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ICSE Class 10 Chemistry Question 3 of 93

Organic Chemistry — Question 15

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15
Question

Question 15.1

Give equations for the conversions of – Methane, Ethane:

Methane toEthane to  
(a) Carbon tetrachloride(a) Hexachloro ethaneby - Substitution [diffused sunlight]
(b) Carbon dioxide(b) Carbon dioxideby - Oxidation - Complete
(c) Methanol
to
Methanal
to
Methanoic acid		Ethanol
to
Ethanal
to
Ethanoic acid		by - Oxidation
(i) catalytic using - catalyst copper [Cu]
(ii) Controlled using acidified K2Cr2O7
(d) MethnalEthanalby- Oxidation - Catalytic - using catalyst MoO
(e) EthyneEtheneby - Pyrolysis [dehydrogenation]
Answer

(a) Conversion of Methane to Carbon tetrachloride by substitution [diffused sunlight]:

CH4 methane+4Cl2→Δdiffused sunlightCCl4Carbon tetrachloride+4HCl\underset{\text{ methane} }{\text{CH}_4} + 4\text{Cl}_2 \xrightarrow[\Delta]{\text{diffused sunlight}} \underset{\text{Carbon tetrachloride}}{\text{CCl}_4} + 4\text{HCl}

(b) Conversion of Methane to Carbon dioxide by complete oxidation:

CH4 methane+2O2[excess]⟶CO2+2H2O+Δ\underset{\text{ methane} }{\text{CH}_4} + 2\text{O}_2\text{[excess]} \longrightarrow \text{CO}_2 + 2\text{H}_2\text{O} + \Delta

(c)(i) Conversion of Methane to Methanol to Methanal to Methanoic acid by catalytic oxidation using catalyst copper [Cu]:

2CH4 methane+O2→200°CCu tube2CH3OHmethanol2CH3OHmethanol+O2→catalystCu2HCHOmethanal+2H2O2HCHOmethanal+O2→catalystCu2H-COOHmethanoic acid\underset{\text{ methane}}{2\text{CH}_4} + \text{O}_2 \xrightarrow[200 \text{\degree C}]{\text{Cu tube}} \underset{\text{methanol}}{2\text{CH}_3\text{OH}} \\[1em] \underset{\text{methanol}}{2\text{CH}_3\text{OH}} + \text{O}_2 \xrightarrow[\text{catalyst}]{\text{Cu}} \underset{\text{methanal} }{\text{2HCHO}} + 2\text{H}_2\text{O} \\[1em] \underset{\text{methanal} }{\text{2HCHO}} + \text{O}_2 \xrightarrow[\text{catalyst}]{\text{Cu}} \underset{\text{methanoic acid} }{\text{2H-COOH}}

(c)(ii) Conversion of Methane to Methanol to Methanal to Methanoic acid by controlled slow oxidation using acidified K2Cr2O7:

CH4 Methane→K2Cr2O7[O]CH3OH methanol→K2Cr2O7[O]HCHO methanal→K2Cr2O7[O]HCOOHmethanoic acid\underset{\text{ Methane} }{\text{CH}_4} \xrightarrow[\text{K}_2\text{Cr}_2\text{O}_7]{\text{[O]}} \underset{\text{ methanol}}{\text{CH}_3\text{OH}} \xrightarrow[\text{K}_2\text{Cr}_2\text{O}_7]{\text{[O]}} \underset{\text { methanal}}{\text{HCHO}} \xrightarrow[\text{K}_2\text{Cr}_2\text{O}_7]{\text{[O]}} \underset{\text{methanoic acid} }{\text{HCOOH}}

(d) Conversion of Methane to Methanal by catalytic oxidation using catalyst MoO:

CH4 methane+O2→350−500°CMoOHCHOmethanal+H2O\underset{\text{ methane}}{\text{CH}_4} + \text{O}_2 \xrightarrow[350 - 500 \text{\degree C}]{\text{MoO}} \underset{\text{methanal} }{\text{HCHO}} + \text{H}_2\text{O}

(e) Conversion of Methane to Ethyne by Pyrolysis [dehydrogenation]:

2CH4 methane→1500°CC2H2ethyne+3H2\underset{\text{ methane}}{2\text{CH}_4} \xrightarrow{1500 \degree \text{C}} \underset{\text{ethyne} }{\text{C}_2\text{H}_2} + 3\text{H}_2

(a) Conversion of Ethane to Hexachloro ethane by substitution [diffused sunlight]:

C2H6 ethane+Cl2→diffused sunlightΔC2H5Clmonochloroethane+HCl\underset{\text{ ethane} }{\text{C}_2\text{H}_6} + \text{Cl}_2 \underset{\Delta}{\xrightarrow{\text{diffused sunlight}}} \underset{\text{monochloroethane}}{\text{C}_2\text{H}_5\text{Cl}}+ \text{HCl}

