Chemistry Test Questions

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  • Topic: Covalent bond, Chemical bonding, Lewis structure
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Honors Chemistry Chapter Nine PracticeExam
Student: ___________________________________________________________________________ 1. Which of these compounds is most likely to be ionic?
A. KF
B. CCl4
C. CS2
D. CO2
E. ICl

2. Which of these compounds is most likely to be ionic?
A. NCl3
B. BaCl2
C. CO
D. SO2
E. SF4

3. Which of these compounds is most likely to be covalent?
A. Rb2S
B. SrCl2
C. CS2
D. CaO
E. MgI2

4. Which of these compounds is most likely to be covalent?
A. CsOH
B. NF3
C. Sr(NO3)2
D. CaO
E. LiF

5. The Lewis dot symbol for the chloride ion is
A.
B.
C.
D.
E.

6. Which of these ionic solids would have the largest lattice energy? A. NaCl
B. NaF
C. CaBr2
D. CsI
E. CaCl2

7. Which of these solids would have the highest melting point? A. NaF
B. NaCl
C. NaBr
D. NaI

8. Which of these solids would have the lowest melting point? A. KI
B. KBr
C. KCl
D. KF

9. Which of these atom is the most electronegative?
A. Li
B. Cs
C. P
D. As
E. Ge

10. A polar covalent bond would form in which one of these pairs of atoms? A.
B.
C.
D.
E.

11. A nonpolar covalent bond (i.e., pure covalent) would form in which of these pairs of atoms? A.
B.
C.
D.
E.

12. Which of these covalent bonds is the most polar (i.e., highest percent ionic character)? A.
B.
C.
D.
E.

13. In which of these pairs of atoms would the bond be the most polar? A.
B.
C.
D.
E.

14. The electron dot formula for O2 shows
A. a single covalent bond.
B. a double covalent bond.
C. an ionic bond.
D. a total of 8 2 = 16 electron dots.
E. a total of 32 electron dots.

15. The electron dot structure for AsCl3 shows
A. a total of 84 electron dots.
B. three single bonds and 10 lone pairs.
C. two single bonds, one double bond, and 9 lone pairs.
D. one single bond, two double bonds, and 8 lone pairs.
E. three single bonds and one lone pair.

16. The total number of lone pairs in NCl3 is
A. 6.
B. 8.
C. 9.
D. 10.
E. 13.

17. The Lewis structure for a chlorate ion, ClO3-, should show ____ single bond(s), ____ double bond(s), and ____ lone pair(s). A. 2, 1, 10
B. 3, 0, 9
C. 2, 1, 8
D. 3, 0, 10
E. 2, 1, 9

18. Which of these choices is a correct Lewis structure for ozone, O3? A.
B.
C.
D.
E.

19. The number of resonance structures for the nitrate ion that satisfies the octet rule is A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.

20. The azide ion, N3-, is very reactive although it is isoelectronic with the very stable CO2 molecule. This reactivity is reasonable because A. a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero. B. there is no valid Lewis structure possible for the azide ion. C. there are resonance structures for azide ion but not for carbon dioxide. D. nitrogen cannot form multiple bonds.

E. charged species always decompose in solution.

21. Which of these statements is a useful guideline for the application of formal charges in neutral molecules? A. A Lewis structure in which there are no formal charges is preferred. B. Lewis structures with large formal charges (e.g., +2,+3 and/or -2,-3) are preferred. C. The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms.

22. The formal charge on the bromine atom in BrO3- drawn with three single bonds is A. -2.
B. -1.
C. 0.
D. +1.
E. +2.

23. What is the formal charge on sulfur in the best Lewis structure for the SCN- (thiocyanate) ion? A. +2
B. -2
C. +1
D. -1
E. 0

24. What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule? A. -2
B. -1
C. 0
D. +1
E. +2

25. In the best Lewis structure for the fulminate ion, CNO-, what is the formal charge on the central nitrogen atom? A. +2
B. +1
C. 0
D. -1
E. -2

26. Each of the three resonance structures of NO3- has how many...
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