Van der Waals forces
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.
This element is strontium (Sr).
helium has the least density, xenon has the highest.
When gas is released in a container the gas molecules spread all over the container and show that they have least force of attraction.
Van der Waals forces
London dispersion forces would generally affect the boiling point the least among intermolecular forces. These forces are relatively weak and depend on the size of the molecules involved rather than their polarity. Hydrogen bonding, dipole-dipole interactions, and ion-dipole interactions are typically stronger and contribute more significantly to the boiling points of substances.
London dispersion forces would affect the melting point the least, as they are the weakest intermolecular force. They are caused by temporary fluctuations in electron density, making them generally less influential on physical properties compared to other intermolecular forces such as hydrogen bonding or dipole-dipole interactions.
Van der Waals forces
Ionic bonds would affect melting point the least. This is because ionic bonds are typically much stronger than the other intermolecular forces mentioned, making them less susceptible to changes in temperature that affect the melting point.
London dispersion forces would affect the melting point the least as they are generally weaker than dipole-dipole and hydrogen bonding forces.
Van der Waals forces APEX
Pepper has the least effect on the temperature or reaction to boiling water ,As well pepper does not dissolve in boiling water like other grains.
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.
Ionic bonds would affect the melting point the least because they involve strong electrostatic interactions between oppositely charged ions, which require a significant amount of energy to break. In comparison, Van der Waals forces, hydrogen bonding, and dipole-dipole interactions are weaker intermolecular forces that are easier to overcome, therefore influencing the melting point to a greater extent.
Van der Waals forces (dispersion forces) - weakest intermolecular force resulting from temporary fluctuations in electron distribution. Dipole-dipole interactions - intermediate strength intermolecular force arising from permanent dipoles in polar molecules. Hydrogen bonding - strongest intermolecular force involving a hydrogen atom bonded to a highly electronegative atom (such as O, N, or F) interacting with another electronegative atom.
Water is a polar molecule whereas methane is a non-polar molecule.The intra- molecular force in water molecule is much stronger compared top the intra- molecular force between a carbon and a hydrogen in methane.Water molecule have hydrogen bonding as its intra molecular force.Hydrogen bonding is the strongest, then comes dipole-dipole and the least strong is the London dispersion force.The molecular bonding of water is higher than that of methane (binding energy), and the intermolecular bonding of water is higher than that of methane (boiling point).