question 4. a chemist is designing a new compound and wants to predict how different nonmetals will behave in chemical reactions. she knows that some elements are more reactive than others. to plan her experiment, she compares several nonmetals to oxygen (o) to identify which ones are less reactive than nitrogen. which of the following elements are less reactive than oxygen (o)? select all that apply.

carbon (c)
chlorine (cl)
nitrogen (n)
fluorine (f)
sulfur (s)

Question

question 4. a chemist is designing a new compound and wants to predict how different nonmetals will behave in chemical reactions. she knows that some elements are more reactive than others. to plan her experiment, she compares several nonmetals to oxygen (o) to identify which ones are less reactive than nitrogen. which of the following elements are less reactive than oxygen (o)? select all that apply.

carbon (c)
chlorine (cl)
nitrogen (n)
fluorine (f)
sulfur (s)

Accepted Answer

# Brief Explanations: To determine which nonmetals are less reactive than oxygen (O), we use the reactivity trends of nonmetals. Nonmetals generally become more reactive as we move up and to the right in the periodic table (excluding noble gases). - **Carbon (C)**: Carbon is less reactive than oxygen. Carbon is in group 14, period 2, while oxygen is in group 16, period 2. Oxygen has a higher electronegativity and is more reactive. - **Chlorine (Cl)**: Chlorine is in group 17, period 3. Oxygen is in group 16, period 2. Chlorine is more reactive than oxygen (higher electronegativity and reactivity in halogens, but oxygen's position and properties make it more reactive than Cl in many contexts? Wait, no—wait, actually, fluorine is the most reactive nonmetal, then oxygen, then chlorine? Wait, no, let's correct. The reactivity of nonmetals (for non-halogen nonmetals and halogens) – the halogens: F > Cl > Br > I. For non-halogen nonmetals, oxygen is very reactive. Let's recall the reactivity series for nonmetals in terms of oxidizing power (ability to gain electrons). Oxygen is a strong oxidizing agent. - **Nitrogen (N)**: Nitrogen is in group 15, period 2. Oxygen is in group 16, period 2. Nitrogen is less reactive than oxygen because oxygen has a higher electronegativity and is more eager to gain electrons. - **Fluorine (F)**: Fluorine is the most reactive nonmetal (highest electronegativity), so it is more reactive than oxygen. - **Sulfur (S)**: Sulfur is in group 16, period 3. Oxygen is in group 16, period 2. As we move down a group, reactivity decreases for nonmetals (since atomic size increases, electronegativity decreases). So sulfur is less reactive than oxygen. So the elements less reactive than oxygen are Carbon (C), Nitrogen (N), and Sulfur (S). Chlorine: Wait, is chlorine less reactive than oxygen? Let's check electronegativity values. Electronegativity: F (4.0), O (3.5), Cl (3.0). So oxygen (3.5) has higher electronegativity than chlorine (3.0), so chlorine is less reactive than oxygen? Wait, I made a mistake earlier. So Cl (3.0) < O (3.5) in electronegativity, so Cl is less reactive than O. Wait, but fluorine is more reactive than O (4.0 > 3.5). So let's re-express: Electronegativity values (Pauling scale): - F: 4.0 - O: 3.5 - Cl: 3.0 - N: 3.0 - C: 2.5 - S: 2.5 So reactivity (as oxidizing agents, gaining electrons) is related to electronegativity. Higher electronegativity means more reactive (since they attract electrons more). So: - F (4.0) > O (3.5) > Cl (3.0) = N (3.0) > C (2.5) = S (2.5) Wait, N and Cl have the same electronegativity (3.0), but their reactivity can also depend on molecular structure. But in terms of elemental reactivity, oxygen is more reactive than Cl and N? Wait, no—for example, chlorine gas is very reactive, but oxygen is also very reactive. However, based on electronegativity, O (3.5) is more electronegative than Cl (3.0), so O is more reactive (better oxidizing agent) than Cl. So Cl is less reactive than O. Wait, but let's think about reactions. Oxygen can react with many substances more readily than chlorine? Or is chlorine more reactive? For example, chlorine reacts with metals vigorously, but oxygen also does. However, the electronegativity scale is a good indicator. Since O has higher electronegativity than Cl, O is more reactive (more likely to gain electrons). So Cl is less reactive than O. So correcting the earlier analysis: - Carbon (C): less reactive (2.5 < 3.5) - Chlorine (Cl): less reactive (3.0 < 3.5) - Nitrogen (N): less reactive (3.0 < 3.5) - Fluorine (F): more reactive (4.0 > 3.5) - Sulfur (S): less reactive (2.5 < 3.5) Wait, but this contradicts some common knowledge. Wait, maybe the confusion is between halogen reactivity and non-halogen. Let's check the reactivity of nonmetals in terms of their ability to form compounds. Oxygen is essential for combustion, and chlorine is also reactive, but which is more reactive? Let's look at the reaction of oxygen and chlorine with hydrogen. Oxygen reacts with hydrogen to form water (H₂O) with a large exotherm. Chlorine reacts with hydrogen to form HCl, also exothermic, but the reaction of F₂ with H₂ is explosive, O₂ with H₂ is very exothermic (combustion), Cl₂ with H₂ is also exothermic but less so than O₂? Wait, no, the bond energy of H₂O: H-O bonds are strong, but the reaction of O₂ and H₂ is highly exothermic. The reaction of Cl₂ and H₂ is also