<p>i dont think the curve changes on the SAT subject tests</p>
<p>mr.fool...i would say the resistances of metal materials generally decrease as temperature increases...superconductor, which works at low temperature, is merely an exception...</p>
<p>I don't really know, as I'm not too good with this kind of stuff... but here's a site that (I think) kinda supports my claim:
<a href="http://hyperphysics.phy-astr.gsu.edu/hbase/electric/restmp.html%5B/url%5D">http://hyperphysics.phy-astr.gsu.edu/hbase/electric/restmp.html</a></p>
<p>One of the first things I learned about semiconductors and conductors was that
semiconductor is more conductive at higher temperature since the "forbidden zones" between the valence band and the conduction band become more narrow so that electrons are able to move from one to the other easier.
However, for a conductor, increasing the temperature only tends to hinder the flow of electrons as the conduction band and the valence bands of the conductor are already touching.</p>
<p>The curve is usually ten questions, or so I've heard.</p>
<p>I'm almost positive that question talked about conductivity after dissolved in water. And aren't metals more malleable... so not brittle?</p>
<p>Im almost positive that the question said after dissolved in water also.</p>
<p>I'm pretty sure it said dissolved in water.
I'm also pretty sure I did horrendously. :eek:</p>
<p>It's ionic because in the princeton review book, they list the properties and also because it said "molten" conducts electricity and that goes with ionic bonds.</p>
<p>dang, another one bites the dust...</p>
<p>what about the one where they had 4 roman numerals and all the answer choices had 2 roman numerals. what was the answer, does anyone remeber putting I and IV. </p>
<p>I am sorry I don't remember the question, this is the only part that I do remember:(</p>
<p>i remember picking I and IV</p>
<p>yeah me too</p>
<p>You guys (or girls) are now my heroes. I thought I got that wrong because I forgot the question, but I guess I didn't get it wrong. Yes, Yes, woohoo! :)</p>
<p>so what was the nitrogen/london dispersion forces question?</p>
<p>What bonds does dinitrogen exhibit between each other?
LD Force I believe was the answer.</p>
<p>yeah it was...</p>
<ol>
<li>S stronger oxidizing agent than Cl- BECAUSE sulfur has more electrons that chlorine (F/F)</li>
</ol>
<p>I don't remember, but if that's definitely Cl- (ion) then it should be T/F. Chlorine is definitely more electronegative than sulfur and thus is a better oxidizing agent (likes to take electrons); however, <em>chloride</em> is not a very good reducing or oxidizing agent, since it already has a full valence shell. Sulfur does not have a full valence shell, and would be a far stronger oxidizing agent than chloride.</p>
<p>It was chlorine, I'm 99% sure...what exactly was the nitrogen/london dispersion question?</p>
<p>I think it was asking what type of bond N2 had. I put London dispersion forces</p>
<p>are you sure it said what <em>type of bond</em>? because idon't think ldf is a kind of bond between atoms. waht were the other choices again? I think i might have put something else</p>