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: **A. P will form an electrovalent bond with R** - An electrovalent bond (ionic bond) typically occurs between a metal and a non-metal, where one atom donates electrons and the other accepts them. In this case, both P (Oxygen) and R (Phosphorus) are non-metals. Therefore, they are more likely to form covalent bonds rather than ionic bonds. This option is incorrect. **B. Q will form a covalent bond with S** - Q (Sodium) is a metal and S (Chlorine) is a non-metal. Metals typically lose electrons to form cations, while non-metals gain electrons to form anions. Therefore, Q will not form a covalent bond with S; instead, it will form an ionic bond. This option is incorrect. **C. R will form an electrovalent bond with S** - R (Phosphorus) is a non-metal and S (Chlorine) is also a non-metal. However, in this case, R can lose electrons to form a cation, and S can gain electrons to form an anion. Phosphorus can form a stable ionic compound with Chlorine by transferring electrons. This option is correct. **D. Q will form an electrovalent bond with S** - As mentioned earlier, Q (Sodium) will indeed form an ionic bond with S (Chlorine) because Sodium will lose its one outer electron to Chlorine, which will gain that electron. However, this option is not the best answer compared to option C, which correctly identifies the bond formation between R and S. This option is weaker in the context of the question. ### Conclusion The correct answer is **C. R will form an electrovalent bond with S**. ### Revision Summary - **Element Identification**: Understand the number of electrons to identify elements and their group in the periodic table. - **Bond Types**: Recognize that ionic bonds typically form between metals and non-metals, while covalent bonds form between non-metals. - **Electron Transfer**: In ionic bonding, one atom donates electrons while the other accepts them, leading to the formation of cations and anions. - **Correct Answer**: C is correct because R (Phosphorus) can form an ionic bond with S (Chlorine) through electron transfer.