Intermolecular forces Definition and 39 Threads

The answer is dipole-dipole and London dispersion forces, but I only chose London dispersion forces. How would you determine whether there is a large or small electronegativity difference between N and O? And therefore how would you determine whether the N-O bond is polar covalent or non polar...

I am able to find and understand T from kinetic theory, but I do not understand how to use pressure gradient per unit of area and per unit pressure gradient.

Hi all, Something I've been wondering - why don't two solid surfaces always stick together when touching each other? As far as I'm aware there are five basic types of solids: Atomic solids: Frozen noble gases containing single atoms held together by London dispersion forces. Molecular...

Homework Statement Do ionic compounds such as NaCl and K2O have intermolecular forces? 2. The attempt at a solution I got stuck conceptually. NaCl and K2O are ionic compounds. Their basic unit is formula units. They are not molecular compounds. Ionic compounds are held together by...

Hello, Let us imagine a rod resting on a frictionless horizontal surface such that the rod is made up of 2 identical molecules. Let these molecules be named A and B from left to right. If we pull A to the left and B to the right with forces of equal magnitude, the rod must remain at equilibrium...

Hello, Let us imagine a solid in a free fall on planet Earth and let us neglect the effect of air resistance on the motion of the solid. According to Newton's Second Law of Motion, since the only force being applied on the solid is its Weight, then its acceleration must be its Weight divided by...

This question might be a stretch, but I was just reading about inter- and intra-molecular forces. And I found that "Intermolecular forces (IMFs) are forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions)"...

I understand that due to the geometry of the CO2 molecule it ends up have no net dipole moment. But why doesn't the central carbon atom experience intermolecular forces from the oxygen atoms of other CO2 molecules. What I mean is why can't CO2 form an arrangement where the dipole forces still...

I've come to understand that intermolecular forces cause the boiling point of hydrochloric acid solutions below 20% to be higher than the boiling point of water. I also understand that dissolving hcl in water is an exothermic reaction. But, what about those intermolecular forces. I assume they...

So i want to understand how concepts like van der waals, electronegavity and covalent bonds were discovered, measured and derived back in the days. I'm looking for a good book to explain this. So far I've looked at a book by Jacob.Intermolecular and Surface Forces, Revised Third Edition -...

When the temperature of a fixed volume of gas increases (higher average kinetic energy), the effect of intermolecular forces becomes less prominent. That's very intuitive, but how can I understand this in terms of force, velocity, momentum and so on?

Homework Statement Estimate the energies of interaction at 25 °C between (i) two hydrogen molecules and (ii) two nitrogen molecules, if each pair is separated by 0.3 nm. Explain fully and clearly your reasoning and any assumptions you make in your answer. State the source of the values of any...

Hi! Boron trifluoride is a nonpolar molecule due to its high symmetry even though the covalent bonds within the molecule are polar. As a result, the only type of intermolecular forces in BF3 would be the London dispersion forces. I understand that these forces are exhibited by nonpolar...

For a van der Waals gas, there are London dispersion forces causing the gas particles to be attracted to each other while the law of excluded volume provides repulsive forces. How do each of these characteristics effect the pressure, volume, and temperature of the gas? I assumed that for the...

< Moderator Note -- thread moved to Homework Help forums > Shouldn't Propylamine (C3H7NH2) be able to form hydrogen bonds with alike molecules? Hexane (c6h14) doesn't seem to have hydrogen bonding capability.

Though there are other atoms with less electronegativity which can form effective attraction forces,why hydrogen is taken as a speacial case?

Hi I have a couple of questions relating to these topic hope you guys can help :) Comparing ethanol and water, ethanol has weaker intermolecular forces than water. However, it has a greater specific heat capacity by kJ/mol.K than water. Meaning more energy would have to be absorbed per mole of...

When a substance undergoes a phase change from a solid to a liquid the substance can absorb heat energy without undergoing a temperature change. But I also read that when a substance melts, the atoms absorb energy and thereby vibrate faster, overcoming the intermolecular forces. Temperature is...

Hi there. I have found the surface tension for liquid etanol on a given problem. Then the problem says: supposing that the coordination number for etanol is 12, what value does the intermolecular interaction energy has? I have ##\gamma=21,26355\frac{dyna}{cm}##, gamma is the surface tension that...

Sorry if this is an obvious question...I understand how the justification via the pressure v temp graph works, but I'm not quite understanding freezing point depression in terms of intermolecular forces and temperature. I was taught that due to attractive IMF between solute and solvent particles...

