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Why second ionization energy of alkali metals are higher than first ionization energy?
Wiki User
∙ 6y ago
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...:)..
Minerva Orn
Wiki User
∙ 12y agoThink 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.
Wiki User
∙ 15y agoThe 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...:)..
Wiki User
∙ 6y agoThe attraction between the electrons involved and the atomic nucleus is stronger.
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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.
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
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.
Sodium an alkali metal and chlorine a halogen are both in Period 3 of the periodic table Which element has a higher ionization energy?
Chlorine has a higher ionization energy. Chlorine's tendency is to gain electrons, not lose them as metals usually do.
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.
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
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.
Sodium an alkali metal and chlorine a halogen are both in Period 3 of the periodic table Which element has a higher ionization energy?
Chlorine has a higher ionization energy. Chlorine's tendency is to gain electrons, not lose them as metals usually do.
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.
Which element has a lower 1st ionization energy than aluminum?
The first level ionization energy oif aluminium is 577,5 kJ/mol.All alkali metals have lower values for the ionization energy.
Which decreases with increases atomic number group 2A?
Group IIA metals (alkali earth) become more reactive with non-metals as you go higher in atomic numbers.
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 low ionization energy?
Francium (Fr) has the lowest Ionization potential.
Is alkali metals most suitable for photoelectric emission?
yes, they are, as they have the least ionization energy among all elements
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.
