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Chlorine Facts

Chlorine Chemical & Physical Properties

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This is a sample of pure chlorine gas. Chlorine gas is a pale greenish yellow color.

This is a sample of pure chlorine gas. Chlorine gas is a pale greenish yellow color.

Greenhorn1, public domain
This diagram shows the electron shell configuration of a chlorine atom.

This diagram shows the electron shell configuration of a chlorine atom.

Greg Robson, Creative Commons License
This is a sample of the element chlorine in its liquid form.

This is a sample of the element chlorine in its liquid form.

Mafi48, Wikipedia Public Domain
Periodic Table of the Elements

Chlorine

Atomic Number: 17

Symbol: Cl

Atomic Weight: 35.4527

Discovery: Carl Wilhelm Scheele 1774 (Sweden)

Electron Configuration: [Ne] 3s2 3p5

Word Origin: Greek: khloros: greenish-yellow

Properties: Chlorine has a melting point of -100.98°C, boiling point of -34.6°C, density of 3.214 g/l, specific gravity of 1.56 (-33.6°C), with a valence of 1, 3, 5, or 7. Chlorine is a member of the halogen group of elements and directly combines with almost all of the other elements. Chlorine gas is a greenish yellow. Chlorine figures prominently in many organic chemistry reactions, particularly in substitutions with hydrogen. The gas acts as an irritant for respiratory and other mucous membranes. The liquid form will burn the skin. Humans can smell as low an amount as 3.5 ppm. A few breaths at a concentration of 1000 ppm is usually fatal.

Uses: Chlorine is used in many everyday products. It is used for disinfecting drinking water. Chlorine is used in the production of textiles, paper products, dyes, petroleum products, medicines, insecticides, disinfectants, foods, solvents, plastics, paints, and many other products. The element is used to manufacture chlorates, carbon tetrachloride, chloroform, and in the extraction of bromine. Chlorine has been used as a chemical warfare agent.

Sources: In nature, chlorine is only found in the combined state, most commonly with sodium as NaCl and in carnallite (KMgCl3•6H2O) and sylvite (KCl). The element is obtained from chlorides by electrolysis or via the action of oxidizing agents.

Element Classification: Halogen

Density (g/cc): 1.56 (@ -33.6 °C)

Melting Point (K): 172.2

Boiling Point (K): 238.6

Appearance: greenish-yellow, irritating gas. At high pressure or low temperature: red to clear.

Isotopes: 16 known isotopes with atomic masses ranging from 31 to 46 amu. Cl-35 and Cl-37 are both stable isotopes with Cl-35 as the most abundant form (75.8%).

Atomic Volume (cc/mol): 18.7

Covalent Radius (pm): 99

Ionic Radius: 27 (+7e) 181 (-1e)

Specific Heat (@20°C J/g mol): 0.477 (Cl-Cl)

Fusion Heat (kJ/mol): 6.41 (Cl-Cl)

Evaporation Heat (kJ/mol): 20.41 (Cl-Cl)

Pauling Negativity Number: 3.16

First Ionizing Energy (kJ/mol): 1254.9

Oxidation States: 7, 5, 3, 1, -1

Lattice Structure: Orthorhombic

Lattice Constant (Å): 6.240

CAS Registry Number: 7782-50-5

Interesting Trivia:

  • Chlorine leaks in containers are detected using ammonia. Ammonia will react with the chlorine and form a white mist above the leak.
  • The most common natural chlorine compound on Earth is sodium chloride or table salt.
  • Chlorine is the 21st most abundant element in the Earth's crust
  • Chlorine is the third most abundant element in the Earth's oceans
  • Chlorine gas was used as a chemical weapon during World War I. Chlorine is heavier than air and would form a deadly layer in low-lying foxholes and trenches.
References: Los Alamos National Laboratory (2001), Crescent Chemical Company (2001), Lange's Handbook of Chemistry (1952), CRC Handbook of Chemistry & Physics (18th Ed.)

Quiz: Ready to test your chlorine facts knowledge? Take the Chlorine Facts Quiz.

Return to the Periodic Table

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