Download CP Chemistry First Semester Final Exam 1

CP Chemistry
First Semester Final Exam
1-20 Matching: Write the letter of the correct answer from Column B in the space before the
term in Column A.
Column A
Column B
____ 1. Reactants
____ 2. Metals
____ 3. Ionic bond
____ 4. Atomic number
____ 5. Isoelectronic
____ 6. Quantum
____ 7. JJ Thomson
____ 8. Anion
____ 9. Cation
____ 10. Mendeleev
____ 11. Atomic mass
____ 12. Covalent bond
(a)
(b)
(c)
(d)
(e)
(f)
(g)
(h)
(i)
(j)
(k)
(l)
____
____
____
____
____
____
____
____
(m)
(n)
(o)
(p)
(q)
(r)
(s)
(t)
13.
14.
15.
16.
17.
18.
19.
20.
Products
Ernest Rutherford
Dissolved in water
Valence electrons
Moseley
Octet rule
Niels Bohr
Ground state
weighted average of all the isotopes of an element
having the same electron configuration as another element
Planetary Model of the atom
He listed the elements in order of increasing atomic mass.
any atom or molecule with a (+) charge
the number of protons in an atomic nucleus
(aq)
atoms bond in order to obtain 8 valence electrons
are found in the outer s and p sublevels
substances found on the left side of a chemical equation
He listed the elements in order of increasing atomic number
all electrons in the atom are in the lowest available
energy levels
substances found on the right side of a chemical equation
results from the attraction between (+) and (-) particles
elements found left of the zig zag line on the periodic table
Plum Pudding model of the atom
any atom or molecule with a (-) charge
occurs as atoms share valence electrons
Gold Foil Experiment
energy needed to move from one energy level to another
21-25 Determine the most common oxidation state (charge) of the following elements:
21. selenium ____
22. oxygen
____
23. aluminum ____
24. barium
____
25. sodium
____
26-27 Name the two subatomic particles found in the nucleus of an atom.
26.
27.
28-29 Write the electron configurations for the following atoms:
28. As
29. Ca
33-36 Determine whether the following compounds contain ionic or covalent bonds.
33. K2Se
34. SO3
35. CCl4
36. KCl
37-39 Name the following polyatomic ions:
37. CrO4-2
38. BO3-3
39. PO4-3
40-42 Write the formulas for the following polyatomic ions:
40. iodate
41. thiosulfate
42. carbonate
43-52 Name the following compounds
43. NaBr
45. H2Se
44. BF3
46. H2CrO4
47. NH4NO3
48. MgCl2
49. KCN
50. Ca3(PO4)2
51. SF6
52. Fe(NO3)3
53-62 Write the formulas for the following compounds
53. carbonic acid
58. tetraphosphorus triselenide
54. sodium chlorate
59. dinitrogen heptoxide
55. potassium bromide
60. lead II sulfide
56. hydrofluoric acid
61. sodium thiosulfate
57. nickel II hydroxide
62. magnesium sulfate
63.
Determine the identity of the element from the following electron configuration.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
64.
How many electrons can fit in the 4th energy level?
65-70 Short answer.
65. What is the family name of the group 1A elements?
66. What is the family name of the group 8A elements?
67. What is the general classification of elements right of the zigzag line on the periodic table?
68. What is a period on the periodic table?
69. What is the family name of the group 7A elements?
70. What occupies the majority of the volume of an atom?
71-74 Determine the number of valence electrons in the following atoms.
71. Kr
72. Ca
73. Li
75.
76.
74. B
Write the symbol for the ion of iodine.
What do you name the ion of iodine?
87-88 Predict the molecular structures of the following substances:
87. NH3
88. CBr4
89.
Determine the number of neutrons in
197
Au+3
79
90.
The identity of an element is determined by the number of what subatomic particle?
91. Place the following atomic models of the atom in the order they were developed.
(a) 4,3,2,1
(b) 3,4,1,2
(c) 1,2,3,4
(d) 2,1,4,3
92) In Rutherfords experiments most of the alpha (α) particles passed through the gold foil while some of
the particles were deflected back towards the particle emitter. The best possible explanation for this is :
(a) the + charged alpha particle is repelled by the + charge of the electrons surrounding the nucleus
(b) there were so many atoms lined up in the gold foil that the alpha particles could not get through the
gold foil and therefore bounced back
(c) the atom is mostly empty space with a small dense + charged nucleus
(d) the alpha particle occasionally collided with a (-) charged electron of one of the gold atoms and
bounced back toward the emitter.
Bonus:
(1) Write the electron dot structure for SO4-2
(2)
Pb(NO3)2 (aq) + 2KI (aq)  2KNO3 (aq) + PbI2 (s)
Suppose you are provided with 100 ml of 0.5 M Pb(NO3)2 and 100 ml of 0.85 M KI. Determine the
limiting reactant for the reaction. (Show your work)
(3)
Determine the energy (in Joules) of the light given off from a hydrogen atom when an electron drops
from the 5th energy level to the 3rd energy level.
90. Convert 165 Kelvin to oC.
92. A sample of a gas has a volume of 1.30 L at 67oC. Assuming constant pressure, determine the
temperature when the volume increases to 2.15 L.
93. At 18oC a sample of neon gas has a volume of 4.22 L and a pressure of 0.645 atm. Determine the
pressure when the temperature changes to 60oC and the volume decreases to 2.40 L.
94. Determine the temperature that must exist for 0.650 moles of argon to exert a pressure of 1330 mmHg
and occupy a volume of 7.75 liters.
95. Determine the graph which best represents how the variables compare in Boyle’s Law
96-97 Discuss the difference between an independent and a dependent variable in a scientific study.
96. independent variable
97. dependent variable
89.
Determine the number of neutrons in
79Au
+3
91. The identity of an element is determined by the number of what subatomic particle?
92-96 Tom and Tessa Toro conducted a chemical experiment in which they added varying amounts of
magnesium to an excess of HCl. They produced magnesium chloride and hydrogen gas. They captured
and measured to hydrogen gas that was produces. The data they collected is presented in the table below:
Mass Mg (g)
0.1
0.2
0.3
0.4
0.5
0.6
Vol H2 (mL)
92
184
276
368
460
553
92. Transfer the data a graph on your answer sheet.
93. What is the dependent variable in Tom and Tessa’s experiment?
(a) The volume of Mg (b) The volume of H2 (c) The mass of Mg (d) The mass of H2 (e) The ‘X’ axis
94. What type of graph should be made with this data?
(a) pie chart
(b) bar graph (c) line graph (d) scatter plot
(e) ”bar and whiskers” graph
95. What type of relationship between the two variables is depicted on the graph you constructed?
(a) neutral
(b) positive
(c) negative
(d) exponential (e) no relationship