Final exam review Sp 16 key

Final exam review Sp 16
Classify the following elements as metal (M) , nonmetal (NM) , or metalloid (Me)
1. Al (M)
5. Si (Me)
2. Be(M)
6. He (NM)
3. P(NM)
7. Cl (NM)
4. H(NM)
8. Hg (M)
Classify the following as an element (E) or a compound (C).
9. AuCl ___(C).______
11. P3N5 _(C).____
10. Cu_____ (E) ___
12. Ag____ (E) ________
Classify the following elements as solid (S), liquid (L) or gas(G) at room temperature.
(Use periodic table)
13. H ___(G) ___
16. Br___(G) ____
14. Hg___(L) ___
17. Mg___(S) ___
15. Cl ___(G) __
18. Be____(S) ____
Classify the following as ionic (I) or covalent (C) compounds
19. AuCl (I)
23. N2O (C)
20. P3N5 (C)
24. AgI (I)
21. PbCl4 (I)
25. HgO (I)
22. KCN (I)
26. I2O5 (C)
27. Ca3P2 calcium phosphide
28. Mg3N2 magnesium nitride
29. KCN potassium cyanide
30. BaCO3 barium carbonate
31. CuO copper (II) oxide
Write the formulas for the following ionic compounds.
32.
K+
and
(OH)-
33.
Al+3 and
34.
Mg+2 and O-2
35
Zn+2 and N-3 Zn3N2
(CO3)-2
K(OH)
Al2(CO3)3
MgO
36. P4O6 tetraphosphorus hexaoxide
37. N2O3 dinitrogen trioxide
38. Cl2O7 dichlorine hexaoxide
39. P4O10 tetraphosphorus decaoxide
40. NO nitrogen monoxide
PCl3
42. sulfur hexachloride
SCl5
43. diphosphorous pentoxide P2O5
44. dinitrogen tetroxide
N2O4
45. carbon monoxide
CO
41. phosphorous trichloride
Classify the following as an acid (A), a base (B), or salt (S)
(B)
47. CaCl2 (S)
48. Na2SO4 (S)
49. H2CO3 (A)
50. HCl (A)
46 NaOH
a) anions
a
b
c
51`. Mg(OH)2 (B)
52 H3PO4 (A)
53. NH4OH (B)
b) cations
c) ions
54. Atoms that gain electrons and have a negative charge . Nonmetals form these.
55 Atoms that lose electrons and have a positive charge. Metals form these
56. Atoms with either a positive (+) or negative (-) electrical charge..
Word Bank
a) Metalloids
b
b) Metals
c) Nonmetals
_57. These are found to the left of the staircase and form ionic bonds with nonmetals: give away electrons and become positive. Hydrogen is the
exception
c
58. These are found to the right of the staircase and form covalent bonds with
each other, or take electrons away from metals to form ionic bonds and
become negative
a
59. These touch the staircase in the periodic table and have properties of both
metals and non- metals.
Classify the following as ionic (I) or covalent (C)
(C) _60. This type of bond uses Greek prefixes.
(I) _ 61. This type of bond has a high melting point.
(C) _62. This type of bond is between two nonmetals.
(I) 63. This type of bond is between a metal and a nonmetal.
(C) 64.This type of bond shares electrons.
(I) 65. This type of bond transfers electrons
(I) 66. This type of bond conducts electricity.
(C) 67. This type of bond does not conduct electricity well.
Word bank
a) solute
b) solvent
b 68. The part of a solution that does the dissolving.
a 69. The part of a solution that is dissolved.
Word bank
a) saturated
b) unsaturated
c) supersaturated
a 70. A solution that has all the solute that can dissolve
c 71. A solution that has more than the maximum of solute
b 72. A solution that has less than the amount of solute than can dissolve
For each description below, write A for an acid, B for a base, N for neutral
A 73. Turns litmus paper red
A. 74 Contains more hydrogen ions than hydroxide ions
B 75. Feels slippery
A 76 Tastes sour
B 77. Turns litmus paper blue
A 78. Formula begins with “H” (hydrogen)
B 79. Turns litmus paper blue
B 80. Formula ends with “OH” (hydroxide)
B 81. Have a pH of 7.1 – 14
N 82 Have a pH 7
B 83. Soap
A 84. lemon juice
B 85. Baking soda
A _86. Vinegar
Circle the correct choice.
