Table of Contents
- 1 Why do the hydrides of N O and F have higher boiling point than the other members in the group?
- 2 Why does the boiling point of hydrides increases down the group?
- 3 Would you expect the hydrides of N O and F lower boiling points than the hydrides of their subsequent group members give reason?
- 4 Would you expect the hydrides of N O and F to have lower boiling points than hydrides of their subsequent group members give reasons?
- 5 Why does water have a higher boiling point than the other hydrides?
- 6 Why does group 16 have higher boiling points than Group 17?
- 7 Why do group VI hydrides have different boiling points?
- 8 Why does water have a higher boiling point than other hydrides?
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.
Why does the boiling point of hydrides increases down the group?
The partial charges, induced by the higher electronegativity of oxygen, mean that the hydrogens and oxygens will be attracted to one another by coloumbic forces. This in turn will increase the energy needed to pull the molecules apart, thus an increase in the boiling point is observed.
Why is the boiling point of water is the highest among the hydrides of the group 16 elements?
Group 16 hydride molecules have a bent shape. Weaker intermolecular forces act between other Group 16 hydride molecules. The melting point and boiling point of water (H2O) molecules is unexpectedly high due to the stronger hydrogen bonds acting between water molecules.
Why H o2 contain higher boiling point than other hydrides of same group?
Due to higher electronegativity of N, O and F; NH3,H2O and HF show hydrogen bonding and hence higher boiling points than the hydrides of their subsequent group members.
Would you expect the hydrides of N O and F lower boiling points than the hydrides of their subsequent group members give reason?
Nitrogen, oxygen and Fluorine are highly electronegative. The boiling points of hydrides of N,O and F are expected to be lower than the hydrides of their subsequent group members on the basis of their molecular masses. But they have higher boiling point because of their higher electronegativity.
Would you expect the hydrides of N O and F to have lower boiling points than hydrides of their subsequent group members give reasons?
Give reasons. The boiling points of NH3, H2O and HF are expected to be lower than those of the subsequent group member hydrides on the basis of molecular masses. This is because of higher electronegativity of N, O and F. As a result, these exhibit hydrogen bonding in their hydrides.
Why are group 16 hydrides polar molecules?
These hydrides all have a bent shape due to the two lone pair of electrons on the central atom. This makes the molecules polar and due to an uneven charge distribution.
Why does the basicity of hydrides decrease down the group?
In group 15, the hydrides have a lone pair on the central atom. Going down the group, size of the atom increases. And hence, electron density over the group 15 elements decreases. Thus tendency to donate electrons decreases and basicity decreases.
Why does water have a higher boiling point than the other hydrides?
These hydrogen-bond attractions can occur between molecules (intermolecular) or within different parts of a single molecule (intramolecular). Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group 16 hydrides that have no hydrogen bonds.
Why does group 16 have higher boiling points than Group 17?
Oxygen as a 1st row element, is far more electronegative than sulfur and tellurium, and the O−H is far more polar as a result. The resultant intermolecular hydrogen bonding between adjacent molecules accounts for the exceptionally high boiling point of water, compared to the lower Group VI hydrides.
Why does CH3CH2OH have a higher boiling point than ch3och3?
(c) Both CH3OH and CH3CH2OH can H-bond but CH3CH2OH has more CH bonds for greater dispersion force interactions. Therefore, CH3CH2OH has the higher boiling point.
Why does water have high melting and boiling points than other hydrides?
Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group 16 hydrides that have no hydrogen bonds.
Why do group VI hydrides have different boiling points?
This same differential boiling point can be seen of the Group VII hydrides. Compare the boiling point of H F versus H Cl and H Br; hydrogen bonding accounts for the disparity. For the other Group VI hydrides, dispersion forces are the dominant intermolecular force. Dispersion forces result from the transient polarization of the electron cloud.
Why does water have a higher boiling point than other hydrides?
The resultant intermolecular hydrogen bonding between adjacent molecules accounts for the exceptionally high boiling point of water, compared to the lower Group VI hydrides. This same differential boiling point can be seen of the Group VII hydrides. Compare the boiling point of H F versus H Cl and H Br; hydrogen bonding accounts for the disparity.
How many valence electrons does a group 16 hydride have?
An atom of hydrogen has 1 valence electron. Bonds between hydrogen and Group 16 atoms are covalent so the hydrides of Group 16 elements are covalent molecules. Group 16 hydride molecules have a bent shape. The most significant intermolecular force acting between water (H 2 O) molecules is the hydrogen bond.
What type of intermolecular forces are present in Group 16 hydride molecules?
Group 16 hydride molecules have a bent shape. The most significant intermolecular force acting between water (H 2 O) molecules is the hydrogen bond. Weaker intermolecular forces act between other Group 16 hydride molecules.