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Answered 2014-08-22 15:39:13

The electron configuration of the 4f energy sublevel is the most stable is 4f to the 14th power. The electron configuration of outer sublevels that are most stable is 4d up to the 5.5s up to the 1st power.

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Answered 2020-10-14 17:29:50

4f13

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Which electron configuration of the 4f energy sublevel is most stable?

The most stable electron configuration of the 4f energy sublevel is 4f7 or 4f14. In the 4f7 configuration, there would be only one electron in each of the seven orbitals and they would all have the same spin.


Why do Cr and Cu doesn't contain a a full 4s orbital?

In the case of chromium (Cr), the electron configuration of 3d54s1 is more stable than 3d44s2. A half-filled sublevel is more stable than a sublevel that is less than half full. In the case of copper (Cu), the electron configuration of 3d104s1 is more stable than 3d94s2, again because a full sublevel and a half-filled sublevel is more stable.


Why do all enzymatic reactions need activation energy?

Energy is required to disrupt a substrate's stable electron configuration


Why is the second ionization energy of boron higher than carbon?

becasue when you remove a second elctron from Boron you are entering a new sublevel, the 2s sublevel, which already contains 2 electrons and is in a stable form, where as when you are removing a second electron from carbon it is still in the same energy sublevel, the 2p sublevel so it requires less energy


Which atom in the ground state has a stable valence electron configuration?

Neon has 8 valence electrons, which is a stable valence electron configuration.



What do many stable ions have an electron configuration of?

Many stable ions have the configuration of a noble gas.


The most stable type of electron configuration?

The noble gas configuration is known as the most stable configuration that an atom can achieve. In other words, the valence shell with ns2 np6 electron configuration.


Why is the first ionization energy of arsenic greater than selenium?

There's two ways to answer this question. First electron configurations with half-filled sublevels are more stable then electron configurations that don't have half-filled sublevels. Since Selenium is one elctron away from achieving a more stable half-filled sublevel configuration it more readily gives up it's outermost electron, so less energy is requires to remove the outermost electron. Arsenic already has the stable configuration of half-filled sublevel so it wouldn't give up it's electron as readily, so more energy is required to remove it. Another way to look at it is that Selenium's outermost electron is in a p orbital that already has an electron so there is electron electron repulsion present in that orbital so it's attraction to the nucleus is less which is why less energy is required to remove it so the ionization energy is less. Arsenic has it's outermost electron unpaired in the p orbital so there is no electron electron repulsion present in that orbital so more energy is required to remove it then for Selenium's outer most electron. Hope this helps!


What is a pseudo-noble gas formation?

Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.


How many electrons must be gained for phosphorus to have a stable electron configuration?

Phosphorus must gain 3 electrons to achieve a stable electron configuration.


What is the formula of the ion formed when sodium achieves a stable electron configuration?

Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.


Why is the second ionization energy of chromium higher than manganese?

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What symbol would represent a chlorine ion that has ionized to have a stable electron configuration?

What symbol would represent a chlorine ion that has ionized to have a stable electron configuration?


What is a stable electron configuration for neon?

The electron configuration of 10Ne is [1s2.2s2. 2p6]; it is very stable, obeying the 'Octet'-rule (like all noble gases do).


How do ionic compound obtain a stable electron configuration?

They achieve stable configuration by sharing their electrons in their outermost shell.


What makes an element inert or inactive?

The electron configuration is responsible for this. If the elements have a stable electron configuration, they become inert.


What does oxygen need to do in order to to achieve a stable electron configuration?

Oxygen atoms need to share or gain two electrons in order to achieve a stable electron configuration.


How many electrons does silicon need to gain or lose to have a stable electron configuration?

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What is the importance of electron configuration?

electronic configuration is important for the matter to be stable or octet to be complete


What is the correct electron configuration for Cu?

The electron configuration of copper is: [Ar]4s13d10. It isn't 4s23d9 because Cu is able to obtain a more stable electron configuration when it takes an electron from the 4s and adds it to 3d. A half filled 4s and a completely filled 3d is more stable.



Why is the ionisation energy of Nitrogen higher than Beryllium?

Beryllium is a metal. It has 2 valance electrons (in the outer shell), and therefore it tends to lose those electrons in order to achieve a stable electron configuration, which in the case of beryllium is also 2 electrons, but in the inner shell. Nitrogen is a nonmetal, with 5 valence electrons, and it tends to acquire more electrons in order to reach a stable electron configuration of 8. Less energy is need to lose electrons when the result is going to be a stable electron configuration.


Describe the type of electron configuration that makes an atom stable and not likely to react?

When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react.


Why is electron gain enthalpy of inert gases positive?

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