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My report on "Intermolecular Attractions"
My report on "Intermolecular Attractions"
Student name: Tony Do
Teacher name: Mrs. Luquire
School: DFA
Submission Time: 11/13/14 2:31 AM
Page 1 : http://mw2.concord.org/public/part2/vdw/page1.cml
1. What is the difference between polar and non-polar molecules? (Be sure to include more than the colors used to represent them in your response!)
Polar molecules have oppositely charged ends, and have stronger charged bonds because one negative end can bond with another positive end; Non-polar molecules do not have clearly indiciated charged ends and there bond are only instaneous dipole-dipole attractions that are not consistent. (1:45:58 AM)
2. Image showing intermolecular attractions:
polar molecules are limited to a lot less bonds than non-polar molecules because they have uneven ends; non-polar molecules are not limited to this, so they can bond with both a positive and negative end of a polay molecule (2:08:14 AM)
3. Which of the following formed intermolecular attractions (check all that apply):
(a) + ends of polar molecules to + ends of other polar molecules
(b) + ends of polar molecules to - ends of other polar molecules
(c) - ends of polar molecules to - ends of other polar molecules
(d) non-polar molecules to other non-polar molecules
(e) non-polar molecules to + parts of polar molecules
(f) non-polar molecules to - parts of polar molecules
My answer is (b) (d) (e) (f) (1:47:02 AM)
Page 2 : http://mw2.concord.org/public/part2/vdw/page2.cml
1. What is the primary attraction between NON-POLAR molecules:
(a) London Dispersion attraction
(b) dipole-dipole attraction
(c) gravitational attraction
(d) magnetic attraction
My answer is (a) (1:49:39 AM)
2. What is the primary attraction between POLAR molecules:
(a) London Dispersion attraction
(b) dipole-dipole attraction
(c) gravitational attraction
(d) magnetic attraction
My answer is (b) (1:50:06 AM)
3. Which type of intermolecular attraction is strongest:
(a) London Dispersion attraction
(b) dipole-dipole attraction
(c) gravitational attraction
(d) magnetic attraction
My answer is (b) (1:50:23 AM)
Page 3 : http://mw2.concord.org/public/part2/vdw/page3.cml
1. Which liquid boiled first (i.e. had the lowest boiling point):
(a) The polar liquid boiled first.
(b) The non-polar liquid boiled first.
(c) They both boiled at the same time.
My answer is (b) (1:53:23 AM)
2. Explain how intermolecular attractions affect the boilng point of a substance.
The weaker the intermolecular attractions the easier it is to boil it creating a low boiling point. (1:53:23 AM)
3. Explain why polar and non-polar substances won't stay mixed with each other.
Because the attractions between polar/polar is stronger than polar/non-polar and there is a trend for the polar molecule to bond with the stronger attractions. (1:57:24 AM)
Page 4 : http://mw2.concord.org/public/part2/vdw/page4.cml
1. Which molecule had the strongest attraction:
(a) the least polar molecule
(b) the medium polarity molecule
(c) the most polar molecule
My answer is (c) (1:59:01 AM)
2. Explain why polarity has an affect on the strength of attraction between molecules.
The negative or positive charged ends are able to attract their opposite with a strong bond. (2:00:28 AM)
3. Which substance will have the highest boiling point:
(a) 1-heptanol
(b) 1,7-heptanediol
(c) 1,4,7-heptanetriol
My answer is (c) (2:01:22 AM)
4. Explain your choice for highest boiling point:
It is the one with the most amount of negative/ postive ends, so that means its the most polar (2:02:07 AM)
Page 5 : http://mw2.concord.org/public/part2/vdw/page5.cml
1. Which molecule pairs had the strongest attraction (check all that apply):
(a) the two small molecules
(b) the two large straight molecules
(c) the large straight and bent molecules
(d) the large straight and circular molecules
(e) the large curved and circular molecules
My answer is (b) (e) (2:03:34 AM)
2. Propane boils at -42°C, butane at 0°C, and pentane at 36°C. They are all straight molecules. Which one is the biggest?
(a) propane
(b) butane
(c) pentane
My answer is (c) (2:03:55 AM)
3. Small molecules did not attract well. However, only some of the large ones had a strong attraction. Describe how both size and shape play a role in the strength of the London Dispersion attraction.
The London Dispersion attraction will be weaker if the shape restricts the possibility of bonds. The larger the molecule the more amount of attractions occurs. (2:06:21 AM)
Page 6 : http://mw2.concord.org/public/part2/vdw/page6.cml
1. Snapshot with annotations indicating hydrogen bonds:
The molecules have strong attractions because they are hydrogen bonds (2:11:40 AM)
2. While not possible, imagine that water molecules had no attraction for each other at all. Would you most likely find water as a solid, liquid, or gas? Explain your reasoning.
Gas, because since their strong hydrogen bonds are not present, they will disassociate a lot easier. (2:12:46 AM)
Page 7 : http://mw2.concord.org/public/part2/vdw/page7.cml
1. Which pair of bases is held together more strongly: C and G, or A and T? How do you know?
C/G because there is two hydrogen bonds occuring (2:15:14 AM)
Page 8 : http://mw2.concord.org/public/part2/vdw/page8.cml
1. Image of the 3D anitibody/antigen from top of page:
(2:23:38 AM)
2. Image of the anitbody you just designed:
(2:23:40 AM)
Page 9 : http://mw2.concord.org/public/part2/vdw/page9.cml
1. Why do you think a gecko's feet stick much better to a wall than your fingers? Think about surface area, intermolecular attractions, and the rough surface (on a microscopic level) of a typical wall.
Because there are tiny hairs on a gecko's feet, there is a lot more surface area causing more possibilities for intermolecular attractions to occur. (2:28:16 AM)
Page 10 : http://mw2.concord.org/public/part2/vdw/page10.cml
1. Which of the following is NOT an attractive force between molecules:
(a) London dispersion
(b) dipole-dipole
(c) covalent bond
(d) hydrogen bond
My answer is (c) (2:25:19 AM)
2. Which factors affect the strength of the intermolecular attractions? (check all that apply)
(a) the color of the molecules
(b) the polarity of the molecules
(c) the shape of the molecules
(d) the size of the molecules
My answer is (a) (2:25:29 AM)
3. You have two substances: A and B. Both have molecules of similar size and shape. Substance A has molecules that attract with London dispersion attraction, and substance B has molecules that attract with dipole-dipole attraction. Which one will have the higher boiling point?
(a) Substance A
(b) Substance B
My answer is (b) (2:25:50 AM)
4. Explain why you chose Substance A or B.
Dipole attractions are a lot stronger than London dispersion; the stronger the attractions, the higher the boiling point. (2:26:43 AM)
5. You have two substances, both of which have the same boiling point (or attraction between their molecules). The first substance is made from molecules that are small (just a few atoms bonded together), and the second substance is made from molecules that are larger (many atoms bonded together). How can it be possible for two such different molecules to yield substances with the same boiling point? Describe the kinds of intermolecular attractions that must be involved and any other properties of the molecules that could cause this result.
The larger the amount of molecules, the more bonds occuring which would increase the strength of attractions. This must mean that either the shape is more favorable to the small molecule, the second substance is a non-polar molecule, and/or the first substance is polar. (2:31:24 AM)
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