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My report on "Intermolecular Attractions"
My report on "Intermolecular Attractions"
Student name: Aaron Meller
Teacher name: Dr. K
School: BMC
Submission Time: 6/29/15 10:47 AM
Page 1 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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 a net dipole moment, whereas non-polar molecules do not. Polalrity greatly affects intermolecular interaction. (10:14:32 AM)
2. 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 a net dipole moment, whereas nonpolar molecules have a net zero dipole moment. (9:34:35 AM)
3. Image showing intermolecular attractions:
1- 2 non-polar molecules
2- 2 polar molecules
3- non-polar and polar molecule (10:47:23 AM)
4. 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) (10:15:26 AM)
5. Image showing intermolecular attractions:
2 polar molecules (9:43:14 AM)
6. 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) (9:37:48 AM)
Page 2 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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) (9:48:00 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) (9:48:06 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) (9:48:09 AM)
Page 3 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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) (9:51:22 AM)
2. Explain how intermolecular attractions affect the boilng point of a substance.
Stronger intermoleclar forces raise the boiling point of a substance - more thermal enery is needed to break polar bonds than london dispersion forces. (9:53:00 AM)
3. Explain why polar and non-polar substances won't stay mixed with each other.
The stronger dipole-dipole forces in the polar water molecules cause the water molecules to bond more to each other and clump together. The weaker lond-dispoersion forces of the oil molecules are forced to the sides. (9:55:00 AM)
Page 4 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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) (9:58:12 AM)
2. Explain why polarity has an affect on the strength of attraction between molecules.
Strength of attraction is directly proportional to the quantity of charge. More polar molecules have greater magnitude of charge (9:59:29 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) (10:00:23 AM)
4. Explain your choice for highest boiling point:
It is the most polar molecule, containing 3 O atoms. (10:00:42 AM)
Page 5 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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) (10:05:16 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) (10:11:30 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.
Size factors in the quantity of charge. Shape factors in how much of that charge quantity bonds. (10:12:17 AM)
Page 6 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\part2\vdw\page6.cml
1. Snapshot with annotations indicating hydrogen bonds:
Currently in a liquid phase - many hydrogen bonds between water molecules (10:22:35 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.
If no attraction- most likely find water as a gas - because there would be less intermolecular force keeping molecules close together in a liquid phase. (10:23:32 AM)
Page 7 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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?
G & C; they have 3 hydrogen bonds, whereas A & T have just 2. (10:25:51 AM)
Page 8 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\part2\vdw\page8.cml
1. Image of the 3D anitibody/antigen from top of page:
The antigen fits snugly into the antibody because of numerous hydrogen bonds (10:32:37 AM)
2. Image of the anitbody you just designed:
Has complementary dipole-dipole attraction, london dispersion forces, as well as the most complementary geometry to maximize bond creation. (10:32:31 AM)
Page 9 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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.
Gecko's feet have greater surface area than human hands, and can create more intermolecular force attractions with other objects than a human's (10:35:17 AM)
Page 10 : C:\Users\menachem\Downloads\cd\cd\CC-MW-CD\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) (10:39:24 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 (b) (c) (d) (10:39:36 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) (10:39:50 AM)
4. Explain why you chose Substance A or B.
dipole-dipole interactions are stronger than london-dispersion, so more energy will be required to break them (=higher boiling point). (10:40:33 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 size of the molecules is just one factor which affects the boiling point - don't forget about the polarity and the shape of the molecules. The smaller molecules may be more polar or have a shape more conducive to intermolecular attraction than the larger molecule. (10:43:36 AM)
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