organic chemistry 600 points by Sir Shamsul Amin

CHAP# 1 ORGANIC COMPOUNDS

1. Organic chemistry deals with carbon based compounds.

2. The world organic means life or living.

3. In 1928, friedrich Wohler synthesized urea from ammonium cyanate.

4. The compounds which contain carbon but nor organic are :

• Carbon containing alloys

• Simple oxides of carbon

• Allotropes of carbon

• Metal carbonates

• Bicarbonates

• Carbonyls

• Cyanides

• Cyanates

• Sulfides

5. Major sources of organic compounds are;

• Fossil remains

• Petroleum

• Natural gas

6. Coal occurs in rock strata in layers called coral beds.

7. Coal formation:

Wood → Peat → Coal

8. Coal exists in different forms like:

• Lignite (low C %)

• Sub- Bituminous coal

• Bituminous coal

• Anthracite (high C %)

9. Coal is major source of aromatic compounds.

10. Petroleum means crude oil

11. Petroleum is also called mineral oil/ crude oil/ liquid gold.

12. Petroleum includes only crude oil in strict sense.

13. Petroleum includes both crude oil and natural gas in common sense.

14. Natural gas and petroleum are found in association with each other.

15. Anticancer agent palliate (Taxol) are obtained from yew tree.

16. Antimalarial agent artemissin are obtained from Artimisia annual.

17. The study of processes and chemical reaction by which organic compounds are made are called Synthetic organic chemistry.

18. An intermediate product of a reaction is used to synthesize a target process is called partial synthesis.

19. Sometime the starting material converts through many steps into targeted products. Such process is called total synthesis.

20. Urea process of Friedrich was commercialized for the first time by Gustaf Kompa from the synthesis of camphor in 1913.

21. Some products of Biotechnology:

• Benzylpencilin → an antibiotic

• Insulin → A hormone

• Polyhydroxybutyrate → A Biodegradable thermoplastics

• Renin → an enzyme  Chemosensory protein(CSP)

22. Destructive distillation of coal:

• Coke → a reducing agent

• Coal tar → used for fertilizer making

• Coal gas

• Ammoniacal liquor → mixture of hydrogen and carbon monoxide

23. Coal gas is also called town gas.

24. Coal is converted to petroleum by Fischer-Tropsch process.

25. A hydrogen and carbon monoxide is converted into alkane by Fischer –Tropsch process.

26. The conversion of source of carbon into gaseous reactants like CO and H₂ in Fishceher-Tropsch plant is called Gasification.

27. The self-linkage of carbon atom to form chains and ring compounds is called Catenation.

28. Two or more compound having same molecular formula but different structural formula is called isomers and this property is called isomerism.

29. Characteristics of organic compounds are;

• Unique properties of carbon like catenation.

• Isomerism

• None-ionic character

• Solubility

• Rates of organic reactions

• Similar structural features and behavior

30. The mostly bonds of organic compounds are covalent which are none-polar.

31. Most of organic compounds are insoluble in water buit soluble in none-polar solvents.

32. The organic reactions are slow because they involves breaking of some bonds and formation of new bonds.

33. Life molecules includes:  Proteins

• Nucleic acids

• Enzymes

• Fats

• Lipids etc

34. Many farmers in USA grow maize for ethanol.

35. Quinonee → antimalarial

36. Aspirine → cardiac disease and pain killer

37. Borneol → anti-inflammatory

38. Benzyle benzoate → scabicide

39. Galantamine hydrobromide → alzheimer’s disease

40. The first fullerenes was discovered in 1885 by Herold Kroto, James Heath, Seam O’Brion, Robert Curl and Richard Smalley.

41. In 2010, fullerenes were also discovered in outer space.

42. Some fullerenes are:

• C₂₀

• _C60

• C₇₀

• C₇₆

• C₈₄

→ Smallest is C₂₀but most common I sC_60.

43. Benzene ring is present in aromatic compound.

44. Organic compound types are

 Hydrocarbons

1. Alkane

2. Alkene

3. alkynes

 Derivatives of hydrocarbons

1. Alkyl halide

2. Alcohol

3. Phenol

4. Ether

5. Ketones

6. Carboxylic acids

7. Aldehydes etc

45. An atom or group of atom that gives certain characteristics properties to an organic compound is called a functional group.

46. Functional group is chemically active part of molecule.

47. A series of organic compounds that are differ by methylene group and have same structural and chemical characteristics are called homologous series.

48. Alkane → C_nH_{2n + 2}

49. Cycloalkanes → C_nH_2n

50. Alkenes → C_nH_2n

51. Alkynes → C_nH_{2n - 2}

52. Alkyl → C_nH_{2n + 1}

53. Characteristics of homologous series:

• Each series have its own formula.

• Members of series have same chemical properties.

• Series members have same method of preparation.

• Physical properties increase with increase in molecular mass.

54. Extract sodium test or Lassaign’s solution(L.S) is prepared by heating the substance with sodium metal in fusion tube till tube become hot and after cooling its filtered.

55. Detection of Carbon in organic compounds

O.C + CuO →CO₂

CO₂+ Ca(OH)₂→ CaCO₃ milky colour

56. Detection of Hydrogen in organic compounds

O.C + CuO →H₂O

H₂O + CuSO₄CuSO₄.5H₂Oblue colour

57. Detection of Nitrogen in organic compounds

L.S + NaOH + FeSO₄ boil-cool +FeCl₃+ HCl/H₂SO₄prussian blue or green colour

58. Detection of Sulphur

L.S +acetic acid + lead acetate black ppt of lead sulphide

59. Detection of Halogens in organic compounds L.S + conc nitric acid +silver nitrate solution →

ü White ppt soluble in ammonium hydroxide indicate Chlorine

ü Yellow ppr slightly soluble in ammonium hydroxide indicate Bromine

ü Deep yellow ppt insoluble in ammonium hydroxide indicate Iodine

60. Detection of Oxygen in organic compounds

ü Can’t be test directly

ü Tests for oxygen containing functional group

ü Formation of water in nitrogen atmosphere

ü Combustion analysis

CHAP# 2 HYDROCARBONS

61. Hydrocarbons are organic compounds that contain carbon and hydrogen only.

62. Petroleum, natural gas and coal are main natural sources of hydrocarbons.

63. The parent member of aromatic hydrocarbons are benzene.

64. The formula of benzene is C₆ H₆.

65. Unsaturated hydrocarbons containing double bond are called alkenes.

66. Unsaturated hydrocarbons containing triple bond are called alkynes.

67. Saturated cyclic hydrocarbon are called cycloalkanes.

68. Unsaturated cyclic hydrocarbons are called cycloalkenes and cycloalkynes.

69. The systematic process of naming of compound is called nomenclature.

70. Some common names or trivial names of compounds are:

• HCOOH →Formic Acid

• CH₃ COOH →Acetic Acid

71. International union of pure and applied chemistry in 1957 set rules for symmetric names of organic compounds on the basis on structure. This is known is IUPAC system of nomenclature.

72. The prefix n is used for organic compound having continuous chain.

73. The prefix iso is used for those alkanes having attached methyl group to second last carbon.

74. The prefix neo is used before alkane having two methyl groups attached to second last carbon atom.

75. Cyclopropane is represented by a triangle.

76. Cyclobutane is represented by a square.

77. Cyclopentane is represented by a pentagon.

78. Cyclohexane is represented by a hexagon.

79. The ring is taken is substituent in naming cycloalkanes if it contain less carbon atoms than straight chain attached carbons.

