Some of the colors were similar but salt solution had its own distinct differences. Flame tests are the best way to determine the color a solution will emit. “Flame tests are a quick method of producing the characteristic color of metallic ions. The colors seen are a combination of the wavelengths of each transition.” Introduction 2: “An atom can react with another atom to form a compound through either a sharing or transfer of electrons in an interaction called bonding.” An Ion by definition is “an electrically charged atom or group of atoms. Metals on the left side of the table, tend to form
Experiment #4 – Properties of Gases May 31, 2014 11:58 am UCHM 240 General Chemistry I Abstract: This lab will give the opportunity to explore some physical and chemical properties of gases and use these properties to identify gases when they are present. Purpose: In this lab we will examine some common visible physical properties of gases. We will also compare chemical properties of gases against one another. We will then attempt to identify these gases with the properties we have observed. The gases being observed in this lab are hydrogen (H2), oxygen (O2), and carbon dioxide (CO2).
AS Applied Science (Chemistry) Unit 3: Finding out about substances Part 1: Qualitative analysis of compounds Introduction ____________________________________________________________ __________ Description of the investigation..................................................................................................................... Page 2 Description and importance of flame tests..................................................................................................... Page2 Background ____________________________________________________________ __________ The Composition of matter or materials…………………………………………………............................... Page 3 Description of the sub-particles of an atom …………………………………………………………………. Page 4 Example and definition of an ion ………………………………………………………………………….... Page 4 List of some metals with symbols ………………………………………………………………………........
When scientists make the different colors, each color has its own element. Also each element is mixed with an oxidizer to help create the color for the fireworks. Strontium is used to produce red fireworks; barium to produce green; sodium to produce yellow; copper to produce blue; and aluminum, magnesium, and titanium to produce white(Roncone, K. 2004). One of
THE EXPERIMENT – Urey and Miller Urey and Millers’ experiment simulated hypothetical conditions thought at the time to be present on the early Earth, and tested for the occurrence of chemical origins of life. The experiment used water (H2O), methane (CH4), ammonia (NH3), and hydrogen (H2). The chemicals were all sealed inside a sterile array of glass tubes and flasks connected in a loop, with one flask half-full of liquid water and another flask containing a pair of electrodes. The liquid water was heated to induce evaporation, sparks were fired between the electrodes to simulate lightning through the atmosphere and water vapor, and then the atmosphere was cooled again so that the water could condense and trickle back into the first flask in a continuous cycle. WHY?
- Make sure the Compounds are no where close to your other sensory organs, remember that only your eyes are protected by the Goggles. -If a compound is spilled, wipe it up immediately and tell the instructor. Materials : powder forms of these compounds - LiNO3 - NaNO3 - KNO3 - Ca(NO3)2 - Ba(NO3)2 - - Unknown compound A - Unknown compound B - Goggles, Bunsen burner, distilled water, Q-tips, paper towel and a striker. Procedures 1- Turn on the Bunsen burner around the 45 degree angle. 2- Feel the gas on the top of the Bunsen burner with your hands, adjust if too high or too low.
The color of KCl is present in a color that is lavande. A mixture of violet and blue. When NaCl is burn the energy is released in packages of light which its color is yellow-orange. When NaCl is burn the energy is released in packages of light which its color is yellow-orange. OBSERVATIONS: Data Table 1: Reactions of elements after been burned.
When the liquid above the precipitate was clear, the solution was tested for completeness of precipitation when a few drops of BaCl2 solution were added from a pipette. Next, filter paper was place into the funnel and streamed with distilled water. A clean 400mL beaker is placed under the funnel and the precipitate was filtered through. When all the precipitate was filtered and removed from the beaker the residue is washed with distilled water. About 3mL of the wash water is collected in a small test tube.
Experiment #9: e/m Ratio Submitted by: Linda Agaby 1255497 Alexandre Belisle 1236050 Instructor: Caroline Viger Experiment performed: May 03, 2013 Report submitted: May 10, 2013 Abstract J.J. Thompson first discovered the charge to mass ratio of the electron by measuring the deflection of electrons when accelerated in a magnetic field, and their kinetic energy. To reproduce this experiment, Helmholtz coils were used to create a magnetic field, and an electron gun was used to create a flow of electrons. The electron gun is composed of a filament, and when the filament is heated, electrons obtain enough energy to escape the metal. These electrons are then accelerated by a potential between the anode and the cathode that is varied during the experiment. The electrons experience a magnetic force due to the field that is perpendicular to the velocity vector, so the electrons follow a circular path.
Flame Tests Practical Write Up Method 1. The following were observed through a hand held speectroscope: a) Patch of sunlight b) Fluorescent light bulb c) Discharge tube containing the element Neon 2. 3. Flame tests were carried out on each of the following elements, the flame was observed through a spectroscope and the resulting colour was noted. a) b) Potassium chloride c) Calcium chloride d) Barium chloride e) Copper (II) chloride f) Lithium chloride g) Strontium chloride h) Sodium chloride Results Part1: | Colour through spectroscope | Patch of sunlight | Continuous spectrum | Flourescent Light bulb | Discrete spectrum | Part2: | Colour through spectroscope | Neon discharge tube | Discrete red | Part 3: Flame tests Compound | Ion | Colour of flame | Colour of flame seen through spectroscope | Literature colour | Potassium chloride | K+ | Lilac and slightly pinkish | Lilac | Lilac | Calcium chloride | Ca+ | Orange | Reds and oranges more distinctive | Brick red | Barium chloride | Ba2+ | Aqua green | Bluey green.