Electromagnetic Spectrum PDF

9/22/24, 6:07 PM TMFS: Electromagnetic Spectrum Electromagnetic Spectrum Wave-shaped electromagnetic energy can range widely, from very long radio waves to very brief gamma rays. Visible light is the narrowest range of this spectrum that is...

9/22/24, 6:07 PM TMFS: Electromagnetic Spectrum Electromagnetic Spectrum Wave-shaped electromagnetic energy can range widely, from very long radio waves to very brief gamma rays. Visible light is the narrowest range of this spectrum that is visible to the human eye. An x-ray machine uses one part of the spectrum, whereas a radio detects a different one. NASA's scientific equipment investigate Earth, the solar system, and the cosmos beyond by utilizing the entire electromagnetic spectrum. Electromagnetic energy is used when you turn on the radio, watch TV, text, or make popcorn in a microwave. Every hour of every day, you are dependent on this energy. The world as you know it would not exist without it. Penetrates Earth's Atmosphere? Radiation Type Radio Microwave Infrared Visible Ultraviolet X-ray Gamma ray Wavelength (m) 103 10−2 10−5 0.5×10 −6 10−8 10−10 10−12 Approximate Scale of Wavelength Buildings Humans Butterflies Needle Point Protozoans Molecules Atoms Atomic Nuclei Frequency (Hz) 10 4 10 8 1012 1015 1016 1018 1020 Temperature of objects at which this radiation is the most intense wavelength emitted 1K 100 K 10,000 K 10,000,000 K −272 °C −173 °C 9,727 °C ~10,000,000 °C Energy is a measure of one's capacity for work and can take on several forms as well as change into new forms. A few examples of potential or stored energy are water behind a dam and batteries. Kinetic energy is exemplified by moving objects. When charged particles, like protons and electrons, move, they produce electromagnetic fields. It is this kind of energy that is known as electromagnetic radiation, or light. Static electricity is the kind of energy that can make hair stand on end. A refrigerator magnet is an example of static magnetism. A shifting electric field will result from a shifting magnetic field, and vice versa—the two are interdependent. Electromagnetic waves arise from these shifting fields. Unlike mechanical waves, electromagnetic waves can propagate without the help of a medium. This implies that electromagnetic waves are capable of passing through space's vacuum in addition to through solid objects like air. A Scottish physicist by the name of James Clerk Maxwell created a scientific theory to explain electromagnetic waves in the 1860s and 1870s. He discovered that electromagnetic waves are created when electrical and magnetic fields combine. https://www.kristujayantiexamlms.com/mod/lesson/view.php?id=202397 1/3 9/22/24, 6:07 PM TMFS: Electromagnetic Spectrum Frequency The frequency of the wave is defined as the number of crests that pass a specific position in a second. Hertz (Hz) is the unit of measurement for one wave, or cycle, per second. The unit is named for Heinrich Hertz, who proved that radio waves exist. A wave with a frequency of 2 Hz has two cycles that pass a spot in a second. Wavelength The crests and troughs of electromagnetic waves resemble those of ocean waves. The wavelength is the separation in crests. The longest wavelengths that scientists are currently studying can be larger than the diameter of our globe, while the shortest wavelengths are only tiny fractions of the size of an atom. Energy Electron volts (eV), a unit of measurement for energy, can also be used to characterize an electromagnetic wave. The kinetic energy required to drive an electron through a single volt potential is measured in electron volts. Energy rises with wavelength shortening as one moves from long to short wavelengths on the spectrum. https://www.kristujayantiexamlms.com/mod/lesson/view.php?id=202397 2/3 9/22/24, 6:07 PM TMFS: Electromagnetic Spectrum https://www.kristujayantiexamlms.com/mod/lesson/view.php?id=202397 3/3 9/22/24, 6:07 PM TMFS: Energy Levels Energy Levels Electrons revolve around a nucleus to form an atom. The tiny, negatively charged particles known as electrons travel around the nucleus in an orbit. They are not free to move in any direction at will. Depending on their energy levels, certain orbits limit their ability to rotate. Simply said, energy levels are the set distances between an atom's electrons and nucleus. Electron shells are another name for the energy levels. An electron can travel between two energy levels, but it cannot remain in one energy level and another. Level 'K' is another name for the initial energy level. The second energy level is referred to as level L, the third as level M, and so on. The electrons at energy level K have the least energy, while the electrons at energy levels farther from the nucleus have higher energy. Valence electrons are another name for electrons that exist in the highest energy level. These valence electrons constitute the basis for several atomic characteristics. Energy State Energy is increased by a predetermined quantity. This fixed energy can be absorbed by electrons to move from one lower energy level to a higher one. In contrast, energy is released as an electron moves from one level to another. Usually, this energy emission takes the form of light. Energy is emitted or absorbed when electrons move between different energy levels. Higher energy levels are referred to be excited states, whereas lower energy levels are known as ground states. Energy Level Diagram Energy level diagrams are used to investigate the type of bonding that occurs between electrons, where electrons are placed in orbits, and how elements behave under specific circumstances. The placements or arrangements of orbitals, often referred to as subshells, in accordance with their increasing energy levels are shown in energy level diagrams. The energy level diagram shown above is blank and can be used to show the electrons for any atom that is being studied. Grotrian diagrams are another name for energy level diagrams. It bears the name Walter Grotrian in honor of the German astronomer who lived in the first part of the 1900s. The energy in the orbitals are different. As can be seen from the diagram above, orbitals 2s and 2p do not have the same energy because they are not positioned at the same levels. Lower energy orbitals are positioned closer to the nucleus. For example, the order s, p, and so forth indicates that orbitals are less energetic than orbital p. The configuration for energy level 3 should be 3s