Concept explainers
a)
Interpretation: Molecule that makes the weakest intermolecular attachments to neighboring molecules should be determined.
Concept introduction: Intermolecular forces are types of forces that are responsible to hold atoms together in a molecule.
There are various types of intermolecular forces as follows:
1. Hydrogen bonding:
As is evident from its name, these types of forces exist if hydrogen is present. Such forces are present when hydrogen atom bonds with highly electronegative elements like N, O, F. It is of two types: intramolecular and intermolecular.
2. Ion-dipole forces:
This force exists between ion and molecules with dipole moment in them. Attraction exists between ion and oppositely charged end of the dipole.
3. Ion-induced dipole forces:
When an ion approaches a non-polar molecule, it induces a temporary dipole in it. Ion gets attracted to the oppositely charged part of the dipole induced in the molecule.
4. Induced dipole-induced dipole attraction:
These forces are also known as London dispersion forces or van der Waals forces. Such forces are present between various atoms and molecules. These are observed generally in non-polar molecules, halogens and noble gases.
b)
Interpretation: Whether dipole moment trends with boiling points for propanal
Concept introduction: Dipole moment is the measure of bond polarity in the molecule. It is defined as the product of charge and distance of separation between opposite charges. Polar molecules consist of dipole moments due to the presence of charges in them whereas non-polar molecules do not have dipole moments. Boiling is used to define when a substance gets converted from its liquid to the vapor phase at the boiling point. The temperature at which the vapor pressure of the liquid becomes equal to atmospheric pressure is called the boiling point.
Want to see the full answer?
Check out a sample textbook solutionChapter 4 Solutions
Organic Chemistry: A Guided Inquiry
- Consider the data in the table. Compound Melting point (°C) ????? (??/???)ΔHfus (kJ/mol) Boiling point (°C) ????? (??/???)ΔHvap (kJ/mol) HFHF −83.11 4.577 19.54 25.18 HClHCl −114.3 1.991 −84.9 17.53 HBrHBr −86.96 2.406 −67.0 19.27 HIHI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ?fusΔSfus and Δ?vapΔSvap for HF.HF. Δ?fus=ΔSfus= J/(K⋅mol)J/(K⋅mol) Δ?vap=ΔSvap= J/(K⋅mol)J/(K⋅mol) Determine the entropy change when 7.60 mol HF(l)7.60 mol HF(l) boils at atmospheric pressure. Δ?=ΔS= J/Karrow_forwardChoose the letter of the word that does NOT belong in the group and explain in one sentence. 1. A. Al B. Zn C. Fe D. Na 2. A. Viscosity B. Melting Point C. Surface Tension D. Vapor Pressure 3. A. Water B. Nylon C. Salt D. Bases 4. A. H2O B. CO2 C. NH3 D. SO2 5. A. London Dispersion B. Dipole-Dipole Forces C. Nitrogen Bonding D. Ion-Dipole Forcesarrow_forwardConsider the data in the table. Compound Melting point (°C) ????? (??/???)ΔHfus (kJ/mol) Boiling point (°C) ????? (??/???)ΔHvap (kJ/mol) HFHF −83.11 4.577 19.54 25.18 HClHCl −114.3 1.991 −84.9 17.53 HBrHBr −86.96 2.406 −67.0 19.27 HIHI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ?fus and Δ?vap for HF. Δ?fus= J/(K⋅mol) Δ?vap= J/(K⋅mol) Determine the entropy change when 8.70 mol HF(g) condenses at atmospheric pressure. Δ?= J/Karrow_forward
- Why should Ne be less soluble in water than F2? Please choose the answer that best explains the difference in solubility. A. The lower molar mass of Ne makes it easier to polarize the molecule to dissolve in polar water. B. The higher molar mass of F2 makes it easier to polarize the molecule to dissolve in polar water. C. The Ne is polar and, therefore, more soluble than F2 in water. D. The F2 is polar and, therefore, more soluble thanNe in water.arrow_forwardA. Predict the type of intermolecular forces that will be formed with the same kind (#1-3)and different kinds of molecules (#4-5). Illustrate or draw the bonding between themolecules.arrow_forwardWhich of the following molecules will have the lowest polarizability? a. A small molecule with little contact area b. A small molecule with a large contact area c. A large molecule with a large contact area d. A large molecule with a small contact area e. A medium sized molecule with an large contact area Which of the following halogens will have the highest boiling point? a. Iodine b. Bromine c. Chlorine d. Fluorinearrow_forward
- -Aside from London dispersion forces, which substance do you expect dipole interactions to be effective? a. Substance A and B b. Substance B and D c. Substance A and C d. Substance B and E -Which substances can react with potassium borohydride, converting the product into alkene alcohol (assuming complete reaction)? a. Substance A and B b. Substance B and D c. Substance C and D d. Substance D and E -The presence of trans pi bonds can influence molecular stacking due to the limitation of bond rotation. Based on this information, which substance is characterized by molecules that have effective molecular stacking? a. Substance A b. Substance B c. Substance C d. Substance D e. Substance E -Which substance CANNOT decolorize bromine water? a. Substance A b. Substance B c. Substance C d. Substance D e. Substance Earrow_forward1. Is the pointed structure intra or H- intermolecular bond 2. What is it? 3. What other IFA is possible for this compoundarrow_forwardMCQ 14: After SnCl, the tetrachloride compound which has the highest boiling point is A. CCI, B. SİCI, C. GeCl D. PbCl4arrow_forward
- Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. chemical symbol, substance chemical formula boiling point or Lewis structure Ar (Choose one) A В Cr (Choose one) v H H. H. H - C - C - ) - C H (Choose one) | H H H. H H - C -H D :N - O - H (Choose one) ♥ Н—С — Н ? :0 : :arrow_forward9. Draw Lewis Structures of the following compounds: (You will use these Lewis Structures to predict intermolecular forces.) 1. Compound V (CH3CH3) 2. Compound W (HOCH2CH2OH) 3. Compound X (CH3CH2CH3) 4. Compound Y (CH3CH2OH). 5. Compound Z (CH3-O-CH3)arrow_forward15. a. Draw two constitutional isomers with the formula CaHsBrCl ( Isomer 1 Isomer 2 b. Describe ALL the intermolecular forces isomer 1 can participate in 16. For the molecule below, OH (a) Circle all functional groups present. (b) Label two of the functional groups next to where you circled them 3arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning