All Chemistry Reactions (AS)

Group 17 Reactions

Reaction with Hydrogen:
- $H_2 + F_2 \longrightarrow 2HF_{(g)}$ (Explosive reaction)
- $H_2 + Cl_2 \longrightarrow 2HCl_{(g)}$ (Very fast reaction, can explode in sunlight)
- $H_2 + Br_2 \longrightarrow 2HBr_{(g)}$ (Slow reaction)
- $H_2 + I_2 \xrightarrow{Heat \ at \ 300^\circ C, Pt \ catalyst} 2HI_{(g)}$ (Very slow reaction, requires strong heating)
Decomposition of Hydrogen Halides:
- HF: No reaction
- HCl: No reaction
- $2HBr \xrightarrow{heat} H_{2(g)} + Br_{2(g)}$ (Red-brown vapor of Bromine seen)
- $2HI \xrightarrow{hot \ glass \ rod} H_{2(g)} + I_{2(g)}$ (Purple vapor of Iodine seen)
- Note: Stability of hydrogen halides decreases down the group
Oxidizing and Reducing Agent Theory:
- Oxidizing power decreases down the group: $F > C l > B r > I$
- Reducing power increases down the group: $I^{-} > B r^{-} > C l^{-} > F^{-}$
- $F + e^- \longrightarrow F^-$ (Reducing agent)
- $Cl + e^- \longrightarrow Cl^-$ (Reducing agent)
- $Br + e^- \longrightarrow Br^-$ (Reducing agent)
- $I + e^- \longrightarrow I^-$ (Reducing agent)

Reactions with Concentrated Sulfuric Acid

$NaCl + H_2SO_4 \longrightarrow NaHSO_4 + HCl$ (No further reaction)
$2NaBr + H_2SO_4 \longrightarrow NaHSO_4 + HBr$
$2HBr + H_2SO_4 \longrightarrow Br_2 + SO_2 + 2H_2O$
$2NaI + H_2SO_4 \longrightarrow NaHSO_4 + HI$
$8HI + H_2SO_4 \longrightarrow 4I_2 + H_2S + 4H_2O$
Observations:
- HCl, HBr, and HI are white fumes
- $B r_{2}$ is a red-brown gas
- $I_{2}$ is a purple gas
- $H_{2} S$ has a rotten-egg smell

Reaction of $C l_{2}$ with NaOH (Disproportionation)

$Cl_2 + 2NaOH_{(aq)} \xrightarrow{15^\circ C \ (cold)} NaCl + NaClO + H_2O$
$3Cl_2 + 6NaOH_{(aq)} \xrightarrow{70^\circ C \ (hot)} 5NaCl + NaClO_3 + 3H_2O$

Identification of Halogens

$A g N O_{3}$ $A g N O_{3}$ added to solutions of halides:
- NaCl: White precipitate
- NaBr: Cream precipitate
- NaI: Yellow precipitate
Solubility in dilute and concentrated $N H_{3}$ $N H_{3}$ :
- NaCl: Soluble
- NaBr: Partially soluble
- NaI: Insoluble

Reaction of Halides with $N H_{3}$

$AgCl + 2NH_3 \longrightarrow [Ag(NH_3)_2]^+Cl^-$ (Soluble)
$AgBr + 2NH_3 \longrightarrow [Ag(NH_3)_2]^+Br^-$ (Partially soluble)

Water Chlorination

$Cl_2 + H_2O \longrightarrow HOCl + HCl$ (Hypochlorous acid kills bacteria)

Displacement Reactions

$2NaBr + Cl_2 \longrightarrow 2NaCl + Br_2$
$2NaI + Cl_2 \longrightarrow 2NaCl + I_2$
$2NaI + Br_2 \longrightarrow 2NaBr + I_2$

