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Answered 2009-10-14 08:28:42

magnesium has a 2 valence electrons. because the third electron is not a valence electron, or in the outer shell, much more energy would be needed to remove it

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The energy needed to remove an electron from an atom (in the gaseous state) is called the IONIZATION ENERGY.


IE is the energy needed to remove one electron from an atom.


Ionization energy is the energy needed to remove an electron from an element, whereas electron affinity is the amount of attraction a substance has for a electron. One is the amount of energy to remove an electron while the other is the likeliness for it to attract an electron.


The energy required to remove an electron from an atom is known as ionization energy. The ionization energy increases as the number of orbits around the nucleus increases.


Magnesium has higher 3rd ionisation energy. It is difficult to remove 3rd electron from completely filled orbit.


The amount of energy needed to remove the outermost electron.


the 1st ionization energy is the energy needed to remove an electron from a neutral atom. the 2nd IE is the energy needed to remove an electron from a +ve ion that carry one +ve charge. the 3rd IE is the energy needed to remove an electron from a +ve ion that carry two +ve charges. note : the nth ionization energy is less than the nth+1 ionization energy.


electrons in energy levels that are further from the nucleus have the most energy.(the electron shells closest to the nucleus have the lowest energy) this means because the second energy level is further from the nucleus than the first electron, more energy is going to be needed to remove the second electron.


The energy needed to remove an electron from an atom generally increases, decrease as you go across a period? Explain why ? please


The energy required to remove an electron from an atom is called ionization energy.


ionization potential energy. but remember the atom must be neutral .


First ionization energy is the energy required to remove the first outermost electron from an atom. The second ionization energy is the energy required to remove the next available electron, and is greater than the first IE. The third IE is that energy needed to remove the third electron, and is greater the the second IE.


the nucleous is positively charged , the electron is negatively charged..the closer to the nucleous an electron is the strongest is the force that attracts it (the force of the nucleous) so more energy is needed to remove it



Imagine that one electron has already been removed from an atom, the energy used to accomplish this is the 1st ionization energy. Now more energy is needed to remove a 2nd electron. That is the 2nd ionization energy.



the energy needed to remove the outermost, or highest energy, electron from a neutral atom in the gas phase. reference related link


Ionization energy is how much energy is needed to remove an electron from the valence shell (the outermost shell). When the atomic radius is smaller, you will need more energy to remove an electron because the pull from the nucleus on the electron is stronger. If the atomic radius is larger, then it will be much easier to remove an electron from the valence shell because there are more layers (shieldings) between the nucleus and valence shell.


As the size of an atom increases, the energy needed to remove an electron decreases. As the size of an atom increases, the atomic radius increases: the distance between the nucleus and the outer electron shell becomes greater. This means that the positive nuclear charge has less of an effect on the negatively charged electron, so the attractive force between the nucleus and the electron is weaker. Less energy is required to overcome the weaker force.



The energy needed to remove a second, third or forth electron from one mole of gaseous ions.



In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.


The amount of energy required to remove an electron form an at is the ionization energy.


A work function is a term used in physics for the minimum amount of energy needed to remove an electron from the surface of a material.



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