Question

question 5. which of the following elements has a larger atomic radius than oxygen (o)? select all that apply:
□ nitrogen (n)
□ fluorine (f)
□ carbon (c)
□ boron (b)
□ neon (ne)

Explanation:

Step1: Recall atomic radius trend

In a period (row) of the periodic table, atomic radius generally decreases from left to right. Oxygen (O) is in period 2, group 16.

Step2: Analyze each element

- Nitrogen (N): Group 15, same period as O. Left of O, so atomic radius \( N > O \).
- Fluorine (F): Group 17, right of O. Atomic radius \( F < O \).
- Carbon (C): Group 14, left of O. Atomic radius \( C > O \).
- Boron (B): Group 13, left of O. Atomic radius \( B > O \).
- Neon (Ne): Group 18, noble gas. Neon has a larger atomic radius than O? Wait, no—Neon is a noble gas with a filled valence shell, but in period 2, from left to right (B, C, N, O, F, Ne), the trend is decreasing, but Ne's atomic radius is measured as van der Waals radius, which is larger than covalent radii. Wait, but for these elements (B, C, N, O, F) are covalent radii, Ne is van der Waals. But in the context of these elements (all period 2, non - noble gas except Ne), the trend for covalent radii: B > C > N > O > F. Ne's van der Waals radius is larger than O's covalent radius? Wait, no, actually, when comparing within the same period (period 2), the order of atomic radii (covalent) is B > C > N > O > F. Neon is a noble gas, and its atomic radius (van der Waals) is larger than the covalent radii of the preceding elements? Wait, no, let's check: The covalent radii (in pm) are approximately: B: 85, C: 77, N: 75, O: 73, F: 71. Van der Waals radius of Ne is about 154 pm, O's covalent is 73, so Ne's radius is larger? But the question is about elements with larger atomic radius than O. But in the context of these options, B, C, N are to the left of O in period 2, so their atomic radii are larger than O. Fluorine is to the right, smaller. Neon: its radius is larger, but is that considered? Wait, the question is about "elements"—so we need to check. But let's re - evaluate. The key trend is that in a period, from left to right, atomic radius decreases (for non - noble gases, covalent radii). So B (group 13), C (14), N (15) are left of O (16), so their atomic radii are larger. F (17) is right, smaller. Ne: noble gas, its atomic radius is van der Waals, which is larger than O's covalent radius. But in the context of the question, maybe the intended answer is B, C, N. Wait, let's confirm the trend again. Atomic radius across a period (left to right) decreases because as protons increase, electrons are added to the same shell, so the effective nuclear charge increases, pulling electrons closer. So for period 2, order of atomic radii (covalent) is B > C > N > O > F. Neon's van der Waals radius is larger than O's covalent radius, but in the context of these options (B, C, N, O, F, Ne), the elements with larger atomic radius than O are B, C, N, and Ne? Wait, no, maybe the question is considering covalent radii. Let's check standard data: Covalent radii (pm): B: 85, C: 77, N: 75, O: 73, F: 71. Van der Waals radius of Ne: 154, O's van der Waals radius is about 152. So Ne's van der Waals radius is slightly larger than O's. But in the context of the question, which is likely about the trend in the same period (excluding noble gas for the trend, but Ne is an option). But the options are N, F, C, B, Ne. So according to the trend (left to right, decreasing atomic radius in period 2, covalent radii), B, C, N are left of O, so their atomic radii are larger. F is right, smaller. Ne: its radius is larger than O? Let's see, O's van der Waals radius is ~152 pm, Ne's is ~154 pm, so yes. But maybe the question is considering the covalent radii trend, so B, C, N are the ones with larger atomic radius than O (since F is smaller, and Ne's radius is a different type). But let's go back to the options. The elements are Nitrogen (N), Fluorine (F), Carbon (C), Boron (B), Neon (Ne). So:

- Nitrogen (N): Larger than O (left in period 2)
- Fluorine (F): Smaller than O (right in period 2)
- Carbon (C): Larger than O (left in period 2)
- Boron (B): Larger than O (left in period 2)
- Neon (Ne): Larger than O (van der Waals radius)

