Ramila Izzayeva - Lab Notebook

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Chemistry

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Feb 20, 2024

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Name: Ramila Izzayeva College: Gwinnett Technical College Course: Inorganic Chemistry Lab 29779 Start Date: August 13, 2023, End Date: October 2, 2023 pg. 1

Table of Contents: Experiment # Experiment Title Pg. # Experiment Date: 1 Density of Liquids and Solids Lab 6-9 8/2 2 Families of Elements Lab 10-12 8/22 3 Chemical Reactions Lab 13-15 9/18 4 VSEPR Theory Lab 16-18 9/15 pg. 2

Reference Sheets pg. 3

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Reference Sheets pg. 4

Reference Sheets pg. 5

Additional Notes/ References: https://www.youtube.com/watch?v=Q8DRfs5D4ds (This is the link I used to create a scatter chart) Observations: For the unknown liquid identification: Appearance: The unknown liquid looked like a clear and transparent liquid. It didn't have any visible particles, and its appearance remained consistent throughout the experiment. Smell: The liquid had no distinct smell. It didn't have a strong or unpleasant odor; it was quite neutral in terms of scent. Thickness: The liquid flowed smoothly and easily, like water. It didn't have a thick or syrupy consistency. Reactions: The liquid did not exhibit any unusual reactions with the air or surroundings. It didn't evaporate quickly or change color during the experiment. For the known liquids (water and vegetable oil) and objects (marbles and chalk): Looks: Water appeared clear and colorless, while vegetable oil had a slightly yellowish color. Both liquids were transparent and did not have any visible impurities. Objects: When marbles were placed in water, they sank to the bottom. In contrast, when chalk pieces were added to water, they floated on the surface. In vegetable oil, both marbles and chalk pieces floated. For plotting density to find the unknown: Graph Plot: The graph showed a clear pattern, but the volume of the liquid increased, the mass also increased. By drawing a line through these points, we could determine the density of the unknown liquid. The slope of the line represented the density value. Calculations: Unknown liquid 3 Using graduated pipette to take out liquid. The tare weight of 50mL graduated cylinder is 53.0868g. 10mL: The total weight of cylinder and 10mL liquid is 62.1356g. The weight of the unknown liquid 62.1356g- 53.0868g=9.0488g D= 9.0488g/10mL= 0.90488g/mL 20mL The total weight of cylinder and 20mL liquid is 72.8114g The weight of the unknown liquid 72.8114g-53.0868g=19.7246g D= 19.7246g/20mL= 0.98623g/mL 30mL The total weight of cylinder and 30mL liquid is 83.3493g The weight of the unknown liquid 83.3493g-53.0868g= 30.2625g D= 30.2625g/30mL= 1.00875g/mL 40mL The total weight of cylinder and 40mL liquid is 93.8121g The weight of the unknown liquid 93.8121g-53.0868g= 40.7253g D= 40.7253g/40mL= 1.0181325g/mL 50mL The total weight of cylinder and 50mL liquid is 104.5107g pg. 6

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The weight of the unknown liquid 104.5107g-53.0868g= 51.4239g D= 51.4239g/50mL= 1.028478g/mL D avg of unknown liquid: 0.9892941g/mL Mountain dew: 1.035g/mL Using 10mL volumetric pipette to take out the liquid. The tare weight of 100mL beaker is 62.7454g 10mL: The total weigh 72.2145g. The liquid weight 9.4691g. 20mL: The total weight 82.6191g. the liquid weight 19.8737g 30mL: The total weight 93.0125g. The liquid weight 30.2671g 40mL: The total weight 103.3960g. The liquid weight 40.6506g. 50mL: The total weight 112.6227g. The liquid weight 49.8773g The tare weight of beaker 48.6165g. Pour 10mL liquid from 10mL cylinder to the burette. Dispense the liquid from burette to beaker. 10mL: The total weight 57.9636g. The liquid weight 9.3471g 20mL: The total weight 67.7786g. The liquid weight 19.1621g 30mL: The total weight 77.5059g. The liquid weight 28.8894g 40mL: The total weight 87.4350g. The liquid weight 38.8185g 50mL: The total weight 97.4545g. The liquid weight 48.8380g Determine the Density of a Known Liquid and Solid Water The weight of 100mL cylinder: 142.87g the weight of cylinder with 20mL water: 161.02g the mass of water: 18.15g Density of liquid 18.15g/20mL= 0.9075g/mL The weight of marble 5.8835g The weight of clip 0.3998g The weight of chalk: 1.8718g The volume of marble with 20mL water: 21mL. Volume of marble: 21mL-20mL= 1mL Density of marble= 5.8835g/1mL= 5.8835g/mL (g/cm3) The volume of chalk, marble and 20mL water: 22mL Volume of chalk: 22mL-21mL=1mL Density of chalk= 1.8718g/1mL= 1.8718g/mL (g/cm3) The volume of clip, chalk, marble and 20mL water: 22.1mL Volume of clip: 22.1mL-22mL= 0.1mL Density of clip= 0.3398g/0.1mL= 3.3398g/mL (g/cm3) Veggie oil, the tare weight of 100mL cylinder: 103.58g pg. 7

