The acids of chlorine having oxygen are the oxy acids , they are four ,HClO hypochlorous acid, HClO2 chlorous acid, HClO3 chloric acid and HClO4 perchloric acid, in these acids the oxidation no of oxygen are +1 ,+3 ,+5 and +7 respectively, the hypochlorous acid only exists in water. with the rise of no of oxygen atoms the acidic strength of oxy acids increases so perchloric acid is the strongest acid among these.
An oxyacid is an acid that contains an oxygen atombonded to a hydrogen atom and at least one other element.
Also Known As: oxoacid
Examples:
Sulfuric acid (H2SO4), phosphoric acid (H3PO4), and nitric acid (HNO3) are all oxyacids.
+5. In oxyacids, oxygen has an oxidation state of -2 and hydrogen an oxidation state of +1. Therefore, the single chlorine atom must have an oxidation state of +5 for the total oxidation states to add to zero.+5. In oxyacids, oxygen has an oxidation state of -2 and hydrogen an oxidation state of +1
Any acid that contains hydrogen and an oxyanion is referred to as an oxyacid. * An oxyanion is a polyatomic ion that contains oxygen
Free Chlorine is the Chlorine which is free to do its work in the pool, as opposed to Combined Chlorine which is chlorine that has combined with contaminants and is tied up and ineffective as a sanitizer in the pool. Sometimes you will see it abbreviated as FAC, which stands for Free Available Chlorine.
Is chlorine explosive?Chlorine alone is not explosive.
chlorine
Fluorine can not form oxyacids because fluorine is more electronegative than oxygen, and oxyacids are formed only from elements that are less electronegative than oxygen.
aluminium is passive towards oxyacids due to formation of protevtive layer of oxide. this protective layer resists the contact of aluminium with water or oxygen thatswhy aluminium is passive towards oxyacids
Sulfuric acid, Sulfurous acid, Nitric acid
In oxyacids, oxygen is always taken to have an oxidation state of -2 and hydrogen to have an oxidation state of +1. Therefore, in this compound, chlorine must have an oxidation state of +1 for the charges to balance.
+5. In oxyacids, oxygen has an oxidation state of -2 and hydrogen an oxidation state of +1. Therefore, the single chlorine atom must have an oxidation state of +5 for the total oxidation states to add to zero.+5. In oxyacids, oxygen has an oxidation state of -2 and hydrogen an oxidation state of +1
Oxyacids of iodine are:- iodic acid: HIO3- iodous acid: HIO2- hypoiodous acid: HIO- ortho periodic acid: HIO4- meta periodic acid: H5IO6
HCl4(AQ)
an acid which contain hydrogen and non metallic element and no oxygen.
Chlorine is number 17 in the periodic table, so using the electron shell arrangement,2:8:7:It has 7 electrons in its valance shell so its charge becomes Cl7+ when these 7 electrons are 'donated' (= lost to, as reductant) to oxygen (only in oxyacid or salt perchlorate).Other valence values are +5, +3 and +1 in oxyacids: chlorate, chlorite and hypochlorite, respectively.
+5. In oxyacids, oxygen has an oxidation state of -2 and hydrogen an oxidation state of +1. Therefore, the single chlorine atom must have an oxidation state of +5 for the total oxidation states to add to zero.+5. In oxyacids, oxygen has an oxidation state of -2 and hydrogen an oxidation state of +1
in my opinion flourine is very electronegative and it cannot exist in positive oxidation states in its compounds .in oxyacids of halogens ,oxygen carries a negative charge while the halogen carries a positive charge.the electronegativity of flourine is 4,while that of oxygen is 3.5. so due to high value of electronegativity ,flourine shows reluctance to form positive oxidation states and donot form oxyacids........
H2 and a polyatomic ion e.g.) H2CO3 (carbonic acid) hope that helps:)