Alkanes

Combustion:
- Complete: $CH_4 + 2O_2 \longrightarrow CO_2 + 2H_2O$
- Incomplete: $CH_4 + \frac{3}{2}O_2 \longrightarrow CO + 2H_2O$ $CH_4 + O_2 \longrightarrow C + 2H_2O$
Cracking:
- Catalytic Cracking: $C_6H_{14} \xrightarrow{500^\circ C, Al_2O_3, SiO_2} C_2H_4 + H_2$
- Thermal Cracking: $C_5H_{12} \xrightarrow{800^\circ C, High \ pressure} C_2H_4 + C_3H_8$
Free Radical Substitution:
- Conditions: UV Light, Halogens
- Initiation: $Cl_2 \longrightarrow 2Cl\cdot$
- Propagation: $CH_4 + Cl\cdot \longrightarrow CH_3\cdot + HCl$ $CH_3\cdot + Cl_2 \longrightarrow CH_3Cl + Cl\cdot$
- Termination: $Cl\cdot + Cl\cdot \longrightarrow Cl_2$ , $Cl\cdot + CH_3\cdot \longrightarrow CH_3Cl$ , $CH_3\cdot + CH_3\cdot \longrightarrow C_2H_6$

Alkenes

Formation: Cracking, Elimination of Alkyl Halides, Dehydration of Alcohols
Reactions with Halogens:
- Electrophilic Addition of Halogens: $C_2H_4 + Br_{2(l)} \longrightarrow C_2H_4Br_2$ (Room temperature and dark conditions)
Reactions with Hydrogen Halides:
- Electrophilic Addition of Hydrogen Halides: $C_2H_4 + HBr \longrightarrow C_2H_5Br$ (Room temperature, Markovnikov's Rule applies)
Electrophilic Addition of Hydrogen (Hydrogenation):
- $C_2H_4 + H_2 \xrightarrow{140^\circ C, Ni \ catalyst} C_2H_6$
- $C_2H_4 + H_2 \xrightarrow{Room \ Temp., Pt/Pd \ catalyst} C_2H_6$
Electrophilic Addition of Bromine (Bromine Water Test):
- $CH_2=CH_2 + Br_{2(aq)} \longrightarrow CH_2BrCH_2OH + HBr$ (Color change from brown to colorless when hydrocarbon is saturated)
Electrophilic Addition of $H_{2} O$ (Hydration):
- $CH_2=CH_2 + H_2O \xrightarrow{300^\circ C, 10 \ atm \ pressure, H_3PO_4 \ catalyst} CH_3CH_2OH$
Combustion:
- Complete: $C_2H_4 + 3O_2 \longrightarrow 2CO_2 + 2H_2O$
- Incomplete: $C_2H_4 + 2O_2 \longrightarrow 2CO + 2H_2O$ , $C_2H_4 + O_2 \longrightarrow 2C + 2H_2O$
Oxidation:
- Mild Oxidation: $CH_2=CH_2 \xrightarrow{Cold, dilute, acidified \ KMnO_4} CH_2OHCH_2OH$
- Strong Oxidation: (Hot, concentrated, acidified $K M n O_{4}$ ) yields carbonyl compounds

