Understanding Atomic Radius and Ionization Energy

Which element has a larger atomic radius, Sodium (Na) or Magnesium (Mg)?

• Sodium (Na)

• Magnesium (Mg)

Which of the following elements has the highest ionization energy?

• Nitrogen (N)

• Oxygen (O)

As you move from left to right across a period in the periodic table, how does the atomic radius change?

• It increases

• It decreases

• It remains constant

Which factor does not affect ionization energy?

• Nuclear charge

• Atomic radius

• Electron shielding

• Color of the element

Which element has a smaller atomic radius, Chlorine (Cl) or Argon (Ar)?

• Chlorine (Cl)

• Argon (Ar)

What trend in ionization energy is observed as you move down a group in the periodic table?

• It increases

• It decreases

• It remains constant

Which of the following elements is expected to have the lowest ionization energy?

• Fluorine (F)

• Lithium (Li)

• Neon (Ne)

• Sodium (Na)

What is the primary reason for the decrease in atomic radius as you move across a period from left to right?

• Decrease in nuclear charge

• Increase in nuclear charge without an increase in energy level

• Increase in electron shielding

• Decrease in electron shielding

Which element has a higher ionization energy, Silicon (Si) or Phosphorus (P)?

• Silicon (Si)

• Phosphorus (P)

Why does ionization energy generally increase as you move from left to right across a period?

• Because atomic radius increases

• Because atomic radius decreases, leading to a stronger attraction between the nucleus and the valence electrons

• Because of increased electron shielding

• Because of decreased nuclear charge