Coordination chemistry
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This document compares and contrasts double salts and coordination compounds. It states that double salts exist only in the solid state and dissociate into their constituent species in solution, losing their identity. Coordination compounds, however, retain their identity in both solid and solution states, and their properties differ from those of the constituent species. The document provides examples of each type of compound.
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This document discusses coordination chemistry and coordination complexes. It defines coordination complexes as compounds formed by the attachment of ligands to a central metal atom, retaining their identity in solution. Addition compounds, in contrast, lose their identity in solution. Coordination complexes find applications in medicine, biology, dyes, metallurgy, photography, and water purification. The central metal ion is usually a transition metal that accepts electron pairs from ligands. Ligands can be negatively charged, positively charged, or neutral. The coordination number refers to the number of donor atoms attached to the central ion, helping to predict the geometry. The central metal and ligands together form the coordination sphere.
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10.short%20 coordinate%20compounds
1. Coordinate compounds are complexes where a central metal ion is coordinated to surrounding ligands. Coordination compounds can be ionic or molecular and the ligands are attached to the central ion via coordinate bonds.
2. The ligands directly attached to the central metal ion make up its coordination sphere. The total number of ligands is the coordination number. Bidentate and tridentate ligands that attach at multiple points contribute more than one to the coordination number.
3. Coordinate compounds can exhibit several types of isomerism including ionization isomerism from interchange of ligands and ions, coordination isomerism from interchange of complex ions, and geometrical isomerism from different spatial arrangements of ligands.
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• Ligands
– an ion or molecule which donates electron density to a metal
atom/ion to form a complex
- Lewis base bonded (coordinated) to a metal ion in a coordination complex.
• Coordination Complex
– a central metal atom/ion and its set of ligands
– often an ion itself
• Coordination Compounds
– a neutral species made up in some part of a complex
– often the salt of a coordination complex
• Coordination Number
– the number of ligands in the primary or inner shell of ligands
Ch23 coordination(a)
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10.short%20 coordinate%20compounds
1. Coordinate compounds are complexes where a central metal ion is coordinated to surrounding ligands. Coordination compounds can be ionic or molecular and the ligands are attached to the central ion via coordinate bonds.
2. The ligands directly attached to the central metal ion make up its coordination sphere. The total number of ligands is the coordination number. Bidentate and tridentate ligands that attach at multiple points contribute more than one to the coordination number.
3. Coordinate compounds can exhibit several types of isomerism including ionization isomerism from interchange of ligands and ions, coordination isomerism from interchange of complex ions, and geometrical isomerism from different spatial arrangements of ligands.
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- The theory can be used to explain the bonding preferences of ambidentate ligands like thiocyanate based on whether they bond to hard or soft metals through nitrogen or sulfur.
- The theory has applications in explaining reactivity patterns in inorganic reactions, organic reactions involving acids and bases of different hardness, and precipitation reactions.
Coordination chemistry/Descriptive Chemistry /Transition Metals
• Ligands
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atom/ion to form a complex
- Lewis base bonded (coordinated) to a metal ion in a coordination complex.
• Coordination Complex
– a central metal atom/ion and its set of ligands
– often an ion itself
• Coordination Compounds
– a neutral species made up in some part of a complex
– often the salt of a coordination complex
• Coordination Number
– the number of ligands in the primary or inner shell of ligands
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This document provides information about elements and compounds for a 7th grade science class. It defines an element as a pure substance made of only one type of atom that cannot be separated into simpler substances. An element can combine with other elements to form compounds. A compound is made of two or more elements chemically bonded together to form a new substance with unique properties. The document lists examples of elements like copper and carbon, and compounds like water and table salt. It describes physical and chemical properties of elements and characteristics of compounds.
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Coordination notes
Double salts are formed when two salts crystallize together in a stoichiometric ratio from their saturated solution. They dissociate into simple ions when dissolved in water. Coordination compounds retain their identity in both the solid and dissolved states. The metal acts as a Lewis acid and provides empty orbitals to accept electrons from ligands, which act as Lewis bases by donating electron pairs. Coordination compounds have defined geometries depending on the metal's hybridization and the ligand environment. Crystal field theory and valence bond theory are used to explain properties like color and magnetism.
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Hsab theory
The document discusses the hard and soft acid and base (HSAB) theory introduced by Pearson in 1963. It explains that hard acids prefer to coordinate with hard bases, and soft acids prefer soft bases, due to their relative polarizabilities. Hard acids and bases are less polarizable, while soft species are more polarizable and form stronger bonds through electron sharing. The HSAB concept is used to understand stability, reactions, and reaction mechanisms based on qualitative descriptions of predominant factors like polarizability.
