Consider the metal complexes shown below. Identify the geometry of each complex. trigonal planar tetrahedral square trigonal planar bipyramidal octahedral [Fe(H₂O)]²+ [Fe(CN).]4- Consider the metal complexes shown below. Identify if the ligands present in each complex is weak field or strong field. weak field strong field [Fe(H₂O)]²+ [Fe(CN)<]4- linear trigonal prismatic

Consider the metal complexes shown below. Identify the geometry of each complex. trigonal planar tetrahedral square trigonal planar bipyramidal octahedral [Fe(H₂O)]²+ [Fe(CN).]4- Consider the metal complexes shown below. Identify if the ligands present in each complex is weak field or strong field. weak field strong field [Fe(H₂O)]²+ [Fe(CN)<]4- linear trigonal prismatic

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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10. Ethylenediamine, abbreviated "en" is a bidentate ligand in which its nitrogen atom (N) forms a coordinate covalent bond with cobalt. Draw the two geometric isomers of the octahedral complex of [Co(en)2Br2]*3
For the complex ion shown below, give the ligand's name as it would appear in the name of the complex ion. 2+
The octahedral structure is not the only possible six-coordinate structure. Other possibilities include a planar hexagonal structure, and a triangular prism structure. In the latter, the ligands are arranged in two parallel triangles, one lying above and the other below the metal atom with their corners aligned in the same directions (the lecture notes has pictures of this geometry). Show that the existence of two and only two isomers of [Co(NH3)4Cl2]+ is evidence against both of these structures.
Some octahedral complexes have distorted shapes. Insome, two metal-ligand bonds that are 180° apart are shorter than the other four. In [Cu(NH₃)₆]²⁺, for example, two Cu−N bonds are 207 pm long, and the other four are 262 pm long. (a) Calculate the longest distance between two N atoms in this complex. (b) Calculate the shortest distance between two N atoms.
Consider the following complex ions: [NiBr6]4-,[Ni(H2O)6]3+ and [Ni(CO)6]3+. Using the Crystal Field Theory, in each case (i) draw d-orbital electron configurations (ii) determine the number of unpaired electrons (iii) predict the magnetic properties (iv) state and explain the complex is high-spin or low-spin.
What is the charge on each of the following complex ions? hexaaquairon(II), [Fe(H2O)6]? tris(carbonato)ferrate(III), [Fe(CO3)3]? diaquatetrachlorovanadate(III), [V(H2O)2Cl4]? Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).
Name the following metal complexes or complex ions: formula name [Fe(OH), (en),] [V(CN),(NH,).] TiF ?
When oxalate (chemical formula: C₂04²; ligand abbreviation: ox) is added to an aqueous solution of nickel(II), the octahedral complex [Ni(ox)3]4 is produced. Given that complex formation is sequential, which reaction corresponds to the stability constant, B₂? O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) = [Ni(ox)₂]4- (aq) + 6 H₂0 (1) O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) = [Ni(0x)2(H₂O)4]² (aq) + 2 H₂O(1) O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) ⇒ [Ni(ox)₂(H₂O)2]² (aq) + 4H₂O(1) O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) = [Ni(ox)₂]² (aq) + 6 H₂0 (1)
A chemist prepared aqueous solutions of the following complex ions: [Cr(OH)6]³, [Cr(NH3)6]³+, and [Cr(NH3)5Cl]²+. He obtained 3 different colors of solution: green, red-violet, and yellow. Match the colored solutions with the correct complex ion. O [Cr(NH3)6]³+ is red-violet; [Cr(NH3)5Cl]²+ is yellow; [Cr(OH)]³- is green O [Cr(NH3)6]³+ is yellow; [Cr(NH3)5Cl]²+ is red-violet; [Cr(OH)6]³¯ is green O [Cr(NH3)]³+ is yellow; [Cr(NH3) 5Cl]²+ is green; [Cr(OH)6]³ is red-violet [Cr(NH3)6]³+ is green; [Cr(NH3)5Cl]²+ is red-violet; [Cr(OH)]³ is yellow
Answer the following questions about the transition metals complexes with the chemical formulas [Co(en)3]3+and [CoCl6]3- Would either the low-spin or high-spin configuration result in a paramagnetic complex? One of the complexes is orange while the other is blue. Which cobalt complex is which color? Justify your answer and identify which color the complex will absorb based on its color.
The energies of the valence d orbitals on the manganese atom in the octahedral [MnF] complex are split according to the electron box level diagram below. (Note: the d orbitals are labeled with just their subscript, to make the labels easier to read.) Complete the diagram by adding the correct number of electrons to each orbital. energy xy 2 yz 2 2 XZ 1 l X S
Indicate the Geometry, total number of "d" and number of unpaired "d" electrons in each of the complex ions shown below. a) Geometry b) Total (valence) "d" electrons c) Number of Unpaired electrons [Pt(en)2]+2 [Re(en)(H2O)4]+2 (high spin) [Fe(CN)6]−3 (low spin)