{"id":3077,"date":"2023-10-04T10:46:35","date_gmt":"2023-10-04T10:46:35","guid":{"rendered":"http:\/\/localhost\/ecole9ja\/?p=3077"},"modified":"2023-10-04T10:48:29","modified_gmt":"2023-10-04T10:48:29","slug":"week-7-ss2-second-term-chemistry-notes","status":"publish","type":"post","link":"https:\/\/ecolebooks.com\/nigeria\/posts\/week-7-ss2-second-term-chemistry-notes\/","title":{"rendered":"Week 7 &#8211; SS2 Second Term Chemistry Notes"},"content":{"rendered":"<p>\u00a0<strong>WEEK SEVEN\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0            DATE: <\/strong>__________<br \/>\n<strong>TOPIC:COMPOUNDS OF NITROGEN<\/strong><br \/>\n\t<strong>CONTENT<br \/>\n<\/strong><\/p>\n<ul>\n<li>Oxides of Nitrogen\n<\/li>\n<li>Ammonia: Preparation, Properties and Uses.\n<\/li>\n<li>Trioxonitrate (V) acid: Preparation, Properties and Uses.\n<\/li>\n<\/ul>\n<p><strong>OXIDES OF NITROGEN<br \/>\n<\/strong><strong>NITROGEN (I) OXIDE, N<sub>2<\/sub>O<br \/>\n<\/strong>Nitrogen (I) oxide is known as laughing gas as it causes uncontrollable laughter when inhaled.<\/p>\n<p>\u00a0<strong>LABORATORY PREPARATION<br \/>\n<\/strong>The gas is prepared in the laboratory by thermal decomposition of ammonium trioxonitrate (V). Ammonium trioxonitrate (V) is not heated directly since the reaction is exothermic and may become uncontrollable leading to an explosion.<br \/>\na.\u00a0\u00a0\u00a0\u00a0KNO<sub>3(s)<\/sub> + NH<sub>4<\/sub>Cl<sub>(s)<\/sub>  \u2192   KCl<sub>(s)<\/sub> + NH<sub>4<\/sub>NO<sub>3(s)<\/sub><br \/>\n\tb \u00a0\u00a0\u00a0\u00a0NH<sub>4<\/sub>NO<sub>3(s)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192\u00a0\u00a0\u00a0\u00a02H<sub>2<\/sub>O<sub>(g)<\/sub> + N<sub>2<\/sub>O<sub>(g)<br \/>\n<\/sub><img decoding=\"async\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1046_Week7SS2Se1.jpg\" alt=\"\"\/><br \/>\n\t<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is a colourless gas with a faint pleasant sickly smell and it has a sweetish taste.\n<\/div>\n<ol>\n<li>\n<div>It is fairly soluble in cold water.\n<\/div>\n<\/li>\n<li>\n<div>It is 1.5 times denser than air.\n<\/div>\n<\/li>\n<li>\n<div>It is neutral to moist litmus paper.\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>CHEMICAL PROPERTIES<br \/>\n<\/strong>1.\u00a0\u00a0\u00a0\u00a0It decomposes on strong heating (about 600<sup>o<\/sup>C) to form nitrogen and oxygen.<br \/>\n                   2N<sub>2<\/sub>O<sub>(g)<\/sub> \u2192 O<sub>2(g)<\/sub>  +\u00a0\u00a0\u00a0\u00a0  2N<sub>2(g)<\/sub><br \/>\n\t2.\u00a0\u00a0\u00a0\u00a0It supports the combustion of any burning substance which is hot enough to decompose it.<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0Mg<sub>(s)<\/sub>  +  N<sub>2<\/sub>O<sub>(g)<\/sub>  \u2192 MgO<sub>(s)<\/sub>  + N<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>\u00a0\u00a0\u00a0\u00a0It is reduced to nitrogen by heated copper or iron\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0Cu<sub>(s)<\/sub> + N<sub>2<\/sub>O<sub>(g)<\/sub>     \u2192\u00a0\u00a0\u00a0\u00a0N<sub>2(g)<\/sub>  + CuO<sub>(s)<\/sub><\/p>\n<p>\u00a0<strong>TEST FOR N<sub>2<\/sub>O<br \/>\n<\/strong>A glowing splinter is inserted into the gas jar containing the unknown gas. If the splinter is rekindled, the gas is either oxygen or nitrogen (I) oxide. If the gas has a pleasant smell and does not produce brown fumes with nitrogen (IV) oxide; then the gas is nitrogen (I) oxide.