To determine the type of IMFA that occurs in each of given substances you can do so by examining the types of molecules which make up the substances and consider the relative strengths of the IMFA between them.
An example of this would be a substance that is composed of nonpolar molecules like methane will have London Dispersion forces as the dominant IMFA.
You can identify the strongest intermolecular force by making a visual model of the intermolecular attractions by drawing the Lewis structures.
Based on how close the electrons or nucleus of one molecule/atom can get to another nucleus or electron pair, you can distinguish what will be stronger.
For instance, H forms Hydrogen bonds with lone pairs on O, N, and F, so it's proximity is very close, since they are small atoms.
Therefore, hydrogen bonding will always be stronger.
Another way to remember the order of intermolecular force strength is to think about the strength of the charges on ions, dipoles, and induced dipoles respectively.
Ions are charged atoms of elements, and thus, already have a full charge associated with them (+1, +3, -2 etc.)
Thus, the interactions between these charged particles will be very strong.
Dipoles on the other hand are due to partial charges.
Dipoles arise in a molecule due to a different in electronegativity, and the charges on the elements in the molecules are not complete charges.
These partial charges are less charged than the full charges associated with ions and so form IMFs that are weaker than those between ions.
Finally, induced dipoles are simply moments of unequal charge distribution.
They are fleeting moments in which different parts of the molecule have either a slightly positive or slightly negative charge.
These are the weakest in terms of full charges and so form the weakest interactions.
After you understand these three, you can make combinations that will give you the order of IMF strength.
Ion-Ion is strongest since it has two of the full charge objects, whereas Ion-dipole is second strongest because it has one full charge and one partial charge "object" in the interaction.
This extend down to dipole-dipole, dipole-induced dipole, and finally, induced dipole-induced dipole.
Hydrogen bonding a specific case that you would just memorize as being an especially strong dipole-dipole interaction, and so would be between ion-dipole and dipole-dipole.
The bonds that have weak intermolecular forces are London dispersion forces which are under the category of van der Waal forces.
The London intermolecular forces exist between all types of molecules, whether ionic or covalent-polar or nonpolar.
The intermolecular forces are forces of attraction or repulsion which act between neighboring particles which include atoms, ions and molecules.
The intermolecular forces are important because they help chemists determine the physical properties of a substance such as it's state, it's boiling and melting point etc.
The strong the intermolecular forces are the higher the boiling points and melting points are.
The weakest of the 4 types of intermolecular forces is the London dispersion forces which are temporary attractive forces which develop temporary dipole and hence they are also known as the induced dipole induced dipole.
The three types of intermolecular forces are similar in that they are all electrostatic in nature.
The positive and negative dipoles on different particles can also interact with each other, ions, etc and especially dipole forces and dispersion forces.
The differences are in the fundamental structures of the interacting particles.
You can identify different intermolecular forces by how much attraction occurs between the molecules.
For example weak intermolecular forces will result in a greater distance between 2 or more molecules.
The intermolecular forces from strongest to weakest are Ion dipole (strongest) > hydrogen bonding > dipole-dipole > London dispersion forces.
The thing that dictates intermolecular forces are how the electrons are shared within the covalent bonds of molecules.
And intermolecular forces refer to the types of interactions which occur between molecules.
The bond that has stronger intermolecular forces are hydrogen bonding and the bond that has weakest intermolecular forces is the London dispersion attraction force.
Hydrogen bonds are formed between all molecules as any molecule that has a hydrogen atom attached directly to an oxygen or a nitrogen is capable of hydrogen bonding.
Hydrogen bonds also occur when hydrogen is bonded to fluorine although the HF group does not appear in other molecules.
Covalent bonds are stronger than hydrogen bonds and a hydrogen bond is an electrostatic attraction between an atom and a positive charge of a hydrogen atom that is covalently bound to something else.
A hydrogen bond is weaker than a covalent bond and can be either intramolecular or intermolecular.
The weakest intermolecular force is the London dispersion force which is a temporary attractive force which results when the electrons in two adjacent atoms occupy positions which make the atoms form temporary dipoles.
The four intermolecular forces from weakest to strongest are van der waals, dipole-dipole, hydrogen bonds, ion-dipole and then ion-ion.
The 4 types of intermolecular forces are Ion-ion interactions, dipole-dipole interactions, hydrogen bonding, and London dispersion force.
To determine the intermolecular forces determine the intermolecular forces in the compounds, and then arrange the compounds according to the strength of those forces.
The strength of attractive forces between two dipoles depends on the electronegativity and the polarity of the molecule.
Electronegativity is the likelihood of an electron to hoard electrons and exhibit a negative charge.
The higher the electronegativity, the stronger the dipole-dipole interaction.
Intermolecular forces are forces that electrostatic in nature and include van der Waals forces and hydrogen bonds.
The molecules in the liquids are held to other molecules by intermolecular interactions, which are weaker than the intramolecular interactions that hold the atoms together within molecules and polyatomic ions.
The 4 different types of intermolecular forces are Ion-ion interactions, dipole-dipole interactions, hydrogen bonding, and London dispersion force.
An intermolecular force is an attractive force that arises between the positive components (or protons) of one molecule and the negative components (or electrons) of another molecule. Various physical and chemical properties of a substance are dependent on this force.
Ion-dipole intermolecular forces are electrostatic reactions between a polar molecule and an ion and are often the result of ionic compounds being dissolved into polar substances.
Dipole-dipole forces are the attraction between the negative end of one polar molecule and the positive end of a different polar molecule.
In a liquid, intermolecular attractive forces hold the molecules in contact, although they still have sufficient KE to move past each other.
Intermolecular attractive forces, collectively referred to as van der Waals forces, are responsible for the behavior of liquids and solids and are electrostatic in nature.
Hydrogen bonds, dipole-induced dipole forces, and London dispersion forces all exist in water.
Polar OH bonds exist in water.
The negative O atoms attract the positive H atoms in adjacent molecules, forming a hydrogen bond, which is an extremely powerful sort of dipole-dipole interaction.
The London dispersion force is the weakest intermolecular force.
The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.