Umair Gaines
The element neon is well-known for its characteristic red-orange glow when electricity is passed through it. This phenomenon occurs due to the excitation of its electrons when electricity is applied, causing them to move to a higher energy state. As these electrons return to their original state, they release energy in the form of reddish-orange light. Neon is commonly used in lighting applications such as neon signs and lamps, which have become iconic and are often associated with bright, colourful advertisements.
| Characteristics | Values |
|---|---|
| Element | Neon |
| State | Gas |
| Type of gas | Noble gas |
| Colour emitted | Red to orange-red |
| Commercial applications | Neon lights, signs, and lamps |
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What You'll Learn
Neon gas
Neon (Ne) is a chemical element and a noble gas that glows red-orange when an electric current is passed through it. It was discovered in 1898 by British chemists Sir William Ramsay and Morris Travers, who extracted it from a sample of liquefied air. Ramsay identified neon as a new element by its distinctive bright red emission spectrum.
Neon is the second-lightest noble gas and is usually found in the form of molecules consisting of a single atom. It is colourless, odourless, and lighter than air under standard conditions, with approximately two-thirds the density of air. On Earth, it is found in minute quantities in the Earth's atmosphere and in the Earth's crust. However, it is the fifth most abundant chemical element in the universe by mass.
Neon has three stable isotopes: 20Ne (90.48%), 21Ne (0.27%) and 22Ne (9.25%). The Allen electronegativity scale identifies neon as the most electronegative element. When an electric current passes through a tube filled with neon gas, the electrons in the neon atoms become excited and move to a higher energy state. As these electrons return to their original state, they release energy in the form of reddish-orange light. This phenomenon is utilized in neon signs, which first became popular in the 1920s.
Neon signs typically consist of a glass tube filled with low-pressure neon gas, with electrodes at either end. When an electric voltage is applied, enough energy is supplied to remove an outer electron from the neon atoms. This excitation of electrons results in the emission of reddish-orange light, characteristic of 'neon' lighting. The colour of the light produced depends on the energy transition of the electrons, with each noble gas emitting a distinct colour. For example, while helium glows pink, krypton emits green light, and argon gives off a blue hue.
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How neon lights work
The phenomenon of neon lights was first demonstrated by French engineer and inventor Georges Claude at the Paris Motor Show in December 1910. Neon lights work by passing an electric current through neon gas in a sealed tube, causing the gas to become excited and shine a bright light. The pressure of the gas inside ranges from 3 to 20 Torr (0.4–3 kPa), which corresponds to a partial vacuum in the tubing. The outer diameters for the glass tubing used in neon lighting range from 9 to 25 mm; with standard electrical equipment, the tubes can be as long as 30 metres (98 ft).
Neon lights work using either AC (alternating current) or DC (direct current), but if DC current is used, the glow is only seen around one electrode. AC current is used for most neon lights. When an electric voltage is applied to the terminals (about 15,000 volts), enough energy is supplied to remove an outer electron from the neon atoms. If there is not enough voltage, there will not be enough kinetic energy for the electrons to escape their atoms and nothing will happen. The positively charged neon atoms (cations) are attracted to the negative terminal, while the free electrons are attracted to the positive terminal. These charged particles, called plasma, complete the electric circuit of the lamp.
The colour of the light produced depends on the gas used, with different gases producing different wavelengths and colours of light. Neon gas produces an orange-red light, while hydrogen makes reddish lights, CO2 makes white, mercury makes blue, and uranium makes green. Noble gases like helium, neon, argon, krypton, xenon, and radon are known for their lack of reactivity and are used in various applications because of their stable and chemically inert nature.
Another way to produce colours is to coat the glass with a phosphor or other chemical that will glow a certain colour when energised. Because of the range of coatings available, most modern lights no longer use neon but are fluorescent lamps that rely on a mercury-argon discharge and a phosphor coating.
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Other noble gases
Neon (Ne) is the noble gas that glows red-orange when an electric current is passed through it. This phenomenon occurs due to the way neon interacts with electricity. When an electric current passes through a tube filled with neon gas, the electrons in the neon atoms become excited and move to a higher energy state. As these electrons return to their original state, they release energy in the form of reddish-orange light. This distinctive red-orange glow is commonly seen in neon signs and lamps.
