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Chemistry of s, p and d block elements6.0 Investigates the properties of elements and compounds of s, p and d block6.1 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 agentWrites 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 solution6.3 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 blockNames 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.
Calculate the experimental percent by mass of copper in the sample and the theoretical mass percent of copper in copper (II) acetate monohydrate.
A liquid fuel mixture contains 31.95 hexane( C6H14) , 15.50 heptane (C7H16) , and the rest octane(C8H18) . What maximum mass of carbon dioxide is produced by the complete combustion of 11.0 kg of this fuel mixture
You are using a Geiger counter to measure the activity of a radioactive substance over the course of several minutes. If the reading of 400 counts. has diminished to 100. counts after 35.2 minutes , what is the half-life of this substance
Which way should the equilibrium shift when HCl is added? How do your results support your answer . Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer?
What is the pH of the solution when the titration is half way to the end point?
From the data below, calculate the total heat (in kJ) needed to convert 13.4 g of water at 25.0°C to steam at 110.0°C.
When 36.6 L ammonia and 39.5 L oxygen gas at STP burn, nitrogen monoxide and water are produced. After the products return to STP, how many grams of nitrogen monoxide are present ............... g NH3(g) + O2(g) NO(g) + H2O(l)
soluble plant fertilizer is 0.070% by weight. if a 19.0g sample of this fertilizer is dissolved in 2.0L of solution, what is the molar consentration
An aqueous solution is 22.0% by mass silver nitrate, AgNO3, and has a density of 1.22 g/mL. What is the molarity of silver nitrate in the solution?
A light green liquid, and informed that someone accidentally spilled a few small flecks of an intensely green-colored crystalline dye in a rather expensive solvent, so it doesn't make sense to throw away the very slightly contaminated solvent.
When 0.0600 mol of HCl(aq) is reacted with 0.0600 mol of NaOH(aq) in 50.0 mL of water, the temperature of the solution increases by 15.1°C. What is the enthalpy of reaction for the following thermochemical equation?
a particular flask has a mass of 17.4916 grams when it is empty. when has mass of the flask is 43.9616 grams filled
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