Undergraduate
  1. General chemistry  1.1. Introduction to Chemistry  1.2. Atomic Structure  1.2.1. Subatomic particles  1.2.2. Atomic Model  1.2.3. Quantum numbers  1.2.4. Electron Configuration  1.2.5. Periodic trends  1.2.6. Isotopes and their applications  1.3. Chemical bond  1.3.1. Ionic bond  1.3.2. Covalent bonds  1.3.3. Metal Bond  1.3.4. Hybridization  1.3.5. Molecular geometry and VSEPR theory  1.3.6. Bond polarity and dipole moment  1.4. Stoichiometry  1.4.1. Mole concept  1.4.2. Empirical and molecular formula  1.4.3. Limiting reactant and excess reactant  1.4.4. Percent Yield and Purity  1.4.5. Dilution calculation  1.5. States of matter  1.5.1. Gas Laws  1.5.2. Matter and Intermolecular Forces  1.5.3. Solid and Crystal Structures  1.5.4. Phase diagram  1.5.5. Plasma and supercritical fluid  1.6. Chemical reactions  1.6.1. Types of Chemical Reactions  1.6.2. Balancing Chemical Equations  1.6.3. Thermochemical reactions  1.6.4. Reaction energy profiles  1.7. Solutions and Mixtures  1.7.1. Concentration units  1.7.2. Syndrome properties  1.7.3. Solubility and Solubility Rules  1.7.4. Henry's Law and Raoult's Law  1.7.5. Partition coefficient  1.8. Chemical equilibrium  1.8.1. Law of mass action  1.8.2. Le Chatelier's principle  1.8.3. Reaction quotient  1.8.4. To use this online calculator for Equilibrium Constant, enter Equilibrium Constant (Eq.) and hit the calculate button. Here is how the Equilibrium Constant calculation can be explained with given input values -> 0.05 = 0.05/0.  1.8.5. Acid-base balance  1.9. Acids and bases  1.9.1. Arrhenius, Brønsted–Lowry, and Lewis definitions  1.9.2. pH and pOH  1.9.3. Acid-base titration  1.9.4. Buffer Solution  1.9.5. Acid-base indicator  1.9.6. Polyprotic Acids and Bases  1.10. Electrochemistry  1.10.1. redox reactions  1.10.2. Galvanic and Electrolytic Cells  1.10.3. Nernst equation  1.10.4. Electrolysis  1.10.5. Faraday's laws of electrolysis  1.11. Thermodynamics  1.11.1. Laws of Thermodynamics  1.11.2. Enthalpy, entropy and Gibbs free energy  1.11.3. Spontaneity of reactions  1.11.4. Thermodynamic cycles (Hess's law, Carnot cycle)  1.12. Kinetics  1.12.1. Rate law and reaction order  1.12.2. Activation Energy and Catalyst  1.12.3. Collision theory  1.12.4. Reaction mechanism  1.12.5. Transition state theory
  2. Organic chemistry  2.1. Structure and relationships  2.1.1. Hybridisation in Carbon Compounds  2.1.2. Resonance and aromatization  2.1.3. Molecular orbitals  2.1.4. Inductive and mesomeric effects  2.2. Hydrocarbons  2.2.1. Hydrocarbons  2.2.2. Alkene  2.2.3. Alkynes  2.2.4. Aromatic compounds  2.2.5. Cycloalkanes and Conformation  2.3. Functional Group  2.3.1. Alcohols and phenols  2.3.2. Ethers and epoxides  2.3.3. Aldehyde and ketone  2.3.4. Carboxylic acids and derivatives  2.3.5. Amin  2.3.6. Esters and amides  2.3.7. Thiols and sulfides  2.4. Stereoscopic  2.4.1. Isomerism in Stereochemistry  2.4.2. Chirality and optical activity  2.4.3. Structural analysis  2.4.4. Diastereomers and Enantiomers  2.5.1. Substitution reactions  2.5.2. Elimination reactions  2.5.3. Addition reactions  2.5.4. Radical reactions  2.5.5. Rearrangement reactions  2.5.6. Pericyclic Reactions  2.6. Spectroscopy and structural analysis  2.6.1. Infrared Spectroscopy  2.6.2. Nuclear magnetic resonance spectroscopy  2.6.3. Mass Spectrometry  2.6.4. UV-visible spectroscopy  2.6.5. X-ray crystallography  2.7. Polymer chemistry  2.7.1. Addition and Condensation Polymers  2.7.2. Polymerization mechanism  2.7.3. Biodegradable Polymer  2.7.4. Conducting and smart polymers
  3. Inorganic chemistry  3.1. Coordination chemistry  3.1.1. Ligands and coordination compounds  3.1.2. Crystal field theory  3.1.3. Molecular Orbital Theory in Coordination Compounds  3.1.4. Jahn–Taylor distortion  3.2. Main Group Chemistry  3.2.1. Alkali and alkaline earth metals  3.2.2. Halogens and Noble Gases  3.2.3. Transition metals and their complexes  3.2.4. Lanthanides and Actinides  3.3. Solid state chemistry  3.3.1. Crystal lattices and unit cells  3.3.2. Defects in solids  3.3.3. Electrical and magnetic properties  3.3.4. Superconductivity  3.4. Bio-inorganic chemistry  3.4.1. Metal ions in biology  3.4.2. Enzymatic reactions with metals  3.4.3. Metal poisoning and detoxification  3.4.4. Metalloproteins and Metalloenzymes
  4. Physical chemistry  4.1. Quantum Chemistry  4.1.1. Wave–particle duality  4.1.2. Schrödinger Equation  4.1.3. Quantum Numbers and Orbitals  4.1.4. Atomic and molecular spectroscopy  4.2. Statistical mechanics  4.2.1. Maxwell–Boltzmann distribution  4.2.2. Partitioning functions  4.2.3. Bose–Einstein and Fermi–Dirac statistics  4.3. Chemical thermodynamics  4.3.1. Gibbs Free Energy  4.3.2. Phase transition  4.3.3. Thermodynamic efficiency  4.4. Surface chemistry  4.4.1. Absorption and Catalysis  4.4.2. Colloids and Emulsions
  5. Analytical Chemistry  5.1. Classical methods  5.1.1. Gravimetric Analysis  5.1.2. titrimeter  5.2. Instrumental methods  5.2.1. Chromatography  5.2.2. Spectroscopy  5.2.3. Electroanalytical methods  5.2.4. X-ray diffraction
  6. Industrial Chemistry  6.1. Petrochemistry  6.2. Chemical engineering principles  6.3. Green Chemistry  6.4. Pharmaceuticals and Drug Synthesis
  7. Biochemistry  7.1. Carbohydrates  7.2. Proteins and enzymes  7.3. Lipids and membranes  7.4. Nucleic acids  7.5. Metabolism and Bioenergetics  7.6. Enzyme kinetics and mechanism