80. First four cycloalkanes are colourless gases.

81. C₅ – C₁₇ are colourless liquids.

82. Onward from C₁₇, alkanes are wax like soft solids.

83. Alkanes are none-polar so insoluble in water.

84. Alkanes are soluble in CCl₄ and C₆ H₆.

85. B.P of alkanes increases with molecular weight.

→ Propane > Ethane > Methane

→ Decane > Noneane > Octane

86. Straight chain alkane have high B.P than isomeric branch chain

→ pentane > iso-pentane

→ hexane > iso hexane >neo-hexane

87. Melting point of alkane increase with molecular weight.

→ Propane > Ethane > Methane

→ Decane > Noneane > Octane

88. There is no regularity in the melting point of alkane with the no of carbon atoms in molecule.

89. The specific gravity of alkanes normally increase with molecular weight.

90. Viscosity of alkanes increase with increase in no of carbon atoms.

→ Propane > Ethane > Methane

→ Decane > Noneane > Octane

91. Cyclopropane and cyclobutane are gases while rest of cycloalkanes are liquids.

92. Melting point and boiling point of cycloalkanes increase with increase in no of carbon atoms.

93. Hybridization in alkane is sp³. 94. Hybridization in alkene is sp².

95. Hybridization in alkyne is sp¹.

96. Angle in alkane is 109.5^o.

97. Angle in alkene is 120^o.

98. Angle in alkyne is 180^o.

99. The geometry of alkane is tetrahedral.

100. The geometry of alkene is planar.

101. The geometry of alkyne is linear.

102. The deviation of normal tetrahedral angle of 109.5⁰ to 60⁰ is called angle strain.

103. Distance between carbon carbon single bond is 1.54⁰A.

104. Distance between carbon carbon double bond is 1.34⁰A.

105. Distance between carbon carbon triple bond is 1.19⁰A.

106. Distance between carbon Hydrogen single bond is 1.09⁰A.

107. Alkanes are also called Paraffins (little affinity).

108. Alkenes are also called Olefins.

109. Alkynes are also called Acetylenes.

110. Electronegativity of carbon is 2.5.

111. Electronegativity of hydrogen is 2.1.

112. Cyclopropane and cyclobutane have greater angle strain and hence undergoes ring opening reactions.

113. Cycleproapne undergo ring opening reaction with H₂/Ni and HBr to give open chain products.

114. Cyclobutane undergo ring opening reaction under severs conditions.

115. Stability of cycloalkanes:

→ cyclohexane > cyclopentane > cyclobutane > cyclopropane

116. A substituent reaction can be initiated by

• Nucleophile  Electrophile

• Free radical

117. The product of hemolytic bond fission are free radicals.

118. The product of heterolytic bond fissions are ions.

119. Electrophile can accept an electron pair.

120. Nucleophile can donate lone pair of electron.

121. An electrophile may be positive ion are neutral molecules with electron deficient centre.

122. A nucleophile may be negative are neutral molecule with lone pair of electrons.

123. Substitution reactions, which are initiated by free radical are called free radical substitution reaction.

124. Example of substitution reaction by radical are chlorination of methane and ethane.

125. In chlorination of methane, if Cl₂ is taken in excess, the major product will CCl₄.

126. In chlorination of methane, if Cl₂ is taken in limited, the major product will CH₃Cl.

127. Combustion of methane gives 890.95 kJ / mol.

128. Combustion of ethane gives 1559 kJ /mol.

129. Along with water molecule combustion of ethane in

• sufficient O₂gives CO₂

• limited O₂ gives CO

• very limited O₂ gives C

130. Lower members of alkenes gives oily product on treatment with chlorine or bromine.

131. In common system alkenes are named as alkylene.

132. In IUPAC system alkenes are named as alkanes.

133. Energy released by combustions;

• 1-butene →2719 kJ/mol

• Cis-2-butene →2712 kJ/mol

• Trans-2-butene →2707 kJ/mol  Isobutylene → 2703 kJ/mol

*(BSTI)

134. Stability of Butene are as:

→1-butene < cis-2-butene < trans-2-butene < Isobutylene

135. Greater no of alkyl groups attached, greater is the stability of alkenes. isobutylene is more stable than 1.butene

136. Dehydrahion of alcohol at 1700⁰ C in presence of sulphuric acid gives alkene.

137. Dehydrohalogenation of alkyl halide in presence of alcoholic solution of KOH/NaOH gives alkene and alkyl halide.

138. The hydrogenation of alkenes is industrially used for the conversion of vegetable oils into ghee.

139. Hydrogenation of alkene is done at 200-250^o C.

140. Hydrohalogenation of alkenes gives alkyl halide. 141. The order of reactivity of halogens are

→ F₂ > Cl₂ > Br₂ > I₂

142. The reactivity of halogen acids are

→ HI > HBr > HCl > HF

143. Markovnikov,s Rule: when polar reagent is added to unsymmetrical alkene, the positive part of reagent attaches itseld to that carbon atom involved in the double bond holding greater no of hydrogen atoms.(+ → H or H → H)

144. The major product of propene with HBr is 2-Bromopropane not 1Bromopropane.

145. Alkenes react with H₂SO₄ to produce hydrogen sulphates, which on hydrolysis yields alcohol at 100^oC.

146. Alkenes react with halogens in presence in presence of inert solvent like CCl₄ forms dihaloalkanes(vicinal dihalides).

147. The bromination of alkenes provides a useful test for the presence of double bond.

148. The colour of bromine rapidly discharge as the colourless dibromo compound is formed.

149. Alkene react with hypohalous acids (X-OH) to form halohydrins.

150. Halohydrins are organic compound having hydroxyl group and halogen at adjacent carbon atom.

151. Alkenes react with oxygen in the presence of silver catalyst at temperature 300⁰C to epoxides.

152. Epoxides on acid hydrolysis produce glycol.

153. When ozone is passed through alkene in presence of inert solvent like CCl₄to form ozonide.

154. Ozonide are being explosive cannot be isolated.

155. Ozonide on treatment with Zn and water cleavage at position of double bond to form carbonyl compounds.

156. Ozonolysis is done for locating the position of the double bond in unknown alkene.

157. The process by which simple molecules chemically join together to form large molecules with high molecular weight, is called polymerization.

158. Polyethylene are also known as polyethene.

159. The temperature for polymerization of ethane is 100-300⁰C with pressure of 1K-2K atm.

160. Conjugated molecules re those compounds in which the carbon ateoms are linked together by alternating single and double bonds 161. Example of conjugated molecules are:

• 1,3 –butadiene

• Benzene

162. The CC single bond in1,3-Butadiene are 1.48^oA not 1.54^oA. 163. The CC double bond in1,3-Butadiene are 1.37^oA not 1.33^oA 164. There are two main types of isomerism:

• Structural isomerism

Ø Chain isomerism or skeletal isomerism

Ø Position isomerism

Ø Functional group isomerism

Ø Metamerism

Ø tautomerism

• Stereoisomerism

Ø Geometric or cis-trans isomerism

Ø Opticle isomerism

165. A structural feature within a molecule that is responsible for its chirality is called chiral centre, of the molecule.