<\/p>\n<p>\u00a0<strong>USE<\/strong>: Nitrogen (I) oxide is used as anesthetic for minor surgical operations. <\/p>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Describe the laboratory preparation of nitrogen (I) oxide.\n<\/div>\n<\/li>\n<li>\n<div>Describe a test to distinguish between nitrogen (I) oxide and oxygen gas.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>NITROGEN (II) OXIDE, NO<br \/>\n<\/strong><strong>LABORATORY PREPARATION<br \/>\n<\/strong>Nitrogen (II) oxide is prepared by reacting 50% trioxonitrate (IV) acid with copper.<br \/>\n3Cu<sub>(s)<\/sub> + 8HNO<sub>3(aq)<\/sub>  \u2192  3Cu(NO<sub>3<\/sub>)<sub>2(aq)<\/sub>  +  4H<sub>2<\/sub>O<sub>(l)<\/sub> + 2NO<sub>(g)<\/sub><br \/>\n\tSome of the nitrogen (II) oxide gas reacts with oxygen in the flask to form brown fumes of nitrogen (IV) oxide which is dissolved in water as the gas is pass through water. <\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is a colourless and poisonous gas.\n<\/div>\n<\/li>\n<li>\n<div>It is a almost insoluble in water.\n<\/div>\n<\/li>\n<li>\n<div>It is slightly denser than air.\n<\/div>\n<\/li>\n<li>\n<div>It is neutral to litmus.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>CHEMICAL PROPERTIES<br \/>\n<\/strong>1.\u00a0\u00a0\u00a0\u00a0It reacts readily with oxygen to form brown fumes of nitrogen (IV) oxide<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02NO<sub>(g)<\/sub>   +    O<sub>2(g)<\/sub> \u2192 2NO<sub>2(g)<\/sub><br \/>\n\t2.\u00a0\u00a0\u00a0\u00a0It decomposes on heating at high temperature to form equal volume of nitrogen and oxygen<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02NO<sub>(s)<\/sub>\u2192 N<sub>2(g)<\/sub> + O<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>It is reduced to nitrogen by hot metals\n<\/div>\n<p>           2Cu<sub>(s)<\/sub>    +    2NO<sub>(g) <\/sub>\u2192  2CuO<sub>(g)<\/sub> + N<sub>2(g)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>It acts as reducing agent decolourizing acidified potassium tetraoxomanganate (VI) slowly\n<\/div>\n<p>3MnO<sub>4<\/sub><sup>&#8211;<\/sup><sub>(aq)<\/sub>  +  4H<sup>+<\/sup><sub>(aq)  <\/sub>+ 5NO<sub>(g)<\/sub>   \u2192  3Mn<sup>2+<\/sup><sub>(aq)  <\/sub>+  5NO<sub>3<\/sub><sup>&#8211;<\/sup><sub>(aq) <\/sub>+  2H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a0<strong>TEST FOR NO<br \/>\n<\/strong><\/li>\n<li>\n<div>Using air: the gas jar containing the unknown gas is opened, if the gas turns reddish-brown, then the gas is NO.\n<\/div>\n<\/li>\n<li>\n<div>Using iron (II) tetraoxosulphate (VI): A solution of FeSO<sub>4<\/sub> which has been acidified with a little dilute H<sub>2<\/sub>SO<sub>4<\/sub> acid is poured into the gas jar containing the unknown gas. If the solution turns dark brown, then the gas is NO.\n<\/div>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong><\/li>\n<li>\n<div>Give an equation to show the laboratory preparation of nitrogen (II) oxide.\n<\/div>\n<\/li>\n<li>\n<div>State TWO physical and TWO chemical properties of nitrogen (II) oxide.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>NITROGEN (IV) OXIDE, NO<sub>2<br \/>\n<\/sub><\/strong><strong>LABORATORY PREPARATION<\/strong><br \/>\n\tNitrogen (IV) oxide is prepared by thermal decomposition of lead (II) trioxonitrate (V) because the nitrate does not contain water of crystallization which can interfere with the preparation.<br \/>\n          Pb(NO<sub>3<\/sub>)<sub>2(s)<\/sub> \u2192 2PbO<sub>(s)<\/sub>    +    O<sub>2(g)<\/sub>   +   4NO<sub>2(g)<\/sub><br \/>\n\tThe gas mixture obtained is passed through a U- tube immersed in a freezing mixture. Nitrogen (IV) oxide liquefies as a green liquid (yellow if pure) in the tube while oxygen escapes out.<br \/>\n<img decoding=\"async\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1046_Week7SS2Se2.jpg\" alt=\"\"\/><br \/>\n\t<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is a reddish \u2013 brown gas.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>It has an irritating smell and is poisonous.\n<\/div>\n<\/li>\n<li>\n<div>It turns damp blue litmus paper red and dissolves in water to form acidic solution.\n<\/div>\n<ol>\n<li>\n<div>It liquefies into yellow liquid at 21<sup>o<\/sup>C.\n<\/div>\n<\/li>\n<li>\n<div>It is much heavier than air.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>CHEMICAL PROPERTIES<br \/>\n<\/strong>1.\u00a0\u00a0\u00a0\u00a0Nitrogen (IV) oxide exists mainly as dinitrogen (IV) oxide, N<sub>2<\/sub>O<sub>4<\/sub> at low temperature. It decomposes on heating as follows.<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0N<sub>2<\/sub>O<sub>4(g)<\/sub>\u00a0\u00a0\u00a0\u00a0      2NO<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0    2NO<sub>(g)<\/sub> + O<sub>2(g)<\/sub><br \/>\n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0Pale \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0     Reddish \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0      colourless<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0yellow  \u00a0\u00a0\u00a0\u00a0     brown \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<br \/>\n2.\u00a0\u00a0\u00a0\u00a0It supports combustion as it decomposes on heating to nitrogen and oxygen<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02NO<sub>2(g)<\/sub> \u2192\u00a0\u00a0\u00a0\u00a0 N<sub>2(g)<\/sub>  + 2O<sub>2(g)<\/sub><br \/>\n\t3.\u00a0\u00a0\u00a0\u00a0It is reduced to nitrogen by reducing agent.<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a04CU<sub>(s)<\/sub>  + 2NO<sub>(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192  4CuO<sub>(s)<\/sub> + N<sub>2(g)<\/sub><br \/>\n\t4.\u00a0\u00a0\u00a0\u00a0It dissolves in water to form a mixture of dioxonitrate (III) and trioxonitrate (V) acids. It is a mixed acid anhydride.<br \/>\n  H<sub>2<\/sub>O<sub>(l)<\/sub>  +  2NO<sub>2(g)<\/sub>   \u2192 HNO<sub>2(aq)<\/sub> + HNO<sub>3(aq)<\/sub><br \/>\n\t5.   \u00a0\u00a0\u00a0\u00a0It reacts with alkalis to form mixture of dioxonitrate (III) and trioxonitrate (V) salts<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02KOH<sub>(aq)<\/sub> + 2NO<sub>2(g)<\/sub> \u2192 KNO<sub>3(aq)<\/sub>   +   KNO<sub>2(aq)<\/sub>   +   H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a0<strong>AMMONIA<br \/>\n<\/strong>Ammonia is a hydride of nitrogen. It is produced in nature when nitrogenous matter decays in the absence of air. Thus, traces of ammonia may be found in the atmosphere but being very soluble in water, it is dissolved by rain water and washed down into the soil.      <\/p>\n<p>\u00a0<strong>LABORATORY PREPARATION OF AMMONIA<br \/>\n<\/strong>Ammonia is prepared in the laboratory by heating calcium hydroxide, Ca(OH)<sub>2<\/sub> (slaked lime) with ammonium chloride.<br \/>\nCa(OH)<sub>2(s)<\/sub>+ 2NH<sub>4<\/sub>Cl<sub>(s)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192  CaCl<sub>2(s)<\/sub> +2H<sub>2<\/sub>O<sub>(l)<\/sub>+2NH<sub>3(g)<\/sub>.