DP Chemistry Questionbank

• Syllabus

Topic 13: The periodic table—the transition metals

Sub sections and their related questions

13.1 First-row d-block elements

• 15M.2.hl.TZ2.8a.i: Draw an orbital diagram (using the arrow-in-box notation) showing the electrons in the 4s and 3d...
• 14M.1.hl.TZ2.4: What is the abbreviated electron configuration of the cobalt(II) ion,...
• 14M.2.hl.TZ1.5d.i: State the full electron configurations of Cr and \({\text{C}}{{\text{r}}^{3 +...
• 14M.2.hl.TZ1.5d.ii: \({\text{C}}{{\text{r}}^{3 + }}\) ions and water molecules bond together to form the complex ion...
• 14M.2.hl.TZ2.2b: State the full electronic configuration of a copper atom.
• 14M.2.hl.TZ2.2c: Explain why most copper(II) compounds are coloured, whereas most copper(I) compounds are not.
• 14N.2.hl.TZ0.11f: (i)     Zinc is found in the d-block of the periodic table. Explain why it is not considered a...
• 13N.1.hl.TZ0.12: Which species have dative covalent bonding? I.    ...
• 13N.2.hl.TZ0.4c: Transition metals have certain characteristic properties. State two properties that are involved...
• 13M.2.hl.TZ1.7b.ii: List three characteristic properties of transition elements.
• 13M.2.hl.TZ1.7b.iii: Identify the type of bonding between iron and cyanide in...
• 13M.2.hl.TZ1.7b.iv: Deduce the oxidation number of iron in...
• 13M.2.hl.TZ2.5d.i: Define the term ligand.
• 12N.2.hl.TZ0.2b: (ii)     Cobalt is a transition metal. One common ion of cobalt is...
• 12N.2.sl.TZ0.4c: (i)     Explain why metals are good conductors of electricity and why they are malleable. (ii)  ...
• 10N.1.hl.TZ0.8: In which complexes does iron have an oxidation number of  \( + 3\)? I.    ...
• 10N.1.hl.TZ0.27: Which solutions have a pH less than 7? I.    ...
• 09N.2.hl.TZ0.3b: Transition elements form complexes such as...
• 10M.2.hl.TZ1.4e: Explain why copper is considered a transition metal while scandium is not.
• 10M.2.hl.TZ2.6f.i: State and explain the type of reaction that takes place between \({\text{F}}{{\text{e}}^{3 + }}\)...
• 10M.2.hl.TZ2.6f.ii: Explain why...
• 09M.2.hl.TZ1.7b.i: \({{\text{[Co(}}{{\text{H}}_{\text{2}}}{\text{O}}{{\text{)}}_{\text{6}}}{\text{]}}^{2 + }}\)
• 09M.2.hl.TZ1.7b.iii: \({{\text{[CoC}}{{\text{l}}_{\text{4}}}{\text{]}}^{2 - }}\)
• 09M.2.hl.TZ1.8b.iii: State what is meant by the term second ionization energy.
• 09M.2.hl.TZ2.3a.iii: Define the term ligand.
• 11M.1.hl.TZ2.9: Which metal nitrate solution is coloured? A.    ...
• 12M.1.hl.TZ2.6: What is the electron configuration of \({\text{S}}{{\text{n}}^{2 + }}\)? A.    ...
• 12M.2.hl.TZ2.9a: (i)     State the full electron configuration of Fe. (ii)     State the abbreviated electron...
• 11N.2.hl.TZ0.7e.i: State two characteristic properties of transition elements.
• 11N.2.hl.TZ0.7e.ii: State the type of bond formed by a ligand and identify the feature that enables it to form this...
• 16M.2.hl.TZ0.4d: In an aqueous solution of vanadium(III) chloride, the vanadium exists as [V (H2O)6]3+, [VCl...
• 16M.2.hl.TZ0.4c: Outline, giving the full electron configuration of the vanadium atom, what is meant by the term...
• 16N.2.hl.TZ0.2f: Explain how ethanedioate ions act as ligands.
• 17M.1.hl.TZ1.8: What is the charge on the iron(III) complex ion in [Fe(OH)2(H2O)4]Br? A.     0 B.     1+ C.   ...
• 17M.2.hl.TZ1.2e: Describe, in terms of the electrons involved, how the bond between a ligand and a central metal...
• 17M.2.hl.TZ1.4a: Formulate an equation for the oxidation of nickel(II) sulfide to nickel(II) oxide.
• 17M.2.hl.TZ1.4b: The nickel obtained from another ore, nickeliferous limonite, is contaminated with iron. Both...
• 17M.2.hl.TZ1.4d: Suggest why experiments involving tetracarbonylnickel are very hazardous.
• 17M.1.hl.TZ2.8: Ammonia is a stronger ligand than water. Which is correct when concentrated aqueous...
• 17M.2.hl.TZ2.2b.iii: Explain why iron forms many different coloured complex ions.
• 17N.2.hl.TZ0.3d.i: State the shape of the complex ion.
• 17N.2.hl.TZ0.3d.ii: Deduce the charge on the complex ion and the oxidation state of cobalt.
• 17N.2.hl.TZ0.3e: Describe, in terms of acid-base theories, the type of reaction that takes place between the...
• 18M.2.hl.TZ1.1h: Describe the bond formation when urea acts as a ligand in a transition metal complex ion.
• 18M.2.hl.TZ2.3d: Explain why transition metals exhibit variable oxidation states in contrast to alkali metals.  

