Download Chemistry I Final Review

Chemistry I Final Review (Ruppel)
Name __________________________________
CUMULATIVE QUIZ #1
Mathematics:
1. Convert:
a. 15 mg to grams
b. .00045 nm to cm
2. Write in scientific notation/regular
a. 156000000
3.
Solve
b. .00000942
c. 7.5 x 103
d. 8.64 x 10-4
b. _____ 200000
c. _____ .00055000
d. _____ 1010
2.5 x 1023

7.56 x 1013
4. How many significant figures?
a. _____ 23
3
5. What is the density of an object with a mass of 2.94 g and a volume of 38 cm ?
Matter & Energy:
6. What has more kinetic energy-a parked truck or a feather floating in the air?
7. Identify as an element (E), compound (C), heterogeneous mixture (M) or solution (S)?
a. __________ sodium carbonate
c. __________ carbon
b.__________sugar water
d.__________rocks and sand
8. Physical (P) or chemical (C) change?
a.___________ burning magnesium
c.___________ powdering a sugar cube
9. Convert to Kelvin
10. Convert to °C
a. 15°C
b. __________melting ice
d. __________ iron rusting
b. -258°C
a. 59K
b. 491K
The Atom:
11. Complete the following table:
isotopic
symbol
atomic
number
mass
number
19
electrons
protons
neutrons
10
8
10
9
1
12. How many electrons, protons and neutrons in a:
a. sodium-23 ion
b. fluoride-19 ion
CUMULATIVE QUIZ #2
Nuclear:
13. Write the nuclear equation for the:
a. alpha decay of Uranium-238
b. beta decay of Lead-214
14. Carbon-14 has a half life of 5700 years. How long will it take for a sample which contains 100. g of carbon -14 to
decay to 12.5 g.
The Electron:
15. In terms of electrons, explain why elements give off light (atomic emission spectrum) when an electric current is
applied.
16. Write the electron configuration for the following atoms and state how many valence electrons each has:
a. Potassium atom
b. Bromine atom
17. Draw the orbital box diagram for Sulfur. How many unpaired electrons does it have?
Periodic Table and Periodic Trends:
18. What is a group, family, period?
19. How many valence electrons do the alkaline earth metals have? The Halogens?
20. What is the ionic charge of the alkali metals? How does that affect their reactivity
21. Which is larger?
a. Ca or K
22. Which has the smaller ionization energy?
b. P or N
c. O or O-2
a. Na or Mg
b. C or Si
2
Naming & Bonding:
23. Using the table of electronegativities, determine the bond type between:
a. K and Cl
b. S and O
24. Draw the dot diagram for the covalent compound CCl
c. C and H
4
25. Draw the dot diagram for the ionic compound Li S
2
26. Name the following ionic compounds
a. NaBr _________________________________
b. Ca(NO ) _______________________________
c. FeF _____________________________ ____
d. Cu SO _________________________________
3
3 2
2
3
27. Write the formulas for the following ionic compounds.
a. potassium oxide ________________________
b. barium chlorite______________________
c. tin (IV) oxide___________________________
d. lead (II) acetate______________________
28. Write the names for the following molecular (covalent) compounds.
a. S O __________________________________
2
3
b. P O _________________________________
2
5
29. Write the formula for the following molecular compounds.
a. dinitrogen pentoxide_____________________
b. sulfur trioxide________________
CUMULATIVE QUIZ #3 
Equations:
30. Balance the following equations:
a. Na + H O →
NaOH +
2
b. C H
8
18
O → CO
+
2
c. Na + Al (SO )
2
4 3
2
+ HO
2
→
H
2
Al
+
Na SO
2
4
31. Predict the products for the following reactions and balance the equations.
HCl →
a.
Mg
+
b.
NaCl
e


c.
CH
+ O
d.
Al
e.
