The 1-butanol has the largest molecules and resulting strongest dispersion forces. This gives it the lowest evaporation rate and the smallest ∆t. 3. The n-hexane has the stronger attractions between its molecules.
Which alkane has the strongest intermolecular forces?
Answer and Explanation: Hexane has the strongest intermolecular force of attraction among the given alkanes in the question. Alkanes have Van der Waals force of attraction between them, so with increase in number of carbon atoms, mass increases, surface area increases and force of attraction increases.
Which dispersion force is strongest?
The table below shows a comparison of the melting and boiling points for each. The dispersion forces are strongest for iodine molecules because they have the greatest number of electrons. The relatively stronger forces result in melting and boiling points which are the highest of the halogen group.
Which element has the strongest intermolecular forces?
The strongest intermolecular force is hydrogen bonding, which is a particular subset of dipole-dipole interactions that occur when a hydrogen is in close proximity (bound to) a highly electronegative element (namely oxygen, nitrogen, or fluorine).
What are the most important intermolecular forces in alkanes?
The four compounds are alkanes and nonpolar, so London dispersion forces are the only important intermolecular forces.
Which alkane has the weakest intermolecular forces?
The alkane with the weakest intermolecular forces is n-Pentane because n-Pentane had a higher change in temperature value.
What is the strongest intermolecular force in propanol?
1-Propanol features several different types of intermolecular bonding including London dispersion forces, dipole-dipole interactions, and hydrogen bonding. Of these, the hydrogen bonds are known to be the strongest.
Which attractive force is the weakest?
Dispersion forces are the weakest intermolecular force (one hundredth-one thousandth the strength of a covalent bond), hydrogen bonds are the strongest intermolecular force (about one-tenth the strength of a covalent bond).
Is Van der Waals bond the weakest?
Van der Waals forces are the weakest intermolecular force and consist of dipole-dipole forces and dispersion forces.
Why is London dispersion the weakest force?
The weakest of these forces is the London dispersion force, one of the Van der Waals forces. … This force is weaker in smaller atoms and stronger in larger ones because they have more electrons that are farther from the nucleus and are able to move around easier.
Which hydrogen bonding is the strongest?
The strength of hydrogen bond depends upon the coulumbic interaction between the electronegativity of the attached atom and hydrogen. Fluorine is the most electronegative element. F−H−−−F bond will be strongest H bond.
What is the strongest intermolecular force in water?
The strongest intermolecular force in water is a special dipole bond called the hydrogen bond. Many molecules are polar and can form bipole-bipole bonds without forming hydrogen bonds or even having hydrogen in their molecule.
Which substance has the weakest intermolecular forces?
- Oil- Only London Dispersion Forces (the weakest intermolecular force)
- Water- London Dispersion, Dipole-Dipole, and Hydrogen Bonding.
What are the 4 types of intermolecular forces?
There are four major classes of interactions between molecules and they are all different manifestations of “opposite charges attract”. The four key intermolecular forces are as follows: Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion forces.
What are 3 types of intermolecular forces?
There are three types of intermolecular forces: London dispersion forces (LDF), dipole- dipole interactions, and hydrogen bonding.
Why are alkanes unreactive?
Alkanes include strong carbon-carbon single bonds and strong carbon-hydrogen bonds. Generally, alkanes are unreactive. Alkanes contain only bonds of C-H and C-C that are comparatively tight and difficult to break. Molecules which are non-polar are provided by similar electronegativities of carbon and hydrogen.