Oxoacid strength number

Oxidation A half-reaction in which there is an increase in oxidation number, 88 chromium, 548 electrolysis and, 498 fluorine, 557 halogens, 557-558 oxoacids, 568-570 oxoanions, 568-570 species strength, 506-507q transition metals, 546t zinc, 86-87... 

The acid strengths and oxidizing abilities of the halogen oxoacids increase with the oxidation number of the halogen. The hypohalous acids, HXO (halogen oxidation number +1), are prepared by direct reaction of the halogen with water. For example, chlorine gas disproportionates in water to produce hypochlorous acid and hydrochloric acid ... 

The interhalogens have properties intermediate between those of the constituent halogens. Nonmetals form covalent halides metals tend to form ionic halides. The oxoacids of chlorine are all oxidizing agents both acidity and oxidizing strength of oxoacids increase as the oxidation number of the halogen increases. 

The relative strength of oxoacids increases with the number of oxygen atoms. 

The acid strengths and oxidizing abilities of the halogen oxoacids (Table 15.8) increase with the oxidation number of the halogen. The... 

Because dissociation of an oxoacid requires breaking an O — H bond, any factor that weakens the O — H bond or increases its polarity increases the strength of the acid. Two such factors are the electronegativity of Y and the oxidation number of Y in the general reaction... 

For oxoacids that contain the same number of OH groups and the same number of O atoms, acid strength increases as the electronegativity of Y increases. For example, the acid strength of the hypohalous acids HOY (Y = Cl, Br, or I) increases as the electronegativity of the halogen increases ... 

For oxoacids that contain the same atom Y but different numbers of oxygen atoms, acid strength increases as the oxidation number of Y increases. The oxidation number of Y increases, in turn, as the number of oxygen atoms increases. This effect is illustrated by the oxoacids of chlorine ... 

F shows oxidation state of-1 others show oxidation state 1, +1, +3, +5, +7 Strength of oxoacids increase in oxidation number of X. 

The correct answer is (C). The general trend for oxoacids is that the greater the number of oxygen atoms, the greater the strength of the acid. 

The strength of oxoacids with a given central element X increases with the number of lone oxygen atoms attached to the central atom. If the formula of these acids is written as XO (OH) the corresponding acid strengths fall into distinct classes according to the value of n, the number of lone oxygen atoms (see... 

Various trends have long been noted in the acid strengths of many binary hydrides and oxoacids. Values for some simple hydrides are given in Table 3.4 from which it is clear that acid strength increases with atomic number both in any one horizontal period and in any... 

How does the strength of an oxoacid depend on the electronegativity and oxidation number of the central atom ... 

All oxoacids have the acidic H atom bonded to an 0 atom, so bond strength (length) is not a factor in their acidity, as it is with the nonmetal hydrides. Rather, two factors determine the acid strength of oxoacids the electronegativity of the central nonmetal (E) and the number of 0 atoms. 

For oxoacids with different numbers of oxygens around a given E, acid strength increases with number of O atoms. The electronegative O atoms pull electron density away from E, which makes the O—H bond more polar. The more O atoms present, the greater the shift in electron density, and the more easily the H ion comes off (Figure 18.12B). Therefore, we predict, for instance, that... 

Strength of halogen-containing oxoacids having the same number of 0 atoms increases from bottom to top. 

To compare their strengths, it helps to divide the oxoacids into two groups, those having different central atoms that are from the same group of the periodic table (and that have the same number of oxygen atoms around the central atom) and those having the same central atom but different numbers of attached groups. 

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