To tackle the problem of identifying paramagnetic allotropic forms of sulphur, we first need to understand what paramagnetism is. Paramagnetic substances are those that have unpaired electrons. Sulphur, in its elemental form, can exist in various allotropic forms, but the most common ones include rhombic sulphur, monoclinic sulphur, and various molecular forms (Sn where n can vary). Most of these forms, such as rhombic and monoclinic sulphur, consist of S8 rings where each sulphur atom bonds covalently to two neighboring atoms, resulting in paired electrons and thus, these forms are diamagnetic. However, if we consider atomic sulphur (a form where sulfur is in its atomic rather than molecular form), it has two unpaired electrons in the 3p orbital, which makes it paramagnetic. Atomic sulphur is not stable in this form and generally exists only under high-energy conditions. Since the problem does not specify unique or obscure allotropes beyond the common molecular structures, we understand that the allotropes naturally occurring or commonly considered are not paramagnetic under standard conditions. Thus, the number of paramagnetic forms of sulphur among the common allotropes is 0, which lies within the provided range of (1,1), indicating the need to interpret the problem's language carefully. By standard definitions, without creating atypical redistribution of electrons or exotic conditions, common sulfur allotropes are generally not paramagnetic under normal circumstances. Solution: The number of common allotropic forms of sulphur showing paramagnetism is 0.
