Which one of the following is an element which never exhibits positive oxidation state in any of its compounds?

Fluorine is the most electronegative element in the periodic table. Due to its extreme electronegativity, it has a much stronger tendency to attract electrons than any other element it bonds with [t2][t4]. Consequently, in all its chemical compounds, fluorine always exhibits an oxidation state of -1 and never shows a positive oxidation state [t2][t6]. In contrast, other elements listed can exhibit positive states. Oxygen typically has an oxidation state of -2 but shows a positive state of +2 in compounds like oxygen difluoride (OF2) because fluorine is more electronegative [t2][t3]. Chlorine can exhibit multiple positive oxidation states, such as +1, +3, +5, and +7, when bonded to more electronegative atoms like oxygen or fluorine [t2][t3]. Carbon also exhibits a wide range of oxidation states from -4 to +4 depending on its bonding environment [t5][t7].