(c) Give the four quantum numbers for the valence electron in aluminium and explain the significance of each.

Use the data from Appendix F to graph the variation ofatomic radius with atomic number for the rare-earth elements from lanthanum to lutetium.(a) What is the general trend in these radii? How do you     account for it?(b) Which two elements in the series present exceptions to      the trend?

(a) Why is ZnO called a amphoteric oxide? Name another amphoteric oxide(b) What are alkali’s? Give one example of alkali

Which of the following has the smallest ionic radius? (A) p3- (B) K1+ (C) Sc3+ (D) Ar 7.

The alkali metals play virtually the same general chemical role in all their reactions. (a) What is this role? (b) How is it based on atomic properties? (c) Using sodium, write two bal-anced equations that illustrate this role.

30.) Give the symbol of the element with the largest ionization energy from group 4A (14).

Which element in each of the following sets would you expect to have the lowest third ionization energy, IE3? (a) O Na O Al O Mg (b) O Ga ок O Mg (c) O Ca O Sc OK ооо

Assume that you have these materials:a) Li (s); b) Br2 (l); Ge (s) and d) Si(s).Choose the best electrical conductor among them and explain why.

Describe the oxidising action of potassium dichromate and write the ionic equations for its reaction with(i) iodine (ii) H2S.

Despite the expected decrease in atomic size, there is an un-expected drop in the first ionization energy between Groups2A(2) and 3A(13) in Periods 2 through 4. Explain this pattern interms of electron configurations and orbital energies.