166. A carbon bonded to four different groups is called chiral carbon atom or asymmetric carbon atom foe example lactic acid.

167. A molecule may not have a chiral atom but still be chiral.

168. A molecule may have one chiral atom but still be achiral.

169. Optical activity of a compound is measured by an instrument called polarimeter.

170. Nicol prism made of calcite, CaCO₃ act as polarizer.

171. Isomer that rotate the plane of polarized light to right or clockwise direction is called dextrorotatory isomer or + isomer.

172. Isomer that rotate the plane of polarized light to left or anticlockwise direction is called Levorotatory isomer or – isomer.

173. Optical isomerism is type of isomerism in which the isomer differ in their interaction towards plane polarized light.

174. Two mirror images of single compound that cannot be superimpose are called enantiomers of each other

175. Isomers have different configuration.

176. Three dimensional arrangement of atoms in space is called configuration.

177. The isomer having two same groups on one side of double bond is called cis isomer. *(cis=same)

178. The isomer having two similar groups of on opposite side of double bond is called trans isomeri.

179. Isomerism due to unequal distribution of carbon atoms on either side of functional group is called Metamerism.

180. A special type of isomerism in which isomer are in dynamic equilibrium with each other is called Tautamerism.

181. Functional group isomerism have same molecular formula but different structural formula.

182. In common system, the first member of alkyne series are named as acetylene.

183. Relative stability of alkynes depends on:

ü Position of triple bond

ü No of substituents

ü Nature of substituents

184. Ethyne, propyne and butyne are gases.

185. C₅– C₁₂ alkynes are liquids and higher are solids at room temperature and pressure.

186. All alkynes are odourless and colourless except acetyls.

187. Acetylene has garlic like odour.

188. Alkanes are insoluble in water.

189. Alkynes are slightly soluble in water.

190. The boiling point of alkyne is higher than corresponding alkane

• pentyne > pentene

• hexyne > 195exane

191. The boiling point of alkynes increase with increase in no of carbon atoms.

• Heptyne > Hexyne > Pentyne

• Butyne > Propyne > Etyhne

192. The melting point of alkynes did not show regular pattern. 193. Alkenes are more denser than alkane and alkene 194. Which one of the following is more denser?

ü Alkane ü Alkene

ü Alkyne ←

195. Compounds having two halogens atoms on adjacent carbon atoms are called vicinal dihalides.

196. Vicinal dihalides when treated with alcoholic KOH followed by NaNH₂ in liquid ammonia forms alkynes.

197. Dehydrohalogination of tetrahalides leads to alkyne.

198. Alkynes are less reactive than alkene.

199. Which one of the following is more reactive?

• Alkane

• Alkene ←

• Alkyne

200. Alkynes in which the triple bond is present at the end of th chain is called terminal alkyne or 1-alkynes.

201. Terminal alkyne and acetylene are acidic in nature.

202. If acetylene or terminal alkyne is treated with solution of sodium amide (NaNH₂) in liquid ammonia, sodium acetylide is obtained.

203. Acetylene and 1-alkyne react with ammoniacal solutions of cuprous chloride and silver nitrate to form acetylides and alkynides of these metals.

204. Copper acetylide → red ppt *(CAR)

205. Silver acetylide → white ppt *(SAW)

206. Copper and cilver acetylides are highly explosives in dry conditions. They are decomposed by acids such as HNO₃ to regenerate acetylene.

207. None-terminal alkynes can be distinguisher from terminal alkynes by Cu₂Cl₂and NH₄ OH or Ag(NO₃ )₂ and NH₄ OH

208. Addition reactions of alkynes are:

Ø Hydrogenation → alkenes

Ø Reduction by dissolving metal → alkynides/ acetylides

Ø Hydrohalogenation → haloalkane

Ø Hydration → carbonyl compounds

Ø Halogination → tetrahaloalkane

Ø Ozonolysis → ozonides →ketones → carboxylic acids

209. Hydrogenation of alkynes leads to alkene and onward to form alkane the reaction is stopped by poisoning Pd catalyst with BaSO₄+ quinolone (lindlar’s catalyst).

210. 1-alkynes and terminal alkynes react with metals in liquid ammonia to form salts like alkynides or acetylides.

211. Alkynes react with water inpresence of mercurin acid or sulphuric acid to form carbonyl compounds,

• Acetylene/ethyne → aldehyde

• Propyne or higher → ketones

212. Alkynes react with ozone to form ozonide.

213. Ozonide may be decomposed by water to give ketones.

214. Ketones are foxidized by H₂O₂ to form carbonyl compounds.

215. Special names of benzene with attached substituent:

• Toluene → CH₃

• Phenol →OH

• Alinine →NH₂

• Nezoic acid →COOH

• O-xylene, m-xylene, p-xylene → 2 CH₃

• Catechol, resorcinol, hydroquinonee → 2OH

• Mesitylene → 3 CH₃

• Durene → 4 CH₃

• Nepthalane → 2 benzene

• Anthracene → 3 benzene

216. Bezene is colourless liquid at room temperature and pressure.

217. Benzene has pecular smell and burning tastes. 218. The specific gravity of benzene is0.8788.

219. M=benzene melts at 5.5⁰C and boils at 80.2⁰C.

220. Benzene is highly inflammable.

221. The representation of real structure as a weighted average of two or more contributing structures is called resonance

222. The hybridization of C in benzene is sp² 223. Benezene have 6 CC and6 CH sigma bonds.

224. Hydrogenation of

ü Cyclohexene evolves 120 kJ /mol

ü 1,3-cyclohexadiene gives 232 kJ/ mol

ü 1,3,5-cyclohexartiene give 208 kL/ mol

225. The resonance energy of benzene is 152 kJ/ mol. *(320-208)due to unusual stability, benzene does not give addition reactions like those of alkenes.

226. Benzene prefers to undergo electrophilic substitution reactions rather than additions reactions.

227. The main types of reactions of benzene are: ü Addition reactions

ü Electrophilic substitution reactions

ü Oxidation reactions

228. Benzene is less reactive than alkene.

229. Benzene react with hydrogen in the presence of Ni or Pt catalyst at 150⁰C, under high pressure to form cycolohexane.

230. Benzene react with chlorine or bromine in the presence of ultralight to form hexachloride.

231. Benzene reacts with concentrated nitric acid in the presence of concentrated sulphuric acid at 60^oC to form nitrobenzene.

