Intermolecular force

Analysis: 2. Of the alcohols tested 1-Butanol was found to contain the strongest intermolecular forces (IMF) of attraction, with Methanol containing the weakest. It was discovered through experimentation that Methanol induced the highest ?T of all alcohols tested, and that conversely 1-Butanol induced the lowest ?T. The atomic structure of all four alcohols is very similar, as starting with 1-Butanol a CH2 group is lost as you move from 1-Butanol to 1-Propanol to Ethanol and then again to Methanol

Intermolecular forces are the attractive and/or repulsive forces among independent particles, such as molecules, atoms, or ions, within a sample of matter. These forces differ from chemical bonds, or intramolecular forces, because chemical bonds exist between the atoms of a single molecule. For example, intermolecular forces could be described as the forces that attract many water molecules together, while chemical bonds refer to the bonds between the hydrogen and oxygen atoms of a single water molecule

The objective of this experiment was to investigate the relationship of dispersion forces and hydrogen bonding forces in intermolecular attractions through the evaporation of different substances. Using temperature probes, the endothermic process of evaporation is measured by inserting the probes into the substance and then taking them out to allow the substance to evaporate, the change in temperature of the substances showed if a lot or not a lot of evaporation occurred and over how long the evaporation

Experiment 2: Intermolecular Forces Performed: 9/12/2011 Submitted: 9/20/2011 Chemistry 1046L PART I: Purpose: The purpose of partI in this experiment is to identify a variety of unknown substances’ properties using observations of the temperature changes that occur during evaporation. We know that substances with weaker intermolecular forces, such as London dispersion, will have a faster vaporization rate and thus a higher temperature difference compared to

Intermolecular attractive forces are forces of attraction that act between different molecules. These forces are substantially weaker than the intramolecular forces acting inside of molecules, however, they are still a vital force that holds molecules together in the solid and liquid phase. In order to fully grasp the importance of intermolecular attractive forces (henceforth referred to as IMAF) we must first understand two central concepts that make IMAF possible: electronegativity and molecular

Lab: Intermolecular Attractions Introduction/Background: A solution consists of two or more different substances. The dissolving process that takes place in a solution occurs due to the intermolecular forces that act between molecules in the solution. The solubility rule, “Likes dissolve likes”, explains why certain solutes dissolve in a given solvent, while other solutes do not. In most cases, ionic or polar solutes dissolve in polar solvents. Similarly, non-polar solutes dissolve in non-polar

Oakland Schools Chemistry Resource Unit Intermolecular Forces  Brook R. Kirouac  David A. Consiglio, Jr.  Southfield‐Lathrup High School Southfield Public Schools    Bonding: Intermolecular Forces Content Statements: C2.2: Chemical Potential Energy Potential energy is stored whenever work must be done to change the distance between two objects. The attraction between the two objects may be gravitational, electrostatic, magnetic, or strong force. Chemical potential energy is the result of

mainly because of their intermolecular bonds and their intramolecular bonds. Intermolecular bonds refer to the attraction and repulsion found between neighbouring ions or molecules. These typically determine the molecules physical properties, such as boiling/melting points, shape/state, hardness/softness, colour, lustre, ductility, brittleness etc. Typically, those with larger and longer bonds will have stronger properties. There are six main types of intermolecular forces, being: Covalent networks

Introduction The strengths of intermolecular forces such as dipole-dipole, London dispersion and hydrogen bonding of various substances change over a wide range. However, intermolecular forces are much weaker than covalent bonds and ionic bonds. It requires less energy to overcome intermolecular attractions of molecules in a liquid to vaporize them as compared to the energy needed to break their covalent bonds. When molecules change from solid to liquid to gas, the molecules themselves do not change

TASK 1-activity 2-M1 The stronger an intermolecular force, the higher the boiling point of the substance will be. This is because more energy is required to break the intermolecular forces. The order of strength of intermolecular forces is; Hydrogen bonding> permanent dipole-dipole interaction> Van der Waal’s force Magnesium Oxide has a very high melting and boiling point of 2852 and 3600 respectively. Magnesium oxide is held toghether with ionic bonds, and therefore require a lot on energy to separate