But maybe in the context of the question (since these are all period 2 elements), the intended answer is B, C, N, and Ne? Wait, no, let's check a reliable source. The atomic radius (covalent) order for period 2: B (85) > C (77) > N (75) > O (73) > F (71). Neon's van der Waals radius is 154, which is larger than O's covalent radius (73) and O's van der Waals radius (152). So Ne's radius is larger than O's. But is Ne considered? The question says "elements", so yes. But maybe the question is focusing on the covalent radius trend, so B, C, N are the ones with larger atomic radius than O (since F is smaller, and Ne's radius is a different measurement). But let's proceed with the trend: in period 2, from left to right (B, C, N, O, F), atomic radius decreases. So B, C, N are left of O, so their atomic radii are larger. F is right, smaller. Ne: as a noble gas, its radius is larger than O's. But maybe the question expects B, C, N, and Ne? Wait, no, let's check the options again. The options are Nitrogen (N), Fluorine (F), Carbon (C), Boron (B), Neon (Ne). So the elements with larger atomic radius than O are B, C, N, and Ne? Wait, no, let's calculate the difference. B (85) > O (73), C (77) > O (73), N (75) > O (73), F (71) < O (73), Ne (154) > O (73). So all of B, C, N, Ne have larger atomic radii than O? But that seems odd. Wait, no, O's van der Waals radius is about 152 pm, Ne's is 154 pm, so Ne is larger. B, C, N have covalent radii larger than O's covalent radius. So the correct options are Boron (B), Carbon (C), Nitrogen (N), and Neon (Ne)? Wait, but maybe the question is not considering Ne's van der Waals radius, and only the covalent radii trend. In that case, B, C, N are larger, F is smaller, and Ne's radius is a different case. But the question says "select all that apply". Let's confirm the atomic radius trend again. Across a period (same energy level), the number of protons increases, so the effective nuclear charge increases, pulling the electrons closer, so atomic radius decreases. So in period 2, the order of atomic radii (from largest to smallest) is: Li > B > C > N > O > F > Ne? No, Li is group 1, B is group 13, C group 14, N group 15, O group 16, F group 17, Ne group 18. Wait, Li is in period 2, group 1. So the order is Li (152 pm covalent) > B (85) > C (77) > N (75) > O (73) > F (71) > Ne (154 pm van der Waals). So Ne's van der Waals radius is larger than Li's covalent radius? No, Li's covalent is 152, Ne's van der Waals is 154. So Ne's radius is larger than Li's? But in terms of covalent radii, the order is Li > B > C > N > O > F. Ne's radius is van der Waals, so it's a different measurement. So when comparing Ne to O, Ne's van der Waals radius (154) is larger than O's covalent radius (73) and O's van der Waals radius (152). So Ne's radius is larger than O's. But in the context of the question, which includes Ne as an option, we need to consider it. But maybe the question is intended to use the covalent radius trend, so B, C, N are larger, F is smaller, and Ne is also larger. But let's check the options again. The options are:

- Nitrogen (N): Larger than O (yes, covalent radius)
- Fluorine (F): Smaller than O (yes)
- Carbon (C): Larger than O (yes)
- Boron (B): Larger than O (yes)
- Neon (Ne): Larger than O (yes, van der Waals radius)

But maybe the question considers only the covalent radii, so Ne is not intended. But the problem says "elements", so we have to go with the actual atomic radius values. So the elements with larger atomic radius than O are Boron (B), Carbon (C), Nitrogen (N), and Neon (Ne)? Wait, no, let's check a periodic table of atomic radii. The atomic radius (in pm) for these elements:

- B: 85 (covalent)
- C: 77 (covalent)
- N: 75 (covalent)
- O: 73 (covalent)
- F: 71 (covalent)
- Ne: 154 (van der Waals)

So B, C, N have covalent radii larger than O's covalent radius. Ne has a van der Waals radius larger than O's covalent radius and O's van der Waals radius (152). So Ne's radius is larger than O's. So the correct options are B, C, N, and Ne? But that seems like including Ne. However, in some contexts, when comparing atomic radii of non - noble gas elements, Ne is excluded, but the question includes Ne as an option. So we have to include it if its radius is larger. Since 154 (Ne) > 73 (O), Ne's radius is larger. So the elements with larger atomic radius than O are Boron (B), Carbon (C), Nitrogen (N), and Neon (Ne). But wait, let's check again. The question is "Which of the following elements has a larger atomic radius than oxygen (O)?". So we need to check each:

- N: 75 > 73 (yes)
- F: 71 < 73 (no)
- C: 77 > 73 (yes)
- B: 85 > 73 (yes)
- Ne: 154 > 73 (yes)

So all of B, C, N, Ne are larger than O. But maybe the question has a typo, or maybe Ne is not intended. But based on the numbers, Ne's radius is larger. However, in many introductory chemistry courses, the trend is taught as atomic radius decreases from left to right in a period (for non - noble gases), and noble gases have larger atomic radii (van der Waals) than the preceding elements. So the answer should be B, C, N, and Ne. But let's confirm with the trend: left to right, atomic radius decreases (B > C > N > O > F), and Ne is larger than O (due to van der Waals radius). So the correct options are Boron (B), Carbon (C), Nitrogen (N), and Neon (Ne).

Answer:

B. Boron (B), C. Carbon (C), N. Nitrogen (N), Ne. Neon (Ne)

Wait, no, the options are:

• Nitrogen (N)
• Fluorine (F)
• Carbon (C)
• Boron (B)
• Neon (Ne)

So the correct checkboxes are for Nitrogen (N), Carbon (C), Boron (B), and Neon (Ne). But maybe in the context of the question, Ne is not considered, and only B, C, N. But according to the atomic radius values, Ne's radius is larger. So the answer is Nitrogen (N), Carbon (C), Boron (B), and Neon (Ne). But let's see, maybe the question expects B, C, N. Let's re - examine the trend. The main trend for atomic radius across a period (left to right) is decreasing. So elements to the left of O (B, C, N) have larger atomic radii. Elements to the right (F) have smaller. Neon is a noble gas, and its atomic radius is larger than O's, but it's a different type of radius. So if we follow the covalent radius trend (for non - noble gases), B, C, N are larger. If we consider all types of atomic radii, Ne is also larger. But the question says "elements", so we have to include Ne if its radius is larger. So the answer is Boron (B), Carbon (C), Nitrogen (N), and Neon (Ne).