<br \/>\nAmmonia is dried using calcium oxide, CaO. Ammonia being alkaline cannot be dried using Conc. H<sub>2<\/sub>SO<sub>4<\/sub> or fused CaCl<sub>2<\/sub>, because they will react.<br \/>\n\u00a0\u00a0\u00a0\u00a0<img decoding=\"async\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1046_Week7SS2Se3.jpg\" alt=\"\"\/><\/p>\n<p>\u00a0<strong>INDUSTRIAL PREPARATION<br \/>\n<\/strong>Ammonia is manufactured from nitrogen and hydrogen by the Haber process. It involves mixing nitrogen and hydrogen in ratio 1:3 by volume. The reaction is reversible so special conditions listed below are required for optional yield of ammonia. <\/p>\n<ol>\n<li>\n<div>Finely divided iron catalyst is used\n<\/div>\n<\/li>\n<li>\n<div>Temperature of about 450<sup>O<\/sup>c is used\n<\/div>\n<\/li>\n<li>\n<div>Pressure of about 200atm is used.\n<\/div>\n<\/li>\n<\/ol>\n<p>The yield is about 15% under this condition<br \/>\n                 N<sub>2(g)<\/sub> +3H<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 2NH<sub>3(g)<\/sub> + heat<\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is a colorless gas with a characteristic choking smell.\n<\/div>\n<\/li>\n<li>\n<div>Ammonia in large quantity is poisonous as it affects respiratory muscles.\n<\/div>\n<\/li>\n<li>\n<div>It is the only known alkaline gas.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>It is about 1.7 times less dense than air.\n<\/div>\n<ol>\n<li>\n<div>Solid ammonia melts at -34.4<sup>O<\/sup>C and the liquid boils at -77.7<sup>O<\/sup>C.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>CHEMICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Ammonia burns readily in oxygen to form water vapor and nitrogen\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a04NH<sub>3(g)<\/sub>   +  3O<sub>2(g)<\/sub>   \u2192\u00a0\u00a0\u00a0\u00a06H<sub>2<\/sub>O<sub>(g)<\/sub>  +  2N<sub>2(g)<\/sub><br \/>\n\t2.\u00a0\u00a0\u00a0\u00a0Ammonia reacts as reducing agents reacting with<br \/>\n\u00a0\u00a0\u00a0\u00a0i.\u00a0\u00a0\u00a0\u00a0Copper II oxide<br \/>\n3CuO<sub>(s)<\/sub> + 2NH<sub>3(g)<\/sub> \u2192   3Cu<sub>(s)<\/sub> +  3H<sub>2<\/sub>O<sub>(l)<\/sub> + N<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>Chlorine\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a03Cl<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0+  8NH<sub>3(g)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192      6NH<sub>4<\/sub>Cl<sub>(s)<\/sub>\u00a0\u00a0\u00a0\u00a0+  N<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>Ammonia reacts with carbon IV oxide to form Urea and water vapour.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02NH<sub>3(g)<\/sub>   +   CO<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192  (NH<sub>2<\/sub>)<sub>2<\/sub> CO<sub>(s)<\/sub>\u00a0\u00a0\u00a0\u00a0+ H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<sup>urea<br \/>\n<\/sup><\/p>\n<ol>\n<li>\n<div>Ammonia reacts with acid to form ammoniums salts.\n<\/div>\n<p>2NH<sub>3(g)<\/sub>  +  H<sub>2<\/sub>SO<sub>4(g)<\/sub>  \u2192  (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4(s)<\/sub><\/p>\n<p>\u00a0<br \/>\n\u00a0<strong>TEST FOR AMMONIA<br \/>\n<\/strong>Ammonia has a choking smell. It can be confirmed using:\n<\/li>\n<li>\n<div>Litmus paper: Damped red litmus is dipped into the gas jar containing the unknown gas. If the litmus paper turns blue, then the gas is ammonia.\n<\/div>\n<\/li>\n<li>\n<div>Hydrochloric acid: a glass rod is dipped in concentrated HCl and then inserted in the gas jar containing the unknown gas. If white fumes are observed on the glass rod, then the gas is ammonia.