13.2 Coloured complexes

• 15M.1.hl.TZ1.8: Which statements are correct about the complex...
• 15M.1.hl.TZ2.8: Which species cannot act as a ligand? A.     \({\text{NH}}_4^ + \) B.    ...
• 15M.2.hl.TZ2.8c.iii: Chromium forms the complex ion...
• 15M.2.hl.TZ2.8c.iv: Chromium forms the complex ion...
• 14M.1.hl.TZ1.8: Which ion is colourless? A.    ...
• 14M.2.hl.TZ1.5d.iii: Explain why the...
• 14N.1.hl.TZ0.8: Cobalt forms the complex...
• 14N.3.hl.TZ0.2c: (i)     Describe why adding excess ammonia to aqueous copper(II) ions causes the shade of the...
• 13N.1.hl.TZ0.8: Which compound is likely to be colourless? A.    ...
• 13N.2.hl.TZ0.4d: Substances like EUK-134 are often coloured. Explain why compounds of transition metals absorb...
• 13M.2.hl.TZ2.5d.ii: Explain why the complex [Cr(H2O)3Cl3] is coloured.
• 12N.2.hl.TZ0.2b: (ii)     Cobalt is a transition metal. One common ion of cobalt is...
• 12N.3.hl.TZ0.A5a: Two octahedral chromium complexes are...
• 10N.2.hl.TZ0.3e: Explain the origin of colour in transition metal complexes and use your explanation to suggest...
• 10N.3.hl.TZ0.A3b: (i)     The energy level diagram showing the electrons in the five 3d orbitals of a chromium atom...
• 09N.1.hl.TZ0.9: Which process is responsible for the colour of a transition metal complex? A.     The absorption...
• 09N.3.hl.TZ0.A4: The complex ion...
• 10M.2.hl.TZ1.1c.ii: Explain why the copper solution is coloured.
• 10M.3.hl.TZ1.A3b: When excess ammonia solution is added to a solution of copper(II) sulfate the oxidation number of...
• 10M.2.hl.TZ2.6f.i: State and explain the type of reaction that takes place between \({\text{F}}{{\text{e}}^{3 + }}\)...
• 10M.2.hl.TZ2.6f.ii: Explain why...
• 09M.2.hl.TZ1.8c.ii: Explain why copper(II) compounds in aqueous solution are coloured whereas scandium(III) compounds...
• 09M.2.hl.TZ2.3a.iv: Explain why the complex...
• 11M.1.hl.TZ1.9: Which electron transitions are responsible for the colours of transition metal compounds? A.   ...
• 11M.3.hl.TZ1.A4b: Copper(II) sulfate forms a pale blue aqueous solution. When aqueous ammonia is added to this,...
• 11M.1.hl.TZ2.8: Ligands can form dative covalent bonds with metal ions to form complex ions. Which of the...
• 11M.2.hl.TZ2.3c.ii: Explain why the...
• 12M.1.hl.TZ2.8: Which complex is colourless in solution? A.    ...
• 12M.2.hl.TZ2.9a: (i)     State the full electron configuration of Fe. (ii)     State the abbreviated electron...
• 12M.3.hl.TZ2.A4a: Transition metal complexes are coloured because electronic transitions occur within split d...
• 11N.2.hl.TZ0.7e.iii: Explain why the complex...
• 16M.1.hl.TZ0.10: Which best explains why transition metal complexes are coloured? A. As electrons return to...
• 16M.2.hl.TZ0.4d: In an aqueous solution of vanadium(III) chloride, the vanadium exists as [V (H2O)6]3+, [VCl...
• 16N.1.hl.TZ0.10: What is the correct explanation for the colour of [Cu(H2O)6]2+? A. Light is absorbed when an...
• 16N.1.hl.TZ0.9: The oxidation state of cobalt in the complex ion [Co(NH3)5Br]x is +3. Which of the...
• 17M.2.hl.TZ1.2f: Outline why transition metals form coloured compounds.
• 17M.2.hl.TZ2.2b.iii: Explain why iron forms many different coloured complex ions.
• 17N.1.hl.TZ0.10: [CoCl6]3– is orange while [Co(NH3)6]3+ is yellow. Which statement is correct? A. [CoCl6]3–...
• 18M.1.hl.TZ1.8: Which complex has the greatest d orbital splitting?
• 18M.1.hl.TZ2.8: Part of the spectrochemical series is shown for transition metal complexes. I−< Cl− < H2O...