Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781337128391
Author: Darrell Ebbing, Steven D. Gammon
Publisher: Cengage Learning
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Chapter 22, Problem 22.19QP
Interpretation Introduction
Interpretation:
The formation of co-ordinate covalent bond between a metal-ion orbital and a ligand orbital has to be explained.
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Give two examples of ligands which form coordination compounds useful in analytical chemistry.
What is the most crucial feature that a molecule should have so that it can be considered a ligand?
Presence of at least one pair of unshared electrons
Presence of a hydrogen atom
Presence of an unfilled d orbital
Presence of an acidic group
The molecule CO is a common ligand in transition metal complexes forming a strong
bond with the metal ion.
b) Based on Lewis structure of CO, which end of the CO molecule do you think is
the electron source to form the metal-ligand bond? Why?
Chapter 22 Solutions
Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2, 4 terms (24 months) Printed Access Card
Ch. 22.3 - Another complex studied by Werner had a...Ch. 22.4 - Prob. 22.1ECh. 22.4 - Prob. 22.2ECh. 22.5 - Prob. 22.2CCCh. 22.5 - Prob. 22.3ECh. 22.5 - Prob. 22.4ECh. 22.5 - Prob. 22.3CCCh. 22.7 - Prob. 22.5ECh. 22.7 - Prob. 22.6ECh. 22.7 - Prob. 22.7E
Ch. 22 - What characteristics of the transition elements...Ch. 22 - Prob. 22.2QPCh. 22 - Prob. 22.3QPCh. 22 - Prob. 22.4QPCh. 22 - Prob. 22.5QPCh. 22 - Prob. 22.6QPCh. 22 - Prob. 22.7QPCh. 22 - Prob. 22.8QPCh. 22 - Silver(I) ion in basic solution is reduced by...Ch. 22 - What evidence did Werner obtain to show that the...Ch. 22 - Define the terms complex ion, ligand, and...Ch. 22 - Prob. 22.12QPCh. 22 - Prob. 22.13QPCh. 22 - Prob. 22.14QPCh. 22 - Prob. 22.15QPCh. 22 - Prob. 22.16QPCh. 22 - Explain the difference in behavior of d and l...Ch. 22 - Prob. 22.18QPCh. 22 - Prob. 22.19QPCh. 22 - a Describe the steps in the formation of a...Ch. 22 - Prob. 22.21QPCh. 22 - Prob. 22.22QPCh. 22 - Prob. 22.23QPCh. 22 - Prob. 22.24QPCh. 22 - Prob. 22.25QPCh. 22 - Prob. 22.26QPCh. 22 - Prob. 22.27QPCh. 22 - Prob. 22.28QPCh. 22 - What is the correct name for the coordination...Ch. 22 - Prob. 22.30QPCh. 22 - Prob. 22.31QPCh. 22 - Prob. 22.32QPCh. 22 - Prob. 22.33QPCh. 22 - Prob. 22.34QPCh. 22 - Prob. 22.35QPCh. 22 - Prob. 22.36QPCh. 22 - Prob. 22.37QPCh. 22 - Prob. 22.38QPCh. 22 - Prob. 22.39QPCh. 22 - Prob. 22.40QPCh. 22 - Prob. 22.41QPCh. 22 - Prob. 22.42QPCh. 22 - Prob. 22.43QPCh. 22 - Prob. 22.44QPCh. 22 - Consider the complex ion [CoCl(en)2(NO2)]+. a What...Ch. 22 - Prob. 22.46QPCh. 22 - Prob. 22.47QPCh. 22 - Name the following complexes, using IUPAC rules. a...Ch. 22 - Prob. 22.49QPCh. 22 - Prob. 22.50QPCh. 22 - Prob. 22.51QPCh. 22 - Give the structural formula for each of the...Ch. 22 - Prob. 22.53QPCh. 22 - Prob. 22.54QPCh. 22 - Prob. 22.55QPCh. 22 - Prob. 22.56QPCh. 22 - Prob. 22.57QPCh. 22 - Prob. 22.58QPCh. 22 - Prob. 22.59QPCh. 22 - Prob. 22.60QPCh. 22 - Prob. 22.61QPCh. 22 - Prob. 22.62QPCh. 22 - Prob. 22.63QPCh. 22 - Prob. 22.64QPCh. 22 - Prob. 22.65QPCh. 22 - Prob. 22.66QPCh. 22 - Prob. 22.67QPCh. 22 - Prob. 22.68QPCh. 22 - There are only two geometric isomers of the...Ch. 22 - Prob. 22.70QPCh. 22 - Prob. 22.71QPCh. 22 - Prob. 22.72QPCh. 