Concept explainers
(a)
Interpretation: The oxidation number of the metal in the given compound has to be determined.
Concept introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
Oxidation number: The total number of electrons in an atom after losing or gaining electrons to make a bond with another atom. It indicates the charge of an ion.
(b)
Interpretation: The oxidation number of the metal in the given compound has to be determined.
Concept introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
Oxidation number: The total number of electrons in an atom after losing or gaining electrons to make a bond with another atom. It indicates the charge of an ion.
(c)
Interpretation: The oxidation number of the metal in the given compound has to be determined.
Concept introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
Oxidation number: The total number of electrons in an atom after losing or gaining electrons to make a bond with another atom. It indicates the charge of an ion.
(d)
Interpretation: The oxidation number of the metal in the given compound has to be determined.
Concept introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
Oxidation number: The total number of electrons in an atom after losing or gaining electrons to make a bond with another atom. It indicates the charge of an ion.
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Chapter 22 Solutions
Chemistry & Chemical Reactivity
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- For the low-spin coordination compound [Fe(en)2Cl2]Cl, identify the following.(a) the oxidation number of iron(b) the coordination number for iron(c) the coordination geometry for iron(d) the number of unpaired electrons per metal atom(e) whether the complex is diamagnetic or paramagnetic(f) the number of geometricisomersarrow_forwardLet us consider the following coordination complexes: [Fe(CN6)]3- Given that the chloride ion and the water molecule are weak field ligands whereas ammonia, CN- and CO are high field ligands, determine the electron structure of the cobalt complex ion using an energy diagram of the d orbitals established according to the crystal field theory.arrow_forwardFor the low-spin coordination compound [Fe(en)2Cl2]Cl, identify the following.(a) the oxidation number of iron(b) the coordination number for iron(c) the coordination geometry for iron(d) the number of unpaired electrons per metal atom(e) whether the complex is diamagnetic or paramagnetic(f) the number of geometric isomersarrow_forward
- Briefly speculate on why many cobalt (III) compounds are prepared by oxidizing CO(II) salts rather than by substitituting ligands in cobalt (III) complexes.arrow_forwardArrange the following complexes in terms of ligand strength: [Cr(OH)6]3–, [Cr(NH3)6]3+, and [Cr(NH3)5Cl]2+arrow_forwardIf this is the only place in the visible spectrum where the complex absorbs light, what color would you expect the complex to be?arrow_forward
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