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

• 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 amount of energy released when an electron is added to a neutral atom in the gaseous state to form a negative ion. Generally, elements with higher electron affinity values are more likely to gain 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 stronger attraction for additional electrons.
3. Analyze the given elements: The elements provided are N (Nitrogen), O (Oxygen), C (Carbon), B (Boron), and Ne (Neon). These elements are all in the second period of the periodic table.
4. Evaluate the electron affinity of each element: Neon (Ne) is a noble gas and typically has a very low electron affinity because it has a complete valence shell. Boron (B) and Carbon (C) have lower electron affinities compared to Nitrogen (N) and Oxygen (O) due to their position in the periodic table.
5. Identify the element with the highest electron affinity: Among the elements N, O, C, B, and Ne, Oxygen (O) has the highest electron affinity. This is because it is more electronegative and is positioned further to the right in the periodic table compared to the other elements listed.