To determine the correct answer among the options provided, we first need to analyze the electronic configurations of the elements P, Q, R, and S based on the number of electrons they have. ### Step 1: Identify the Elements and Their Electron Configurations - **Element P** has 6 electrons. This corresponds to the element Oxygen (O), which is in Group 16 of the periodic table. Oxygen typically needs 2 more electrons to achieve a stable octet configuration. - **Element Q** has 11 electrons. This corresponds to the element Sodium (Na), which is in Group 1 of the periodic table. Sodium has 1 electron in its outer shell and tends to lose this electron to achieve a stable configuration. - **Element R** has 15 electrons. This corresponds to the element Phosphorus (P), which is in Group 15 of the periodic table. Phosphorus typically has 5 electrons in its outer shell and can either gain 3 electrons or share electrons to achieve stability. - **Element S** has 17 electrons. This corresponds to the element Chlorine (Cl), which is in Group 17 of the periodic table. Chlorine has 7 electrons in its outer shell and needs 1 more electron to complete its octet. ### Step 2: Analyze the Bonding Possibilities Now, let's evaluate the bonding possibilities based on the electron configurations: - **Option A: P will form an electrovalent bond with R** - **Analysis**: P (Oxygen) and R (Phosphorus) both have a tendency to share electrons rather than transfer them. Oxygen typically forms covalent bonds, especially with nonmetals. Therefore, this option is incorrect. - **Option B: Q will form a covalent bond with S** - **Analysis**: Q (Sodium) is a metal and tends to lose its one valence electron to form a cation (Na⁺). S (Chlorine) is a nonmetal that tends to gain an electron to form an anion (Cl⁻). Therefore, Q and S are more likely to form an ionic bond rather than a covalent bond. This option is incorrect. - **Option C: R will form an electrovalent bond with S** - **Analysis**: R (Phosphorus) can form covalent bonds, especially with nonmetals like S (Chlorine). While it is possible for phosphorus to form ionic bonds under certain conditions, it is more common for it to share electrons with chlorine. Therefore, this option is not the best choice. - **Option D: Q will form an electrovalent bond with S** - **Analysis**: Q (Sodium) will lose its one valence electron to become Na⁺, and S (Chlorine) will gain an electron to become Cl⁻. The electrostatic attraction between these oppositely charged ions (Na⁺ and Cl⁻) leads to the formation of an ionic bond (electrovalent bond). This is the correct option. ### Summary of the Correct Answer The correct answer is **D: Q will form an electrovalent bond with S**. Sodium (Q) loses an electron to become Na⁺, and Chlorine (S) gains an electron to become Cl⁻, resulting in an ionic bond. ### Revision Summary - **Element Identification**: Understand the electron configurations of elements to determine their bonding behavior. - **Bond Types**: Metals typically form ionic bonds by losing electrons, while nonmetals tend to form covalent bonds by sharing electrons. - **Electrovalent Bonds**: Formed between cations and anions due to electrostatic attraction. - **Common Pitfalls**: Confusing covalent bonds (sharing electrons) with ionic bonds (transfer of electrons) based on the nature of the elements involved.