Final 1-14 & 16 Flashcards
(222 cards)
1
Q
The general formula for carboxylic acid
A
RCOOH
2
Q
Phosphorous-30 decays by positron emission. The product is
A
Silicon - 30
30 30 0
P –> Si + e-
15 14. +1
3
Q
An ionic bond is formed when electrons are
A
Transferred
4
Q
An electron-dot structure is a convenient method of representing
A
Valence electrons of an atom
5
Q
Copper is played on zinc by immersing a piece of zinc into a solution containing copper (ll) ions. In the plating reaction, copper (ll) ions
A) lose two electrons and are oxidized
B) lose two electrons and are reduces
C) gain two electrons and are reduced
D) gain two electrons and are oxidized
A
Gain two electrons and are reduced
6
Q
The formula of iron (ll) phosphate is
A
Fe3(PO4)2
7
Q
Hydrogen gas converts tungsten oxide to tungsten metal. Hydrogen (H2) is a(n)
A) reducing agent
B) base
C) oxidizing agent
D) acid
A
Reducing agent
8
Q
Which of the following processes involved the removal of energy (heat)?
A) sublimation
B) melting
C) condensation
D) vaporization
A
Condensation
9
Q
Which type of radioactive emission is very similar to x-rays
A) gamma ray
B) transmutation
C) beta particle
D) alpha particle
A
Gamma ray
10
Q
Which of the following metals does the U.S. Import from other countries
A) Sn
B) Cr
C) Pt
D) all of the above
A
D) all above
11
Q
Which of these is a chemical change
A) bleaching powder dissolves in water
B) silkworms convert mulberry leaves into silk
C) wool is spun into yarn
D) the hair stylist curls your hair
A
Silkworms convert mulberry leaves into silk
12
Q
A piece of fossilized wood has a carbon-14 radioactivity that is 1/4 that of a new wood. The half-life of carbon-14 is 5730 years. His old is the fossilized wood?
A
2 x 5730 = 11,460
13
Q
The polymer segment ~CH2CH2CH2CH2CH2CH2CH2~ represents
A) polyethylene
B) polystyrene
C) polypropylene
D) polyvinyl chloride
A
A) polyethylene
14
Q
Fuels are ____ forms of matter
A
Reduced
15
Q
Which of these common human activities contribute to BOD
A) paddling a boat across a lake or pond
B) fishing in a lake or pond
C) swimming in a lake or pond
D) dumping lawn clippings in a lake or pond
A
Dumping lawn clippings in a lake or pond
16
Q
When the equation below is balanced, the coefficient of sulfuric acid, H2SO4 is
(NaCN + H3SO4 –> Na2SO4 + HCN)
A
1
17
Q
Alkane a are often called
A
Saturated hydrocarbons
18
Q
The reaction between a carboxylic acid and an anime yields a(n)
A
Amide
19
Q
A sample of rainwater has a pH of 3.5. What ion is sure to be present in relatively large concentration in this rain sample
A
H3O+
20
Q
The word polymer means many
A
Parts
21
Q
In the late stages of extended starvation or fast, the body uses what as a source of energy?
A
Protein
22
Q
CO3 ALWAYS contains 3g of C for every 8g of O. This is an example of
A
Proust’s Law of Definite Proportions
23
Q
Foods that are acidic can be identified by their _______ taste.
A
Sour
24
Q
Fat soluble vitamins are stores..
A
In the body
25
Molarity is a measure of
The concentration of a solute in a solution
26
A horizontal row in the modern periodic table is called a
Period
27
A vertical row in the modern periodic table is called
A group
28
Which substance has polar covalent bonds?
A) O2
B) Cl2
C) Ca2C
D) NH3
NH3
29
Which physical state has the highest entropy
A) solid
B) gas
C) liquid
D) all have the same entropy
Gas
30
Another name for the first law of thermodynamics is
The law of conservation of energy
31
In the reaction CH4 + 2O2 --> CO2 + 2H2O how many miles of oxygen are required to burn 8.0 g of methane?
1
32
The valence she'll electron pair repulsion theory (VSEPR) is used to
Predict the three dimensional structure of molecules
33
In terms of composition, 9 elements compose approximately what % of the earth's crust
> 95%
34
One difference between a chemical reaction and a nuclear reaction is that in a nuclear reaction
Atoms often change from one element to another
35
The production of biomass as an energy source is an example of the conversion of
Solar energy to chemical energy
36
Molasses is a byproduct of the refining of sugar from sugar cane. The specific composition molasses varies depending upon the source of the sugar cane. Which one of the following is the best classification of molasses?
