In coordination compounds, a coordination entity refers to the central metal atom or ion bonded to a fixed number of ions or molecules, known as ligands. Examples include [CoCl₃(NH₃)₃]²⁺ or [Fe(CN)₆]³⁻. The central atom/ion in a coordination entity, to which ligands are attached, is termed the centrRead more
In coordination compounds, a coordination entity refers to the central metal atom or ion bonded to a fixed number of ions or molecules, known as ligands. Examples include [CoCl₃(NH₃)₃]²⁺ or [Fe(CN)₆]³⁻. The central atom/ion in a coordination entity, to which ligands are attached, is termed the central atom or ion. Counter ions, on the other hand, are charged ions or groups outside the square brackets that balance the charge of the coordination entity. For instance, in [Cu(NH₃)₄]²⁺, Cu(NH₃)₄ is the coordination entity, and the counter ion is the 2⁻ charge. Both components collectively constitute the coordination compound.
According to Alfred Werner, octahedral, tetrahedral, and square planar geometrical shapes are more common in coordination compounds of transition metals. In octahedral complexes like [Co(NH₃)₆]³⁺, six ligands surround the central metal. Tetrahedral complexes, as seen in [Ni(CO)₄], involve four liganRead more
According to Alfred Werner, octahedral, tetrahedral, and square planar geometrical shapes are more common in coordination compounds of transition metals. In octahedral complexes like [Co(NH₃)₆]³⁺, six ligands surround the central metal. Tetrahedral complexes, as seen in [Ni(CO)₄], involve four ligands. Square planar complexes, exemplified by [PtCl₄]²⁻, exhibit a planar arrangement of four ligands. These shapes arise from the coordination number, representing the number of ligands directly attached to the central metal. Werner’s contributions revolutionized the understanding of these spatial arrangements, providing a foundation for modern coordination chemistry.
Double salts and complexes differ in their behavior when dissolved in water. Double salts, such as KCl⋅MgCl₂⋅6H₂O or FeSO₄⋅(NH₄)₂SO₄⋅6H₂O, dissociate into simple ions completely, releasing individual ions upon dissolution. In contrast, complexes, like [Fe(CN)₆]⁴⁻ in K₄[Fe(CN)₆], do not dissociate inRead more
Double salts and complexes differ in their behavior when dissolved in water. Double salts, such as KCl⋅MgCl₂⋅6H₂O or FeSO₄⋅(NH₄)₂SO₄⋅6H₂O, dissociate into simple ions completely, releasing individual ions upon dissolution. In contrast, complexes, like [Fe(CN)₆]⁴⁻ in K₄[Fe(CN)₆], do not dissociate into Fe²⁺ and CN⁻ ions upon dissolution. The complex remains intact in the solution, maintaining its structural integrity. This distinction arises from the nature of bonding; double salts consist of separate ions, while complexes involve coordination compounds with ligands tightly bound to a central metal ion.
The coordination compound [Cr(NH₃)₃(H₂O)₃]Cl₃ is named as triamminetriaquachromium(III) chloride. In the name, "triammine" denotes three ammonia ligands, "triaqua" refers to three water ligands, and "chromium(III)" indicates the chromium ion in the +3 oxidation state. The oxidation number of chromiuRead more
The coordination compound [Cr(NH₃)₃(H₂O)₃]Cl₃ is named as triamminetriaquachromium(III) chloride. In the name, “triammine” denotes three ammonia ligands, “triaqua” refers to three water ligands, and “chromium(III)” indicates the chromium ion in the +3 oxidation state. The oxidation number of chromium is determined by considering the charge on the complex and the ligands. Since chloride (Cl⁻) has a charge of -1 and there are three chlorides, the overall charge is -3. Chromium must have a +3 oxidation state to balance the charge, indicating the oxidation number of the central metal in the complex.
The coordination compound [Co(H₂NCH₂CH₂NH₂)₃]₂(SO₄)₃ is named as tris(ethane-1,2-diamine)cobalt(III) sulfate. In the name, "tris" denotes three ethane-1,2-diamine ligands, "cobalt(III)" indicates the oxidation state of cobalt, and "sulfate" represents the counter anion. The oxidation state of cobaltRead more
The coordination compound [Co(H₂NCH₂CH₂NH₂)₃]₂(SO₄)₃ is named as tris(ethane-1,2-diamine)cobalt(III) sulfate. In the name, “tris” denotes three ethane-1,2-diamine ligands, “cobalt(III)” indicates the oxidation state of cobalt, and “sulfate” represents the counter anion. The oxidation state of cobalt is determined by considering the overall charge on the complex. Since there are three sulfate ions (SO₄²⁻) with a total charge of -6, each cobalt must have a +3 oxidation state to balance the charge, indicating the oxidation number of the central metal in the complex.
Define coordination entities and counter ions in the context of coordination compounds.
