(a) The first ionisation energies of silicon and sulphur are lower than that of phosphorus. Explain.

(b) Explain the use of cation to anion radius ratio.

(c) Arrange the following according to the increasing order of covalence:

NaF, NaCl, NaBr, NaI

(a) The first ionization energy refers to the energy required to remove one mole of electrons from one mole of atoms in the gaseous state. In the case of silicon, sulfur, and phosphorus, their positions in the periodic table play a crucial role. Silicon is a metalloid located in the p-block, while sulfur and phosphorus are nonmetals. The effective nuclear charge increases from left to right across a period, making it more difficult to remove electrons. However, going down ___ _________ ___ _____ ____ ___ _____ ___ ________ ___.
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