Determine which atom in the following set has the largest electron affinity: N, O, C, B, Ne

• A. N
• B. O
• C. C
• D. B
• E. Ne

Answer: (B)

Verified step by step guidance

1. Understand the concept of electron affinity: Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state to form a negative ion. Generally, the more negative the electron affinity, the more an atom attracts electrons.
2. Consider the periodic trend: Electron affinity generally increases across a period from left to right in the periodic table. This is because atoms become more electronegative and have a greater tendency to gain electrons as you move across a period.
3. Analyze the given elements: The elements provided are N, O, C, B, and Ne. These elements are all in the second period of the periodic table.
4. Identify the exceptions: While the trend suggests that electron affinity increases across a period, there are exceptions. For example, noble gases like Ne have very low electron affinities because they have a complete valence shell and do not tend to gain electrons.
5. Compare the elements: Among the elements N, O, C, B, and Ne, oxygen (O) has the highest electron affinity. This is because it is more electronegative and has a greater tendency to gain an electron compared to the others in the set.