232. An electrophile NO₂⁺ is produced by reaction of H₂ SO₄ and HNO₃.

233. Benzene react with concentrated H₂ SO₄at 120⁰C or fuming H₂ SO₄ at room temperature to give benzene sulphonic acid.

234. Fuming sulphuric acid is concentrated sulphuric acid in which SO₃has been dissolved.

235. Electrophilic aromatic substitution reaction: ü Nitration → nitrobenzene

ü Sulphonation →benzene sulphonic acid

ü Halogenation → halobenzene

ü Friedel-crafts’s acylation → alkyl benzene

ü Friedel craft’s acylation → aromatic ketones

236. Treatment of benzene with n-propyl chloride gives isopropyl benzene rather than the expected n-propyl benzene.

237. Benzene reacts with alkyl halides in the presence of AlCl₃ to form alkyl benzenes.

238. Benzene reacts with acid halides in the presence of a lewis acid catalyst (AlCl3) to give aromatic ketones.

239. Effects of substitution of benzene:

• Directive or orientation effect  Effect on reactivity of benzene ring 240. Ortho/para directing substituents:

• OR

• OH

• NH₂

• NR₂

• NHR

• CH₃

• C₂ H₅

• C₆ H₅

• halogens

• *(R groups) 241. Meta directing substituents:

• CR

• COR

• CH

• COH

• CN  NO₂

• SO₃ H

242. Ortho/para directing groups are activators except halogens.

243. Meta directing groups are deactivators.

244. When phenol is nitrated, the reaction yield only the n-nitrophenol and pnitrophenol in ratio of 53% and 47%.

245. Using nitrated mixture (conc HNO₃ + conc H₂ SO₄), benzene can be nitrated at 60⁰C to form nitrobenzene.

246. Dinitrobenzene is obtained if reaction is carried at 100⁰C.

247. Trinitrobenzebe is obtained by using mixture of fuming nitric acid and sulphuric acid at 100⁰C.

248. Trinitrotoluene is widely used as a powerful explosives.

CHAP# 3 ALKYL HALIDES

249. Monohaloalkanes are usually called alkyl halides.

250. The functional group of alkyl halides are halogens.

251. The general formula of alkyl halides are C_n H_2n+1 X.

252. In common system alkyl halide are named as “alkyl halide”.

253. In IUPAC system, alkyl halide are named as derivative of alkane (1-chloro,2methyl propane).

254. Methyl and ethyl halides are gases at room temperature.

255. Alkyl halide upto C₁₈are colourless liquids.

256. Alkyl halides are water insoluble.

257. Alkyl halides have high boiling point than corresponding alkane.

258. For a given alkyl group, the boiling point increase with increase of size of halogen atom.

259. For given halogen atom the boiling point increase with increasing size of alkyl group.

260. Reaction of halogen acids with alcohol gives alkyl halide and water.

261. By the action of phosphorous trihalides on alcohol, alkyl halides are obtained.

262. Phosphorous trihalides are produced in situ by the action of red phosphorus on halogen.

263. By the action of thionyl chloride on alcohol, alkyl halides are produced along with HCl.

264. Pyridine being base absorbs HCl after its production.

265. Alkanes react with halogens in presence of uv light or at 400⁰C to yield alkyl group.

266. The reactive group of organic compound is alkyl halides.

267. Order of strength of C-X bonds,

→ C-F>C-Cl>C-Br>C-I

268. Order of reactivity of alkyl halide,

→ R-F<R-Cl<R-Br<R-I

269. Greater the no of alkyl groups, greater is the stability of the carbocation.

270. Tertiary carbocation is more stable than secondary and primary.

271. Base has a species that have affinity for proton.

272. Nucleophile has the ability to form bond with carbon atom.

273. A base attack hydrogen atom in the elimination reaction.

274. A nucleophile attacks carbon atom in the substitution reactions.

275. Tertiary alkyl halide undergo unimolecular substitution (SN¹).

276. Primary alkyl halides undergo bimolecular substitution (SN²).

277. Unimolecular substitution (SN¹) followed by tertiary alkyl halide in polar solvent.

278. Bimolecular substitution (SN²) follower by primary alkyl halide in none-polar solvent.

279. If medium is polar for secondary alkyl halide the substitution will SN¹. If it’s none-polar the substitution will SN².

280. The group or species which leaves the substrate or which is being replaced by incoming entering group is called leaving group. It’s also called nucleophuge.

281. Elimination reaction takes place in the presence of base.

282. E¹ are followed by tertiary alkyl halide.

283. E² are followed by primary alkyl halide.

284. E¹ has double step reaction.

285. E² has single step reaction.

286. A stronger base will favour in elimination.

287. A stronger nucleophile will favour substitution.

288. Ethoxide is strong base.

289. Anion of thioalcohol (C₂H₅S^-) is strong nucleophile.

290. Crowding within molecules of substrate also generally favours elimination over substitution reaction.

291. Alkyl groups stabilizes alkene more than the substitution product.

292. All those organic compound that contain at least one carbon metal bond are called organometallic compound.

293. Alkyl or aryl magnesium halides are commonly known as Grignard Reagents. 294. The general formula of Grignard reagents are R-Mg-X.

295. Grignard reagents are prepared by action of alkyl or aryl halide on freshly prepared magnesium metal in the presence of anhydrous or dry ether.

296. Grignard reagents cannot be isolated, therefore, it’s ethereal solution is directly used in the synthetic reactions.

297. Increasing size of alkyl or aryl group make the formation of Grignard reagents difficult. → I > Br > Cl

298. Alkyl or aryl magnesium fluorides are not known.

299. Alkylbromides are most suitable for preparation of Grignard reagents because alkyliodides are expensive.

300. Characteristics reactions of Grignard reagents are nucleophilic substitution and nucleophilic addition reactions.

301. Formaldehyde on reaction with Grignard reagents gives primary alcohol.

302. Higher aldehyde on reaction with Grignard reagents gives secondary alcohol.

303. Ketones on reaction with Grignard reagents gives tertiary alcohol.

304. Grignard reagents react with esters to form carbonyl compounds.

305. Grignard reagents react with ethyl formate gives secondary alcohol at the end.

306. Grignard reagents on reaction with ethyl acetate to give tertiary alcohol.

307. Grignard reagents reacts with CO₂ and forms carboxylic acids.

308. Hemoglobin have iron while plants chlorophyll has Magnesium.

309. Amines are important nitrogen containing organic compounds.

310. Amines are derivatives of NH₃ in which one or more hydrogen group is replaced by one or more similar or different alkyl groups.

311. The functional group of amine may be:

NH₂NH N

312. On basis of number of alkyl groups directly bonded to nitrogen atom, amines may be primary, secondary and tertiary amines.

313. Amines in common system are named as “Alkyl amine”.

314. In IUPAC naming, alkynes are named as substituent attached to alkane and named as “n-Aminoalkane”.

315. Lower molecular weight amines are generally gases or lower boiling liquids at room temperature.

316. Amines has ammonia like smell.

317. Amines have high boiling point than alkane due to hydrogen bonding.

318. All primary secondary and tertiary amines have hydrogen bonding with water molecules.

319. Only primary and secondary amine are able to form hydrogen bonding among their molecule.

320. Molecules of tertiary amine can’t form hydrogen bonding so its boiling point is lower than other.

321. Boiling point trend: ter < sec < pri

322. Amines have trigonal pyramidal shape.

323. Amines are basic in nature due to lone pain of electron on nitrogen.

324. Amine react with acids to form salts.

325. Basidity is directly proportional to no of alkyl groups.

326. Order of basidity: R₃N > R₂NH > RNH₂ > NH₃

327. When R-X is heated with alcoholic NH₃, it yields a mixture of primary, secondary and tertiary amines and quaternary ammonium salt.

328. The reaction of R-X with alcoholic NH₃ is also called alkylation of ammonia.

329. Primary amines are prepared by the reduction of nitro alkanes(R-NO₂) in the presence of “Pt/Pd/Ni or lithium aluminum hydride (LiAlH₄) in ether.

