Trends in Ionization Energy

The video tutorial explores ionization energy, the energy needed to remove the highest energy electron from an atom. It examines trends in ionization energy across groups and periods in the periodic table. Generally, ionization energy decreases down a group and increases across a period. The video explains these trends by discussing atomic structure, electron shielding, and nuclear charge. As you move down a group, increased electron shielding and atomic radius make it easier to remove electrons. Conversely, moving across a period, increased nuclear charge makes it harder to remove electrons.

What is ionization energy?

• The energy required to split an atom into ions

• The energy required to add an electron to an atom

• The energy released when an atom gains an electron

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

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

• Ionization energy fluctuates randomly

• Ionization energy decreases

• Ionization energy remains constant

• Ionization energy increases

Which of the following best describes the trend in ionization energy across a period?

• Ionization energy decreases

• Ionization energy increases

• Ionization energy remains constant

• Ionization energy fluctuates randomly

What causes the decrease in ionization energy as you move down a group?

• Decrease in nuclear charge

• Increase in nuclear charge

• Decrease in atomic radius and electron shielding

• Increase in atomic radius and electron shielding

Why does ionization energy generally increase across a period?

• Decrease in atomic radius and increase in nuclear charge

• Increase in atomic radius and decrease in nuclear charge

• Increase in electron shielding

• Decrease in electron shielding

What is the effect of electron shielding on ionization energy?

• It decreases ionization energy

• It increases ionization energy

• It causes ionization energy to fluctuate

• It has no effect on ionization energy

How does atomic radius affect ionization energy?

• Larger atomic radius decreases ionization energy

• Atomic radius has no effect on ionization energy

• Smaller atomic radius decreases ionization energy

• Larger atomic radius increases ionization energy

Which element would have a lower ionization energy, cesium or hydrogen?

• Cesium

• Hydrogen

• It depends on the temperature

• Both have the same ionization energy

What happens to the effective nuclear charge as you move across a period?

• It increases

• It decreases

• It remains constant

• It fluctuates randomly

Why is it harder to remove an electron from bromine compared to potassium?

• Potassium has a higher nuclear charge

• Bromine has a larger atomic radius

• Potassium has more electron shielding

• Bromine has a higher nuclear charge