Emilee Abbott


Since it combines directly with nearly every element, chlorine is never found free in nature. Chlorine was first produced by Carl Wilhelm Scheele, a Swedish chemist.
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Properties and Uses

Chlorine kills bacteria, it's a disinfectant. It is used to treat drinking water and swimming pool water. Another major use for chlorine is in organic chemistry. It is used as an oxidizing agent and in substitution reactions. n the past chlorine was commonly used to make chloroform. However, both of these chemical is now strictly controlled as it can cause liver damage.

Periodic table

The atomic number of Chlorine is 17 and the mass is 35.425. There are 17 protons, 18 neutrons and 17 electrons.

Chlorine - 37

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Halogens are in group 17 of the periodic table and they are highly electronegative and reactive. As you go down the group, the atom size increases. They have a very "effective nuclear charger." Halogens can be harmful and lethal.

At room temperature it appears as a light green gas. Since the bond that forms between the two chlorine atoms is weak, the Cl2 molecule is very reactive. Chlorine reacts with metals to produce salts called chlorides. Chloride ions are the most abundant ions that dissolve in the ocean. Chlorine also has two isotopes: 35Cl and 37Cl.

Reaction Type

Iron and Chlorine

This is an ionic compound with single replacement.

2Fe(s) + 3Cl2(g) ------------> 2FeCl3(s)

You have one mole Cl2 reacting with one mole of Fe.
n Cl2 reacting = ( 0.100 mole Fe ) ( 1.0 mole Cl2 / 1.0 mole Fe )
n Cl2 reacting = 0.100 mole


Two of the most familiar chlorine compounds are sodium chloride(NaCl) and hydrogen chloride (HCl). Another one commonly known is Chloroform (CHCl3).

Ionic bond

% of Na is 39.34

% of Cl is 60.66