Finals Flash Cards
(232 cards)
1
Q
Matter is defined as anything that occupies space and has
A
Mass
2
Q
Which pair Is classified as a substance
A
Elements and Compounds
3
Q
Which of the following statements is an identifying characteristic of a mixture?
A
Can be separated by physical means
4
Q
When sample X is passed through a filter paper, a white residue, Y, remains on the paper and a clear liquid, Z, passes through. When liquid Z is vaporized, another white residue remains. Sample X is best defined as
A
Heterogeneous Mixture
5
Q
What best describes a chemical property of the element Iodine?
A
It reacts with Hydrogen to form a gas
6
Q
Ductility and malleability are examples of
A
Physical Properties
7
Q
How man kilo-joules is the equivalent of 750 joules
A
.750 kj
8
Q
Review 8-12 in the packet
A
Skip
9
Q
Compounds are usually broken down into their component elements by
A
Chemical Changes
10
Q
Which Substance can be decomposed by chemical change?
A
Ammonia (Anything that is a substance and not an element)
11
Q
What is an EXTENSIVE physical property?
A
Mass
12
Q
How many kilo-joules of heat energy are absorbed when 100 grams of water is heated from 20 degrees Celsius to 30 degrees Celsius
A
4.18kj
13
Q
What is the total number of joules of heat energy released when 20 grams of water is cooled from 20 degrees Celsius to 10 Degrees Celsius
A
836J
14
Q
Homo means
A
Evenly Mixed
15
Q
Hetero means
A
Unevenly Mixed
16
Q
Intensive means
A
Value stays the same
17
Q
Study 19 In Packet
A
Skip
18
Q
An ideal gas is made up of gas particles that
A
are in random motion
19
Q
What are the qualities of an ideal gas
A
Random Motion, Little attraction for each other, Insignificant volume, Hit wall and build up pressure, Hit each other and transfer energy but total energy remains the same
20
Q
What are the qualities of a real gas?
A
Has volume, have force of attraction
21
Q
Normal Units of pressure
A
STP, 1 atm, 0 degrees Celsius, 760 mmHg, 273 Kelvin, 760 torr
22
Q
Equation for Volume Pressure, Temperature and Moles
A
V1 Phave 1 = V2 P2
____________
T1 n1 = T2 n2
23
Q
An assumption of the kinetic theory of gas is that the particles of a gas have
A
little attraction for each other and an insignificant volume
24
Q
The pressure on 30 milliliters of an ideal gas icreases from 101.3 kPa to 202.6 kPa at constant temperature. The new volume is equal to
A
101.3 kPa
30 mL x ________
202.6 kPa
25
A sample of gas has a volume of 2.0 liters at a pressure of 1.0 atm. When the volume increases to 4.0 liters, at a constant temperature, the pressure will be
.5 atm
26
a 2.5 liter sample of gas is at STP. When the temperature is raised to 273 degrees Celsius and the pressure remains constant the new volume of the gas will be
5.0 Liters
27
S 16 Liter sample of CH4(g) is at 0 degrees Celsius and 1 atm. The volume of the gas sample in liters at 27 Degrees Celsius and 1 atm is equal to
300
22.4 x _____
273
28
When 7.0 Moles of gas A and 3.0 moles of Gas B are combined, the total pressure exerted by the gas mixture is 1.0 atm. What is the partial pressure exerted by gas A in this mixture
.7 atm
29
Which gas will diffuse at the rate under the same conditions of temperature and pressure
H2
30
A .50 mole sample of CO2(g) at 2.0 atm occupies 11.2 liters. What is the temperature of the sample
546 K
31
The density of a gas is 3.00 grams per liter at STP What is the gram molecular mass of the gas
22.4g
32
What is the formula for Lead (II) Oxide
PbO
33
No "o"
Hydro
34
O
Hydro
35
Ate becomes your
Ic
36
Ite becomes your
Ous
37
Complete Combustion
-----> CO2 + H2O
38
Incomplete Combustion
-----> CO + H2O
39
What order you go in when balancing equation
HCO
40
What is the formula for Chromium (III) Oxide
Cr2O3
41
Which Formula is correctly paired with its Name
CuCl2 -----> Copper (II) Chloride
42
