F325: Module 3 Specification

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A-Level Chemistry (F325: Module 3 - Transition Elements) Note on F325: Module 3 Specification, created by gallen96 on 04/02/2014.

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5.3.1 Transition Elements Properties Candidates should use sub-shell notation, eg for Fe: 1s22s22p63s23p63d64s2. No detail of how colour arises is required. No detail of catalytic processes required. Candidates should be able to: (a) deduce the electron configurations of atoms and ions of the d-block elements of Period 4 (Sc–Zn) , given the atomic number and charge; (b) describe the elements Ti–Cu as transition elements, ie d-block elements that have an ion with an incomplete d sub-shell; (c) illustrate: (i) the existence of more than one oxidation state for each element in its compounds, (ii) the formation of coloured ions, (iii) the catalytic behaviour of the elements and/or their compounds; Precipitation reactions Non-complexed formulae such as Cu(OH)2 and Fe(OH)3 are acceptable. Oxidation of alkaline Fe(II) and Co(II) not required. (d) describe, including ionic equations, the simple precipitation reactions and the accompanying colour changes of Cu2+(aq), Co2+(aq), Fe2+(aq) and Fe3+(aq) with aqueous sodium hydroxide; Ligands and complex Ions Examples should use H2O, Cl–, NH3 as simple monodentate ligands. In examinations, other ligands might be introduced. (e) explain the term ligand in terms of coordinate bonding; (f) state and use the terms complex ion and coordination number; (g) state and give examples of complexes with sixfold coordination with an octahedral shape; (h) explain and use the term bidentate ligand (eg NH2CH2CH2NH2, ‘en’); (i) describe the types of stereoisomerism shown by complexes, including those associated with bidentate and multidentate ligands: (i) cis-trans isomerism, eg Ni(NH3)2Cl2, (ii) optical isomerism, eg [Ni(NH2CH2CH2NH2)3]2+; (j) describe the use of cis-platin as an anticancer drug and its action by binding to DNA in cancer cells, preventing division; Ligand substitution (k) describe the process of ligand substitution and the accompanying colour changes in the formation of: (i) [Cu(NH3)4(H2O)2]2+ and [CuCl4]2– from [Cu(H2O)6]2+, (ii) [CoCl4]2– from [Co(H2O)6]2+; (l) explain the biochemical importance of iron in haemoglobin, including ligand substitution involving O2 and CO; (m) state that the stability constant, Kstab,, of a complex ion is the equilibrium constant for the formation of the complex ion in a solvent from its constituent ions; (n) deduce expressions for the stability constant, Kstab, of a ligand substitution, eg M2+(aq) + 6X–(aq) MX6 4–(aq) Kstab = [MX6 4–(aq)]/[M2+(aq)][X–(aq)]6 (o) relate ligand substitution reactions of complexes to stability constants and understand that a large Kstab results in formation of a stable complex ion; Redox reactions and titrations Non-structured titration calculations could be examined in the context of both acid–base and redox titrations. (p) describe, using suitable examples, redox behaviour in transition elements; (q) carry out redox titrations, and carry out structured calculations, involving MnO4– and I2/S2O3 2; (r) perform non-structured titration calculations, based on experimental results.

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