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


Inorganic chemistry is a branch of chemistry that deals with the properties and behavior of inorganic compounds. Unlike organic chemistry, which focuses on carbon-containing compounds, inorganic chemistry deals with compounds that are not primarily composed of carbon. The field involves many types of substances, including minerals, metals, and organometallic compounds. Inorganic chemistry is important to a variety of industries, including catalysts, materials science, pigments, surfactants, coatings, medicine, fuels, and agriculture. This narrative provides information about some of the key concepts, principles, and practical applications of inorganic chemistry.

Importance of inorganic chemistry

Inorganic chemistry is fundamental to understanding the chemical universe. Most of the elements in the periodic table are metals or nonmetals which fall under the field of inorganic chemistry. Here are several areas where inorganic chemistry plays an important role:

  • Catalysts: Catalysts are necessary to speed up chemical reactions. Many industrial processes rely on catalysts made from inorganic compounds, such as the Haber process for ammonia synthesis.
  • Materials science: Inorganic compounds are used to develop materials such as ceramics, superconductors, and semiconductors, which have important technological applications.
  • Medicine: Many inorganic compounds are used in healthcare, including as diagnostic agents and medications. For example, platinum-based compounds are used in the treatment of cancer.
  • Environmental chemistry: Inorganic chemists study the effects of metals and other inorganic compounds on the environment, developing methods for pollution control and waste management.

Structure of the atom and the periodic table

Understanding inorganic chemistry begins with understanding the structure of an atom and the organization of the elements in the periodic table. Each atom has a nucleus made up of protons and neutrons, surrounded by electrons in orbitals. The number of protons in the nucleus defines the element, while the arrangement of the electrons determines the chemical properties.

The periodic table is a chart that arranges the elements based on increasing atomic number and recurring chemical properties. The elements are classified into groups and periods. Groups are vertical columns that contain elements with similar chemical behavior due to having the same number of electrons in their outer shell. For example, group 1 contains the alkali metals such as Li, Na, and K, which are highly reactive, especially with water.

Periods are horizontal rows in the periodic table. As you move from left to right across a period, the atomic number increases, which typically decreases the atomic radius and increases the ionization energy and electronegativities. This knowledge is fundamental in predicting how different elements react and combine during chemical reactions.

Coordination chemistry

Coordination compounds are one of the most interesting topics in inorganic chemistry. These compounds contain a central metal atom or ion that is bound to surrounding molecules or ions, known as ligands. The number and type of ligands, as well as their spatial arrangement around the central metal ion, significantly affect the properties of the coordination compound.

Example: A common example of a coordination compound is [Cu(NH 3) 4]SO 4, better known as tetraamminecopper(II) sulfate. In this compound, the copper ion is surrounded by four ammonia molecules that act as ligands.

Coordination number and geometry

The coordination number is the number of ligand atoms bonded to the central metal ion. Common coordination numbers are 4 and 6, which lead to geometries such as tetrahedral, square planar, and octahedral. For example, [Ni(CN) 4] has a square planar geometry, while [Fe(CN) 6] 4- has an octahedral arrangement.

Crystal field theory (CFT)

Crystal field theory is a model that describes the electronic structure of transition metal complexes. It assumes that ligands act as point charges, which generate a crystal field affecting the d orbital energy of the central metal ion. This splitting of the d orbitals results in different electronic configurations and affects properties such as colour, magnetic behaviour and reactivity.

For example, in an octahedral field, the five d orbitals split into a higher energy set (e.g. g, which includes the d z² and d x²-y² orbitals) and a lower energy set (t 2g, which includes the d xy, d yz, and d xz orbitals). This splitting is represented as Δ, which is the crystal field splitting energy.

Acids, bases and salts

Inorganic chemistry involves the in-depth study of acids, bases, and salts, which are fundamental substances with a wide range of applications. Acids are compounds that donate protons (H +) in solution, while bases accept protons. For example, hydrochloric acid (HCl) is a strong acid that dissociates completely in water, releasing H + and Cl- ions.

Bases include substances such as sodium hydroxide (NaOH), which dissociates to form hydroxide ions (OH -) in solution. The reaction between an acid and a base usually results in the formation of water and a salt, as shown in the reaction:

    HCl + NaOH → NaCl + H 2 O

Oxidation and reduction

Oxidation and reduction (redox) reactions are processes in which electrons are transferred between substances. In these reactions, one species gains electrons (reduction), while the other loses electrons (oxidation). These processes are important in energy production, especially in electrochemical cells and batteries. For example, consider the redox reaction between zinc and copper sulfate:

    4Zn + CuSO4 → ZnSO4 + Cu

Here, zinc is oxidized to Zn 2+ while copper (II) ions are reduced to metallic copper. The transferred electrons facilitate this reaction.

This HTML file provides a structural basis for learning and understanding the diverse and complex field of inorganic chemistry. Although it could be extended with discussions of topics such as main group chemistry, f-block elements, and industrial inorganic chemistry, the foundation laid here provides a solid starting point for a deeper exploration of inorganic compounds and their properties.

Conclusion

Inorganic chemistry is a vast and fascinating field of study, essential to understanding a wide range of substances and their behavior. From the fundamental structure of atoms and the organization of the periodic table to the intricacies of complex coordination compounds and crystal field theory, the topics covered are integral to understanding how chemistry drives both natural phenomena and technological advancements. A thorough understanding of inorganic chemistry opens the door to numerous applications, playing a vital role in science and industry. By learning inorganic chemistry, one gains knowledge not only of chemical reactions and compounds but also of the materials that constitute our world.


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Inorganic chemistry

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