Effective Nuclear Charge and Atomic Radius Comparison

Very Hard General Chemistry Atomic Structure And Periodic Trends

Consider the properties of atomic structure and how periodic trends can be explained by the arrangement of electrons in an atom. The effective nuclear charge (Z_eff) experienced by valence electrons determines various chemical behaviors, including ionization energies and atomic radii across a period. When analyzing a course of elements from lithium to sodium in the periodic table, which of the following statements regarding the effective nuclear charge and electron configurations for these elements is correct?

Lithium has a greater Z<sub>eff</sub> than sodium because it is in a higher period.

The increase in Z<sub>eff</sub> from lithium to sodium accounts for the decrease in ionization energy.

Sodium's larger atomic radius relative to lithium is primarily due to increased shielding and a higher n value.

Both lithium and sodium exhibit the same effective nuclear charge due to their shared group in the periodic table.

Hint

Submitted13.9K

Correct8.2K

% Correct59%