Log in
HomeClass Notes1,200,000US530,000

CHE-1102 Lecture Notes - Lecture 6: Surface Tension, Problem Solving, Intermolecular Force

11 views3 pages
School
App State
Department
Chemistry
Course
CHE-1102
Professor
Jennifer Cecile

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Intermolecular forces and physical properties: the strength of intermolecular forces can greatly affect the properties of a substance or solution, the physical properties affected including boiling point, melting point, viscosity, and surface tension. Boiling point: boiling point: the temperature where liquid molecules convert into gas molecules, the stronger the intermolecular forces, the higher the boiling point. Thus, the more heat needed to change from a liquid to a gas: problem solving, read the problem, identify all imf present, solve for the question, check your work. Melting point: melting point: the temperature needed to convert from solid to liquid, the melting point increases as the intermolecular forces become stronger, ionic compounds have extremely high melting points. Viscosity: viscosity: the resistance of the flow of a liquid. Includes the ability of molecules in a substance to pass each other: as intermolecular forces get stronger, viscosity increases, viscosity decreases with increased temperature.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related Documents

CHE-1102 Chapter Notes - Chapter 13: Strong Electrolyte, Miscibility, Freezing-Point Depression
aquamarinewasp815
CHE-1102 Lecture Notes - Lecture 3: Colligative Properties, Mole Fraction, Molar Mass
coralporcupine226
CHE-1102
Final Exam
Study Guide
CHE-1102 Study Guide - Quiz Guide: Electronegativity, Viscosity, Exothermic Process
aquamarinewasp815

Related Questions


* Circle the intermolecular force(s) that is/are present in each of the following species. [Hint: there may be more than one correct answer.]

Ar (hydrogen bonding, dipole-dipole forces, dispersion forces)

CH4 (hydrogen bonding, dipole-dipole forces, dispersion forces)

HBr (hydrogen bonding, dipole-dipole forces, dispersion forces)

HF (hydrogen bonding, dipole-dipole forces, dispersion forces)

CHCl3 (hydrogen bonding, dipole-dipole forces, dispersion forces)

* For the following pairs of atoms/molecules, circle the species that has the higher boiling point.

Ne or Xe

Cl2 or F2

HBr or HF

HCl or HI

H2O or H2S

* Phase changes always associate with change of enthalpy. For the following situations, name the phase

transition and indicate whether the process is exothermic or endothermic.

(a) Dry ice (solid carbon dioxide) turns to gaseous carbon dioxide.

Answer:

(b) Water vapor turns to liquid water.

Answer:

(c) Solid iron turns to liquid iron.

Answer:

(d) Iodine vapor turns to solid iodine.

Answer:

(e) Liquid helium turns to helium gas.

Answer:

* True or false

1. Intermolecular forces are stronger than ionic and covalent bonds. Answer:

2. For molecules with similar size and molar mass, those with higher polarity would have higher boiling

point. Answer:

3. Ion-dipole forces exist between ionic potassium bromide and polar water.

Answer:

4. Dispersion forces exist between argon and helium. Answer:

5. Instantaneous dipoles exist in all molecules and atoms. Answer:

6. The strength of dispersion forces depends on the molar mass but the shape of the molecules have no effect on dispersion forces. Answer:

7. Ice has a higher density than water because ice has an ordered cagelike structure. Answer:

8. Liquids with weaker intermolecular interactions have lower viscosity. Answer:

9. Viscosity decreases with increasing temperature. Answer:

10. For any molecules, the heat of vaporization is always lower than the heat of fusion because it takes more energy to make molecules to move past one another in a solid lattice. Answer:

Phase changes always associate with change of enthalpy. For the following situations, name the phase transition and indicate whether the process is exothermic or endothermic.

. Dry ice (solid carbon dioxide) turns to gaseous carbon dioxide. Answer:

. Water vapor turns to liquid water. Answer:

. Solid iron turns to liquid iron. Answer:

. Iodine vapor turns to solid iodine. Answer:

. Liquid helium turns to helium gas. Answer:

True or false

. Intermolecular forces are stronger than ionic and covalent bonds. Answer:

. For molecules with similar size and molar mass, those with higher polarity would have higher boiling point. Answer:

. Ion-dipole forces exist between ionic potassium bromide and polar water. Answer:

. Dispersion forces exist between argon and helium. Answer:

. Instantaneous dipoles exist in all molecules and atoms. Answer:

. The strength of dispersion forces depends on the molar mass but the shape of the molecules have no effect on dispersion forces. Answer:

. Ice has a higher density than water because ice has an ordered cagelike structure. Answer:

. Liquids with weaker intermolecular interactions have lower viscosity. Answer:

. Viscosity decreases with increasing temperature. Answer:

. For any molecules, the heat of vaporization is always lower than the heat of fusion because it takes more energy to make molecules to move past one another in a solid lattice. Answer: