Group chlorides
The table below gives the physical state and the acid-base properties of chlorides containing Group elements in either the +2 or the +4 oxidation state.
Note that E2+ cations are only important for elements at the bottom of the group. The nonmetallic and metalloid elements do NOT exist as cations in aqueous solution.
The E(IV) chlorides are all molecular substances with covalent bonds between the Group element and chlorine. Because the attractive forces between molecular substances are weaker than between ions, these compounds are all liquids.
The chlorides of the heavier elements are all reactive compounds that fume in the presence of water. They cannot be recovered from their aqueous solution due to the reaction below. The solution produced in strongly acidic due to four moles of HCl having been produced for each mole of the tetrachloride consumed.
Note that E2+ cations are only important for elements at the bottom of the group. The nonmetallic and metalloid elements do NOT exist as cations in aqueous solution.
| nonmetal | |
| oxides | C |
| ECl4 | inert liquid |
| ECl2 | none |
| E2+(aq) | none |
| metalloids | |
| Si | Ge |
| liquid reacts with water | liquid reacts with water |
| none | water-soluble solid |
| none | acidic hydrate |
| metals | |
| Sn | Pb |
| liquid reacts with water | liquid reacts with water |
| water-soluble solid | water-insoluble solid |
| acidic hydrate | pH inactive hydrate |
The image shows the tetrahedral arrangement of the chlorine atoms about the central atom in SiCl4.
The chlorides of the heavier elements are all reactive compounds that fume in the presence of water. They cannot be recovered from their aqueous solution due to the reaction below. The solution produced in strongly acidic due to four moles of HCl having been produced for each mole of the tetrachloride consumed.
ECl4(l) + 4H2O 
E(OH)4(s) + 4HCl(aq)
E(OH)4(s) + 4HCl(aq)