A) element
B) mixture
C) compound
D) pure substance
Mixture
37
Which sets of compounds illustrates the law of multiple proportions
A) NH3, NF3, NCl3
B) NH3, PH3, AsH3
C) NH3, N2H4
D) all the above
NH3, N2H4
38
Which part of the water supply is most isolated from the purifying capacity of the water cycle
Groundwater
39
In the balanced chemical equation for the neutralization of calcium hydroxide with nitric acid, HN03, the coefficient of nitric acid is
2
40
The element tin (Sn) occurs naturally as 10 isotopes. Each of these isotopes has
A) a different number of neutrons
B) 50 protons
C) 50 electrons
D) all above
All above
41
Saturated fat's have
Primarily C-C (single) bonds
42
The presence of nitrogen dioxide and smog is most easily recognized by
Color
43
And a reaction, the substance undergoing reduction serves as the _____ agent
Oxidizing agents
44
The following nuclear reaction is an example of
226 4 222
Ra--> He + Rn
88 2 86
A) beta decay
B) alpha decay
C) gamma decay
D) an impossible reaction
Alpha decay
45
Many materials can be recycled, but some can also be reused. Which of the following statements about returnable glass beverage bottles is not correct
A) it takes more energy to make a returnable bottles then to make a non-returnable bottle
B). It takes less energy to make a returnable bottle of then to make it non-returnable bottle
C) it takes more energy to recycle a glass bottle than to reuse it
D) there are energy costs associated with collecting and refilling a returnable bottle
It takes less energy to make a return of the bottle than to make a non-returnable bottles
46
A student working in the lab needs 200 g of a liquid chemical who's density is .69 g/cm cubed. What volume of this liquid should be the measure
A) 200 cm cubed
B) 290 cm cubed
C) 69 cm cubed
D) 138 cm cubed
290 cm cubed
47
How many milligrams are in .010 mg?
A) 10 nanograms
48
Ammonia is classified as a weak base in water. This means that it produces
I relatively small fraction of the maximum number of hydroxide ions
49
Assume that you have a sample of gas. You know the volume, the temperature and the number of moles of the sample. Which of the following laws would you use if you wanted to calculate the pressure of the sample?
A) ideal gas law
B) Charles law
C) Boyles law
D) law of combining volumes
Ideal gas law
50
Which of the following does not contribute to acid rain
A) volcanic eruptions
B) lightning
C) coal-burning power plants
D) none--all above contribute
None--all above contribute
51
The element with the ground state electron configuration of 1s2 2s2 2p6 3s2 3p5 is
Cl
52
Ether
ROR'
53
Esther
RCOOR'
54
Carboxylic acid
RCOOH
55
Alcohol
ROH
56
Aldehyde
R-C=O
|
H
57
Ketone
O
||
R-C-R
58
Amine
Replace H with NH3
59
Amide
```
O
||
-C-N-
|
O
```
60
Alpha
4
He
2
61
Beta
O
e-
-1
62
Gamma
X-Ray
63
Sublimation
Directly solid to gas
64
Backbone of majority of chains
Polyethylene
65
Polystyrene
Benzene rings
66
Polypropylene
3 C before repeating
67
Hydrocarbons latch onto
Oxygen
68
Dalton's law of multiple proportions
2 diff. Compounds
69
Dalton's atomic theory
Everything has atoms
70
Lavoisier's Law of Conservation of Mass
Reaction
71
How to determine polar covalent
2 non metals and not diatomic
72
Polar =
Different
73
> or equal to 2 compounds =
Mixture
74
Just 1 compound =
Compound
75
Element or compound =
Pure substance
76
Are alkanes saturated or unsaturated
Saturated
77
Data summarized by statement
Law
78
Work oriented toward the solution any particular problem in industry of the environment
Applied
79
The search for knowledge for its own sake
Basic
80
Desirability quotient =
Benefit/risk
81
Mass + volume =
Matter
82
Measure of quantity of matter
Mass
83
Measures a force; varies with gravity unlike mass
Weight
84
Set shape and volume
Solid
85
Shape changes and set volume
Liquid
86
Shape and volume change
Gas
87
Characteristics of a substance
Physician properties
88
Alteration of physical appearance without changing chemical identity of compositions
Physical changes
89
How one substance reacts with another
Chemical property
90
Substance changes into something new
Chemical change
