6 posts • Page 1 of 1
ionization energy increases as it goes up and to the right. Up because the radius is much smaller so that the energy of removing an electron is higher and to the right because there are more protons to attract the electrons so the energy to remove an electron is much higher.
Ionization decreases down a group and increases across a period. The ionization energy decreases down a group because as the number of shells increases, the electrons are shielded from the nucleus, so it takes less energy to remove the last electron. The ionization energy increases across a period because the atomic radius decreases, so the nuclear charge increases and the electrons are pulled closer together to the nucleus so the energy to remove an electron is higher.
Ionization energy increases as you go up the periodic table and to the right of the table. As you travel up the periodic table, the atomic radius of a molecule gets smaller. This places electrons much closer to the nucleus than in a larger molecule making the electrons harder to remove from the smaller molecule. This means they require a higher ionization energy to remove the electrons.
Who is online
Users browsing this forum: No registered users and 5 guests