Moving from left to right across a period, the general rise in the first ionization energy can be attributed to the?
decrease in nuclear charge
increase in nuclear charge
decrease in screening effect
increase in screening effect
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Ionization energy is inversely proportional to atomic radius. Across the period frm left to right, ionization increases due to decrease in d atomic radius which causes increase in d nuclear charge (addition of neutron).
As we move across the periodic table from left to right, the ionization energy increases , due to the effective nuclear charge increasing. This is because the larger the effective nuclear charge, the stronger the nucleus is holding onto the electron and the more energy it takes to release an electron
ionization energy is directly proportional to the nuclear charge . ionization energy moving from left to right across the period means the ionization enrgy is increasing. since ionization energy increases , nuclear charge increases.
From khanacademy.org
On the periodic table, first ionization energy generally increases as you move left to right across a period. This is due to “increasing nuclear charge”, which results in the outermost electron being more strongly bound to the nucleus.
Generally ionization energy increases across the period and decreases down the group. and when there is a decrease down a group there is always an increase in the nuclear charge so the answer is B.
