Unit 2, Lab 1: Flame Test
Name: Date:
Lab Results
Compounds |
Flame Color |
lithium |
|
strontium |
|
calcium |
|
magnesium |
|
zinc |
|
copper |
|
barium |
|
manganese |
|
lead |
|
bismuth |
|
arsenic |
|
potassium |
Conclusions
Explain a reason why a flame test would not match the expected colors listed in the background
III. Flame and Precipitation Tests of Metals A. Metal Tested Flame Test Color Precipitation Results barium solution calcium solution copper solution lithium solution potassium solution sodium solution strontium solution B. Unknowns Unknown number (even number) Flame Test Color Precipitation Results Formula of unknown Name of unknown Unknown number (odd number) Flame Test Color Precipitation Results Formula of unknown Name of unknown
Compare the flame test and solution reaction observations for the unknown to the observations for the known solutions. Identify the metal present in your unknown solution and circle it below. Strontium Sodium Lithium Potassium Barium Calcium Report Sheet Questions For 1) and 2) below use all six metals (from above), but use each only once. 1. A fireplace log is available for the holiday season that burns with a green and red flame. Based on your observations, which elements produce...
Material science class Suppose 1 at % of the following elements is added to aluminum (forming a separate alloy with each element) without exceeding the solubility limit. Which one of the following would be expected to give the higher strength alloy. Mn: Ga: Be; or Li? The Atomic and lonic Radii of Selected Elements Valence Element Aluminum Antimony Arsenic Barium Beryllium Bismuth Boron Bromine Cadmium Calcium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Fluorine Gallum Germanium Atomic Radius (A) 1.432...
Pre-Lab Study Questions Name Electronic Structure of the Atom and Flame Tests 1. Why do metal-containing ions produce glowing colors when heated in flames? 2. Why is it that different metal ions produce different colors in flames? 3. It is necessary to clean the testing wire each time a sample is changed. Give a reason for this. 4. Write down the electron configuration of Na 5. Write down the electron configuration of Na
DATE NAME SECTION POSTLABORATORY ASSIGNMENT 1. Predict the empirical formula for each of the following compounds given the formula of magnesium oxide, MgO. (a) calcium oxide (b) strontium oxide (c) barium oxide (d) radium oxide 2. Predict the empirical formula for each of the following compounds given the formula of sodium chloride, NaCl. (a) sodium fluoride (b) potassium chloride (c) lithium bromide (d) rubidium iodide 3. A 1.250 g sample of copper wire was heated in air and reacted with...
Compound tested Ion responsible for color Color to naked eye Characteristic line colors viewed with spectroscope 2 3 4 5 6 7 Lithium chloride Sodium chloride Potassium chloride Strontium chloride Calcium chloride Copper(II) chloride Unknown Part E: Qualitative heat measure Observed effects of light source Energy Source Ultraviolet lamp Incandescent lamp Heat lamp Hot Plate (IR) ATOMS AND SPECTRA QUESTIONS: 1. What is line spectra and explain why it is important to chemical analysis? 2. What do the distinct lines...
RESULTS: Exercise 1: Qualitative Anion Tests Data Table 1. Anion Confirmation Tests. Chemical Anion Addition of AgNO3 Addition of HCl NaBr Bromide It became white and cloudy Still was white and cloudy Na2CO3 Carbonate Clear inside white and cloudy around the outside Still white and cloudy but bubbles start to form. NaCl Chloride Turn white cloudy on bottom clear on top Still white cloudy on bottom clear on top NaI Iodide In the middle very dark and cloudy fades out...
Study Exercise 3 Name Write chemical formulas for the following compounds: 1. 2. 3. Potassium iodide Barium sulfate Aluminum nitrate Copper (II) carbonate Gold (III) chloride Ferric hydroxide 7. Lead (II) chromate Nickel (II) hydroxide Mercury (II) bromide Silver acetate Magnesium chlorate 12. Sodium peroxide 13. Manganese (II) phosphate Ammonium sulfide 15. Platinum (IV) fluoride Chromium (III) hydroxide Calcium oxalate Antimony trichloride Ammonia Silicon dioxide Carbon monoxide 22. Hydrobromic acid Nitrous acid 24. - Acetic acid 25. Sulfuric acid
need help, convert them like below pic S. OH- t. 10 w. CIO2 2- X. CO24 y. HSO3 z. CIO, u. HCO3- v. 104 5. Ionic Compounds with Polyatomic lons & Constant Charge lons a. CaCO3 i. potassium hydroxide b. KCIO j. beryllium hydroxide C. CASO k. strontium acetate d. Li2SO3 I. ammonium oxide e. Ag3PO4 m. silver cyanide f. NH,F n. zinc carbonate g. Al(NO2)3 0. aluminum bicarbonate h. Ba(HCO3)2- p. magnesium phosphate b. NiP04 6. Tonic Compounds with...
This lab is the ten test tube mystery The ten solutions are as followed: 1: ammonium chloride, NH4Cl 2:barium chloride, BaCl2 3:copper sulfate, CuSO4 4:salt hydrochloric acid, HCl 5:potassium iodide, KI 6:silver nitrate, AgNO3 7:salt sodium bromide, NaBr 8:sodium hydroxide, NaOH 9:sodium sulfide, Na2S 10:sulfuric acid, H2SO4 I am just totally lost as it wants me to test all the reactions and say which solution is what, if you could please just answer which solution goes where and possibly fill...