When the temperature of water is decreased and ice is formed then the molecules become more regular and this regularity extends throughout the whole structure. Empty spaces are left behind as shown in the figure below. That is why when water freezes it occupy 9% more space and its density decreases. The result is that…
Soaps and detergents perform the cleaning action because the polar parts of their molecules are water soluble due to hydrogen-bonding and non-polar parts remain outside water.
When we consider the hydrides of group VA, VIA, VIIA then NH3, HF and H2O show maximum boiling points in the respective series. The reason is the enhanced electronegative character of N, O and F. That is why, water is liquid at room temperature, but H2S and H2Se are gases. Comparatively high boiling points of…
In addition to water, ethyl alcohol (C2H5OH) also has the tendency to form hydrogen bonds. So, ethyl alcohol can dissolve in water because both can form hydrogen bonds with each other. Similarly, carboxylic acids are also soluble in water, if their sizes are small. Hydrocarbons being non-polar are not soluble in water at all, and…
Definition: The electrostatic force between a hydrogen atom bonded to a strongly electronegative atom and Hydrogen bond lone pair electrons of another Covalent bond strongly electronegative atom is called hydrogen bonding. Strength: Hydrogen bonds are not really chemical bonds in formal sense. These are weaker than covalent bond. However, hydrogen bonds are stronger than dipole-dipole…
Definition: The momentary forces of attraction which are created between and induced dipole is called Instantaneous dipole-induced dipole forces or London Dispersion Forces. Or The forces of attraction between non-polar molecules which are formed polar for an instant are called instantaneous dipole-induced dipole forces or London forces. Explanation: The forces of attraction present among the…