2
6
→
Cl →
+
Ca(OH)
2
2
2
+
AlF
3
→
32. Identify the reaction type for each equation in #2 to the left of the letter.
3
Moles:
33. What is the molar mass of Ca (PO ) ?
3
4 2
34. Convert
a. 6.5 g of NaCl to moles
22
b. 3.58 x 10 atoms of He to liters.
c. 39.7 g C H O to molecules
12
22
11
35. Determine the percent composition of Al(NO )
3 3
36. A compound is determined to consist of 85.7 % carbon and 14.3 % hydrogen
a. determine the empirical formula of the compound.
b.
if the compound has a molar mass of 56 g/mol, determine the molecular formula.
Stoichiometry:
37. How many grams of chlorine gas are needed to react completely with 23.0 g of sodium in the following unbalanced
reaction? Na + Cl2 → NaCl
38. How many liters of hydrogen gas are produced when a 0.250 g piece of magnesium is placed in a beaker of
hydrochloric acid? Assuming all the Mg is used up. Write the balanced equation first.
39. If 3.50 L of nitrogen gas react with hydrogen gas, how many molecules of ammonia gas are produced at STP?
N2 + 3H2 ↔ 2NH3
4
CUMULATIVE QUIZ #4
Heat:
40. An exothermic /endothermic reaction absorbs heat and its ∆H is negative/positive. (circle one each)
41. If the average kinetic energy of the particles of a gas decreases, what happens to the temperature?
_________________
42. What quantity of heat is released when 14.9 g of SO reacts according to the following equation?
2
2SO
2
+
O → 2SO
2
3
H= -197.8 kJ
43. How much heat is released when 432 g of water cools from 71.0 ºC to 18.0 ºC? (C water = 4.184 J/g ºC)
44. From the following enthalpy changes,
Cu(s) + Cl2(g) → CuCl2(s)
2Cu(s) + Cl2(g) → 2CuCl(s)
∆Hº = -206.0 kJ
∆Hº= -136.0 kJ
Calculate the value of ∆Hº for the reaction
CuCl2(s)
+
Cu(s)
→
2CuCl(s)
Gas Laws:
45. If pressure is held constant, what happens to the volume as the temperature is doubled? __________________
46. If temperature is held constant, what happens to the volume if the pressure is quadrupled? _________________
47. At 75 ºC, a gas has a volume of 3.22 L. What volume will it occupy at 75 K?
48. If the volume of a gas is 19.4 L at 4.99 atm, what is the volume at 1580 mm Hg?
5
49. If CO2 gas occupies 22.4 L at STP, what will its temperature be if it is compressed to 15.0 L at a new pressure of
2.00 atm?
50. What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 dm3 container at a temperature of
20.ºC? (Ideal Gas Constant = 0.0821 L•atm / mol•K)
--------------------------------------------------------------------------------------------------------------------------- ----------------------Solutions:
51. What is the molarity of a solution formed by mixing 8.0 g of NaOH with enough water to make 150. mL of
solution?
52. How many grams of potassium bromide should be added to water to prepare 0.50 L of solution with a molarity
of 0.125 M?
53. Using your solubility curve if you dissolve 50. g of NH4Cl at 40 °C what kind of solution do you have?
(saturated, unsaturated or supersaturated)
54. Using your solubility curve, what is the solubility of NH3 at 50°C?
Reaction Rates:
55. Draw an energy diagram for an exothermic reaction. Label the following items: reactants, products,
activation energy of the forward reaction, the activated complex, reaction progress, and potential energy
6
56. How does the catalyst speed up a reaction?
57. In general the rate of a reaction ______________________ as temperature increases.
Equilibrium/LeChatlier:
Answer the following about the classic Haber Process Reaction:
N2(g) + 3H2 (g) ↔ 2NH3(g) + Heat
58. If you add nitrogen the forward reaction will increases / decreases. (circle one)
59. If you remove ammonia from the reaction vessel, the reaction will shift ___________ to make more _________.
60. If you heat up the above reaction, the forward reaction will decrease / increase. (circle one)
61. If you increase pressure the forward / reverse reaction will increase. (circle one)
Acids & Bases:
62. An acid turns litmus paper red/blue, has a bitter/sour taste, does/does not react with metals. (circle one each)
63. When an acid and base react the products are usually a ________________ and _________________.
64. What is the pH of a 3.4 x 10−5M solution of HCl? Name this substance.
65. Determine the pH of a 0.015 M LiOH solution.
66. a) What is the conjugate acid of NH3?
b) Identify the conjugate acid-base pairs in the following reaction.
