<p>From Barrons 2007 8th ed. (pg 6)</p>
<p>Why is there a significant difference in the boiling point of H2S and H20?</p>
<p>Is it because H20 is the hardcore bonds of bonds b/c its water?</p>
<p>If this problem was not compared to water but H2Se o.O? Would there be a significant difference in boiling point?</p>
<p>Not exactly sure what a hardcore bond is, but when hydrogen is bonded to any of these: NOF, then there is a strong hydrogen bond. Sulfur w/ hydrogen doesnt create a hydrogen bond. Due to the stronger intermolecular forces, H20 has a higher boiling point.</p>
<p>thanks dr.crocodile.</p>
<p>Just an FYI: hydrogen bonds (an intermolecular force) are created between bonds of between hydrogen and one of the following: fluoride, oxygen, or nitrogen (FON, like phone.) That's how I remember it. :)</p>
<p>oo. thats good. I'll try to remember that.</p>
<p>you could also try to remember it like i do: H-bonds are between hydrogen and the three atoms with the highest EN</p>
<p>you both are good. I'll incorporate both tips. THank you. Now I have other questions that need to be answered =].</p>