le> Bohr Atomic Model Bohr Atomic Model :In 1913 Bohr proposed his quantized shell model of the atom to define howelectrons can have secure orbits approximately the nucleus. The motion of theelectrons in the Rutherford version was unsecure because, according toclassical mechanics and electromagnetic concept, any type of charged particlerelocating on a curved route emits electromagnetic radiation; thus, theelectrons would shed energy and spiral into the nucleus. To remedy thestcapability problem, Bohr modified the Rutherford design by requiring thatthe electrons relocate in orbits of resolved size and also energy. The power of anelectron depends on the size of the orlittle bit and also is lower for smaller sized orbits.Radiation can take place just once the electron jumps from one orbit toan additional. The atom will be totally steady in the state with the smallestorlittle, given that there is no orbit of lower energy right into which the electron canjump.

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Bohr"s founding point wregarding realize that classical mechanics by itselfcould never before define the atom"s stcapacity. A steady atom has a details sizeso that any equation describing it should contain some standard constantor combicountry of constants through a dimension of length. The classicalstandard constants--namely, the charges and the masses of the electronand the nucleus--cannot be unified to make a length. Bohr noticed,yet, that the quantum constant formulated by the Germale physicist MaxPlanck has dimensions which, as soon as merged through the mass and also charge of theelectron, produce a measure of size. Numerically, the measure is closeto the recognized dimension of atoms. This motivated Bohr to usage Planck"s constantin looking for a theory of the atom.Planck had introduced his constant in 1900 in a formula explaining thelight radiation emitted from heated bodies. According to classical concept,equivalent quantities of light power have to be developed at all frequencies.This is not just contrary to observation yet additionally means the absurdoutcome that the total energy radiated by a heated body have to be infinite.Planck postulated that energy have the right to just be emitted or soaked up in discretequantities, which he referred to as quanta (the Latin word for "just how much"). Theenergy quantum is related to the frequency of the light by a newstandard consistent, h. When a body is heated, its radiant energy in aspecific frequency selection is, according to timeless theory, proportionalto the temperature of the body. With Planck"s hypothesis, yet, theradiation deserve to occur just in quantum amounts of power. If the radiantenergy is less than the quantum of energy, the amount of light in thatfrequency range will be lessened. Planck"s formula appropriately describesradiation from heated bodies. Planck"s consistent has actually the dimensions ofactivity, which might be expressed as systems of power multiplied by time,devices of momentum multiplied by size, or devices of angular momentum. Forexample, Planck"s constant have the right to be written as h = 6.6x10-34 joulesecs.Using Planck"s consistent, Bohr acquired an accurate formula for the energylevels of the hydrogen atom. He postulated that the angular momentum ofthe electron is quantized--i.e., it can have just discrete worths. Heassumed that otherwise electrons obey the regulations of timeless mechanics bytraveling approximately the nucleus in circular orbits. Because of thequantization, the electron orbits have fixed sizes and energies. Theorbits are labeled by an integer, the quantum number n.With his design, Bohr explained how electrons might jump from one orlittle bit toan additional only by emitting or taking in power in addressed quanta. For instance,if an electron jumps one orlittle closer to the nucleus, it need to emit energyequal to the difference of the energies of the two orbits. Conversely,when the electron jumps to a bigger orbit, it must absorb a quantum oflight equal in power to the difference in orbits.

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Excerpt from the Encyclopedia Britannica without permission.