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Ionic bonding occurs between a metal and a non-metal. Electrons are transferred from the metal to the non-metal to achieve full outer shells. When the electrons are transferred, it creates charged particles called ions. Oppositely charged ions attract through electrostatic forces to form a giant ionic lattice. Example:
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- INTRODUCTION TO INTERMOLECULAR FORCES
- Intermolecular Bond Strengths
- Na Cl
- Viscosity
- Capillary Action
- Surface Tension
- ΔHvap
As we ended the lectures on gases, we were introduced to an idea that serves as foundation for the material in this lecture: As we were introduced to ideal gases, we learned from kinetic molecular theory exhibit that no attractions occur between colliding molecules. ...BUT THIS IS NOT TRUE So at the gas material we learned that non-ideality ar...
So now let’s get quantitative with bonding. Note, intramolecular bonds are 1 to 2 orders of magnitude stronger (But it is weak intermolecular attractions intermolecular forces) that allow liquids and solids to form.) intermolecular forces are responsible for solution properties like boiling point and viscosity the relative magnitude of int...
Na- - - - - - - Notice ambiguity in inter and intramolecular exists Na Cl Na Cl that a single Na-Cl unit does not actually exist. Now the rest of the lecture. What are the solution properties? (You need only to know their definitions and a brief theoretical explanation for relationship to intermolecular forces.)
: stickiness when pouring; consequences of IMF attraction between molecules. This “resistance to flow” is a surface phenomenon. Ex. honey vs ether Honey Note: The stronger the IMF, the more viscous the solution Ether
this is the tendency to climb the walls of a capillary. It is what created the meniscus you see in burettes and straws filled with water Note: The stronger the IMF, the greater the capillary action so water is observed to crawl up the walls. H2O hexane
The phenomenon that maintains the surface interface between liquid and gas. It allows you to place needles and insects on surfaces despite being denser. H2O Note: The greater the IMF, the greater the surface tension. Here, water is has a much greater surface tension than acetone. Acetone The demo in class with the ants is recreated here with ...
Thermodynamic term for which is the energy for a liquid to become a gas. It is found in boiling and evaporation equations. Note: The larger the IMF, the greater the ΔHvap.
Chapter 8 – Chemical Forces Understanding the relative melting/boiling points of two substances requires an understanding of the forces acting between molecules of those substances. These intermolecular forces are important for many additional reasons. For example, solubility and vapor pressure are governed by intermolecular forces.
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• Intermolecular Force (IMF): between molecules. This is the force that holds molecules together. It is a form of “stickiness” between molecules. Examples of intermolecular forces are London dispersion forces (LDF), dipole-dipole forces (DDF), and hydrogen bridging forces (HBF).
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• The term “INTERmolecular forces” is used to describe the forces of attraction BETWEEN atoms, molecules, and ions when they are placed close to each other • This is different from INTRA molecular forces which is another word for the covalent
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Revision notes on 1.5.3 Types of Forces Between Molecules for the AQA A Level Chemistry syllabus, written by the Chemistry experts at Save My Exams.
People also ask
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Define and explain van der Waals forces. How do they hold molecules together. Learn their different types and importance, and check out a few examples.
