Why does boiling point of hydrides increases down the group?

For hydrides of group 16, the boiling point and melting point definitely increases down the group as molecular mass increases. But then, water has an exceptionally high boiling point due to the presence of stronger intermolecular hydrogen bonding between the water molecules.

Why do the hydrides of N O and F have higher boiling point than the other members in the group?

However, due to high electro negativity of nitrogen, oxygen and fluorine, their hydrides form strong intermolecular hydrogen bond and hence they have boiling point higher than the hydrides of subsequent group members.

Which has the higher boiling point HF HF or HCL HCL Why?

Since the van der Waals bond is stronger than hydrogen, HF will have a higher boiling temperature. c) The intermolecular bonding for HF is hydrogen, whereas for HCL, the intermolecular bonding is van der Waals. Since the hydrogen bond is stronger than van der Waals, HF will have a higher boiling temperature.

Why does boiling point increase with hydrogen bonding?

The evidence for hydrogen bonding The increase in boiling point happens because the molecules are getting larger with more electrons, and so van der Waals dispersion forces become greater. These relatively powerful intermolecular forces are described as hydrogen bonds.

Why does boiling point decrease down group 6?

The 7A elements (Fluorine, Chlorine, Bromine, Iodine) make weakly polar hydrides, and correspondingly weaker Van der Waals forces and intermolecular attraction; therefore their boiling points are lower.

Why does the bond angle of hydrides decrease down the group?

Dipole moment is proportional to electronegativity of the central atom. So it decreases down the group. These hydrides are pyramidal in shape with a lone pair of electrons in one of the orbits. The bond angle gradually decreases down the group due to the decrease in bond pair- bond pair repulsions.

What is the trend of boiling point of hydrides of Nof?

Due to higher oxidation states of N, O and F, the boiling points of NH3, H2O and HF are higher than the hydrides of their subsequent group members.

What is the trend of boiling point of hydrides of NO and F?

There is no regular trend in the boiling points of hydrides. Due to higher oxidation states of N, O and F, the boiling points of NH3,H2O and HF are higher than the hydrides of their subsequent group members. Due to higher electronegativity, the extent of hydrogen bonding is quite appreaciable.

Why does intermolecular forces affect boiling point?

Higher the intermolecular forces between the liquid particles, harder it is for it to escape into the vapor phase, ie., you need more energy to convert it from liquid to the vapor phase, in other words, higher its boiling point.

Why does HF have a higher boiling point than NH3?

This is due to weak van der Waal’s force existing between any 2 molecules. Also, there is a factor of hydrogen bonding. The H-F bond is more polar than H-N bond, hence there is stronger hydrogen bond in HF compared to NH3. Due to this reasons, HF has higher boiling point than NH3.

Why do 14-17 hydrides have different boiling points?

Such that in the chart below comparing boiling points of groups 14-17 hydrides, the values of ammonia (NH 3 ), water (H 2 O), and hydrogen fluoride (HF) break the increasing boiling point trend. Supposedly, as the molecular mass increases, the boiling points increase as well.

What is the effect of hydrogen bonding on boiling point?

Stronger hydrogen bonding leads to a higher boiling point. Therefore you have a higher charge difference between the hydrogen atom and the fluoride atom leading to a greater attraction and strongness of the hydrogen bonding.

Which has a higher melting point HF or HBr?

Melting and Boiling points of Hydrogen Fluoride (HF) are higher than Hydrochloric acid (HCl), Hydrobromic acid (HBr) and Hydrogen iodide (HI). Fluorine has the highest electronegativity of an atom.