Ionic And Covalent Compounds Essay

The compound was tested for the presence of ammonium, carbonate, sulfate, chloride, and nitrate, as seen in Table 2. The nitrate test produced a precipitate, indicating the presence of the nitrate ion in the compound. At this point it was hypothesized that our unknown compound was calcium nitrate.

A topic of great importance to all scientists is the identification of compounds, which is relevant in all aspects of their work in some way shape or form. Weather it may be determining what is causing sickness or what is polluting the air, it is very prevalent in the science world. In project 2, identification of cations and anions was preformed through a series of confirmation and elimination tests that ultimately led to identifying an unknown ionic compound made of cations and anions.

In order to gently heat the sample, move the burner back and forth to achieve minimal heating. It is important to not overheat the sample. After heating the sample, turn off the burner and let the sample fully cool with the lid on top. After about ten minutes, lift the crucible lid and observe any changes that occurred to the sample. You must reheat the sample if there are blue-green crystals. Heat the sample until the crystals turn brown. After the sample has fully cooled, measure and record the mass of the crucible with the lid and sample.

There are three types of bonds ionic,polar, and nonpolar.Ionic bonds is between metals and nonmetals where the electrons are transferred.Polar bonds are between two nonmetals and they do not share electrons equally.Nonpolar two nonmetals share electrons equally. For example of NaCl is a ionic covalent.Na is 0.9 and Cl is 3.0. Subtract 3.0 and 0.9 and the difference is 2.1 for it to Ionic it has to be greater than 1.9.Also ionic is a nonmetal and a metal.CO2 is an example of 0% of ionic. C and O are both nonmetals. Oxygen is 3.5 and Phosphorus is 2.1. This is polar because 3.5- 2.1 is 1.4 . This is an example of intermediate degree. Another way to determine if a compound is polar, ionic or nonpolar is to test the melting point ,solubility in water, and conductivity.The purpose of this lab Bonding

After being further heated with the Bunsen burner the copper (II) sulfate hydrate starts to turn from a light blue coloring to a white coloring

An unknown compound was obtained and the ID number was recorded. A capillary tube was loaded with the unknown powder and inserted into the melting apparatus. The temperatures at which the crystals first started to liquefy and when the entire sample became liquid were recorded. The melting point was then compared with previous known mixture samples to identify the unknown compound.

* If the compound starts with a metal, it is most likely ionic. Use the naming binary ionic compounds rules.

Prepare the unknown anion solutions for the students to analyze from the four 0.2 M stock solutions of anions. Any combination of these four anions may be prepared. Using a graduated Beral-type pipet, add 2 mL of each ion selected to a 13 X 100 mm test tube. Add distilled water to give a total volume of 8 mL. Stopper the test tube. A matrix of combinations, similar to the cation unknowns, can be generated for the anions.

Identifying Substances Using Properties Purpose: To identify unknown substances by observing their physical and chemical properties (e.g. colour, state, clarity, crystal shape, behaviour in water, behaviour in acid), and comparing them to the physical and chemical properties of known substances. Hypothesis: I predict that by observing and testing the properties, as well as comparing them to those of known substances, we can identify all 5 of the unknown substances.

5. Record observation of whether it dissolved or did not dissolve, in the results table below; and repeat for the other 5 substances.

measure the adsorbent, fill the column one-half to two-thirds full, and then pour the powder into

Before I start the experiment, I predicted that all crystal form solutes would dissolve while powder form solutes will not, but my prediction was partially supported. A baking soda was a one that showed an unexpectedly result because even though it is in a powder form, it dissolved in the water. Except for a baking soda, everything could be observed from what I predicted. Sugar and salt, which are in a crystal form dissolved in water and had high solubility while flour and cornstarch, which are in a powder form didn’t dissolve and had low solubility.

From the following ionic compounds, choose the name-formula pair that is not correctly matched. (a) (b) (c) (d) (e) sodium sulfide ammonium nitrate zinc hydroxide sodium sulfate calcium oxide Na2S NH4NO3 Zn(OH)2 Na2SO3 CaO

Ionic bonds form by the nature of the atoms themselves. When the atoms chemically combine together, the atoms create a compound that has different properties. The electronegativity between the atoms in the bond determines what type it is. Atoms with higher electronegativity hold atoms more tightly than those with a lower electronegativity. Therefore, when two elements bond, they must fill each others orbitals to create a stable energy electron configuration. Each will have eight electrons in their outer energy. The solubility and bond type lab was to use the compounds solubility to predict the type of bond it contains. To determine so, I added sodium chloride to water in a test tube and some of it dissolved. When the sodium chloride was put

The first step me and my partner had to do was take a white chalk/or crayon and label the black construction paper into four sections (Baking Soda, Sugar, Salt, and Cornstarch). We did this so that it would be easier to know which powder is which. Continuing the first step, we then placed 1/4tsp (1ml) each of the four different white powders onto the black construction paper. To make things a little easier for me and my partner, we used a spatula to get the powders out of their container/bag. After using the spatula, we then poured it into the graduated beaker. Each powder had it’s own beaker. After measuring it and making sure it was 1/4tsp (1ml), we then poured it onto the black construction paper, underneath the labeled section. We knew that we would have to come