A community for students.
Here's the question you clicked on:
 0 viewing
vera_ewing
 one year ago
Which of the following illustrates an everydaylife example of how London forces are induced?
A. The attraction of a magnet with a metal object
B. The attraction of your hair to a balloon after the balloon is rubbed against it
C. The attraction between sodium and chloride in table salt
D. The attraction of an object to Earth through gravity
vera_ewing
 one year ago
Which of the following illustrates an everydaylife example of how London forces are induced? A. The attraction of a magnet with a metal object B. The attraction of your hair to a balloon after the balloon is rubbed against it C. The attraction between sodium and chloride in table salt D. The attraction of an object to Earth through gravity

This Question is Closed

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0which do u think it is @vera_ewing

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2I feel like you asked this question before or someone did. I also remember that no one could figure out an answer for it as none of them make any firm sense.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2Oh i found it http://openstudy.com/study#/updates/5571da24e4b0edc5dbb7fc68

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2London Dispersion forces from what I remember is when electrons become to close to each other and end up repelling. This in turn induces an attraction between molecules.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Correct answer is B. The attraction of your hair to a balloon after the balloon is rubbed against it

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2Alright I feel like you would have to have some underlying knowledge of some areas of physics to answer that...

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0How does entropy change when an ionic solid dissolves in water? A. The entropy can only decrease since the system becomes more disordered. B. The entropy can only increase since the system becomes more disordered. C. The entropy typically increases since the crystal lattice and the ordered water become less ordered, but it can decrease if the hydrated ions become more ordered. D. The entropy typically decreases since the crystal lattice and the ordered water become less ordered, but it can increase if the hydrated ions become more ordered.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2C. makes sense as the first statement is true and the second statement is true if a non polar compound is dissolved the entropy will actually decrease as the hydrated ions become more ordered. Then again the question is asking specifically about ionic solids dissolving. That leaves B a possibility.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2Things that will affect boiling point are the mass of the substance and usually what kind of forces are acting on the substance.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2The higher the mass the higher the boiling point and the stronger the forces acting on the substance the higher the boiling point.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0So which one do you think it is?

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2I think it might be D,B,C,A

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2D has the highest molar mass and experiences hydrogen bonding, B has hydrogen bonding, c has a higer molar mass than A, and A is nonpolar experiencing only weak intermolecular forces with low mass

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0If a balloon is filled with helium and has a volume of 1.56 L at 25°C, what will happen to the balloon if it is placed in a refrigerator at 4°C? (Assume the pressure remains constant.) A. The volume of the balloon will decrease by 1.45 L. B. The volume of the balloon will decrease by 1.31 L. C. The volume of the balloon will decrease by 0.110 L. D. The volume of the balloon will increase by 0.118 L.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2convert to kelvins first

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2so 1.56L/298K= XL/274K then you can solve for X which will give you a value in Liters

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2this is using the equation of V1/T1=V2/T2

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2anyways because the temperature decreased we know that the volume of the gas will decrease as well as the root mean square speed of the gas is smaller our answer becomes 1.45L

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2I should have done 1.561.45 = .110

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2it asked how much did it decrease by. My bad...

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0:) It's okay. If a gas tends to exhibit ideal gas behavior under certain laboratory conditions, which statement best describes the gas at these conditions? A. It contains few covalent bonds. B. It experiences a large number of intermolecular interactions. C. It contains many covalent bonds. D. It experiences few intermolecular interactions.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2ideal gas behaviour will usually have gases experiencing few intermolecular interactions

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Ideal gas is the one that has few attractive forces in the molecules, has high and constant kinetic energy and they behave as small spheres. Therefore, I would go for D.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Nice, thanks @Hoslos

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0The trick was that, it cannot be A, which would be your answer @sweetburger , because if for instance you have nitrogen molecules in a container, they are full of covalent bonds between every 2 N atoms. The interaction between these is what is scarce.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Ohh. Okay thank you @Hoslos ! How about this one?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0An organic compound with a large chain, rather than a branched one has a higher boilinh point. Thus, C.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0C. A is the answer or D. C ?