91
____ is required to make something happen that wouldn't happen by itself
Energy
92
Fundamental building blocks of all material that retain individual characteristics
Elements
93
Definite + fixed components + set properties =
Pure substance
94
2 or more elements in a fixed ratio
Compound
95
Do mixtures have variable proportions
Yes
96
Homogeneous =
Uniform "look like one thingy"
97
Heterogenous
Separated into parts (oil & water)
98
Joule =
SI unit of energy
99
Heat required to raise 1g H20 1 degree
Calorie
100
Kelvin =
C + 273
101
Measure of the amount of energy
Heat
102
Measure of how much energy a particle has
Temperature
103
Mass per unit volume
Density
104
Can you see atoms
No
105
Metals that carry current
Electrode
106
Compounds that conduct electricity
Electrolyte
107
Charged atoms or group of atoms
Ions
108
Atoms of an element can have different masses
Isotopes
109
Hyphen method
C-12
110
Nuclear symbol
12
C
6
111
Bohr Model
1st shell
2e-
112
Bohr Model
2nd shell
8e-
113
Bohr Model
3rd shell
18 e-
114
Unstable nuclei =
Radioactive decay
115
Positron emission
0
e-
+1
116
Electron capture
11
B
5
Nucleus absorbs electron from inner shell
117
The period of time equites for 1/2 the original # of atoms to decay to a new element
Half-life
118
Elements + conpounds
Pure substance
119
Forces that hold atoms together in molecules & ions together in ionic compounds
Chemical bonds
120
T/F: when 2 elements combine to form a compound they keep their same properties
False! They don't keep their original properties. They turn into a completely new substance with new properties
121
Octet =
8 valence e-
122
Outer most e-
Valence e-
123
For main group elements the # of valence e- correlates with the ____ the element is in
Group
124
Same electron configuration as a noble gas structure
Isoelectronic
125
Ionic bond
Metal + nonmetal
| Compound
126
A group of covalent it bonded atoms that lost or gained e- in order to obey the octet rule
Polyatomic atoms
127
Polar =
Unequally, partial shared (dipole)
128
Nonpolar =
Equal & no difference in electronegativity (diatomic)
129
Sometimes there's more than one way to draw a Lewis structure
Resonance
130
VSEPR
2 groups =
Linear shape
131
VSEPR
3 groups =
Triangular
132
VSEPR
4 groups
Tetrahedral shape
133
When energy is absorbed to overcome forces holding tight
Melting point
134
When energy is absorbed to overcome attractive forces
Vaporization
135
Intermolecular
Between compounds
136
Intramolecular
Inside compound
137
Dipole =
Weaker than ionic forces/polar molecules
138
Hydrogen bonding
O, N, F
139
Weakest intermolecular forces
Dispersion
140
Generally the strongest of the forces that hold solids &a liquids together
Ionic interactions
141
Number of atoms or molecules in one mol
Avagadro's number
142
How much 1 mole of a substance weighs
Molar mass
143
1 mole of any volume =
22.4 L
144
* constant motion
* small compared to distance
* little attraction between molecules
* elastic collisions
* Temperature is a measure of the average ___________ of gas particles
Kinetic molecular theory
145
Coefficients correspond to _______
Volume
146
Describes has behavior. Relate volume, temperature, & pressure
Gas Laws/Equations
147
****ALWAYS CONVERT TEMPERATURES TO _______ FIRST!!****
Kelvin
148
V1/T1 = V2/T2
Charles Law
149
P1V1 = P2V2
Boyle's Law
150
PV = NRT
```
P=pressure (atm = 0.0821) (kpa = 8.314)
V=volume
N=moles
R=constant based on pressure
T=temperatures
```
Ideal gas law
151
Solute
Dissolvee
152
Solvent
Dissolver
153
Molarity =
Mol/L
154
% by volume =
Volume of solute/volume of solution x 100%
155
% by mass =
Mass of solute/mass of solution x 100%
156
Properties of acid (4)
* sour taste
* red on litmus paper
* dissolve active metals = H2
* react with base = salt & water
157
Properties of base (4)
* bitter taste
* blue on litmus paper
* slippery
* react with acid = salt & water
158
Neutral substances that change certain colors with acids and bases
Indicators
159
Arrhenius Theory:
Molecular substances that breaks up an aqueous solution into H+ & anions(ionize)
Acids
160
Arrhenius Theory:
Release hydroxide in an aqueous solution
