Task 1: Intermolecular Force

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.

While the other two compounds melted within a couple of seconds. Vapor might have formed on the sides of the test tube for unknown 1 because of the reason that the distilled water within the compound began to evaporate. If the distance between the flame and the test tube differed, the test might have gone wrong, yielding in incorrect results. Because of the strength of ionic compounds, it takes more energy to break their bonds. With the rise of heat, comes the rise of energy, which is the reason why ionic compounds have high melting points as well as high boiling points. The melting point of sodium chloride is 801°C and copper chloride is 498°C. The melting point of citric acid is 153°C and sucrose is

Other substances that dissolve in water also lower the freezing point of the solution. The amount by which the freezing point is lowered depends only on the number of molecules dissolved, not on their chemical nature. This is an example of a colligative property. In this project, you'll investigate different substances to see how they affect the rate at which ice cubes melt. You'll test substances that dissolve in water (i.e., soluble substances), like salt and sugar, as well as substances that don't dissolve in water (i.e., insoluble substances), like sand and pepper. Which substances will speed up the melting of the ice?

What special bond (in water) opposes water’s molecular movement when water absorbs energy requiring water to have more heat added to raise its temperature? Hydrogen Bond.

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.

The purpose of this experiment was to determine the melting point and the boiling point of various unknown solids and liquids supplied by the laboratory. In the process of exploring the most basic physical properties of the given samples, skills such as: proper determination of compound purity through different means and how to

The electrons in the molecule are on the oxygen side of the molecule. By doing this it causes a reaction of giving this side a negative charge and the hydrogen side a positive charge. Only other polar molecules can dissolve in water because polar molecules dissolve only in polar solvents and non-polar molecules dissolve only in non-polar solvents .Oil and water don't mix because oil is made up of non-polar molecules while water molecules are polar in nature. Since water molecules are electirically charged they get attracted to other water molecules an extract the oil molecules . This eventually causes the oil molecules ,or lipids to clump together.

Salt uses some basic laws of chemistry to break down accumulation of ice. As you know, salt is an ionic compound, Sodium Chloride. According to intermolecular forces, ionic compounds have the highest melting and boiling rates. Ice’s melting point is at 0 degrees whereas Salt’s is about 800 degrees.

The bent geometry of water molecule gives a slight overall negative charge to the side of the oxygen atom and a slight overall positive charge to the side of the hydrogen atom. This slight separation of charge gives the entire molecule an electrical polarity so water molecules are dipolar.

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.

Ionic compounds have high melting points because ionic bonds are very strong and take a lot of energy to break. They can only conduct electricity when they are in their liquid form because their ions must be able to move around.

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 took place depending on if the change in temperature was high or low.

The hydrophobic effect very clearly displays the properties of water. Nonpolar molecules are not able to participate in ionic interactions, or even in hydrogen bonding. The interactions between water molecules and nonpolar molecules are not as favorable as the interactions between the water molecules with each other. The water molecules form “cages” around the nonpolar molecules when they are interacting with each other. But, some of the water molecules are released when 2 of the nonpolar molecules are interacting with each other. The water molecules being released

Water consists of 2 atoms of hydrogen and 1 atom of oxygen. Each hydrogen atom is covalently bonded to the oxygen through a shared pair of electrons. Water’s chemical structure and physical factors gives it the ability to be the ‘universal solvent.’ This characteristic of water is because the water molecules have structured the oxygen and hydrogen atoms in a polar arrangement. The hydrogen atoms of the molecule give off a slightly positive electrical charge and the oxygen atoms of the molecule give off a slightly negative electrical charge. As a result, this allows the molecule to be attracted to many different types of molecules. As an example of its solubility, water can become heavily attracted to a salt molecule (NaCl). This attraction to the salt molecules can disrupt the intermolecular forces holding the sodium and chloride atoms together and as a result, the water dissolves the salt molecule. (Howard Perlman, 2017)

Water is a special type of covalent bond called a hydrogen bond, this bond is similar to dipole dipole forces but has a greater intermolecular force. A hydrogen bond is the intermolecular force of attraction between a