142_R01_Intro_IMF_KEY
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Michigan State University *
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Chemistry
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Feb 20, 2024
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CEM 142 Recitation 1 KEY
IMF Review
1a. Draw 3 molecules of CH
3
CH
2
CH
2
CH
3 (butane) in the liquid state showing the strongest interactions that are present between the molecules. 1b. What type of interaction did you show in your picture? Identify the important features of the interaction and how they were depicted in your picture. Make sure your interaction is labeled.
Revise your picture if necessary. London dispersion forces are temporary interactions between an instantaneous dipole and the subsequently induced dipole. Therefore, the dipoles should be labeled
as such. These temporary dipoles should be indicated on both electron clouds using partial positives and partial negatives. The molecules should be lined up so that the partial positive end of one is interacting with the partial negative end of another molecule. For clarity, the LDF interaction
is labeled, and an arrow is used to specify the place where the interaction occurs.
1c. Are there any other intermolecular forces present in liquid CH
3
CH
2
CH
2
CH
3
? If so, list them below.
none
2a. Draw 3 molecules of (CH
3
)
3
N (trimethylamine) in the liquid state showing the strongest interactions that are present between the molecules.
2b. What type of interaction did you show in your picture? Identify the important features of the interaction and how they were depicted in your picture. Make sure your interaction is labeled.
Revise your picture if necessary.
Dipole-dipole is an interaction between the molecular dipoles of two polar molecules. Therefore, showing the 3D-shape of the molecule and using a molecular dipole arrow is the best way to indicate the overall polarity. The molecules should then be ordered in a way that
clearly indicates that the interaction is taking place between the positive end of one molecule and the negative end of another. For clarity, the dipole-dipole interaction is labeled, and an arrow is used to specify the place where the interaction occurs.
2c. Are there any other intermolecular forces present in liquid (CH
3
)
3
N? If so, list them below.
LDFs
3a. Draw 3 molecules of CH
3
COOH (acetic acid) in the liquid state showing the strongest interactions that are present between the molecules.
3b. What type of interaction did you show in your picture? Identify the important features of the interaction and how they were depicted in your picture. Make sure your interaction is labeled. Revise your picture if necessary.
Hydrogen bonding is a directed interaction between a lone pair on a very electronegative atom, in this case O, to a hydrogen that is covalently bonded to a very electronegative atom,
in this case O. Therefore, the dashed line indicating the hydrogen bond is specifically starting
and ending at those positions. For clarity, the hydrogen bonding interaction is labeled, and an arrow is used to specify the place where the interaction occurs.
3c. Are there any other intermolecular forces present in liquid CH
3
COOH? If so, list them below.
Dipole-dipole interactions
LDFs
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4. Based on your answers to questions 1, 2, and 3 which substance do you predict to have the highest ∆H
vap
and why? Make sure your explanation includes a claim, evidence, and reasoning.
Claim:
Acetic acid has the highest ∆H
vap
.
Evidence:
In a liquid sample of butane, the only intermolecular force is LDF. In a liquid sample of trimethylamine, dipole-dipole interactions and LDFs are present between the molecules. In a liquid sample of acetic acid, hydrogen bonding interactions, dipole-dipole interactions, and LDFs exist between the molecules.
Reasoning:
Hydrogen bonding interactions are stronger than dipole-dipole interactions and LDFs.
The substance with the stronger IMFs (acetic acid) would need more energy to overcome the stronger interactions. More energy means the ∆H
vap
(energy needed to vaporize the substance) would be highest.
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Name:
1. Circle and label the functional groups for the following compounds.
OH
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2. Here are the list of melting point for starting materials and products. Explain why the melting
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6
N. Garg, J. Singh, J. Sun, CC BY-NC-SA 4.0
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yout References
2 v
Font
₂x²A - A
V
Mailings Review View Help
A A Aa AEE ALT
Y
f3
5
United States) Text Predictions: On
O
14 101
===
Paragraph
Search (Alt+Q)
4.All are correct
V
Accessibility: Good to go
15
5
1.To the polarity of water and that organic compounds are nonpolar.
f6 D
Normal
Organic compounds tend not to mix with water. What is the reason for this chemical
characteristic of organic compounds with water?
2.Because water forms a hydrogen bond and hydrocarbons do not have polarity for this,
unless they have an oxygen in the chain.
3.Some alkanes can mix with water if they have a carbonyl or hydroxyl group.
No Spacing
f7 40
Styles
hp
18
Heading 1
19 0
0
f10
F17
5
F12
Find
Replac
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Editing
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CH,CH,
CH,CH,
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O structural isomers
O geometric isomers
and
same molecule
no relationship
41
Boiling points depend on the mass of the compound and the attraction between molecules of the compound
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False
0000
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H
H
H
H
H
H
H
H
H
-H
Indicate with a Y (yes) or an N (no) which apply.
dipole forces
induced dipole (London dispersion) forces
hydrogen bonding
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of 305.7 µg/m³. What is this concentration in ppm?
Assume the air temperature is 300 K.
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0.0290 ppm
40.2 ppm
0.250 ppm
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Compound
Melting point (°C)
????? (??/???)ΔHfus (kJ/mol)
Boiling point (°C)
????? (??/???)ΔHvap (kJ/mol)
HFHF
−83.11
4.577
19.54
25.18
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1.991
−84.9
17.53
HBrHBr
−86.96
2.406
−67.0
19.27
HIHI
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2.871
−35.38
21.16
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Δ?fus= J/(K⋅mol)
Δ?vap= J/(K⋅mol)
Determine the entropy change when 8.70 mol HF(g) condenses at atmospheric pressure.
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????? (??/???)ΔHfus (kJ/mol)
Boiling point (°C)
????? (??/???)ΔHvap (kJ/mol)
HFHF
−83.11
4.577
19.54
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−114.3
1.991
−84.9
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2.406
−67.0
19.27
HIHI
−50.91
2.871
−35.38
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J/(K⋅mol)J/(K⋅mol)
Δ?vap=ΔSvap=
J/(K⋅mol)J/(K⋅mol)
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Δ?=ΔS=
J/K
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Fat
or oil
Palmitic
A
24.6
B
14.6
C
8.5
D
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Sample B
Sample C
Sample D
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Part 2 out of 2
57
Which of these molecules can hydrogen bond with water?
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|>|||>|| >IV
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111
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