\n<\/div>\n<p>\u00a0<strong>USES OF AMMONIA<br \/>\n<\/strong><\/li>\n<li>\n<div>Ammonia is used in the manufacture of trioxonitrate (V) acid and Sodium trioxocarbonate (IV) by the Solvay process.\n<\/div>\n<\/li>\n<li>\n<div>Liquid ammonia is used as a refrigerant.\n<\/div>\n<\/li>\n<li>\n<div>Aqueous ammonia is used in softening temporary hard water.\n<\/div>\n<\/li>\n<li>\n<div>Aqueous ammonia is also used in laundries as a solvent for removing grease and oil stains.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>EVALUATION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Briefly describe the laboratory preparation of ammonia.\n<\/div>\n<p>2.\u00a0\u00a0\u00a0\u00a0StateTWO physical and THREE chemical properties each of ammonia.\n<\/li>\n<\/ol>\n<p>\u00a0<strong>TRIOXONITRATE (V) ACID, HNO<sub>3<br \/>\n<\/sub><\/strong><strong>LABORATORY PREPARATION<br \/>\n<\/strong>Trioxonitrate (V) acid is a volatile acid and it is prepared in the laboratory by its displacement from any trioxonitrate salt by concentrated H<sub>2<\/sub>SO<sub>4<\/sub> which is less volatile. Trioxonitrate (V) of potassium or sodium is usually used because they are cheap.<br \/>\nKNO<sub>3(s)<\/sub>    +   H<sub>2<\/sub>SO<sub>4(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192  KHSO<sub>4(aq)<\/sub>  +  HNO<sub>3(aq)<\/sub><\/p>\n<p>\u00a0<strong>NOTE:<\/strong> An all glass apparatus must be used in this preparation because the hydrogen trioxonitrate (V) acid vapour will attack cork or rubber.<br \/>\n<img decoding=\"async\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1046_Week7SS2Se4.jpg\" alt=\"\"\/><br \/>\n\t<strong>INDUSTRIAL PREPARATION<br \/>\n<\/strong>Trioxonitrate (V) acid is obtained by the catalytic oxidation of ammonia:<br \/>\n&#8211;    Ammonia is treated with excess air using Platinum-rhodium catalyst at 700<sup>o<\/sup>C to produce nitrogen (II) oxide (96% conversion of NH<sub>3<\/sub> is obtained)<br \/>\n4NH<sub>3(g)<\/sub>    +    5O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192 4NO<sub>(g)<\/sub>  +  6H<sub>2<\/sub>O<sub>(g)<\/sub><br \/>\n\t&#8211;    Nitrogen (II) oxide formed is cooled and mixed with excess air to produce nitrogen (IV) oxide.<br \/>\n2NO<sub>(g)<\/sub>    +    O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192  2NO<sub>2<\/sub>(g)<br \/>\n&#8211;    Nitrogen (IV) oxide formed is dissolved with excess air in hot water to yield trioxonitrate (V) acid solution of up to 50% concentration.<br \/>\n4NO<sub>2(g)<\/sub>  +  2H<sub>2<\/sub>O<sub>(l)<\/sub>  +    O<sub>2(g)<\/sub> \u2192  4HNO<sub>3(aq)<br \/>\n<\/sub><br \/>\n\u00a0<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>The pure acid is a colourless fuming liquid with sharp choking smell. The acid turns yellow due to its decomposition to nitrogen (IV) oxide which redissolves in the acid.\n<\/div>\n<ol>\n<li>\n<div>The pure acid boils at 86<sup>0<\/sup>C and melts at -47<sup>o<\/sup>C\n<\/div>\n<\/li>\n<li>\n<div>The density of the pure acid is 1.52 gcm<sup>-3<\/sup>\n\t\t\t\t\t<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<li>\n<div>The pure acid is miscible with water in all properties and forms constant boiling mixture with it at 121<sup>o<\/sup>C\n<\/div>\n<ol>\n<li>\n<div>The concentrated form of the acid is corrosive.\n<\/div>\n<\/li>\n<li>\n<div>The dilute acid turns blue litmus red.