AP Chemistry                                                                           Unit 8

Chapter 8                                                                                 Bonding

Daily

 

1. Which of the following bonds do you expect to be polar covalent?

a. H-N      b. H-H       c. Cs-F            d. H-O

 

2.What is the electronegativity difference  between At and H

a. 0.1      b. –0.1       c. 4.3         d. 0.1

 

3.Order for the following bonds in order of increasing bond polarity

    1. C-At<Se-Cl<C-O<H-F
    2. C-O<Se-Cl< H-F<C-At
    3. H-F<C-O<Se-Cl<C-At
    4. C-At <C-O<Se-Cl<H-F

 

4.Which of the following molecules would you expect to exhibit the greatest polarity (all are tetrahedronal)

            a. CHCl3  b. CH4             c.CCl4              d.CH3Cl

 

5. Which ion could the following electron configuration describe, 1s22s22p63s23p4

            a. K+                b. Cl+               c. S-2                d. Ca+2

 

6. Place the following species in order of increasing size

a.       B+3<Be+2<Ne<O-2

b.      Ne<B+3<Be+2<O-2

c.       O-2<Ne<Be+2<B+3

d.      Ne<O-2<B+3<Be+2

 

7. Select the system with the largest lattice energy

            a. NaCl            b. KCl              c. K2S              d. CaO

 

8. Two bonded atoms

a.       react more readily with other substances

b.      are less reactive than their free form

c.       share all their electrons

d.      behave in unpredictable ways

 

9. A truck uses propane (C3H8) to power the engine. Calculate the heat released when 5 moles of propane are burned (typical combustion products formed)

            a. 7330 kj         b. 25kj             c. 10,000kj            d. 4784 kj

 

10. How many valence electrons does selenium have

            a. 6            b. 4            c. 3            d. 5

 

11. How many of the 6 valence electrons for oxygen are typically used in covalent bonding?

            a. 4            b. 3            c. 6            d. 2

 

12. Which of the following molecules possesses a triple bond

            a. SF4               b. PCl5             c. C2H2                        d. C2H6

 

13. Which of the following contains a central atom that violates the octet rule

            a. SF4               b. COF2   c. Si(OH)4            d. PBr3

 

14. Calculate the number of valence electrons on the central atom in ClO4-1

            a. 6                  b. 8                  c. 10                d. 12

 

15. Indicate the bond type in the following

a.       O-H

b.      Cs-Cl

c.       H-Cl

d.      Br-Br

 

16. Calculate the energy interaction between a Ag+1 and a Br-1 if the internuclear bond length is 0.12nm

 

17. Using the table, order the following in terms of electronegativity

            F, Nb, N, Si, Rb, Ca, Pt

 

18. Place the following in terms of increasing polarity

            NaBr, I2, H2O, MnO2, CN-1

 

19. How will the charge be distributed on each of the following molecules

            HF, NO, CO, HCl

 

20. Determine and draw the orientation of the dipole on the following

            AlCl3, CH3F, N2O, AgCl4-1 (square planar)

 

21. Which of the following have a dipole of zero

            KI, CF4, H2Se

 

22. List 4 ions that are isoelectric with Ar and have a charge from +2 to –2 and arrange these in size

 

23. Determine the formula for

a.       Ca and O

b.      K and Cl

c.       Rb and S

d.      Ba and P

 

24. Using shorthand notation list the lewis structures for

a.       Mg and N

b.      Na and F

c.       Ca and S

d.      Sr and Te

 

25. Place the following in order of increasing size

            Cl-1, F-1, Sr+2, Ca+2

 

26. Use bond energies to determine ΔH for the following reactions (not balanced)

a.       C2H2 +  H2 à C2H4

b.      CH4  +  O2  à  CO  + H2O(g)

c.       N2  +  H2  à  N2H4

 

27. Calculate the enthalpy for the following reaction

 

            H2  +  C2H4  à  C2H6

 

28. Draw Lewis structures for

            a. H+1            b. C            c. P            d. P+5            e. Cl-1

 

29. Draw Lewis structures for

            a. BCl3             b. AsF5            c. BrO3-1  d. S2F10

 

30. Draw as many reasonable resonance structures for C and O as possible

 

31. Draw a resonance structure for benzene C6H6

 

32. Discuss the nature of the bonds in the following (indicate # of sigma and pi bonds)

 

33. Determine the geometry and # of electrons on the central atom for the following

            SCl4, H2Se, IF4-1, SnCl5-1, TiCl2