Calcium
Start with the big picture
Calcium has atomic number 20, an outer configuration of 4s², and a typical oxidation state of +2. It occurs in minerals including limestone, gypsum, and fluorite, and can be isolated by electrolysis of fused calcium chloride. Its reactions range from slow interaction with cold water to formation of calcium oxide in air. Important compounds include quicklime, calcium carbonate, and hygroscopic calcium chloride. The topic also covers water hardness associated with dissolved calcium ions and qualitative identification using a brick-red flame and a white calcium oxalate precipitate. In biology, calcium contributes to bone and tooth structure and is important in coagulation, muscle, and nerve function; its blood level is hormonally regulated. Industrial applications include metal treatment and alloy processing.
What you'll learn
- Describe calcium’s electronic configuration, physical properties, and common natural sources.
- Summarize calcium’s reactions with water, air, and nitrogen.
- Relate key calcium compounds to their preparation, properties, and uses.
- Identify calcium using its flame colour and oxalate precipitation test.
- Explain calcium’s biological functions, hormonal regulation, and health effects of imbalance.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
