C.their atomic radius is small
D.layers of electron shells shield the protons' attractive force
fewer layers of electron shells create less shielding of the protons' attractive force
Apex:
layers of electron shells shield the protons' attractive force
their atomic radius is large
Their atomic radius is small
They have fewer electron shells to shield the protons from the electrons
The outermost electron is furthest from the nucleus, so it's less strongly attracted to the nucleus. Thus it's easier to remove (so it has a lower activation energy than a closer electron).
Ionization energies go down of course. This is because radii are becoming larger due to addition of electron levels. These farther from the nucleus electrons require less and less energy to liberate from the atom.
The ionization energy increases going across a periodic table.This is because of increasing nuclear charge.
Group 8 (noble gases) have the highest first ionization energy because they are already stable and don't want to lose any electrons. Ignoring the noble gases, however, group 7 halogens (F, Cl, Br, I, etc.) have the highest first ionization energy. That's because these elements have seven valence electrons, and they don't want to give up any electrons - they want another one!
Bottom left elements of the periodic table have low first ionization energies. Ionization energy is the minimum energy required to remove the outermost electron from an isolated gaseous atom to covert it into monovalent ion. Ionization energy depends on the electrostatic force of attractionbetween the nucleus of the atom and the outermost or valence electron. More the attraction more the energy needed.First of all the size of atoms of bottom left elements is larger as compared to other elements. Therefore, the electrons in the valence or outermost shell are at large distance from nucleus and feel less electrostatic force of attraction and are easier to remove. With increase in atomic number the number of inner shells of electron increases as a result of which shielding or screening effect increases. Since these elements have more number of inner shells so screening effect is more which further decreases the force of attraction. However, the high nuclear charge should cause more attraction but combined effect of nuclear charge, screening effect and large distance from nucleus result in decrease in attraction. Decreased attraction means it will be easier to remove valence electron and ionization energy will be low. It should be noted that only first ionization energy in case of group 1 elements and first and second ionization energy in case of group 2 elements is low but once the atoms of these elements acquire noble gas configuration by losing electrons their ionization energy becomes unusually high.
Nitrogen has the highest first Ionization potential.
Fluorine because it is the furthest right on the periodic table. Do no include noble gases in energies.
All of the elements on the top half of the periodic table belong in upperionizationenergy because the trend is top to bottom. Top being lowest and getting bigger as it goes down.------------------------------------------------------* In a group: the ionization energy decrease from the lighter elements to heavier elements.* In a period: the ionization energy increase from the left elements to the elements of the right.* When the atomic radius decrease the ionization energy increase.
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.
The noble gases of each period have the highest ionization energies in their periods. Refer to the related link to see a graph showing the ionization energies of the elements across each period.
Ionization energies decrease moving down a group, because the shielding effect reduces the pull of the nucleus on valence electrons. Making them easier to remove.
Ionization energies go down of course. This is because radii are becoming larger due to addition of electron levels. These farther from the nucleus electrons require less and less energy to liberate from the atom.
The ionization energy increases going across a periodic table.This is because of increasing nuclear charge.
Moving from left to right across a period, the first ionization energy increases because it becomes increasingly difficult to remove an electron.
Group 8 (noble gases) have the highest first ionization energy because they are already stable and don't want to lose any electrons. Ignoring the noble gases, however, group 7 halogens (F, Cl, Br, I, etc.) have the highest first ionization energy. That's because these elements have seven valence electrons, and they don't want to give up any electrons - they want another one!
Non-metals have higher ionization energies within the same period. This is because non-metals want to gain electrons to be able to be like the nearest noble gas.
Bottom left elements of the periodic table have low first ionization energies. Ionization energy is the minimum energy required to remove the outermost electron from an isolated gaseous atom to covert it into monovalent ion. Ionization energy depends on the electrostatic force of attractionbetween the nucleus of the atom and the outermost or valence electron. More the attraction more the energy needed.First of all the size of atoms of bottom left elements is larger as compared to other elements. Therefore, the electrons in the valence or outermost shell are at large distance from nucleus and feel less electrostatic force of attraction and are easier to remove. With increase in atomic number the number of inner shells of electron increases as a result of which shielding or screening effect increases. Since these elements have more number of inner shells so screening effect is more which further decreases the force of attraction. However, the high nuclear charge should cause more attraction but combined effect of nuclear charge, screening effect and large distance from nucleus result in decrease in attraction. Decreased attraction means it will be easier to remove valence electron and ionization energy will be low. It should be noted that only first ionization energy in case of group 1 elements and first and second ionization energy in case of group 2 elements is low but once the atoms of these elements acquire noble gas configuration by losing electrons their ionization energy becomes unusually high.
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.