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Why is there a large jump between 10 and 11 ionization ehergies of magnisium?
Wiki User
∙ 13y ago
- the large jump is caused because magnisium is such a powerful element that if it was combined in an explosive it have the power of an atomic bomb
Wiki User
∙ 13y ago
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What does large standard deviation signify?
That there is quite a large amount of variation between the observations.
Between his large number of friends?
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Which element's second ionization energy level is large compared to its first ionization energy?
Cl
In which of these galaxies would you be least likely to find an ionization nebula?
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Which has lower ionization energy an atom with a small radius or an atom with a large radius?
Lower ionization energy would be associated with the larger atom, as the outer most electrons would be further from the nucleus, and not held as tightly.
The atoms of the most active non-metals have?
large atomic radii and low ionization energies
How are charges developed in the Large Hadron Collider?
Like most high energy accelerators, the LHC begins the ionization process with Cockcroft-Walton Generators.
Which alkali metal is most reactive with oxygen?
Francium is an alkaline metal, which means that its one electron is easily given away, making it highly reactive. Because the atom is so large, there is a shielding effect between the protons in the nucleus, and the valence electron. This blocks the attractive forces, and the other layers of electrons work to repel the valence electron, decreasing the ionization energy even further. The low ionization energy is what makes francium so reactive, that none of it can be isolated effectively.
Is medium between small and large?
Yes, medium is between small and large.
Why the first ionization energy for sodium is much smaller than the second ionization energy for sodium?
Ionization energy is referred to the amount of energy required to remove an electron from it's nucleus.The first ionization energy refers to the valence electron (the electron on the outer most shell)Blatantly, we can say that is requires less energy to remove valence electrons, rather than electrons in other orbitals, because it is farther away from the proton and therefore take less energy to remove that electron (ionization energy).The large discrepancy between the first and second ionization energies can be accounted for, by some of these factors:- such as shielding: basically the inner most electrons block some of the attractive forces from the nucleus (protons) and the valence electrons therefore have the most electrons blocking for them, because they are "in front" of all of the other electrons, on the outer most shell. Having this energy blocked means they are more free to move about.-Inverse square relationship between the first and Nth (n) shell: I won't write the entire equation but basically:the energy to be removed from the first shell is / by n^2, where n is the shell where the electron is removed from.Hence for the first (n=1) shellIE from 1st/ 1^2 = IE/1 = IE , this means that the energy to be removed from the first shell relative to itself is = which is true. This step is important.However, if we use the second shell (n=2), this is the second ionization energy.IE/2^2 = IE/4 , this means 4Xtimes LESS energy is needed to remove an electron from the second shell compared to the firstand then, if we use the third shell (n=3), which is the valence electron , also the FIRST Ionization energy.IE/3^2 = IE/9 , this means 9Xtimes LESS energy is needed to remove an electron from the third shell compared to the first.Conclusion: if we compare the first and second ionization energies, they are radically different from one another and there's a large discrepancy between the values due to the inverse square relationship between IE from the first energy level to the Nth level.
Why do group 1 elements have a low density?
The group one elements have the lowest ionization energies because of their large atomic size which makes the outermost electron only weekly held by the nucleus.
Why is there such a large jump in ionization enery between the second and third ionization energies for magnesium?
The second ionization involves the removal of an electron from the outer S orbital to give a stable noble gas-like electron configuration. However, the third ionization removes an electron from the inner shell, which is much less energetically favorable.
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Why boron is non metal?
THE STRONGER THE TENDENCY TO LOSE ELECTRONS,THE MORE ELECTROPOSITIVE AND MORE METALLIC AN ELEMENT IS.SINCE BORON IS VERY SMALL AND THE FORCE OF ATTRACTION BETWEEN THE NUCLEUS AND THE VALENCE ELECTRON IS VERY HIGH,AS WELL AS LARGE VALUE OF IONIZATION POTENTIAL INDICATES THAT BORON DOES NOT HAVE THE TENDENCY TO LOSE ELECTRONS THAT IS WHY IT IS LESS ELECTROPOSITIVE AND THEREFORE IT IS A NON-METAL
