Descriptive Inorganic Chem: Ch 5 & 6

24 flashcards · Other · by Grace Wilson

1. Arrhenius Acid

   Substance that dissociates to form H+ ions

2. Arrhenius Base

   Substance that dissociates in water to form OH- ions

3. Bronsted-Lawry Acid

   Substance that donates H+ ions

4. Bronsted-Lawry Base

   Substance that accepts H+ ions

5. Lewis Acid

   Substance that accepts and electron pair

6. Lewis Base

   Substance that donates an electron pair

7. What is the bond that forms between a Lewis acid and a lewis base?

   A coordinate bond

8. What does a high Ka value mean?

   Strong acid

9. What does a low Ka value mean?

   Weak acid

10. What does a low PKa value mean?

    Strong acid

11. What does a high PKa value mean?

    Weak acid

12. Amphiprotic

    Both donates and accepts H+ ions

13. Amphoteric

    Both an acid and a base

14. What are the 6 strong acids?

    HCl, HI, HBr, HClO4, H2SO4, HNO3

15. What does it mean if an acid is classified as a strong acid?

    The acid fully deprotonates in water

16. What are the 6 strong bases?

    LiOH, NaOH, Ca(OH)2, KOH, Sr(OH)2, Ba(OH)2

17. What does it mean if a base is classified as a strong base?

    The base is fully protonated in water

18. What happens to the Ka values as a polyprotic acid loses a second or third H+ ion?

    The Ka decreases, because it is harder to take away a second and third H+ ion from the molecule

19. What kind of acid is shown?

    Aqua Acid

20. What kind of acid is shown?

    Hydroxoacid

21. What kind of acid is shown?

    Oxoacid

22. The strength of aqua acids generally increases with increasing positive charge

23. The strength of aqua acids generally decreases with increasing ionic radius

24. Pauling's Rules for oxoacids

    More oxo groups lead to stronger acids, more oxygen atoms lead to stronger acids