The Alkaline Earths and the Halogens: Two Families in the Periodic Table

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

3. Examine the luster of the minerals in Figure 1.2 (p. 4 lab book). Place the letter A, B, C, D, or E in

Based the data collected, the identity of the unknown #42 is lithium chloride. Because the unknown compound produced a bright red pinkish flame, shown in Table 1, the possible cations based on the CRC Handbook were lithium or strontium 1.The known 1M lithium chloride also produced the same colored flame as the unknown, suggesting that the unknown compound has lithium. Since lithium produces no precipitate with the compounds in Table 2 and strontium produces a precipitate with the same compounds, the observations in Table 2 indicate that the unknown’s cation is lithium 4. Using the solubility table, process of elimination, and the results in Table 3 the possible anions for the unknown compound were chloride and bromide4. The production of precipitate

On your own: Continue to practice identifying minerals. (There are 26 samples in the Gizmo – A through Z.) Record your findings in your notebook or on separate sheets of paper.

We repeated this for a total of 6 known substances and 3 unknown substances. We also made a table for each element showing the color of the flame that we saw,

The first part of the Identification and Synthesis of an Unknown Ionic Compound (Project 3 Week 1) experiment was to determine the unknown compound #202 that is given to the experimenter. The second part to the experiment (Project 3 Week 2) was to discover different tests the experimenter can conduct in order to prove that they have the specific ionic compound that they discovered in part one. Some of the ways that the experimenter can determine the unknown compound #202 they have includes, preliminary tests, physical state tests, solubility testing, analysis of anions, analysis of cations and flame tests (Dealing with Unknown Compound). There are many ways an experimenter can determine the ionic compound that they have, including pH tests, flammability tests (liquids and solids), solubility tests and heavy metal tests, just to name a few (Identifying Unknown Chemicals in Science Labs).

the ions of SO42-, CO32-, Cl-, and I-,identify them separately, and use the observation to identify the unknown.

The purpose of this experiment is to identify the periodic trends in the solubility of the alkaline earth metals and compare the results to that of lead

Identifying an unknown substance can be accomplished with the use of multiple scientific tests, which help narrow down the possibilities of the unknown compound. The unknown substance that I was given was unknown number A84841BIR, and posed to be a real challenge since I needed to test two different molecular combinations for this specific substance. Once the number of moles in substance was calculated using the ideal gas law, I divided it from the sample mass number after heating and obtained that the molarity of my unknown chemical was 58.93 g/mol. To find my molecular formula I calculated the mass of each element, then the moles, lastly I took the smallest whole-number ratio. Using the molarity calculated I was able to do some research to get a better understanding about what my unknown chemical could possibly be. Once I’ve collected all my data together and strenuously researched the web for articles relating to understanding Infa-Red spectroscopy, I should be able to make an educated guess upon what my unknown solution could be.

At the beginning of Salt: A World History, the author, Mark Kurlansky, describes a pink rock he got in Spain. However, this rock is not just any ordinary rock. The rock was almost completely pure salt, with only a small bit of magnesium. It had many unique qualities, which fascinate the author. Firstly, white crystals started appearing on the pink after rain fell on the rock. The rock also produced brine puddles in humid weather. Yet, it never seemed to get any smaller. When the author placed the rock on a small copper tray, the rock produced a green crust that polished the copper. At first sight, the author thought the rock was just like any other, but after only a couple days, he knew it was something special.

Unknown 1 is sodium chloride(NaCl) which is ionic because sodium is a metal and chlorine is a nonmetal, unknown 2 is copper chloride(CuCl2), unknown 3 is citric acid(C6H8O7), and unknown 4 is sucrose(C12H22O11) which is also known as table sugar. From this information gathered from the facts, it can be concluded that unknown 1 and 2 are ionic, and 3 and 4 are covalent.

The objective of this experiment is to experimentally investigate which elements show similar chemical properties.

Mass Spectrometry Results: Observation: There is a pair of high masses values which peak at 78 m/z at an intensity of 1.5 and 80 m/z at an intensity of 0.5. Conclusion: The pair of peaks can be used to determine that the parent ion is Chlorine.

When holding the wire in the Bunsen flame, which had been previously dipped in the unknown solution, the edge of the flame appeared to emit a pale green color, which would indicate that our unknown sample would contain the element barium. This conclusion was incorrect and upon redoing the Flame test and making the unknown solution more concentrated by adding less water, it was found that the edge of the flame was actually pale violet in color, indicating that the element in our sample was potassium. Additionally, in week 1, our group encountered another error while analyzing the properties of our unknown sample through the anion tests. The two cation tests; Flame and Ammonium concluded that the first element in our compound was in fact potassium.

The start of the experiment consisted of filling up four beakers with de-ionized water to 150 ml. After the beakers were filled to the appropriate amounts they were then labeled with the