Essay on Intermolecular Forces

Of the two alkane liquids studied n-Hexane was determined to have the stronger IMF of attraction by virtue of its experimentally determined lower ?T. Conversely n-Pentane has weaker IMF of attraction due to its larger ?T. As explained at length above, this is because it takes more energy to excite a molecule in liquid to leave (vaporize or become gaseous), when there are stronger IMF of attraction holding the molecules together in liquid form.

The makeup of a compound drastically changes its intermolecular forces (IMFs) with the polar silica gel of a TLC plate; this concept is responsible for the variability of Rf values observed throughout the course of lab. The weaker the IMFs, the further a compound will travel through the silica. For instance, ionic interactions are the strongest IMF, but were not present during this experiment. H-bonding IMFs had the greatest impact for our specific compounds. Resorcinol and 3-chlorobenzoic acid exhibited low Rf values, due to its ability to H-Bond to silica’s hydrogen donors and oxygens acceptors (See graph 1). Both were adept to strongly H-bonded to silica because the compounds contained at least 1 H-donor and 2 H-acceptors. Thus, stronger/more

As a result of the water molecule bond, each (hydrogen; oxygen) has a slightly negative charge and each (hydrogen; oxygen) has a slightly positive charge.

A greater number of electrons correspond to a great polarizability of a molecule. Greater polarizability leads to greater dispersion forces. Thus, as molar mass increases, the number of electrons increase, which increases the polarizability of the molecule and hence the strength of the dispersion forces of the substance.

Substance A and B were weighed; Substance A weighed 0.502 g and substance B weighed 0.503 g. Both substances were put into two different test tube with approximately 8 ml of DI water into the test tub. Substance A and B were stirred and B dissolved while A did not. This shows that B is soluble in water compared to A. Thus, shows that B is soluble in water than A. The reason why B is soluble in water is because it has a higher dipole moment than A. With a higher dipole moment, it shows that it is soluble in water since it is polar and the bonds were easily broken.

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

There are many types of chemical bonds and forces that bind molecules together. The two most basic types of bonds are characterized as either ionic or covalent. In the lab we separated Citric Acid, Calcium Chloride, Sucrose, Potassium Iodine, Phenyl Salicylate ,and Sodium Chloride into two groups ionic and Covalent bonds .The Chemical Difference between ionic bonding and covalent bonding is, a covalent bond is formed between two nonmetals that have similar electronegativities. Metals are left half and center of the Periodic Table and Nonmetals are upper right of the Periodic Table. The electrical attraction between large numbers of cations and anions which is the transfer of the

By identifying the solubility of the unknown, it could lead to a closer interpretation as to what the functional group the unknown may be. Solubility is determined based on intermolecular attractive forces, such as hydrogen bonding, dipole-dipole, and London dispersion forces. Intermolecular attractive forces arise due to different electron environments in different molecules. For example, water molecules are good at dissolving

It takes very little energy to break these forces; therefore simple covalent compounds have very low melting points and generally appear as gases. You can also get multiple bonds; this is where atoms can share more than 2

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

In water, Hydrogen bonding pulls molecules close together by the negative oxygen made by another molecule of water is attracted to a positive hydrogen atom. Thanks to hydrogen bonds, water boils at 212 degrees Fahrenheit instead of -108.4 degrees. Hydrogen bonds are also make up proteins and DNA (wisegeek). Covalent bonds are bonds between two non-metals that share electrons with one another. Covalent bonds occur when they have similar electronegativity (diffen). An Ionic bond is where a metal and a non-metal bond when the metal gives up electrons to complete the outer shell of a non-metal, and then an attracting another with the now polarized atoms (differencebetweenExplain the 7 characteristics of life.In order for something to be considered a living being, they need to follow a set of seven rules. The first is that living things are made of cells, either single celled or multicellular. The next rule says that a living thing must have both molecular and cellular organization on several levels. Multicellular beings must have tissue, organs, and organ systems to be considered an organism. Livings must use energy for maintenance and growth; Energy can come from other

This article used chemical bonds because in addition to the last paragraph to have compounds to need to have chemical bonds. A chemical bond is an attraction between atoms that allows the formation of a chemical. In the article they bonded together different elements to make compounds, which they in turn helped de-ice the streets. The chemical bond helped make a salt-polymer composite which would help the CHKO2 compound to stay in the road for years. Chemical bonds help the atoms stay together and keep compounds

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.

After completing the lab, we will be able to identify covalent, ionic, and hydrogen bonds. Hydrogen bonds are the weakest between all the three types of bonds we will be observing and it occurs between hydrogen and oxygen atom or nitrogen atom; hydrogen bonds are a type of dipole-dipole bond. A dipole-dipole interaction occurs because of polar molecules. We should know that the bond between hydrogen and oxygen in a water molecule is covalent. Another example, of covalent bond is the bond between all the atoms that compose ethane. Another objective that we will observe is solubility, the lab mentions. An example, of an ionic bond is NaCl, this is an ionic bond because the Na+ and Cl-, the sodium atom (cation) gives a pair of electrons to the

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