There is no denying the fact that Chlorine is the second halogen in the periodic table, being a nonmetal in group 17. Hence, its properties are similar to fluorine, bromine, and iodine, and are generally intermediate among those of the first two. Chlorine has the electron configuration [Ne]3s23p5, with the seven electrons serving as its valence electrons in the third and outermost shell. As all halogens, it is thus one electron short of a full octet, and is thus a strong oxidizing agent, interacting with other elements to complete its outer shell.
This element is intermediate in the electronegativity between fluorine and bromine (the electronegativity of fluorine is 3.98, the electronegativity of chlorine is: 3.16, the electronegativity of bromine is 2.96, and the electronegativity of iodine is 2.66). This element is less reactive than fluorine and more reactive than bromine, in line with periodic patterns. Even though it is a weaker oxidizing agent than fluorine, it is stronger than bromine. In comparison, the chloride ion is a weaker reduction agent than bromide, but one stronger than fluoride.