3 Forgotten brackets are back

I would like to ask a question about europium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of europium in its neutral state is $$\ce{[Xe] 4f^7 6s^2}$$$$\ce{[Xe] (4f)^7 (6s)^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] 4f^7}$$$$\ce{[Xe] (4f)^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] 4f^6}$$$$\ce{[Xe] (4f)^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled $$\ce{f}$$ sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for europium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?

I would like to ask a question about europium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of europium in its neutral state is $$\ce{[Xe] 4f^7 6s^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] 4f^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] 4f^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled $$\ce{f}$$ sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for europium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?

I would like to ask a question about europium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of europium in its neutral state is $$\ce{[Xe] (4f)^7 (6s)^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] (4f)^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] (4f)^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled $$\ce{f}$$ sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for europium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?

2 added 7 characters in body; edited tags; edited title

# Europium stability in $+2$+2 and $+3$+3 state

I would like to ask a question about Europium'seuropium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of Europiumeuropium in its neutral state is $$\ce{[Xe] 4f^7 6s^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] 4f^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] 4f^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled f$$\ce{f}$$ sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for Europiumeuropium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?

# Europium stability in $+2$ and $+3$ state

I would like to ask a question about Europium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of Europium in its neutral state is $$\ce{[Xe] 4f^7 6s^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] 4f^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] 4f^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled f sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for Europium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?

# Europium stability in +2 and +3 state

I would like to ask a question about europium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of europium in its neutral state is $$\ce{[Xe] 4f^7 6s^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] 4f^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] 4f^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled $$\ce{f}$$ sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for europium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?

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# Europium stability in $+2$ and $+3$ state

I would like to ask a question about Europium's stability in the $$+2$$ and $$+3$$ oxidation state.

The electronic configuration of Europium in its neutral state is $$\ce{[Xe] 4f^7 6s^2}$$.

Now, when in the $$+2$$ oxidation state, the electronic configuration is $$\ce{[Xe] 4f^7}$$ and in the $$+3$$ oxidation state, it is $$\ce{[Xe] 4f^6}$$.

Now, I thought the $$+2$$ oxidation state is more stable because it's a half-filled f sub-shell so there is less mutual repulsion between electrons in the same sub-shell.

However, an article from nature.com reads the following:

Europium metal is now known to be highly reactive; the element's most stable oxidation state is +3, but the +2 state also occurs in solid-state compounds and water.

Now, I would like to ask, how is it possible for Europium to be most stable in its $$+3$$ oxidation state, knowing what I have mentioned above?