Question

Consider the following electron configurations to answer the question: (1) 152 252 2p 3s (ii) 182 282 2p 3s2 (ii) 1s2 282 2p 3s 3p1 (iv) 152 2s 2p 352 3p4 (v) 152 2s 2p 3s 3p5 The electron configuration of the atom with the most negative electron affinity is 1) (11) (iv) 0

Answer 1

The atom with the most negative electron affinity based on the given electron configurations is Chlorine, which corresponds to configuration (v) with 1s² 2s² 2p¶ 3s² 3p⁵.

Step-by-step explanation:

The question asks for the atom that has the most negative electron affinity based on given electron configurations. Electron affinity generally increases (becomes more negative) as you move across a period from left to right on the periodic table, and decreases (becomes less negative) as you move down a group.

Here's the breakdown of the mentioned configurations (ignoring the typos in the original question):

• (i) is incomplete and likely represents an alkali metal.
• (ii) represents an alkaline earth metal.
• (iii) likely represents the 13th group element in the third period (element Aluminum).
• (iv) seems to represent a chalcogen in the third period (element Sulfur).
• (v) represents a halogen in the third period (element Chlorine).

Since halogens have the most negative electron affinities in a given period, the configuration with the most negative electron affinity here is (v) 1s² 2s² 2p¶ 3s² 3p⁵, which is the electron configuration of Chlorine.