The weight of 20mL oil with cylinder: 121.83g The weight of 20mL oil: 121.83g-103.58g= 18.25g Density of oil= 18.25g/20mL= 0.9125g/mL The clip weight 0.4579g the chalk weight 1.7732g The marble weight 6.2302g The volume of marble with 20mL oil: 23mL Volume of marble: 23mL-20mL= 3mL The density of marble= 6.2302g/3mL= 2.0767g/mL (g/cm3) The volume of chalk, marble and 20mL oil: 25mL Volume of chalk: 25mL-23mL= 2mL The density of chalk: 1.7732g/2mL= 0.8822g/mL (g/cm3) T he volume of chalk, marble, clip and 20mL: 25.1mL Volume of clip: 25.1mL-25mL= 0.1mL The density of clip: 0.4579g/0.1mL= 4.579g/mL (g/cm3) Data: 5 10 15 20 25 30 35 40 45 50 55 0 10 20 30 40 50 60 Finding Density of Unknown Volume (mL) Mass (g) Also, we used the D=M/V equation to figure out the density. pg. 8

Lab Date: August 22, 2023 Exp. Title: Density of Solids & Liquids Lab Objective: We want to find out what a mystery liquid is by checking how dense it is using different tools. Being precise is super important to figure out what the liquid is. We'll also see how good these tools are at measuring density accurately. Protocol: Start by picking one of the six containers with an unknown liquid in it, about 70 mL. Get a 50 mL beaker or a graduated cylinder and weigh it empty. This will help us figure out the weight of just the liquid later. Pour 10 mL of the mystery liquid into the beaker and write down how heavy it is. Keep adding 10 mL more of the liquid and writing down the weight each time until you've added 50 mL in total. Don't throw away the leftover liquid; we'll need it soon. Now, take another empty container (like a beaker) and weigh it after finding out how much it weighs when it's empty. Then, use a special tool (a 10 mL pipet) to take out 10 mL of the mystery liquid you saved earlier and put it in the container. Write down how heavy it is. Keep adding the liquid in 10 mL portions and writing down the weight each time until you've added 50 mL in total. Remember, keep the leftover liquid for later. Now, set up a special stand with a clamp and attach a tube (a 50 mL buret) to it. Make sure a little valve on the tube is closed (turned sideways). Put a funnel at the bottom of the tube. Find out how heavy another empty container (like a beaker) is. Fill the tube up to a special line marked "0 mL" with the mystery liquid you saved. Write down exactly how much liquid you put in there. Now, let out 10 mL of the liquid from the tube into the container and write down how heavy it is. Keep letting out the liquid in 10 mL parts and writing down the weight each time until you've let out 50 mL in total. By doing all this, we can figure out the density of the unknown liquid by measuring its weight at different amounts. Results: In our experiment, we measured the heaviness of things and how much space they take up. This helps us find out how tightly packed the stuff is inside them, which we call density. We found out how dense the mystery liquid is by measuring how heavy it is for a given amount of space. We also figured out the densities of water, vegetable oil, marbles, and chalk. Our results matched what we expected. Different things have different densities, and denser stuff has more matter squeezed into a small space. Sometimes, our measurements might not be perfect. The tools we used might not be super exact, which can affect our measurements. Temperature changes can slightly change the density of liquids, which could affect our results. Small mistakes in writing down numbers or measuring liquids could make our results a bit off. To see how close our measurements are to what we expected, we can calculate something called "percent error." If the percent error is small, it means our measurements are pretty accurate. So, by considering possible mistakes and calculating percent error, we can tell if our density measurements are on target or not. Conclusion: In our experiment, we followed a step-by-step procedure to measure the density of an unknown liquid. By comparing the measured density to known values, we successfully identified the unknown liquid as mountain dew. We also determined the densities of other substances: vegetable oil, marbles, and chalk. Our results matched our expectations based on the theory of density. While there were minor sources of error, such as pipette precision and possible measuring mistakes, our measurements provided accurate density values. pg. 9