exothermic, but maybe O₂ is more reactive. Alternatively, maybe the question is using the periodic table trend: for nonmetals, reactivity increases as we move up and to the right. So the position: - O: group 16, period 2 - C: group 14, period 2 (left of O, so less reactive) - Cl: group 17, period 3 (below and to the right of O? O is period 2, Cl is period 3. So moving down a period (higher period number) decreases reactivity, moving right increases. So Cl is to the right of O (group 17 vs 16) but down a period (period 3 vs 2). The effect of period (atomic size) is more significant? So O is more reactive than Cl. - N: group 15, period 2 (left of O, less reactive) - F: group 17, period 2 (right of O, more reactive) - S: group 16, period 3 (below O, less reactive) So according to this trend, the elements less reactive than O are C (left, same period), N (left, same period), S (below, same group), and Cl (right but below, so less reactive than O). Wait, but earlier electronegativity: O (3.5), Cl (3.0), so O is more electronegative, hence more reactive. So Cl is less reactive than O. So the correct elements less reactive than O are Carbon (C), Nitrogen (N), Sulfur (S), and Chlorine (Cl)? Wait, but that contradicts the initial thought. Wait, let's check a reference. The reactivity of nonmetals: the most reactive nonmetal is fluorine, then oxygen, then chlorine, then nitrogen, then carbon, then sulfur? Wait, no, sulfur is below oxygen, so less reactive. Let's list the nonmetals in order of decreasing reactivity (most reactive first): Fluorine (F) > Oxygen (O) > Chlorine (Cl) > Nitrogen (N) > Carbon (C) > Sulfur (S) Yes, that makes sense. Because: - F is the most reactive (highest electronegativity) - O is next (very reactive, essential for life, strong oxidizer) - Cl is next (halogen, reactive, but less than O) - N is next (relatively unreactive due to triple bond, but still reactive in some contexts) - C is next (forms many compounds, but less reactive than N, O, Cl, F) - S is next (below O, so less reactive) Wait, but this order: F > O > Cl > N > C > S. So in this case, the elements less reactive than O are Cl, N, C, S. But that can't be, because Cl is a halogen and is very reactive. Wait, maybe the question is considering only non-halogen nonmetals? But the options include Cl, which is a halogen. Alternatively, maybe the question is using the reactivity of nonmetals in terms of their chemical activity in reactions. Let's think about the reaction of these elements with oxygen. Wait, no, the question is about their reactivity compared to oxygen, i.e., which are less reactive than O (so O is more reactive than them). Let's check each: - **Carbon (C)**: O is more reactive than C. Correct. - **Chlorine (Cl)**: Is O more reactive than Cl? Let's see, O₂ can oxidize Cl⁻ to Cl₂? No, Cl₂ can oxidize O²⁻? Wait, the standard reduction potentials: O₂ + 4H⁺ + 4e⁻ → 2H₂O: E° = 1.23 V Cl₂ + 2e⁻ → 2Cl⁻: E° = 1.36 V Ah! Here's the key. The standard reduction potential of Cl₂ (1.36 V) is higher than that of O₂ (1.23 V). So Cl₂ is a stronger oxidizing agent than O₂, meaning Cl is more reactive than O. Oh! So my earlier electronegativity approach was wrong. The reduction potential is a better indicator of reactivity in redox reactions. So Cl₂ has a higher reduction potential (1.36 V) than O₂ (1.23 V), so Cl₂ is more reactive (a stronger oxidizing agent) than O₂. That changes things. So let's recast: - **Carbon (C)**: O is more reactive than C. Correct, because O₂ can oxidize C to CO₂. - **Chlorine (Cl)**: Cl₂ is more reactive than O₂ (higher reduction potential), so Cl is more reactive than O. So Cl is not less reactive. - **Nitrogen (N)**: O is more reactive than N. N₂ is relatively unreactive (triple bond), and O₂ can react with N₂ (but only at high temperatures, like in lightning) to form NO. So O is more reactive than N. - **Fluorine (F)**: F₂ has a very high reduction potential (2.87 V), so F is more reactive than O. - **Sulfur (S)**: O is more reactive than S. S is below O in group 16, so less reactive. So the correct elements less reactive than O are Carbon (C), Nitrogen (N), and Sulfur (S). Chlorine is more reactive than O (due to higher reduction potential), so it's excluded. Let's confirm the reduction potentials: - F₂ + 2e⁻ → 2F⁻: E° = 2.87 V (most reactive) - Cl₂ + 2e⁻ → 2Cl⁻: E° = 1.36 V - O₂ + 4H⁺ + 4e⁻ → 2H₂O: E° = 1.23 V - Br₂ + 2e⁻ → 2Br⁻: E° = 1.07 V - I₂ + 2e⁻ → 2I⁻: E° = 0.54 V - N₂ + 6H⁺ + 6e⁻ → 2NH₃: E° = -0.037 V (very low, so N₂ is not a strong oxidizing agent) - C: The oxidation of C to CO₂ has a high positive E° (since O₂ is a strong oxidizer) So from the reduction potentials, Cl₂ (1.36 V) is a stronger oxidizing agent than O₂ (1.23 V), so Cl is more reactive than O. Therefore, Cl is not less reactive than O. So the elements less reactive than O are: - Carbon (C): O is more reactive (O₂ oxidizes C) - Nitrogen (N): O is more reactive (O₂ can react with N₂ at high temps) - Sulfur (S): O is more reactive (S is below O in group 16, less reactive) Chlorine (Cl) is more reactive than O (higher reduction potential), so it's excluded. Fluorine (F) is more reactive than O (highest reduction potential), so excluded. So the correct options are Carbon (C), Nitrogen (N), and Sulfur (S). # Answer: A. Carbon (C) C. Nitrogen (N) E. Sulfur (S)

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