87. A neutral solution is a/an (salt).
88.A compound that produces hydrogen ions when dissolved in water is a/an(acid).
89. A compound that produces hydroxide ions when dissolved in water is a/an
(base).
90. Stirring a solid solute (increases the solubility of the solid.
91. Heating a gas-liquid solution (decreases) the solubility of the gas.
92. A set of assumptions about how particles act; used to explain the physical
properties of gases. kinetic model
93. The force acting on a certain area. pressure
94. A gas that is described by the kinetic model. ideal gas
95. An instrument that measures atmospheric pressure. barometer
96. The SI unit for measuring pressure. pascal
97. The temperature at which particles in matter stop moving and have no kinetic
energy; 0 K.absolute zero
98. A gas is collected at 120°C. This temperature is equal to 393K.
99. A gas mixture contains ammonia, hydrogen, and methane. The partial
pressures of the gases are 2.0 atm, 1.75 atm, and 8.70 atm, respectively.
The total pressure of the mixture is 12.45 atm.
(use Dalton's law of Partial Pressures)
2.0 atm + 1.75 atm + 8.70 atm = 12.45 atm
100. An “empty” aerosol can at 110 K still contains gas at 1.40 atmosphere
pressure. If an “empty” can is thrown into a 675 K fire, what is the final
pressure in the heated can?
P1= 1.40 atm
T 1= 110 K
(use formula P2 = P1 x T2  T 1)
P2 = 1.40 atm x 675 K  110 K = 8.59 atm
T2= 675 K
101. A gas has a volume of 6.50 L and a pressure of 90.0 kPa. The volume of the gas
expands to 14 L. If the temperature remains constant, the new pressure of the
gas will be 41.79 kPa.
(use formula P2 = P1 x V1  V 2)
P1 = 90.0 kPa
V 1 69.50 L
V 2 = 14 L
P2 = 90.0 kPa x 6.50 L  14 L = 41.79 kPa
102. The splitting of a large nucleus into smaller ones is called fission reaction
103.All transuranium elements have a(n)_ atomic number greater than 92.
104..After one half-life _ one-half of an isotope will still remain. The other fraction
will have decayed.
105. The portion of the electromagnetic spectrum with the shortest wavelength is
Gamma rays
106.The nuclear reactor
is the location where a fission reaction occurs inside a
nuclear power plant
107. During a meltdown in a nuclear power plant, ionizing radiation can escape into
the environment.
108. The portion of the electromagnetic spectrum with the longest wavelength is_ radio
waves
.
109. A CAT scan is a special type of electromagnetic radiation called X-rays
110. The distance from one wave peak to the next is called a wavelength
.
111. The number of wave peaks that pass a given point in a set time is the frequency
112. Ionizing radiation that can pass through soft body tissue, but not bone is
X-rays
113. Isotopes are considered _radioactive__ if their nucleus is unstable.
114. Isotopes can change from one element to another. This is called
transmutation
115. High-energy electromagnetic waves possessing no electric charge are gamma
rays
116. A helium nucleus consisting of two protons and two neutrons is an alpha
particle
117. The joining of two small nuclei into a larger one is a fusion reaction
118. _ Electromagnetic radiation is also called radiant energy.
119. The chemical equation 2 H2O → 2 H2+ O2 is an example
of a decomposition reaction.
120. The chemical equation C3H8 + 5 O2→4 H2O+ 3 CO2 is an example of a
combustion reaction.
121. The chemical equation Ca(OH) 2+ HCl→ CaCl2 + H2O is an example of a
double replacement reaction.
122. The chemical equation 2 H2+ O2→2 H2O
is an example of a synthesis
reaction.
123. The chemical equation
Ba +2H2O →Ba(OH)2 +H2 is an example of a
single replacement reaction.
124. 2 Li2SO4 + Pb(NO3)4  4 LiNO3 + Pb(SO4)2
125. N2 + O2  2 NO
126. Al + 3 CuSO4  Al(SO4)3 + 3Cu
127. 2C4H10 +13O2  8CO2 + 10H2O
128. NaOH Sodium hydroxide
129. HCl hydrochloric acid
130. H3PO4 phosphoric acid
131. H2SO3
sulfurous acid
132. H2CO3 carbonic acid