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Lab 2 Observations: During the flame tests, we observed the colors of flames when various metal ions were introduced into the flame: Barium Chloride (BaCl2): The flame turned green. Potassium Chloride (KCl): The flame turned lilac or pale purple. Lithium Chloride (LiCl): The flame turned crimson or deep red. Copper (II) Chloride (CuCl2): The flame turned blue green. Strontium Chloride (SrCl2): The flame turned red. Using a cobalt glass as a filter, we observed the colors more distinctly. Precipitation Test with Known Cations: In the precipitation tests, we mixed different metal ions with specific anions to check for the formation of solid precipitates: Barium Chloride (BaCl2) + Sodium Carbonate (Na2CO3): A white precipitate formed. Potassium Chloride (KCl) + Sodium Phosphate (Na3PO4): No visible reaction occurred. Lithium Chloride (LiCl) + Sodium Sulfate (Na2SO4): No visible reaction occurred. Copper (II) Chloride (CuCl2) + Sodium Carbonate (Na2CO3): A greenish-blue precipitate formed. Strontium Chloride (SrCl2) + Sodium Carbonate (Na2CO3): A white precipitate formed. Halide Tests of Known Solutions: In the halide tests, we mixed different sodium halide solutions with reagents to observe the color of the upper hexane layer: Sodium Bromide (NaBr): The hexane layer turned orange. Sodium Chloride (NaCl): The hexane layer turned yellow. Sodium Iodide (NaI): The hexane layer turned pink. Identification of an Unknown Solution: Using the flame test, we identified the cation in the unknown solution as barium (Ba). The precipitation test indicated the presence of chloride ions (Cl) in the unknown solution. Overall, these observations helped us identify the unknown solution as containing barium cations and chloride anions. Calculations: We had no calculations for this lab. pg. 10

Data: pg. 11

Lab Date: Families of Elements Lab Exp. Title: August 28, 2023 Objective: We want to figure out what a mystery substance is by doing tests with other substances that are similar in the periodic table. We're going to see how the mystery substance reacts compared to these similar substances to find out what it is. Protocol: In this experiment, we're doing different tests to find out what a mystery substance is. First, we use a flame test to see what color the flame turns when we put the mystery substance in it. We also use a special glass to help us see the colors better. Then, we mix the mystery substance with some other substances to see if they make a solid appear or change color. This helps us figure out what's in the mystery substance. Next, we test the mystery substance with some chemicals to check if it contains certain things. Finally, we compare the mystery substance to known substances to see if we can match them up. Results: From our experiments, we learned, when we put different metals in a fire, they made the fire change colors. For example, barium made the fire green, potassium made it lilac, lithium made it crimson, copper made it blue-green, and strontium made it red. We used a special glass to see the colors better. When we mixed certain metals with other stuff, some turned into solid bits, and some didn't change at all. For our mystery liquid, we found out it has barium in it because the fire turned green. We also saw that it has chloride in it because of the solid bits. So, our conclusion is that the mystery liquid contains barium and chloride. These tests show that simple experiments can help us figure out what unknown stuff is based on how it reacts. Conclusion: In our experiment, we did tests to find out what unknown things were. We found that different metals make fire change colors in a special way. For example, barium made the fire green, potassium made it purple, lithium made it red, copper made it blue-green, and strontium made it red. We used a special glass to help see these colors better. We also mixed metals with other stuff, and sometimes it turned into solid bits. Our mystery liquid had barium and chloride in it because the fire turned green, and there were solid bits. So, what we learned is that simple tests can help us figure out what unknown stuff is based on how it acts. These tests can be used in real life, like in crime investigations, checking water for pollution, or making sure chemicals are right in factories. The goal of this lab was to identify unknown substances using various tests and observations. These tests included flame tests to see how substances change the color of a flame, precipitation tests to check if mixing substances creates solid particles, and other chemical tests to reveal the presence of specific elements in the unknown substances. pg. 12