In coordination compounds, a coordination entity refers to the central metal atom or ion bonded to a fixed number of ions or molecules, known as ligands. Examples include [CoCl₃(NH₃)₃]²⁺ or [Fe(CN)₆]³⁻. The central atom/ion in a coordination entity, to which ligands are attached, is termed the centrRead more
In coordination compounds, a coordination entity refers to the central metal atom or ion bonded to a fixed number of ions or molecules, known as ligands. Examples include [CoCl₃(NH₃)₃]²⁺ or [Fe(CN)₆]³⁻. The central atom/ion in a coordination entity, to which ligands are attached, is termed the central atom or ion. Counter ions, on the other hand, are charged ions or groups outside the square brackets that balance the charge of the coordination entity. For instance, in [Cu(NH₃)₄]²⁺, Cu(NH₃)₄ is the coordination entity, and the counter ion is the 2⁻ charge. Both components collectively constitute the coordination compound.
See lessAccording to Alfred Werner, what geometrical shapes are more common in coordination compounds of transition metals, and provide examples.
According to Alfred Werner, octahedral, tetrahedral, and square planar geometrical shapes are more common in coordination compounds of transition metals. In octahedral complexes like [Co(NH₃)₆]³⁺, six ligands surround the central metal. Tetrahedral complexes, as seen in [Ni(CO)₄], involve four liganRead more
According to Alfred Werner, octahedral, tetrahedral, and square planar geometrical shapes are more common in coordination compounds of transition metals. In octahedral complexes like [Co(NH₃)₆]³⁺, six ligands surround the central metal. Tetrahedral complexes, as seen in [Ni(CO)₄], involve four ligands. Square planar complexes, exemplified by [PtCl₄]²⁻, exhibit a planar arrangement of four ligands. These shapes arise from the coordination number, representing the number of ligands directly attached to the central metal. Werner’s contributions revolutionized the understanding of these spatial arrangements, providing a foundation for modern coordination chemistry.
See lessHow do double salts and complexes differ in their behavior when dissolved in water?
Double salts and complexes differ in their behavior when dissolved in water. Double salts, such as KCl⋅MgCl₂⋅6H₂O or FeSO₄⋅(NH₄)₂SO₄⋅6H₂O, dissociate into simple ions completely, releasing individual ions upon dissolution. In contrast, complexes, like [Fe(CN)₆]⁴⁻ in K₄[Fe(CN)₆], do not dissociate inRead more
Double salts and complexes differ in their behavior when dissolved in water. Double salts, such as KCl⋅MgCl₂⋅6H₂O or FeSO₄⋅(NH₄)₂SO₄⋅6H₂O, dissociate into simple ions completely, releasing individual ions upon dissolution. In contrast, complexes, like [Fe(CN)₆]⁴⁻ in K₄[Fe(CN)₆], do not dissociate into Fe²⁺ and CN⁻ ions upon dissolution. The complex remains intact in the solution, maintaining its structural integrity. This distinction arises from the nature of bonding; double salts consist of separate ions, while complexes involve coordination compounds with ligands tightly bound to a central metal ion.
See lessHow is the coordination compound [Cr(NH₃)₃(H₂O)₃]Cl₃ named, and how is the oxidation number of chromium determined?
The coordination compound [Cr(NH₃)₃(H₂O)₃]Cl₃ is named as triamminetriaquachromium(III) chloride. In the name, "triammine" denotes three ammonia ligands, "triaqua" refers to three water ligands, and "chromium(III)" indicates the chromium ion in the +3 oxidation state. The oxidation number of chromiuRead more
The coordination compound [Cr(NH₃)₃(H₂O)₃]Cl₃ is named as triamminetriaquachromium(III) chloride. In the name, “triammine” denotes three ammonia ligands, “triaqua” refers to three water ligands, and “chromium(III)” indicates the chromium ion in the +3 oxidation state. The oxidation number of chromium is determined by considering the charge on the complex and the ligands. Since chloride (Cl⁻) has a charge of -1 and there are three chlorides, the overall charge is -3. Chromium must have a +3 oxidation state to balance the charge, indicating the oxidation number of the central metal in the complex.
See lessProvide the name for the coordination compound [Co(H₂NCH₂CH₂NH₂)₃]₂(SO₄)₃ and explain how the oxidation state of cobalt is determined.
The coordination compound [Co(H₂NCH₂CH₂NH₂)₃]₂(SO₄)₃ is named as tris(ethane-1,2-diamine)cobalt(III) sulfate. In the name, "tris" denotes three ethane-1,2-diamine ligands, "cobalt(III)" indicates the oxidation state of cobalt, and "sulfate" represents the counter anion. The oxidation state of cobaltRead more
The coordination compound [Co(H₂NCH₂CH₂NH₂)₃]₂(SO₄)₃ is named as tris(ethane-1,2-diamine)cobalt(III) sulfate. In the name, “tris” denotes three ethane-1,2-diamine ligands, “cobalt(III)” indicates the oxidation state of cobalt, and “sulfate” represents the counter anion. The oxidation state of cobalt is determined by considering the overall charge on the complex. Since there are three sulfate ions (SO₄²⁻) with a total charge of -6, each cobalt must have a +3 oxidation state to balance the charge, indicating the oxidation number of the central metal in the complex.
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