22 - Prob. 22.73QPCh. 22 - Prob. 22.74QPCh. 22 - Prob. 22.75QPCh. 22 - Prob. 22.76QPCh. 22 - Consider the complex ion [CoCO3(NH3)4], where the...Ch. 22 - Prob. 22.78QPCh. 22 - Prob. 22.79QPCh. 22 - Prob. 22.80QPCh. 22 - Prob. 22.81QPCh. 22 - Prob. 22.82QPCh. 22 - What is the name of K2[MoOCl4]?Ch. 22 - Write the formula and draw the structure of...Ch. 22 - Prob. 22.85QPCh. 22 - Prob. 22.86QPCh. 22 - Is it possible to have a paramagnetic...Ch. 22 - Prob. 22.88QPCh. 22 - Prob. 22.89QPCh. 22 - Prob. 22.90QPCh. 22 - Prob. 22.91QPCh. 22 - Prob. 22.92QP
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- Draw a molecular orbital diagram to show that CH3 molecule is a o-donor ligand.arrow_forwardHow does Ligand Field Theory explain the interaction between the ligand with the central metal leading to increase or decrease of Δo ? Use the concepts of π-donor and π-acceptor ligands.arrow_forwardDraw the Lewis structure of NH₃. Can this molecule act as a ligand?arrow_forward
- Coordination Compounds form when one or more ligands donate lone pairs to a transition metal forming a dative bond. Consider different structural aspects of coordination compounds. A ligand must have a lone pair of electrons to donate to the transition metal. Usually, drawing a Lewis structure is the best way to determine whether a compound has a lone pair. Draw the Lewis structure of BF,. 3' Can this molecule act as a ligand?arrow_forward11) In aqueous solution, Beryllium ion becomes attached to four water molecules to give a complex ion with the formula [Be(H2O)4]2+. Explain this chemistry using valence bond theory.arrow_forwardThe complex [Fe(H2O)6]+2 exhibits only σ-donor behavior. Using ligand field theory, draw the molecular orbital diagram mixing the d-orbitals on the metal and the molecular orbitals on the ligands and fill in the available electrons. What is the nature of the t2g orbitals that are part of Δo, bonding, antibonding, or non-bonding? Explain your answer.arrow_forward
- Apply the concept of crystal-field theory to explain some of the interesting spectral and magnetic properties of coordination compounds?arrow_forwardConsider an octahedral complex where strong field ligands are bound to a central metal having a d electronic configuration of 3d5. Which of the following is most likely to be TRUE about the 3d orbitals in this complex following the concept of valence bond theory? The five 3d orbitals are split into two levels, with three orbitals in the lower level. All the 3d orbitals are occupied so hybridization of orbitals involves the vacant 4s, 4p, and 4d orbitals, forming six sp3d2 hybrid orbitals. The five 3d orbitals are split into two levels, with three orbitals in the upper level. There are two vacant 3d orbitals, and these may combine with the unoccupied 4s and 4p orbitals to form six d2sp3 hybrid orbitals.arrow_forward3a) The nitrosyl ion, NO*, is a very rare case of a cationic ligand that can function as a Lewis base. Draw the Lewis structure of this ligand under consideration of the VSEPR rules and indicate any formal charges on the constituent atoms. 3b) How many electrons does the NO* ligand contribute on the ionic model and the neutral model, respectively? Assume that the Metal-N-O bonding angle is 180° upon coordination.arrow_forward
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