What Is Calcium?
Calcium, an alkaline earth metal with the atomic number 20, was first isolated by Humphry Davy in the early 1800s through electrolysis. This highly reactive element is crucial for both plant growth and human health, comprising 1-2% of the human body’s weight, predominantly in bones and teeth as calcium phosphate.
Uses of Calcium
Various calcium salts have broad applications, from deicing roads with calcium chloride to using calcium carbonate in chalk and animal feed. Calcium oxide acts as a desiccant and soil conditioner, while calcium hydroxide is used in food processing and as a soil neutralizer.
Properties of Calcium
With a melting point of 842 °C (1547.6 °F) and boiling point of 1484 °C (2703.2 °F), calcium’s reactivity with water, oxygen, and carbon dioxide necessitates storage under inert gas or in mineral oil to prevent oxidation.
Structure of Calcium
Symbolized as Ca, calcium’s atomic weight is 40.08, exhibiting a cubic close-packed structure at room temperature. It has four stable isotopes (40Ca, 42Ca, 43Ca, 44Ca), and natural radioactive isotopes like 46Ca and 48Ca.
Other Information on Calcium
1. Reactions of Calcium
Calcium reacts vigorously with air and water, producing hydrogen gas and calcium hydroxide, respectively. It forms calcium carbonate when reacted with carbon dioxide, a reversible process useful in various industrial applications.
2. Calcium in Nature
Found in limestone and marble, calcium plays a significant role in carbon sequestration and is essential for the cellular functions of eukaryotic organisms and plant nutrition. However, excessive calcium intake has been linked with health risks, including an increased likelihood of dementia.