What is the correct name for the compound with the formula CrPO4
Chromium (III) Phosphate
43
What is the name of the compound whose formula is H2SO4
Sulfuric Acid
44
The chemical equation 4Na(s) + O2 ---> 2Na^2O(s) is best described as a
Synthesis reaction
45
What type of reaction is illustrated by the following chemical equation 2H2O(l) ---> 2H2(g) + O2(g)
Decomposition
46
The chemical reaction Zn(s) + CuSO4(aq) ---> ZnSO4(aq) + Cu(s) is best described as a
Single replacement reaction
47
What type of reaction best describes the following chemical reaction 2AlCl3(aq) + 3Na2CO3(aq) ---> Al2(CO3)3(s) + 6NaCl(aq)
Double replacement reaction
48
C2H4(g) + 3O2(g) ---> 2CO2(g) + 2H2O(g)
Complete Combustion
49
When the equation C2H4 + 3O2 ---> 2CO2 + 2H2O balanced using the smallest whole numbers, what is the coefficient of the O2
3
50
Al2(SO)3 + 3ZnCl2 ---> 2AlCl3 + 3ZnSO4 is correctly ballanced using the smallest whole number coefficient, the sum of the coefficients is
9
51
KCl(aq) + AgNO3(aq) ---> KNO3(aq) + X What is the correct formula for the product representing X
AgCl
52
In the 1880's JJ Thomson proved the cathode ray hadn a negative charge. What subatomic particle makes up the cathode rays
Electrons
53
What did the discovery of cathode rays reveal about the structure of the atom
Made of subatomic Particles
54
Most alpha articles passed through the gold foil undeflected. What conclusion was made about the structure of the atom based on this observation
Mostly empty space, had to be some postive ions
55
A few alpha particles were deflected back at the source. What did this observation reveal about the structure of the atom
Small dense positive nucleus
56
What term refers to the region of an atom where an electron is most likely to be found
orbital
57
The atomic number of an atom is always equal to the total number of
Protons and Neutrons
58
All atoms of an element have the same
Atomic Number
59
The mass number of an atom is equal to the number of
Neutrons plus electrons
60
What is the mass number of the atom below? 3 H
| 1
3
61
Where is mass
On top
62
How do you find neutrons
Subtract two numbers
63
In which pair of atoms do both neclei contain the same number of neutrons
Whichever two subtract to the same number
64
What is the total number or nucleons (protons and neutrons) in the atom below
Top number is mass and mass is equal to protons+neutrons= Nucleons
65
What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons
45
66
Find the average mass of a sample of magnesium which contains 78.7% Mg-24, 10.1% Mg-25 and 11.2% Mg-26
(24)(.787)+(25)(.101)+(26)(.112)=24.3
67
Element X has two isotopes. If 72% of the element has an isotopic mass of 84.9 atomic mass units, and 28% of the element has an isotopic mass of 87 atomic mass units, the average atomic mass of element X is numerically equal to
(72.0 x 84.9) (28.0 x 87.0)
___________ + ____________
100 100
68
The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (show percents) produces this average mass?
75%^35Cl and 25%^37Cl
69
Which electron dot symbol could represent a metalloid (B, Si, As, Te, At)
If it has 5 dots around it
70
The characteristics bright-line spectrum of an element is produced when its electron
Returns to a lower energy state
71
Which electron configuration represents a potassium ion in the excited state
Add up then identify element if matches, ground state if not excited
72
What is the total number of occupied sublevels in an atom of chlorine in the ground state
5
73
An atom has 8 electrons in a d sublevel. How many d orbitals in this sublevel are half filled
2
74
How do the orbitals go
2, 8, 18, 32, 50
75
What is the total number of sublevels in a principal energy level
2
76
How much does one principal energy level go up by
1 Each Time
77
How many protons are in the nucleus of a magnesium atom?
