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Metals and Nonmetals, CHAPTER3, Part 2

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What happens when Metals react with, Acids?, , , Metal + Dilute acid → MetalSalt + Hydrogen, , , , metals react with acids to give a salt and hydrogen gas., , Do, , all metal react with acid ?

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Reactivity series, The reactivity series is a list of metals arranged in the order, of their decreasing activities, This list was created experimentally by studying the reactions, between metals and oxygen, water and acid

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What happens when Metals react with, Acids?, , , The metal which are placed above H in the reactivity series react with dil, acid to form metal salt and hydrogen gas ., , , , These reactions are exothermic, , , , 2Na+2HCL2Nacl+H2, , 1., , sodium and potassium react vigorously even with cold water, , 2., , Mg react rapidely but the reaction is less vigerous, Mg+2HclMgcl2+H2, , 3., , Al react with acid , but the reaction is slow at the beginning because the, surface of aluminum is already covered with asluminium oxide .after the, layer is dissolved in acid the reaction becomes faster, 1., , 4., , 2Al+6Hcl2Alcl3+3H2, , The reaction was also the most exothermic in this case. The reactivity, decreases in the order Mg > Al > Zn > Fe.

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Cu,Hg,Ag,Au do not react with dil acid, EXCEPTION (nitric acid), , Hydrogen gas is not evolved when a metal reacts with nitric acid. It is, because HNO3 is a strong oxidising agent. It oxidises the H2 produced to, water and itself gets reduced to any of the nitrogen oxides (N2O, NO,, NO2 ), EXCEPTION, But magnesium (Mg) and manganese (Mn) react with very dilute HNO3 to, evolve H2 gas

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How do Metals react with, Solutions of other Metal Salts?, , , You will observe that the reaction has occurred in the, test tube containing iron nail and copper sulphate, solution. Iron takes the sulphate away from copper, , , , Copper sulphate + Iron---------► Iron sulphate +, Copper

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Metals react with Solutions, , , MORE REACTIVE METAL CAN REPLACE LESS REACTIVE METALS FROM THEIR SALT, SOLUTION.

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WHY DO METALS AND NON-METALS, REACT?, , , THE ATOMS COMBINE WITH ONE ANOTHER TO ACHIEVE THE INERT GAS, ELECTRONIC CONFIGURATION AND TO BECOME STABLE., , , , AN ATOM CAN ACHIEVE THE INERT GAS ELECTRONIC CONFIGURATION IN 3 WAYS, , 1., , BY LOSING ONE OR MORE ELECTRONS, , 2., , BY GAINING ONE OR MORE ELECTRONS, , 3., , BY SHARING ONE OR MORE ELECTRONS

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IONS, , , AN IONS IS AN ELECRICALLY CHARGED ATOM., , , , IT IS FORMED BY LOSS OR GAIN OF ELECTRON, , IONS, CATIONS, , ANIONS

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IONIC BOND, , , AN IONIC BOND IS FORMED WHEN ONE OF THE ATOMS CAN DONATE, ELECTRONES TO ACHIEVE INERT GAS CONFIGURATION AND THE OTHER ATOM, NEEDS ELECTRONES TO ACHIEVE THE INERT GAS CONFIGURATION, , , , NA + CL  NACL, , , , K + CL  KCL, , , , Mg + Cl  Mgcl2

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Properties of Ionic Compounds, , , (i) Physical nature: Ionic compounds are solids and are somewhat hard, because of the strong force of attraction between the positive and negative, ions. These compounds are generally brittle and break into pieces when, pressure is applied., , , , (ii) Melting and Boiling points: Ionic compounds have high melting and boiling, points (see Table 3.4). This is because a considerable amount of energy is, required to break the strong inter-ionic attraction., , , , (iii) Solubility: Electrovalent compounds are generally soluble in water and, insoluble in solvents such as kerosene, petrol, , , , (lv)Ionic compounds in the solid state do not conduct electricity because, movement of ions in the solid is not possible due to their rigid structure. But, ionic compounds conduct electricity in the molten state. This is possible in, the molten state since the elecrostatic forces of attraction between the, oppositely charged ions are overcome due to the heat. Thus, the ions move, freely and conduct electricity