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Coordination chemistry/Descriptive Chemistry /Transition Metals
Coordination chemistry/Descriptive Chemistry /Transition Metals
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This document provides information on coordination compounds and coordination chemistry concepts:
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Coordination compounds result from the combination of two or more stable molecular compounds. They retain their identity in solid and solution states and have properties different from their constituents. There is a central metal atom that provides vacant orbitals and ligands that donate electron pairs. Coordination compounds differ from double salts in that double salts exhibit characteristics of all constituent ions but coordination compounds do not. Terms related to coordination compounds include complex ion or entity, central atom or ion, and ligands. Ligands are electron donating species bound to the central metal and can be unidentate, bidentate, or polydentate.
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This document discusses coordination compounds and Werner's theory of coordination compounds. It provides details on:
- Coordination compounds are molecular compounds where a central metal atom is bound to surrounding ligands by dative bonds.
- Werner's theory successfully explained the structure and bonding in coordination compounds using the concept of primary and secondary valencies on the metal center.
- The theory was based on experimental evidence and helped explain the geometry and bonding in complexes, but had some limitations like not explaining color properties.
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This document discusses coordination compounds and Werner's theory of coordination compounds. It provides details on:
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- Some limitations of Werner's theory are that it does not explain factors influencing complex stability or the directional properties of bonds in complexes.
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The document provides an overview of coordination compounds, including their structure, bonding, naming conventions, and properties. Key points covered include:
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1. Coordination compounds are formed by the combination of metal ions and ligands, where the ligands are neutral molecules or negatively charged ions that are bound to the metal center.
2. Werner's coordination theory established that metal ions can satisfy both primary valency through ionic bonds and secondary valency through coordinate covalent bonds to ligands.
3. Key aspects of coordination compounds include the central metal ion, ligands, and the coordination number determined by the metal's secondary valency.
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Coordination complexes consist of a central metal ion bonded to surrounding ligand molecules or ions. Alfred Werner established the modern theory of coordination complexes in the late 19th century. According to Werner's theory, the metal ion exhibits both a primary valence based on its oxidation state and a secondary valence equal to its coordination number. Coordination complexes can be named systematically based on the ligands bonded to the metal ion and the metal's identity and oxidation state.
Bases
Bases are substances that can accept protons and release hydroxide ions in water. They have properties such as turning litmus paper blue, reacting with acids to form salts, and having a pH greater than 7 when dissolved in water. Common bases include alkali metal and alkaline earth metal hydroxides like NaOH and Ca(OH)2. Bases are classified based on their strength as strong, weak, or superbases. They can also be classified as organic or inorganic based on their source.
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Co ordination chemistry
This document provides information about coordination compounds and coordination chemistry. It defines key terms such as coordination compounds, coordination entities, central atoms/ions, ligands, and discusses the classification of ligands. It also covers topics like oxidation number, coordination number, coordination polyhedra, classification of complexes, and Werner's theory of coordination compounds. IUPAC nomenclature for naming coordination compounds is also presented.
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Coordination chemistry
- 3. Complex compounds are a special class of compounds in which the metal atoms or ions are bound to a number of anions or neutral molecules. In modern terminology these compounds are called Coordination compounds. Coordination compounds are a type of addition compounds.
- 5. Double Salts They exist only in solid state and dissociate into constituent species in their solution. They loose their identity in dissolved state. Coordination Compounds They retain their identity in solid as well as in solution state. They do not loose their identity in dissolved state.
- 6. Double Salts There properties are essentially the same as those of constituent species. In double salts the metal atom/ion exhibits normal valency. Eg:FeSO4(NH4)2SO4.6H2O Coordination Compounds There properties are different from those of constituent species. The number of negative ions or molecules surrounding the central metal atom is beyond its normal valency. Eg:K4[Fe(CN)6]
- 7. An aqueous solution of potash alum will give the tests for K+,Al3+and SO4 2-. K2SO4.Al2(SO4)3.24H2O→2K++ 2Al3+ + 4SO4 2- +24H2O When potassium ferroyanide is dissolved in water, it does not give the usual tests for Fe2+and CN1-
- 8. The molecule or ions which are coordinated to the metal atom or ion. Eg:K4[Fe(CN)6],the 6 cyanide group coordinated by Fe2+ and are the ligands. Ligands can be negative ions, positive ions or neutral molecules. Ligands are lewis base. Central metal atoms are lewis acid
- 9. One donor atom or one point of attachment and can coordinate with the metal ion at only one site in a complex. Eg:Cl -,NH3, H2O etc.
- 10. Two or more donor atom or points of attachments. Polydentate ligands are further classified as bi, tri, tetra etc.
- 18. A complex ion has a metal ion at its centre with a number of other molecules or ions surrounding it.