3. Give the electron configurations for the following ions. For each set of isoe

Question

3. Give the electron configurations for the following ions. For each set of isoelectronic species (atoms/ions with the same number of electrons), specify which has the largest atomic radius and give your reasoning. a. K+ b. Cr3+ d. S2 4. According to experimental data, the electron affinities of C and N are -153.9 kJ/mol and -7 kJ/mol, respectively. Does this agree with the periodic trend for electron affinity? If not, explain why these values differ from the expected trend. (Hint: Look at the orbital diagrams for both atoms. What happens to each of the atoms? What configurations are the most stable?)

Explanation / Answer

1. A. K+=1s22s22p63s23p6

B. Cr+3=1s2 2s2 2p6 3s2 3p6 3d3

C. Mn+4=1s2 2s2 2p6 3s2 3p6 3d3

D. S2-=1s2 2s2 2p6 3s2 3p6

Option B has largest radius since it has more no of electrons (21). Even though Option C has 21 electrons, it has more positive charge.

2. Yes, since carbon has electronic configuration = 1s2 2s2 2p4 and N has 1s2 2s2 2p3, more stable half filled configuration, hence it releases less energy by adding the electron.

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