This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Lewis acid definition A Lewis acid is a substance (atom, ion, or molecule) that can accept a pair of electrons to form a coordinate covalent bond. A Lewis base is a substance that can donate a pair of electrons. Step 2: Common inorganic and organic Lewis acids Inorganic Lewis acids: BF_3, AlCl_3, BeCl_2, Fe^3+, H^+, SO_3. Organic Lewis acids: carbocations like CH_3^+, (CH_3)_3C^+, acyl chlorides like CH_3COCl. Step 3: Lewis acids and bases in daily life Lewis acids: CO_2 (in carbonated drinks, accepts electrons from water), SO_2 (in pollution, from burning coal). Lewis bases: NH_3 (in household cleaners), OH^- (in soaps). Step 4: Lewis structures for the acids HNO_3: Central N bonded to one OH (single bond), one =O (double bond), one O^- (single bond, resonance). N has 8 electrons (one from charge). &H--O--N \\ & || \\ & O (with lone pairs: O in OH has 2, =O has 2, terminal O has 3; resonance forms). H_2SO_4: Central S bonded to two OH (single), two =O (double). S has 12 electrons (expanded octet). & HO--S--OH \\ & || || \\ & O O HClO: H--O--Cl, O has 2 lone pairs, Cl has 3 lone pairs. H--O--Cl (: on O and Cl) HBr: H--Br, Br has 3 lone pairs. H--Br: HClO_4: Central Cl bonded to three =O, one OH. Cl has 12 electrons. &HO--Cl \\ & || \\ & O \\ & | \\ & O (resonance, all O equivalent). Step 5: Lewis structures for NH_4^+ and H_3O^+ NH_4^+: Central N with 4 N--H single bonds (8 electrons on N). [H--N--H | H-- --H]^+ H_3O^+: Central O with 3 O--H bonds, 1 lone pair on O. [H--O--H | H]^+ (: on O) Step 6: Formulas for conjugate bases Formula first: Conjugate base = acid - H^+. HClO_4 ClO_4^-. HClO4 ->[ -H^+ ] ClO4^- H_2SO_4 HSO_4^-. H2SO4 ->[ -H^+ ] HSO4^- HNO_3 NO_3^-. HNO3 ->[ -H^+ ] NO3^- Step 7: Formulas for conjugate acids Formula first: Conjugate acid = base + H^+. ClO_4^- HClO_4. ClO4^- ->[ +H^+ ] HClO4 SO_4^2- HSO_4^-. SO4^2- ->[ +H^+ ] HSO4^- NO_3^- HNO_3. NO3^- ->[ +H^+ ] HNO3 Step 8: Amphoteric and amphiprotic substances Amphoteric (act as both Lewis acid and base): Al(OH)3, Zn(OH)2, Sn(OH)2. Example: Al(OH)3 + OH^- -> Al(OH)4^- (accepts e^- pair, Lewis acid); Al(OH)3 + 3H^+ -> Al^3+ + 3H2O (Lewis base). Amphiprotic (act as both Brønsted acid and base): H2O, HCO3^-, HSO4^-. Example: H2O + HCl -> H3O^+ + Cl^- (acid); H2O + NH3 -> NH4^+ + OH^- (base). Step 9: Sulfur atom in SO_2 as Lewis acid Lewis structure of SO_2: Central S with 1 lone pair, double bond to one O, single bond to other O (resonance, 10 electrons on S). & O \\ & || \\ O=S S has incomplete octet (can accept e^- pair), so SO_2 is Lewis acid (e.g., forms adduct with amines). This explains corrosion in pipes: SO_2 from pollution accepts electrons from metal oxides, breaking layers. ClO_4^-, HSO_4^-, NO_3^- HClO_4, HSO_4^-, HNO_3