Explain the following observations: (i) Many of the transition elements are known to form interstitial compounds. (ii) There is a general increase in density from titanium (Z = 22) to copper (Z = 29). (iii) The members of the actinoid series exhibit a larger number of oxidation states than the corresponding members of the lanthanoid series.

Explain the following observations: (i) Many of the transition elements are known to form interstitial compounds. (ii) There is a general increase in density from titanium (Z = 22) to copper (Z = 29). (iii) The members of the actinoid series exhibit a larger number of oxidation states than the corresponding members of the lanthanoid series.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter19: Transitition Metals, Coordination Chemistry And Metallurgy

Section: Chapter Questions

Problem 19.4QE

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State reasons for the following observations: (i) The enthalpies of atomisation of transition elements are quite high. (ii) There is a greater horizontal similarity in the properties of the transition elements than of the main group elements.
Explain the following observations: (i) The enthalpies of atomisation of transition metals are quite high. (ii) There is a close similarity in physical and chemical properties of the 4d and 5d series of the transition elements, much more than expected on the basis of usual family relationship. (iii) The members in the actinoid series exhibit larger number of oxidation states than the corresponding members in the lanthanoid series.
Account for the following: (a) (i) Transition elements form interstitial compounds. (ii) Mns+(3d4) is strongly oxidising, whereas Cr2+(3d4) is strongly reducing. (iii) Transition metals have high melting points. (b) What is misch metal? Write its one use.
Give the oxidation state of the metal for each of the following oxides of the first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than oneoxidation state. It is possible to write these compound formulas in the equivalent format MO∙M2O3, to permit estimation of the metal’s two oxidation states.)(a) Sc2O3(b) TiO2(c) V2O5(d) CrO3(e) MnO2(f) Fe3O4(g) Co3O4(h) NiO(i) Cu2O
Assign a reason for each of the following observations:(i) The transition metals (with the exception of Zn, Cd and Hg) are hard and have high melting and boiling points.(ii) The ionization enthalpies (first and second) in the first series of the transition elements are found to vary irregularly.
Explain the following observations giving appropriate reasons: (i) The stability of +5 oxidation state decreases down the group in group 15 of the periodic table. (ii) Solid phosphorus pentachloride behaves as an ionic compound. (iii) Halogens are strong oxidizing agents.
(a) What is the range in electronegativity across the first (3d)transition series? (b) What is the range across Period 4 of main-group elements? (c) Explain the difference.
Explain the ways in which the elements act: (a) How do you explain that fluoride, a small anion, is responsible for a weak field while water, a neutral molecule, gives rise to a much stronger binding field? (b) Explain why, for the same metallic cation and the same ligands, the energy of the binding field is lower in tetrahedral compounds than in octahedral compounds.
How would you account for the following?(i) Many of the transition elements are known to form interstitial compounds.(ii) The metallic radii of the third (5d) series of transition metals are virtually the same as those of the corresponding group members of the second (4d) series.(iii) Lanthanoids form primarily +3 ions, while the actinoids usually have higher oxidation states in their compounds, +4 or even +6 being typical.
(a) Calculate the number of unpaired electrons in the following gaseous state ions: Mn2+, Cr3+, V3+ and Fe2+ which one of these in the most stable in aqueous solutions? (At. nos. V = 23, Cr = 24, Mn = 25, Fe = 26) (b) Explain the following observations: (i) The transition metal ions are usually coloured in aqueous solutions. (ii) Cu(I) is not stable in an aqueous solution. (iii) The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.
Give an explanation for each of the following observations: (i) The gradual decrease in size (actinoid contraction) from element to element is greater among the actinoids than that among the lanthanoids (lanthanoid contraction). (ii) The greatest number of oxidation states are exhibited by the members in the middle of a transition series. (iii) With the same d-orbital configuration (d4), Cr2+ ion is a reducing agent but Mn3+ ion is an oxidising agent.
Explain the following observations :(i) Copper atom has completely filled d orbitals (3d10) in its ground state, yet it is regarded as a transition element.(ii) Cr2+ is a stronger reducing agent than Fe2+ in aqueous solutions.