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How do dipole dipole forces affect the melting and boiling points of substances?
Wiki User
∙ 13y ago
Think relationships here... really London Dispersion Force is like an acquaintance, Dipole Dipole is like boyfriend/girlfriend and Hydrogen Bonding is like marriage. Now out of the three London dispersion is the easiest to break the bonds, Di Pole Di pole are a little harder to break up and Hydrogen bonding are the hardest to break up the bonds. Hydrogen Bonding will always have the strongest bond. London dispersion is when for a split second their is a short attraction and doesn't last long. It is very weak therefore making this non- polar. Dipole Dipole means 2 opposite sides. Positive and negative charges. This molecule is a Polar molecule. Hydrogen Bonding is a Polar molecule which attaches itself to either N,O,or F. A melting point takes a low energy to melt so the bonds are weak. the higher the boiling temperature the stronger the bonds. Think H20. Melting is comparing how hard it is to separate the molecules. Same Concept. Ex.1.) CH4 / LiCl
CH4 more soluable / LiCl low soluability
CH4 low melting point / LiCL higher melting point
CH4 low boiling point/ LiCL Higher boiling point
CH4 London Dispersion / LiCl Dipole Dipole
Example2: H2O / NaCl
H2O high boiling point/ NaCl lower boiling point
H2O Hydrogen bonding/ NaCl Dipole Dipol
Wiki User
∙ 13y ago
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Weak dipole-dipole forces result in a what melting point?
The stronger the bonds between molecules; the higher the melting/boiling points. This makes sense if you think about it, melting/boiling is splitting up the molecules - the stronger they are bonded the more energy you will need
Why do dipole forces have an impact on the melting and boiling points of substances?
Dipoles are a form of intermolecular force which holds molecules together. The greater the intermolecular force, usually the greater the boiling point, for example.
Which intermolecular force would affect melting point the least Ionic bonds Van der Waals forces hydrogen bonding or Dipole-dipole interactions?
Van der Waals forces
Which intermolecular force would affect melting point the least Ionic bonds Van der Waals forces hydrogen bonding or Dipole dipole interactions?
Van der Waals - they're the weakest.
Are dipole-dipole forces moderate or weak?
They are weaker as compared to the ionic bonds. Since Ionic bonding takes place when one element loses an electron and another gains it. Due to this ionic compounds are stronger and have high melting and boiling points.
Weak dipole-dipole forces result in a what melting point?
The stronger the bonds between molecules; the higher the melting/boiling points. This makes sense if you think about it, melting/boiling is splitting up the molecules - the stronger they are bonded the more energy you will need
Why do dipole forces have an impact on the melting and boiling points of substances?
Dipoles are a form of intermolecular force which holds molecules together. The greater the intermolecular force, usually the greater the boiling point, for example.
How do The dipole-dipole forces affect the melting and boiling points of substances?
Think relationships here... really London Dispersion Force is like an acquaintance, Dipole Dipole is like boyfriend/girlfriend and Hydrogen Bonding is like marriage. Now out of the three London dispersion is the easiest to break the bonds, Di Pole Di pole are a little harder to break up and Hydrogen bonding are the hardest to break up the bonds. Hydrogen Bonding will always have the strongest bond. London dispersion is when for a split second their is a short attraction and doesn't last long. It is very weak therefore making this non- polar. Dipole Dipole means 2 opposite sides. Positive and negative charges. This molecule is a Polar molecule. Hydrogen Bonding is a Polar molecule which attaches itself to either N,O,or F. A melting point takes a low energy to melt so the bonds are weak. the higher the boiling temperature the stronger the bonds. Think H20. Melting is comparing how hard it is to separate the molecules. Same Concept. Ex.1.) CH4 / LiCl CH4 more soluable / LiCl low soluability CH4 low melting point / LiCL higher melting point CH4 low boiling point/ LiCL Higher boiling point CH4 London Dispersion / LiCl Dipole Dipole Example2: H2O / NaCl H2O high boiling point/ NaCl lower boiling point H2O Hydrogen bonding/ NaCl Dipole Dipol
What are the factors that affect the boiling point?
There are basically two types of bonding in substances that affect the boiling point. Some compounds are composed of extensive networks of atoms held together by either ionic or covalent bonds. These network substances have very high melting and boiling points. NaCl is an example of an ionic network and SiO2 is an example of a covalent network. The key factors that affect the boiling points of molecular compounds are the intermolecular forces which attract one molecule to another. For covalent compounds these intermolecular forces are called van der Waals forces and consist of hydrogen bonding, dipole-dipole attraction, and London dispersion forces. Hydrogen bonding is usually stronger than dipole-dipole interactions. London dispersion forces, often weaker forces, are found between all molecules, even if other van der Waals forces are present. The boiling point of a solution is also affected by the ambient pressure. Boiling occurs at a temperature where the vapor pressure of the liquid is equal to the ambient pressure. The third thing that affects the boiling point of a solution is any substance that is dissolved in the liquid. The more particles (ions or molecules) there are dissolved in the solution, the higher the boiling point.
What are the factors affecting the melting point of the substance?
There are basically two types of bonding in substances that affect the boiling point. Some compounds are composed of extensive networks of atoms held together by either ionic or covalent bonds. These network substances have very high melting and boiling points. NaCl is an example of an ionic network and SiO2 is an example of a covalent network. The key factors that affect the boiling points of molecular compounds are the intermolecular forces which attract one molecule to another. For covalent compounds these intermolecular forces are called van der Waals forces and consist of hydrogen bonding, dipole-dipole attraction, and London dispersion forces. Hydrogen bonding is usually stronger than dipole-dipole interactions. London dispersion forces, often weaker forces, are found between all molecules, even if other van der Waals forces are present. The boiling point of a solution is also affected by the ambient pressure. Boiling occurs at a temperature where the vapor pressure of the liquid is equal to the ambient pressure. The third thing that affects the boiling point of a solution is any substance that is dissolved in the liquid. The more particles (ions or molecules) there are dissolved in the solution, the higher the boiling point.
Which intermolecular force would affect melting point the least Ionic bonds Van der Waals forces hydrogen bonding or Dipole-dipole interactions?
Van der Waals forces
Which intermolecular force would affect melting point the least Ionic bonds Van der Waals forces hydrogen bonding or Dipole dipole interactions?
Van der Waals - they're the weakest.
Are dipole-dipole forces moderate or weak?
They are weaker as compared to the ionic bonds. Since Ionic bonding takes place when one element loses an electron and another gains it. Due to this ionic compounds are stronger and have high melting and boiling points.
What happens to the boiling point of benzene when a solute is added?
if you put an ionic compound in a polar substance it will raise the boiling point because the resulting ion dipole bonds will be stronger than the previously existing dipole dipole bonds
Does ch3ch2ch3 have a higher or lower boiling point than ch3cn?
Lower. CH3CN is polar and has a dipole-dipole attraction.
What molecular solid would have the lowest boiling point?
A. One with induced dipole attractions B. One that has hydrogen bonding C. One with dipole-dipole attractions D. One made of polar molecules C. One with dipole-dipole attractions - The molecular solids would have the lowest boiling point because of WEAK INTERMOLECULAR FORCES.
What substances would exhibit dipole-dipole intermolecular force bcl2 cf4 co2 cl2 nh3?
co2
