I am a bit rusty so I will do this the long way. Get frequency first(Hz).
Hz = (3.29 X 10^15 Hz) * Z^2 * (1/n final^2 - 1/n initial^2)
( Z =1 for hydrogen, so no problems there )
Hz = (3.29 X 10^15 Hz) * (1/2^2 - 1/6^2)
Hz = 7.31 X 10^14 Hertz
Wavelength = speed of light/Hertz
2.998 X 10^8 m/s/7.31 X 10^14 Hz
= 4.10 X 10^-7 meters
that is 410 nanometers
The color would be violet
a crazy boy who jumps around
It modifies or qualifies and adjective or a phrase jumps swiftly
Depending how long the frog takes to jump the 3ft and slide back 2ft between jumps, it will take it 17 times this duration (the frog will escape on the 18th jump and I assume the jumps take no time relative to the sliding back bit), which will then possibly be needed to be converted into hours.
The word jumping has two syllables.
1. He sees a poodle eat 2. She jumps over it
The electron emits a photon of light which we can see in a spectrograph as color. Four colors are normally seen in a hydrogen atom subjected to energy.
Depends on the isotope can be 0 or 1 hydrogen is a highly unstable element that the electron Jumps betweent the two energy levels
Bohr did not discover protons, neutrons, or electrons. Bohr used the energy changes in line emission spectra to develop a model that accounted for discrete energy changes. He used the signature spectra of hydrogen to design a model of a Hydrogen atom that showed the possible jumps that an electron could make after absorbing and then releasing energy. Some of the jumps create the visible bands we see by breaking down the light of glowing Hydrogen, while other jumps, non-visible, would still be created in the Electromagnetic Spectrum according to the energy changes of an electron jumping from outer electron rings to inner electron rings.
The atomic spectra of an element is basically the lines of color that appear when an electron jumps down or up an energy level. Depending on the shells that an electron jumps is the intensity or the color omitted. The colors that we see (yellow, orange, red, green, blue, purple) mean different level jumps with purple being the highest and yellow being the lowest. The higher the energy level the lower the wavelength omitted and the lower the energy jump the higher the wavelength.
Hydrogen atom = 1 proton 1 electron Hydrogen's 1 electron occupies the lowest energy level, 1s orbital. The atom is therefore in its "ground state". When a photon of correct frequency "collides" with a electron in hydrogen's 1s orbital the energy contained in the photon is transferred to the electron. The electron then gets added energy, so it is at a higher energy state. When it reaches this higher energy state the electron jumps to the next energy level and there it starts its new orbit. Hydrogen atom is now "excited" For any other atoms it is the same thing because all atoms can undergo excitation. The only difference between hydrogen's 1 electron and other atom's many electrons is WHICH ELECTRON will be "excited"
It jumps from one electron to the other.
no
Electrons are negative energy. When an electron jumps orbitals, it can either absorb or radiate energy in the form of photons.
the atom gains or loses energy
Because they absorb energy.
They are specialized diodes. When an electron jumps the "forbidden zone" , a photon is emitted.
if an electron gains enough energy it jumps to a higher energy level. when this happens the atom is in an "excited" state.