Octane Has The Strongest Intermolecular Forces Of Nonane

alcohol, making it either primary (1° ), secondary (2° ), or tertiary (3° ). If the OH is bonded to only one other carbon, it is a primary alcohol (eg. 1-butanol); if bonded to two other carbons, it is a secondary alcohol (eg. 2-butanol); if bonded to three other carbons, it is a tertiary alcohol (eg. 2-methyl-2-propanol). Due to the placement of the hydroxyl functional group in each of the degrees of alcohol, the reactivity of each should be impacted. This means that all three

The Hydroxyl group on alcohols relates to their reactivity. This concept was explored by answering the question “Does each alcohol undergo halogenation and controlled oxidation?” . Using three isomers of butanol; the primary 1-butanol, the secondary 2-butanol and the tertiary 2-methyl-2-propanol, also referred to as T-butanol, two experiments were performed to test the capabilities of the alcohols. When mixed with hydrochloric acid in a glass test tube, the primary alcohol and secondary alcohols were expected to halogenate, however the secondary and tertiary ended up doing so. This may have been because of the orientation of the Hydroxyl group when butanol is in a different

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. Each structure is fairly linear and contains an H-bond with Oxygen, so the real change is found in the loss of the CH2 group, this lowers the liquid’s Molecular Mass, thus lowering the London forces as you move from 1-Butanol through

Attractions between water and other molecules, which is adhesion, is also possible because of the polarity as well. In relation to hydrogen bonds, water’s high specific heat is changed when hydrogen bonds are made or broken. When a hydrogen bond breaks, heat is absorbed whereas when a hydrogen bond forms, heat is released. In addition to HSH, ice is able to float in liquid water because hydrogen bonds in ice is more structured than in water, making the ice less dense. Also, water is a versatile solvent because of its polarity, which helps it form hydrogen bonds (mentioned above). The structure of water molecules also affects the dissociation of water, where H2O breaks into H+ and OH- due to the polarity of the

Benzophenone was soluble in methyl alcohol whiles biphenyl was partially soluble. Benzophenone and biphenyl are both nonpolar molecules. Methanol is intermediately polar, allowing both nonpolar molecules to be dissolved as it is not too polar or nonpolar. However, biphenyl is less polar than benzophenone. Since methyl alcohol is somewhat polar, the more polar benzophenone is more soluble in methyl alcohol than biphenyl. Also, benzophenone can make hydrogen bonds. Thus, benzophenone is more soluble in methyl alcohol than

B. Claim: As we go from methanol  ethanol  1-propanol  1-butanol the dispersion forces increase.

A London dispersion force is the name given to intermolecular forces in a non-polar compound. It greatly depends on the amount of electrons in a molecule. The larger/ heavier molecules have more electrons resulting in a greater attractive London force. This is because as the external force causes a temporary shift, the electrons will move to one side and it will become more negative resulting in a greater attraction. Then it will return to its previous state of the dispersion of

False because what keeps them together is Hydrogen bonding.Repellant forces would repel the molecules if the hydrogen bonds weren’t there.

fewest electrons, lowest melting point. methyl propane is more compact than butane so it packs

Tell what kinds of intermolecular forces could occur between the following pairs of solute and solvent, and place the list in order from weakest to strongest solute-solvent attraction. Some pairs may experience more than one type of force.

Put hydrogen bonds, dispersion forces and dipole-dipole forces in order of how strong they are and give an example of each

A hydrogen bond is an interaction involving a hydrogen atom and a highly electronegative atom

Densities, for three binary mixtures- Cyclohexane (CHXN) + Toluene (TN), + o-Xylene (OXN) and + Mesitylene (MSTN) were measured at T = (303.15, 308.15, 313.15, 318.15 and 323.15) K. The measurements were carried out over the whole range of composition, using a 10 cm3 bi-capillary pycnometer. The excess molar volumes, VmE, apparent molal volumes, v, thermal expansivities, , and excess thermal expansivity, , were calculated from the density data. The VmE results were correlated with the fourth-order Redlich-Kister equation. Variations in the calculated excess properties for the liquid mixtures were studied in terms of intermolecular interactions. It was found that the values of VmE are dependent on temperature and in all cases increases

If I was to do an experiment like this again I could use a different variable instead of alcohols. Instead I could investigate a chain of alkanes or alkenes, “in order to test alkenes I would have to look into the association double carbon bonds have with one

As mentioned in the discussion, olive oil, vegetable oil, crisco, and lard were soluble in nonpolar solvents and insoluble in polar solvents. This is due to the chemical composition of polar and nonpolar substances which results from the molecular shape as well as properties of dissolving solutes in solution. Polar substances are hydrophilic and contain polar Van Der Waals interactions (intermolecular forces) such as dipole-dipole forces, ion-dipole forces, and hydrogen bonding. Nonpolar substances are hydrophobic and contain non-polar Van Der Waals interactions. ‘Like dissolve like’ is the reason only polar solutes dissolve in polar solvents and why nonpolar solutes dissolve in nonpolar solvents. Molecules with similar polarity have similar intermolecular forces and therefore, can interact with each, or in this case dissolve9. Additionally, the solubility of a compound is determined by the length of the hydrocarbon chain. Long hydrocarbon chains such as the one found in oleic acid makes a compound more insoluble10. Therefore, since the lipids used in this experiment were hydrophobic substances and each lipid has long hydrocarbon chains, the results were consistent with the scientific literature and principles.