Lab #4 Chemical Names and Formulas Lab Report Purpose: The purpose of this lab is to observe the colors and textures of several ionic compounds, also known as precipitates and to learn how to properly write names and formulas of chemical and ionic compounds. This lab will help us develop our knowledge of distinguishing cations and anions in ionic compounds, familiarize ourselves with how to write the chemical formulas and names of ionic and chemical compounds, observe the physical properties of the precipitates formed from chemical compounds, and overall build a better understanding of the structure of ionic and chemical compounds. Understanding the structure of ionic compounds can help us figure out the name of an ionic compound using their formula, or their formula using their name. In this lab, we will observe the colors and textures of the precipitates (ionic compounds) by putting 2 drops of each chemical compound given on their corresponding reaction table squares and then mixing the different chemical compound drops on the squares together by blowing air with the blower pipette to form and observe the precipitates. Material List: ● Pipette of Silver Nitrate: AgNO 3 ● Pipette of Lead II Nitrate: Pb(NO3)2 ● Pipette of Copper II Sulfate: CuSO4 ● Pipette of Magnesium Sulfate: MgSO4 ● Pipette of Iron III Chloride: FeCl3 ● Pipette of Potassium Iodide: KI ● Pipette of Sodium Hydroxide: NaOH ● Pipette of Sodium Carbonate: Na2CO3 ● Pipette of Sodium Phosphate: Na3PO4 ● Bins of water (2) (One with soap water, one with just water) ● Blower Pipette ● Red/Blue cup to contain the pipettes (1) ● Plastic sheet protector (1) ● Reaction sheet (1) ● Paper towels (2) Safety Precautions: There are several safety precautions you should be aware of to keep yourself and your peers safe from harm during this lab. Eye Goggles and a Lab Apron should be worn at all times. They will keep your body, eyes, and clothes safe while performing lab experiments from chemicals, glass, and other potential dangers to your health, which in this case are chemical compounds stored in pipettes. These chemicals could potentially have a toxic and irritant effect on us, so be careful when handling them. When putting drops of the chemical compounds onto the reaction sheet, do it carefully so the chemicals don’t spill outside of their designated X square. Make sure when the pipettes are in the cup, the tips of the pipettes are facing upwards and don’t let the tips come into contact with each other when putting drops of chemicals onto the X squares and when mixing them with the blower pipette to prevent contamination and change of results. In addition, safely dispose of the precipitates formed from the chemical compounds by soaking them up with two paper towels, wiping the towels thoroughly across the reaction sheet, and throwing the towels into the trash can. In addition, thoroughly wash and clean the sheet protector that covers the reaction sheet to prevent contamination. Lastly, when returning the pipettes back to their designated cups, make sure the tips face upward to prevent contamination. Procedures: 1. Grab a blue or red cup and pick up a blower pipette and each of the pipettes containing Silver Nitrate: AgNO 3, Lead II Nitrate: Pb(NO3)2, Copper II Sulfate: CuSO4, Magnesium Sulfate: MgSO4, Iron III Chloride: FeCl3, Potassium Iodide: KI, Sodium Hydroxide: NaOH, Sodium Carbonate: Na2CO3, and Sodium Phosphate: Na3PO4 and place them into your cup where the tips face upward to prevent contamination. 2. Grab a reaction sheet, a sheet protector, and bring them with the cup with the pipettes back to your table. (if the sheet protector is dirty, dip it inside the water bin without getting water inside the protector, and dry it completely with a paper towel) 3. Put the reaction sheet inside your sheet protector and place it on a hard and sturdy surface with a lot of space around it so you don’t confine yourself and cause risk of potential chemical spills. 4. Place the chemical compound pipettes to where they correspond with the names on the reaction sheet by placing the Iron III Chloride, Potassium Iodide, Sodium Hydroxide, Sodium Carbonate, and Sodium Phosphate pipettes in a horizontal position to their name, placing them below each other in that order. (make sure the tips don’t touch with each other to prevent contamination) 5. Repeat step 4 with Silver Nitrate, Lead II Nitrate, Copper II Sulfate, and Magnesium Sulfate but place them in a vertical position from left to right in that order. (the Iron III Chloride pipette is already placed before) 6. Put two drops of Silver Nitrate and two drops of Iron III Chloride on the top left X square corresponding with their names on the sides. 7. Repeat step 6 for the other chemical compounds with their corresponding names and X squares. 