Chemical 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__

The purpose of this experiment was to explore the properties of chemical substances that can be used to identify the types of bonds in a chemical substance using a laboratory procedure. The two types of bonds being identified were ionic and covalent. Based on a substance’s properties, how can you determine whether its bonds are ionic or covalent? This is the question I posed before starting the experiment.

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

What is the percentage yield of the reaction of iron and copper chloride when steel wool and copper chloride dehydrate are used as reactions?

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

Substances A and B have an appearance of a white solid like. Substances A and B were put into a test tube and on the Bunsen burner. As a result, B melted faster than A. A was slow to melt. The reason why B melted faster than A is because it has a lower boiling point than substance A which made it melt faster. It also shows that A needs more energy than B to be broken down.

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.

In ionic bonding one atom transfers electrons to another, creating ions with differing electrical charge.

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

In this lab, students observed reactions, or lack thereof, between metals Mg, Cu, Zn, and Fe; when placed in solutions of Hydrochloric acid (HCl), Cu(NO3)2, Zn(NO3)2, Fe(NO3)3 and Mg(NO3)2. Students were tasked with observing whatever reaction took place and recording the characteristics of said reaction. To set up the lab, students placed a piece of each metal in a pocket on a spot plate. The plates had four pockets in a row, one for each metal, and 3 rows of pockets. Students would then put a solution in each of the rows and observe the effects of that particular solution on each metal.

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

The atoms are bound by shared electrons in a covalent bond. Even though they share electrons, they do not share them equally. Even though most of the time covalent bonding occurs between nonmetals, there have been times where this type of bonding occurs between a metal and a non metal. Covalent bonds are most likely to occur when molecules have a similar electro negativity level (Gray 76). Elements follow the octet rule because they are the most stable when they have eight electrons in their outer shell. Therefore, by sharing those electrons they fulfill the octet rule and the noble gas configuration. Another way covalent bonds satisfy the octet rule is too form single, double, and triple bonds. It’s easy to differentiate between those bonds, for example a single bond is when two atoms share one pair of electrons, a double bond is when two atoms share two pairs of electrons, and a triple bond is when two atoms share three pairs of electrons. Bond order and length are used to describe the strength of covalent bonds; they both have a direct relationship. Bond order is the amount of bonded pairs between two atoms. Bonding length is the distance between two covalent bonds. Compared to ionic bonds, covalent bonds are have a lower melting and boiling point. They are also less likely to dissolve in water. Not all the pairs of the molecules have the same characteristics. When a pair is not sharing any electrons, that pair is called a lone pair. When a pair is sharing electrons, they are called a bond pair. And finally, a Lewis dot structure is a great way to illustrate a covalent

Ionic compounds and covalent compounds have many similarities and differences. Ionic compounds are only formed with metals and non-metals. Covalent compounds are formed with non-metals. Ionic compounds have an overall neutral charge, but covalent compounds don’t have charge. Ionic compounds are formed when non-metals take electrons from metals. This gives both of them noble gas configuration. Covalent compounds are formed by two non-metals sharing their unpaired electrons, so they can mutually have noble gas configuration. What properties do compounds form when forming ionic and covalent bonds?