C2H5Clmonochloroethane+Cl2[excess]⟶C2H4Cl2dichloroethane+HCl\underset{\text{monochloroethane} }{\text{C}_2\text{H}_5\text{Cl}} + \underset{\text{[excess]}}{\text{Cl}_2} \longrightarrow \underset{\text{dichloroethane}}{\text{C}_2\text{H}_4\text{Cl}_2}+ \text{HCl}

C2H4Cl2dichloroethane+Cl2⟶C2H3Cl3trichloroethane+HCl\underset{\text{dichloroethane}}{\text{C}_2\text{H}_4\text{Cl}_2} + \text{Cl}_2 \longrightarrow \underset{\text{trichloroethane}}{\text{C}_2\text{H}_3\text{Cl}_3}+ \text{HCl}

C2H3Cl3trichloroethane+Cl2⟶C2H2Cl4tetrachloroethane+HCl\underset{\text{trichloroethane}}{\text{C}_2\text{H}_3\text{Cl}_3} + \text{Cl}_2 \longrightarrow \underset{\text{tetrachloroethane}}{\text{C}_2\text{H}_2\text{Cl}_4}+ \text{HCl}

C2H2Cl4tetrachloroethane+Cl2⟶C2HCl5pentachloroethane+HCl\underset{\text{tetrachloroethane}}{\text{C}_2\text{H}_2\text{Cl}_4} + \text{Cl}_2 \longrightarrow \underset{\text{pentachloroethane}}{\text{C}_2\text{H}\text{Cl}_5}+ \text{HCl}

C2HCl5pentachloroethane+Cl2⟶C2Cl6hexachloroethane+HCl\underset{\text{pentachloroethane}}{\text{C}_2\text{H}\text{Cl}_5} + \text{Cl}_2 \longrightarrow \underset{\text{hexachloroethane}}{\text{C}_2\text{Cl}_6}+ \text{HCl}

(b) Conversion of Ethane to Carbon dioxide by complete oxidation:

2C2H6 ethane+7O2[excess]⟶4CO2+6H2O+Δ\underset{\text{ ethane}}{2\text{C}_2\text{H}_6} + 7\text{O}_2\text{[excess]} \longrightarrow \text{4CO}_2 + 6\text{H}_2\text{O} + \Delta

(c)(i) Conversion of Ethane to Ethanol to Ethanal to Ethanoic acid by catalytic oxidation using catalyst copper [Cu]:

2C2H6 ethane+O2→200°CCu tube2C2H5OHethanol2C2H5OHethanol+O2→catalystCu2CH3CHOethanal+2H2O2CH3CHOethanal+O2→catalystCu2CH3COOHethanoic acid\underset{\text{ ethane}}{2\text{C}_2\text{H}_6} + \text{O}_2 \xrightarrow[200 \text{\degree C}]{\text{Cu tube}} \underset{\text{ethanol}}{2\text{C}_2\text{H}_5\text{OH}} \\[1em] \underset{\text{ethanol}}{2\text{C}_2\text{H}_5\text{OH}} + \text{O}_2 \xrightarrow[\text{catalyst}]{\text{Cu}} \underset{\text{ethanal}}{2\text{CH}_3\text{CHO}} + 2\text{H}_2\text{O} \\[1em] \underset{\text{ethanal}}{2\text{CH}_3\text{CHO}} + \text{O}_2 \xrightarrow[\text{catalyst}]{\text{Cu}} \underset{ \text{ethanoic acid} }{2\text{CH}_3\text{COOH}}

(c)(ii) Conversion of Ethane to Ethanol to Ethanal to Ethanoic acid by controlled slow oxidation using acidified K2Cr2O7:

C2H6 Ethane→K2Cr2O7[O]C2H5OHethanol→K2Cr2O7[O]CH3CHOethanal→K2Cr2O7[O]CH3COOHethanoic acid\underset{\text{ Ethane} }{\text{C}_2\text{H}_6} \xrightarrow[\text{K}_2\text{Cr}_2\text{O}_7]{\text{[O]}} \underset{ \text{ethanol}}{\text{C}_2\text{H}_5\text{OH}} \xrightarrow[\text{K}_2\text{Cr}_2\text{O}_7]{\text{[O]}} \underset{\text{ethanal}}{\text{CH}_3\text{CHO}} \xrightarrow[\text{K}_2\text{Cr}_2\text{O}_7]{\text{[O]}} \underset{\text{ethanoic acid}}{\text{CH}_3\text{COOH}}

(d) Conversion of Ethane to Ethanal by catalytic oxidation using catalyst MoO:

C2H6 ethane+O2→350−500°CMoOCH3CHOethanal+H2O\underset{\text{ ethane}}{\text{C}_2\text{H}_6} + \text{O}_2 \xrightarrow[350 - 500 \text{\degree C}]{\text{MoO}} \underset{\text{ethanal} }{\text{CH}_3\text{CHO}} + \text{H}_2\text{O}

(e) Conversion of Ethane to Ethene by Pyrolysis [dehydrogenation]:

C2H6 ethane→catalyst [Al2O3]500°CC2H4ethene+H2\underset{\text{ ethane}}{\text{C}_2\text{H}_6} \xrightarrow[\text{catalyst [Al}_2\text{O}_3\text{]}]{500 \degree \text{C}} \underset{\text{ethene}}{\text{C}_2\text{H}_4} + \text{H}_2

Chapter Overview: Organic Chemistry

Organic Chemistry is the study of carbon compounds. Carbon's unique ability to form four covalent bonds and catenate (form long chains) makes organic chemistry vast and diverse. The ICSE syllabus covers hydrocarbons (alkanes, alkenes, alkynes), their nomenclature (IUPAC), structural formulae, isomerism, and characteristic reactions. Alkanes (CnH2n+2) are saturated hydrocarbons that undergo substitution reactions. Alkenes (CnH2n) and alkynes (CnH2n−2) are unsaturated and undergo addition reactions. Students learn homologous series, functional groups, and the distinction between saturated and unsaturated compounds. The chapter introduces alcohols (with −OH group) and carboxylic acids (with −COOH group) as basic functional group chemistry. Students must write structural formulae, name compounds using IUPAC rules, and understand reactions like combustion, substitution, and addition. Practical tests like decolourising bromine water or acidified KMnO4 to distinguish between saturated and unsaturated compounds are important.

Key Concepts & Homologous Series

Term / Series Details
CatenationAbility of carbon to form bonds with other carbon atoms, creating chains and rings
Homologous SeriesFamily of compounds with same general formula and functional group, differing by CH2
AlkanesCnH2n+2; single bonds only; saturated (e.g., CH4, C2H6)
AlkenesCnH2n; one C=C double bond; unsaturated (e.g., C2H4, C3H6)
AlkynesCnH2n−2; one C≡C triple bond; unsaturated (e.g., C2H2, C3H4)
IsomerismCompounds with same molecular formula but different structural arrangements
Functional GroupAtom or group responsible for characteristic chemical properties (−OH, −COOH, C=C)
IUPAC NamingPrefix (substituent) + Root (chain length) + Suffix (functional group)

Must-Know Concepts

  • Carbon prefixes: Meth- (1C), Eth- (2C), Prop- (3C), But- (4C), Pent- (5C)
  • Combustion: CH4 + 2O2 → CO2 + 2H2O (complete); 2CH4 + 3O2 → 2CO + 4H2O (incomplete)
  • Substitution: CH4 + Cl2 → CH3Cl + HCl (in presence of UV light)
  • Addition: C2H4 + Br2 → C2H4Br2 (ethene decolourises bromine water)
  • Unsaturated compounds decolourise bromine water and acidified KMnO4; saturated compounds do not
  • Ethanol: C2H5OH; Ethanoic acid: CH3COOH (vinegar); Ester: CH3COOC2H5 (fruity smell)
  • Isomers of butane (C4H10): n-butane and isobutane (2-methylpropane)

Saturated vs Unsaturated Hydrocarbons

Feature Saturated (Alkanes) Unsaturated (Alkenes/Alkynes)
BondsOnly single bonds (C−C)Double (C=C) or triple (C≡C) bonds
Typical ReactionSubstitutionAddition
Bromine WaterNo decolourisationDecolourised
CombustionClean blue flameSmoky/luminous flame (higher C%)

Important Diagrams to Practice

  • Structural formulae of first five members of alkanes, alkenes, and alkynes
  • Isomers of butane and pentane with structural formulae
  • Laboratory preparation of ethylene from ethanol (dehydration)

Common Mistakes

  • Writing wrong general formulae (alkenes are CnH2n, NOT CnH2n+2)
  • Confusing substitution (alkanes) with addition (alkenes) reactions
  • Not showing all bonds in structural formulae
  • IUPAC naming errors: not selecting the longest carbon chain or wrong numbering
  • Forgetting conditions (UV light for substitution, Ni catalyst for hydrogenation)

Scoring Tips

  • Draw clear structural formulae showing every C-H and C-C bond
  • For IUPAC naming: identify longest chain, number from the end nearest to substituent/functional group
  • Always mention conditions (catalyst, temperature, UV) in reaction equations
  • Practice writing isomers for C4H10, C5H12, and C4H8

Frequently Asked Questions

Why is carbon's chemistry so vast?

Carbon has four valence electrons and can form four strong covalent bonds. Its small size allows strong C-C bonds, enabling catenation (long chains, branches, rings). This versatility leads to millions of organic compounds.

How do you test whether a hydrocarbon is saturated or unsaturated?

Add bromine water to the hydrocarbon. If the orange-brown colour of bromine water is decolourised, the compound is unsaturated (alkene or alkyne). If the colour persists, it is saturated (alkane).

What is the difference between structural isomers?

Structural isomers have the same molecular formula but different structural arrangements of atoms. For example, n-butane has a straight chain while isobutane (2-methylpropane) has a branched chain. They have different physical properties despite the same formula.