8. Put the pipettes back into the red/blue cup with their tips facing upwards. 9. Mix the two drops of Silver Nitrate and the two drops of Iron III Chloride together by blowing steady air from the blower pipette until the chemical drops coagulate into a solid. 10. Repeat step 9 for the rest of the chemical drop combinations on the X squares on the reactive sheet. 11. Record and observe the colors and textures of each of the newly formed ionic compounds. 12. Get two paper towels and lay them over the entire reactive sheet to soak up all the compounds. 13. Wipe the reactive sheet with the paper towels thoroughly to clean up all the compounds and throw the paper towels away in the trash can. 14. Remove the reactive sheet paper from the sheet protector, dip the sheet protector into the soap water bin to clean any extra compound residue off, use a paper towel to dry off the sheet protector, and place the sheet protector back where it came from. 15. Return the pipettes containing the chemical compounds back to their designated cups with the tips facing upwards and return the cup back to where it came from. Data: Table 1: Potassium Iodide Sodium Chloride Magnesium Sulfate Copper II Sulfate KI NaCl MgSO4 CuSO4 NaHCO3 AgNO3 NaNO2 KF Sodium Bicarbonate Silver Nitrate Sodium Nitrite Potassium Fluoride Sodium Carbonate Lead II Nitrate Sodium Acetate Ammonium Chloride NaCO3 Pb(NO3)2 NaC2H3O2 NH4Cl Sodium Phosphate Calcium Hydroxide Tin IV Chloride Potassium Bromide Na3PO4 Ca(OH)2 SnCl4 KBr CaCl2 FeCl3 Na2HPO4 NaH2PO4 Calcium Chloride Iron III Chloride Sodium Hydrogen Phosphate Sodium Dihydrogen Phosphate Table 2: AgNO3 Ag+ Pb(NO3)2 Pb2+ FeCl3 (Cl- ) Silver Chloride AgCl Color: Light Orange Texture: Flaky Lead II Chloride PbCl2 Color: Light Orange Texture: Grainy KI (I- ) Silver Iodide AgI Color: Light Yellow (Creamy White) Texture: Milky Lead II Iodide PbI2 Color: Bright Yellow Texture: Grainy CuSO4 Cu2+ MgSO4 Mg2+ FeCl3 Fe3+ NaOH (OH- ) Silver Hydroxide AgOH Color: Brown Texture: Flaky Lead II Hydroxide Pb(OH)2 Color: White Texture: Copper II Hydroxide Cu(OH)2 Color: Green Texture: Magnesium Hydroxide Mg(OH)2 Color: White Texture: Iron III Hydroxide Fe(OH)3 Color: Dark Orangish Milky Gelatinous Cloudy Brown Texture: Grainy Na2CO3 (CO3 2-) Silver Carbonate Ag2CO3 Color: White Texture: Grainy Lead II Carbonate PbCO3 Color: White Texture: Milky Copper II Carbonate CuCO3 Color: Emerald Green Texture: Cloudy Magnesium Carbonate MgCO3 Color: White Texture: Grainy Iron III Carbonate Fe2(CO3)3 Color: Dark Orangish Brown Texture: Cloudy Na3PO4 (PO4 3-) Silver Phosphate Ag3PO4 Color: Olive Green Texture: Grainy Lead II Phosphate Pb3(PO4)2 Color: White Texture: Grainy Copper II Phosphate Cu3(PO4)2 Color: Neon Blue (Turquoise) Texture: Flaky Magnesium Phosphate Mg3(PO4)2 Color: White Texture: Cloudy Iron III Phosphate FePO4 Color: Light Orangish Yellow Texture: Cloudy Observations: I observed that all of the chemical substance drops took some time to coagulate into ionic compounds and it required a lot of air from the blower pipette to help it coagulate. In addition, all of the chemical drops changed completely in a physical and chemical stance because the chemical drops combined to create a completely new ionic compound. For example, when Sodium Phosphate and Copper II Sulfate combined, they created a completely new blue ionic compound called Copper II Phosphate which is different in chemical and physical structure in terms of combinations of ions and the color from the two previous chemical substances. All the substances had ranging changes from becoming grainy, flaky, cloudy, gelatinous, etc. and ranging in different colors. Questions: 1. Write the formulas (with charges) and names of all the cations represented in this experiment: Silver: Ag + Lead II: Pb2+ Copper II: Cu2+ Magnesium: Mg2+ Iron III: Fe3+ 2. Write the formulas (with charges) and names of all the anions represented in this experiment: Chloride: ClIodide: IHydroxide: OHCarbonate: CO3 2Phosphate: PO43- 3. Write some simple rules for naming ionic compounds: Ionic compounds are composed of positive ions (cations) and negative ions (anions). The first name of the ionic compound is determined from the cation, while the second name of the ionic compound is determined from the anion. Anions that are monatomic make the second name of the ionic compound the name of the element with the suffix ending of -ide. Anions that are polyatomic make the second name of the ionic compound the name of the polyatomic ion. 4. When are the Roman numerals used in naming compounds? Roman numerals are used in naming compounds when the cation of an ionic compound has more than one ion and charge. 