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2@Hoslos My answer to the previous question was also D. as I said "ideal gas behaviour will usually have gases experiencing few intermolecular interactions" which is the exact wording of D. I was just complementing on how well you explained it :)

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0@Hoslos Is it C. A or D. C ?

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Which of the following would cause a gas to deviate most significantly from ideal behavior? A. Metallic bonds B. Non polar bonds C. Hydrogen bonds D. London forces

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Oh, no problem @sweetburger !

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2if you ever see a metal in a gaseous state its probably pretty hot lol

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Which molecule has the strongest intermolecular forces? A. HOCH2CHOHCHOHCH2OH B. CH3CH2CH2OH C. CH3CH2CH2CH3 D. HOCH2CH2CH2OH

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2I think A. looks like it has the most OH bonds which would correspond with the most hydrogen bonding sites on the molecule

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Correct @sweetburger .

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Last one! Two atoms with charges of +1 and 1 are separated by a distance of 0.5 angstroms. What would happen to the lattice energy between ions if the distance increases to 2 angstroms? A. The lattice energy decreases by a factor of 16. B. The lattice energy decreases by a factor of 4. C. The lattice energy increases by a factor of 4. D. The lattice energy increases by a factor of 16.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2Im not sure if this a application of Coloumbs Law, but I am thinking it is.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0@Hoslos What do you think the answer is?

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2F=k(q1)(q2)/r so if The distance is increasing between the molecules then the radius would become larger which would in turn decrease the lattice energy by what I am assuming is a factor of 4

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2I am not completely sure somewhat might want to confirm or have another idea.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2I do know from this application though that the lattice energy/ energy of attraction would decrease with a larger radius so it probably will not be C. or D.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0@chmvijay What do you think?

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2You could look at this from another stand point Lets say this isnt 2 different atoms and say its the earth and the sun The earth and the sun have set force of attraction between themselves. If you distance between each other became increased the force of attraction between the earth and the sun would become smaller. I remember learning this in Physics as a source.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2If you increase the distance between the earth and the sun the force of attraction between the earth and the sun would become smaller.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0So @sweetburger the answer is B?

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0The lattice energy decreases by a factor of 4.

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0apply by born lande equation

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0ok let me check out again

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.24/.25=16 the coloumbs equation is r^2 in the bottom which of course i forgot to add

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0coulombs equation wont apply for lattice energy

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2Oh yea this should be the BornLande equation, but I am not sure how this works out.

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0its inversely proportion to Distance and not the square of it that is so its 4 and not 16

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0The formula of attraction of ions based from their relative distance is given by\[F=\frac{ q _{1}*q _{2} }{ r ^{2} }\] Given the charges and distances of them, we find the first answer, which is \[F=\frac{ +1*1 }{ (0.5*10^{10})^{2} }=4*10^{20}\] Let us assume that energy can be like that of kinetic, Ke=Fv and that v or velocity is constant. The other case is \[F=\frac{ 1*1 }{ (2*10^{10})^{2} }=2.5*10^{19}\] Finding the ratio between them , will be \[(\frac{ 2.5*10^{19} }{ 4*10^{20} })^{1}=0.062^{1}=16\] This is how I take it. Therefore, the answer shall be A.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Yep, that's correct @Hoslos :) Thank you!

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0My pleasure. Nice question though.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2Nice job @Hoslos :)

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0For columbs law we see that F = kQ1Q2/r^2 where r is the distance between the two charges. If we look at the formula we can see that the force is inversely proportional 1/r^2. If you increase the distance r between two charges the force should go down by a factor of 1/r^2

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Thanks @sweetburger !

rvc
 one year ago
Best ResponseYou've already chosen the best response.0good job @sweetburger @Hoslos :)

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.2These are all based off the equation that F=(k)(m1)(m2)/(r)^2 which appears to have many applications in which k is a specific constant and m1 and m2 are 2 objects/charges and r will always be the distance between them. This allows for a force of attraction to be found between objects/charges.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0If you look at columbs law you see that F is inversely proportional to 1/r^2 The distance goes up by a factor of 4 So 1/(4)^2 = 16 the force decreases by a factor of 16 when the distance goes up by a facto of 4.
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.