Oxygen is a Group 16 element. $$\(\mathrm{H}_{2} \mathrm{O}\)$$ reacts with both inorganic and organic compounds. (i) Complete Table 2.1 to give details of the reactions of some Period 3 oxides with $$\(\mathrm{H}_{2} \mathrm{O}\)$$. Table 2.1 (ii) Write an equation for the reaction of $$\(\mathrm{CH}_{3} \mathrm{CN}\)$$ with $$\(\mathrm{H}_{2} \mathrm{O}\)$$ in acidic conditions. $$\(\mathrm{CH}_{3} \mathrm{CN}+\ldots \ldots . \mathrm{H}_{2} \mathrm{O}+\ldots . . . \mathrm{H}^{+}\)$$ ........................................................................................... .. (iii) Draw the structures of the two alcohols formed in the reaction shown in equation 1. equation $$\(1 \quad \mathrm{C}_{3} \mathrm{H}_{6}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \xrightarrow{\mathrm{H}_{3} \mathrm{PO}_{4}} \mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}(\mathrm{g})\)$$ (iv) Explain why alcohols are less acidic than water. ....................................................................................................................................... . ....................................................................................................................................... . .................................................................................................................................
Exam No：9701_w24_qp_22 Year：2024 Question No：2(b)
Answer:
Knowledge points:
16.1.1.1 electrophilic addition of steam to an alkene, catalyst
16.1.1.2 reaction of alkenes with cold dilute acidified potassium manganate(VII) to form a diol
16.1.1.3 substitution of a halogenoalkane using NaOH(aq) and heat
16.1.1.4 reduction of an aldehyde or ketone using
16.1.1.5 reduction of a carboxylic acid using
16.1.1.6 hydrolysis of an ester using dilute acid or dilute alkali and heat
16.1.2.1 the reaction with oxygen (combustion)
16.1.2.2 substitution to halogenoalkanes
16.1.2.3 the reaction with Na(s)
16.1.2.4 oxidation with acidified or acidified to:
16.1.2.5 carbonyl compounds by distillation
16.1.2.6 carboxylic acids by refluxing (primary alcohols give aldehydes which can be further oxidised to carboxylic acids, secondary alcohols give ketones, tertiary alcohols cannot be oxidised)
16.1.2.7 dehydration to an alkene, by using a heated catalyst, e.g. or a concentrated acid
16.1.2.8 formation of esters by reaction with carboxylic acids and concentrated or as catalyst as exemplified by ethanol
16.1.3.1 classify alcohols as primary, secondary and tertiary alcohols, to include examples with more than one alcohol group
16.1.3.2 state characteristic distinguishing reactions, e.g. mild oxidation with acidified K2Cr2O7, colour change from orange to green
16.1.4 deduce the presence of a group in an alcohol, , from its reaction with alkaline (aq) to form a yellow precipitate of tri-iodomethane and an ion,
16.1.5 explain the acidity of alcohols compared with water
7.2.1 state the names and formulae of the common acids, limited to hydrochloric acid, HC/, sulfuric acid, ethanoic acid,
7.2.10 select suitable indicators for acid-alkali titrations, given appropriate data
7.2.2 state the names and formulae of the common alkalis, limited to sodium hydroxide, NaOH, potassium hydroxide, KOH, ammonia,
7.2.3 describe the Brønsted–Lowry theory of acids and bases
7.2.4 describe strong acids and strong bases as fully dissociated in aqueous solution and weak acids and weak bases as partially dissociated in aqueous solution
7.2.5 appreciate that water has pH of 7, acid solutions pH of below 7 and alkaline solutions pH of above 7
7.2.6 explain qualitatively the differences in behaviour between strong and weak acids including the reaction with a reactive metal and difference in pH values by use of a pH meter, universal indicator or conductivity
7.2.7 understand that neutralisation reactions occur when
7.2.8 understand that salts are formed in neutralisation reactions
7.2.9 sketch the pH titration curves of titrations using combinations of strong and weak acids with strong and weak alkalis
Solution:
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