12 (atomic number)
78
Write the electron configuration for Magnesium in the ground state
1s22s22p63s2
79
How does an atom of magnesium become Mg+2 ion
Loses 2 electrons
80
What noble gas has the same electron configuration as Mg+2
Neon
81
Name three elements that could be X
Oxygen, Sulfur, Selenium
82
The pair of elements with the most similar chemical properties are
The ones right on top and below each other are the closest
83
Which atom has the largest atomic radius?
The one closest to the lower left of the table
84
As the elements of Group 16 are considered from top to bottom on the Periodic Table , the atomic radii
Increase and the ionization energies decrease
85
The S-2 ions differ from the S0 atom in that the S-2 ion has a
Larger radius and more electrons
86
What type of energy represents in the equation Na+energy----> Na+ + e-
Ionization energy
87
Define Ionization Energy
The ionization energy is the exact quantity of energy that it takes to remove the outermost electron from the atom.
88
In which reaction is the first ionization energy greatest
The one closest to the top right
89
Which element in period 2 has the greatest tendency to gain electrons (electronegativity)
One closest to upper right
90
Period is
Horizontal
91
Group is
Vertical
92
What group in the periodic table contains the elements to the alkaline earth family
2
93
When oxygen combines with any alkaline metal, M, the formula of the compound produced usually is
MO2
94
Which Element is a halogen
Group 7A
95
Ozone is an allotropic form of the element
Oxygen
96
Who was credited with creating the first periodic table that organized the elements according to atomic mass
Dmitri Mendeleev
97
A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- Which particle (X or Z) most likely represents a metal atom?
X is metal because it becomes a smaller positive ion
98
A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- which most likely represents a nonmetal atom?
Z because it become a larger negative ion
99
Which metal is the most reactive metal?
The closest to the bottom left is
100
Which is the most reactive non metal
The closest to top right
101
Which element has properties of both metals and non metals
Any metalloid (on the line)
102
Which two elements would most likely combine to form an ionic compound
The metal and non metal farthest from each other
103
Which element can lose electrons from its two outermost energy level
Any transition metal (One of the metals in the middle)
104
Which element exists as a monoatomic gas at STP
Any of the Noble Gases
105
Which element exists as a diatomic gas at STP
C,N,O,F,Cl,Br,I,H
106
Define a transition metal
Is more than one color and can take electrons from more than 1 energy level, can have more than one binary compound
107
Given the reaction: H2 + Cl2 ----> 2HCl
| Which of the following statements best describes the energy change as bonds are formed and broken in this reaction
The forming of the H---Cl bind releases energy
108
Which formula represent an Ionic Compound
Any one with a metal and non metal
109
If the last element is an even coefficiant what is it
Non polar
110
If the last element is an odd coefficient what is it?
Polar
111
Review Questions number 89-93 + Compounds in back of packet
SKIP
112
Which combination of atoms can form a polar covalent bond?
H and Br
113
Which two compounds contain only polar molecules
2 elements with odd coefficients
114
In a nonpolar covalent bond, electrons are
Shared equally by two atoms
115
Which of the following statements best explain why a CH4 molecule is non polar
CH4 has a symmetrical charge distribution
116
```
The table below shows four compounds and the boiling point of each: Which type of molecular attraction accounts for the high boiling points
Compound | Boiling Point
H2O 100 C
H2S -60.7 C
H2Se -41.5 C
H2Te -2.2 C
```
Hydrogen Bonding
117
```
The table below shows four compounds and the boiling point of each: Compared the boiling points of H2S, the boiling point of H2O is relatively high. Which type of bonding causes this different?
