Download nomenclature review

Name______________________________________
Period _________
AP Chemistry Midterm I Review
1. Indicate the number of significant figures for each number:
a. 354 ____
b. 0.00809 ____ c. 4,000
____ d. 5,000,300 ____
5
f. 6.75 x 10 ____
32
g. 9.9000 x 10 ____
h. 0.00000008 ____
e. 600.0
____
i. 0.7702 ____
2. Make the following calculations and give your final answers with correct number of sig figs.
a.
7.992
4.67
+ 12.887
b. 9.66
-7
c.
4.44
x 2.1_
d. 824.8 ÷ 2
e.
9.83
- 7.0
f.
2.35
+80.9
3. Determine if each situation is accurate, precise, both, or neither.
a. After 4 trials, Seth determined that the density of water was 1.0g/mL, 1.1 g/mL, .9 g/mL and 1.0 g/mL
b. After 4 trials, Aidan determined that the density of water was 2.0 g/mL, 2.5 g/mL, 1.98 g/mL and 1.0
g/mL
c. After 4 trials, Sheldon determined that the density of water was 2.5g/mL, 2.6 g/mL, 2.56 g/mL and
2.45 g/mL
4. Put the following into proper scientific notation.
a. 40,000
__________________
c. 567
__________________
b. 0.0065
__________________
d. 0.0002022 __________________
e. 20,000,000 __________________
f. 23,000
__________________
g. 92.3
h. 210,000
__________________
__________________
5. DENSITY – Show all work. Don’t forget units and sig figs!!!!! Circle your final answer.
a. What is the density of a piece of wood that has a mass of 25.0 grams and a volume of 29.4 cm3?
b. You have a box filled with 15 vials of aqueous sodium chloride. The total mass of the sodium
chloride is 52.5g and each vial holds 3.2 mL of the solution. What is the density of the solution in
kg/L?
c. An ice cube measuring 5.80 cm by 5.80 cm by 5.80 cm has a density of 0.917 g/mL. What is the
mass?
6. Identify each of the following as an element (E), compound (C), or mixture (M).
______soil
______kool-aid
______paper
______copper
______sulfur
______baking soda, (sodium
______milk
______helium
hydrogen carbonate)
______carbon dioxide
_____mercury
______sugar
______water
Name______________________________________
Period _________
7. Which from #6 would be considered pure substances?
8. List the signs of a chemical change
9. Why are the changes -heat released and color change- not considered chemical changes unless
accompanied by another sign of a chemical reaction?
10. Identify each mixture below as homogeneous or heterogeneous mixtures.
_______________ chocolate chip cookie
_______________
river water
_______________
cough syrup
_______________
salt water solution
_______________
steel
_______________
pure air
_______________
Diet Coke
_______________
granite
11. Identify the described properties as Physical (P) or Chemical (C).
_______ odorless
_______ mass of 5.00 grams
_______ tarnishes rapidly in air
_______ boiling point of 883 C
_______ soft, silver-white
_______ reacts violently with water
_______ reacts with acid
12. Indicate Physical (P) or Chemical (C) change for each example.
________ Metal is heated until it turns red.
________ Aluminum & oxygen react to produce aluminum oxide.
________ An iron nail rusts.
________ Copper metal is hammered into a thin sheet.
________ An ice cube melts.
________ Magnesium chloride is dissolved in water.
________ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water.
13. Why are phase changes considered only physical changes?
14. Sketch an example of the following at the molecular level:
a. a gaseous compound
b. a mixture of elements that is a solid
c. a gaseous mixture of elements and compounds
15. What is the percentage of sodium (by mass) in sodium phosphate? (42.1%)
16. For the hydrate sodium sulfate decahydrate, calculate the following:
(a) the percent of sodium (by mass) in the hydrate (14.3%)
(b) percent of TOTAL oxygen (by mass) in the hydrated compound. (69.6%)
(c) Percent of water (by mass) in the hydrate (55.9%)
17. Calculate the percentage of nitrogen (by mass) in the ammonium nitride (82.4%)
18. Find the empirical formula for a compound that contains 32.8 g chromium and 67.2 g chlorine.(CrCl3)
19. The hydrocarbon used in the manufacture of foam plastics is called styrene. Styrene contains 92.25%
carbon and 7.75% hydrogen. What is the empirical formula of styrene? If the molar mass of styrene is 104
g/mol, what is the molecular formula?
