Burning Salts Lab Report

In our lab, we were given the task of burning seven different salts and taking notes of what we observed. The different salts included Potassium chloride, Calcium chloride, Strontium chloride, Lithium chloride, Copper II chloride, Sodium Chloride, and Barium Chloride. Burning a pinch of each salt separately by holding a nichrome wire over a Bunsen burner, we found that each salt emitted a different color of light. For example, Potassium Chloride burnt a bright pink flame when burned, while Calcium burnt orange. No color was truly identical. What was the cause of this phenomenon? To answer this question, we need to dive deep into the heart chemistry, right down to individual atoms and electrons. According to chemicalconnection.org.uk, “The heat of the flame causes electrons in the metal atom to rise up to higher energy levels. This
Electrons do not stay in the nucleus, the center of an atom, they are found outside the nucleus. Energy levels, at this point, are best described as areas which contain electrons. Each increasing energy level is farther and farther away from the nucleus. Electrons must fill lower energy levels before they can move to higher energy levels. Electrons will go to any lower energy level if possible. The relationship between energy levels and electrons can be thought of like fans at a football game. The electrons are represented as fans, and the energy levels are the seats. The fans want the lowest seat possible so they can be close to the game. They fill the lowest seats first before they move to the seats higher up. If a fan in lower seat moves, someone from a higher seat would come and fill its spot. When all the electrons in an atom are in all of the lowest possible energy levels it is called a ground state. If any electrons are in higher energy levels when there are possible lower energy levels to be located it is called an excited