Alkyl Halides

Formation:
- Free Radical Substitution of Alkanes
- Electrophilic Addition of Hydrogen Halides
- Electrophilic Addition of Halogens
- Nucleophilic Substitution of Alcohols (Bromination, Chlorination)
Nucleophilic Substitution:
- $S_{N} 1$ (Unimolecular) - Tertiary Alkyl Halides
- Mechanism: See source for a diagram of the mechanism.
- $S_{N} 2$ (Bimolecular) - Primary Alkyl Halides *Mechanism: See source for a diagram of the mechanism.
- Conditions: NaOH, Heat, Aqueous conditions
Nucleophilic Substitution of $N H_{3}$ :
- $CH_3CH_2Br + NH_3 \longrightarrow CH_3CH_2NH_2 + HBr$
- $CH_3CH_2Br + CH_3CH_2NH_2 \longrightarrow CH_3CH_2NHCH_2CH_3 + HBr$
- $CH_3CH_2Br + CH_3CH_2NHCH_2CH_3 \longrightarrow CH_3CH_2 -N^+ -(CH_2CH_3)_2 + HBr$
- $CH_3CH_2 -N^+ -(CH_2CH_3)_2 + CH_3CH_2Br \longrightarrow [CH_3CH_2-N^+ -(CH_2CH_3)_3]Br^-$
- Conditions: Ethanol as solvent, Heat
Nucleophilic Substitution by NaCN:
- $CH_3CH_2Br + NaCN \longrightarrow CH_3CH_2CN + NaBr$ (Forms propanenitrile)
- Conditions: Ethanol as solvent, Heat
Elimination of Alkyl Halides
- Conditions: NaOH as reagent, Heat, Ethanol as solvent
- Primary: $CH_3CH_2Br + NaOH \longrightarrow CH_2=CH_2 + H_2O + NaBr$
- Tertiary: $C(CH_3)_3Br + NaOH \longrightarrow (CH_3)_2C=CH_2 + H_2O + NaBr$
- Secondary: (Mechanism): See source for a diagram of the mechanism. Forms 3 products : transbut-2-ene (33%), cisbut-2-ene (33%) and but-1-ene (33%).

Period 3 Elements

Combustion:
- $4Na + O_2 \longrightarrow 2Na_2O$ (Burns with yellow flame)
- $2Mg + O_2 \longrightarrow 2MgO$ (Burns with intense white flame)
- $4Al + 3O_2 \longrightarrow 2Al_2O_3$ (Burns with yellow or white flame, Insoluble oxide)
- $Si + O_2 \longrightarrow SiO_2$ (Burns with yellow flame, Insoluble oxide)
- $4P + 3O_2 \longrightarrow P_4O_6$ $4P + 5O_2 \longrightarrow P_4O_{10}$ (Burns with white flame)
- $S + O_2 \longrightarrow SO_2$ (Burns with blue flame)
- $2SO_2 + O_2 \xrightarrow{Vanadium(V) \ oxide} 2SO_3$ $SO_3 + H_2O \longrightarrow H_2SO_4$
Reaction of Period 3 Oxides with Water:
- $Na_2O + H_2O \longrightarrow 2NaOH$ (pH = 13-14)
- $MgO + H_2O \longrightarrow Mg(OH)_2$ (pH = 9, slightly soluble)
- $Al_2O_3 + H_2O \longrightarrow$ No reaction (Insoluble)
