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1. Name the compound CoI3.

a) cobalt iodide
b) cobalt triiodide
c)* cobalt(III) iodide
d) cobaltous triiodide

2. What is the correct name for Ca(NO2)2?

a) calcium nitride
b)* calcium nitrite
c) calcium nitrate
d) calcium(II) nitrate

3. The oxidation number of N in NO is:

a) 0
b) +1
c) -1
d)* +2

4. Which of the following acids is(are) correctly named?

(i) H2SO3, sulfurous acid
(ii) HClO3, chlorous acid
(iii) H3PO3, phosphorous acid

a) i
b) ii and iii
c)* i and iii
d) all of them

5. Iron(II) nitrate is:

a)* Fe(NO3)2
b) Fe2NO3
c) Fe(NO2)2
d) Fe2N

6, The melting point of brimstone is 119C. Calculate this temperature in F.

a)* 246 F
b) 151 F
c) 87.0 F
d) 98.1 F

7. The density of aluminum is 2.70 g/mL and the density of water is 1.00 g/mL. Find the specific gravity of aluminum.

a)* 2.70
b) 0.370
c) 48.6
d) 3.70

8. The % S in NiSO4 is:

a) 16.19
b)* 20.68
c) 15.49
d) 36.58

9. Which of the following products would result from the reaction of H3PO4 and NaOH?

a) NaPO4 + H2O
b) Na(PO4)2 + H2O
c)* Na3PO4 + H2O
d) Na(PO4)3 + H2O

10. When the following equation is balanced, the sum of the coefficients is:

F2 + NaI ----------> NaF + I2

a) 4
b)* 6
c) 3
d) 5

11. When the following equation is balanced, the sum of the coefficients is:

P2O5 + H2O ----------> H3PO4

a) 5
b)* 6
c) 4
d) 7

12. How many grams of a 6.0 percent KOH solution by weight are necessary to yield 120 grams of KOH?

a) 1000 g
b)* 2000 g
c) 3000 g
d) 4000 g

13. 50.0 g of LiOH is mixed with 50.0 g of HCl. Which chemical is in excess and what weight of LiCl is produced?

a) LiOH, 37.6 g
b) HCl, 3.9 g
c) HCl, 19.2 g
d)* LiOH, 58.1 g

14. Which of the following electron configurations represents a paramagnetic atom?

a) 1s22s22p3
b) 1s22s22p4
c) 1s22s22p5
d)* All of the above

15. How many orbitals are present in the 4d subshell?

a) 0
b) 1
c) 3
d)* 5

16. Identify the species which is not isoelectronic with argon.

a)* P3+
b) S2-
c) Cl-
d) K+

17. Which of the following atoms is the most electronegative?

a)* Cl
b) Br
c) As
d) Ge

18. A column on the periodic table represents:

a) a certain orbital
b)* a chemical family
c) a certain physical property
d) uniform crystal structure

19. How many protons are contained in the lead-208 nucleus?

a)* 82
b) 126
c) 208
d) no correct answer given

20. What is the charge carried by a positron?

a) -1
b) 0
c)* +1
d) +2

21. At the same ______, the molecules of all samples of ideal gases have the same average kinetic energies.

a)* temperature
b) pressure
c) mass
d) density

22. What mass of CH4 is contained in a 500-mL sample of CH4 gas at -40.0C and 300 torr?

a) 0.0870 g
b)* 0.165 g
c) 0.322 g
d) 0.734 g

23. Water reacts with oxides of non-metals to form a(n):

a) solution containing a base
b)* solution containing an acid
c) anhydride
d) hydride

24. What is the name of Ni(ClO4)2?

a)* nickel(II) perchlorate
b) nickel(II) chlorate
c) nickel(II) hypochlorite
d) nickel perchlorate

25. Name the compound HCl(aq).

a) hydrogen chlorine
b)* hydrochloric acid
c) chloric acid
d) chlorous acid

26. How many grams of sucrose (C12H22O11) must be dissolved in 300 g of water if a 0.250 molal solution is required?

a.* 25.6 g
b. 342 g
c. 741 g
d. 3.72 g

27. How many grams KF are needed to prepare 600 mL of a 2.25 M solution of KF?

a. 23.2 g
b.* 78.4 g
c. 34.9 g
d. 12.8 g

28. A 0.397-gram sample of a gas occupies a volume of 275 mL at 10C and 365 torr. What is the molecular weight of the gas?

a) 85.9 g/mol
b) 72.8 g/mol
c)* 69.8 g/mol
d) 61.3 g/mol

29. A sample of a gas occupies a volume of 350 mL at 3000 torr and 25C. Calculate the number of moles of gas present.

a)* 5.65 10-2 moles
b) 8.39 10-3 moles
c) 1.25 10-2 moles
d) 1.38 10-2 moles

30. The strength of an electrolyte is determined by the

a. oxidation state of an ion
b.* concentration of its ions in solution
c. number of ionic bonds
d. number of covalent bonds

31. What is the pH of a 0.0010 M KOH solution?

a. 3.00
b. 4.00
c.* 11.00
d. 10.00

32. What is the equilibrium expression for the reaction:

2 SO2(g) + O2(g) ----------> 2 SO3(g)

a. Kc = [SO3]2/ [O2] + [SO2]2
b.* Kc = [SO3]2/[O2][SO2]2
c. Kc = 2[SO3]/2[SO2][O2]
d. Kc = [SO2]2[O2]/ [SO3]2

33, Which of these compounds would be an acid anhydride?

a)* CO2
b) NH3
c) CaO
d) Na2O

34. Which of the following products would result from the reaction of H3PO4 and NaOH?

a) NaPO4 + H2O
b) Na(PO4)2 + H2O
c)* Na3PO4 + H2O
d) Na(PO4)3 + H2O

35. Significant figures in a number comprise

a) only all digits known with certainty
b) two uncertain digits
c)* all the digits known with certainty plus the first digit that is uncertain
d) the number of digits including the one after the decimal point

36. An ion is an atom (or a group of atoms) which is:

a) electrically neutral
b)* electrostatically charged
c) always positive
d) always negative

37. A 1.367-gram sample of a compound was heated in the air to yield 3.002 g CO2 and 1.640 g H2O. If the compound contained only C, H, and O, what is its empirical formula?

a) CHO
b) C2H2O
c) C2H6O
d)* C3H8O

38. Uranium reacts with fluorine to produce a gas whose density is 13.0 g/L at 57C and 1 atm pressure. What is its molecular formula?

a) UF5
b)* UF6
c) UF3
d) UF4

39. When freezing, a liquid:

a)* loses energy
b) gains energy
c) decreases in temperature
d) increases in temperature

40. An anion is an atom (or a group of atoms) which is:

a) electrically neutral
b) electrostatically charged
c) always positive
d)* always negative

41. With one exception, the elements of the Noble Gas Family have an outer shell composed of:

a) 1 electron pair
b) 2 electron pairs
c) 3 electron pairs
d)* 4 electron pairs

42. The sum of the atomic weights of all the atoms present in the formula of any compound is called the

a) empirical formula
b) molecular weight
c)* molar mass
d) equation weight

43. The oxidation number of hydrogen in a metal hydride is

a)* -1
b) 0
c) +1
d) +2

44. The name for the element with the symbol Bi is:

a) lead
b)* bismuth
c) titanium
d) potassium

45. Calculate the freezing point of a solution that contains 40. g of glucose (C6H12O6) in 500 g of water.

a. 0.83 C
b.* -0.83 C
c. 1.04 C
d. -1.04 C