Ion Flame
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Ion Flame
The Lithium Ion Battery(1)?
The Lithium Ion Battery(1)?
The Lithium Ion Battery(1)?Pioneer work with the lithium battery began in 1912 under G.N. Lewis but it was not until the early 1970s that the first non-rechargeable lithium batteries became commercially available. Attempts to develop rechargeable lithium batteries followed in the 1980s, but failed due to safety problems.
Lithium is the lightest of all metals, has the greatest electrochemical potential and provides the largest energy density per weight. Rechargeable batteries using lithium metal anodes (negative electrodes) are capable of providing both high voltage and excellent capacity, resulting in an extraordinary high energy density.
After much research on rechargeable lithium batteries during the 1980s, it was found that cycling causes changes on the lithium electrode. These transformations, which are part of normal wear and tear, reduce the thermal stability, causing potential thermal runaway conditions. When this occurs, the cell temperature quickly approaches the melting point of lithium, resulting in a violent reaction called ‘venting with flame’. A large quantity of rechargeable lithium batteries sent to Japan had to be recalled in 1991 after a battery in a mobile phone released flaming gases and inflicted burns to a person’s face.
Because of the inherent instability of lithium metal, especially during charging, research shifted to a non-metallic lithium battery using lithium ions. Although slightly lower in energy density than lithium metal, the Li-ion is safe, provided certain precautions are met when charging and discharging. In 1991, the Sony Corporation commercialized the first Li-ion battery. Other manufacturers followed suit. Today, the Li-ion is the fastest growing and most promising battery chemistry.
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What do colors of flame show about energy and electron movement?
After burning six solutions over a Bunsen Burner during chemistry, I observed these flame colors given off:
Lithium chloride - Red
Sodium chloride - Yellow
Potassium chloride - Violet
Calcium chloride - Red-orange
Strontium chloride - Red-orange
Barium chloride - Green
Can someone explain what the flame test shows in terms of energy and electron movement?
Also, how would a flame test be used to identify ions, and what limitations does the flame test have in doing so?
"What do colors of flame show ..."? Only that electrons are being excited to higher energy levels and then falling back to lower ones and emitting energy with a particular wavelength. What you see are characteristic colors which are in the visible part of the spectrum. Each element has a unique spectral fingerprint when you look at all of the lines in the spectrum. The colors you've listed are simply the ones that are brightest and stand out more.
For instance, the sodium spectrum consists of many more lines, but only a narrow cluster of lines are in the yellow part of the spectrum. Calcium has several lines in the visible spectrum, but it is the red-orange lines which are brightest and swamp the others. See the whole visible spectra of several elements here: http://www.amazingrust.com/experiments/background_knowledge/Images/line_spectrum.jpg
Knowing the particular wavelength(s) of the light being emitted by the excited elements is more useful than the simple flame test since it is possible that more than one element could appear the same color.
Flame Tests and Ion Colors HD
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