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There is no single boiling point. A variety of substances can form hydrogen bonds, all with different boiling points.

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Why is there a difference in boiling points between h2o and h2s?

The difference in boiling points between water (H2O) and hydrogen sulfide (H2S) is primarily due to differences in molecular structure and intermolecular interactions. Water molecules form stronger hydrogen bonds compared to hydrogen sulfide molecules, leading to a higher boiling point for water. Additionally, water molecules are more polar compared to hydrogen sulfide molecules, which also contributes to the difference in boiling points.


Which one has a higher boiling point a dispersion force or hydrogen bond or covalent bond or ionic bond?

Compounds with fully ionic bonds have higher boiling points than compounds without this feature, except for a few unusual, extensively three-dimensionally-bonded covalent compounds such a diamond and silica.


Why do aldehydes and ketones have lower boiling points than their correspending alcohols?

Ketones and aldehydes do not have hydrocarbon atoms which bond to nitrogen or oxygen, individual molecules do not hydrogen bond to each other which makes them have lower boiling points than alcohols.


In both liquid water and ice a hydrogen bond forms between .?

Oxygen atoms. The hydrogen bond is a weak attraction between a slightly positive hydrogen atom and a slightly negative oxygen atom within the water molecule. This bond gives water its unique properties such as high boiling and melting points.


How do you determine which molecule has a higher boiling point?

Compounds with Hydrogen bonds (Hydrogen bonded to N,O or F) will tend to have stronger bonds thus a higher BP, then the compounds with a stronger polarity determine bond strength, and finally dispersion forces (Molecular mass) So in conclusion if you have ex. HF and CO2 HF has a higher BP because it has a stronger bond than CO2 (it has a hydrogen bond, while CO2's strongest bond is a polar bond)

Related Questions

Why is there a difference in boiling points between h2o and h2s?

The difference in boiling points between water (H2O) and hydrogen sulfide (H2S) is primarily due to differences in molecular structure and intermolecular interactions. Water molecules form stronger hydrogen bonds compared to hydrogen sulfide molecules, leading to a higher boiling point for water. Additionally, water molecules are more polar compared to hydrogen sulfide molecules, which also contributes to the difference in boiling points.


Which one has a higher boiling point a dispersion force or hydrogen bond or covalent bond or ionic bond?

Compounds with fully ionic bonds have higher boiling points than compounds without this feature, except for a few unusual, extensively three-dimensionally-bonded covalent compounds such a diamond and silica.


Why Compounds having hydrogen bond generally have high boiling points?

Compounds that exhibit hydrogen bonding typically have higher boiling points due to the strong intermolecular forces associated with these bonds. Hydrogen bonds occur when hydrogen is covalently bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine, creating a significant dipole moment. This strong attraction between molecules requires more energy (in the form of heat) to overcome, resulting in higher boiling points compared to compounds that do not engage in hydrogen bonding.


Why do aldehydes and ketones have lower boiling points than their correspending alcohols?

Ketones and aldehydes do not have hydrocarbon atoms which bond to nitrogen or oxygen, individual molecules do not hydrogen bond to each other which makes them have lower boiling points than alcohols.


In both liquid water and ice a hydrogen bond forms between .?

Oxygen atoms. The hydrogen bond is a weak attraction between a slightly positive hydrogen atom and a slightly negative oxygen atom within the water molecule. This bond gives water its unique properties such as high boiling and melting points.


What are two ways that a covalent bond differs from a hydrogen bond?

A covalent bond is an actual sharing of electrons, whereas a hydrogen bond is an attractive force due to electronegativities. A hydrogen bond also adjusts a molecule's boiling point upwards.


How do you determine which molecule has a higher boiling point?

Compounds with Hydrogen bonds (Hydrogen bonded to N,O or F) will tend to have stronger bonds thus a higher BP, then the compounds with a stronger polarity determine bond strength, and finally dispersion forces (Molecular mass) So in conclusion if you have ex. HF and CO2 HF has a higher BP because it has a stronger bond than CO2 (it has a hydrogen bond, while CO2's strongest bond is a polar bond)


How does a hydrogen bond form and what role does it play in molecular interactions?

A hydrogen bond forms when a hydrogen atom is attracted to a highly electronegative atom, like oxygen or nitrogen, in a neighboring molecule. This bond is weaker than covalent bonds but still important in molecular interactions, as it helps stabilize the structure of molecules and influences properties like boiling points and solubility.


What is the melting point and boiling point of hydrogen?

The freezing point (same as melting point) of H2 is 14.01 K (−259.14 °C, −434.45 °F)The boiling point of H2 is 20.28 K (−252.87 °C, −423.17 °F)


What is the relationship between the melting point and boiling point of a compound and the compounds bond strength?

Several factors affect boiling point, including the forces between the molecules in a compound. The harder the molecules are holding on to each other, the more energy it takes to boil. Water molecules hold on to each other with hydrogen bonds, so it has relatively high boiling point.So, to answer your question, high boiling points might indicate strong intermolecular forces.


What compounds would have the highest boiling points?

ionic


Where does the dipole in the nitrogen-hydrogen bond point?

The dipole in the nitrogen-hydrogen bond points towards the nitrogen end. The arrow showing a dipole moment points towards the more electron rich region, with its tail at the electron poor region.