Chemical Compounds

Chemical compounds are the building blocks of all matter, formed when atoms of two or more elements link up. A familiar example is water (H₂O), where two hydrogen (H) atoms join with one oxygen (O) atom, creating a stable molecule. From the air we breathe to the diverse materials that make up the world around us, chemical compounds are integral, each with a unique formula that tells the story of its atoms’ type and proportions—like methane’s simple yet distinct CH₄ arrangement. Understanding these compounds unlocks the mysteries of chemistry and the elemental dance that constructs our universe.

What is a Chemical Compound?

Types Of Chemical Compounds

1. Ionic Compounds:
   • Formed by the electrostatic attraction between oppositely charged ions.
   • Usually consist of metal and nonmetal ions.
   • Example: Sodium chloride (NaCl), where sodium (Na) donates an electron to chlorine (Cl), creating charged ions that attract each other.
2. Covalent Compounds:
   • Created by the sharing of electrons between nonmetal atoms.
   • The shared electrons allow each atom to attain the electron configuration of a noble gas, thereby stabilizing the molecule.
   • Example: Water (H₂O), with oxygen sharing electrons with hydrogen atoms.
3. Molecular Compounds:
   • A type of covalent compound that exists as discrete molecules.
   • Often formed between two nonmetal elements.
   • Example: Carbon dioxide (CO₂), a gas comprised of molecules with one carbon atom double bonded to two oxygen atoms.
4. Acidic Compounds:
   • Compounds that donate protons (H⁺ ions) when dissolved in water.
   • Typically start with hydrogen, and they increase the concentration of H⁺ ions in a solution.
   • Example: Hydrochloric acid (HCl), which dissociates in water to release H⁺ ions and Cl⁻ ions.
5. Basic Compounds:
   • Also known as alkalis, these compounds accept protons or donate hydroxide ions (OH⁻) in solution.
   • Usually metal oxides, hydroxides, or sometimes carbonates.
   • Example: Sodium hydroxide (NaOH), often used in soaps and detergents.
6. Complex Compounds or Coordination Compounds:
   • Consist of a central metal atom or ion, surrounded by molecules or anions, called ligands.
   • These ligands are typically bonded to the central atom by coordinate covalent bonds.
   • Example: [Fe(CN)₆]³⁻, a complex ion where six cyanide ions are coordinated to an iron ion.
7. Organic Compounds:
   • Contain carbon atoms bonded to hydrogen and typically other elements like oxygen, nitrogen, sulfur, and phosphorus.
   • The carbon atoms form a carbon skeleton or backbone.
   • Example: Methane (CH₄), the simplest organic compound and a natural gas.
8. Inorganic Compounds:
   • Compounds that do not contain carbon-hydrogen bonds.
   • Include metals, salts, minerals, and substances made from single elements.
   • Example: Ammonia (NH₃), a compound made of nitrogen and hydrogen.

List of Chemical Compounds

Properties of Compounds

Compounds exhibit distinct properties that arise from the combination of their constituent elements and the type of chemical bonds that hold them together. Some of these properties include:

1. Fixed Composition: Each compound has a specific ratio of elements, defined by its chemical formula.
2. Chemical Structure: Compounds have a unique spatial arrangement of atoms which determines many of their physical and chemical properties.
3. Distinctive Properties: The properties of compounds, such as melting point, boiling point, and density, are different from the properties of the individual elements that comprise them.
4. Chemical Reactivity: Compounds can undergo chemical changes through reactions, resulting in the formation of new compounds.
5. Electrical Conductivity: Ionic compounds typically conduct electricity when dissolved in water or melted, while covalent compounds generally do not.
6. Solubility: The solubility of compounds in various solvents can vary widely, with ionic compounds often being soluble in water, while organic compounds are more likely to dissolve in organic solvents.
7. Energy Content: Compounds have a certain amount of energy associated with the formation and breaking of bonds, which can be released or absorbed during chemical reactions.
8. Color: Many compounds have characteristic colors, which are used in identifying substances and are due to the wavelengths of light absorbed by the electrons of the atoms.