Water has a high boiling point compared to other main-group hydrides because of its unique hydrogen bonding properties. The hydrogen bonds between water molecules are stronger than the typical dipole-dipole interactions found in other hydrides, leading to a higher boiling point.
i only got uses of ionic hydrides her it is: Ionic hydrides and their complexes are used as reducing agents. They evolve hydrogen when heated. Hence they are used as solid fuels as they ignite spontaneously. (source: WWW.tutorvista.com)
hydrogen bonding exists in compounds having partially positively charged hydrogen and highly electronegative atoms bearing partial -ve charge. such intermolecular forces of attraction infleuence the physical properties like melting and boilingg points. the greater the size of atoms the greater the polarazability hence the greater the boiling points for example: the hydrides of fourth period show greater boiling point than those of third period due to ggreater size and greater polarizability.
Yes, alcohols generally have higher boiling points compared to other substances due to the presence of hydrogen bonding between alcohol molecules.
Boiling occurs at a higher temperature and involves the entire liquid reaching its boiling point, whereas evaporation happens at the surface of the liquid. Boiling provides more energy to break the intermolecular forces holding the liquid molecules together, leading to a faster transition to the gas phase compared to evaporation.
The reason ch3br or ch3f have higher boiling points compared to other compounds is because they have stronger intermolecular forces due to the presence of hydrogen bonding.
Hydrogen bonding.
Hydrogen sulfide (H2S) has the lowest boiling point among the hydrides of the chalcogen group (oxygen, sulfur, selenium, and tellurium). This is because hydrogen sulfide is a smaller molecule with weaker intermolecular forces compared to the other chalcogen hydrides.
i only got uses of ionic hydrides her it is: Ionic hydrides and their complexes are used as reducing agents. They evolve hydrogen when heated. Hence they are used as solid fuels as they ignite spontaneously. (source: WWW.tutorvista.com)
hydrogen bonding exists in compounds having partially positively charged hydrogen and highly electronegative atoms bearing partial -ve charge. such intermolecular forces of attraction infleuence the physical properties like melting and boilingg points. the greater the size of atoms the greater the polarazability hence the greater the boiling points for example: the hydrides of fourth period show greater boiling point than those of third period due to ggreater size and greater polarizability.
Evaporation is very slow at converting liquid to gas compared to boiling.
Water has a boiling point of 100 degrees celcius. This is about average compared to the boiling point of other substances.
To speak of an application of hydrogen bonding implies that we make it happen to suit our purposes, but it's a natural phenomenon. It would be more appropriate to discuss its occurrences. It is responsible for the anomalously high boiling point of water and therefore the existence of life on Earth.
The boiling point of sea water is higher compared with pure water. Temperature remain constant during boiling.
Yes, alcohols generally have higher boiling points compared to other substances due to the presence of hydrogen bonding between alcohol molecules.
Boiling occurs at a higher temperature and involves the entire liquid reaching its boiling point, whereas evaporation happens at the surface of the liquid. Boiling provides more energy to break the intermolecular forces holding the liquid molecules together, leading to a faster transition to the gas phase compared to evaporation.
A liquid with a lower boiling point will boil quicker because it requires less energy to reach its boiling point compared to a liquid with a higher boiling point.
Hexane has a lower boiling point compared to butanol. The difference in boiling points arises from the difference in molecular weights, functional groups, and intermolecular forces present in the two compounds. Butanol, with its hydroxyl group, exhibits stronger hydrogen bonding interactions, leading to a higher boiling point compared to hexane.