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Why is the 2nd ionisation energy of Cr higher and not lower than of Mn?
Wiki User
∙ 8y ago
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.
Wiki User
∙ 12y ago
Wiki User
∙ 13y agoThe answer is probably not what you would expect. Iron and chromium are both found to readily turn into Cr+3 and Fe+3 ions. Manganese does not naturally form a Mn+3 ion. Why does this matter? When iron, chromium, and manganese go through their third ionization they form their respective +3 ions. Since manganese does not readily form a +3 ion, it takes a greater energy to strip the electron away from it compared to iron and chromium.
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Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
Why does Ca have a higher ionization energy than Ga?
because it lower than Ba as you go down ionization energy increases
Do x-rays have a higher or lower energy than gamma rays?
lower
Why boron has a lower first-ionization energy than beryllium?
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
Is the ionization energy of alkali metals larger or smaller than the alkaline earth metals in the same period?
It is about first ionization energy. It is less than alkaline earth metals.
Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
Why sulfur has a lower ionisation energy than phosphorus?
because it has many number of shells.
Why the first ionisation energy of potassium is only a little less than the ionisation energy of sodium?
both are in the same period which accounts for closeness. they are nonetheless different because there are more protons in the nucleus which means electrons are brought closer to it so there is a higher ionisation energy or potential
Why does Ca have a higher ionization energy than Ga?
because it lower than Ba as you go down ionization energy increases
Does higher energy light have a higher frequency than lower energy light does?
yes
Why does helium has a higher first ionization energy than argon?
The ionisation energy depends on the orbital from which the electron is removed and also the distance of the orbital from the nucleus. In the case of Helium, the electron is removed from 1s orbital whereas in the case of argon it is from 3p orbital. As 1s is closer to the nucleus, the force of attraction experience by these electrons is higher and hence helium will have higher 1st ionisation energy.
Do x-rays have a higher or lower energy than gamma rays?
lower
Why boron has a lower first-ionization energy than beryllium?
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
Is the ionization energy of alkali metals larger or smaller than the alkaline earth metals in the same period?
It is about first ionization energy. It is less than alkaline earth metals.
How do energy differences between higher energy levels of an atom compare to lower energy levels?
They are smaller in magnitude than those between lower energy levels.
Why does bromine have higher ionization energy then lead?
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
Are infrared waves higher or lower energy than visible light waves?
no
