Question
Id like to have the answers with the steps or full explaination of it to get the 1500 points
that im offering ! The questions
are in the images attached ..
Peaks in ionization energy occur at atomic numbers equal to 10, 18, 36, and 54, but these elements have very small or zero electron affinities. Peaks in the electron affinity occur at atomic numbers equal to 9, 17, 35, and 53. Why does a change of one unit for the atomic number result in such a drastic change in electron affinity? (Note: A high quality answer will provide and explanation that relates the electron configurations to the electron-electron repulsion and the electron-nucleus attraction.) Why are the periodic trends in electron affinity and ionization energy more similar to each other than they are to the trend in atomic radii? How can you use the periodic table and orbital diagrams to predict relative atomic radii, ionization potentials, and electron affinities of atoms? Explain why the first ionization energy of sulfur is less than the first ionization energy of phosphorus. Explain why the first ionization energy of aluminum is less than the first ionization energy of magnesium. Explain why is the electron affinity of Be very small or zero and the electron affinity of F very large (328 kJ/mole). In going from hydrogen to helium, what do the changes in atomic radius (37 to 32 pm) and ionization energy (1311 kJ/mole to 2377 kJ/mole) suggest about the relative magnitudes of the changes in the electron - nucleus attraction and the electron - electron repulsion? Given that the atomic radius and ionization energy of lithium are 152 pm and 520 kJ/mole, respectively, how does the orbital box diagram for lithium in the preliminary activity help to explain the observed differences in atomic radius and ionization energy between helium and lithium? In moving across the second period of the Periodic Table, is the general trend in atomic radius consistent with the trend in going from hydrogen to helium? Explain. For the ionization potentials in the second period where do the exceptions to the general trend occur, and how do the orbital box diagrams in the preliminary activity help to explain these exceptions? What happens to the atomic radii and ionization energies in going down a group, e.g., from Ne to Xe or Li to Rb? atomic radii down a group ionization energies down a group How do the electron configurations of the atoms explain the trends you identified in question 14?
Explanation / Answer
16) due to octet configuration in valence shell or stable electronic config. of those elments have o or smallelectron affinities
17) elctron affinity and IP vales are energies released or required this energy is inversely varies w.r.t size of the atoms
18)when we move from top to bottom atomic radii increaseas,IP and EA values decreases
when we move from left to right atomic size decreases ,IP and EA values increases
19)because P = [Ne]3s23P3 half filled electronic config. more stable thvalue than San Sulfur so it can have more 1st IP value than Sulfur
20) Mg = [Ne]3s2 full filled electronic config. morestable that is why it is having more 1st IP than Al
21) Be = 1s22s2
in the 2s orbital max. electrons are 2 so those electrons filled so it is having small IP values
F = 1s22s22p5
1 e^- less than to octet config. so it can take 1 electron immediately and releases more energy
10)electron -nucleous attraction increaseand e- ..e- repulsions increases
12) yes because every time new electron is added to same shell so size decreases
13)Be is havin more IP than B,N is more IP than O
14)atomic radii increases down agroup
IP values decreases down gp.