- $SiO_2 + H_2O \longrightarrow$ No reaction (Insoluble)
- $P_4O_{10} + 6H_2O \longrightarrow 4H_3PO_4$ (pH = 2)
- $P_4O_{6} + 6H_2O \longrightarrow 4H_3PO_3$ (pH = 2)
- $SO_2 + H_2O \longrightarrow H_2SO_3$ (pH = 1) $SO_3 + H_2O \longrightarrow H_2SO_4$ (pH = 1)
- $Cl_2O + H_2O \longrightarrow 2HOCl$
- $Cl_2O_7 + H_2O \longrightarrow 2HClO_4$
Neutralization of Period 3 Oxides:
- Basic Oxides: $Na_2O + 2HCl \longrightarrow 2NaCl + H_2O$ and $MgO + 2HCl \longrightarrow MgCl_2 + H_2O$
- Amphoteric Oxide: $Al_2O_3 + 6HCl \longrightarrow 2AlCl_3 + 3H_2O$ and $Al_2O_3 + 2NaOH + 3H_2O \longrightarrow 2NaAl(OH)_4$
- Acidic Oxides: $SiO_2 + 2NaOH \longrightarrow Na_2SiO_3 + H_2O$ , $P_4O_{10} + 12NaOH \longrightarrow 4Na_3PO_4 + 6H_2O$ , $SO_2 + 2NaOH \longrightarrow Na_2SO_3 + H_2O$ , $SO_3 + 2NaOH \longrightarrow Na_2SO_4 + H_2O$ , $Cl_2O_7 + 2NaOH \longrightarrow 2NaClO_4 + H_2O$
Reaction of Period 3 elements with $C l_{2}$ :
- $2Na + Cl_2 \longrightarrow 2NaCl$ (Burns with orange flame, white solid formed)
- $Mg + Cl_2 \longrightarrow MgCl_2$ (Burns with intense white flame)
- $2Al + 3Cl_2 \xrightarrow{Room \ Temp} 2AlCl_3$
- $2Al + 3Cl_2 \xrightarrow{Heat} Al_2Cl_6(g)$ (Dimer)
- $Si + 2Cl_2 \xrightarrow{Heat} SiCl_4(l)$ (Covalent colorless liquid)
- $2P + 3Cl_2 \xrightarrow{Heat} 2PCl_3$ (Covalent colorless liquid)
- $PCl_3 + Cl_2 \longrightarrow PCl_5$ (White solid)
- $2S + Cl_2 \longrightarrow S_2Cl_2$ (Orange liquid with a bad smell)
Period 3 Chlorides in $H_{2} O$ :
- $NaCl_{(aq)} \longrightarrow Na^+_{(aq)} + Cl^-_{(aq)}$ (pH = 7)
- $MgCl_2 + 6H_2O \longrightarrow [Mg(H_2O)_6]^{2+}_{(aq)} + 2Cl^-_{(aq)}$ , $[Mg(H_2O)_6]^{2+}_{(aq)} \longrightarrow [Mg(H_2O)_5OH]^+_{(aq)} + H^+_{(aq)}$ (pH = 6.5)
- $AlCl_3 + 6H_2O \longrightarrow [Al(H_2O)_6]^{3+}_{(aq)} + 3Cl^-_{(aq)}$ , $[Al(H_2O)_6]^{3+}_{(aq)} \longrightarrow [Al(H_2O)_5OH]^{2+}_{(aq)} + H^+_{(aq)}$ (pH = 3)
- $SiCl_4 + 2H_2O \longrightarrow SiO_2 + 4HCl$ (pH = 1-2, white ppt)
- $PCl_3 + 3H_2O \longrightarrow 3HCl + H_3PO_3$ (pH = 1-2)
- $PCl_5 + 4H_2O \longrightarrow 5HCl + H_3PO_4$ (pH = 1-2)
- $S_2Cl_2 + 2H_2O \longrightarrow H_2S + SO_2 + 2HCl$ (pH = 1-2)
Important Reaction:
- $Cl_2 + H_2O \rightleftharpoons HCl + HOCl$
- $2HOCl \rightleftharpoons 2HCl + O_2$

