Covalent Bonds Lab

6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__

We decided to do the McMush Lab. The lab was designed to see the biomolecules inside an average McDonald’s Happy Meal. We decided to use a meal we have all had and to see what we were eating. Our results showed certain biomolecules.

***Repeat steps 2-4 for each of the following: 5 mL of oil and 2 g each of cornstarch, sodium chloride, and sodium bicarbonate.

The purpose of this lab is to study some of the physical properties of two types of solids – ionic and molecular. The samples used are sodium chloride (ionic) and camphor (molecular). The physical properties studied are odour, hardness, melting point, solubility in water and solubility in 2-propanol. It is observed that some of the physical properties of sodium chloride are no odours, hard, a high melting point, soluble in water and insoluble in 2-propanol; some of the physical properties of camphor are a strong odour, soft, a low melting point, insoluble in water and soluble in 2-propanol. A few conclusions can be drawn from these

In determining the melting point range of the aspirin, a capillary tube (sealed at one end) was one-third-filled with the dried aspirin. The capillary tube and a thermometer were immersed in an oil bath. The temperature at which the solid started to melt and the temperature when the entire sample was completely liquefied were recorded as the melting point temperature range.

6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,

Day 1. Michael was coming home for vacation from college. When he got home he found out that

1. Place a small amount of wax from a birthday candle into a test tube. Heat gently over a burner flame until the wax melts completely; then allow

5. Zoom Out by clicking on the green arrow next to the Save button. Click on the Stockroom and then on the Clipboard and select Balloon Experiment N2. Again, set the temperature, pressure, and moles to 298 K, 1.00 atm, and 0.300 moles, respectively. You may have to click on the Units button to change some of the variables to the correct units. Repeat the experiment with this gas labeling the data link ‘Real Gas N2.’

In experiment 3.11, we found out whether or not a larger amount of a liquid would get hotter when it boils. To answer this, we heated a specific amount of unknown liquid and recorded the temperature every fifteen seconds. In our scatter plot, we were able to find the boiling point of our liquid. We know that the slope of our graphs is when the liquid molecules were moving around and heating up. The plateau of our graph points is where the liquid started to evaporate and boil. This is were we found our boiling point at. Shantel and I decided that our boiling point was about 98º Celsius. If you had another slope in your graph, that was when you were simply heating the leftover gas. The histogram showed us that there were about equal amounts of data in the higher temperature (about 95º Celsius) bins for both 20mL of liquid and 10mL of liquid. Also, in the lower temperature bins (75º to 80º Celsius) there was about equal amount of data for 20mL of liquid and 10mL of liquid. There was 7 pieces of data for 10mL of liquid in the lower bins, and 6 pieces of data for 20mL of liquid. If a larger amount of liquid did have a higher boiling point, the clusters would be organized by volumes or amount. For example, all of the 20mL pieces of data would be in the higher temperature bins, and all of the 10mL pieces of data would be in the lower temperature bins or flipped. Rather, the bins were clustered by identity. The boiling point is a characteristic property.

Ionic and Covalent Bonding Ionic and covalent bonding is involved when the atoms of an element chemically combine to make their outer shells full and to make the atoms stable. The first type of bonding you can get is ionic bonding. Electrons are transferred from one atom to another to try and create full outer shells, this gain and loss of electrons on the atoms results in positive and negative ions. In these compounds you get electrostatic force, this is the force/attraction that occurs between the positive and negative ions that hold the compound together.

The purpose of the lab was to make observations and inferences, on how 2 types of packing material reacts to different liquids. In part one of the lab, 2 different types of packing material was placed in separate beakers of acetone and water. After a minute of stirring using the glass stirring rod, iodine, an indicator, was added to each beaker. In part 2, tin foil was rolled and placed in a solution of water and crystals. Observations were taken in all parts of the lab.

In the experiment four compounds were observed, two of which were ionic compounds. Compounds A and D were proven to be ionic, because both when tested resulted on the ionce end of the spectrum. First, when observing the appearance each when juxtaposed were strikingly similar. Compound A and D were each while, but more importantly formed as a crystal lattice and geometric shapes (cubes/rectangles), and this is blaringly a trait of ionic compounds. Secondly, when testing the electrical conductivity of compounds A and D once again both tested very highly, proving that they were highly conductive of electricity. These results in conductivity are congruent to those of ionic compound, once more corroborating that compounds A and D are in fact ionic.

The purpose of this lab was to study colligative properties. These properties are properties that are affected when a solute is added to a solvent. Thus, the amount is important, not the actual type of substance, for the colligative properties. A couple types of this property are the freezing point and boiling point of a substance. (1)

The objectives of this lab are, as follows; to understand what occurs at the molecular level when a substance melts; to understand the primary purpose of melting point data; to demonstrate the technique for obtaining the melting point of an organic substance; and to explain the effect of impurities on the melting point of a substance. Through the experimentation of three substances, tetracosane, 1-tetradecanol and a mixture of the two, observations can be made in reference to melting point concerning polarity, molecular weight and purity of the substance. When comparing the two substances, it is evident that heavy molecule weight of tetracosane allowed