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Lab 3 Additional Note & References… N/A Observations: Reaction 1 - Combustion and Combination: When you burn the magnesium ribbon, you will see it glowing brightly and producing a white powder. Reaction 2 - Decomposition: When you heat the copper sulfate crystals, you'll notice them changing color, from blue to white, and they release some smoke. Reaction 3 - Single Displacement: After mixing copper wire with silver nitrate, the copper wire getting covered with a silvery substance, while in the other test tube with magnesium and hydrochloric acid, see bubbles forming. Reaction 4 - Double Displacement: When you mix sodium carbonate with different metal nitrates, you see a cloudy or milky substance forming in some of the test tubes. Reaction 5 - Double Displacement: Mixing acids with sodium hydroxide led to color changes. For example, the solution turns red when adding sodium hydroxide to nitric acid. Calculations: We didn’t have any numerical data for this lab. Data: pg. 13

Experiment Date: September 15, 2023 Experiment Title: Chemical Reactions Lab Protocol: Reaction 1 - Burning Magnesium: Connect a Bunsen burner to the gas and light it. Place something called a Thermoplate near the flame to keep things safe. Cut a small piece of magnesium. Hold the magnesium in the flame and see what happens. Put the hot magnesium in a beaker to cool. Turn off the Bunsen burner when you're done. Reaction 2 - Changing Copper Sulfate: Take a few crystals of blue stuff called copper sulfate and put them in a test tube. Heat the test tube with a flame (the same Bunsen burner). Notice what happens as it heats up. Rinse the test tube with water to clean it. Reaction 3 - Mixing Copper and Magnesium: Get two test tubes. Put a piece of copper in one and magnesium in the other. Add silver nitrate to the copper and hydrochloric acid to the magnesium. Wait and watch what's going on in both test tubes. Reaction 4 - Mixing Sodium Carbonate with Different Liquids: Take three test tubes and add sodium carbonate to each. Add different liquids like silver nitrate, copper nitrate, and aluminum nitrate to the test tubes. See if anything interesting happens in each test tube. Reaction 5 - Mixing Acids and Sodium Hydroxide: Set up three test tubes in a row. Add acids like nitric acid, sulfuric acid, and phosphoric acid to them. Put a special drop of something called phenolphthalein in each. Slowly add sodium hydroxide to each test tube and count how many drops it takes to change the color. pg. 14

Results: Result 1 - Burning Magnesium: When we put the magnesium in the flame, it produced a very bright and white light. It looked like a sparkler or fireworks. After it burned, we had a white powder left behind in the beaker. Result 2 - Changing Copper Sulfate: The blue copper sulfate crystals turned into a white powder when we heated them. It lost its blue color and changed into a different substance. Result 3 - Mixing Copper and Magnesium: In the test tube with copper and silver nitrate, we saw a brownish- red stuff forming. But with magnesium and hydrochloric acid, we noticed bubbles and fizzing. Result 4 - Mixing Sodium Carbonate with Different Liquids: When we mixed sodium carbonate with silver nitrate, it formed a white solid at the bottom. With copper nitrate, we saw a blue solid. But with aluminum nitrate, nothing really happened. . Result 5 - Mixing Acids and Sodium Hydroxide: We added sodium hydroxide to the test tubes with acids. In the first one with nitric acid, it turned pink after a few drops. In the second one with sulfuric acid, it turned cloudy. The third one with phosphoric acid turned cloudy too, but it took more drops. \ Conclusion: We observed the combustion of magnesium, decomposition of copper sulfate, single displacement reactions with copper and magnesium, double displacement reactions involving sodium carbonate, silver nitrate, copper nitrate, and aluminum nitrate, and the reaction between different acids and sodium hydroxide. These findings are essential for building a strong foundation in chemistry and have practical applications in fields such as pharmaceuticals, materials science, and environmental science. Overall, this protocol was a valuable learning experience that enhanced our knowledge of chemical reactions and their significance in the world around us. pg. 15