H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4−(aq)
67. In a titration experiment, a 12.5 mL sample of 1.75 x 10−2 M NaOH neutralized 14.5 mL of an HNO3 solution.
What is the molarity of the HNO3 solution?
7
Answer Key
Mathematics:
1.
2.
3.
4.
5.
b. 4.5 x 10-11cm
b. 9.42 x 10-6
a. .015g
a. 1.56 x 108
3.3 x 109
2;1;5;3
0.077g/cm3
c. 7500
d. 0.000864
Matter & Energy:
6. feather
7. C;S;E;M
8. C;P;P;C
9. 288K; 15K
10. -214 ºC; 218 ºC
Atom:
11.
23
11
Na
11
23
11
11
12
18
8
O -2
8
18
10
8
10
Cu
29
65
29
29
36
F
9
19
9
9
10
65
29
19
9
12. a. 11p+, 12nº, 10e-
Nuclear:
13a.
238
92
U
b. 9p+, 10nº, 10e-
4
2
α+
Th
234
90
b.
214
82
Pb  -10 β +
214
83
Bi
14. 17,100 years
Electron:
15. When electrons become excited, they jump to a higher energy level. At this level they are unstable and fall
back to a lower energy level. When they fall, they release energy.
16. a. 1s22s22p63s23p64s1 , 1
b. 1s22s22p63s23p64s23d104p5 , 7
        
17.
1s
2s
2p
3s
,2
3p
Periodic Table:
18.
19.
20.
21.
22.
Group and Family (vertical columns); Period (Horizontal row)
2; 7
+1; very reactive – loose their 1 valence electron easily
a) K b) P c) O-2
a) Na b) Si
Bonding & Formulas:
23. a) Ionic b) Polar Covalent c) Covalent
24.
8
25.
26. a) sodium bromide
27. a) K2O
28. a) disulfur trioxide
29. a) N2O5
Equations:
30. a. 2,2,2,1
31 & 32.
a.
b.
c.
d.
e.
Mole:
33.
34.
35.
36.
Gases
b) calcium nitrate
c) iron (III) fluoride
b) Ba(ClO2)2
c) SnO2
b) diphosphorus pentoxide
b) SO3
b. 2,25,16,18
c. 6,1,2,3
Mg + 2HCl → MgCl2 + H2
2NaCl → 2Na + Cl2
2C2H6 + 7O2 → 4CO2 + 6H2O + heat
2Al + 3Cl2 → 2AlCl3
3Ca(OH)2 + 2AlF3 → 3CaF2 + 2Al(OH)3
310.3 g/mol
0.11 mol; 1.33 L; 6.99 x 1022 molecules
12.7 % Al, 19.7% N, 67.6% O
CH2; C4H8
45. doubles
46. quartered
47. 0.69 L
48. 46.5 L
49. 366 K
50. 0.13 atm
Reaction Rates
Activated Complex
R
d) copper (I) sulfite
d) Pb(CH3COO)2
(Single Replacement)
(Decomposition)
(Combustion)
(Synthesis)
(Double Replacement)
Stoichiometry:
37. 35.5 g Cl2
38. Mg + 2HCl → MgCl2 + H2
38. 0.230 L H2
39. 1.88 x 1023 molecules
Heat:
40. endo/positive
41. decreases
42. -23.0 kJ
43. -95.8 kJ
44. +70.0 kJ
Solutions
51. 1.3 M
52. 7.5 g KBr
53. supersaturated
54. 30 g /100g H2O
Equilibrium/LeChatlier
58. increases
59. right, NH3
60. decrease
61. forward
Acids & Bases
62. red, sour, does
63. salt and water
64. pH = 4.47 hydrochloric acid
65. pH = 12.18
66a. NH4+
b. H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4−(aq)
A
B
CA
CB
67. 0.0151M
P
Reaction Progress
56. Catalyst speeds up the reaction by providing an alternate pathway requiring less activation energy.
57. increases
9