Compound | Boiling Point
H2O 100 C
H2S -60.7 C
H2Se -41.5 C
H2Te -2.2 C
```
Hydrogen
118
What is the Gram Formula Mass of Al2(SO4)3
342g
119
What is the total number of moles contained in 115 grams of C2H5OH
2.50
120
A sample of nitrogen containing 3.0x10^23 molecules has the same number of molecules as a sample of
.50 (Half) Moles of Ne
121
What is the mass of 3.0x10^23 atoms of Neon
10 grams
122
Which sample of O2 contains a total of 3.01x10^23 molecules at STP
16.0 grams
123
The percent bny mass of oxygen in H2C2O4
64
____ x 100
90
124
The empirical (reduced) formula of the compound whose molecular formula is P4O10
P2O5
125
What is an empirical formula?
The most reduced formula
126
A 10 gram sample of a hydrate was heated until all the water of hydration was driven off. The mass of anhydrous product remaining was 8.00 grams. What is the percent of water in the hydrate?
Second number/First Number= T
T - 100 = Answer
20%
127
What is the empirical formula of a compound consisting of 29.6% Oxygen and 70.4% Fluorine by mass
Divide percents by the elements mass then divide the smalled number by all other numbers should equal .0 or .9 if not multiply by (5 3 5 2 5 3 5)
128
A compound contains .5 moles of sodium, .5 moles of Nitrogen, and 1 mole of hydrogen. The empirical formula of the compound is
NaNH2
129
A 16 gram sample of a compound containing only copper and sulfur is decomposed to produce 12.8 grams of copper and 3.2 grams of sulfur. What is the empirical formula of the compounds
Cu2S
130
NaOH + HCl ---> NaCl + H2O
| What is the total number of grams of H2O produced when 116 grams of the product, NaCl is formed?
36g
131
N2(g) + 3H2(g) ---> 2NH3(g)
| What is the total number of liters of NH3 Formed when 20 liters of N2 react completely
40L
132
C8H16 + 12O2 ---> 8CO2 + 8H2O
| How many moles of H2O are produced when 11.2 liters of C8H16 gas measure at STP react completely
4.00
133
In the reaction N2 + 3H2 ---> 2NH3 how many grams of H2 are needed to produce exactly 1 moles of Ammonia
3 gram
134
4Al(s) + 3O2(g) ---> 2Al2O3(s)
| Calculate the gram molecular mass of Al2O3
102 grams
135
4Al(s) + 3O2(g) ---> 2Al2O3(s)
| How many moles of Al are needed for the production of 3.00 moles of Al2O3
6 moles
136
4Al(s) + 3O2(g) ---> 2Al2O3(s)
| Calculate the mass in grams of 3.00 moles of Al2O3
306 grams
137
What is the percent by mass of water present in 1.0 mole of CaSO4 o 2H2O
36
____ = 21%
172
138
What is the total number of grams of KCl (formula mass = 74.6) in 1 liter of .200 moles solution
14.9 grams
139
What is the molarity of a solution of KNO3 (molecular mass = 101) that contains 404 grams of KNO3 in 2.00 liters of solution
2.00 M
140
What is the total number of solute contained in .5 liters of 3.0 M HCl
1.5
141
How many grams of ammonium chloride (gram formula mass = 53.5 g) are contained in .500L of 2.00 liters of solution
53.5 grams
142
How many grams of KI are dissolved in 250 grams of a 20% solution
50 grams
143
A solution will boil at the highest temperature when it contains 1 mole of nonvolatile solute dissolved in
250 grams of solvent
144
When 2.00 moles of sugar (C6H12O6) are dissolved in 1.00 grams of water the boiling point of the resulting solution is closest to
101 C
145
Which solute, when qdded to 1000 grams of water, will produce a solution with the highest boiling point
58 grams of NaCl
146
The heat of reaction (Delta H) is equal to the
Heat content of the products minus the heat content of the reactants
147
Review 126-130 In Packet
