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The configuration 3d4 4s2 is more stable than the configuration 3d5 4s1?
Wiki User
∙ 10y ago
False
Wiki User
∙ 10y ago
The configuration 3d4 4s2 is more stable because it fills up the 4s orbital before filling the 3d orbital. This follows the Aufbau principle, which states that orbitals are filled in order of increasing energy. In the case of 3d5 4s1, the electron is placed in the higher energy 3d orbital before the 4s orbital is completely filled, making it less stable.
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Electron configuration of tin is Ar4s23d2 but that of Cr2 plus is Ar3d4?
The electron configuration of tin is [Kr]5s24d10. The electron configuration of Cr2+ is [Ar]3d4. When chromium loses two electrons to form Cr2+, the 4s electrons are removed before the 3d electrons.
Electron configuration of chromium II ion?
The electron configuration of a chromium II ion (Cr^2+) is [Ar] 3d^5. Chromium normally has an electron configuration of [Ar] 3d^5 4s^1, but when it loses two electrons to form the Cr^2+ ion, the 4s^1 electron is lost first, resulting in a 3d^5 configuration.
What are two elements with ground-state electron configurations that are well-known exceptions to the Aufbau principle?
Chromium and copper are well-known exceptions to the Aufbau principle. Chromium has an electron configuration of [Ar] 3d5 4s1 instead of the expected [Ar] 3d4 4s2, and copper has an electron configuration of [Ar] 3d10 4s1 instead of the expected [Ar] 3d9 4s2.
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
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 for chromium?
Long way: 1s2 2s2 2p6 3s2 3p6 4s2 3d4Short way: [Ar] 4s2 3d4
Electron configuration of tin is Ar4s23d2 but that of Cr2 plus is Ar3d4?
The electron configuration of tin is [Kr]5s24d10. The electron configuration of Cr2+ is [Ar]3d4. When chromium loses two electrons to form Cr2+, the 4s electrons are removed before the 3d electrons.
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.
Electron configuration of chromium II ion?
The electron configuration of a chromium II ion (Cr^2+) is [Ar] 3d^5. Chromium normally has an electron configuration of [Ar] 3d^5 4s^1, but when it loses two electrons to form the Cr^2+ ion, the 4s^1 electron is lost first, resulting in a 3d^5 configuration.
What are two elements with ground-state electron configurations that are well-known exceptions to the Aufbau principle?
Chromium and copper are well-known exceptions to the Aufbau principle. Chromium has an electron configuration of [Ar] 3d5 4s1 instead of the expected [Ar] 3d4 4s2, and copper has an electron configuration of [Ar] 3d10 4s1 instead of the expected [Ar] 3d9 4s2.
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
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 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
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