330. When nitriles or alkyl cyanides(R-CN) are reduced they yield the corresponding primary amines.

331. Primary amines are obtained when simple amides are reduced by lithium aluminum hydride in water.

332. On the basis of lone pair on nitrogen, Amines act as nucleophilic reagent.

333. The lone pair of nitrogen in amine are available to the electron deficient reagents called electrophiles.

334. When primary amine are treated with alkyl halides, they produce a mixture of secondary, tertiary amines and quaternary ammonium salts.

335. Primary amine react with aldehyde and ketones yielding condensation products called imines.

336. Imines are also called Schiff’s bases.

337. Primary amines react with acid chloride or acid anhydride to produce Nsubstituent amides.

338. Secondary amines react with acid chloride to N,N-disubtituted amides.

339. Tertiary amine have no directly attached hydrogen therefore they do not react with acid chloride to produce amides.

340. Which one of the following does not form amides on reaction with acid chloride or acid anhydride?

• Primary amine

• Secondary amine

• Tertiary amine ←

• None of these

• All of the above

341. When primary aliphatic amines are treated with nitrous acid, they yield highly unstable diazonium salt.

342. Nitrous acid being unstable acid is prepared in situ by the reaction of NaNO₂and dil HCl.

CHAP# 4 ALCOHOLS, PHEOLS & ETHERS

343. Alcohols, phenols and ethers are derivatives of water.

344. In alcohol one H of water has been replaced by alkyl group.

345. In phenol one H of water has been replaced by aromatic ring.

346. In ether both H of water has been replaced by two alkyl groups.

Water	HOH
Alcohol	R-OH
Phenol	Ar-OH
Ether	R-O-R

347. The general formula of alcohol is C_nH_2n+1OH.

348. Alcohol may be monohydric, dihydric or polyhydric.

349. Dihydric alcohol (diols) are usually called glycols because of sweet taste.

350. In common system, alcohol are named as “n/sec/ter Alkyl alcohols”.

351. In IUPAC system, “e” of alkane is replaced by “ol”. (alkane→alkanol).

352. Lower alcohols are colourless, toxic liquids.

353. Alcohols have characteristics sweet smell.

354. Boiling point of alcohol is higher than alkane due to hydrogen bonding.

355. Boiling point of alcohol increase regularly with the increase in the number of carbon atoms.

356. Among isomeric alcohols, as the branching increases, the boiling point decreases.

357. Which one of the following have high boiling point?

• Ethanol

• Propanaol

• 2-Methyl-2-Propanol

• 2-Butanol

• 1-Butanol ←

358. Lower alcohols C₁-C₄ are completely soluble in water in all proportions.

359. Which one is incomplete soluble in water?

• Methanol

• Ethanol

• Propanol

• Butanol ← 360. Angle in water is 109.5⁰C.

361. Angle in alcohol is 109⁰C.

362. The structure of alcohol and water is angular.

363. Alcohols are acidic in nature.

364. The O-H bond in alcohol is polar due to difference in E.N of two atoms.

365. Alcohols are less acidic than water because alcohols have electron donating groups.

366. The R groups in alcohol increase negative charge of oxygen so loss of hydrogen become difficult.

367. Which one of the following is more acidic?

• Primary alcohol ←

• Secondary alcohol

• Tertiary alcohol

368. Order of acidity of alcohols: pri > sec > ter

369. Alcohols are not acidic enough to react with aqueous NaOH or KOH.

370. R-OH + NaOH → No Reaction.

371. Alkenes react with concentrated sulphuric acid to produce alkyl hydrogen sulphates, which on hydrolysis yields alcohols.

372. Alcohols can be prepared by hydrolysis of alkyl halides by means of water or an aqueous alkali.

373. Formaldehyde react with Grignard reagent to produce primary alcohol.

374. Aldehyde react with Grignard reagent to give secondary alcohol.

375. Ketones react with Grignard reagent to produce tertiary alcohols.

376. Reduction of aldehyde and ketone to alcohol is done at 200⁰C and 10atm.

377. Formate esters on reaction with Grignard reagent secondary alcohol while other esters form tertiary alcohol.

378. Which one of the following on reaction with Grignard reagent give primary alcohol?

• Formate esters

• Ethyl acetate

• Propyl acetate

• None of the above ←

379. Both carboxylic acid and esters can be reduced to primary alcohols with Li Al

H₄.

380. Carboxylic acid cannot be reduced with H₂/Ni or Na+C₂H₅ -OH

381. The reactions of alcohol may be substitution reaction or elimination reactions.

382. Alcohols react with halogen acids to form corresponding alkyl halides.

383. Order of reactivity:

• HI > HBr > HCl

• Ter > sec > pri (alcohols)

384. HCL react only in the presence of catalyst (anhydrous ZnCl₂).

385. Lucas test: in lucas test, alcohols are treated with a solution of HCl and ZnCl₂ to form alkyl halides.

• Tertiary alcohols react with Lucas reagent immediately.

• Secondary alcohols react with Lucas reagent slower.

• Primary alcohols react with Lucas reagent more slowly.

386. Alcohols react with thionyl chloride to form alkyl chlorides.

387. Phosphorus Trihalides also form alkyl halides with alcohols.

388. Alcohols when treated with concentrated sulphuric acid at 170⁰C undergo dehydration to form alkenes.

389. Alcohols react with carboxylic acid to form esters (RCOOR). This process is called Esterification.

390. In Esterification, concentrated H₂SO₄ is used as catalyst.

391. The reaction of Esterification is reversible

392. Using strong oxidizing agent such as “Na₂Cr₂O₇ + H₂SO₄” or “KMnO₄ + H₂SO₄”, alcohols can oxidized to carbonyl compounds and finally to acids.

393. Primary alcohols are first oxidized to aldehydes and then to acids. 394. Secondary alcohols are first oxidized to ketone and then to carboxylic acids 395. Tertiary alcohols are stable to oxidation under normal conditions.

396. Under normal condition, which one of the following did not oxidized?

• Primary alcohol

• Secondary alcohol

• Tertiary alcohol ←

• All of the above

397. Ethylene glycol when treated with acidic KMnO₄ or K₂Cr₂O₇ results in the formation of formic acid.

398. Ethylene glycol when treated with periodic acid (HIO₄) or lead tetra acetate ((C₂H₅COO)₄ Pb) , ethylene glycol gives formaldehyde.

399. The sulphur analogues of alcohols are called Thiols and are called Thiols or alkyl hydrogen sulphdes or Mercaptans.

400. The functional group of thiols is –SH.

401. Thiols react with insoluble salts and hence named is Mercaptans.

402. Methanthiol is gas while ethanthiol and higher members are colourless, volatile liquids at STP.

403. Which one of the following is gas?

• Methanthiol ←

• Ethanthiol

• Propanthiol

• butanthiol

404. methanthiol and ethanthiol are added to natural gas in minute amounts to make gas leakage detectable by smell.

