CHEM 113 1nd Edition Lecture 22 Outline of Last Lecture- Weak bases and their relation to weak acid- The relation between Ka and Kb of a conjugate acid-base pairOutline of Current Lecture - Acid strength of nonmetal hydrides- Acid strength of oxoacids- Hydrated metal ions- Salts that yield neutral solutions- Salts that yield acidic solutions- Salts that yield basic solutionsCurrent Lecture- Molecular properties and acid strength- Strong acids can be broken down into two groups, the nonmetal hydrides and the oxoacids.o Acid strength of nonmetal hydrides For nonmetal hydrides (nonmetal bonded to H), acid strength depends on two things.- 1). The electronegativity of the central nonmetal, which increases across a period.- 2). The strength of the bond between the H and the nonmetal. The strength of an acid increases across a period, because electronegativity increases across a period. Therefore the acidity of a nonmetal hydride increases. The strength of an acid increases down a group, this is because the lengthof the bond increases down a groups and therefore its strength decreases.o Acid strength of oxoacids An oxoacid is an acid where the acidic H is bonded to an O atomThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute. The strength of these acids depend on the following.- 1). The electronegativity of the central nonmetal - 2). The number of O atoms around the central nonmetal For oxoacids with the same number of O atoms, acid strength increases as the electronegativity of the central nonmetal atom increases. For oxoacids with different numbers of O atoms, acid strength increases with the number of O atoms. - ~These ideas are used when comparing acids.- When an acid is more electronegative and/or has more oxygen molecules, it can also be said to be more stable.  Examples of oxoacids include H2SO4, HNO3 and HClO4o Hydrated metal ions The aqueous solutions of certain metal ions are acidic because the hydrated metal ion transfers and H+ ion to water. If M^n+ is small and highly charged, it will withdraw enough electron density from the oxygen and hydrogen bonds of the water molecules to release H+ and produce the following equation. This process is visually shown in Figure 18.12 on page 746.- Acid-base properties of salt solutionso When a salt dissolves one or both of its ions may react with water and affect the pH of the solution.o Salts that yield neutral solutions A salt that consists of the anion of a strong acid and the cation of a strong base yields a neutral solution. This is neutral because neither the cation nor anion will react with water to any great extent.o Salts that yield acidic solutions A salt that consists of the anion of a strong acid and the cation of a weak base yields and acidic solution. This solutions will be acidic (smaller pH) because the cation will react withthe water molecules to produce H3O+o Salts that yield basic solutions A salt that consists of the anion of a weak acid and the cation of a strong base yields a basic solution. This solution will be basic because the anion will react with water molecules to produce