Ch. 7 (pages 395-404): 6, 8, 16, 22, 28, 32, 40, 46, 56, 60

 

6. Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:

(a) I

(b) Sr

(c) K

(d) N

(e) S

(f) In

 

8. Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater):

(a) Cl

(b) Na

(c) Mg

(d) Ca

(e) K

(f) Br

(g) Sr

(h) F

 

 

16. From its position in the periodic table, determine which atom in each pair is more electronegative:

(a) N or P

(b) N or Ge

(c) S or F

(d) Cl or S

(e) H or C

(f) Se or P

(g) C or Si

 

 

22. Which of the following molecules or ions contain polar bonds?

(a) O3

(b) S8

(c) O22−

(d) NO3−

(e) CO2

(f) H2S

(g) BH4−

 

 

28. Write Lewis structures for the following:

(a) H2

(b) HBr

(c) PCl3

(d) SF2

(e) H2CCH2

(f) HNNH

(g) H2CNH

(h) NO–

(i) N2

(j) CO

(k) CN–

 

32. Write Lewis structures for:

(a) PO4 3−

(b) IC4 −

(c) SO3 2−

(d) HONO

 

40. A compound with a molar mass of about 28 g/mol contains 85.7% carbon and 14.3% hydrogen by mass. Write the Lewis structure for a molecule of the compound.

 

46. Write the resonance forms of ozone, O3, the component of the upper atmosphere that protects the Earth from ultraviolet radiation.

 

56. Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in nitrosyl chloride: ClNO or ClON?

 

60. Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule:

(a) IF

(b) IF3

(c) IF5

(d) IF7

 

 

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