Resemblance with alkali metals:
1. Like alkali metals, hydrogen contains one valence electron in its valency shell.
Hence, it can lose one electron to form a unipositive ion.
2. Like alkali metals, hydrogen combines with electronegative elements to form oxides, halides, and sulphides.
Resemblance with halogens:
1. Both hydrogen and halogens require one electron to complete their octets.
Hence, hydrogen can gain one electron to form a uninegative ion.
2. Like halogens, it forms a diatomic molecule and several covalent compounds. Though hydrogen shows some similarity with both alkali metals and halogens, it differs from them on some grounds. Unlike alkali metals, hydrogen does not possess metallic characteristics. On the other hand, it possesses a high ionization enthalpy. Also, it is less reactive than halogens.
Owing to these reasons, hydrogen cannot be placed with metals (group I) or with halogens (group VII). In addition, it was also established that ions cannot exist freely as they are extremely small. ions are always associated with other atoms or molecules. Hence, hydrogen is best placed separately in the periodic table.
Q: 2. Write the names of isotopes of hydrogen. What is the mass ratio of these isotopes?
Hydrogen has three isotopes. They are:
2. Deuterium, or D, and
3. Tritium, or T
The mass ratio of Protium, deuterium and tritium is
Q: 3. Why does hydrogen occur in a diatomic form rather than in a monoatomic form under normal conditions?
The ionization enthalpy of hydrogen atom is very high Hence, it is very hard to remove its only electron. As a result, its tendency to exist in the monoatomic form is rather low. Instead, hydrogen forms a covalent bond with another hydrogen atom and exists as a diatomic molecule.
Q: 4. How can the production of dihydrogen, obtained from ‘coal gasification’, be increased:
Dihydrogen is produced by coal gasification method as:
This reaction is called the water-gas shift reaction. Carbon dioxide is removed by scrubbing it with a solution of sodium arsenite.
Q: 5. Describe the bulk preparation of dihydrogen by electrolytic method. What is the role of an electrolyte in this process?
Dihydrogen is prepared by the electrolysis of acidified or alkaline water using platinum electrodes. Generally, 15 - 20o of an acid (H2S04) or a base (Na0H) is used. Reduction of water occurs at the cathode as:
At the anode, oxidation of ions takes place as:
∴ Net reaction can be represented as:
Electrical conductivity of pure water is very low owing to the absence of ions in it. Therefore, electrolysis of pure water also takes place at a low rate. If an electrolyte such as an acid or a base is added to the process, the rate of electrolysis increases. The addition of the electrolyte makes the ions available in the process for the conduction of electricity and for electrolysis to take place.