Question

1. the ionic radius of p³⁻ is larger than the atomic radius of p because (10 pts) ____________________ which increases its ionic radius.
2. sulfur has a higher electronegativity than magnesium because (10 pts) ____________________ which increases its ability to attract electrons and increases its electronegativity.
3. lithium has a higher electronegativity than rubidium because (10 pts) ____________________

Explanation:

Question 6

To determine why the ionic radius of \( P^{3-} \) is larger than the atomic radius of \( P \), we analyze the electron configuration. A phosphorus atom (\( P \)) has 15 electrons. When it forms the \( P^{3-} \) ion, it gains 3 electrons, resulting in a total of 18 electrons. These additional electrons increase electron - electron repulsion within the electron cloud. Also, the effective nuclear charge experienced by the outermost electrons decreases because the same nuclear charge (from 15 protons) is now spread over more electrons. This causes the electron cloud to expand, thus increasing the ionic radius.

Electronegativity depends on factors like atomic radius and effective nuclear charge. Sulfur (\( S \)) and magnesium (\( Mg \)) are in the same period (period 3). As we move from left to right across a period, the atomic radius decreases and the effective nuclear charge increases. Sulfur is to the right of magnesium in period 3. So, sulfur has a smaller atomic radius and a higher effective nuclear charge than magnesium. A smaller atomic radius and higher effective nuclear charge mean that the nucleus of a sulfur atom can attract electrons more strongly, leading to a higher electronegativity.

Lithium (\( Li \)) and rubidium (\( Rb \)) are in the same group (group 1). As we move down a group, the number of electron shells increases, which leads to an increase in atomic radius. Lithium is above rubidium in group 1, so lithium has a smaller atomic radius. A smaller atomic radius means that the valence electrons of lithium are closer to the nucleus. When the valence electrons are closer to the nucleus, the nucleus can attract electrons (including bonding electrons) more strongly, resulting in a higher electronegativity for lithium compared to rubidium.

Answer:

\( P^{3 - } \) has gained 3 electrons, increasing electron - electron repulsion and decreasing effective nuclear charge on outer electrons, so the electron cloud expands.

Question 7