405. Thiols have lower boiling point than alcohol due to lack of hydrogen bonding.

406. Thiols are insoluble in water.

407. The world phenol is used for specific compound “hydroxyl benzene”.

408. Phenols are usually named as derivatives of the parent phenol (C₂H₅OH).

409. The C-O-H angle in phenol is 109.5⁰.

410. The C-O-H angle in methanol is 108.5⁰.

411. In phenol the cix carbon atoms are sp² hybridized and internal angle is 120⁰.

412. The C-O bond in phenol is slightly shorter than that of methanol.

413. The C-O bond length in phenol is 1.36⁰A and in methanol is 1.42^o.

414. Phenol are colourless liquids or low melting crystalline solids at room temperature.

415. Phenols have characteristics odour.

416. The vapours of phenol is itself toxic.

417. The boiling point of phenol is slightly higher than that of alcohol due to strong hydrogen bonding.

418. Phenol are more soluble than alcohol in water.

419. Above 65^oC, phenol and water are completely soluble.

420. The liquid phenol containing 5% of water is known as carbolic acid. 421. Carbolic acid is used as disinfectant and germicide.

422. Acidity: Carboxylic acid > water > phenol > alcohol

	Pka	Ka
Carboxylic acid	5	10-5
Water	7	10-7
Phenol	10	10-10
Alcohol	46-18	10-16 - 01-18

423. Being acidic, phenol react with NaOH or Na metal to form salt (Ar-ONa).

424. Phenol can be prepared from bezene sulphonic acid.

425. The sodium phenoxide is treated with dilute HCl to form phenol.

426. Chlorobenzene is hydrolysed with aqueous NaOH at high temperature and pressure to form phenol. this process was developed by Dow company of USA in 1928.

427. Cumene is also called isopropyl benzene.

428. A solution of benzenediazonium chloride is warmed on a water bath at 50⁰C 429. Benzenediazonium chloride is prepared from aniline. 430. Phenol exhibit two types of reactions:  Reaction due to hydroxyl group  Reaction due to aromatic ring.

431. The presence of OH group in phenol increase the reactivity of phenol.

432. Phenol react with bromine water or aqueous bromine to give ppt of 2,4,6 tribromophenol.

433. Chlorine react with phenol and forms:  O-Bromophenol 15%

 P-Bromophenol 85%

434. With dilute HNO₃, phenol reacts to form ortho and para nitrophenool.

435. 2,4,6-Trinitrophenol is also known as Picric acid.

436. Phenol being acidic in nature, react with sodium metal to form salt with the release of H₂ gas.

437. Phenol undergo oxidation with air (O₂) or chromic acid (CrO₃) to form pBenzoquinonee.

438. Compounds which contain a hydroxyl group in side chain attached to an aromatic ring are not phenols. they are called aromatic alcohols.

439. The first person to demonstrate ether’s use as anesthetic was Dr. Morton in 1896.

440. The common home disinfectant is chlorine bleach.

441. Chlorine bleach, a 5% solution of sodium hypochlorite.

442. Antiseptics are antimicrobial substances that are applied to living tissues to reduce possibility of infection.

443. All disinfectants which kill bacteria are called bactericidal.

444. All disinfectants which kill fungi are called fungicidal.

445. All disinfectants which kill bacteria spores are called sporicidal.

446. All disinfectants which kill viruses are called virucidal.

447. Ether are class of compound in which oxygen atom is linked to two alkyl groups or two aryl groups or one alkyl and one aryl group.

448. The functional group of ether is C-O-C.

449. Common naming of ether is “alkyl alkyl ether”.

450. IUPAC naming of ether: The larger alkyl group is taken for parent name and smaller alkyl group along with oxygen atom is named as alkoxy before the parent name such as “alkoxy alkane”.

451. Symmetrical ethers are prepared by heating an excess of alcohol with concentrated H₂SO₄ at 140⁰C. if temperature is not favored higher than will lead to formation of alkene.

452. In William synthesis, ether are prepared by treating sodium alkoxide with alkyl halide.

453. Dimethyl ether and ethyl methyl ether are gases at STP, while others are colourless volatile liquids with pleasant odours.

454. Ethers are highly inflammable.

455. Ether have low boiling point than alcohol.

456. Lower molecular ether are water soluble.

457. Ethers are generally less denser than water.

458. Ethers are quite stable they do not react with bases, active metals, oxidizing agents, reducing agents, they are also stable to dilute acids.

459. Ethers form oxonium salts with strong concentrated acids.

460. Ether donate a pair of electrons to hydrogen to form oxonium salts on reaction with cold concentrated HCl or H₂SO₄.

461. Ethers react with hot concentrated HI or HBr to form alcohol and alkyl halide. 462. Ethers react with acetyl chloride in the presence of anhydrous ZnCL₂ on heating to form alkyl chloride and ethyl acetate.

CHAP# 5

CARBONYL COMPOUNDS 1:

ALDEHYDES AND KETONES

463. A carbonyl group is functional group composed of carbon atom doubly bonded to an oxygen atom.

464. Aldehyde have at least one hydrogen atom attached to carbonyl carbon.

465. The functional group of aldehyde is formyl group or –COH.

466. In ketone the carbon atom is connected to two other carbon atoms.

467. The ketone functional group is called keto group and is represented by –CO-

468. Common system naming of Aldehyde: their names derived from carboxylic acid containing same carbon atom but “ic acid” is replaced by aldehyde.

• HCOOH → formic acid

• HCOH → formaldehyde

469. In IUPAC naming of aldehyde “e” of alkane is replaced by “al”.

• CH₄ → Methane

• HCOH → Methanal

470. In common naming system, ketone are named as “alkyl ketone”.

471. If two same groups are attached to carbonyl carbon, it’s called symmetrical ketone.

472. If two different groups are attached to carbon, it’s called unsymmetrical carbon.

473. In IUPAC naming of ketone “e” of alkane is replaced by “one” like

• CH₃CH₂CH₃ → Propane

• CH₃COCH₃ → Propanonee

474. The no of carbon at which oxygen is written before name of ketone like 2Pentanonee.

475. Which one of the following have sharp pungent odour?

• Formaldehyde ←

• Acetaldehyde ←

• Propinaldehyde

• butyrlaldehyde

476. Formaldehyde is gas at room temperature while other aldehyde are colourless liquids.

477. Which one of the following has pleasant smell?

• Formaldehyde

• Acetaldehyde

• Butyrlaldehyde ← 478. Which one of the following is gas?

• Formaldehyde ←

• Acetaldehyde

• Propinaldehyde

• Butyrlaldehyde

479. Acetone, the simplest ketone is liquid is room temperature with pleasant odour

480. All the members of ketones are colourless liquids except acetone.

481. Lower members of aldehyde and ketones upto C₄ are water soluble. Their solubility decreases as the size of the molecules increase.

482. Which one of the following will be less soluble in water?

• Propionaldehyde

• Butyraldehyde

• Penatnaldehyde

• Hexanaldehyde ←

483. The most soluble in water is fomaldehyde.

484. Carbonyl compounds do not form hydrogen bonding with each other.

485. Carbonyl compounds form hydrogen bonding with water molecule due to oxygen.

486. Which one of the following high boiling point?

• Alkane

• Ether

• Aldehyde and ketone

• Alcohols ←

487. Order of boiling point: alkane/ether < aldehyde/ketone < Alcohol

488. The boiling point of aldehyde and ketone increase with increase in the molecular weight. Ethanol > Methanal.

489. The carbon and oxygen of carbonyl group are sp² hybridized.

490. The length of CO single bond is 1.43⁰A.

491. The length of CO double bond is 1.23⁰A.

492. Ozone react vigorously with alkene and form ozonide which is unstable.

493. Ozonide is reduced directly to aldehydes and ketones by zinc and water. This reaction is called ozonolysis.

494. Water adds to alkene in presence of mercuric sulphate and sulphuric acid to form enol which is unstable,.

495. The enol intermediate undergoes arrangement to form aldehydes and ketones depending on starting alkyne used.

496. Friedel-Crafts acylation of aromatic gives aromatic ketones.

497. When benzene is treated in the presence of Lewis acid, AlCl₃ with acid halide, an aromatic ketone is produced.

498. The aldehydes and ketones undergoes addition reactions as compared to alkenes.

499. The presence of base increase the nucleophilic character of the reagent.

500. The presence of acid increase the electrophilic character of the carbonyl carbon atom inducing more positive charge on it and thus enhances its ability to be attacked by weak nucleophiles.

