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- b. (i) Define Electron Affinity and explain why the electron affinity may either havepositive or negative values. [The transition and inner transition metals, it is necessary to removethe s electrons before the d or f electrons. Then, for each ion, give the electron configuration:(a) cerium(III)(b) lead(II)(c) Ti2+(d) Am3+(e) Pd2+For the examples that are transition metals, determine to which series they belong.On the basis of periodic trends, determine which element in each pair has the higher first ionization energy (if possible).(a) Al or S (b) As or Sb (c) N or Si (d) O or Cl
- (ii) How would you expect the second ionization energies for Na and Mg to compare? Explain using both a qualitative and quantitative (Slater’s rules) argument. (iii) Does your answer for (ii) correspond to what you know about the common ions formed by Na and Mg? Explain.An element has the following successive ionization energies in kJmol-1. The first valuecorresponds to the first ionization energy. 762, 1540, 3300, 4390, 18950, 24900 i. Predict the group of the element. ii. Briefly explain you answer in (i).Write the full electron configuration of the ion oxide, O2- You can indicate superscript through the ^ symbol (e.g. 3s2 could be written as 3s^2) or use the superscript text formatting tool above.
- Which of the following would be the expected electron configuration for a vanadium (II) cation?(a) Write the electron configuration for the element titanium,Ti. How many valence electrons does this atom possess?(b) Hafnium, Hf, is also found in group 4B. Writethe electron configuration for Hf. (c) Ti and Hf behaveas though they possess the same number of valence electrons.Which of the subshells in the electron configurationof Hf behave as valence orbitals? Which behave ascore orbitals?Question 4 The two Group VB elements niobium and tantalum have the same atomic radii. This is because of... O A. Lanthanide contraction; the filling of 4f orbitals through the lanthanide elements causing a steady increase in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. B. Scandide contraction; the filling of 4f orbitals through the Scandide elements causing a steady increase in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. O C. Lanthanide contraction; the filling of 4f orbitals through the lanthanide elements causing a steady decrease in the effective nuclear charge. This contraction offsets the expected increase of second and third series of transition metals. D. Scandide contraction; the filling of 4f orbitals through the Scandide elements causing a steady decrease in the effective nuclear charge. This contraction offsets the…