Chemistry Redefined

Understanding reaction mechanisms helps predict product formation and reaction rates.

• SN1 Mechanism: Two-step unimolecular substitution
• SN2 Mechanism: One-step bimolecular substitution
• E1 Mechanism: Elimination with carbocation intermediate

Chemical equilibrium occurs when a reversible reaction’s forward and reverse reactions happen at the same rate. At this point, the reaction continues in both directions, but the concentrations of reactants and products remain constant. This is why it is called a dynamic equilibrium. pH is a measure of the acidity or basicity of a solution, based on the concentration of hydrogen ions (H⁺): pH = − log ⁡ [ 𝐻 + ] pH=−log[H + ] A solution with pH 7 is neutral, pH less than 7 is acidic, and pH greater than 7 is basic. In acid–base reactions, the equilibrium between ions in the solution determines its pH.

Reaction kinetics is the branch of chemistry that deals with the study of the speed or rate of chemical reactions and the factors that influence them. It focuses on how quickly reactants are transformed into products and provides insight into the steps involved in a chemical reaction. The rate of a reaction depends on several factors, including concentration of reactants, temperature, pressure (for gases), surface area (for solids), and the presence of catalysts. By studying these factors, chemists can predict and control how reactions proceed over time. Kinetics also helps in understanding the reaction mechanism, which is the step-by-step sequence of events at the molecular level that leads from reactants to products. This knowledge is essential in fields like industrial chemistry, biochemistry, and environmental science, where controlling reaction rates is crucial for efficiency, safety, and yield.

Redox reactions are chemical reactions that involve the transfer of electrons between two species. In these reactions, one species loses electrons (oxidation) while another gains electrons (reduction). Because oxidation and reduction always occur together, they are collectively called redox (reduction–oxidation) reactions. Redox reactions are important in many processes, such as combustion, corrosion, respiration, and electrochemical cells. The concept of oxidation numbers is often used to identify which species is oxidized and which is reduced. These reactions play a key role in both industrial applications, like the extraction of metals, and biological processes, such as energy production in cells.