Group 2 Reactions

Combustion of Group 2 metals:
- $2Mg + O_2 \longrightarrow 2MgO$ (Intense white flame)
- $2Ca + O_2 \longrightarrow 2CaO$ (Brick red flame)
- $2Sr + O_2 \longrightarrow 2SrO$ (Crimson flame)
- $2Ba + O_2 \longrightarrow 2BaO$ (Apple green flame)
Reaction of Group 2 Oxides with water:
- $MgO + H_2O \longrightarrow Mg(OH)_2$ (pH = 9)
- $CaO + H_2O \longrightarrow Ca(OH)_2$ (pH = 11)
- $SrO + H_2O \longrightarrow Sr(OH)_2$ (pH = 13)
- $BaO + H_2O \longrightarrow Ba(OH)_2$ (pH = 13)
- Note: Solubility of Group 2 hydroxides increases down the group
Reaction of Group 2 Oxides with Acids:
- $MgO + H_2SO_4 \longrightarrow MgSO_4 + H_2O$ ( $M g S O_{4}$ is soluble)
- $CaO + H_2SO_4 \longrightarrow CaSO_4 + H_2O$
- $SrO + H_2SO_4 \longrightarrow SrSO_4 + H_2O$
- $BaO + H_2SO_4 \longrightarrow BaSO_4 + H_2O$ $B a O + H_{2} S O_{4} ⟶ B a S O_{4} + H_{2} O$ ( $B a S O_{4}$ $B a S O_{4}$ is a white precipitate)
  - Note: Solubility of Group 2 sulfates decreases down the group
Decomposition of Group 2 Nitrates:
- $Mg(NO_3)_2 \longrightarrow MgO + 2NO_2 + \frac{1}{2}O_2$
- $Ca(NO_3)_2 \longrightarrow CaO + 2NO_2 + \frac{1}{2}O_2$
- $Sr(NO_3)_2 \longrightarrow SrO + 2NO_2 + \frac{1}{2}O_2$
- $Ba(NO_3)_2 \longrightarrow BaO + 2NO_2 + \frac{1}{2}O_2$ $B a (N O_{3})_{2} ⟶ B a O + 2 N O_{2} + \frac{1}{2} O_{2}$
  - $N O_{2}$ is a brown gas.
Decomposition of Group 2 Carbonates:
- $MgCO_3 \longrightarrow MgO + CO_2$
- $CaCO_3 \longrightarrow CaO + CO_2$
- $SrCO_3 \longrightarrow SrO + CO_2$
- $BaCO_3 \longrightarrow BaO + CO_2$
Flue Gas Desulfurization:
- $SO_2 + CaO \longrightarrow CaSO_3$
- $CaSO_3 \xrightarrow{Further \ oxidation} CaSO_4$
Limewater Test:
- $Ca(OH)_2 + CO_2 \longrightarrow CaCO_3 + H_2O$ (White precipitate)
- $CaCO_3 + H_2O + CO_2 \longrightarrow Ca(HCO_3)_2$ ( $C a (H C O_{3})_{2}$ dissolves in water, so the precipitate disappears with further oxidation)
Reaction of Group 2 metals with water and steam
- $Ca + 2H_2O_{(l)} \longrightarrow Ca(OH)_2 + H_2$ (Calcium sinks in water)
- $Ca + H_2O_{(g)} \longrightarrow CaO + H_2$

Sulfur and Nitrogen

Formation of $N O_{x}$ :
- $N_2 + O_2 \longrightarrow 2NO$ (Intense heat caused by lightning, catalytic converters, and volcanoes)
- $2NO + O_2 \longrightarrow 2NO_2$ ( $N O_{2}$ is highly unstable)
Formation of Acid Rain:
- $2NO_2 + H_2O \longrightarrow HNO_3 + HNO_2$
- $HNO_2 + \frac{1}{2}O_2 \longrightarrow HNO_3$
- $2NO_2 + H_2O + \frac{1}{2}O_2 \longrightarrow 2HNO_3$ (Nitric Acid)
- $SO_2 + H_2O \longrightarrow H_2SO_3$ (Sulfurous Acid)
Dangerous Gases formed in Car Engines:
- $SO_2 + NO_2 \longrightarrow SO_3 + NO$
- $NO + \frac{1}{2}O_2 \longrightarrow NO_2$ (Regenerated)
- $SO_3 + H_2O \longrightarrow H_2SO_4$
Reaction in Rain Clouds: See Formation of Acid Rain
Catalytic Converters:
- Conditions: Pt/Pd as catalyst at 200°C, honeycomb ceramic surface
- Increases surface area
- Withstand high temperatures
- $2NO \longrightarrow N_2 + 2CO_2$
- $2CO + O_2 \longrightarrow 2CO_2$
- $C_8H_{18} + 12.5O_2 \longrightarrow 8CO_2 + 9H_2O$
Flue Gas Desulfurization: (See Group 2 reactions)
Natural Ozone Reactions:
- $O_2 \xrightarrow{UV \ Light} 2\dot{O}$
- $O_2 + \dot{O} \longrightarrow O_3$
- $O_3 \xrightarrow{UV \ Light} O_2 + \dot{O}$
Disrupted Ozone Reactions:
- $Cl_2 \xrightarrow{UV \ Light} 2Cl\cdot$
- $Cl\cdot + O_3 \longrightarrow ClO\cdot + O_2$
- $ClO\cdot + O_3 \longrightarrow Cl\cdot + 2O_2$ (Regenerated)
Ammonia as a Base:
- $NH_3 + HCl \longrightarrow NH_4Cl$
- $2NH_3 + H_2SO_4 \longrightarrow (NH_4)_2SO_4$
- $NH_3 + HNO_3 \longrightarrow NH_4NO_3$
- $NH_4Cl + NaOH \longrightarrow NaCl + NH_3 + H_2O$
- $(NH_4)_2SO_4 + 2NaOH \longrightarrow Na_2SO_4 + 2NH_3 + 2H_2O$
- $NH_4NO_3 + NaOH \longrightarrow NaNO_3 + NH_3 + H_2O$

