/sci/ - Science & Math

the only one thats polar

>octane
>soluble in water

what the fuck?

>>3803789
This.

Dude, pyridene is the only one that's polar.
You gotta know that.

>>3803769
>Taking organic chemistry without understanding general chemistry
ISHYGDDT

Wow, I really hope I was high or drunk when I took this test, Either that or I fail at life.

it's been a while since I did HS chemistry, but I'd guess whichever is most polar or exhibits the most hydrogen bonding

>>807

This is gen. chem. not orgo.

carbon tetrachloride is a wild guess, i did organic like years ago and have never defragged my brain since.

shows the difference between learning and interest

ccl4 has polar bonds, so i assume it's the answer.
the large surface area gives it a low BOILING POINT do to the induced van der waal forces, maybe you got boiling point and solubility mixed up?

>>3803838
>the large surface area gives it a low BOILING POINT
what the fuck am i reading?

>>3803847
>large surface area
>more surface contact between molecules
>stronger van der waals forces
>lower boiling point
i don't know what the fuck you're reading.

E. its the only polar molecule. like solutes like. water is polar. the others are highly to moderately non-polar

>>3803859
>thinking more contact = lower boiling point
>2011
ISHYGDDT

Okay, everyone but >>3803784 in this thread fails at chemistry, and even his answer is only kind of correct. The correct answer is Pyridine, partially because, as was said, it's the only one that's polar (Toulene technically has a nonzero dipole moment, but it's damn close to zero so for most purposes you wouldn't call it polar anyway). The better reason is that it has a nitrogen nucleus and that can act as a hydrogen bonding acceptor, allowing it to be more effectively surrounded

Chemfag, the thing to remember in determining solubility is that "like dissolves like", so you need to find whichever solute molecule is most like your solvent. In the case of water, your top priority for this is to figure out if the compound is ionic, and if it's not, if it has hydrogen bonding donors or acceptors (remember, hydrogen bonding only works with Nitrogen, Oxygen, and Flourine) and failing that, polarity. The easiest way to determine polarity of compounds is to check for larger differences in electronegativity (basically whichever is closest to the top right of the periodic table is more electronegative with a couple exceptions and the larger the gap between them the more polar the covalent bonds). The other thing to watch out for is symmetry. A highly symmetrical molecule is not going to be very polar. This is why carbon tetrachloride is nonpolar, despite having fairly polar individual bonds, the net dipole moment of the molecule is zero. This is also how you could predict Toluene and Pyridine to be the only ones with dipole moments, as they each only have one axis of symmetry.

The answer is C. Pyridine is the only molecule there that has any potential for hydrogen bonding, being both an H-bond acceptor and donor.

It's true that Carbon Tetrachloride has polar bonds but they're all polar so that means that there is no net dipole moment. Therefor the molecule, on the whole, is not polar.

But yeah, remember guys, Hydrogen bonding is FON!!!

>>3803896

thanks, i stand corrected.

>896

Thanks for answering my question and being polite about it. If you're a chick i'd date you, If you're a guy i'd high five you.