Exploring Periodic Table Trends in AP Chemistry

This video tutorial covers periodic table trends, focusing on atomic radius, ionization energy, electronegativity, and electron affinity. It explains each term, discusses trends across periods and down groups, and highlights the importance of understanding these trends for exams. The video emphasizes the role of protons, electron shells, and effective nuclear charge in determining these trends.

Which of the following is NOT one of the four key trends discussed in the video?

• Electronegativity

• Atomic Radius

• Molecular Weight

• Ionization Energy

How is atomic radius defined in the context of the periodic table?

• Half the distance between two adjacent nuclei

• The distance from the nucleus to the outermost electron

• The distance from the nucleus to the valence shell

• The distance between two electrons in the same shell

What does ionization energy refer to?

• The energy required to break a chemical bond

• The energy released when an atom gains an electron

• The energy required to remove the most loosely bound electron

• The energy required to add an electron to an atom

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Which electron is removed first in the ionization process of a transition metal?

• The electron in the 2s orbital

• The electron in the 3p orbital

• The electron in the 3d orbital

• The electron in the 4s orbital

What does electronegativity measure?

• The number of valence electrons

• The attraction an atom has for an electron

• The energy required to remove an electron

• The size of an atom

What is electron affinity?

• The energy required to remove an electron

• The size of an atom

• The attraction an atom has for an electron

• The change in energy when a neutral atom gains an electron

What happens to atomic radius as you move across a period?

• It fluctuates

• It increases

• It decreases

• It remains the same

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How does ionization energy change across a period?

• It remains the same

• It fluctuates

• It increases

• It decreases

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

• It fluctuates

• It remains the same

• It decreases

• It increases

Why is there no strong trend for electron affinity down a group?

• Because the ionization energy remains the same

• Because the atomic radius remains the same

• Because the number of valence electrons remains the same

• Because the number of protons remains the same

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