Chemical Reactions Overview

A mineral composed of calcium sulfate dihydrate (CaSO₄·2H₂O), used in construction.

A white powder made by heating gypsum (CaSO₄·2H₂O) to remove some water, forming calcium sulfate hemihydrate (CaSO₄·½H₂O). It is used for plastering and sculptures.

A solution of calcium hydroxide (Ca(OH)₂) turns milky white when exposed to carbon dioxide (CO₂), forming a precipitate of calcium carbonate (CaCO₃).

A soft, silvery-white metal, highly reactive and not found free in nature. It's a strong reducing agent and used in mining, producing sodium cyanide, and organic reactions.

Sodium is highly reactive and ignites when exposed to air. It's stored in non-reactive liquids like benzene and kerosene to prevent air contact.

Sodium is used in mining to remove oxygen combined with metals or dissolved in their melts.

When a sodium-containing compound is heated in a flame, the flame turns bright yellow (golden) due to the excitation of sodium ions.

NaCl is a common compound found in salt deposits, seawater, and lakes. Extraction methods include mining and solar evaporation.

Does not absorb moisture from air (non-hygroscopic).

Absorbs moisture from air (hygroscopic) due to impurities like calcium chloride or magnesium chloride.

Used in food preservation, leather tanning, ice production, dye fixation, and preparing other chemicals.

Group 1 elements (Li, Na, K, Rb, Cs, Fr) are called alkali metals because their aqueous solutions are alkaline.

Group 2 elements (Be, Mg, Ca, Sr, Ba, Ra) are called alkaline earth metals.

Highly reactive, one electron in the outermost shell, low electronegativity and ionization energy.

Less reactive than alkali metals, two electrons in the outermost shell, higher ionization energy.

A lithium-containing compound produces a crimson flame when heated.

A sodium-containing compound produces a bright yellow (golden) flame when heated.

A calcium-containing compound produces a brick red flame when heated.

A strontium-containing compound produces a crimson flame when heated.

A barium-containing compound produces a yellowish-green flame when heated.

They readily lose valence electrons, making them good reducing agents.

Sodium has 11 electrons arranged in three energy levels: 2 in the first, 8 in the second, and 1 in the third.

Sodium reacts with oxygen in the air, forming a white coating on its surface, losing its metallic sheen.

Sodium reacts directly with chlorine gas, igniting to form sodium chloride (NaCl).

Sodium reacts vigorously with water, generating sodium hydroxide (NaOH) and hydrogen gas.

A strong base that absorbs moisture from air, reacts with CO₂ to form sodium carbonate (Na₂CO₃), and is used in various industries.

A reactive element, not found free in nature, found in minerals like limestone, gypsum, and phosphate.

Include calcium sulfate (CaSO₄), used for plaster, and calcium hydroxide (Ca(OH)₂), used for detecting CO₂.

The process of adding water to calcium oxide (CaO) to form calcium hydroxide (Ca(OH)₂) and limewater.