Alcohols

Preparation of Alcohols: Hydration of Alkenes, Nucleophilic Substitution of Alkyl Halides, Reduction of Carbonyl Compounds, Reduction of Carboxylic Acids, Hydrolysis of Esters, Fermentation of Glucose
- $C_6H_{12}O_6 \xrightarrow{38^\circ C, \ no \ air, \ steam, \ Yeast} 2C_2H_5OH + 2CO_2$
Nucleophilic Substitution by HBr:
- $CH_3CH_2OH + HBr \longrightarrow CH_3CH_2Br + H_2O$ (HBr is toxic) *Mechanism: See source for a diagram of the mechanism.
Nucleophilic Substitution by Chlorination:
- $3CH_3CH_2OH + PCl_3 \longrightarrow 3CH_3CH_2Cl + H_3PO_3$ (Heat with $P C l_{3}$ )
- $CH_3CH_2OH + PCl_5 \longrightarrow CH_3CH_2Cl + POCl_3 + HCl$ $C H_{3} C H_{2} O H + PC l_{5} ⟶ C H_{3} C H_{2} Cl + POC l_{3} + H Cl$ (Reaction at r.t.p with $P C l_{5}$ $PC l_{5}$ )
  - White fumes of HCl observed
- $CH_3CH_2OH + SOCl_2 \longrightarrow CH_3CH_2Cl + HCl + SO_2$ (Heat $S O C l_{2}$ with pyridine as solvent, white fumes observed. Bleaches litmus paper)
Dehydration of Alcohols:
- $CH_3CH_2OH \xrightarrow{180^\circ C, H_2SO_4 \ catalyst, \ Heat} CH_2=CH_2 + H_2O$ *Mechanism: See source for a diagram of the mechanism.
Oxidation of Alcohols: *Conditions: Acidified $K_{2} C r_{2} O_{7}$ $K_{2} C r_{2} O_{7}$ or $K M n O_{4}$ $K M n O_{4}$ , Heat
- Primary Alcohol: $CH_3CH_2OH \xrightarrow{Distillation} CH_3CHO \xrightarrow{Further \ oxidation} CH_3CO_2H$ (Heat under reflux)
- Secondary Alcohol: $CH_3CH(OH)CH_3 \longrightarrow CH_3COCH_3$ (Forms Ketone)
- Tertiary Alcohol: No reaction
Reaction with Metals:
- $CH_3CH_2OH + Na \longrightarrow CH_3CH_2ONa + \frac{1}{2}H_2$
Reaction with Acids:
- $CH_3CH_2OH + CH_3CH_2OH \xrightarrow{Conc. \ H_2SO_4} CH_3CH_2OCH_2CH_3 + H_2O$
Combustion:
- Complete: $CH_3CH_2OH + 3O_2 \longrightarrow 2CO_2 + 3H_2O$
- Incomplete: $CH_3CH_2OH + 2O_2 \longrightarrow 2CO + 3H_2O$ and $CH_3CH_2OH + O_2 \longrightarrow 2C + 3H_2O$
Lucas Test:
- $CH_3CH_2OH + HCl \xrightarrow{ZnCl_2, Heat} CH_3CH_2Cl + H_2O$
- Observations:
- Primary Alcohol: No cloudiness until strong heating
- Secondary Alcohol: Cloudiness in 5 minutes
- Tertiary Alcohol: Immediate cloudiness