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>CHEMICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>As an acid it neutralizes bases and alkalis to form metallic trioxonitrate (V) and water only\n<\/div>\n<p>NaOH<sub>(aq)<\/sub> + HNO<sub>3(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192  NaNO<sub>3(aq)<\/sub> + H<sub>2<\/sub>O<sub>(l)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>As an acids it reacts with metallic trioxocarbonate (IV) to liberate\n<\/div>\n<p>carbon (II) oxide<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0CaCO<sub>3(s)<\/sub>   +    HNO<sub>3(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192 Ca(NO<sub>3<\/sub>)<sub>2(aq)<\/sub>  +   H<sub>2<\/sub>O<sub>(l)<\/sub>  + CO<sub>2(g)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>Unlike other acids, it rarely gives out hydrogen with metals except when very dilute solution is reacted with Ca, Mg or Mn.\n<\/div>\n<\/li>\n<li>\n<div>As an oxidizing agent, it reacts with non \u2013 metal to form the corresponding oxides of the non \u2013 metals.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0S<sub>(s)<\/sub> + 6HNO<sub>3(aq)<\/sub>   \u2192  H<sub>2<\/sub>SO<sub>4(aq)<\/sub> + 2H<sub>2<\/sub>O<sub>(l)<\/sub> +    6NO<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>As an oxidizing agent, it oxidizes Cu, Pb, Hg and Ag to yield the\n<\/div>\n<p>respective trioxonitrate (V) and nitrogen (IV) oxide if concentrated, but nitrogen (II) oxide if the concentration is moderate.<br \/>\nAluminum and iron are not oxidized to their oxides by concentrated HNO<sub>3(aq)<\/sub> due to formation of a surface coating of oxide which is passive do not allow further reaction with the metals. Aluminum or iron lined container can be used to transport concentrated HNO<sub>3(aq)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>As an oxidizing agent, it oxidizes hydrogen sulphide to sulphur\n<\/div>\n<p>H<sub>2<\/sub>S<sub>(g)<\/sub> + 2HNO<sub>3(aq)<\/sub>  \u2192\u00a0\u00a0\u00a0\u00a0S<sub>(s)<\/sub>  + 2H<sub>2<\/sub>O<sub>(l)<\/sub>  +  2NO<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>As an oxidizing agent, it oxidizes iron (II) salts to iron (III) salts\n<\/div>\n<p>6Fe<sup>2+<\/sup><sub>(aq)<\/sub> + 8H<sup>+<\/sup><sub>(aq) <\/sub>+ 2NO<sub>3<\/sub><sup>&#8211;<\/sup><sub>(aq)<\/sub>      \u2192   6Fe<sup>3+<\/sup><sub>(aq)<\/sub> + 4H<sub>2<\/sub>O<sub>(l)<\/sub> + 2NO<sub>(g)<\/sub><\/p>\n<p>\u00a0<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>USES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is used as an acid, oxidizing agent and nitrating agent in the laboratory.\n<\/div>\n<\/li>\n<li>\n<div>It is used in nylon production and Terylene.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>It is used as rocket fuel.\n<\/div>\n<ol>\n<li>\n<div>It is used in production of fertilizers, dyes, drugs and explosives.\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>GENERAL EVALUATION\/REVISION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Describe the laboratory preparation of trioxonitrate (V) acid.\n<\/div>\n<\/li>\n<li>\n<div>Write TWO equations of reactions in which trioxonitrate (V) is acting as an acid.\n<\/div>\n<\/li>\n<li>\n<div>Write an equation to show the reaction of nitrogen (IV) oxide as a mixed anhydride.\n<\/div>\n<\/li>\n<li>\n<div>Describe the electrolysis of CuSO<sub>4<\/sub> solution using platinum electrodes.