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An excited state is an energy level of an atom, ion, or molecule in which an electron is at a higher energy level than its ground state. An electron is normally in its ground state, the lowest energy state available. After absorbing energy, it may jump from the ground state to a higher energy level, called an excited state.
An excited state means that (typically) the valence electron has moved from its ground state orbital (i.e. lowest available energy) to some other higher energy orbital. So any electron configuration in which the last electron (again, the valence electron) is in a higher energy orbital, this element is said to be in an excited state. For example, if we look at the ground state (electrons in the ...
Phosphorus has atomic number 15. As such its electronic configuration in ground state is 1s^2 2s^2 2p^6 3s^2 3p^3 The following electronic configurations could be excited states 1s^2 2s^2 2p^6 3s^1 3p^4 Here one of 3s electrons has been promoted to 3p sub level 1s^2 2s^2 2p^6 3s^2 3p^2 3d^1 Here one of 3p electrons has been promoted to 3d sub level 1s^2 2s^2 2p^6 3s^2 3p^2 4s^1 Another ...
The first excited state is the same configuration as the ground state, except for the position of one electron. As an example, sodium goes through a #3s -> 3p# transition. The ground state electron configuration for sodium is: #color(blue)(1s^2 2s^2 2p^6 3s^1)# And the first excited state electron configuration for sodium is:
An excited state electron configuration of carbon is "1""s"^"2""2s"^1"2p"^3". This is the state of carbon when it undergoes chemical bonding to form four covalent bonds, as in methane, "CH"_"4". However, the experimental evidence shows that all four bonds have the same energy, which can only be explained by the concept that the 2s and 2p ...
Still magnesium In chemistry, excited state means that an electron from an orbital absorbs incoming radiation or a photon that corresponds to its energy level and hence is elevated to a higher energy level. Hence, when an element is excited, only electrons are concerned, thus not affecting the identity of the element. In order for an element to transmute or decay into another element, such as ...
So, Electronic Configuration after becoming a univalent ion (Al^+): 1s^2 2s^2 2p^6 3s^2 [3p shell is empty now.] Electronic Configuration after becoming a bivalent ion (Al^(2+)): 1s^2 2s^2 2p^6 3s^1 Electronic Configuration after becoming a trivalent ion (Al^(3+)): 1s^2 2s^2 2p^6 [Now 3s is empty] The Most Excited State here is the third one.
This is only known exactly for the hydrogen-like atoms. Otherwise, it is done experimentally via photoelectron spectroscopy. For hydrogen-like atoms, i.e. "H", "He"^(+), "Li"^(2+), etc., the energy levels are given by: E_n = -Z^2 cdot "13.61 eV"/n^2 where Z is the atomic number and n is the quantum level. So for "He"^(+), the first excited state energy level would be the 1s^0 2p^1 ...
The excited state of an electron is the energy level that an electron moves to after absorbing energy. The electron would rather be in its ground state, or the state that requires less of its energy. When this happens, the law of conservation of energy is manifested as an emission of color
Well, the ground-state electron configuration of "Sc" is [Ar] 3d^1 4s^2 "Sc" has many excited states, but let's choose an intuitive one... one where a valence electron is promoted to a clearly higher energy level. We'll assume the 4s -> 4p transition. That would give one of the excited states as: [Ar] 3d^1 4s^color(red)(2) -> barul(|stackrel(" ")(" "[Ar] 3d^1 4s^1 4p^color(red)(1)" ")|) (There ...