catalyst to produce benzyl chloride.
• Benzenetriozonide’s molecular formula is C6H6O9.
• Benzenetriozonide yields glyoxal upon hydrolysis.
• In benzene sulphonic acid, the sulphonic group is attached through sulfur.
• Aniline is a derivative of benzene containing an amino group.
• Nitration of chlorobenzene gives o-chloronitrobenzene and p-chloronitrobenzene.
• Gallium arsenide’s conductivity increases with temperature.
• Benzene reacts with soda lime at 500?C to produce n-hexane.
• Benzene reacts with alkyl halides and aluminum chloride to undergo Friedel & Craft alkylation.
• Naphthalene is a fused cyclic aromatic compound.
• Acetophenone is a ketone.
• Benzene doesn’t undergo polymerization reactions.
• Nitronium ion is NO2+.
• Benzene heated with V2O5 at 450°C undergoes oxidation.
• Second ionization potential of alkali metals is low.
• Francium is the most reactive alkali metal.
• Cesium and rubidium are the most reactive alkali metals.
• Halogens belong to the same group as alkali metals.
• Lithium is the smallest alkali metal.
• Francium is synthetic and highly unstable.
• Cesium is the most electropositive metal.
• Francium has the highest ionization potential among alkali metals.
• Cesium has the smallest atomic radius among alkali metals.
• Alkali metals have low melting and boiling points.
• Alkali metals are soft and can be cut with a knife.
• The alkali metal group has seven valence electrons.
• Alkali metals are found in various minerals and mineral springs.
• Alkali metals have a +1 oxidation state.
• The alkali metals have low atomic and ionic sizes.
• Alkali metals are readily soluble in nonpolar solvents.
• Francium is often used in glow-in-the-dark paints.
• Cesium is the least reactive alkali metal.
• Alkali metals are generally denser than other metals.
• Lithium has the highest ionization potential among alkali metals.
• Francium is typically found in large amounts in the Earth’s crust.
• The alkali metals have a silvery appearance when freshly cut.