| Nickel ChlorideNiC12 | The substance was green originally but turned yellow after being exposed to the flames. The flames emitted were sparks of strips of bright yellow. | Copper ChlorideCuc12 | The flames that were emitted were sparks of stripy colors. The flames was first blue then it turned green. Gradually turning yellow.
The fact that the energy needed to break the necessary bonds falls within the visible light spectrum is the basis on which the experiment is based. This brings up the issue of selectivity. For example, the bromine radical is more selective than the chlorine radical. This has to do with electronegativity. It is known that chlorine is more electronegative than bromine, and thus chlorine is more reactive, and less discriminatory as to what it will react with, thus making bromine more “selective”.
During the electrolysis, a gray solid formed on the negative wire of the battery and the dark red solution formed at the positive wire of the batter. Account for this in terms of the positive and negative ions. Iodide ions have the symbol I-, indicating they are negatively charged, which cause them to be attracted to be something with a positive charge, which is why there was a red-brown solution at the positive end. Zinc ions have the symbol Zn2+, indicating a postive charge, which cause them to be attracted to something with a negative charge, which is why a grayish solid formed at the negative wire. 3.
As an example, Model Science (2011) provided “sodium burns orange, potassium -purple/blue, barium - green, and lithium – red”. After this experiment is completed, the following questions will be answered. * Why do different compounds have different colors in their visible emissions? * Would you expect the emissions to vary if metal fluorides were used rather than metal
obseRvations The color of the flame is expected to be as follows: Metallic ion Flame color Sodium Na+ Bright Orange Strontium Sr2+ Red/Orange Potassium K+ Pink Barium Ba2+ Yellow Copper Cu2+ Yellow/Green Lithium Li+ Red Calcium Ca2+ Deep Orange Unknown Red-Lithium Questions A. All chemical used in this test are binary compounds. What portion of the periodic table is responsible for the color observed? Groups 1&2 (Alkalil metals) B. In cooking over an open flame, a yellow flame is often observed when some food is spilled into the flame?
Multiple resonance is created from the movement of electrons. The hydrogen atom which is released reacts with HSO4 to make sulphuric acid H2SO4 which is known to be used as a catalyst. The mechanism is as follows: [pic] Health and safety: |Chemical Name |Oxidising |Flammable |Toxic |Harmful |Corrosive |Irritant |Carcinogenic | |Sulphuric acid | | | | | | | | |Methyl Benzoate | | | | | | | | |Methanol | | | | | | | | |Nitric Acid | | | | | | | | You will be using very harmful drugs so before starting make sure te
4. In test 1, which test tube showed signs of a change? Do you think it is a physical or chemical change? Why? The test tube that showed signs of change was the test tube that contained I2 & H, which turned dark red and had some strong odor and did dissolved.
The source of electrons that will reduce the DPIP is light. The spectrophotometer measured how much light that was not absorbed by the pigments. Darkness on the reduction of DPIP was that they did not get overly excited causing less light to travel through the
In this step, as we watched the chemical reaction with the solids, we noticed a thinning in the substance. Also, the solids became lighter and moved to the top. When stirred, the solution began to turn green and then back to light blue, where copper began in the end of the first step. A combination reaction took place, and the balanced equation is: CuOs+H2SO4aq→CuSO4aq+H2O(I) Following this step, step 5 began, in which we added 300 mg of zinc to the solution. Once the zinc was added slowly to the solution, a gas was released and the solution began to change colors.
HCI and blue dye. Blue dye and NaOCl (sodium hypochlorite). Observe, then add 1 drop of HCl. KI (potassium iodide) and Pb(NO3)2 (lead nitrate). Describe the precipitate formed.