Question

1. the bohr models for sodium (na) and sulfur (s) are shown below. examine the differences between each atom and note their placement on the periodic table.

explain which element has a larger radius. use the following word bank if desired. protons, electrons, opposites, repel, attract, force of attraction, size, quantity of charge, separation distance.
circle one: sodium (na) or sulfur (s)

Explanation:

Sodium (Na) has a larger atomic radius than Sulfur (S). In the periodic table, as we move from left to right across a period (Na and S are in the same period - period 3), the number of protons in the nucleus increases. Sodium has 11 protons, while sulfur has 16 protons. The increased positive charge in sulfur's nucleus pulls the electrons closer (higher effective nuclear charge). Also, the force of attraction between protons (positive charge) and electrons (negative charge) is stronger in sulfur due to more protons. The separation distance (average distance of electrons from the nucleus) is less in sulfur. So, sodium, with weaker proton - electron attraction (fewer protons for the same number of electron shells as sulfur in the same period), has a larger atomic radius.

Answer:

Circle Sodium (Na). Sodium has fewer protons (11) compared to sulfur (16). In the same period (period 3), as the number of protons (positive charge) increases in sulfur, the force of attraction between protons and electrons is stronger. The separation distance of electrons from the nucleus is less in sulfur. So, sodium, with weaker proton - electron attraction, has a larger atomic radius.