6- Place only the edge of the Q-tip at the top the Flame. 7- Remove it when you see the of light being given off to avoid burning the Q-tip. 8- Clean up procedure: Discard used Q-tips to the bin, cover back compounds and put them up in a safe place, pour away distilled water in the sink, disconnect the Bunsen burner and clean it if stained,clean the lab test surroundings with paper towel to ensure no stain is left, wash your hands remove your goggles only when all equipments have been placed in safe places. Compound | Flame Colour Observation | 1 LiNO3
I. Bean Bag Isotope II. The purpose of this experiment is to investigate the mass properties and relative abundance of isotopes for the “bean bag” element and to calculate the atomic mass of this element. III. Pre-Lab Questions A. The first possible property of electrons and protons that led to their discovery was their “positive rays,” positively charged streams of atoms generated in gas discharge tubes from J.J. Thomson’s experiment.
The Flame Test Lab Objective- Given Materials- Given Procedure- Given Results- Element Color Sr- Red Orange Ba- Yellow Orange Na- Bright Orange Li- Hot Pink Ca- Orange Cu- Green, Aqua, Blue Conclusion Questions- 1. The process by which the colored flame is produced is the release of light energy. When heat energy is added to an element, its electrons move from their ground state, to an excited state. This means the element's electrons are jumping from one orbital to another. When the heat is released, the electron then jumps back into its ground state, or back into its original orbital.
On top of this, the helium nucleus is clearly labeled and is shown containing two neutrons and two protons (which are also labeled using an “N” and a “+”). Similarly, my model of beta decay is labeled in the same manner as that of the alpha decay model. In beta decay, an unstable atom uses its natural tendency to become stable to “transform” one neutron into a proton. Subsequently, the new positive charge requires an electron to be released from the atom’s orbit. This process is shown clearly in my model due to the fact that it states that the atom gets the energy to carry out this process from the instability of itself.
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.
Another would be that some ions my produce the same flame color and not all may produce a flame color. D. When heated the electrons gain energy and can jump to any empty orbitals at higher levels, and when they move back into a lower orbital energy is released in the form of light and that is the color of the flame. Conclusions: It was concluded from the experiment that the unknown ion is Strontium. This was based on subjective open flame tests. It was learned that when metallic ions are heated and the electrons are
On each of these wafers the quantum dots are in between the substrate. On the last page it is shown, where the Indium quantum dots lie. In Kevin's assessment each quantum dot can "hold electrons. This control of the electrons causes them to emit light. If the quantum dots are placed in the cavity, the spot on the wafers where there are no crystals, in the middle, and capture electrons then the aims of the process are a success.
When LiCl is burned the color of the light is an intense red. When BaCl2 is burned the energy is released in packages of light which its color is yellow-green. When BaCl2 is burned the energy is released in packages of light which its color is yellow-green. Data Table 2: Data processing | Metallic Element | Hypothesis | Observation | Sodium ChlorideNaCl | I though that the light of the energy release was going to be red. Because the number of electrons in this compound is no too high in comparison of other compounds.
Page 7 Flame Test …………………….………………………………………………………...…………………….. Page 7 - 8 Identification of the two unknown compounds ………………………………………………………………... Page 8 Testing for ions (chloride, carbonate and sulphate ions) ……………………………………………………… Page 9-11 Equipment ____________________________________________________________ __________ Equipment used.................................................................................................................................................. Page 11 Labelled diagram of the Bunsen burner flame ………………………………………………………………..... Page 11
The Magnesium strip dissolved in the process and the test tube got hotter. gas test observations: The Hydrogen burned up in the test tube causing a loud pop|The final products were Hydrogen gas and MgCl (a clear/transparent liquid).| |Mg|A shiny opaque metal. -Grey/metallic||| Discussion Questions 1. Identify the reaction in procedure steps 3 and 5 as endothermic or exothermic. Explain why.