Why do different elements produce distinct colors in the flame test?

• A. The color observed is due to impurities present in the sample rather than the element itself.
• B. Elements react with oxygen in the flame to form colored compounds that emit light.
• C. Each element has a unique arrangement of electrons, which leads to characteristic energy transitions and emission of specific wavelengths of light.
• D. The temperature of the flame changes depending on the element, causing different colors to appear.

Answer: (C)

Verified step by step guidance

1. Understand that when an element is heated in a flame, its electrons absorb energy and get excited to higher energy levels.
2. Recognize that each element has a unique electronic structure, meaning the energy differences between electron levels are specific to that element.
3. When the excited electrons return to their lower energy states, they release energy in the form of light with specific wavelengths corresponding to those energy differences.
4. The wavelength (color) of the emitted light can be calculated using the equation \(E = h \nu = \frac{hc}{\lambda}\), where \(E\) is the energy difference, \(h\) is Planck's constant, \(\nu\) is frequency, \(c\) is the speed of light, and \(\lambda\) is the wavelength.
5. Therefore, the distinct colors observed in flame tests arise from the unique set of energy transitions in each element's electrons, not from impurities, chemical reactions, or flame temperature changes.