Assignment

Part 1: Conversion Problems

Directions: Convert each of the following metric units as indicated.

1. 8.3 Kg = ______________ g           6. 1 cm² = ______________ mm²
2. 346.5 m = ______________ mm     7. 13.5 mL = ______________ μL
3. 193.0 μL = ______________ mL     8. 0.0573 Mg = ______________ lbs
4. 0.6962 mL = ______________ μL   9. 36 s = ______________ ms
5. 235 mL = ______________ cm³     10. 1.25x10⁵ mL = ______________ L

Part 2: Multiple-Choice Questions

1. Which of the following elements is a transition element?
a) oxygen b) chlorine c) bromine d) argon e) nickel

2. Which of the following is a characteristic of the modern periodic table?
a) A group is a column on the periodic table.
b) The period number indicates the subshell being filled by the elements in that period.
c) The elements in each period have similar chemical properties.
d) The group 1A contains the transition elements.
e) The B groups contain the metalloids.

3. What is the smallest particle of an element that retains the properties of that element?
a) an atom b) an electron c) a proton d) a neutron e) a molecule

Part 3: Naming Problems

Directions: Write formulas for these compounds.

4. Magnesium (IV) acetate _________________
5. Iron (III) fluoride _________________
6. dinitrogen pentoxide _________________
7. sodium chloride _________________
8. potassium fluoride _________________
9. ammonium sulfate _________________
10. magnesium iodide _________________
11. copper (II) sulfite _________________
12. aluminum phosphate _________________
13. lead (II) nitrite _________________

Complete the following table by determining the atomic number, mass number, charge, protons, neutrons, and electrons for each element or ion.

Part 4: Short Answer Problems

For each problem below, write the equation and show your work. Always use units and box in your final answer.

14. A patient at a hospital has a temperature of 89.5^oF. What is the temperature in degrees Celsius and in degrees Kelvin?

15. Find the formula mass of:

(a) tin (IV) sulfide, SnS₂ (a) __________________
(b) ammonium bromide, NH₄Br (b) __________________
(c) chromium (III) sulfate, Cr₂(SO₄)₃ (c) __________________
(d) silver cyanide (d) __________________

16. A sample of calcium chloride, CaCl₂, has a mass of 8.4 grams. How many moles are in this sample?

17. What is the mass of 0.10 mole of ammonium carbonate, (NH₄)₂CO₃?

18. How many molecules are contained in 4.0 moles of chlorine gas, Cl₂?

19. Calculate the percent composition by mass of potassium chromate, K₂CrO₄.

20. How many moles are present in 5.6 grams of copper (II) carbonate, CuCO₃?

21. A sample of oxygen gas, O₂, has a mass of 10.0 grams. How many molecules and how many atoms are present in this sample?

22. What is the mass of 8.5 x 10²² molecules of ammonia, NH₃?

23. Calculate the percentage composition of BaC₄H₄O₆.

24. A sample compound weighing 1.587 g is found to contain 0.483 g N and 1.104 g O. Determine the percentage composition.

25. Ethane gas, C₂H₆, reacts with oxygen according to the following balanced chemical reaction:

2C₂H₆ + 7O2 → 4CO₂ + 6H₂O

If 2 moles of ethane gas are allowed to react, how many grams of water will be formed?

26. Calculate the frequency associated with light of wavelength 656 nm.

27. What is the energy of a photon corresponding to microwave radiation of frequency 1.145 x 1010 Hz?

28. Indium compounds give a blue-violet flame test. The atomic emission responsible for this blue-violet color has a wavelength of 451 nm. Obtain the energy of this wavelength?

29. Calculate the temperature of a 345 mL sample of a gas, if the sample occupied 415 mL at 10^oC.

30. What is the pressure on a gas measuring 155 mL if the same gas measured 225 mL at 89.65 kPa?

31. A sample of NO₂ gas with a mass of 3.4 g is measured at 800 mmHg and 25^oC. What is the volume of this gas?

32. Calculate the density of a gas at S.T.P. if 0.244 g of the gas occupies 356 mL at 97.3 kPa and 15^oC.

33. How many moles are in a gas sample occupying 0.500 L at 480 mmHg and 25^oC?

Directions: Calculate the molarity from the given information

a) 145 g of ammonium chromate in 500.0 mL of solution
b) 45.1 g of cuprous sulfate in 250 mL of solution
c) 41.4 g of ammonium nitrate in 100 mL of solution
d) 70.0 g of cadmium (II) iodide in 1000 mL of solution
e) 49.9 g of lead (IV) perchlorate in 200 mL of solution
f) 35.0 g of calcium carbonate in 50.0 mL of solution
g) 45.1 g of cupric dichromate in 1000 mL of solution

Direction: Calculate the number of grams needed to prepare each of the following solutions

a) 1000 mL of 3.00 M sodium hypochlorite
b) 250 mL of 4.00 M ferrous hydroxide
c) 500 mL of 1.50 M mercury (II) sulfide
d) 250 mL of 0.05 M aluminum phosphate
e) 250 mL of 0.0020 M potassium tartrate

34. Determine the concentration of the resulting solution when 267 ml of NaBr is mixed with 233 mL of water

35. How much water must be added to 450 mL of 2.0 M HCl to prepare a solution of 0.75 M HCl?

36. How much water must be added to 550 mL of 3.5 M Ca(OH)₂ to prepare a solution of 2.0 M Ca(OH)₂?

37. How much 2.5 M NaOH is required to prepare a 500 mL of a 1.0 M NaOH solution?

38. How much 6.0 M H₂SO₄ is required to prepare 250 mL of 1.0 M H₂SO₄?

39. Write the electron configurations for the following:

a. Br
b. Sn
c. Ru
d. Fe³⁺
e. C
f. Y
g. Ag⁺
h. Eu
i. I

40. The maximum number of electrons in a P sublevel is: [A] 2 [B] 4 [C] 6 [D] 8 [E] 10

41. The maximum number of orbitals in a D sublevel is: [A] 1 [B] 2 [C] 3 [D] 5 [E] 10

42. The maximum number of electrons in the 3rd energy level is: [A] 2 [B] 8 [C] 18 [D] 10 [E] 32

43. The maximum number of electrons in the S orbital is: [A] 2 [B] 4 [C] 6 [D] 8 [E] 10

44. The maximum number of electrons in the 6th energy level is: [A] 50 [B] 72 [C] 18 [D] 10 [E] 32

45. The maximum number of orbitals in the 2nd energy level is: [A] 1 [B] 2 [C] 3 [D] 4 [E] 5

46. The total number of electrons in the 4th energy level of a chromium atom is: [A] 1 [B] 2 [C] 3 [D] 4 [E] 5

47. The total number of unpaired electrons in a manganese atom is: [A] 1 [B] 2 [C] 3 [D] 4 [E] 5

48. Which of the following sets of quantum numbers represent an electron in the same sublevel as an electron with quantum numbers of: 2 1 -1 +½

a. 3 2 1 -½
b. 2 1 0 +½
c. 3 1 -1 -½
d. 2 0 0 -½
e. 2 0 0 +½

49. Which of the following sets of quantum numbers are ILLEGAL?

a. 6 3 1 +½
b. 3 2 -2 -½
c. 1 0 -1 +½
d. 5 4 -2 +½
e. 2 1 -1 +½

50. A photon of yellow light has a wavelength of 585 nm. Calculate the

a. frequency
b. energy in joules per particle
c. energy in kilojoules per mole.