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Why does ionization energy increase as atomic radius decreases?


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Answered 2008-02-11 01:35:13

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.

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due to increase in atomic number,the ionization energy decreases within a group. therefore hydrogen has grater ionization energy than lithium.


Atomic radius is inversely proportional to first ionization energy. As atomic radius increases, first ionization energy decreases.



Atomic radius is inversely proportional to first ionization energyAs Atomic radius INCREASE, Ionization energy DECREASE


as atomic number increases, ionization energy also decreases


As the atomic number increases within a group, the ionization energy decreases .


Ionization energy decreases with the rise of atomic number in a group of periodic table.


Ionization energy decreases down due to increase in shielding effect.


there is an increase in atomic number and atomic size down the group due to addition of extra shells.this increase in the atomic size overcomes the effect of an increase in the nuclear charge.Therefore ionisation energy decreases with an increase in atomic size i.e.,it decreases as one moves down a group..


Radon (as down a group, the atomic size increases and the ionization energy decreases)


as atomic radius increases, ionisation energy decreases.


No, ionization energy increase when we move from left to right (in a period) in periodic table, because atomic size decreases and nuclear charge increases.


As you move down a column (group) in the periodic table, the electronegativity decreases, the ionization energy decreases, the electron affinity decreases, and the atomic radius increases.


Ionization energy increase from left to right. Ionization decreases going down a cloumn. Answer= Cs, K, Li


because chlorine has larger size than oxygen and ionization energy decreases with increase in size


Ionization energy increases as we go across a period and decreases as descend in a group.


In a group the ionization energy decrease when the atomic radius increase; in a period this relation is not generally valid.


The atomic size decreases (with some exceptions) , the ionization energy , electronegativity and electron affinity also increase from left to right.


IONIZATION ENERGYWhen it increases the energy level increases and the atoms start to vibrate more often, there is a state which is when crossed then the state of the body changes ....... and when the ionization energy decreases the vibration of the body and the energy also decrease so the state of the body changes again.


Yes, it is. Use the following as a general rule for metals. In a period, reactivity for metals will decrease when atomic number increases becasue the ionization energy increase. In groups, reactivity of metals increases because the ionization energy decreases. Source: http://www.chemcool.com


Ionization energy increase across a period and decreases down a group, therefore the the element with the greater ionization energy would be found in the top right of the periodic table. In this instance fluorine, F would have the greater ionization energy.


The relationship between atomic numbers and first ionization energies is that within the same period, as atomic number increases so does first ionization because as nuclear charge increases and atomic radius decreases, electrons become harder to remove. However, within the same group, the first ionization energy decreases as atomic number increases because of the added energy level, the electrons are farther from the nucleus and easier to remove.


More the atomic size lesser ionization energy.


On the periodic table, ionization energy increases moving left to right within a period and up within a group. It decreases as the atomic radius increases in size.


From left to right on the periodic table, ionization energy increases. From top to bottom in a column (group) the ionization energy decreases.



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