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The configuration 3d4 4s2 is more stable than the configuration 3d5 4s1?
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Electron configuration of chromium II ion?
The electronic configuration of chromium is 1s2 2s2 2p6 3s2 3p6 3d5 4s1.
How many valence electrons in chromium?
The valence electron configuration of Cr is 3d5 4s1 , whereas it should be 3d4 4s2 but it is not like that because there is more stability of the element if it is like 3d5 4s1 as 5 orbitals of d subshell and 1 orbital of s subshell are singly filled means there is one electron in each orbital and it is stable. But if it would have like 3d4 4s2 then there would be 4 orbitls of d subshell filled and one would be empty and not much stable, so one electron from 4s jumps to 3d to fill that empty orbital and make it more stable. So its full configuration is 1s2 2s2 2p6 3s2 3p6 4s1 3d5. If u have any more confusion about orbitals, configuration etc. tell me.Added:Oxidation state (possibilities) +6, 5, 4, 3, 2, 1, -1, -2.Valence electrons (transition group no.6, [Ar]4s13d5)[1s2 2s2 2p6 3s2 3p6] 4s1 3d5
What is the quantum number for the last electron in cobalt?
expected configuration for Cr is 1s2 2s2 2p6 3s2 3p6 4s2 3d4 but in real, it is 1s2 2s2 2p6 3s2 3p6 4s1 3d5 electron from 4s orbital jumps to 3d orbital to get stable configuration. so the last electron comes in 3d orbital as filling of 3d takes place after filling of 4s orbital. Hence,quantum numbers for last electron in Cr is :- n = 3 l = 2 m = +2 s = +1/2
What is the electron configuration for Cr4?
Long-hand version: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5 Short-hand version: [Ar] 4s^2 3d^4 Note: The "^" symbol means the the following number is in the form of a superscript. The above is wrong because Cr is an exception. the actual answer is [Ar] 4s^1 3d^5 because it has a half filled subshell
Which electron configurations indicates an atom with atomic number of 24?
[Ar]4s13d5 note it is NOT [Ar]4s23d4. The reason for this is to achieve maximum spin multiplicity and hence lowest energy, the first arrangement gives 6 half - filled orbitals (maximum spin multiplicity) whereas the 2nd arrangement gives on 4 half filled orbitals.
Electron configuration of chromium II ion?
The electronic configuration of chromium is 1s2 2s2 2p6 3s2 3p6 3d5 4s1.
Electron configuration for chromium?
Long way: 1s2 2s2 2p6 3s2 3p6 4s2 3d4Short way: [Ar] 4s2 3d4
What is the complete electron configuration for the chromium III ion?
Chromium has atomic no. of 24. Its electronic configuration is 1s22s22p63s23p64s13d5 . It should be 4s23d4 but it is not because the half filled d-sub shell provides extra stability to chromium atom.
What happens to chromium that makes it an exception to the order of filling orbitals?
Chromium is an exception to the electron configuration pattern because electrons will occupy subshells until half-full and THEN start pairing up. We would expect chromium to follow the trend after Vanadium: V 'Ar' 3d3 4s2- All the subshells are either full or half full (or empty) Cr 'Ar' 3d4 4s2- this is the configuration expected- but this is less STABLE for the atom. The true configuration is: Cr 'Ar' 3d5 4s2 This is so the d block is completely half full as is the s block meaning it is more stable. This links with the fact that electrons occupy subshells until half full and THEN start pairing up.
Why is the 2nd ionisation energy of Cr higher and not lower than of Mn?
The electron configuration of a neutral chromium atom is [Ar]3d54s1. The electron configuration for manganese is [Ar]3d54s2. The first electron removed from a chromium atom is the single 4s electron, leaving the electron configuration [Ar]3d5. The first electron removed from a magnesium atom is one of the 4s2 electrons, leaving the electron configuration [Ar]3d54s1. Removal of a second electron from a chromium atom involves the removal of one of the 3d electrons, leaving a configuration of [Ar]3d4, which is not a very stable configuration, and requires more energy to achieve. Removal of a second electron from a magnesium atom involves the removal of the second 4s electron, leaving a configuration of [Ar]3d5, which is more stable and requires less energy to achieve.
How many valence electrons in chromium?
