25 Questions
What is the term used to describe a ligand that binds to a central metal atom through two atoms?
Bidentate
Which of the following ions has the same number of electrons as Cu+?
Mn2+
What is the oxidation state of iron in the ore ilmenite?
Fe3+
Why is vanadium less dense than chromium despite having the same crystal lattice?
Due to a difference in atomic radius
Which of the following elements would you expect to form an oxide with the formula MO3?
V
What type of bond is formed when a ligand donates a pair of electrons to a central metal atom?
Dative covalent bond
What is the term used to describe compounds containing a central metal atom bonded to surrounding ligands?
Coordination compounds
What is the oxidation number of the metal ion in the complex [Mn(NH3)6]SO4?
3+
What is the minimum requirement for a ligand to bond to a metal?
A lone pair of electrons
What is meant by the term 'coordinate covalent bond'?
A bond between a metal and a ligand, where both electrons are from the ligand
What is the coordination number of the complex [Co(NH3)4Cl2]Cl?
6
What is the correct formula for the complex [CrCl3NH3].2H2O?
[CrCl2NH3(H2O)]Cl.2H2O
What is the geometry of the complex [PtCl2(NH3)2]?
Square planar
What is the correct formula and name of the pink salt CoCl3.5NH3.H2O?
[CoCl2(NH3)(H2O)]Cl.2NH3, dichloroaquopentaamminecobalt(II) chloride
What is the geometry of the complex [Co(NH3)5NO2]+?
Octahedral
What is the reason behind the lanthanide contraction?
The lanthanide contraction is due to the poor shielding of the nuclear charge by the f-orbitals, resulting in a decrease in the atomic radius of the elements.
Why do transition metals exhibit a wide range of oxidation states?
Transition metals exhibit a wide range of oxidation states due to the ability of their d-orbitals to participate in bonding, resulting in the formation of multiple ions with different oxidation states.
What is the significance of the ionisation energy table in understanding the properties of transition metals?
The ionisation energy table is significant in understanding the properties of transition metals as it provides information about the energy required to remove electrons from the metal, which affects its reactivity and oxidation states.
What is the oxidation number of the metal ion in each of the following complexes: [Fe(NH3)6]2+ and [Zn(CN)4]2-?
The oxidation number of the metal ion in [Fe(NH3)6]2+ is 2+, and in [Zn(CN)4]2- is 2-.
What must a ligand have in order to bond to a metal, and what is meant by the term 'coordinate covalent bond'?
A ligand must have at least one lone pair of electrons to bond to a metal. A coordinate covalent bond is a type of bond where a ligand donates a pair of electrons to a metal atom.
How do the electronic configurations of transition metal ions influence their properties and uses?
The electronic configurations of transition metal ions influence their properties and uses by determining their oxidation states, reactivity, and ability to form complexes.
What is the role of coordination compounds in the uses of transition elements?
Coordination compounds play a crucial role in the uses of transition elements as they are often involved in catalytic reactions, biological systems, and pigment formations.
Determine the coordination number and predict the geometry of the complex species [Ir(en)3]3+.
The coordination number is 6, and the predicted geometry is octahedral.
Draw the correct structure of the complex [CrCl3NH3].2H2O, and explain why the original formula was incorrect.
The correct structure is [CrCl2NH3(H2O)]Cl.2H2O. The original formula was incorrect because it did not account for the water molecule bonded to the Cr atom.
Write the correct formula and name the pink salt CoCl3.5NH3.H2O, and predict its geometry.
The correct formula is [CoCl2(NH3)3(H2O)]Cl.2H2O, and the name is pentaaquamminedichlorocobalt(II) chloride. The predicted geometry is octahedral.
This worksheet covers transition elements, coordination compounds, and their properties. Exercises include naming complexes and writing formulas.
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