Bases
161
Problems with Arrhenius theory (3)
* H+ won't exist in H2O
* doesn't explain why ammonia is a base
* only applies to aqueous solutions
162
Bronsted-Lowry Theory
Proton donor
Acid
163
Bronsted-Lowry Theory
Proton acceptor
Base
164
Substance can be acid or base
Amphiprotic
165
Anhydrides:
| Acid =
Nonmetal oxide + H2O
166
Anhydrides:
| Base =
Metal oxide + H2O
167
Strong vs. Weak:
| Strong _______ ionizes in water (________ breaks into ions)
Completely
168
Strong vs. Weak
| Weak
Mostly insoluble
169
T/F: neutralization = acid + base --> salt + water
True
170
A lab technique used for analyzing unknown solutions. Works with acids & bases because they neutralize each other
Titrations
171
Equation for pH
pH = -log [H3O+]
172
Electrochemistry
Cells and batteries
173
E- transferred from one substance to anther producing electricity
Redox
174
2 components -- electrodes -- anode to cathode flow
Electrochemical cell
175
Anode = (oxidized/reduced)
Oxidized
176
Cathode = (oxidized/reduced)
Reduced
177
Series of electrochemical cell
Battery
178
When battery supplies electricity
Discharge
179
Car moving & electric current reapplied to battery
Charge
180
1) takes organic fuel & oxidizes @ anode & oxygen reduced @ cathode
2) most use hydrogen as fuel source
3) 70% efficient
Fuel cells
181
Metal starts deteriorating
Corrosion
182
Rusting of iron
Fe(OH)3
183
More reactive than iron, but hold up better because it forms a layer of ________ oxide for protection
Aluminum
184
Most common oxidizing agent
Oxygen
185
Are oxidizing agents or reaction clean??
Oxidized AGENTS
186
4 properties of reducing AGENTS
* colorless
* odorless
* light density
* explosive
187
What is a catalyst
Speeds up reactions
188
Oxidation and reduction in Photsynthesis
Oxidation of H2O to O2
| Reduction of CO2 to glucose
189
Chemistry of Carbon containing compounds
Organic chemistry
190
Carbon atom must make ___ bonds
4
191
Simplest organic compounds. Contain only Carbon & hydrocarbon
Saturated hydrocarbons
192
```
Meth:
Eth:
Prop:
But:
Pent:
Hex:
Hept:
Oct:
Non:
Dec:
```
1,2,3,4,5,6,7,8,9,10
193
Equation for alkanes
CnH2n + 2
N = # carbons
194
Carbon can connect to form closed rings
Cyclic hydrocarbons
195
2 kinds of Unsaturated hydrocarbons
Alkene
| Alkyne
196
Unsaturated hydrocarbons:
Contain more than or equal to 1 C=C double bond
Alkene
197
Formula for alkene
CnH2n
198
Unsaturated hydrocarbons:
Contain more than or equal to 1 Triple bond
Alkyne
199
Formula for alkyne
CnH2n-2
200
Additions reactions add to break
Multiple bonds
201
Contain a benzene ring or similar properties to benzene
Aromatics
202
Hybrid bonds - in between bonds (C6H6)
Benzene
203
Chlorinated hydrocarbon
Add less than or equal to 4 Cl to chain
204
Chlorofluorocarbons (CFC) contain
Cl & F
205
Multifunctional alcohols
Can contain > 1 OH group
206
Heterocyclic organic compounds
Contain elements other than C in ring
207
Alkaloids = acidic or basic
Basic
208
3 layers of atmosphere from closest to farthest away from earth
1. Troposphere
2. Stratosphere
3. Mesosphere & thermosphere
209
Components of dry air
N = 78%
O = 21%
Ar & CO2
210
3 types of N2 fixations
• bacteria legumes
• lightning
• industrially
*complete by microbes
211
O2 cycle (2)
1. Green plants & phytoplankton
| 2. 3O2 + energy (UV light) --> 2O3 (stratosphere)
212
Temperature inversions =
Warm air trapped over cold air
213
4 types natural pollution
Volcanoes
Dust storms
Wildfires
Swamps/marshes
214
Too much of any substance in the wrong place or @ wrong time
Pollutants
215
Types of smog
Industrial (London)
| Photochemical (L.A.)
216
Industrial (London) smog:
SO2 from coal
Coal + O2 --> CO2 + CO
soot + CO
particulate matter
217
Solid & liquid particles of greater than molecular size (PM2.5)
Particulate matter
218
Prevent industrial smog (5)
```
Electrostatic precipitators
Filter
Cyclone separation
Wet scrubbers
SO2 from coal = problem
```
219
Stack gases spiral up, particles settle bottom
Cyclone separations
220
Formula for photochemical smog
Hydrocarbons + nitrogen
221
Reduce hydrocarbons & CO emission in car exhaust
Catalytic converters
222
Acid rain
pH
