Inorganic Compound
Table of Contents
Inorganic compounds are chemical substances that usually do not contain carbon-hydrogen (C–H) bonds. Inorganic compounds are mostly present in non-living systems, such as minerals, metals, and the Earth’s crust. These compounds are composed of various elements, including metals, nonmetals, and halogens, and often involve oxygen, nitrogen, sulfur, or phosphorus. [1-4]
A defining feature of inorganic compounds is their chemical diversity. They can form ionic, covalent, or metallic bonds, depending on the elements involved. Common examples include water (H2O), sodium chloride (NaCl), and carbon dioxide (CO2).
Properties [1-4]
- High melting and boiling points: Ionic inorganic compounds have high melting and boiling points due to strong electrostatic forces.
- Water solubility: Many inorganic salts and acids dissolve well in water, enabling chemical reactions.
- Electrical conductivity: In their molten or aqueous forms, many substances can conduct electricity due to the presence of free-moving ions.
- Crystalline structure: Many form solid crystals with a regular geometric pattern, such as NaCl.
- Colorful appearance: Transition metal compounds often have vivid colors (e.g., blue copper sulfate, purple potassium permanganate).
Types [1-4]
1. Acids
Acids are substances that release hydrogen ions (H⁺) when dissolved in water. According to the Arrhenius definition, acids increase H⁺ concentration in aqueous solutions. The Brønsted-Lowry theory defines acids as proton donors.
List of Common Acids:
| Name | Formula | Uses |
|---|---|---|
| Hydrochloric acid | HCl | Cleaning agents, digestion (stomach acid), metal processing |
| Sulfuric acid | H2SO4 | Fertilizer production, car batteries, industrial processes |
| Nitric acid | HNO3 | Explosives, fertilizers, dye manufacturing |
| Acetic acid (vinegar) | CH3COOH | Food preservation, cleaning, plastics production |
| Phosphoric acid | H3PO4 | Soft drinks, fertilizers, dental products |
2. Bases
Bases are substances that release hydroxide ions (OH⁻) in water (Arrhenius) or act as proton acceptors (Brønsted-Lowry). They are often slippery and bitter-tasting.
List of Common Bases:
| Name | Formula | Uses |
|---|---|---|
| Sodium hydroxide | NaOH | Soap making, drain cleaners, paper and textile industries |
| Calcium hydroxide | Ca(OH)2 | Whitewash, water treatment, neutralizing acidic soils |
| Potassium hydroxide | KOH | Battery electrolytes, making soft soaps, biodiesel production |
| Magnesium hydroxide | Mg(OH)2 | Antacids, laxatives, flame retardants |
| Aluminum hydroxide | Al(OH)3 | Water purification, antacids, fire retardant coatings |
3. Salts
Salts, along with water, are formed when an acid reacts with a base in a neutralization reaction. A salt consists of a cation (from the base) and an anion (from the acid). Salts can be neutral, acidic, or basic, depending on the strength of the reacting acid and base.
List of Common Salts:
| Name | Formula | Uses |
|---|---|---|
| Sodium chloride | NaCl | Table salt, food preservation, de-icing roads |
| Potassium nitrate | KNO3 | Fertilizers, fireworks, gunpowder |
| Copper(II) sulfate | CuSO4 | Fungicide, algicide, electroplating |
| Calcium carbonate | CaCO3 | Antacids, cement and lime production, chalk |
| Sodium bicarbonate | NaHCO3 | Baking soda, antacid, cleaning agent |
4. Oxides
Oxides are compounds formed when oxygen bonds with another element. They are categorized based on their chemical behavior.
- Acidic oxides are formed by nonmetals and react with water to produce acids.
- Basic oxides are formed by metals and react with water to form bases.
- Amphoteric oxides show both acidic and basic behavior.
- Neutral oxides do not react as acids or bases.
List of Common Oxides:
| Name | Formula | Type | Uses |
|---|---|---|---|
| Carbon dioxide | CO2 | Acidic oxide | Carbonated drinks, fire extinguishers, photosynthesis |
| Calcium oxide (quicklime) | CaO | Basic oxide | Cement, steelmaking, soil treatment |
| Zinc oxide | ZnO | Amphoteric oxide | Sunscreens, rubber industry, paint additives |
| Nitrous oxide | N2O | Neutral oxide | Anesthetic, whipped cream propellant |
Organic vs. Inorganic Compounds [1-4]
| Feature | Organic Compounds | Inorganic Compounds |
|---|---|---|
| Main Elements | Mostly carbon and hydrogen | Metals, nonmetals, wide range of elements |
| Source | Living organisms (e.g., human being, animals) | Non-living sources (e.g., minerals, atmosphere) |
| Bond Type | Mostly covalent bonds | Ionic, covalent, or metallic bonds |
| Structure | Complex chains or rings | Simple or crystalline solids |
| Melting/Boiling Point | Generally lower | Usually higher |
| Solubility | Often in organic solvents | Often in water |
| Conductivity | Usually poor | Often conductive in solution/molten form |
| Examples | Methane (CH4), Glucose (C6H12O6), Ethanol (C2H5OH) | Water (H2O), Sodium chloride (NaCl), Sulfuric acid (H2SO4) |
In conclusion, inorganic compounds are chemical substances that do not contain carbon-hydrogen bonds and are primarily found in non-living systems like rocks, water, and minerals. They include a wide range of substances such as acids, bases, salts, and oxides, each with essential applications in nature, industry, and everyday life. Their versatility and unique properties make them a vital part of the chemical world.
