Ionization Energy and Atomic Structure

The video tutorial explains ionization energy as the energy required to remove an electron from an atom. It uses an analogy of stealing purses to illustrate the concept, comparing it to the effort needed to remove electrons. The tutorial also discusses atomic size trends in the periodic table, explaining how atoms get larger as you move down a group and smaller across a period. It relates these trends to ionization energy, noting that larger atoms have lower ionization energy. Finally, it explains why metals tend to form positive ions and non-metals form negative ions based on their ionization energies.

What is ionization energy best described as?

• The energy required to add an electron to an atom

• The energy required to combine two atoms

• The energy required to remove an electron from an atom

• The energy required to split an atom

In the analogy used, what does a low ionization energy correspond to?

• A locked purse

• A strong grip on a purse

• A weak grip on a purse

• A heavy purse

How does ionization energy change as it becomes easier to remove an electron?

• Ionization energy fluctuates

• Ionization energy decreases

• Ionization energy increases

• Ionization energy remains constant

What happens to atomic size as you move down a group in the periodic table?

• It decreases

• It increases

• It remains the same

• It fluctuates

As you move from left to right across a period, what happens to the atomic size?

• It remains constant

• It decreases

• It fluctuates

• It increases

What causes the atomic size to decrease across a period?

• Loss of energy levels

• Addition of more electrons

• Addition of more protons

• Loss of protons

How does a larger atomic size affect ionization energy?

• Has no effect

• Fluctuates ionization energy

• Decreases ionization energy

• Increases ionization energy

Which type of atoms hold their electrons more tightly?

• Larger atoms

• Smaller atoms

• Atoms with fewer protons

• Atoms with more energy levels

Why do metals tend to form positive ions?

• They have tightly held electrons

• They have small atomic size

• They have low ionization energy

• They have high ionization energy

What is a characteristic of non-metals in terms of ion formation?

• They form positive ions

• They form negative ions

• They form both positive and negative ions

• They do not form ions