Now before we can talk about dipole moments, we have to take a look at electronegativity. We're going to say it's the measurement of an element's ability to attract electrons to itself. So basically, the higher electronegativity value an element has, the more it desires electrons near it. We're going to say in 1932, it was the American chemist, Linus Pauling, who proposed electronegativity values for the elements. I thought this was good to include because at this point we've heard a lot about chemists from Germany, from Russia, and from France. We don't usually hear too much about old school chemists from the US. Here, we're going to say that the periodic trend of electronegativity is as we're moving from left to right across a period and going up a group, our electronegativity should increase. So electronegativity increases in this movement. And we're going to say as we head towards the top right, basically, our electronegativity is increasing. Now remember, we said that electronegativity is the element's ability to attract electrons to itself. The noble gases are perfect. They don't really want electrons. Of course, there are exceptions to this in the form of Krypton and Xenon. They exist in the sweet spot of group 8A where they could potentially accommodate additional electrons to themselves to help make different types of Lewis dot structures. But what's most important in this description is that fluorine is the most electronegative. An easy way to remember that is in college, we're all looking for that perfect 4.0 GPA. Fluorine is 4.0 in terms of electronegativity. So as we head towards fluorine, things become more and more electronegative. Alright, so this is the basic trend that you need to keep in mind when talking about electronegativity as a periodic trend.