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9.13. When hydrogen is burnt in oxygen the reaction is highly exothermic, it produces very high temperature nearly 4000°C which is used for cutting and welding purposes.

9.12. Metallic hydrides are useful for ultra-purification of dihydrogen and as dihydrogen storage media. In metallic hydrides, hydrogen is adsorbed as H-atoms. Due to the adsorption of H atoms the metal lattice expands and become unstable. Thus, when metallic hydride is heated, it decomposes to form hydrogen and finely divided metal. The hydrogen evolved can be used as fuel.

11.61 

In ortho nitrophenol there is intra-molecular H bonding, whereas in para-nitrophenol there is inter-molecular H bonding, as shown below:

And because of that para-nitrophenol get tightly bounded with water and ortho nitrophenol is steam volatile and it will leave the solution.

9.11. Those hydrides which do not have fix composition are called non-stoichiometric hydrides, and the composition varies with temperature and pressure. This type of hydrides is formed by d- and f-block elements. They cannot be formed by alkali metals because alkali metal hydrides form ionic hydrides.

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11.60

The different forms of cresol is formed with given molecular formula:

2-methylphenol

3-methylphenol

4-methylphenol

11.57 

Due to the presence of –OH group, alcohols form hydrogen-bonds with water but hydrocarbons cannot form hydrogen-bonds with water.

Due to inter moleculer hydrogen bonding between Alcohol and water molecular they remain tightly bounded to water molecules and have higher solubility. Whereas in case of hydrocarbon there is no chance of hydrogen bonding.

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11.56

Here, propanol undergoes intermolecular H-bonding because of the presence of -OH group while butane has no such property

(intermolecular Hydrogen bonding in propanol)

Therefore, extra energy will be required to break those hydrogen bonds which in turn causes higher boiling point for propanol when compared to butane.

9.10. Carbon hydrides of the type C_nH_2n+2 are electron precise hydrides. Because they have atom with exact number of electrons to form covalent bonds. Thus, they do not behave as Lewis acid or base. Since they have no tendency to accept or lose electrons.

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9.8.  (i) Electron deficient hydrides: Compounds in which central atom has incomplete octet, are called electron deficient hydrides. For example, BeH₂, BH₃ are electron deficient hydrides.

(ii) Electron precise hydrides: Those compounds in which exact number of electrons are present in central atom or the central atom contains complete octet are called precise hydrides e.g., CH₄, SiH₄, GeH₄ etc. are precise hydrides.

(iii) Electron rich hydrides: Those compounds in which central atom has one or more lone pair of excess electrons are called electron rich hydrides, e.g., NH₃, H₂O.

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9.7. This is due to its small atomic size and small bond length (74 pm) of H-H bond.H? H bond has very high bond enthalpy (435.9 kJ/mol) which results in low reactivity at room temperature. The reactivity is increased at high temperature or in presence of catalyst. Under these conditions, hydrogen reacts with many metals and non-metals to form hydrides.