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Questions and Answers
Which metal ions have two vacant d orbitals available for octahedral hybridisation?
Which metal ions have two vacant d orbitals available for octahedral hybridisation?
What is the general effect of having more than three 3d electrons on octahedral hybridisation?
What is the general effect of having more than three 3d electrons on octahedral hybridisation?
Which coordination compound of manganese shows a magnetic moment corresponding to two unpaired electrons?
Which coordination compound of manganese shows a magnetic moment corresponding to two unpaired electrons?
Which coordination compound of iron has a magnetic moment of a single unpaired electron?
Which coordination compound of iron has a magnetic moment of a single unpaired electron?
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Why do compounds containing d4 and d5 ions present complications in magnetic behavior?
Why do compounds containing d4 and d5 ions present complications in magnetic behavior?
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What is the magnetic characteristic of [Co(C2O4)3]?
What is the magnetic characteristic of [Co(C2O4)3]?
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How many unpaired electrons are found in [FeF6]3–?
How many unpaired electrons are found in [FeF6]3–?
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What phenomenon causes the differences in magnetic moments among compounds of the same metal ion?
What phenomenon causes the differences in magnetic moments among compounds of the same metal ion?
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What is the color of the complex [Co(NH3)6]3Cl?
What is the color of the complex [Co(NH3)6]3Cl?
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Which of the following complexes corresponds to a 1:3 electrolyte?
Which of the following complexes corresponds to a 1:3 electrolyte?
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What term describes compounds like [CoCl2(NH3)4]Cl that have identical empirical formulas but distinct properties?
What term describes compounds like [CoCl2(NH3)4]Cl that have identical empirical formulas but distinct properties?
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According to Werner's theory, what type of valences are satisfied by negative ions?
According to Werner's theory, what type of valences are satisfied by negative ions?
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Which geometric shapes are mentioned as common in coordination compounds of transition metals?
Which geometric shapes are mentioned as common in coordination compounds of transition metals?
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What does the coordination number refer to in coordination compounds?
What does the coordination number refer to in coordination compounds?
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Which complex is correctly matched with its empirical formula?
Which complex is correctly matched with its empirical formula?
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What is the solution conductivity of the complex [CoCl(NH3)5]2Cl?
What is the solution conductivity of the complex [CoCl(NH3)5]2Cl?
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What color is observed for the coordination entity [CoCl(NH3)5] when it absorbs yellow light?
What color is observed for the coordination entity [CoCl(NH3)5] when it absorbs yellow light?
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For the coordination entity [Co(NH3)5(H2O)]3+, which color is observed?
For the coordination entity [Co(NH3)5(H2O)]3+, which color is observed?
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What is the role of the absorbed wavelength in determining the color of coordination entities?
What is the role of the absorbed wavelength in determining the color of coordination entities?
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Which color is absorbed by the coordination compound [Cu(H2O)4]2+?
Which color is absorbed by the coordination compound [Cu(H2O)4]2+?
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In the context of crystal field theory, what happens when light corresponding to the blue-green region is absorbed by [Ti(H2O)6]3+?
In the context of crystal field theory, what happens when light corresponding to the blue-green region is absorbed by [Ti(H2O)6]3+?
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Which of the following coordination entities appears pale yellow?
Which of the following coordination entities appears pale yellow?
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What is the next higher energy state for the electron in [Ti(H2O)6]3+ after the t2g level?
What is the next higher energy state for the electron in [Ti(H2O)6]3+ after the t2g level?
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Which of the following coordination entities absorbs light in the ultraviolet region?
Which of the following coordination entities absorbs light in the ultraviolet region?
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What does crystal field theory primarily consider the metal-ligand bond to be?
What does crystal field theory primarily consider the metal-ligand bond to be?
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What happens to the d orbitals in an isolated gaseous metal atom/ion?
What happens to the d orbitals in an isolated gaseous metal atom/ion?
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In an octahedral coordination, which d orbitals experience more repulsion from ligands?
In an octahedral coordination, which d orbitals experience more repulsion from ligands?
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What is the outcome when the degeneracy of d orbitals is lifted in crystal field theory?
What is the outcome when the degeneracy of d orbitals is lifted in crystal field theory?
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What type of splitting occurs in a crystal field with octahedral coordination?
What type of splitting occurs in a crystal field with octahedral coordination?
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How does the presence of ligands affect the energy levels of d orbitals?
How does the presence of ligands affect the energy levels of d orbitals?
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Which statement regarding ligands is accurate in the context of crystal field theory?
Which statement regarding ligands is accurate in the context of crystal field theory?
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What does crystal field theory fail to predict accurately for 4-coordinate complexes?
What does crystal field theory fail to predict accurately for 4-coordinate complexes?
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What geometry does tetracarbonylnickel(0) exhibit?
What geometry does tetracarbonylnickel(0) exhibit?
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Which of the following homoleptic carbonyls has a trigonal bipyramidal geometry?
Which of the following homoleptic carbonyls has a trigonal bipyramidal geometry?
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What kind of bond is present in octacarbonyldicobalt(0) that connects two cobalt atoms?
What kind of bond is present in octacarbonyldicobalt(0) that connects two cobalt atoms?
