Atomic structure - transition metals-revision

Transition metal revision

The bonds within the water molecule are polar covalent.
Water molecules bond more strongly to Fe³⁺ than to Fe²⁺ because of the greater charge on the ion leading to a greater electrostatic force of attraction.

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Transition metals can form coloured compounds. Cobalt, iron and copper. Zinc is a transition metal but does not form coloured compounds. The reason for this is that all its 3d orbitals are full.

All transition metals can form complex ions.
Zn(H₂O)₆⁺², Fe(H₂O)₆⁺², Cu(H₂O)₆⁺², CoCl₄^-2.

Group 1 and 2 elements are metals that can form ions with only one oxidation state. In this case it is Na.

Group 1 and 2 metals can form basic oxides that are not coloured. In this case it is Na.

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Transition metals have electrons in a "d" subshell. Since the "d" subshell can accomodate up to ten electrons we have a series of ten transtion metals.

One series for the 3d another for the 4d and so on.

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Polar molecules, such as NH₃ and H₂O, can be attracted to the Fe³⁺ ion and form ligands via ion-dipole bonding.

Negative ions, such as OH^- can also form ligands with Fe³⁺ via ion-ion bonding

Positive ions are unlikely to form ligands as there will be no electrostatic force of attraction.

Transition metal revision
Sketch the complex ion Fe(H₂O)₆³⁺ Label the bonds: - between the Fe³⁺ ion and the H₂O molecule - within the H₂O molecule. Suggest a reason why H₂O might bond more strongly to Fe³⁺ than to Fe²⁺	The bonds within the water molecule are polar covalent. Water molecules bond more strongly to Fe³⁺ than to Fe²⁺ because of the greater charge on the ion leading to a greater electrostatic force of attraction. Hide the solution Hide solution Transition metals can form coloured compounds. Cobalt, iron and copper. Zinc is a transition metal but does not form coloured compounds. The reason for this is that all its 3d orbitals are full. All transition metals can form complex ions. Zn(H₂O)₆⁺², Fe(H₂O)₆⁺², Cu(H₂O)₆⁺², CoCl₄^-2. Group 1 and 2 elements are metals that can form ions with only one oxidation state. In this case it is Na. Group 1 and 2 metals can form basic oxides that are not coloured. In this case it is Na. Solution
Most transition metals form coloured compounds. Suggest a reason why this is so. Explain why zinc does not form coloured compounds.	Solution
Manganese exhibits many oxidation states. Explain why the greatest oxidation state of manganese is +7. Give the oxidation state of manganese in the following. Mn MnO Mn₂O₃ Explain why calcium has only one oxidation state while iron exists as a 3+ or 2+ ion.	Solution
Explain why the electronic configuration given below is not found amongst the transition metals. 1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁴, 4s² Give the likely electronic configuration
Why does a series of transition metals have 10 elements?	Solution Hide solution Transition metals have electrons in a "d" subshell. Since the "d" subshell can accomodate up to ten electrons we have a series of ten transtion metals. One series for the 3d another for the 4d and so on.
Give the element in the first transition series that forms a 3+ ion with a half filled d sub shell.
Nitrogen, sodium, cobalt, iron, copper, zinc Which of the elements above: -can form coloured compounds; -can form complex ions; -is a metal and has only one oxidation state when it reacts to form different compounds. -can form a basic oxide that is not coloured.	Solution
Which one of the following is least likely to form a ligand with Fe³⁺ ions? NH_3,NH₄⁺, H₂O, OH^-	Solution Hide solution Polar molecules, such as NH₃ and H₂O, can be attracted to the Fe³⁺ ion and form ligands via ion-dipole bonding. Negative ions, such as OH^- can also form ligands with Fe³⁺ via ion-ion bonding Positive ions are unlikely to form ligands as there will be no electrostatic force of attraction.
What is the oxidation state of iron in the complex ion K₃[FeCl₆]?