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Referring to the figure below how much energy is needed to move an electron in a hydrogen atom from n 3 to n 6 Give the answer (a) in joules and and Atilde and 151 10 J (b) in eV. e?
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What is hydrogen outermost energy level?
If you are referring to the valence shell; the answer is one.
What is second ionization energy of hydrogen?
hydrogen has only one electron so after you remove that electron you do not have any electrons left to remove so hydrogen doesn't have a 2nd ionization energy. hydrogen has 1 proton and 1 electron.
What is the number for electrons on hydrogen's first energy level?
Hydrogen's electron configuration is 1s1. It has only one electron. It is located in the first energy level.
How do you find the energy of Hydrogen in electron volts?
We can find kinetic energy of hydrogen by using the formula,1/2mv2/1.60217646 into -19th power of 10in electron volts.
How much energy is needed to completely remove an electron from n2 in a hydrogen atom?
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
What is hydrogen outermost energy level?
If you are referring to the valence shell; the answer is one.
What is second ionization energy of hydrogen?
hydrogen has only one electron so after you remove that electron you do not have any electrons left to remove so hydrogen doesn't have a 2nd ionization energy. hydrogen has 1 proton and 1 electron.
The outer electron levels of hydrogen?
Hydrogen has only 1 electron and has only 1 energy level.
What is the number for electrons on hydrogen's first energy level?
Hydrogen's electron configuration is 1s1. It has only one electron. It is located in the first energy level.
How do you find the energy of Hydrogen in electron volts?
We can find kinetic energy of hydrogen by using the formula,1/2mv2/1.60217646 into -19th power of 10in electron volts.
How much energy is needed to completely remove an electron from n2 in a hydrogen atom?
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
What is the difference between excited hydrogen atom and any other atom?
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"
What is more- potential energy or kinetic energy of an electron in hydrogen atom?
Both are equal.
What happens to excess energy when the electron jumps from a higher energy orbit to a lower energy orbit in the hydrogen atom?
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.
What uses energy from the high-energy electrons to transport hydrogen across the thylakoid membrane?
Electron transport chain
Can the electron in the ground state of hydrogen absorb a photon of energy 13.6eV and greater than 13.6eV?
yes , the electron in the ground state of the hydrogen atom will absorb a photon of energy 13.6ev but not greater than 13.6 ev . because 13.6 ev is the energy which excites the hydrogen atom
How do you explain the diagram that shows 4 energy levels of hydrogen - 1 at the bottom 4 at the top - the values are n4-0.85eV n3-1.51eV n2-3.4eV n1-13.6eV?
The diagram shows the ionization energies of hydrogen. The ionization energy for a ground-state electron in hydrogen is 13.6eV. Let's jump. An electron orbits an atom of hydrogen in as low an energy level as possible. That's the ground state of hydrogen. To tear that electron away, it takes some amount of energy. In this case, it takes 13.6eV to strip off that electron. But what if the electron is in the next higher allowable energy level because the gas it hot? In that case, it takes less energy to tear that electron away because you've got a "head start" owing to the fact that the electron is in a higher orbital than the ground state. And what if it's in the next higher allowable energy level? Or the next? Less and less energy is required to strip off the electron as it moves to higher energy levels. These are the ionization energies of hydrogen. These energy levels are specific to hydrogen. Each other element will have a different set if ionization energies associated with it. And with atoms with many electrons and complex electron structures, the problem can quickly become very complex.