501. Carbonyl compounds are weak Lewis bases which can be protonated.

502. In addition reaction of carbonyl atom its geometry changes from trigonal to tetrahedral as its changes from sp² to sp³.

503. An acid catalyzed reaction will take place with weak nucleophile.

504. A base catalyzed addition reaction will take place with strong nucleophile. 505. Ketones are less reactive than aldehyde

506. Which one of the following is less reactive.

• formaldehyde

• Acetaldehyde

• Butyraldehyde

• Acetones ←

507. Ketone is less reactive than aldehyde due to

• Steric Hindrance

• Electronic effect

508. An alkyl group neutralize positive charge on carbonyl atom decreasing its reactivity towards nucleophile.

509. Addition of hydrogen to aldehyde and ketones is called reduction.

510. Aldehydes and ketones can be reduced to saturated hydrocarbons by:  Clemmenson Reduction: by using Zinc amalgam and conc HCl  Wolf-Kishner method: by using hydrazine.

511. Aldehydes and ketones are reduced to alkanes in the presence of Zinc amalgam and HCl as reducing agent.

512. When aldehyde or ketone is treated with hydrazine (NH₂NH₂), ahydrazone is obtained.

513. A hydrazine on heating with KOH in boiling with ethylene glycol gives corresponding alkanes.

514. In Clemmenson-reducation and Wolf Kishner reducation, alkane is produced at the end.

515. Aldehydes and ketones are easily reduced to primary and secondary alcohols respectively by using metal hydrides as reducing agents.

516. The most common metals hydrides are Lithium aluminum hydride (LiAlH₄) and sodium borohydride (NaBH₄).

517. Formaldehyde gives primary alcohol by reaction with Grignard Reagent.

518. Reduction of aldehydes and ketones by using hydrocyanic acid is done in basic medium.

519. Acetophenonee react with hydrocyanic acid to form acetophenonee cyanohydrin.

520. Aldehydes react with ammonia to form solid aldehyde ammonia.

521. Some important ammonia derivatives are:

• Alkyl amine R-(NH₂)

• Hydroxyl amine (NH₂OH)

• Hydrazine (NH₂NH₂)

• Phenyl hydrazine (C₆H₅NHNH2)

522. Primary amine react with aldehyde and ketone to form unstable compound which losses water to form product with CH double bond, called imines.

523. Aldehydes and ketones form oxime on reaction with hydroxyl amine.

524. Aldehyde and ketone react with hydrazine to form hydrazine.

525. Alcohols are weak nucleophile, an acid catalyst (H₂SO₄) is used.

526. Hemiacetal contain both alcohol and ether is functional group.

527. Acetal have two ether functional group.

528. Aldehydes are more easily oxidized than ketones.

529. The hydrogen atom attached to carbonyl group in aldehyde is oxidized to OH group. (RCHO → RCOOH)

530. Aldehydes can be oxidized by much milder oxidizing agent such as:

• Tollen’s Reagent

• Fehling’s Solution

• Benedict’s Solution

531. The Tollen’s Reagent is ammonium silver nitrate (2Ag (NH₃)₂ OH).

532. Tollen’s reagent reaction is also called mirror test.

533. Ammonioum carboxylate is formed by the reaction of aldehyde with ammonical silver nitrate.

534. Silver mirror is due to :

• 2Ag (NH₃)₂ OH

• 2Ag ←

• H₂O

• 3 NH₃

535. The fehling’s solution is 2Cu(OH)₂ + NaOH.

536. If aldehyde react with Fehling’s solution, the deep blue colour of cupric ion is reduced to ret ppt of cupric oxide.

537. Oxidation by Fehling solution is used widely for the estimation of glucose in blood and urine.

538. Ketones having hydrogen attached to alkyl group or also called alpha carbon can be oxidized in the presence of K₂Cr₂O₇ / H₂SO_4,KMnO₄ / H₂ SO₄ / conc HNO₃ etc which involves breaking C-C bondin case of unsymmetrical ketone, the carbonyl group remain smaller alkyl group as oxidation takes place at this site.

CHAP# 6 CARBONYL COMPOUNDS 2: CARBOXYLIC ACID AND FUNCTIONAL DERIVATIVES

539. Carboxylic acid is organic compound which contain carboxyl group (COOH).

540. The carboxyl group consist of carbonyl and hydroxyl group.

541. Acid containing one carboxyl group is called mono carboxylic acids.

542. Acid containing two carboxylic acids are called di carboxylic acids.

543. Carboxylic acids may be aliphatic are aromatic.

544. The general formula of aliphatic Carboxylic acid are RCOOH.

545. The general formula of aliphatic carboxylic acids are ArCOOH.

546. Aliphatic carboxylic acids are also commonly called fatty acids because esters of several higher members are fats.

547. Some derivatives of Carboxylic acid are:

• Acid halide/ Acyl halide

• Acid amide

• Ester

• Acid anhydrides 548. Names of some carboxylic acid:

Formula	Name	Language	Word
HCOOH	Formic acid	Latin	Formica → ant
CH₃COOH	Acetic acid	Latin	Acetum → vinegar
CH₃ CH₂COOH	Propionic acid	Greek	Protos, prion → first fat
CH₃ CH₂CH₂COOH	Butyric acid	Latin	Butyrum → fat

549. In IUPAC naming of carboxylic acid, “e” of alkane is replaced by “oic acid” like

• HCOOH → Methanoic acid

• CH₃COOh → Ethanoic acid

550. Carboxylic acid containing two carboxyl groups are called dicarboxylic acids or dioic acids (IUPAC).

551. The lower members of the apiphatic acids C₁-C₁₀ are liquids with distinctive odours.

552. Acetic acid which constitutes about 4-5% of vinegar has a characteristic smell which is recognizable in vinegar.

553. Butyric acid is substance that can be smelled in rancid butter.

554. Higher members of acid homologous series are wax-like solids.

555. Anhydrous ethanoic acid freezes at 17⁰C to form a solid which look like ice.It is, therefore also known as glacial acetic acid.

556. Carboxylic acid are more polar than alcohol.

557. Solubility of carboxylic acid in water decreases as their relative molecular mass increases.

558. Which one of the following is more soluble in water?

• Methanoic aid ←

• Ethanoic acid

• Propionic acid

• Butyric acid

559. The structural features of the carboxyl group are most apparent in formic acid.

560. The bond length between CO double bond is 120 pm. 561. The bond length between CO single bond is 134 pm.

562. The bond angles of H-C-O in carboxylic acids is 111⁰A.

563. The bond angles of H-C=O in carboxylic acids is 124⁰A.

564. The bond angle of O-C=C in carboxylic acids is 125⁰A.

565. The hybridization of hydroxyl oxygen in carboxylic acid is sp².

566. Lone pair from hydroxyl oxygen makes the carbonyl group less electrophilic than that of aldehyde and ketone.

567. Carboxylic acid is weak acid than mineral acids.

568. Carboxylic acid is more acidic than water, phenol and alcohol.

569. Monocarboxylic acid are monobasic acids.

570. Any electron withdrawing substituent will tend to stabilize the carboxylate ion by dispersing its negative charge and thus increase the acidity of acid.

