| Reactions of Sodium |
 Reactions with water |
| Sodium metal reacts rapidly with water to form a colourless solution of sodium hydroxide and hydrogen gas. The is an exothermic reaction, the sodium metal may well become so hot that it catches fire and burns with a characteristic orange colour. The
reaction is slower than that of potassium but faster than that of lithium.
|
2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) |
| Reactions with air |
| The shiny surface of sodium soons becomes dull due to the reaction of air and moisture. |
| When sodium is burnt in air the result is white sodium peroxide together with some white sodium oxide. |
| 2Na(s) + O2(g)2Na2O(s) |
| 4Na(s) + O2(g)2Na2O2(s) |
| Reactions with halogens |
| Sodium reacts vigorously with all halogens to form sodium halides. |
| 2Na(s) + F2(g)NaF(s) |
| 2Na(s) + Cl2(g)NaCl(s) |
| 2Na(s) + Br2(g)NaBr(s) |
| 2Na(s) + I2(g)NaI(s) |
| Reactions with acids |
| Sodium readily dissolves in dilute sulphuric acid to form a solution containing the Na(I) ion and hydrogen gas.
|
| 2Na(s) + H2SO4(aq)2Na+(aq) + SO42-(aq) + H2(g) |
| Reactions with bases |
| Sodium metal reacts rapidly with water to form a colourless solution of sodium hydroxide and hydrogen gas. The is an exothermic reaction, the sodium metal may well become so hot that it catches fire and burns with a characteristic orange colour. The
reaction is slower than that of potassium but faster than that of lithium.
|
| 2Na(s) + 2H2O(l)2NaOH(aq) + H2(g) |
Na(s)