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The structure of hexacarbonyl chromium(0) is categorized as which of the following?
The structure of hexacarbonyl chromium(0) is categorized as which of the following?
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What is the primary type of bonding in metal carbonyls?
What is the primary type of bonding in metal carbonyls?
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What type of bonds do the metal-carbon bonds in metal carbonyls possess?
What type of bonds do the metal-carbon bonds in metal carbonyls possess?
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What connects the two square pyramidal units in decacarbonyldimanganese(0)?
What connects the two square pyramidal units in decacarbonyldimanganese(0)?
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Which statement is true regarding the formation of the M–C s bond in metal carbonyls?
Which statement is true regarding the formation of the M–C s bond in metal carbonyls?
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Study Notes
Cobalt(III) Chloride-Ammonia Complexes
- There are four stable cobalt(III) chloride-ammonia complexes with different colours and conductivities.
- The colour and conductivity of the complexes are determined by the number of chloride ions outside the coordination sphere.
- Yellow [Co(NH3)6]3+ 3Cl- is a 1:3 electrolyte, meaning it dissociates into four ions in solution.
- Purple [CoCl(NH3)5]2+ 2Cl- is a 1:2 electrolyte, meaning it dissociates into three ions in solution.
- Green [CoCl2(NH3)4] + Cl- is a 1:1 electrolyte, meaning it dissociates into two ions in solution.
- Violet [CoCl2(NH3)4] + Cl- is a 1:1 electrolyte, meaning it dissociates into two ions in solution.
- The green and violet complexes have the same empirical formula, CoCl3.4NH3, but different properties, making them isomers.
Werner's Theory of Coordination Compounds
- Werner's theory explains the bonding and structure of coordination compounds.
- It describes two types of valences: primary and secondary.
- Primary valences are ionizable and satisfied by negative ions, while secondary valences are non-ionizable and satisfied by neutral molecules or negative ions.
- Secondary valence equals the coordination number and is fixed for a specific metal.
- Ions/groups bound by secondary linkages to the metal have specific spatial arrangements called coordination polyhedra.
- Coordination entities or complexes are enclosed in square brackets, while ions outside the brackets are counter ions.
- Common coordination polyhedra in transition metal complexes include octahedral, tetrahedral, and square planar.
Magnetic Properties of Coordination Compounds
- The magnetic properties of coordination compounds are determined by the number of unpaired electrons in the metal ion.
- Coordination compounds with up to three d electrons have two vacant d orbitals for octahedral hybridisation, resulting in similar magnetic behaviour to their free metal ions.
- When more than three d electrons are present, pairing of d electrons is required for octahedral hybridisation, influencing magnetic behaviour.
- Magnetic data generally agrees with maximum spin pairing, especially for d6 complexes.
- Exceptions exist for d4 and d5 complexes. For example, [Mn(CN)6]3- has two unpaired electrons while [MnCl6]3- has four unpaired electrons.
- Werner's theory has limitations, failing to predict tetrahedral and square planar structures for four-coordinate complexes and to distinguish between weak and strong ligands.
Crystal Field Theory
- Crystal Field Theory (CFT) explains bonding and structure of coordination compounds using an electrostatic model.
- CFT considers the metal-ligand bond as purely ionic, arising from electrostatic interactions between the metal ion and ligands.
- Ligands are treated as point charges for anions or point dipoles for neutral molecules.
- In an isolated metal atom/ion, all five d orbitals are degenerate (have the same energy).
- This degeneracy is lifted when a non-spherical field of negative charges from ligands surrounds the metal atom/ion.
- The splitting pattern of d orbitals depends on the crystal field.
- In octahedral coordination entities, ligands cause repulsion with metal d orbitals, leading to energy splitting.
- d x2-y2 and d z2 orbitals, pointing towards ligands, experience greater repulsion and are raised in energy.
- dxy, dyz, and dxz orbitals, directed between axes, are lowered in energy.
Colour of Coordination Compounds
- The colour of coordination compounds is explained by CFT and relates to the absorption of specific wavelengths of light.
- The colour observed is the complementary colour of the absorbed light.
- For example, [Ti(H2O)6]3+ appears violet because it absorbs blue-green light.
- Light absorption excites an electron from a lower energy level (t2g) to a higher energy level (eg).
Metal Carbonyls
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Homoleptic carbonyls are compounds containing only carbonyl ligands and form readily with most transition metals.
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They exhibit well-defined structures such as tetrahedral, trigonal bipyramidal, and octahedral.
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Examples include:
- Tetracarbonylnickel(0) - tetrahedral
- Pentacarbonyliron(0) - trigonal bipyramidal
- Hexacarbonyl chromium(0) - octahedral
- Decacarbonyldimanganese(0) - two square pyramidal units joined by a Mn-Mn bond
- Octacarbonyldicobalt(0) - Co-Co bond bridged by two CO groups
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The metal-carbon bond in metal carbonyls has both σ and π character.
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The σ bond is formed by donation of the lone pair from the carbonyl carbon to a vacant metal orbital.
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Explore the fascinating world of cobalt(III) chloride-ammonia complexes through this quiz. Learn about their colors, conductivities, and the principles underlying Werner's theory of coordination compounds. Test your understanding of this important topic in coordination chemistry.