Ionization Energy Trends in the Periodic Table

The video tutorial explains ionization energy, the energy needed to remove the highest energy electron from an atom. It discusses trends in ionization energy across the periodic table, noting that it generally decreases down a group and increases across a period. The video also explores the reasons behind these trends, such as atomic radius, electron shielding, and nuclear charge.

What is ionization energy?

• The energy required to add an electron to an atom

• The energy required to remove the highest energy electron from an atom

• The energy required to split an atom

• The energy required to form a chemical bond

What general trend is observed in ionization energy as you move down a group in the periodic table?

• Ionization energy decreases

• Ionization energy remains constant

• Ionization energy increases

• Ionization energy fluctuates randomly

As you move from left to right across a period, what happens to the ionization energy?

• It remains the same

• It increases

• It fluctuates

• It decreases

Why does ionization energy decrease as you move down a group?

• The atomic radius decreases

• The number of core electrons decreases

• The outer electrons are further from the nucleus and more shielded

• The number of protons decreases

What effect does increased shielding have on ionization energy within a group?

• It causes ionization energy to fluctuate

• It has no effect on ionization energy

• It decreases ionization energy

• It increases ionization energy

As you move across a period, why does ionization energy generally increase?

• The outer electrons are further from the nucleus

• The number of core electrons increases

• The number of protons increases, pulling electrons closer

• The atomic radius increases

What happens to atomic radius as you move from left to right across a period?

• It fluctuates

• It remains constant

• It decreases

• It increases

Which element would have a higher ionization energy, bromine or potassium?

• Both have the same ionization energy

• Potassium

• It depends on the temperature

• Bromine

What is the relationship between the number of protons and ionization energy across a period?

• The number of protons has no effect

• Fewer protons lead to higher ionization energy

• More protons lead to higher ionization energy

• More protons lead to lower ionization energy

Why is it easier to remove an electron from cesium compared to hydrogen?

• Cesium has fewer protons

• Cesium's outer electrons are more shielded and further from the nucleus

• Hydrogen has more electrons

• Hydrogen's electrons are more shielded