571. Any electron donating group will tend to destabilize the carboxylate ion and thus decrease the acidity of the acid.

572. Oder of acidity; trichloro acetic acid> Dichloroacetic acid > chloro acetic acid > methanoic acid > Ethanoic acid > Propionic acid.

573. Carboxylic acids can be prepared by the action of Grignard reagent with carbon dioxide.

574. Reaction of carbon dioxide with Grignard reagent is known as carboxylation of Grignard reagent.

575. The reaction that provide an extension to length of carbon chain is reaction of CO₂ with R-Mg-X.

576. Compounds having cyanide (–CN) group are called alkyl nitriles or alkyl cyanides.

577. The carbon nitrogen triple bond in alkyl nitriles can be hydrolyzed to carboxylic acid in aqueous acid medium.

578. Primary alcohol can be oxidized to carboxylic acids by oxidizing agents like acidified potassium permanganate or potassium dichromate etc.

579. Primary alcohol on oxidation, gives aldehyde which on further oxidation converts to carboxylic acid.

580. Oxidation of aldehydes in the presence of oxidizing agents like KMnO₄, K₂Cr₂O₇ or Ag₂O gives carboxylic acid with the same number of carbon atoms.

581. Aromatic carboxylic acids can be prepared by the oxidation of aliphatic side chain (alky group) present on the benzene ring, with oxidizing agent like KMnO₄, K₂Cr₂O₇.any side chain is converted to carboxyl group.

582. In oxidation of alkyl benzene, the methyl group is oxidized not the aromatic ring, this show the striking stability of aromatic rings towards oxidizing agents.

583. The carboxylic acid is named so because it contains both carboxyl group and hydroxyl group.

584. Carbon atom of carboxylic acid is less positive than that of aldehyde and ketones so it did not undergoes addition or condensation reactions like that of aldehyde and ketone.

585. The OH donate electron to CO in carboxylic acid and hence reduce its partial positive charge so it I not attacked by nucleophiles as compared to aldehyde and ketone.

586. Acyl halides or acid halides are derivatives of carboxylic acids that are obtained by replacing OH of carboxylic acid by halogen atoms.

587. The most reactive derivatives of carboxylic acid derivatives are alkyl halide.

588. Acyl chloride are most common and less expensive than bromides and iodides.

589. Alkyl chlorides can be prepared by the reaction of acids with thionyl chlorides or phosphorus pentachloride (PCl₅).

590. Acid anhydrides are derived formic aids by removing water from two carboxylic acid molecules.

591. Naming of acid anhydrides: the name of acid of carboxylic is replaced by anhydride like carboxylic acid → carboxylic anhydride.

• CH₃-CO- O- CO-CH₃ acetic anhydride

592. The most important and commercially available anhydride are acetic anhydride or ethanoic anhydride.

593. The dehydrating agent is P₂O₅.

594. Esters are formed by replacing OH of acid by OR.

595. While naming ester the R part of OR is named first and then followed by the name of the acids, where by “ic acid“ is replaced by “ate”.

• Carboxylic acid → carboxylate

• CH₃-CO-OCH₃ → methyl ethanoate (ethanoic acid)

596. When a carboxylic acid and alcohol are heated in the presence of acid catalyst, an equilibrium is established with the formation of ester and water.

597. Esterification is reaction of an acid with alcohol.

598. Ethyl acetate is important ester which can be prepared by the reaction of acetic acid with ethanol.

599. Esters can also be prepared by the reaction of an alcohol with acid halides or acid anhydride.

600. Amides are least reactive derivative of acid which is formed by the replacement of OH of acid by NH₂ group.

601. Amides are named by replacing “ic acid” corresponding acid by word “amide”.

• Carboxylic acid → carboxylamide

• H-CO-NH₂ → formamide/Methanamide

• CH₃-CO-NH₂ → acetaide/ Ethanamide

602. Amides can be prepared by the reaction of ammonia with carboxylic acid to form first ammonium salts which on heating produces acid amides.

603. Amides can also be prepared by the reaction of ammonia with ester or acetyl chloride.

604. Order of acid derivatives towards nucleophile are:

Acylhalide > acid anhydride > ester > amide >Nitrile *(Cl-O-OR-NH₂-CN)

605. Acylhalide, acid anhydride, ester, amide and nitrile on hydrolysis yield corresponding carboxylic acid.

606. Acylhalide and acid anhydride on reaction with alcohol yield ester.

607. Acylhalide, acid anhydride and ester on ammonolysis yield an amide.

608. Carboxylic acid can be reduced to the corresponding alcohols using lithium tetrahydrido aluminate in dry ethoxy ethane.

609. The removal of carbon dioxide from a carboxylic acid takes place is known as decarboxylation.

610. Decarboxylation of carboxylic acid takes place when its sodium salt is heated with soda lime to form alkanes.

611. Soda lime is dry mixture of caustic soda, NaOH and quick lime CaO.

612. Ascorbic acid occur naturally in fruit, used as preservatives.

613. Ascorbic acid inhibits fungal growth but allow bacterial growth.

614. Benzoic acid and sodium benzoate have inhibitory effect on the growth of yeast.

615. The tartness in lemon is due to carboxylic acid.

616. Oranges have citric acid.

617. Acetic acid present in vinegar is responsible for giving sour taste.

618. Malic acid found in unripe fruit gives these fruit a sour or tart taste.

619. Acyl group react with benzene in the presence of lewis acid to form aromatic ketones.

620. On hydrolysis, anhydrides form corresponding carboxylic acid.

621. Hydrolysis of esters is called saponification.

622. Hydrolysis of esters is used to make soaps from fats.

623. Ester can be reduced to primary alcohol in the presence of reducing agent in ether which is used as solvent.

624. Ester react with two equivalent of Grignard Reagent to give tertiary alcohol.

625. Ester react with R-Mg-X to form ketone, ketone react with another R-Mg-X to form tertiary alcohols.

626. Amides on hydrolysis form the corresponding carboxylic acids. This reaction is slow and requires acid or base as catalyst.

627. Catalyst for hydrolysis of amide is?

• Acid

• Base

• Both ←

• No catalyst

628. Amides can be reduced to primary amine in presence of aluminium hydride.

629. Alkyl nitriles or simply nitriles are also considered as derivatives of carboxylic acid.

630. Alkyl nitriles can be obtained from carboxylic acids, through they do not contain acyl group.

631. On boiling with a dilute minerals acid or dilute alkali, nitriles are hydrolysed forming carboxylic acids.

632. Alkyl cyanide when treated with a reducing agent such as sodium and ethanol or lithium aluminium hydride (lithium tetra hydrioaluminate(III) in ethoxyethane, itriles are primary reduced to amines.

633. Nitriles on reaction with Grignard reagent produce Ketones.

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