Periodic table binary acids, strengths

For binary acids of elements in the same row of the periodic table, changes in the H-A bond strength are smaller, and the polarity of the H-A bond is the most important determinant of acid strength. The strengths of binary acids of the second-row elements, for example, increase as the electronegativity of A increases ... 

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... 

The same general acidity trends are observed in aqueous solution. The three heaviest hydrohalic acids—HCl, HBr, and HI— are equally strong in water because of the leveling effect. All the other binary hydrogen compounds are weaker adds, their strength decreasing toward the left in the periodic table. Methane and ammonia exhibit no acidic behavior in aqneous solution, nor do silane (SiH4) and phosphine (PH3). 

Indicate whether each of the following statements is true or lse. For each statement that is false, correct the statement to make it true, (a) In general, the acidity of binary adds increases from left to right in a given row of the periodic table, (b) In a series of adds that have the same central atom, add strength increases with the number of hydrogen atoms bonded to the... 

Acid strengths for binary acids of elements in other groups of the periodic table vary in the same way as those of the 7A elements. The order of bond strengths for the 6A hydrides is... 

In Chapter 10 we studied the strengths of binary acids as a function of the position of the anion on the periodic table. We also studied the strengths of ternary acids containing the same central element as a function of the oxidation state of the central element. Those were empirical trends. We can now use and pIQ values to make much more precise conclusions about compounds acidity or basicity. The following example illustrates a correlation between IQ values and properties. 

As you go across a row of elements of the periodic table, the atomic radius decreases slowly. For this reason, the relative strengths of the binary acids of these elements are less dependent on the size of atom X. Now the polarity of the H—X bond becomes the dominant factor in determining acid strength. Going across a row of elements of the periodic table, the electronegativity increases, the H—X bond... 

When comparing binary acids of elements in the same row of the periodic table, acid strength increases as the polarity of the bond increases. 

---