\n<\/div>\n<\/li>\n<li>\n<div>Classify the following oxides: CuO, Na<sub>2<\/sub>O, PbO, NO<sub>2<\/sub>, N<sub>2<\/sub>O<strong><br \/>\n\t\t\t\t<\/strong><\/div>\n<p>\u00a0<strong>READING ASSIGNMENT<br \/>\n<\/strong><\/li>\n<\/ol>\n<p>New School Chemistry for Senior Secondary Schools by O. Y. Ababio (6<sup>th<\/sup> edition), pages 406-409, 411-419. <\/p>\n<p>\u00a0<strong>WEEKEND ASSIGNMENT<br \/>\n<\/strong><strong>SECTION A: <\/strong>Write the correct potion ONLY.<\/p>\n<ol>\n<li>\n<div>Pure trioxonitrate (V) acid is colourless but the product of its laboratory preparation is yellow because of the presence of dissolved a. N<sub>2<\/sub>O b. NO c. NO<sub>2<\/sub> d. NH<sub>3<\/sub>\n\t\t\t<\/div>\n<\/li>\n<li>\n<div>Common laboratory drying agents are not used for drying ammonia because a. ammonia is alkaline b. ammonia forms complexes with them c. ammonia reacts with them and disappears into products d. ammonia is highly soluble in water\n<\/div>\n<\/li>\n<li>\n<div>Ammonia has relatively high boiling point when compared with other similar compounds because a. ammonia is stable b. ammonia is easily liquefied c. ammonia has hydrogen bonding d. ammonia is soluble in water.\n<\/div>\n<\/li>\n<li>\n<div>Aqueous ammonia solution used in the laboratory is referred to as aqueous ammonia and not ammonium hydroxide because a. ammonia dissolves in water without forming bond b. ammonia solution easily decomposes and liberated free ammonia when the temperature of the room rises leaving water in the bottle c. bond between ammonia and OH<sup>&#8211;<\/sup> of water is weakly acidic d. ammonia is less dense than air.\n<\/div>\n<\/li>\n<li>\n<div>Which of the following metals would be in passive state when treated with concentrated HNO<sub>3<\/sub>? a. Zinc b. Sodium c. Tin d. Iron\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>SECTION B<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Give reason for the following\n<\/div>\n<ol>\n<li>\n<div>The flask used for the laboratory preparation of ammonia is mounted in a slanting position\n<\/div>\n<\/li>\n<li>\n<div>An all glass apparatus is used for the laboratory preparation of trioxonitrate (V) acid.\n<\/div>\n<\/li>\n<\/ol>\n<p>2.\u00a0\u00a0\u00a0\u00a0Give an example of a reaction in which ammonia behaves as a \u00a0\u00a0\u00a0\u00a0<br \/>\n\u00a0\u00a0\u00a0\u00a0a. reducing agent \u00a0\u00a0\u00a0\u00a0b. base c. precipitating agent<\/p>\n<p>\u00a0<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"<p>\u00a0WEEK SEVEN\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 DATE: __________ TOPIC:COMPOUNDS OF NITROGEN CONTENT Oxides of Nitrogen Ammonia: Preparation, Properties and&#8230;<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1,248],"tags":[],"class_list":["post-3077","post","type-post","status-publish","format-standard","hentry","category-posts","category-second-term-ss2-chemistry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3077","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/comments?post=3077"}],"version-history":[{"count":1,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3077\/revisions"}],"predecessor-version":[{"id":3078,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3077\/revisions\/3078"}],"wp:attachment":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/media?parent=3077"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/categories?post=3077"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/tags?post=3077"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}