Look at the table in Figure 5-8. (There is only one correct answer for each blank) In Row 1 [a or b] is the stronger acid because [ a) O is more electronegative than S or b) S is bigger than O] . In Row 2 [a or b] is the stronger acid because [a) because O is more electronegative than C or H, b)because the conjugate base is resonance stablalized or c) because of indction from the Cl] . In Row 3 [a or b] is the stronger acid because [a)because F is more elecronegative than Cl or b) because Cl is bigger than F]. In Row 4 [a or b] is the stronger acid because [a) because the two chlorines are further apart delocalizing the indicative effect in the conjugate base or because the two chlorines are closer to the negative charge in the conjugate base] .
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Look at the table in Figure 5-8. (There is only one correct answer for each blank)
- In Row 1 [a or b] is the stronger acid because [ a) O is more electronegative than S or b) S is bigger than O] .
- In Row 2 [a or b] is the stronger acid because [a) because O is more electronegative than C or H, b)because the conjugate base is resonance stablalized or c) because of indction from the Cl] .
- In Row 3 [a or b] is the stronger acid because [a)because F is more elecronegative than Cl or b) because Cl is bigger than F].
- In Row 4 [a or b] is the stronger acid because [a) because the two chlorines are further apart delocalizing the indicative effect in the conjugate base or because the two chlorines are closer to the negative charge in the conjugate base] .
More the stability of conjugate base, more stronger the acidic strength of acid is.
Electro withdrawing group stabilize the conjugate base.
More the electron donating power, more stable the conjugate base.
More the number of electron withdrawing group near to the negative charge of conjugate base, more the stability.
Electron withdrawing power of halogen increases in this order:
I < Br < Cl < I
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