Match the following:- Column I Column II (Elements) (Symbol) (i) Acidic Radicals K + , Na + (ii) Basic Radicals Fe 2 + , Fe 3 + (iii) Monovalent Radicals CO 3 2 - , SO 4 2 - (iv) Variable Valency Cl - , K + (v) Tetravalent elements Pb 4 + , Pt 4 +

Acidic Radicals and Basic Radicals :- Negatively charged radicals are called acidic radicals . Positively charged radicals are called basic radicals . Acid radicals are formed by the removal of hydrogen ion ( H + ) . Basic radicals are formed by the removal of hydroxide ion ( OH - ) . Monovalent Radical:- A radical formally derived by the removal of one hydrogen atom from any position of any other parent hydride, is named by adding the suffix "-yl" to the name of the parent hydride, eliding the final "e" of the name of the parent hydride. Variable valency :- This property is called as variable valency. Some elements show variable valency because of the different electronic configurations. An atom of an element can sometimes lose more electrons than are present in its valence shell i.e. loss from the penultimate shell and hence exhibit more than 1 or variable valency. Tetravalent elements are those elements which have a valency of four i.e. have four electrons in the outermost shell. Examples are the elements belonging to group 14 like carbon , silicon , germanium etc. The symbol of radicals are - Column I Column II (Elements) (Symbol) (i) Acidic Radicals CO 3 2 - , SO 4 2 - (ii) Basic Radicals K + , Na + (iii) Monovalent Radicals Cl - , K + (iv) Variable Valency Fe 2 + , Fe 3 + (v) Tetravalent elements Pb 4 + , Pt 4 +

Balance the chemical equation Na 2 S 2 O 3 + HCl → H 2 O + NaCl + SO 2 + S

Redox reactions are oxidation-reduction chemical reactions in which the reactants undergo a change in their oxidation states. The term ‘redox’ is a short form of reduction-oxidation. All the redox reactions can be broken down into two different processes – a reduction process and an oxidation process. Na 2 S 2 O 3 + 2 HCl → H 2 O + 2 NaCl + SO 2 + S This is an oxidation-reduction (redox) reaction: S 2 + + 2 e - → S 0 (reduction) S 2 - - 2 e - → S 4 - (oxidation) Na 2 S 2 O 3 is both an oxidizing and a reducing agent (disproportionation (dismutation)reaction)

Balance the chemical equation:- NH 3 + O 2 → H 2 O + N 2

Redox reactions are oxidation-reduction chemical reactions in which the reactants undergo a change in their oxidation states. The term ‘redox’ is a short form of reduction-oxidation. All the redox reactions can be broken down into two different processes – a reduction process and an oxidation process. 4 NH 3 + 3 O 2 → 6 H 2 O + 2 N 2 This is an oxidation-reduction (redox) reaction: 4 N 3 - - 12 e - → 4 N 0 (oxidation) 6 O 0 + 12 e - → 6 O 2 - (reduction) NH 3 is a reducing agent, O 2 is an oxidizing agent.

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TOGETHER WITH CHEMISTRY>Chapter 1 - The Language of Chemistry>Self Evaluation Test>Q 7

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9th ICSE

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The formula of Ferric sulphate is

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Important Questions on The Language of Chemistry

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9th ICSE

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TOGETHER WITH CHEMISTRY>Chapter 1 - The Language of Chemistry>Self Evaluation Test>Q 7

Write the correct answer.

The Formula for Magnesium Nitride.

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9th ICSE

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TOGETHER WITH CHEMISTRY>Chapter 1 - The Language of Chemistry>Self Evaluation Test>Q 8

Match the following:-

	Column I	Column II
	(Elements)	(Symbol)
(i)	Acidic Radicals	$K^{+}, {Na}^{+}$
(ii)	Basic Radicals	${Fe}^{2 +}, {Fe}^{3 +}$
(iii)	Monovalent Radicals	${CO}_{3}^{2 -}, {SO}_{4}^{2 -}$
(iv)	Variable Valency	${Cl}^{-}, K^{+}$
(v)	Tetravalent elements	${Pb}^{4 +}, {Pt}^{4 +}$