20. Phenanthrene is a hydrocarbon, a compound consisting only of C and H. If you burn 0.215 g of the
compound, and find that it produces 0.747 g of CO2 and 0.109 g of H2O, determine the empirical formula
of the compound.
21. How many moles are there in 768 grams of iron (III) sulfate?(1.92 mol)
22. How many moles are there in 1200g of potassium dichromate?(4.1 mol)
23. You have 13.2 moles of lead (II) nitrate. How many grams is this? (4.37 x 103 g)
24.
How many moles are there in 78 grams of nitrogen gas?(2.8 mol)
25. NAME THE FOLLOWING COMPOUNDS:
1.
BaSO3
14. AgNO3
2.
(NH4)3PO4
15. As2O5
3.
PBr5
16. Fe2O3
4.
MgSO4
17. HClO
5.
CaO
18. N2O3
6.
H3PO4
19. HF
7.
Na2Cr2O7
20. H2C2O4
8.
MgO
21. NaHCO3
9.
SO3
22. SiBr4
10. Cu(NO3)2
23. CuCl2
11. HI
24. HNO2
12. N2O
25. SnO2
13. MnO
26. BaCrO4
WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS:
27. hydrobromic acid
40. diphosphorus pentoxide
28. chromium(III) carbonate
41. sulfurous acid
29. magnesium sulfide
42. lead(II) nitrate
30. iodine trichloride
43. dihydrogen monoxide
31. lithium hydride
44. sodium oxalate
32. ammonium hydroxide
45. perchloric acid
33. calcium chloride
46. chlorous acid
34. hydroselenic acid
47. silicon dioxide
35. iron(II) nitride
48. carbonic acid
36. aluminum hydroxide
49. sodium chlorate
37. tin(II) fluoride
50. xenon hexafluoride
38. sulfur tetrachloride
51. nickel nitrate
39. mercury(II) iodide
52. potassium perchlorate
26. Calcium nitrate can be produced by reacting excess nitric acid with calcium
hydroxide.
a.
If 7.40g of calcium hydroxide reacts with excess nitric acid, how many
grams of calcium nitrate are formed?(16.4grams)
b.
If you performed the same reaction above in the lab and obtained 14.3g
of calcium nitrate, what is your percent yield?
c.
How many grams of nitric acid are needed for a complete reaction (all
7.40 g of calcium hydroxide are consumed)
Write the net ionic equation for the following:
27. Solutions of lead (II) nitrate and lithium chloride are mixed
(Pb2+ + 2Cl- → PbCl2)
28. Solutions of silver acetate and barium chloride are mixed
(Ag+ + Cl- → AgCl)
29. Solutions of tin (II) fluoride and lithium carbonate are mixed.
(Sn2+ + CO32- → SnCO3)
30. Solid sodium bicarbonate is mixed with a concentrated solution of acetic acid
(NaHCO3 + HC2H3O2 → Na+ + C2H3O2- + H2O + CO2)
31. Hydrochloric acid is mixed with a solution of sodium hydroxide
(H+ + OH- → HOH)
32. Ammonia is added to water
(NH3 + H2O ↔ NH4+ + OH-)
33. What is the equilibrium expression (Keq) dependent upon?
34. If the equilibrium constant for A + B
2C
2A + 2B is___________.
C is 0.56, then the equilibrium constant for
35. If the concentration of the product were to double, what would happen to the
equilibrium constant?
36. For the reaction H2(g) + Cl2(g)
2HCl(g), Kc = 1.22 x 1033 at a temperature of
301 K. What is Kp at this temperature? (1.22x 1033)
37. Consider the reaction
What is the
At 1273 K, the Kp value is 167.5.
at equilibrium if the
is 0.17 atm at this temperature? (5.3atm)
38. Consider the following reaction:
2HF(g)
H2(g) + F2(g)
(K = 1.00
10–2)
Given 1.00 mole of HF(g), 0.362 mole of H2(g), and 0.750 mole of F2(g) are mixed in a
5.00 L flask, determine the reaction quotient, Q. (Q = 0.272)
39. Carbon disulfide and chlorine react according to the following equation:
CS2(g) + 3Cl2(g)
S2Cl2(g) + CCl4(g)
When 2.14 mol of CS2 and 5.85 mol of Cl2 are placed in a 2.00-L container and
allowed to come to equilibrium, the mixture is found to contain 0.620 mol of CCl4.
