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
OBSERVATIONS: Data Table 1: Reactions of elements after been burned. | Metallic Element | Observations | Sodium ChlorideNaCl | | Potassium ChlorideKCl | | Calcium ChlorideCaCl2 | | Barium ChlorideBaCl2 | | Strontium ChlorideSrCl2 | | Copper (II) ChlorideCuCl2 | | Lithium ChlorideLiCl | | The flame color of SrCl2 is crimson. The flame color of SrCl2 is crimson. The light’s color of CuCl2 is green. But there’s a combination between Green and blue but the color that predominate is Green.
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
This leaves a positive charge on one material and a negative one on the other, the charge depends on the material. Electrically charged objects attract small objects placed near them. Positive and negative electrostatic charges are only ever produced by the movement of the negative electrons, positive charges do not move. A positive static charge is created when electrons move away, and cause negative charges to move away as well. The key point that allows photocopiers, powder paint and precipitators work, is the face that objects with the same charge repel each other, whereas objects with opposite charges are attracted to each other.
PHOSPHORUS The element phosphorus was discovered by Hennig Brand in 1669.He was trying to create the philosophers stone but instead made something else. He took buckets of urine and tried to evaporate it. In the process he produced a white material that glowed in the dark and burned brilliantly .He boiled it into a paste, heated it to a high temperature and led the vapors through water, hoping it would condense to gold. Instead he obtained a white, waxy substance that glowed in the dark.He named it phosphorus, the name originates from the Greek words “phos” meaning light and “phoros” meaning bearer. Phosphorus is classified as an element in the nonmetals section.
Chemistry Lab Types of Chemical Reactions OBSERVATION DATA TABLE Step|Name of Reactants|Description of Reactants|Description of reaction taking place (evidence of chemical reaction)|Description of Products| 1|Zn|Solid, small chunky bits, Silvery-grey, dull|As the Zinc and Sulfur heated up it expanded in the test tube and shot out Zinc Sulfide.-light and heat are produced|White powder was created and the leftovers of the reactions was a black powder.| |S|Solid, resembles powder, Off-yellowOpaque||| 2|KI|-dull yellow liquid-transparent|Instantaneously changed colour to a bright yellow.|-Bright yellow liquid-Opaque| |Pb(NO3)2|-liquid, transparent, very clear-bubbly||| 3|H2O2|-liquid-clear-transparent|A dark grey bubbling liquid was created. It got hotter as it reacted.gas test observations:The splint relit. Oxygen was present.|Oxygen gas was created and a dark grey opaque liquid was left behind in the test tube. | |MnO2|-solid-powder-black||| 4|AgNO3|A clear, transparent liquid.|As the copper reacted with the Silver Nitrate, the ball of Copper changed colour to grey and subsequently developed a ‘furry-like’ characteristic on its coating.|-Clear liquid-Copper changes to a grey colour, ‘furry-like’.| |Cu|-brown/red-solid-stringy||| 5|HCl|A clear, transparent liquid.|When the Magnesium was inserted the HCl liquid started to bubble and fizz releasing Hydrogen. The Magnesium strip dissolved in the process and the test tube got hotter.
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
3. A dark central spot was observed when the opaque hole was illuminated. 4. The laser light was coherent (in phase), collimated (beam diverges very little) and monochromatic (narrow range of wavelengths). If a white light had been used, the different light waves, out of phase light waves and divergence of the beam would have interfered with one another giving different
| | | The energy of a single photoelectron depends only on the frequency of the incident light. | | | The energy of a photoelectron is equal to the sum of the photon energy and the energy needed to remove the electron from the metal. | | | A higher intensity of the incident light means a higher number of emitted photons. | 1 points Question 7 1. In an unexcited atom, the electrons occupy Answer | | the levels with lowest energies.
Some of the photons are absorbed by the silicon block. Some of the absorbed photon will have energy greater than the energy gap between valence and conduction band of valence electrons of the silicon atoms. Hence, some of the valence electrons in the covalent bond will be excited and jump out from the bond leaving behind a hole in the bond. In this way electron-hole pairs are generated in the crystal due to incident light. The holes of these light generated electron-hole pairs in the n-type side have enough probability of recombination with enormous electrons (majority carriers).