Which statement best describes a limitation of the kinetic molecular theory for a gas?
A limitation of the kinetic-molecular theory for a gas is the theory assumes that particles do not experience intermolecular forces. This cannot be completely true since interactions between particles is normal.
Which would you expect to have the higher melting point C8H18 or C4H10?
C8H18 would have the higher melting/boiling point. C4H10 is smaller, that’s why it has fewer sites available for London forces to form.
Which substance would you expect to have the highest melting point?
2 Answers By Expert Tutors. You might expect MgCl2 (an ionic compound) to have the highest melting point.
What IMF has the highest boiling point?
Compounds I and IV would be higher boiling point compounds because of additional hydrogen bonding (strong intermolecular forces). Compound IV would be the highest boiling because the hydroxy group and carboxylic acid group could BOTH participate in intermolecular hydrogen bonding.
Which has a higher boiling point C2H6 or C4H10?
C2H6 < C3H8 < C4H10. All of these compounds are nonpolar and only have London dispersion forces: the larger the molecule, the larger the dispersion forces and the higher the boiling point. CO has the highest boiling point. CO and N2 both have LDF, but N2 is non polar so it only has LDF.
Which of the following interactions are the strongest?
ANSWER: The strongest among the given interactions is ionic interactions.
What is the relationship between boiling point and IMFs?
Intermolecular forces (IMFs) can be used to predict relative boiling points. The stronger the IMFs, the lower the vapor pressure of the substance and the higher the boiling point. Therefore, we can compare the relative strengths of the IMFs of the compounds to predict their relative boiling points.
Why does intramolecular hydrogen bonding decreases boiling point?
Intramolecular hydrogen bonding occurs in two atoms of same molecule. It decreases the melting and boiling point because of chelation. Formation of chelation reduces the possibility of intermolecular hydrogen bonding and thus prevents association of the molecules which would have raised the melting or boiling point.
What is the relationship between hydrogen bonding and boiling point?
In water because of the hydrogen bonding attraction between molecules greater energy is needed to separate them from against their inter molecular attraction, therefore higher boiling point.
Does intramolecular affect melting point?
A solid’s molecules hold each other in a rigid, ordered structure called a lattice, while a liquid’s molecules have weaker interactions and move around. Heating a solid transfers energy to the molecules. The stronger the intermolecular forces are, the more energy is required, so the higher the melting point is.
What is the effect of hydrogen bonding on boiling point?
Molecules with hydrogen bonds will always have higher boiling points than similarly sized molecules which don’t have an an -O-H or an -N-H group. The hydrogen bonding makes the molecules “stickier,” such that more heat (energy) is required to separate them.
Which type of hydrogen bond is stronger?
Third, water has a higher boiling point than HF, yet fluorine is more electronegative than oxygen, it is also smaller, and so you would expect the HF hydrogen bond to be stronger than the OH hydrogen bond.
What is the weakest intermolecular force?
London dispersion force
Is Covalent stronger than metallic?
Covalent bond means overlapping of two electron clouds. So, in metallic bond there is actually no overlapping between any two atoms. So , we can conclude that a covalent bond is more stronger than a metallic bond.