Principle quantum number and atomic radius

Question

Assignment:

Question 1. Briefly explain what is wrong with the following orbital diagrams.

Question 2. Briefly explain what is wrong with the following electron configurations.

a.   1s²2s²2p⁵3s²3p³

b.   1s²2s²2p⁶3s¹3p⁴

c.   1s²2s²2p⁶3s²3p⁷

d.   1s²2s²2p⁶3s²3p⁶3d²

Question 3. (Periodic Trends: Atomic Radius)

a. As you go down a column in the periodic table, atomic size increases.  Explain why in terms of principle quantum number and effective nuclear charge.

b.  As you go left-to-right across a row in the periodic table, atomic size decreases.  Explain why in terms of principle quantum number and effective nuclear charge.

Question 4. (Periodic Trends: Ionization Energy) 

a. As you go down a column in the periodic table, ionization energy decreases.  Explain why in terms of  principle quantum number and atomic radius.

b. As you go left-to-right across a row in the periodic table, ionization energy increases.  Explain why in terms of effective nuclear charge and atomic radius.

Question 5. (Periodic Trends: Electron Affinity)

a. As you go down a column in the periodic table, electron affinity becomes less negative.  Explain why in terms of principle quantum number and atomic radius.

b. As you go left-to-right across a row in the periodic table, electron affinity becomes more negative.  Explain why in terms of effective nuclear charge and atomic radius.