SKIP
148
A(g) + B(g) --> C(g)
| As the concentration of A(g) increases, the frequency of collisions of A(g) with B(g)
Increases
149
In a gaseous system, temperature remaining constant, an increase in pressure will
Increase reaction rate
150
In an gaseous system, temperature remaining constant, a decrease in pressure will
Decrease reaction rate
151
As the surface area of the Zn(s) used in the reaction Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g) is increased, the rate of the reaction will
Increase
152
The addition of a catalyst to a reaction will cause a change in the
Activation Energy
153
CAT (Catalyst)--->
ACT (Activation energy)
154
Delta H
```
- = Exo
+ = Endo
```
155
Delta S
```
- = Less Disorder
+ = More Disorder
```
156
Delta G
```
- = Spontaneous
+ = Non Spontaneous
```
157
The pair of changes would indicate that a reaction is endothermic but occurs spontaneously
A positive Delta H and a Negative Delta G
158
A chemical reaction will always occur spontaneously if the reaction has
Negative Delta G
159
BaSO4(s) = Ba+2(aq) + SO4-2(aq)
| As the concentration of the SO4-2(aq) ions increases, at a constant temperature, the concentration of Cl- Ions
Decrease
160
CH3COOH(aq) + H2O(l) = H3O+(aq) + CH3COO-(aq)
| The addition of what ion will cause the decrease in the concentration of CH3COO-(aq)
H3O-
161
N2(g) + 3H2(g) = 2NH3(g) + heat
| Which change favors the formation of ammonia?
Increasing the concentration of N2(g)
162
2SO2(g) + O2(g) = 2SO3(g)
| As the pressure is increased at the constant temperature, the number of moles of SO3(g) produced will
Increase
163
2A(g) + B(g) + 10 kcal = C(g)
| Which condition would yield the most product
High temperature and high pressure
164
What is the equilibrium equation for the reaction 3A(g) + B(g) = 2C
[C]2
----------
[A]3[B]
165
Which of the following is the correct equilibrium expression for
4NH3(g) + 7O2(g) = 4NO2(g) + 6H2O(g)
[NO2]4[H2O]6
----------------------------
[O2]7[NH3]4
166
A + B =AB
| The greatest amount of AB would be produced if the equilibrium constant of the reaction is eqaul to
1.0x10^5
167
AgI(s) = Ag+(aq) + I-(aq)
| Which of the following is the correct solubility product constant expression for the reaction
Ksp = [Ag+][I-]
168
C(s) + CO2(g) + heat ----> 2CO2(g)
| Which stress on the system would favor production of CO(g)
An increase Pressure
169
A2(g) + 3B2(g) = 2AB3(g) + heat
State two stresses that could be applied to this system that would cause this equilibrium to shift to the right. Explain why each stress would cause a shift in the equilibrium
Temperature and Pressure because those can change the state of the substance
170
What is the pH of a solution that has an OH- ion concentration of 1x10^-9 mole per liter (Kw = 1 x 10^-14)
5
171
What is the pH of a .00001 molar HCl solution
5
172
If the OH- equals 1 x 10-10 at 298 k for a given soltuion, the H+ of the solution equals
1 x 10-4
173
What s the H+ ion concentration of an aqueous solution that has a pH of 11
1 x 10-11 mol/L
174
The H3O+ ion concentration of a solution is 1x10-5 mole per liter. This solution is
Acidic and has a pH of 5
175
Which equation represents a neutralization reaction
Any equation with the product of NaCl + H2O
176
What is a neutralization reaction
A reaction resulting in NaCl + H2O
177
If 100 milliliters of .75 M HCl is required to exactly neutralize 50 milliliters of KOH, what is the concentration of the base?
1.5 M
178
If you see exactly neutralized in an equation what do you do?