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Additional Notes/References:  PhET Interactive Simulations o https://phet.colorado.edu/sims/html/molecule-shapes/latest/molecule-shapes_en.html  PubChem Data Bank o https://pubchem.ncbi.nlm.nih.gov  Electronegativity o https://ptable.com/#Properties/Electronegativity Observations In our lab, we looked at different molecules and ions to understand how they're put together and what makes them tick. We drew pictures (called Lewis structures) to show how the atoms were connected and how their electrons were spread out. Sometimes, we noticed that atoms didn't always follow the eight- electron rule. We also figured out how electrons were grouped and predicted the shapes of the molecules. To really see what these molecules looked like in 3D, we used a special kit. We even checked to see if the bonds between atoms had a plus and minus side. Overall, we learned whether the molecules were kind of like magnets, with one end being more positive and the other more negative. Our observations helped us understand how these tiny building blocks of matter come together to make different substances. Calculations: N/A, we focused more on shapes. Data: pg. 16

Experiment Date: September 18, 2023 Experiment Title: VSEPR Theory Lab Protocol: In this lab, we'll work with different chemicals: a. SiO2 b. SnCl2 c. PBr3 d. CH2O e. CH2I2 f. NH4+ b. Drawing Lewis Structures: For each of these compounds and ions, we need to draw their structures on paper. Think of it as making diagrams of how their atoms are connected to each other. We also check if there are any special cases where atoms don't follow the usual rules for bonding. Counting Electrons: We'll count how many electrons each atom brings to the party and add them up for the whole compound. Bonding and Nonbonding Pairs: We'll figure out how these electrons pair up in the compound – some will form bonds, and others won't. Electron-Pair Geometry: Based on the number of electron groups, we'll predict the overall shape of the molecule. Molecular Geometry: We'll predict the 3D shape of the molecules and their bond angles. To help with this, we can use a molecular modeling kit to build physical models. Checking Bond Polarities: We'll look at how electrons are shared between atoms to determine if the bonds are polar (with a positive and negative end). Overall Molecular Polarity: Finally, we'll see if the entire molecule is polar or not. If it is, we'll figure out in which direction the polar part points. Results: SiO2: Lewis Structure: It forms a covalent network structure where each silicon atom is bonded to two oxygen atoms. Electron-Pair Geometry: Tetrahedral. Molecular Geometry: Tetrahedral. Bond Polarities: Polar due to the difference in electronegativity between Si and O. SnCl2: Lewis Structure: One tin (Sn) atom bonded to two chlorine (Cl) atoms. Electron-Pair Geometry: Trigonal planar . Molecular Geometry: Bent or V-shaped. Bond Polarities: Polar due to the difference in electronegativity between Sn and Cl. PBr3: Lewis Structure: Phosphorus (P) bonded to three bromine (Br) atoms. Electron-Pair Geometry: Tetrahedral. Molecular Geometry: Trigonal pyramidal. Bond Polarities: Polar due to the difference in electronegativity between P and Br. CH2O (Formaldehyde): Lewis Structure: Carbon (C) bonded to two hydrogen (H) atoms and one oxygen (O) atom. Electron-Pair Geometry: Trigonal planar. pg. 17

Molecular Geometry: Bent. Bond Polarities: Polar due to the electronegativity difference between C and O. CH2I2: Lewis Structure: Carbon (C) bonded to two hydrogen (H) atoms and two iodine (I) atoms. Electron-Pair Geometry: Tetrahedral . Molecular Geometry: Tetrahedral. Bond Polarities: Polar due to the difference in electronegativity between C and I. NH4+ (Ammonium ion): Lewis Structure: Nitrogen (N) bonded to four hydrogen (H) atoms with a positive charge on N. Electron-Pair Geometry: Tetrahedral. Molecular Geometry: Tetrahedral. Bond Polarities: Polar due to the difference in electronegativity between N and H. Conclusion: In summary, this experiment helped us learn more about how molecules are shaped and whether they are polar or not. We figured out the structures of different compounds and ions and how the atoms in them are connected. By doing this, we found that if some atoms in a molecule really like electrons, they can make the molecule polar. This information isn't just for science class; it's useful in jobs where people work with chemicals, like making better products and processes. So, this experiment taught us important things about molecules and how they can be important in real life. pg. 18

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