10.2 eV ??
En = 13.6(1 - 1/n2)
So. a transition from the second energy level to ground state seems indicated if you mean electron volts. ( eV )
En = 13.6(1 - 1/22)
En = 13.6(3/4)
= 10.2 eV
=======
No, an atom typically emits photons of the same or lower energy than the absorbed photons. In this case, a red photon has lower energy than a blue photon, so it's not possible for an atom to absorb a red photon and emit a blue photon.
Light waves have electromagnetic energy. Could be considered as quantum of energy with an expression E = h v. v is the frequency of light wave. h - Planck's constant. E - the energy possessed by the quantum. This quantum is also known as photon
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Niels Bohr's theory of the atom provided a new understanding of how electrons move in specific energy levels around the nucleus. This theory helped lay the foundation for quantum mechanics and contributed to the development of modern atomic and nuclear physics. Bohr's work also influenced our understanding of the behavior of matter at the atomic and subatomic levels.
Heat energy increases the kinetic energy of water molecules, allowing them to overcome intermolecular forces and escape into the air as vapor during evaporation. Higher temperatures speed up the rate of evaporation by providing more energy for water molecules to transition from liquid to gas state.
No, an atom typically emits photons of the same or lower energy than the absorbed photons. In this case, a red photon has lower energy than a blue photon, so it's not possible for an atom to absorb a red photon and emit a blue photon.
No, as energy is absorbed. When the reverse happens, the higher state to lower state, the electron is returning to its lower energy level ground state and energy is released in the form of a photon.
Particles that exhibit wave- particle duality are considered high energy particles. One example is a photon. There is debate about whether these are real particles.
Light waves have electromagnetic energy. Could be considered as quantum of energy with an expression E = h v. v is the frequency of light wave. h - Planck's constant. E - the energy possessed by the quantum. This quantum is also known as photon
Light waves have electromagnetic energy. Could be considered as quantum of energy with an expression E = h v. v is the frequency of light wave. h - Planck's constant. E - the energy possessed by the quantum. This quantum is also known as photon
There is no need for the line to be related to energy. The line in the graph could represent height against age of adults. No relation to energy, I'd suggest.
Simple - it could never happen. An individual photon, no matter how energetic, has enough energy by millions of trillions to move anything like even the smallest toy. from Beano in the UK
not possible, as visible light photons have less energy and ultraviolet photons need more energy. Energy can neither be created nor be destroyed. So by conservation principle ultraviolet photon as they fall on fluorescent material could give out less energetic light photons, but the converse is not possible.
It could represent pain because they sting you. :)
Light waves have electromagnetic energy. Could be considered as quantum of energy with an expression E = h v. v is the frequency of light wave. h - Planck's constant. E - the energy possessed by the quantum. This quantum is also known as photon
It is not meaningful to talk about "amplitude of the visible light spectrum". One might think that more intense light would mean greater amplitude of the light wave, but it just means more photons. "Visible light" is made up of photons. A single photon has a certain quantifiable energy, and that energy is discussed in terms of frequency or wavelength. A photon with low frequency (towards the red end of the visible light spectrum, for instance) is less energetic than a photon with high frequency (towards the blue end and beyond). For all intents and purposes, the amplitude of a photon wave-packet could be said to be of "unit amplitude", the amplitude of light.
Niels Bohr's theory of the atom provided a new understanding of how electrons move in specific energy levels around the nucleus. This theory helped lay the foundation for quantum mechanics and contributed to the development of modern atomic and nuclear physics. Bohr's work also influenced our understanding of the behavior of matter at the atomic and subatomic levels.