Multiply the first two numbers you see and then divide it by the last
179
In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:
Write a balance equation for HNO3 and LiOH
HNO3 + LiOH ---> H2O + LiNO3
180
In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:If 50 milliliters of .50 M LiOH is required to exactly neutralize 100 milliliters of an HNO3 solution, what is the molarity of the HNO3 solution?
.25 M
181
In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:What indicator was used in the titration
Moles
182
What color does Phenothaline turn in Acid
Colorless
183
What color does Phenothaline turn in Base
Pink
184
What color does Litmus turn in Acid
Red
185
What color does Litmus turn in Base
Blue
186
Arrhenius Acid
Gives H+
187
Arrhenius Base
Gives OH-
188
Bronsted Lowry Acid
Gives H+ (Proton)
189
Bronsted Lowry Base
Accepts H+ )Proton
190
Lewis Acid
e- pair Acceptor
191
Lewis Base
e- pair Donor
192
How do you know what the Bronsted Lowry Bases are
Compare the two similar elements on each side and the one with the less H's is the base
193
In a redox reaction there is conservation of
Both mass and charge (everything)
194
Review 161 and 162 In Packet
SKIP
195
How do you know which substance is being oxidized?
Pick the first element in the equation or the metal
196
How do you know a reaction is redox
Look for a single element and not compounds
197
If there is no metal in the equation how do you know what was oxidized?
Look for an increase in ions
198
0
e-
-1
Beta
199
4
He
2
Alpha
200
0
e-
1
Positron
201
0
V
0
Gamma
202
1
Beta
203
2
Gamma
204
3
Positron and Alpha
205
To solve a Nuclear Problem what do you do?
Equal Everything
206
What is the equation for Decay
TGB
------- = Decay
HL
207
At the end of 12 days 1/4 of an original sample of a radioactive element remains. What is the half life of the element
6 Days
208
An Original Sample of a radioisotope has a mass of 10 grams. After 2 days, 5 grams of the radioisotope remains unchanged. What is the half life of the radioisotope
2 Days
209
In 6.20 Hours a 100 gram sample of Ag-112 decays to 25 grams. What is the half life of Ag-112
3.10 Hours
210
The half life of carbon-14 is 5730 years. What fraction of a 1 gram sample of carbon-14 would remain after 17190 years?
1/8
211
```
Which quantity expresses the sum of the values below to the proper degree of precision
2.1
33.566
+12.22
--------------
```
47.9g
212
Using the rules for sig fig, the sum of .027g and .0023 grams should be expressed
.029
213
What is the product of (2.324 cm x 1.11 cm) expressed to the correct sig fig
2.58 cm2
214
During a titration, a student used 50 milliliters of .1 M acid. How many moles of acid, expressed to proper significance, were used?
.005
215
What is the number 215 expressed in proper scientific notation with the correct number of sig fig,
2.150 x 102
216
A student investigated the physical and chemical properties of a sample of an unknown gas ans then identified the gas. Which of the following statements represents a conclusion rather than an experimental observation
The gas is carbon dioxide
217
What is the number 2.1 x 10^3 expressed in conventional form with the proper number of sig fig
2100
218
The solid block shows below has a mass of 146 and a length and width of 3 and a height of 6 what is the density
2.7
219
The process of filtration is preformed in the laboratory to
Separate insoluble substances in an aqueous mixture
220
Linear CH4
CO2
221
Tetrahedral
CH4
222
Bent
H2O
223
Trigonal Pyramidal
NH3
224
NP
LDF
225
P
DD
226
Equation for moles
Moles
--------------
C
227
Equation for Grams
G
------------
C (mass)
228
Equation for Liters
L
--------------
C (22.4)
229
Equation for Molecules
Molecules
------------------
C (6.02x10^23)
230
When in Doubt
PV=nRT
231
What is another equation for Grams
gRT
---------
LP
232
What is another equation for Density
DRT
---------
P
