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Why second ionization energy of alkali metals are higher than first ionization energy?
The alkali metals are Li,Na,K,Rb,Cs,Fr.If v see their general electronic configuration,v see that its (n-1)p6 ns1.That means the outer most s orbital contains 1 unpaired electron and just in the inner shell there is fully filled p orbital. 1st ionisation energy is the amount of energy required to remove 1st electron from the outermost shell of an isolated gaseous ion.here v see that the energy required 2 remove 1 electron from outermost shell will be very less cos it helps the atom to achieve fully filled stable electronic configuration. On the other hand,2nd ionisation energy is the energy required 2 remove an electron from isolated gaseous +1 atom,means atom from where 1 electron has already been removed. So here,it is very difficult to remove 1 more electron from the stable fully filled p orbital and large amount of energy is needed.Hence the 2nd IE shoots up considerably as compared to d 1st IE. Hope it's clear...:)..
Think about what happens when you ionize an alkali metal (keeping in mind that alkali metals are the first group and contain 1 valence electron). When you ionize an alkali metal, you remove it's one valence electron. The first ionization energy is relatively low, because this actually stabilizes the atom. However, the second ionization energy is much higher because the already ionized alkali metal now contains a stable outer shell and is much less willing to lose another electron.
The alkali metals are Li,Na,K,Rb,Cs,Fr.If v see their general electronic configuration,v see that its (n-1)p6 ns1.That means the outer most s orbital contains 1 unpaired electron and just in the inner shell there is fully filled p orbital. 1st ionisation energy is the amount of energy required to remove 1st electron from the outermost shell of an isolated gaseous ion.here v see that the energy required 2 remove 1 electron from outermost shell will be very less cos it helps the atom to achieve fully filled stable electronic configuration. On the other hand,2nd ionisation energy is the energy required 2 remove an electron from isolated gaseous +1 atom,means atom from where 1 electron has already been removed. So here,it is very difficult to remove 1 more electron from the stable fully filled p orbital and large amount of energy is needed.Hence the 2nd IE shoots up considerably as compared to d 1st IE. Hope it's clear...:)..
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What is the relationship between ionization energy and the alkali metals?
There is no relation ship. They have the lowest ionization energies.
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.
What is the group trend for the ionization energy for the alkali metals?
As you go down the group (any group), ionization energy decreases. So in terms of ionization energy, for the alkali metals, Lithium > Sodium > Potassium > Rubidium > Caesium > Francium
Do alkali metals react slower or faster than alkaline earth metals?
Alkali metals react faster than alkaline earth metals due to their lower ionization energy and higher reactivity. Alkali metals readily lose their outermost electron to form a +1 cation, making them highly reactive with water and air. Alkaline earth metals, on the other hand, are less reactive as they have higher ionization energies and require more energy to lose their outer electron.
What element in family IA has the lowest ionization energy?
the lowest ionization energy in IA :hydrogen ,lithiun ,sodium and potassium
What is the relationship between ionization energy and the alkali metals?
There is no relation ship. They have the lowest ionization energies.
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.
What is the group trend for the ionization energy for the alkali metals?
As you go down the group (any group), ionization energy decreases. So in terms of ionization energy, for the alkali metals, Lithium > Sodium > Potassium > Rubidium > Caesium > Francium
Do alkali metals react slower or faster than alkaline earth metals?
Alkali metals react faster than alkaline earth metals due to their lower ionization energy and higher reactivity. Alkali metals readily lose their outermost electron to form a +1 cation, making them highly reactive with water and air. Alkaline earth metals, on the other hand, are less reactive as they have higher ionization energies and require more energy to lose their outer electron.
What element in family IA has the lowest ionization energy?
the lowest ionization energy in IA :hydrogen ,lithiun ,sodium and potassium
Why do alkali metals have lower ionization energies than the alkali earth metals?
Alkali gases only have 1 electron needing to be removed to reach a stable noble gas configuration. Alkaline earths have two electrons. Alkali metals thus have the lower ionization energy of the two groups.
Alkali metal and alkaline earth metal have how many ionization energies?
Alkali metals (group 1 elements) have one valence electron. Hence have one ionization energy Alkaline earth metals (group 2 elements) have two valence electron. Hence have two ionization energy
Which element has a lower 1st ionization energy than aluminum?
The element that has a lower 1st ionization energy than aluminum is magnesium.
What Alkali metal has the highest ionization energy?
Among the alkali metals, lithium has the highest ionization energy. This is because it is the smallest alkali metal, so the outermost electron is held more tightly due to increased nuclear charge and decreased atomic size.
Is alkali metals most suitable for photoelectric emission?
yes, they are, as they have the least ionization energy among all elements
Which two families in the periodic table have the most reactive metals?
The alkali metals (Group 1) and the alkaline earth metals (Group 2) are the two families in the periodic table with the most reactive metals. Alkali metals are more reactive than alkaline earth metals due to their lower ionization energy and higher reactivity with water and air.
Why do the alkali metal have lower ionization energies than the alkaline earth metals?
Alkali gases only have 1 electron needing to be removed to reach a stable noble gas configuration. Alkaline earths have two electrons. Alkali metals thus have the lower ionization energy of the two groups.
