Separate Chemistry 2

Alkali Metals

Alkali Metals

Group 1 elements in the periodic table characterized by high reactivity, low melting points, forming strong bases in water, and having various industrial applications.

Halogens

Group 7 elements known for high reactivity, forming salts with metals, decreasing reactivity down the group, and having diverse industrial and health applications.

Noble Gases

Group 0 elements with stable electron configurations, inertness, increasing boiling points down the group, and crucial applications in various industries.

Transition Metals

Elements in the d-block with variable oxidation states, high melting points, conductivity, catalytic roles, and essential biological functions.

Quantitative Chemistry

Involves measuring and calculating quantities in chemical reactions, focusing on the mole concept, chemical formulas, stoichiometry, and various calculations.

Chemical Analysis

Techniques for identifying and quantifying chemical composition, including qualitative and quantitative analysis, instrumental methods, and applications in different industries.

Organic Chemistry

Study of carbon-containing compounds, emphasizing structures, properties, reactions, and synthesis, with key concepts like structure and bonding, functional groups, and isomerism.

Energy Changes in Reactions

Understanding energy changes in reactions, including exothermic reactions releasing energy and endothermic reactions absorbing energy, crucial for industrial processes and life processes.

Enthalpy Change (ΔH)

A measure of the total energy change in a reaction, where negative ΔH indicates an exothermic reaction and positive ΔH indicates an endothermic reaction.

Activation Energy (Ea)

The minimum energy required for a reaction to proceed, influencing the reaction rate. Catalysts lower Ea, enhancing reaction rates without being consumed.

Electrolysis

A chemical process using electrical energy to induce non-spontaneous reactions, decomposing electrolytes into simpler substances.

Electrolyte

A substance producing ions in water or when melted, facilitating electrical conductivity and movement of ions in electrolysis.

Electrodes

Conductive materials in electrolytic cells aiding electron transfer during oxidation and reduction reactions, crucial for controlling reaction rates.

Oxidation and Reduction

Fundamental processes involving electron transfer, where oxidation leads to electron loss and reduction involves electron gain.

Electrolysis Cell

Setup for conducting electrolysis, comprising an electrolyte, electrodes, and an external power source to drive non-spontaneous reactions.

Equilibrium Constant (K)

Numerical expression relating reactant and product concentrations at equilibrium, indicating the extent of equilibrium for a reaction.

Le Chatelier's Principle

States that systems at equilibrium adjust to counteract external stresses, like changes in temperature, pressure, or concentration, to restore a new equilibrium position.

Acids, Bases, and Salts

Essential chemical compounds with distinct properties, where acids release H⁺ ions, bases accept H⁺ or release OH⁻ ions, and salts are formed in neutralization reactions.

Environmental Chemistry

Investigates chemical processes in the environment, focusing on pollution sources, chemical reactions, transport and fate of chemicals, ecological effects, and remediation and management strategies.

Exothermic Reactions

It release energy into the surroundings, typically in the form of heat, resulting in an increase in temperature. These reactions have a negative enthalpy change (ΔH), indicating that the energy of the products is lower than that of the reactants.

Endothermic Reactions

Absorb energy from their surroundings, usually as heat, resulting in a decrease in temperature. These reactions have a positive enthalpy change (ΔH), indicating that the energy of the products is higher than that of the reactants.

Dynamic Nature

This refers to a chemical equilibrium’s continuous change and adaptation over time, particularly in chemical contexts where reactions are ongoing. This leads to reactions where bonds are broken and formed, resulting in the transformation of reactants into products.