Ionization Energy Trends in the Periodic Table

The video explains ionization energy, the energy needed to remove an electron from a gaseous atom or ion. It covers how ionization energy varies across the periodic table, increasing from left to right and bottom to top. Metals have low ionization energy, while non-metals have high ionization energy. The video also discusses the concept of first and second ionization energies, emphasizing that removing additional electrons becomes progressively harder. An analogy is used to illustrate this concept, comparing it to repeatedly asking for money.

What is ionization energy?

• The energy required to add an electron to an atom

• The energy required to remove an electron from a gaseous atom or ion

• The energy released when an atom gains an electron

• The energy required to split an atom into ions

Which of the following statements is true about ionization energy?

• It applies to all elements once they are in gaseous form

• It is the energy released when an atom loses an electron

• It is only applicable to gaseous elements at room temperature

• It is the energy needed to add an electron to a solid atom

What does a low ionization energy indicate about an element?

• It is difficult to remove an electron

• It is easy to remove an electron

• The element is a non-metal

• The element is stable

How does ionization energy change across a period on the periodic table?

• It decreases from left to right

• It remains constant

• It increases from left to right

• It decreases from top to bottom

Which element has the highest ionization energy?

• Oxygen

• Helium

• Francium

• Lithium

What happens to ionization energy as you move from the bottom to the top of a group in the periodic table?

• It remains the same

• It increases

• It decreases

• It fluctuates randomly

Which element is expected to have the lowest ionization energy?

• Francium

• Carbon

• Helium

• Neon

What is the term for the energy required to remove the first electron from an atom?

• First ionization energy

• Electron affinity

• Electronegativity

• Second ionization energy

Why does removing each successive electron from an atom require more energy?

• The atom becomes larger

• The remaining electrons are more tightly bound

• The atom gains more electrons

• The atom becomes more stable

What analogy is used to explain the concept of successive ionization energies?

• Giving away dollars one at a time

• Climbing a staircase

• Removing layers of an onion

• Filling a bucket with water