Homework Statement The question asks to list all the intermolecular forces operating in each of the two liquids. H_2O CH_3OHHomework Equations N/A The Attempt at a Solution I'm mostly getting confused about the London Dispersion Force with water, and London Dispersion Force and...

For a non-ideal gas expanding in a vacuum, the kinetic energy of each of the molecules does NOT remain consant as the gravitational effect of the other molecules would "slow down" these velocities by deceleration. What are those forces referred to? Are they "Newton" forces or what? I can't...

If I have to explain why instantaneous dipole-induced dipole attraction can be greater than permanent dipole- permanent dipole attraction, should I write : 1) It's because for larger molecules, they have higher polarizability, and therefore, so as the instantaneous dipole induced dipole...

Homework Statement This is the worksheet: http://webcache.googleusercontent.com/search?q=cache:9jyqtuswY1AJ:www.chemmybear.com/groves/apch13_imfans.doc+ap+chem+pasadena+imf%27s&cd=1&hl=en&ct=clnk&gl=us&client=firefox-a Homework Equations None, as far as I know The Attempt at a...

I am given question with a number of compounds such as He, Ne, Cl2, (CH3)2CO, O2, O3 I have to arrange it in increasing/decreasing order of their boiling points. It is related to intermolecular forces i.e London forces, dipole-dipole interactions and also deals with the concepts of...

1. Predict which two interactions are stronger than the other two. Check all that apply. [ ] Forces on the picture (a). [ ] Forces on the picture (b). [ ] Forces on the picture (c). [ ] Forces on the picture (d). http://i41.tinypic.com/3wwug.jpg 2. Which member of the following...

After a ligand bonds to a receptor through intermolecular forces, how is it unbound and what happens to it after it is?

Homework Statement I know that there are three types of Intermolecular forces but while searching on the internet I found that there are six intermolecular forces i.e. Dipole-Dipole Interaction, Hydrogen bond, London Dispersion, Ion-Dipole Interaction, Dipole-Induced Dipole Interaction and...

Hi, my question is this. Is a gas with a positive intermolecular potential like a gravity potential in a pendulum? By this I mean if you compress and the expand the gas the force goes from max potential to a minimum ,creating molecular acceleration in the process and then reverses the...

Homework Statement There are two compounds, butane and pentane. one is a liquid at at room temp and the other is gas. which is a liquid and why? Homework Equations The Attempt at a Solution I'm guessing that its pentane. For a gas to liquify, it should have a have a higher melting...

what is the strongest intermolecular force, dipole-dipole, london dispersion, or hydrogen bonding. also, how do you know if a molecule is dipole-dipole, london dispersion, or dydrogen?

I am really confused in my advanced chemistry class. We are currently doing intermolecular and intramolecular forces. For example, a book problem that has me frustrated is : "What is the strongest interaction between hexane and iodine?" What's the difference between "dipole-dipole" and...

I tried posting a similar question before, however, I've found the 1 reply is actually wrong. Hopefully with better illustrations, someone will know. The situation in the picture is a drop of water entering a capillary tube. It is located here...

Hi, I need some help with my homework. I have three questions which I'm not quite sure which answer it is, though I give it my best try. If anyone can help, it'll be much appreciated. Thanks in advance... Question One: Which of the following substances will have hydrogen bonds between...

My chemistry textbook states the following: "In general, larger molecules tend to have greater polarizabilities because they have a greater number of electrons and their electrons are farther from the nuclei. The strength of the dispersion forces, therefore, tends to increase with increasing...

Hi everyone. I have recently just started studying chemistry for my Junior year in High School. So you could say that I am a newbie at this. :smile: I have small knowledge on the relationship between Intermolecular Forces and Physical changes. (Example: Boiling Point.) So if the IMF of a...

I have been trying to get my head around this question, but do not understand it. Consider the two isoelectronic substances, bromine (Br2) and Iodine monochloride (ICl). Based upon your knowledge of intermolecular forces, explain the difference in their boilings pts. (Bromine: 59 degrees C...

Why the boiling point of HBr will smaller than the Cl2 ? Since the relative molecular mass of HBr is bigger than Cl2 , so the temporary dipole induced dipole forces should be bigger . Thus , the boiling point of HBr should be bigger .

For the compounds I to VII pick the letter that corresponds to the correct interactions between particles of that particular compound. If more than one type of interaction exists for a compound, pick the letter that corresponds to the strongest interaction. a) Ion-Ion b)...