Helium
Helium (He) is a noble gas with several unique qualities. It has the lowest boiling point of any known substance at 1 atm and is the only element known to exhibit superfluidity. Additionally, helium is the only element that cannot be solidified by cooling at atmospheric pressure. Under high pressure and extremely low temperatures, it can be solidified. Helium glows pink when an electric current is passed through it.
Argon
Argon (Ar) is another noble gas that was discovered by Sir William Ramsay in 1894. It has a very low chemical reactivity and a cryogenic boiling point. Argon produces a blue-purple light when electrified.
Krypton
Krypton (Kr) is a noble gas discovered by Ramsay in 1898. It emits a whitish light when an electric current is passed through it. Krypton also has a naturally occurring radioisotope, Kr-81, with a very long life expectancy.
Xenon
Xenon (Xe) was also discovered by Ramsay in 1898. It is one of the noble gases with multiple stable isotopes. The first chemical compound of xenon, xenon hexafluoroplatinate, was discovered in 1962 by Neil Bartlett.
Radon
Radon (Rn) was first identified in 1898 by Friedrich Ernst Dorn and was later established as a noble gas in 1904. It has similar characteristics to other noble gases, including a full outer shell of valence electrons, making it chemically inert. Radon difluoride (RnF2) was identified as a compound of radon in 1962.
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Phosphor coatings
Phosphors can be classified into two main categories: fluorescent and phosphorescent substances. Fluorescent substances emit energy immediately when exposed to radiation and stop glowing when the radiation source is removed. On the other hand, phosphorescent substances emit energy with a delay, continuing to glow even after the radiation source is turned off, gradually decaying in brightness.
The specific colour emitted by a phosphor coating depends on the wavelength of emission maximum, peak width, and decay time. Various chemical compositions of phosphors allow for different colours to be produced. For instance, yttrium oxide-sulfide activated with europium is used as a red phosphor in colour CRTs, while zinc sulfide with copper as an activator yields a blue-green light. Additionally, calcium sulfide combined with strontium sulfide and bismuth as an activator produces blue light, with modifications to the formula resulting in red and orange emissions.
The versatility of phosphor coatings in producing a wide range of colours has made them indispensable in modern lighting technology. By combining different noble gases with phosphor coatings, over 100 neon colours can be achieved. Phosphor coatings have also contributed significantly to the aesthetics of glowing signs, enabling neon sign makers to expand their creative possibilities and offer a broader spectrum of attractive colours.
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Mercury/argon discharge
Mercury-argon lamps are a type of gas-discharge lamp that combines the characteristics of mercury vapour and argon gas to produce light. These lamps are made from a sealed quartz or glass tube filled with a small amount of mercury and a large amount of argon gas, with electrodes installed at both ends. When the lamp is turned on, an electric current passes through the electrodes, heating the gas inside the tube. As the temperature rises, the mercury evaporates into a vapour state and mixes with the argon gas. Under the influence of a high-voltage electric field, electrons in the mixed gas are accelerated and collide with mercury atoms, exciting them to a high-energy state. When these excited mercury atoms return to their ground state, they emit energy in the form of photons, primarily in the ultraviolet range.
The presence of argon gas affects the spectral characteristics and stability of the emitted light. While the spectral lines of mercury-argon lamps are typically distributed in the violet, blue-green, and yellow-green bands, the argon gas can influence the spectrum by enhancing or suppressing certain spectral line intensities. This results in a broad spectral range that spans from ultraviolet to visible light, with parts of the infrared spectrum as well.
Mercury-argon lamps have several advantages, including high light intensity, a long lifespan of up to several thousand hours, low energy consumption, and excellent spectral characteristics. These features make them suitable for various applications, including spectral analysis, fluorescence detection, UV curing, UV sterilization, and specialised lighting situations. For example, they are commonly used for wavelength calibration in spectrometers and as a light source in laboratory research to excite fluorescent materials in samples.
However, it is important to take appropriate precautions when using mercury-argon lamps due to the production of ultraviolet radiation, which can be harmful to human health. Additionally, mercury-argon lamps may not be suitable for all lighting situations due to their spectral characteristics and the potential impact of argon gas on the spectrum.
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Frequently asked questions
The element that glows red-orange with electricity is neon.
When electricity energises neon gas within a tube, its electrons become excited and move to a higher energy state. As these electrons return to their original state, they release energy in the form of reddish-orange light.
Neon's red-orange glow is commonly used in neon signs and lamps, which have become famous in cities at night.
Different colours can be produced by using another gas or a mixture of gases. For example, a mixture of argon and mercury will give off a blue glow.