Undergraduate → Inorganic chemistry ↓


Bio-inorganic chemistry


Bioinorganic chemistry is a field that explores the role of metals and inorganic compounds in biological systems. It is an interdisciplinary field where biology and inorganic chemistry overlap, and it helps to understand many biological functions and phenomena. The field studies the interactions between inorganic substances and biological systems, examining how metals are used in nature and their functions within enzymes and proteins.

Fundamentals of bio-inorganic chemistry

At its core, bioinorganic chemistry addresses several important questions:

  • How do living organisms use inorganic elements?
  • What is the role of metals in enzymes?
  • How do metal ions stabilize biological structures?

The study mainly involves metalloproteins and metalloenzymes, where transition metals such as iron (Fe), copper (Cu), manganese (Mn), cobalt (Co), and zinc (Zn) are found. These metals play a vital role in various biological processes, including respiration, photosynthesis, and detoxification of harmful substances.

Important concepts in bio-inorganic chemistry

This area requires learners to understand several key concepts:

1. Function of metal ions in biological systems

Metals are essential to life, providing catalytic capabilities that organic molecules cannot accomplish efficiently on their own. These ions act as Lewis acids and are important in processes such as electron transfer, structural stabilization, and catalysis.

2. Coordination chemistry

Bioinorganic chemistry involves the study of how metal ions combine with ligands to form coordination complexes. Coordination compounds arise from the combination of metal ions with organic or inorganic ligands, and their geometry can have a significant impact on their biological activity and stability.

Metal ions Ligand Ligand Ligand Ligand

3. Metalloenzymes

Metalloenzymes are enzymes that contain one or more metal ions that are essential for their biological activity. These enzymes play a key role in many important biochemical processes:

  • Catalysis: Enzymes such as cytochrome c oxidase and nitrogenase require metal ions for catalytic functions.
  • Electron transfer: Iron-sulfur proteins and cytochromes are involved in the electron transport chain.
  • Structural role: Metal ions such as zinc stabilize protein structure in zinc fingers.

Applications of bio-inorganic chemistry

The principles of bioinorganic chemistry are applied in many areas:

Photography of biological systems

Bioinorganic compounds are used to visualize biological tissues. For example, metal-containing contrast agents in MRI scans help depict detailed organ structures.

Drug design and therapeutics

Bioinorganic chemistry is important in the development of pharmaceuticals:

  • Anti-cancer agents: Platinum-containing drugs, such as Cisplatin, are used in chemotherapy to destroy cancer cell DNA.
  • Antibacterial agents: Silver and bismuth compounds are used for their antimicrobial properties.

Understanding disease mechanisms

Deficiency or imbalance of metal ions can cause diseases, such as iron deficiency which can cause anemia. Bioinorganic chemistry helps in understanding these conditions at the molecular level.

Examples of bio-inorganic chemistry in nature

1. Photosynthesis

Plants have a magnesium ion (Mg) at the center of the chlorophyll molecule. This metal ion plays an important role in capturing light energy.

    Chlorophyll-a structure: porphyrin ring complexed with Mg
                  ,
         ,
        ,
          ,
            ,
            ,
           Milligrams

2. Hemoglobin and myoglobin

These important proteins use iron ions in the porphyrin structure to transport oxygen in the blood and muscles. The iron ion binds reversibly with oxygen, facilitating its transport and release.

    Structure of the heme group:
          ,
         , 
       ,
        , 
         ,
        Fe

3. Carbonic anhydrase

This enzyme, which catalyzes the conversion of carbon dioxide and water into bicarbonate and protons, depends on zinc ions (Zn) for its biological activity.

Conclusion

Bioinorganic chemistry is a fascinating and essential field that bridges the gap between inorganic chemistry and biology. It provides information about the roles of metals in life processes, advances medical science, and helps us understand the functionality of various biological systems. The study of bioinorganic chemistry continues to expand our knowledge of the natural world and offers exciting possibilities for future research and applications.


Undergraduate → 3.4


U
username
0%
completed in Undergraduate

← Prev (3.3.4)
Superconductivity
Next (3.4.1) →
Metal ions in biology

Comments 



Bio-inorganic chemistry

https://www.chemistryelite.com/ug/3.4?ceal=en