Intermolecular forces
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The document discusses intermolecular forces and their relationship to solubility. It defines intermolecular forces as forces between molecules that are weaker than intramolecular forces. There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding, with hydrogen bonding being the strongest. Compounds with stronger intermolecular forces are harder to separate and therefore have higher melting and boiling points, making them more likely to be liquids or solids, while those with weaker forces are more likely to be gases.
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Intermolecular Forces are foces actingwithin a molecule.You should.pdf
Intermolecular Forces are foces actingwithin a molecule.
You should first note whehter the molecule is metallic, ionicor covalent.
There are three different types of Intermolecular Forces thatapplies for covalent molecules:
Dispersion force,Dipole-dipole interactions and hydrogen bonds.
The relative strength of these forces are: dispersion forces< dipole-dipole interactions <
hydrogen bonds
Hence, dispersion forces are the weakest and hydrogen bondsare the strongest.
Dispersion forces (aka. van der Waals Forceor London Force) are for non-polarmolecules.Non-
polar molecules have no dipoles, or the dipoledoesn\'t extend throughout the molecule, and only
dispersion forces.They are generally don\'t mix with water, and are usually anyelement and
carbon compounds.
For example:Cl2,CO2,N2O4,CH4
Dipole-Dipole forces occur between moleculesthat have permanent net dipoles, (hencepolar
molecules)
Polar molecules usually have a dipole and may contain a highlyelectronegative element bonded
to hydrogen, allowing hydrogenbonding. They are also usually soluble in water.
For example: SCl2 , PCl3,CH3Cl
Hydrogen Bonds occur between molecules thathave permanent net dipole resulting from
hydrogen beingcovalently bonded to either fluorine, oxygen ornitrogen.
For example: HF, H2O, H2O2 ,CH3OH, CH3COOH,CH3NH2
These forces operate between covalentmolecules.
As for your answer,
Na+: Dispersion
H3C-CH3: Dispersion
K2O : Ionic Bond
H2O: Hydrogen bonding, the hydrogen has a verylow electronegativety resulting in the oxygen
atoms having greateraffinity to the covalently shared electrons.
NH3 : polar, hence dipole-dipole and hydrogenbonding, since the hydrogen is slightly +ve and
the nitrogenslightly -ve. There more electronegative nitrogen pulls thehydrogen electron towards
it, giving a dipole moment .
Ne: non polar, hence dispersion forces only(randomness of electron clouds instantaneously
causes oppositecharges at the ends of the molecule which induces the same effectin another)
If you want to learn more, this site might help:
http://science.uwaterloo.ca/~cchieh/cact/c123/intermol.html
Solution
Intermolecular Forces are foces actingwithin a molecule.
You should first note whehter the molecule is metallic, ionicor covalent.
There are three different types of Intermolecular Forces thatapplies for covalent molecules:
Dispersion force,Dipole-dipole interactions and hydrogen bonds.
The relative strength of these forces are: dispersion forces< dipole-dipole interactions <
hydrogen bonds
Hence, dispersion forces are the weakest and hydrogen bondsare the strongest.
Dispersion forces (aka. van der Waals Forceor London Force) are for non-polarmolecules.Non-
polar molecules have no dipoles, or the dipoledoesn\'t extend throughout the molecule, and only
dispersion forces.They are generally don\'t mix with water, and are usually anyelement and
carbon compounds.
For example:Cl2,CO2,N2O4,CH4
Dipole-Dipole forces occur between moleculesthat have permanent net dipoles, (hencepolar
molecu.
Intermolecular forces of attraction ( IMF)
This is a ppt for the topic IMF this is only a brief lectures that i made for my reporting.
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- 1. T U E S D A Y R E V I E W S E S S I O N O C T O B E R 4 , 2 0 1 0 Intermolecular Forces and Solubility
- 2. Intermolecular Forces Definition: Forces between molecules Intermolecular forces are much weaker than intramolecular forces There are three different types London Dispersion Forces/ Van der Waals Dipole-Dipole Interactions Hydrogen Bonds
- 3. London Dispersion Forces Also referred to as Van der Waals forces Occurs because of momentary dipole (uneven distributions of electrons in a molecule causing a partially negative end and a partially positive end) These are the weakest intermolecular forces
- 4. Dipole-Dipole Interactions Occurs when polar molecules align so that their oppositely charged ends are attract each other This bond is stronger than Van der Waals forces
- 5. Hydrogen Bonding A type of dipole-dipole bond that occurs when hydrogen is bonded to a highly electronegative atom (O, F, N) This is the strongest intermolecular force
- 6. Intermolecular Forces Trends Compounds with stronger intermolecular forces will be harder to separate therefore they will have larger melting points and boiling points This means compounds with weak intermolecular forces are more likely to be found in gaseous form, while compounds with stronger molecular forces are more likely to be found as liquids or solids