How many moles of Cl2 are present at equilibrium? (3.99 mol)
40. Given the equation 2A(g)
2B(g) + C(g). At a particular temperature,
K = 1.6 x 104. If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter
container, which direction would the reaction initially proceed? (to the left)
41. Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and is allowed to reach
equilibrium described by the equation N2O4(g)
2NO2(g)
If at equilibrium the N2O4 is 37% dissociated, what is the value of the equilibrium
constant, Kc, for the reaction under these conditions? (0.87)
42. Consider the following system at equilibrium: N2(g) + 3H2(g)
2NH3(g) + 92.94 kJ
Which of the following changes will shift the equilibrium to the right? (II, IV, V, VIII)
I.
increasing the temperature
II.
decreasing the temperature
III.
increasing the volume
IV.
decreasing the volume
V.
removing some NH3
VI.
adding some NH3
VII.
removing some N2
VIII.
adding some N2
43. Consider the reaction, which is exothermic as written, PCl5
3(g) + Cl2(g). Which of
the following changes would result in the production of MORE Cl2(g)? (II, VI, VII, VIII)
I.
II.
III.
IV.
V.
VI.
VII.
VIII.
IX.
adding PCl3(g)
removing PCl3(g)
reducing the volume of the container
removing PCl5(g)
increasing the temperature
increasing the volume of the container
adding PCl5(g)
reducing the temperature
adding a suitable catalyst
44. Given the equation 2A(g)
2B(g) + C(g). At a particular temperature, K = 1.6 x 104. At a
higher temperature, K = 1.8 x 10–5. Placing the equilibrium mixture in an ice bath (thus
lowering the temperature) will shift the reaction to the _______________.
45. A 50.0-mL sample of 0.10 M HNO2 (Ka = 4.0 x 10–4) is titrated with 0.12 M NaOH. The pH
after 25.0 mL of NaOH have been added is________. (3.57)
46. For nitrous acid, HNO2, Ka = 4.0 x 10–4. Calculate the pH of 0.27 M HNO2. (1.98)
47. Which of the following is the correct order for increasing pHs for equimolar solutions of
HNO3, KCl, NH4Cl, KOH, and NaC2H3O2? (Ka for HC2H3O2 is 1.80 x 10–5, Ka for NH4+ is
5.56 x 10–10). (HNO3, NH4Cl, KCl, NaC2H3O2, KOH)
48. The following question refers to a solution that contains 1.59 M hydrofluoric acid, HF
(Ka = 7.2 x 10–4), and 3.00 M hydrocyanic acid, HCN (Ka = 6.2 x 10–10).
What is the pH of this mixture of weak acids? (1.47)
NOMENCLATURE REVIEW
ANSWER KEY
1. barium sulfite
2. ammonium phosphate
3. phosphorus pentabromide
4. magnesium sulfate
5. calcium oxide
6. phosphoric acid
7. sodium dichromate
8. magnesium oxide
9. sulfur trioxide
10. copper(II) nitrate
11. hydroiodic acid
12. dinitrogen monoxide
13. manganese(II) oxide
14. silver nitrate
15. diarsenic pentoxide
16. iron(III) oxide
17. hypochlorous acid
18. dinitrogen trioxide
27. HBr
28. Cr2(CO3)3
29. MgS
30. ICl3
31. LiH
32. NH4OH
33. CaCl2
34. H2Se
35. Fe3N2
36. Al(OH)3
37. SnF2
38. SCl4
39. HgI2
40. P2O5
41. H2SO3
42. Pb(NO3)2
43. H2O
44. Na2C2O4
19. hydrofluoric acid
20. oxalic acid
21. sodium bicarbonate
22. silicon tetrabromide
23. copper(II) chloride
24. nitrous acid
25. tin(IV) oxide
26. barium chromate
45. HClO4
46. HClO2
47. SiO2
48. H2CO3
49. NaClO3
50. XeF6
51. Ni(NO3)2
52. KClO4