<p>HCl is polar and linear.</p>
<p>thats so false…there are millions of molecules in the world that are nonpolar and not linear…shape has NOTHING to do with polarity of a molecule…h-cl…h-c-n…both lilnear and polar</p>
<p>why would III not be true? Cooling the solution would cause the reverse reaction to be favored; the aqueous ions would precipitate again.</p>
<p>ALSO- the polarity of a molecule is depending upon the spread of molecular charge and the electronegativity of the atoms involved.</p>
<p>Right, I forgot about those molecules. I still think it is CE. The diatomic molecules are nonpolar because of the linear structure, otherwise, the dipoles won’t cancel out.</p>
<p>@hffighter
But if you are asked to explain why a molecule is non-polar it is not enough to say it is linear. Diatomic doesn’t require they are the same atom, someone posted a link about this earlier. I feel like this is going to be hard to decide either way when we don’t have the exact wording though.</p>
<p>I had 5 TTCEs.
Not many FF, I think.</p>
<p>For the hydrogen one I guessed.
Is the P vs. V graph curved or linear?!</p>
<p>what were the lab equipment quetsions again?</p>
<p>P vs. V would be curved. I think the graph was E, specifically. Whichever one was the hyperbola (it’s inversely related)</p>
<p>P vs V graph was an isotherm so it has to be curved…</p>
<p>@hffighter…ur making an ok point but think about the fact the all x2 molecules are linear…so it was a true statement but that isnt wut is explaining the nonpolarity in the molecule so it cant be CE for the fact that there is such thing as polar linear…aka there is an exception…for example there is no exception that an increased average kinetic energy is due to increasing temperature</p>
<p>**** i put linear, i now see why its curved</p>
<p>what score is 3 wrong?</p>
<p>
</p>
<p>(As far as I know,) Le Chatelier’s Principle only applies to reactions that can proceed appreciably both forward and backward, which is represented with the double arrow. The KCl equation only had the forward arrow; Le Chatelier’s Principle does not apply.</p>
<p>As for the diatomic thing, I think that the first step to a molecule possibly becoming polar is the presence of polar bonds. No polar bonds are present in a diatomic molecule (since it’s the same atom bonded to itself).</p>
<p>what do you think 1 omit and 3 wrong will be</p>
<p>What about the hydrogen absorbing certain wavelengths and if hydrogen has quantized energy levels.</p>
<p>Well, even if the equation didn’t show it, the problem stated that the solution had reached equilibrium…I think that might have been an error not putting the equilibrium sign on the equation</p>
<p>@314159265
Are you sure there was only a forward arrow? Because it said something like “when the reaction reaches equilibrium, which is correct?”, so wouldn’t Le Chatelier’s apply?</p>
<p>3 wrong and 1 omit is 800 for sure…i put T T CE for the hydrogen absorbing certain wavelengths</p>
<p>also it wasnt a le chatlier stress because no equilibrium and last time i checked dissolving doesnt increase when the solution is cooled</p>
<p>^I remember looking at the equation, seeing the enthalpy, seeing only a forward arrow, looking at choice III, and thinking to myself, “I got tricked on the APUSH MC yesterday; I’m not going to get tricked by a CB test writer again.”</p>
<p>So yeah, I’m sure there was only a forward arrow, which makes sense, since KCl is highly soluble.</p>