Chemical Element Sodium (Na)

Study Notes

NA (Sodium, Chemical Element)

Symbol: Na
Atomic Number: 11
Classification: Alkali metal
Position in the Periodic Table: Group 1, Period 3

Physical Properties

Appearance: Silvery-white metallic solid
Density: 0.97 g/cm³
Melting Point: 97.79 °C
Boiling Point: 883 °C

Chemical Properties

Reactivity: Highly reactive, especially with water; reacts to form sodium hydroxide and hydrogen gas.
Electropositivity: Strong electropositive nature; readily loses one electron to form cations (Na⁺).
Compounds: Forms various compounds such as sodium chloride (NaCl), sodium bicarbonate (NaHCO₃), and sodium sulfate (Na₂SO₄).

Occurrence

Natural Abundance: Commonly found in nature, primarily in the form of salts (e.g., halite).
Biological Role: Essential for living organisms; important in nerve function and maintaining fluid balance.

Uses

Industrial: Used in the production of glass, soaps, and paper.
Food Industry: Commonly used as table salt (sodium chloride) for seasoning and preservation.
Chemical Reactions: Acts as a reducing agent in chemical synthesis.

Safety

Hazards: Highly flammable; reacts violently with water and air.
Handling Precautions: Should be stored under oil or in an inert atmosphere to prevent reactions.

Isotopes

Stable Isotopes: Sodium has only one stable isotope, Na-23.
Radioactive Isotopes: Several radioactive isotopes exist but are not commonly encountered.

Key Facts

Sodium is crucial for various physiological functions including muscle contraction and nerve impulse transmission.
The sodium-potassium pump is vital for maintaining cellular homeostasis.

Sodium (Na) Overview

Symbol: Na, with an atomic number of 11.
Classified as an alkali metal, positioned in Group 1, Period 3 of the periodic table.

Physical Properties

Appears as a silvery-white metallic solid.
Density measured at 0.97 g/cm³, indicating it is lighter than water.
Melting point is 97.79 °C, while boiling point is 883 °C.

Chemical Properties

Sodium is highly reactive, particularly with water, producing sodium hydroxide and hydrogen gas.
Exhibits strong electropositive character by readily losing one electron to form sodium cations (Na⁺).
Forms various compounds, including sodium chloride (NaCl), sodium bicarbonate (NaHCO₃), and sodium sulfate (Na₂SO₄).

Occurrence

Naturally abundant, primarily found as salts such as halite.
Plays a crucial role in biological systems, essential for nerve function and fluid balance.

Uses

In industry, sodium is key in manufacturing glass, soaps, and paper products.
Widely utilized in the food industry as table salt (sodium chloride) for flavoring and preservation.
Acts as a reducing agent in various chemical reactions during synthesis.

Safety Precautions

Sodium is highly flammable and reacts vigorously with both water and air, posing hazards.
Must be stored under oil or in an inert atmosphere to mitigate risks of dangerous reactions.

Isotopes

Sodium has one stable isotope, Na-23.
While several radioactive isotopes exist, they are rarely encountered in typical scenarios.

Key Biological Functions

Essential for several physiological processes, including muscle contraction and nerve impulse transmission.
The sodium-potassium pump is critical for cellular homeostasis, regulating ion concentrations in cells.

Description

Explore the fascinating properties of sodium, also known as Na, including its physical and chemical traits, natural occurrence, and various uses. This quiz will test your knowledge on alkali metals and their significance in both industrial applications and biological functions.