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Because they have many electron shells.
The reduction in the force of attraction between the nucleus and outer most electron is known as shielding effect
Shielding actually reduces ionization energy. Let's look at some atomic structure and see why. Electrons form shells around an atomic nucleus. The inner electrons shells shield the outer electrons shells and reduce the affect of the nuclear "pull" on those outer electrons. The shielding provided by the inner electrons means it will take less energy to free outer electrons from their orbitals, and thus the ionization energy of an outer electron is reduced by the effects of shielding.
s > p > d > f
yes, increases from left to right
in metals due to shielding effect ionization value is low
The shielding effect reduces the ionization energy and so makes cation formation easier.
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.
Because they have many electron shells.
Na have higher shielding effect than Li *According to my chemistry book
YES
The reduction in the force of attraction between the nucleus and outer most electron is known as shielding effect
The shielding effect in chemistry refers to inner electrons shielding outer electrons from the attraction of the nucleus in an atom. This results in a decrease in the effective nuclear charge felt by the outer electrons, leading to changes in atomic and chemical properties such as ionization energy and atomic size in elements across a period.
When a period of elements are considered, the element in group 18 has the highest shielding effect.
Shielding actually reduces ionization energy. Let's look at some atomic structure and see why. Electrons form shells around an atomic nucleus. The inner electrons shells shield the outer electrons shells and reduce the affect of the nuclear "pull" on those outer electrons. The shielding provided by the inner electrons means it will take less energy to free outer electrons from their orbitals, and thus the ionization energy of an outer electron is reduced by the effects of shielding.
Because fluorine's size is lower than that of iodine, it has a greater ionization energy than iodine. Fluorine, on the other hand, appears to have a smaller shielding effect. As a result, fluorine's nucleus attracts more valence electrons than iodine's.
In electronegativity, the first ionization energy increases as it moves from left to right across a period . The nuclear charge also increases and the shielding effect is constant when moving across.