Which statement best describes the trends of atomic properties in the periodic table?

The statement that atomic properties show consistent trends based on atomic number accurately reflects the organization and behavior of elements as you move across the periodic table. As you progress from left to right across a period, there are clear patterns in atomic radius, ionization energy, electronegativity, and electron affinity.

For instance, atomic radius generally decreases across a period due to the increased effective nuclear charge that pulls electrons closer to the nucleus, making the atom smaller. Conversely, as you move down a group, the atomic radius increases because additional electron shells are added, which outweighs the increased nuclear charge.

Additionally, ionization energy tends to increase across a period, as the attraction between the nucleus and the outermost electrons becomes stronger, making it harder to remove an electron. Electronegativity also shows a similar increasing trend across a period, as atoms that are closer to achieving a full valence shell tend to attract electrons more strongly.

This systematic variability in atomic properties based on atomic number highlights the underlying principles of periodicity, confirming that atomic properties are not random or confined to specific groups of elements but rather follow predictable trends throughout the periodic table.