The objectives of this lab are to: Background Electromagnetic radiation is energy in the form of waves.
Demonstrate work habits that ensure personal safety and the safety of others, as well as consideration for the environment. Select and use scientific equipment appropriately and safely.
Synthesize information obtained from a variety of sources. Describe examples of the relationship between chemical principles and applications of chemistry. The energy of the various parts of the electromagnetic em spectrum is directly related to the frequency of the wave.
If a wave has a high frequency, then it will contain a higher amount of energy. For example, gamma rays are high-energy waves due to their very high frequency Hz. Radio waves are low-energy waves, as their frequency is approximately Hz.
Visible light, with its colours ranging from red to violet, is the portion of the electromagnetic spectrum that is detected by the human eye. Within this range of colours, red light has the largest wavelength small frequency.
At the other end of the spectrum, violet light has the smallest wavelength large frequency.
When an iron nail is heated in a Bunsen burner flame, it will glow bright red. The human eye is sensitive to the frequency and wavelength of the electromagnetic radiation within this range, and it is seen as red. If you place your hand near the iron nail, your hand will detect the warmth of the nail, which is represented by the infrared region of the electromagnetic spectrum.
Demonstrations Several quick demonstrations can be performed to show the visible spectrum.
Hold up a glass prism to an overhead light and have students observe the white light that passes through the prism break apart into a range of colours, known as a spectrum. This can be projected on the classroom wall, ceiling, or overhead screen.
Have students look at light being diffracted by a CD. This also shows a spectrum of colours. Describe qualitatively the electromagnetic spectrum in terms of frequency, wavelength, and energy. Recognize, through direct observation, that elements have unique line spectra.
A common occurrence with which students should be familiar is the rainbow, an uninterrupted sequence of colours ranging from red to violet. · Flame analysis or atomic emission spectroscopy (AES) is based on the physical and chemical principle that atoms — after being heated by flame — return to their normal energy state by giving off the excess energy in the form of light.
The frequencies of the light given off timberdesignmag.com /atomic-emission-spectroscopy. •Part 4: In Part 4, students will be introduced to real world applications of topics covered in the Flame Test Lab.
This activity includes a reading assignment, reading comprehension questions and applied calculations which tie Parts Flame Tests, Atomic Spectra and Applications Activity Essay (See teacher background information in Flame Tests, Atomic Spectra and Applications Activity) Introduction: Have you ever seen a .
you will research various applications and/or natural occurrences of line spectra such as astronomy, aurora borealis, fireworks and neon lights. Part One: Flame Tests (As an option, this could be a demo rather than a student activity). · The use of atomic spectroscopy in the pharmaceutical industry for the determination of trace elements in pharmaceuticalstimberdesignmag.com As observed in pilot scale flame spectra that resulted from the combustion of coal at ambient pressures (Fig.
2, Fig. 3), the coal flame spectra from the gasifier test also showed the sodium peak at nm and the potassium peaks at and timberdesignmag.com://timberdesignmag.com