Periodic Table Trends: Electronegativity, Atomic Radius, and More

The video tutorial covers four key periodic table trends: electronegativity, atomic radius, ionization energy, and electron affinity. It explains how these trends generally increase across periods and the role of effective nuclear charge (Zeff) in influencing these trends. The tutorial also highlights exceptions, such as noble gases, and provides detailed comparisons between elements like lithium and fluorine to illustrate these concepts.

Which of the following is NOT one of the four periodic table trends discussed?

• Ionization Energy

• Melting Point

• Atomic Radius

• Electronegativity

What is the Zeff nuclear charge?

• The charge of the nucleus

• The charge of the outermost electron

• The effective nuclear charge experienced by an electron

• The total number of protons in the nucleus

Why does electronegativity increase as you move to the right in the periodic table?

• Because the number of protons decreases

• Because the number of neutrons increases

• Because the number of electrons decreases

• Because the number of protons increases

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which element is more electronegative, carbon or fluorine?

• Neither

• Both have the same electronegativity

• Fluorine

• Carbon

Why does atomic radius decrease as you move to the right in the periodic table?

• Because the Zeff nuclear charge decreases

• Because the number of electron shells increases

• Because the number of protons decreases

• Because the Zeff nuclear charge increases

Tags

NGSS.HS-PS1-1

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

• It remains the same

• It first increases then decreases

• It decreases

• It increases

What is ionization energy?

• The energy required to remove an electron from an atom

• The energy required to add an electron to an atom

• The energy released when an atom gains an electron

• The energy required to break a chemical bond

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Why does ionization energy increase as you move to the right in the periodic table?

• Because the number of electron shells increases

• Because the Zeff nuclear charge increases

• Because the atomic radius increases

• Because the number of protons decreases

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

What is electron affinity?

• The energy released when an atom loses an electron

• The energy released when an atom gains an electron

• The energy required to remove an electron from an atom

• The energy required to add a proton to an atom

Tags

NGSS.HS-PS1-4

How are ionization energy and electron affinity related?

• They are the same magnitude but opposite in sign

• They both decrease as you move to the right in the periodic table

• They are unrelated

• They both increase as you move down a group

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2