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All transitions in which electrons move from a lower to a higher level require a gain of energy. example: 2nd to 3rd shell
Wiki User
∙ 15y ago
Wiki User
∙ 9y agoThe emission of energy requires an electron to move down an orbital. When this happens, the electron will release the potential and kinetic energy in the form of a photon.
Wiki User
∙ 11y agoEnergy has to be supplied when electron moves from lower energy level to higher energy level.
Wiki User
∙ 13y agoThe transition where the electron 'drops' or 'falls' to a lower energy state, visualized
as an orbit closer to the nucleus, or a 'flip' to the spin state of lower energy.
Wiki User
∙ 11y ago3p to 1s
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What happens when a 3s electron becomes a 2s electron?
Any electron is not fixed to any sub-shell or orbital. If you provide sufficient energy to an electron, it would make transition to any of the higher energy orbitals and then come back to the lower orbitals radiating energy.
What happens when a chlorine atom gain an electron in its outer energy shell?
It becomes a negative ion.
What is the difference between electron affinity and electron gain enthalpy?
electron affinity is the negative of electron gain enthalpy. for example, the electron gain enthalpy of fluorine is -328, and electron affinity is 328 which is -(-328)
Why do non metals have higher ionization energies than metal?
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
Why halogens have highest negative electron gain enthalpy?
Good question. Halogens have their outer electronic configuration as ns2np5 and require only one more electron to gain a stable electronic configuration. So they have a great affinity for electrons and will accept them very easily by releasing energy. So they have the highest electron gain enthalpy.
What happens when a 3s electron becomes a 2s electron?
Any electron is not fixed to any sub-shell or orbital. If you provide sufficient energy to an electron, it would make transition to any of the higher energy orbitals and then come back to the lower orbitals radiating energy.
What can happenn if an electron moves to a higher energy level?
the electron will gain energy
What is electron gen enthalpy?
Electron Gain Enthalpy is the amount of Energy released when an isolated gaseous atom accepts an electron to become a monovalent gaseous anion.For Example:Atom(gas) +Electron ---->Anion(gas) +Energy(Electron Gain Enthalpy)
What is the measure of how electric energy an electron in a circuit can gain from a battery?
Voltage
What does the energy hill represents on an energy diagram?
The additional potential energy the reactants must gain in order to react
How does NAD gain energy in cellular respiration?
it lose a hydrogen ion and one electron
How does NAD gain energy cellular respiration?
It loses a phosphate and one electron. Apex
Does electron affinity gain electrons?
Yes. Electron affinity is the process by which a neutral atom gains an electron and the EA is the measure of energy released. The resulting ion will be negative.
What happens when a chlorine atom gain an electron in its outer energy shell?
It becomes a negative ion.
What is the difference between electron affinity and electron gain enthalpy?
electron affinity is the negative of electron gain enthalpy. for example, the electron gain enthalpy of fluorine is -328, and electron affinity is 328 which is -(-328)
Why is electron gain enthalpy of inert gases positive?
Inert gases are the most stable ones, so if we try to add another electron, the stable electronic configuration is disturbed. So, we have supply energy for this process. Hence, electron gain enthalpy is positive.
Why do non metals have higher ionization energies than metal?
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
