Ionization Energy Trends and Concepts

The video tutorial introduces ionization energy, defining it as the minimum energy required to remove an electron from an atom or ion in its gaseous state. It explains the first and second ionization energies with examples, highlighting that the second is greater than the first. The tutorial discusses factors affecting ionization energy, such as atomic radius, effective nuclear charge, and electron shielding. It also covers trends in ionization energy across periods and groups, noting that energy generally increases across a period due to increased nuclear charge and decreases down a group due to increased atomic radius and shielding.

What is the minimum energy required to remove an electron from an atom or ion called?

• Atomic radius

• Electronegativity

• Ionization energy

• Electron affinity

Which of the following statements is true about the first ionization energy?

• It is the energy required to remove 1 mol of electrons from 1 mol of gaseous ions.

• It is the energy required to remove 1 mol of electrons from 1 mol of gaseous atoms.

• It is the energy required to add 1 mol of electrons to 1 mol of gaseous atoms.

• It is the energy required to add 1 mol of electrons to 1 mol of gaseous ions.

Why is the second ionization energy generally higher than the first?

• Because the electron is removed from a neutral atom.

• Because the electron is removed from a negatively charged ion.

• Because the electron is removed from a stable atom.

• Because the electron is removed from a positively charged ion.

Which factor does NOT affect ionization energy?

• Atomic radius

• Nuclear charge

• Shielding effect

• Molecular weight

How does a larger atomic radius affect ionization energy?

• Decreases ionization energy

• Doubles the ionization energy

• Increases ionization energy

• Has no effect on ionization energy

What happens to ionization energy as effective nuclear charge increases?

• Ionization energy becomes zero

• Ionization energy remains constant

• Ionization energy increases

• Ionization energy decreases

What is the effect of increased shielding on ionization energy?

• Has no effect on ionization energy

• Decreases ionization energy

• Increases ionization energy

• Doubles the ionization energy

What trend is observed in ionization energy across a period?

• It fluctuates randomly

• It remains constant

• It increases from left to right

• It decreases from left to right

Why does ionization energy increase across a period?

• Due to decreased electron affinity

• Due to decreased shielding effect

• Due to increased nuclear charge

• Due to increased atomic radius

What is the overall trend of ionization energy across a period?

• It becomes zero

• It decreases

• It increases

• It remains the same