Related Experiment Video
Updated: Jun 1, 2026
10:45
Stable Aqueous Suspensions of Manganese Ferrite Clusters with Tunable Nanoscale Dimension and Composition
Published on: February 5, 2022
Tris(ethyl-enediamine)manganese(II) sulfate
1School of Chemistry and Chemical Engineering, Liaocheng University, Liaocheng 252059, People's Republic of China.
Summary
This study details the crystal structure of a manganese(II) sulfate complex with ethylenediamine ligands. The compound exhibits a distorted octahedral geometry around the manganese ion and disordered sulfate anions, forming a 3D network via hydrogen bonds.
Area of Science:
- Inorganic Chemistry
- Crystallography
- Coordination Chemistry
Background:
- Manganese complexes with amine ligands are studied for their diverse structural and magnetic properties.
- Ethylenediamine is a common bidentate ligand in coordination chemistry.
- Sulfate anions can influence crystal packing and hydrogen bonding networks.
Purpose of the Study:
- To characterize the crystal structure of the title compound, [Mn(ethylenediamine)3]SO4.
- To investigate the coordination geometry around the manganese ion.
- To analyze the role of sulfate anions and hydrogen bonding in the crystal structure.
Main Methods:
- Single-crystal X-ray diffraction was used to determine the molecular and crystal structure.
- Analysis of bond lengths, bond angles, and intermolecular interactions (hydrogen bonds).
- Disorder analysis of the sulfate anion was performed.
Main Results:
- The manganese(II) ion is coordinated by six nitrogen atoms from three ethylenediamine ligands in a distorted octahedral geometry.
- The sulfate anion exhibits significant orientational disorder over four positions.
- A three-dimensional network is formed through N-H⋯O hydrogen bonds between the complex cations and sulfate anions.
Conclusions:
- The crystal structure reveals a [Mn(ethylenediamine)3]2+ complex cation and a sulfate anion.
- The observed coordination geometry and anion disorder provide insights into the packing forces within the crystal.
- Hydrogen bonding plays a crucial role in stabilizing the overall three-dimensional structure.
Related Concept Videos
01:22EDTA: Chemistry and Properties
Polydentate ligands are most widely used in complexometric titrations because they form more stable complexes with the metal ions than mono- or bidentate ligands due to the chelate effect. Examples of polydentate ligands are ethylenediaminetetraacetic acid (EDTA), crown ethers, and cryptands. The most important feature of optimal polydentate ligands is the ability to form 1:1 complexes in a single-step process. Amino carboxylic acid derivatives are frequently used as complexing agents. EDTA is...
01:26EDTA: Auxiliary Complexing Reagents
EDTA titrations are usually carried out in highly basic conditions, where the fully deprotonated form of EDTA, Y4−, actively complexes with the free metal ions in the solution. Several metal ions precipitate as hydrous oxide (hydroxides, oxides, or oxyhydroxides) under these conditions, lowering the concentration of free metal ions in the solution. For this reason, auxiliary complexing agents or ligands such as ammonia, tartrate, citrate, or triethanolamine are used in EDTA titrations to...
03:02Colors and Magnetism
Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.
02:42Valence Bond Theory
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
02:52Stereoisomerism
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula.
Transition metal complexes often exist as geometric isomers, in which the same atoms are connected through the same types of bonds but with differences in their orientation in space. Coordination complexes with two different ligands in the cis and trans positions from a ligand of interest form isomers. For example, the octahedral [Co(NH3)4Cl2]+ ion has two isomers (Figure 1) In the cis...
Isomers are different chemical species that have the same chemical formula.
Transition metal complexes often exist as geometric isomers, in which the same atoms are connected through the same types of bonds but with differences in their orientation in space. Coordination complexes with two different ligands in the cis and trans positions from a ligand of interest form isomers. For example, the octahedral [Co(NH3)4Cl2]+ ion has two isomers (Figure 1) In the cis...