The valence electron configuration of Cr is 3d5 4s1 , whereas it should be 3d4 4s2 but it is not like that because there is more stability of the element if it is like 3d5 4s1 as 5 orbitals of d subshell and 1 orbital of s subshell are singly filled means there is one electron in each orbital and it is stable. But if it would have like 3d4 4s2 then there would be 4 orbitls of d subshell filled and one would be empty and not much stable, so one electron from 4s jumps to 3d to fill that empty orbital and make it more stable. So its full configuration is 1s2 2s2 2p6 3s2 3p6 4s1 3d5. If u have any more confusion about orbitals, configuration etc. tell me.Added:Oxidation state (possibilities) +6, 5, 4, 3, 2, 1, -1, -2.Valence electrons (transition group no.6, [Ar]4s13d5)[1s2 2s2 2p6 3s2 3p6] 4s1 3d5
What is the quantum number for the last electron in cobalt?
expected configuration for Cr is 1s2 2s2 2p6 3s2 3p6 4s2 3d4 but in real, it is 1s2 2s2 2p6 3s2 3p6 4s1 3d5 electron from 4s orbital jumps to 3d orbital to get stable configuration. so the last electron comes in 3d orbital as filling of 3d takes place after filling of 4s orbital. Hence,quantum numbers for last electron in Cr is :- n = 3 l = 2 m = +2 s = +1/2
What is the electron configuration for Cr4?
Long-hand version: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5 Short-hand version: [Ar] 4s^2 3d^4 Note: The "^" symbol means the the following number is in the form of a superscript. The above is wrong because Cr is an exception. the actual answer is [Ar] 4s^1 3d^5 because it has a half filled subshell
How many s- electrons are there in the atom Cr in ground state?
There are a total of 7 s-electrons in the ground state of chromium. It has the electron configuration of 1s2 2s2 2p6 3s2 3d5 4s1. It is unusual (along with copper) in not following the rules very well, so instead of the anticipated 3d4 4s2, it is as shown above.
Which electron configurations indicates an atom with atomic number of 24?
[Ar]4s13d5 note it is NOT [Ar]4s23d4. The reason for this is to achieve maximum spin multiplicity and hence lowest energy, the first arrangement gives 6 half - filled orbitals (maximum spin multiplicity) whereas the 2nd arrangement gives on 4 half filled orbitals.
What are the limitations of aufbau principle?
1. The Aufbau principle cannot be used to predict electron configuration of atoms on ionization. In other words, it does not tell us which electrons are to be removed when an ion is formed form an atom. For example, the configuration of Fe based on Aufbau principle is 1s2 2s2 2p6 3s2 3p6 4s2 3d6. It has been experimentally confirmed by spectral and magnetic studies than tFe2+ has configuration 1s2 2s2 2p6 3s2 3p6 3d6 and not 1s2 2s2 2p6 3s2 3p6 4s2 3d4. It means that ionization results in the loss of 4s electrons in preference to 3d electron even thought the 3d were the last to be added in building up the configuration of Fe atom. It means that in Fe2+ ,3d has lower energy than 4s which is contrary to Aufbau order of filling. This can be said of any transition element on ionization. 2. Although (n-1) d subshells and ns subshells lie quite close together , yet the former is somewhat higher in energy. Accordingly the predicted Aufbau outer configurations of Cr (Z = 34) is .....3d4 5s2 but the experimentally supported configuration is ....3d5 4s1. 3. In the sixth period , 4f and 5d subshells are exceedingly close in energy . At lanthanum (Z = 57),the last electron does not go to 4f as predicted in Aufbau order but is added to 5d subshell to give it a configuration ....4d10 5s3 5p6 5d1 6s3. However, the next electron for valium (Z =58) is added to the 4f subshell and the previous electron in 5d in lanthanum is also shifted to 4f to give it a configuration ....4d10 5s2 5d6 4f2 5d0 6s2. 4. The Aufbau order configuration of zirconium (Z =40) is ....5s2 4d2 and that the predicted order for the next element niobium Nb (Z =41) would be ...5s2 4d3 . However, the observed configuration of Nb is... 5s1 4d4. It is understandable that the next element molybdenum Mo (Z =42) acquires.....5s1 4d5 configuration due to higher stability associated with half-filled configuration. However, the next element technetium Tc (Z =43) with observed configuration 5s1 4d6 in place of predicated 5s2 4d6 shows that the preference for half-filled or completely-filled configuration is not the only controlling factor but some complex nucleus=electron and electron-electron forces also have some role to plat in deterring these configuration. 5. In case of palladium pd (Z=46), the predicted Aufbau configuration is 5s2 4d8 but the experimentally observed configuration is 5s0 4d10. This is perhaps the only case where the observed configuration has two misplaced electron.
What does the principal quantum number n designated?
it means the major level of orbital like 2S1, the 2 is the quantum number 3D4, the 3 is the quantum number
