Why do ionization energy increase across a period but decrease down a group?

Why do ionization energy increase across a period but decrease down a group?

The ionization energy of the elements within a period generally increases from left to right. This is due to valence shell stability. The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding.

Why does ionization energy increase across a period quizlet?

As you move across a period, the first ionization energy increases. The atomic radii (size of the atom) becomes smaller as you move across the period because there is a progressively higher nuclear charge. This makes it harder to remove the outermost electron.

What is ionization energy How does it vary in period of the periodic table?

The ionization energy of an element increases as one moves across a period in the periodic table because the electrons are held tighter by the higher effective nuclear charge.

Why does ionization energy increase from left to right quizlet?

Ionization energy increases left to right across a period. As you go down a group, the valence electrons are farther away from the nucleus, and so it takes less energy to pull them away from the atom. The more electrons in the outside energy level, the less eager an atom will be to lose an electron.

What is ionization energy explain the factors affecting ionization energy?

Ionization energy depends on two factors: The force of attraction between electrons and the nucleus. The force of repulsion between electrons.

What is ionization energy How does ionization energy vary in a group and period?

In a group as we move down , ionization energy decreases and in a period , as we move from left to right , the ionization energy increases .

What is ionization energy describe how it changes going across a period and going down in a group use details to support your answer?

Moving left to right within a period or upward within a group, the first ionization energy generally increases. As the atomic radius decreases, it becomes harder to remove an electron that is closer to a more positively charged nucleus.

What happens across a period?

Elements in the same period have the same number of electron shells; moving across a period (so progressing from group to group), elements gain electrons and protons and become less metallic. This arrangement reflects the periodic recurrence of similar properties as the atomic number increases.