Explain the stability of the complexes TiCl62- and [Zn(en)3]2+

Q: Briefly speculate on why many cobalt (III) compounds are prepared by oxidizing CO(II) salts rather…

A:

Q: In the coordination compound (NH4)2[Fe(OH2)F5 ], the Fe complex is octahedral. a) Given that F- is a…

A: Given that NH4)2[Fe(OH2)F5 is a octahedral complex

Q: The octahedral complex [Ti(H2O)6]3+ has a single d electron. To excite this electron from the ground…

A: First find frequency as follows,

Q: Why are low spin tetrahedral complexes not formed?

A: The division of d-orbitals present in central metal ion in sets of two different energies occur in…

Q: Which ions are unlikely to form colored coordination complexes in an octahedral ligand environment?…

A: Colour for the complex is arise due to electronic transition. If no any transition possible compound…

Q: For each of the following pairs of complexes, identify the one that has the larger Crystal field…

A:

Q: The zinc(II) complexes have greater stability than the copper(II) complexes. Explain.

A: Applying concept of realation between stability and hydration energy of metal ion .

Q: For the low spin coordination compound [Fe(en)2Cl]Cl, identify the Oxidation number of iron

A: Note : I think the complex should [Fe(en)2Cl2]Cl. So I'm giving answer for both the complex.

Q: Draw all the possible geometrical isomers for the complex [Cr(en),(CN),]*

A:

Q: (b) Give 5 properties of metal ions that will affect the structure and bonding in coordination…

A: The answer is attached below-

Q: What is the coordination number of the central metal in [Cr(acac)3] ?  The acac ligand can be…

A: Coordination number of the central metal which is Chromium in [Cr(acac)3]  is 6.

Q: Name the following coordination compound: K3[CrF6].

A: Coordination compounds: These are complexes that have a metal centre attached to groups of atoms.…

Q: Explain the differences between high-spin and low-spin metal complexes.

A: Complexes with weak field ligands have the same number of unpaired electrons as the free metal ion…

Q: Explain why many transition metal complexes are paramagnetic?

A: ANSWER IS DISCUSSED BELOW :

Q: Differentiate between monodentate ligands, bidentate ligands,and polydentate ligands?

A: Difference between monodentate ligands, bidentate ligands,and polydentate ligands has to be given,

Q: Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a)…

A: a) The given compound is [V(H2O)6]3+ The Oxidation state of ‘V’ is +3. The electronic configuration…

Q: The complex [COF6]¯ absorbs light at a wavelength of 290 nm. What is the value of the crystal filed…

A:

Q: why do some d-block elements form colored complexes with various ligands

A: in complexes of the transition metals the D orbitals do not all have the same energy. the pattern of…

Q: 9 A complex with the composition [MA₂B₂]X₂ is found to have no geometrical isomers. Both A and B are…

A:

Q: The absorption spectrum of the complex ion [Rh(NH,)6+ has maximum absorbance at 295 nm. Calculate…

A: Given, Maximum absorbance of the ion  295 nm ∆ = hc/ λ = [( 6.626 x 10 -34 Js ) x ( 3 x 10 8 m/s) x…

Q: The coordination complex [Cr(CO)6] forms colorless, diamagnetic crystals that melt at 90 °C. Given…

A: A substance is diamagnetic in nature if all the electrons are paired. For a complex to be colored,…

Q: Though both [COF6]3 and [Co(CN)6]³- octahedral complexes, the crystal field stabilization energy…

A: If weak field ligand is present,than no pairing occur and filling of electron occur according to…

Q: Let us consider the following coordination complexes: [Fe(CN6)]3- Given that the chloride ion and…

A: The given coordination complex is a cyanide containing complex, and cyanide is a strong field…

Q: Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a)…

A:

Q: The coordination complex [Cr(CO)6] forms colorless, diamagnetic crystals that melt at 90 °C. What is…

A: The oxidation number of chromium in Cr(CO)6 has to be given.

Q: Why are tetrahedral complexes high spin?

A: In tetrahedral molecular geometry, a central atom is located at the center of four substituent…

Q: A coordination compound has been determined to be composed of 18.4% Co, 26.6% NH3, 30.0% SO4 , and…

A: A co-ordination compound is a compound containing a central metal atom bound to ligands. The central…

Q: (c) Explain crystal field splitting in the case of tetrahedral complexes.

A: Crystal field splitting in tetrahedral complexes:

Q: What is the coordination number for the transition metal in the following complexes?   a)…

A: Coordination number : it is the total number of atoms are attached to the central atom.

Q: A complex absorbs photons with an energy of 4.51 * 10-19 J. If this is the only place in the visible…

A: Given: Energy, E=4.51×10-19 J

Q: What is the coordination number of the central metal in [Co(en)3]Cl2 ?  The en (NH2CH2CH2NH2)…

A: The coordination number of Co is calculated below.  The coordination sphere is  [Co(en)3]2+

Q: Explain why tetrahedral complexes are mostly low-spin or high-spin.

A: The central atom in the tetrahedral geometry is linked to four surrounding atoms. All of these are…

Q: What is the oxidation state of the metal centre in the [Cr(CO3)3(C6H6)] complex?

A: Explanation-       Cr(CO3)3(C6H6)] complex is the name (η 6 -benzene ) tricarbonyl chromium(0).…

Q: Using crystal field theory, prove [NiCl4]2¯ is a tetrahedral paramagnetic complex.

A: Crystal field theory ia an electrostatic model which considers the metal-ligand bond to be ionic…

Q: Use your knowledge of electronic transitions in coordination compounds to justify why the compound…

A: If a sample absorbs all wavelengths of visible light, none reaches our eyes from that sample, and…

Q: 7. For an octahedral transition metal complex with maximum absorbance at a wavelength of 580 nm,…

A:

Q: Arrange the following complexes in terms of ligand strength: [Cr(OH)6]3–, [Cr(NH3)6]3+, and…

A: The ligand strength is determined by the value of ∆° ie splitting energy. Various ligands are…

Q: 4. Using crystal field theory, prove [NiCla]²- is a tetrahedral paramagnetic complex.

A: The given complex is NiCl42-, has nickel metal as the central metal atom and the ligands are four…

Q: Explain the bonding in coordination compounds in terms of Werner's nostulate

A:

Q: Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a)…

A: (a)

Q: 9 A complex with the composition [MA₂B₂]X₂ is found to have no geometrical isomers. Both A and B are…

A: [MA2B2]X2 ->The coordination number of metal is 4.

Q: Given: CN^- is a stronger field ligand compared to SCN^-. Briefly explain why a complex formed…

A: CN- is strong field ligand than SCN- ,          When it forms complex with Iron. There will be…

Q: What is the coordination number for the transition metal in the following complexes? a)…

A: To calculate coordination numbers of complexes , we have to look about ligands surrounding the…

Q: Give the IUPAC name for this coordination compound. [Cr(H, O),CIJSO4

A: Write IUPAC name of the given coordination compound-

Q: why d³ and d⁸ high spin complexes are more stable than other configurations?

A: High spin complexes: According to crystal field theory, two types of complexes are formed. High spin…

Q: Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a)…

A:

Q: What are the electron configurations for an octahedral d7 complex with 1 weak-field and 2…

A: Strong field ligands: Those ligands which cause larger splitting of d orbitals and favour pairing of…

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.