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Fe3+ ; (1) NO3– (1)

Identify all the species in the table which could convert I – aq) into I 2 (aq) but which could not convert Br – (aq) into Br 2 (l). Fe3+ ; (1) NO3– (1). EOMT next Tuesday. Transition metals. L.O.: Deduce the electron configurations of atoms and ions of the d-block elements.

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Fe3+ ; (1) NO3– (1)

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  1. Identify all the species in the table which could convert I–aq) into I2(aq) but which could not convert Br–(aq) into Br2(l).

  2. Fe3+ ; (1) NO3– (1)

  3. EOMT next Tuesday

  4. Transition metals L.O.: Deduce the electron configurations of atoms and ions of the d-block elements. Describe the elements Ti–Cu as transition elements.

  5. First row of the transition metal block

  6. Energy-level diagram showing the overlap of the 3d and 4s sub-shells

  7. Tip: 4s orbital is filled before 3d, but 4s electrons are removed before any electrons are taken out from the 3-d sub-shell.

  8. Write electronic configurations of: Sc, Ti, Cu and Zn. To which block of the periodic table do Sc, Ti and Cu belong to? Why? Write the electronic configurations of Sc3+, Zn2+, Cu+ and Cu2+. Why Sc and Zn are not transition metals?

  9. A transition element is a d-block element that forms an ion with an incomplete d sub-shell

  10. Give the electronic configuration of the following atoms: a) V b) Cr c) Co • d) Cu • e) Zn

  11. 2. Give the electronic configuration of the following ions: • a) Co2+ • b) Cu+ • c) V3+ • d) Cr3+ • e) Fe3+

  12. L.O.: • Illustrate the existence of more than one oxidation state for a transition element in its compounds. • Illustrate the formation of coloured metal ions.

  13. Properties of transition metals List all of the properties metals exhibit : • Good conductors of heat and electricity • High melting and boiling points • Malleable • Ductile • Shinny • Usually strong (high tensile and compressive strength) • Ions are usually brightly coloured • Often can be used when in compounds or as metals as a catalyst

  14. Oxidation numbers and colours of the common d block metal ions

  15. Catalysis and precipitation • Illustrate the catalytic behaviour of the transition elements and/or their compounds. • Describe the simple precipitation reactions of Cu2+ (aq), Co2+(aq), Fe2+(aq) and Fe3+(aq) with aqueous sodium hydroxide.

  16. Hydrogenation of the C=C bond in alkenes

  17. Catalytic properties of transition metals Two main causes for their catalytic properties • They can provide a solid surface onto which the reactant can ADSORB and thereby hold it in place • Their variable oxidation state allows them to form intermediates with reactants that lowers the activation energy of the reaction

  18. Catalysts dependent on transition metals • Catalytic converters – use platinum, rhodium and palladium • Haber process uses iron • Hydrogenation of alkenes uses nickel metal • Decomposition of hydrogen peroxide uses MnO2 • CONTACT PROCESS uses vanadium (V) oxide to convert sulfur dioxide into sulfur trioxide which is needed to make sulfuric acid

  19. Precipitating out transition metal ions • Transition metals in aqueous solution can be precipitated out using NaOH(aq) to produce a insoluble transition metal hydroxide • Write out the balanced equation for each of these metals

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