Intermolecular Forces

Okay, so let's talk about

intermolecular

forces

. You may have also heard that like imfs that is the attraction between two or more molecules, I hope you don't get confused with

intermolecular

forces

so it's an easy way like you. Think about when you think about the Internet being like the Internet is how you interact with other people around the world, but if you have an intranet, I don't know if your school or your job, maybe your job has something called an intranet. just within that particular school or within that particular job, it's not that you can't communicate with people everywhere, so there are differences between intermolecular forces and intermolecular forces, so the intermolecular forces with which You may be familiar with ionic bonds in molecular forces. the C and Anthion attract each other, hot bonds are also internal molecular forces, they are actually the bonds between which they share valence electrons, hot bonds are actually internal molecular forces and lastly they are metallic forces. the metal Cal and the mobile um electrons flow between the cations the sea of ​​electrons those three are intermolecular forces they are within a compound um intermolecular forces are between one compound and another compound so let's talk about those types, okay, so there are three imfs main um the first one is called hydrogen bonds this is misleading because hydrogen bonds are not really bonds they are not bonds but they are called bonds because they are very strong compared to the rest of them these guys are really strong.

You may have noticed that they are called H-bonds and what they are is when a hydrogen atom in one molecule is attracted to a highly electronegative atom in another molecule. The highly electronegative atoms I'm talking about are F Florine, oxygen and nitrogen, um, these are the only ones that hydrogen can bond to to form hydrogen bonds, so for example, what I mean by that, let me take a pen. What I mean by that is let's take water for example, this is what water looks like and it's a water molecule and another water molecule, these are the hot bonds, not the IMF, okay, these are the hot bonds inside of the water molecule, okay, and we know that oxygen is much more electronegative than hydrogen, so the electrons are going to flow much more around the oxygen atom than around the hydrogen atom, so this will be slightly negative, we'll denote it with a Delta with a negative charge and these guys will be slightly positive, the same goes for This electron is going to flow into the oxygen making this slightly positive and this slightly negative, and we know that negative and positive charges attract each other. yeah, so we're going to have a very strong attraction here, this is our H link, okay, this guy.

It is responsible for the boiling point of water being quite high, it is responsible for how things freeze and the way the crystal structure is, it is responsible for many things within water that make water water, this hydrogen bond is is quite important and is quite strong is very strong High attraction a mod one water molecule to another um another type of IMF is dipole dipole this is when the attraction between regions with opposite charges of a polar molecule now let's not forget that In a polar bond we have one that is a highly electronegative atom bonded to another non-electronegative atom not chosen, so it is not as electronegative as Florine's oxygen and nitrogen, but it is pretty close, so the electrons here will flow towards chlorine.

Okay, make this positive and negative, the same thing happens here. making this positive and this negative and again we know that negative and positive attract each other very similar to hydrogen bonding, but these guys are much more different in electronegativity values ​​than these guys, this is not as strong, so this guy here is the dipole dipole interaction Okay, so these guys are the strongest and these guys are strong, but not that strong. Well, the last one is the London scatter. All you might have known is that, like Vanderwell forces, it's an induced dipole, that might be something you've heard before. dipole when something is induced we force it to be a certain way so it is called an induced dipole between two non-polar molecules so here is the nitrogen which is the non-polar electrons will be shared equally between this nitrogen as they are in this nitrogen, no matter how we do it.

I know that electrons are constantly moving, they are always in motion, so at some points, sometimes electrons will be here at some certain time, so let's just do this for a second, this could be slightly negative and this could be slightly positive, which then induces this molecule to say electron. I don't like being close to another electron, so this guy will flow over here, making this guy positive and this guy negative, creating an attraction here, here's the induced, we induce this one to actually change so here's the induced dipole this is very, very weak because the electrons are constantly moving this will break and the electrons will flow back here because we know this is non-polar there is no reason for it to be here versus here these are non-polar electrons they are going to be shared by same, so they will break, so they are very, very weak, the things that have, that are not polar, are typically gases, because they are, they won't be, it will take a lot of effort. any energy actually to turn them into gases because these electrons are.

Sorry this link is very very weak and the attraction is very very weak so they will be everywhere so they are usually gases then liquids and these are usually solids at room temperature um because of these imfs so um that's basically imfs