The Group 14 elements show a change from non-metallic to metallic character down the group. Carbon is found in inorganic compounds such as carbonates. (i) Write an equation for the reaction of magnesium carbonate with dilute $$$\mathrm{HCl}(\mathrm{aq})$$$. ................................................................................................................................. (ii) Describe the thermal stability of the carbonates down Group 2. ................................................................................................................................. (iii) Ammonium carbonate undergoes an acid-base reaction with $$$\mathrm{NaOH}(\mathrm{aq})$$$. Explain this statement. ....................................................................................................................................... . ....................................................................................................................................... . .................................................................................................................................

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_w24_qp_21 Year：2024 Question No：3(b)

Answer:

Knowledge points:

10.1.1 describe, and write equations for, the reactions of the elements with oxygen, water and dilute hydrochloric and sulfuric acids

10.1.2 describe, and write equations for, the reactions of the oxides, hydroxides and carbonates with water and dilute hydrochloric and sulfuric acids

10.1.3 describe, and write equations for, the thermal decomposition of the nitrates and carbonates, to include the trend in thermal stabilities

10.1.4 describe, and make predictions from, the trends in physical and chemical properties of the elements involved in the reactions in 10.1.1 and the compounds involved in 10.1.2, 10.1.3 and 10.1.5

10.1.5 state the variation in the solubilities of the hydroxides and sulfates

2.3.1.1 the prediction of ionic charge from the position of an element in the Periodic Table

2.3.1.2 recall of the names and formulae for the following ions:

2.3.2 write and construct equations (which should be balanced), including ionic equations (which should not include spectator ions)

2.3.3 use appropriate state symbols in equations

2.3.4 define and use the terms empirical and molecular formula

2.3.5 understand and use the terms anhydrous, hydrated and water of crystallisation calculate empirical and molecular formulae, using given data

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

Answer:

Knowledge points:

Solution:

Related Question