Electromagnetic radiation of wavelength 242 nm

[ "article:topic", "authorname:openstax", "electromagnetic spectrum", "radio waves", "visible light", "blackbody", "gamma rays", "Stefan-Boltzmann law", "energy flux", "infrared", "microwave", "ultraviolet", "Wien\u2019s law", "X-rays", "license:ccby", "showtoc:no", "program:openstax", "source[1]-phys-3638", "source[2]-phys-3638", "licenseversion:40", "source@https://openstax.org/details/books/astronomy" ] \( \newcommand\) • • • • • • Learning Objectives By the end of this section, you will be able to: • Understand the bands of the electromagnetic spectrum and how they differ from one another • Understand how each part of the spectrum interacts with Earth’s atmosphere • Explain how and why the light emitted by an object depends on its temperature Objects in the universe send out an enormous range of electromagnetic radiation. Scientists call this range the electromagnetic spectrum, which they have divided into a number of categories. The spectrum is shown in Figure \(\PageIndex\) Radiation and Earth’s Atmosphere. This figure shows the bands of the electromagnetic spectrum and how well Earth’s atmosphere transmits them. Note that high-frequency waves from space do not make it to the surface and must therefore be observed from space. Some infrared and microwaves are absorbed by water and thus are best observed from high altitudes. Low-frequency radio waves are blocked by Earth’s ionosphere. Types of Electromagnetic Radiation Electromagnetic radiation with the shortest wavele...

https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FProvidence_College%2FCHM_331_Advanced_Analytical_Chemistry_1%2F09%253A_Applications_of_Ultraviolet-Visable_Molecular_Absorption_Spectrometry%2F9.02%253A_Absorbing_Species%2F9.2.01%253A_Electronic_Spectra_-__Ultraviolet_and__Visible__Spectroscopy_-_Organics Expand/collapse global hierarchy • Home • Campus Bookshelves • Providence College • CHM 331 Advanced Analytical Chemistry 1 • 9: Applications of Ultraviolet-Visable Molecular Absorption Spectrometry • 9.2: Absorbing Species • 9.2.1: Electronic Spectra - Ultraviolet and Visible Spectroscopy - Organics Expand/collapse global location Objectives After completing this section, you should be able to • identify the ultraviolet region of the electromagnetic spectrum which is of most use to organic chemists. • interpret the ultraviolet spectrum of 1,3-butadiene in terms of the molecular orbitals involved. • describe in general terms how the ultraviolet spectrum of a compound differs from its infrared and NMR spectra. Study Notes Ultraviolet spectroscopy provides much less information about the structure of molecules than do the spectroscopic techniques studied earlier (infrared spectroscopy, mass spectroscopy, and NMR spectroscopy). Thus, your study of this technique will be restricted to a brief overview. You should, however, note that for an organic chemist, the most useful ultraviolet region of the electromagnetic spectrum is ...

Gives λ = 242 n m = 242 × 10 − 9 m From planck's theory , we have E = h v = h c λ or E = 6.63 × 3 × 10 8 242 × 10 − 9 J = 6.63 × 3 × 10 − 17 242 = 8.21 × 10 − 19 J Ionisation potential of Na = N A × E (where N A is Avogadro's number) = 6.022 × 10 23 × 8.21 × 10 − 19 J m o l − 1 = 494.5 k J m o l − 1

Hint:Sodium has a symbol Na and has an atomic number of \[11\] it is known to be a very reactive metal as it is a group \[1\] element. All elements in group \[1\] are highly reactive and as they donate electrons, they are called metals. They are highly malleable and good conductors of electricity. It does not occur as a free metal in nature but as a compound. Complete step-by-step answer: Sodium is known to exist in various minerals such as rock salt and sodalite. Its salts are very highly water soluble and they have been leached by the process of water. By the electrolysis of sodium hydroxide, we can obtain sodium metal. Sodium is essential for both plants and animals which makes it a major cation in the extracellular fluid and its osmotic pressure and compartment volume. Electromagnetic radiation occurs when photons flow. This can also be called light quanta that occur in space. They are called the packets of energy and this energy can be transferred in the form by the equation \[E = Hv.\] This always moves in the speed of light which is universal. Here $h$ is called as the Planck’s constant, where $h$ is the symbol of the same. And here \[v\] is the same as the frequency of electromagnetic waves. The ionization energy of sodium will be equal to the energy possessed by the radiation of wavelength \[242\;nm\] It is \[E = \frac = 494000J = 494kJ.\] Note: The spectrum changes as per the frequencies of these electromagnetic radiation which can be the low values such as radio...

Tetra Images / Getty Images Some people can see further into the The wavelengths of visible light are: • Violet: 380–450 nm (688–789 THz frequency) • Blue: 450–495 nm • Green: 495–570 nm • Yellow: 570–590 nm • Orange: 590–620 nm • Red: 620–750 nm (400–484 THz frequency) Violet light has the shortest Angel Gallardo / Getty Images There is no wavelength assigned to indigo. If you want a number, it's around 445 nanometers, but it doesn't appear on most spectra. There's a reason for this. English mathematician spectrum (Latin for "appearance") in his 1671 book "Opticks." He divided the spectrum into seven sections—red, orange, yellow, green, blue, indigo, and violet—in keeping with the Greek sophists, to connect the colors to days of the week, musical notes, and the known objects of the solar system. So, the spectrum was first described with seven colors, but most people, even if they see color well, can't actually distinguish indigo from blue or violet. The modern spectrum typically omits indigo. In fact, there is evidence Newton's division of the spectrum doesn't even correspond to the colors we define by wavelengths. For example, Newton's indigo is the modern blue, while his blue corresponds to the color we refer to as cyan. Is your blue the same as my blue? Probably, but it may not be the same as Newton's. Bloomberg Creative Photos / Getty Images Just because humans can't see beyond the visible spectrum doesn't mean animals are similarly restricted. Bees and other insects ...

https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_(Physical_and_Theoretical_Chemistry)%2FSpectroscopy%2FElectronic_Spectroscopy%2FElectronic_Spectroscopy_Basics%2FElectromagnetic_Radiation \( \newcommand\) • • • • • • This page is a basic introduction to the electromagnetic spectrum sufficient for chemistry students interested in UV-visible absorption spectroscopy. If you are looking for any sort of explanations suitable for physics courses, then I'm afraid this isn't the right place for you. Light as a wave form Any wave is essentially just a way of shifting energy from one place to another - whether the fairly obvious transfer of energy in waves on the sea or in the much more difficult-to-imagine waves in light. In waves on water, the energy is transferred by the movement of water molecules. But a particular water molecule doesn't travel all the way across the Atlantic - or even all the way across a pond. Depending on the depth of the water, water molecules follow a roughly circular path. As they move up to the top of the circle, the wave builds to a crest; as they move down again, you get a trough. The energy is transferred by relatively small local movements in the environment. With water waves it is fairly easy to draw diagrams to show this happening with real molecules. With light it is more difficult. The energy in light travels because of l...