5. What does a subscript following an element in a chemical formula mean? A subscript following an element in a chemical formula means the number of the monatomic ions that are present in the chemical substance. 6. What does a subscript following a set of parentheses in a chemical formula mean? A subscript following a set of parentheses in a chemical formula means the number of polyatomic ions that are present in the chemical substance. 7. Write some simple rules for writing the formulas for ionic compounds? Some simple rules for writing the formulas for ionic compounds are to write the charges of cations and anions as subscripts on the top right of their symbol. The subscripts are used to identify the number of cations or anions there are depending on what part of the chemical formula the subscript is located. In addition, some other rules are to put parentheses around the polyatomic ion groups if they have more than one ion and the charge of the cation must be equal to the charge of the anion so they cancel out with each other to equal zero. If the cation and anion by themselves can’t balance out each others’ charges, subscripts can be added to help them balance out their charges. Conclusion: In this lab experiment, we mixed different drops of chemical compounds together to form ionic compounds by dropping two drops of each chemical compound on their designated X squares on a reaction sheet and mixed them by blowing air with an empty pipette. We also observed the colors and textures of the ionic compounds. We also observed how reactions happen when cations and anions from different chemical compounds come together to form new ionic compounds. This lab was done so we can better understand the structure of ionic compounds, specifically their cations and anions, so we can write chemical formulas of ionic compounds based on their names, and vise-versa. In this lab we mixed two drops of cations from some chemicals with two anions from some other chemicals. We found that the cations and anions would form a completely new substance with new textures and colors from their original counterparts. For example, two chemical compounds we combined in this lab were Sodium Phosphate and Copper II Sulfate. Copper II Sulfate was in liquid form and it was blue, while Sodium Phosphate was in liquid form and white. When combined, the cation from Copper II Sulfate and the anion from Sodium Phosphate formed to create the ionic compound Copper II Phosphate which coagulated into a solid and it turned neon blue (turquoise). This shows that cations and anions from different chemical substances will ultimately combine to create a new ionic compound that’s different from two original substances. In addition, I observed trends in the colors and textures of the ionic compounds that we created. For example, substances with the Cu2+ cation resulted in ionic compounds with a blue greenish color to them such as Copper II Phosphate and Copper II Hydroxide, and ionic compounds with the Pb2+ cation were either grainy or milky in texture such as Copper II Phosphate and Copper II Carbonate. These results overall show that the combination of cations and anions from different chemical compounds will result in an entirely new ionic compound, but will show consistency throughout in terms of color or texture depending if the ionic compounds have a consistent cation or anion in each of them. Some uncertainties I had in this lab were when determining the textures of some ionic compounds and if I mixed enough air into the ionic compound for it to completely coagulate. For example, my partner and I were debating on whether Lead II Phosphate was milky or grainy. To make sure, I mixed more air into the Lead II Phosphate compound to see if it would coagulate more, and we noticed that there were some grains forming. This could potentially mean that we might not have blown enough air into some of the ionic compounds or mischaracterized the textures of some of them, which would affect our results. Some questions I have are what would happen if the cation and anions in ionic compounds swapped charges and what would happen if a compound had two cations or two anions instead of one of each? From this lab, I have learned about the structure of ionic compounds and how to name and write the formulas for ionic compounds based on their cations and anions. In addition, I discovered that cations and anions react to form a completely new ionic compound that’s different from the two original chemical compounds with unique colors and textures. I also learned that if substances have consistent cations or anions in their structure, they will show a consistent color or texture in each of them. Overall, I understand the concept of ionic compounds more in depth and how cations and anions affect the ionic compounds they form.