Reference no: EM132347714

Chemistry of s, p and d block elements

6.0 Investigates the properties of elements and compounds of s, p and d block

6.1 Investigates the properties of elements in the s block.

Describes the occurrence of s block elements and compounds.

Describes the nature of the reactions by means of balanced chemical equations of elements of the first and second groups with air/O₂ , water, acids, N₂  and H₂.

Observes reactions of Na and Mg with air, oxygen, water, acids taking them as representative elements.

Explains that s block elements can function as reducing agents by forming stable cations with noble gas configuration by giving up outermost shell electrons (oxidation) which are loosely bonded to the nucleus.

Identifies the s elements using flame test.

State the results of flame test using electron transitions (emission spectrum).

6.2 Investigates the properties of elements and compounds of p block.

Describes the occurrence of p block elements and compounds compared to s block.

Describes reactions of aluminium with acids and strong bases.

Describes the reactions of aluminium and aluminium oxide to show their amphoteric nature.

Describes electron deficiency of AlCl₃ and the formation of Al₂ Cl₆.

Explains the structure and properties of graphite and diamond.

Present structures of CO and CO₂  and their properties.

Presents structure of H₂ CO₃  and explains its acidic property.

Writes examples for different oxidation numbers of nitrogen.

Present structures of oxides and oxoacids of nitrogen.

Writes balanced equations for reaction of HNO₃  with specified metals and nonmetals.

Writes reactions of ammonia as an oxidizing agent and a reducing agent

Writes balanced equations for thermal decomposition of ammonium salts.

Identifies ammonia gas and ammonium ion experimentally.

Presents information about allotropic forms of oxygen and sulphur.

Presents structure of oxoacids of sulphur.

Writes reactions to explain the oxidizing ability of conc. H₂ SO₄ with metals, C and S.

Writes oxidizing and reducing reactions of H₂ O₂ , H₂ S and SO₂.

Describes physical states and colours of halogens.

Writes balanced equations for the reactions of chlorine with Cu ,Fe and NH₃.

Writes balanced equations for displacement reactions of halogens.

Compares the relative oxidation powers of the halogens.

Describes the disproportionation of chlorine and chlorate(I) ions with balanced eqations.

Presents structures of the oxoacids of chlorine of different oxidation states.

Compares the acidity and oxidizing ability of oxoacids of chlorine using oxidation states.

Describes giving suitable examples, the acidity of hydrogen halides in aqueous medium.

States the properties of the noble gases and gives examples of some compounds they form.

Identifies the anions using precipitation method .

Explains the solubility of the precipitates in acids based on the nature of the anions.

Examines the presence of nitrogen in air.

Identifies the halide ions.

Determines the concentration of a given thiosulphate solution

6.3 Investigates the properties of compounds and their trends associated  with s and p block elements.

Compares the solubility of the salts of s block elements in water.

Compares the thermal stability of the nitrates, carbonates and bicarbonates of s block elements.

Explains how the acidic/ basic/ amphoteric nature of the oxides and hydroxides of s and p blocks vary along the 3rd period.

Writes balanced chemical equations for reactions of hydrides and halides with water to understand the trends of hydrolysis.

Compares the solubility of the salts of s block experimentally.

Compares the thermal stability of carbonates and nitrates experimentally.

Compares the hydrolysing ability of halides of group 15 elements.

6.4Investigates properties of elements of d block and their variation  across the period.

Describes the occurrence and uses of some d block elements and their compounds.

States the variable oxidation states shown by the d block elements of the fourth period using electron configuration.

Compares the ability to form variable oxidation states of d block elements with that of s and p block elements.

Compares electronegativity of d block elements with that of s block  elements.

Compares the metallic properties of d block elements with those of s block elements.

Describes the catalytic property of d block elements.

Describes the ability of d block elements to form coloured complexes.

Identifies the colours of d block complex ions experimentally.

6.5 Investigates properties of compounds of the d block.

Expresses acidic/basic/amphoteric nature of oxides of chromium and manganese.

Gives examples for reactions in which oxoanions of chromium and manganese act as oxidizing agents.

Writes balanced equations for oxidation and reduction reactions of oxoanions of Cr and Mn.

Determines the concentration of Fe²⁺ in a given sample using acidified KMnO₄  experimentally.

Determines the concentration of K₂ C₂ O₄  solution using acidified KMnO₄ experimentally.

6.6 Investigates properties of  Complex compoundsof the d block

Names complexes containing only one type of ligand using IUPAC rules.

Writes reaction of d block cations with NaOH and NH₃  (aq)

Shows how the central atom, the oxidation state and the ligand system of a complex ion affect the colour of a complex compound by giving suitable examples.

Observes the colours of copper(II), cobalt(II) and nickel(II) salts with hydrochloric acid and ammonia.

Observes the colours relevant to the oxidation states +2, +4, +6 and +7 of manganese using redox reactions.

Identifies Ni²⁺, Fe²⁺, Fe³⁺, Cu²⁺ and Cr³⁺ ions in aqueous solution experimentally.