DATA SHEE6.2 Post-Lab Questions Although Mendeleev and Meyer developed their dis

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DATA SHEE6.2 Post-Lab Questions Although Mendeleev and Meyer developed their discovered, their work was nonetheless directed "behind the scenes" by the questions below, rationalize the periodic trends in atomic radius, ionization energy n terms of the electron configuration of the elements periodic tabies betore the clectron, proton and neutron were the electronic structure of atoms, in the and electron affinity you observed Consider the atomic radus of the atoms in Period 2. Notice that the radius decreases from left to right aos the period, even though the number of valence electrons increases. Why doesn't atomic radius increase a period? (Hint: Consider effective nuclear charge) 2 The fist ionization energies for the p-block elements in Period 2 are shown in Table 6.12. in general, the ionization energy increases with atomic number across a period, but notice that the ionization energy of oxygen is lower than that for nitrogen. How do you explain this observation? 6.12ationEnegs of Vanious Element Boron Carbon Nitrogen Oxygen Fluorine Neon 8.30 11.26 4.53 3.62 17.42 21.56

Explanation / Answer

Q1

This is mainly due to the amount of electrons being added

recall that

nucleus = protons + neutrons

cloud = electrons

therefore, as we increase aotmic number, we increase electrons

According to couloumb:

F = k*Q1*Q2 / d^2

where Q is the charge( protons) and Q2 the electorn charge, as we increase Q1 and Q2, then the "d" value must increases

since it is to the sqaure, expect a small amount of decrease in "d"

this is seen as we increase electrons from left to right of th eperioc table ( 1 electron in valence vs. 7 electrons)

Q2

Oxygen v.s Nitrogen

ionization energy --> energy required to form an ion

Nitrogen has 7 electrons --> 1s2 2s2 2p3

Oxygen, has 8 eelectrons--> electorn config. 1s2 2s2 2p4

note that according to Hund rule, we must find the most stable configuration

For N, it has much better electron configuraiton, since the px,py,pz orbitals are all half filled, whereas the oxygen:

has 1 filled px, half filled py,pz

therefore, the electron ionization is readily faster for Oxygen (easier to stirp 1 e- from px filled up orbital) to leave all 50% px,py,pz filled

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