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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...:)..
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BlakeThink 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