Carbonyl Compounds

Formation of Carbonyl Compounds: Oxidation of Alcohols
Nucleophilic Addition of HCN:
- $CH_3CHO + HCN \xrightarrow{Trace \ amounts \ of \ NaCN} CH_3CH(OH)(CN)$ *Mechanism: See source for a diagram of the mechanism.
Reduction of Carbonyl Compounds
- Reagents: $N a B H_{4}$ in $H_{2} O$ , $L i A l H_{4}$ in dry ether, $Na_{(s)}$ in ethanol
- Aldehydes: $CH_3CHO + [H] \longrightarrow CH_3CH_2OH$ (Forms Primary Alcohol)
- Ketones: $CH_3COCH_3 + [H] \longrightarrow CH_3CH(OH)CH_3$ (Forms Secondary Alcohol)
Condensation Reactions of Carbonyl Compounds:
- Reagent: 2,4-DNPH
- Observation: Initial - Yellow or orange solution, Final - Yellow or orange precipitate
- See source for a diagram of the reaction mechanism.
Nitrile Reactions:
- Hydrolysis: $CH_3CH(CN)OH \xrightarrow{Dilute \ HCl, Heat \ under \ reflux} CH_3CH(COOH)OH$ (Lactic Acid)
- Reduction: $CH_3CH(CN)OH \xrightarrow{Na_{(s)} \ in \ ethanol} CH_3CH(CH_2NH_2)OH$
Tollen's Test:
- Example Reagent: Aldehyde ( $C H_{3} C H O$ )
- Output: $C H_{3} C O O H + 2 A g$ (Silver mirror forms if the test is positive)
- A silver mirror is formed only if the reagent is an aldehyde
Fehling's Test:
- Testing Reagent: Copper (II) Tartarate in alkaline solution (Light blue solution)
- Example Reagent: Aldehyde ( $C H_{3} C H O$ )
- Output: $C H_{3} C O_{2} H + C u_{2} O$ (Brick-red precipitate)
- A brick-red precipitate is formed only if the reagent is an aldehyde

Carboxylic Acids

Formation of Carboxylic Acids: Oxidation of Primary Alcohols, Oxidation of Aldehydes, Hydrolysis of Esters (Acidic Hydrolysis), Hydrolysis of Nitriles
Reaction with Metals:
- $CH_3CO_2H + Na \longrightarrow CH_3CO_2Na + \frac{1}{2}H_2$
Reaction with Carbonates:
- $2CH_3CO_2H + Na_2CO_3 \longrightarrow 2CH_3CO_2Na + CO_2 + H_2O$
Reaction with Bases:
- $CH_3CO_2H + NaOH \longrightarrow CH_3CO_2Na + H_2O$
Reactions with Alcohols (Esterification)
- $CH_3CO_2H + CH_3CH_2OH \xrightarrow{Conc. \ H_2SO_4 \ catalyst} CH_3CO_2CH_2CH_3 + H_2O$
Reduction
- $CH_3CO_2H + 4[H] \xrightarrow{LiAlH_4 \ in \ dry \ ether} CH_3CH_2OH + H_2O$
Reaction with Chlorinating Agents:
- $CH_3CO_2H + SOCl_2 \longrightarrow CH_3COCl + SO_2 + HCl$
- $CH_3CO_2H + PCl_5 \longrightarrow CH_3COCl + POCl_3 + HCl$
Hydrolysis of Esters:
- Acidic: $CH_3CO_2CH_2CH_3 \xrightarrow{Dilute \ HCl, Heat \ Under \ Reflux} CH_3CO_2H + CH_3CH_2OH$
- Alkaline: $CH_3CO_2CH_2CH_3 \xrightarrow{NaOH(aq), Room \ Temperature} CH_3CO_2Na + CH_3CH_2OH$

Iodoform Test

Reagent: Iodine in alkaline solution with heat provided
Test is positive for: Substances with a $C H_{3} - C (= O) - R$ structure, and Alcohols that oxidize to form

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