Periodic Table Trends and Electron Behavior

The video tutorial covers three major trends in the periodic table: ionization energy, electron affinity, and atomic radius. Ionization energy is the energy required to remove electrons from an atom, increasing across a period and decreasing down a group. Electron affinity, the energy change when an electron is added, follows a similar trend. Examples with sodium and aluminum illustrate these concepts, highlighting the role of valence and core electrons.

What are the three major trends discussed in the periodic table?

• Color, texture, hardness

• Ionization energy, electron affinity, atomic radius

• Melting point, boiling point, density

• Conductivity, malleability, ductility

What happens to ionization energy as you move across a period in the periodic table?

• It decreases

• It remains constant

• It increases

• It fluctuates randomly

Why is it easier to remove electrons as you move down a group in the periodic table?

• Electrons are farther from the nucleus

• The number of protons decreases

• The atomic mass decreases

• Electrons are closer to the nucleus

Which electron is removed first from sodium during ionization?

• 2s electron

• 1s electron

• 2p electron

• 3s electron

How many valence electrons does aluminum have?

• One

• Four

• Two

• Three

What is electron affinity?

• The energy released when an electron is added

• The size of an atom

• The number of protons in an atom

• The energy required to remove an electron

How does electron affinity change as you move across a period?

• It decreases

• It increases

• It remains constant

• It fluctuates randomly

What is the trend for electron affinity as you move down a group?

• It fluctuates randomly

• It remains constant

• It decreases

• It increases

Which of the following trends is similar for both ionization energy and electron affinity?

• Both fluctuate randomly across a period

• Both remain constant across a period

• Both decrease across a period

• Both increase across a period

Why is it less favorable for electron affinity as you move down a group?

• The atomic mass decreases

• Electrons are closer to the nucleus

• Electrons are farther from the nucleus

• The number of protons decreases