<p>o.O? I thought hydrogen bonds were the STRONGEST; however, the book says hydrogen bonds are the weakest? Clarification please.</p>
<p>And also, could some clarify this:</p>
<p>Why does a linear structure result from minimum repulsion between two electron pairs in a molecular compound?</p>
<p>And, why: VSEPR model says like charges will orient themselves so as to diminish the repulsion between them
^^^^ I thought that like charges will increase repulsion?</p>
<p>Hydrogen bonds are stronger than dipole-dipole and london dispersion, but otherwise pretty weak. By your reasoning, and according to that question, water would have a higher boiling point than solid iron!</p>
<p>The same charges ALWAYS avoid each other. Therefore they align as far away from each other as possible. FOr two charges, this is linear.</p>
<p>I'm pretty sure that it's London Dispersion < dipole-dipole < Hydrogen < Metallic < Ionic < covalent < polar covalent. I'm not sure about metals and ions, but I don't think you'll ever be tested on the differences between those two on the SAT or AP tests. But covalent bonds are definetley the strongest (diamonds are basically just one really big molecule with a whole bunch of carbon atoms, and sand, which I think is SiO2 is also the same thing with silicon and oxygen both have ridiculous melting points).</p>
<p>Covalent Network bonds are the bonds in C (diamond), and SiO2. </p>
<p>London Dispersion and Dipole-Dipole and H-Bonding are intermolecular attractions. These intermolecular attractions are WAY lower than the bonding that occurs BETWEEN atoms. </p>
<p>I'm not sure if ionic bonding is stronger than metallic bonding though. Lattice energies differenciante heavily due to charge and electronegativity.</p>
<p>Intermolecular forces are not bonds between atoms.</p>
<p>Covalent bonds can be seen in stuff like methane. The bonds in methane are weaker than the bonds in stuff like NaCl and HCl. Covalent Network bonds are like diamonds and SiO2. Those are really strong.</p>
<p>Yes, don't confuse the difference between bonds and intermolecular forces. And my bad about polar covalent vs covalent. I forgot which one was stronger :P </p>
<p>But here's an easy way to remember bonds:</p>
<p>Covalent is the weakest, because there is a very small EN difference, so not as much force holding them together. Polar covalent is stronger, because there is a higher EN difference and therefore more force. And Ionic is basically such a big EN difference that the electrons are nearly transferred, so it's stronger. And then you have the network covalent, which is the strongest (diamond).</p>
<p>As far as metallic and ionic, I'm not totally sure but I still think metallic is higher (?). I actually think though that there isn't a general rule that governs the difference between the two, and I doubt you'll be tested on it.</p>
<p>None of these are right. Bond strength and EN difference are two different issues. Rather than weight in with another opinion, I am going to suggest something radical: Check a textbook!</p>
<p>There are several contributing factors but usually the most important is the difference in the electronegativity of the two atoms bonding together."</p>