Chemistry for Engineers Flashcards
1
Q
Empirical Formula of the human DNA
A
C39H50O22N15P3
2
Q
Most suitable in creating the most effective bulletproof vest
A
Polyethylene Fiber (Ultra High Molecular Weight Polyethylene, UHMWP)
3
Q
Common material of construction for radiation protection
A
plexiglass
4
Q
Production of plexiglass
A
polymethacrylate fiber
5
Q
for bulletproof windows
A
polycarbonate fiber
6
Q
previous answer for a bulletproof vest
A
polyamide fiber (Kevlar)
7
Q
relationship of boiling point to atmospheric pressure
A
directly proportional
(high BP, high Patm)
8
Q
relationship of atmospheric pressure to elevation
A
inversely proportional
(high Patm, low elevation)
9
Q
relationship of cooking time to boiling point
A
inversely proportional
(low cooking time, high BP)
10
Q
relationship of cooking time to elevation
A
directly proportional
(low cooking time, low elevation)
11
Q
The pressure that a gas will exert in a container assuming it was alone
A
partial pressure
12
Q
laughing gas
A
N2O (nitrous/ nitrogen oxide)
13
Q
Cleveite
A
UO2 (Uranium dioxide)
14
Q
nitroglycerin
A
C3H5N3O9
15
Q
chlorophyll
A
C55H72MgN4O5
16
Q
Baking soda
A
NaHCO3 (sodium bicarbonate)
17
Q
It denotes the relative amount of bonds formed between the atoms of a molecule
A
Empirical Formula
18
Q
It denotes the actual number of each atom in a molecule
A
Molecular Formula
19
Q
Balancing redox reactions:
If the medium is acidic, __ is used to balance O
A
H2O(l)
20
Q
Balancing redox reactions:
If the medium is acidic, __ is used to balance H
A
H+
21
Q
Balancing redox reactions:
If the medium is a base, __ is used to balance O
A
OH-
22
Q
Balancing redox reactions:
If the medium is a base, __ is used to balance H
A
H2O
23
Q
Matter cannot be created nor destroyed but only change from one form into another
A
Law of Conservation of Mass
24
Q
Law of Conservation of Mass by
A
Antoine Lavoisier
25
Regardless of the extensive amount, the percent content of an atom in a molecule must remain constant
Law of Definite Composition
26
Law of Definite Composition by
Joseph Louis Proust
27
Atoms have the tendency to bond with one another into appreciable whole number integers, each one being a distinct species.
Law of Multiple Proportions
28
Law of Multiple Proportions by
John Dalton
29
discovered by Joseph John Thomson
electron
30
The term electron is coined by
George Stoney
31
Model used by JJ Thomson
Plum Pudding Model
32
the charge/mass ratio of an electron was determined through __ by JJ Thomson
Cathode Ray Experiment
33
Oil Drop experiment was conducted by __. He precisely determined the magnitude of the electron's charge for about 5 significant figures.
Robert Millikan
34
Discovered proton
Ernest Rutherford
35
Ernest Rutherford's experiment
Geiger-Marsden Experiment (Gold Foil Experiment)
36
Model used by Ernest Rutherford. (electrons are randomly scattered)
Atomic Model
37
Discovered neutron
James Chadwick
38
___ is the model where electrons are revolving around the nucleus by ___
Bohr Model; Niels Bohr
39
Platinichloride Salt formula
B2H2PtCl6
(B = sample)
40
Chloroplatinic Acid
H2PtCl6
41
Commonly used in identifying the molecular mass (actual mass) of a compound
Platinichloride Method
42
Ratio of a sample to chloroplatinic acid
2:1
43
He proposed that Energy, like matter, is discontinuous (Quantum Theory)
Max Planck
44
First spectroscopy (they discovered two alkali metals, cesium and rubidium, with the aid of the spectroscope they had invented the year before)
Robert Bunsen and Gustav Kirchhoff
45
Color of Caesium (Latin: Caesius)
sky blue
46
color of rubidium (Latin: Rubidius)
deep red
47
Greek: Helios, which means ___
Helium; the Sun
48
It places no limitation (infinite) on the amount of energy
Classical Physics
49
A system may only possess a finite (limited), discrete (absolute) amount of energy
Quantum Theory
50
the smallest discrete unit of a phenomenon
quanta
51
TRUE OR FALSE:
The energy of a quantum of electromagnetic radiation is proportional to the frequency of the radiation
TRUE
52
Planck's Equation
E = hf = hc/λ
53
phenomenon in which electrically charged particles are released from or within a material when it absorbs electromagnetic radiation. The effect is often defined as the ejection of electrons from a metal plate when light falls on it.
Photoelectric effect
54
Photoelectric effect was discovered by
Heinrich Hertz
55
Light particle conceived by Einstein
photon
56
ejected electron in the photoelectric effect
photoelectrons
57
Energy that binds an electron to a metal surface. It is constant for every particular metal.
Work Function
58
light can behave as a wave or as a particle (photon)
Wave-Particle Duality
(Albert Einstein)
59
The minimum frequency that a light must possess in order to initiate the photoelectric effect
threshold frequency, fo
60
the energy of an object because of its motion
kinetic energy (KE = 1/2 mv^2)
61
De Broglie's Wavelength
λ = h/mv
62
fl < fo
no photoelectric effect
E < WF + KE
WF = work function
KE = kinetic energy
63
fl = fo
photoelectric effect, but Ve = 0
E = WF; KE = 0
WF = work function
KE = kinetic energy
64
fl > fo
photoelectric effect (electrons are moving away)
E > WF + KE
Ve > 0
WF = work function
KE = kinetic energy
65
fl > fo
photoelectric effect (electrons are moving away)
E > WF + KE
Ve > 0
WF = work function
KE = kinetic energy
66
Cumulative energy that each particle of a system possesses
internal energy
67
examples of internal energy
translational
rotational
vibrational
68
How many water molecules can attach to methanol via hydrogen bonding?
3
69
TRUE OR FALSE:
Heat and work can be conserved in a system by distributing it evenly amongst the systems constituents.
False
70
Energies in transit; Exists only as energy being transferred between 2 bodies/ systems
heat (Q) and work (W)
71
TRUE OR FALSE:
delta U being equal to the summation of heat and work is an interpretation of the First Law of Thermodynamics
True
72
TRUE OR FALSE:
delta H can be interpreted as the heat transferred under constant volume conditions.
False
73
Bonds that occur between atoms to form a compound
Intramolecular forces
74
Examples of intramolecular forces
ionic bond
covalent bond
metallic bond
75
TRUE OR FALSE:
Intramolecular forces need high temperature to break the bond
True
76
The minimum temperature to break intramolecular forces is __, while for intermolecular forces is ___.
600°C; 100°C
77
transfer of electrons between metals and non-metals
Ionic bond
78
sharing of electrons (non-metals)
Covalent Bond
79
Metal atoms lose their outermost electron to form positively charged ions (metals)
Metallic bond
80
TRUE OR FALSE:
Intramolecular forces are weaker than intermolecular forces
FALSE
81
Bonds that occur between molecules, identical or not.
Intermolecular Forces
82
Examples of intermolecular forces
Van der Waals Forces
Dipole-dipole forces
Hydrogen bonding
83
Weakest intermolecular force. Its relative strength depends on the molecules' polarizability
Van der Waals forces
84
TRUE OR FALSE:
Van der Waals forces occur in every compound/ molecule
True
85
Van der Waals is also known as
dispersion forces
london forces
instantaneous-induced dipole interaction
86
Rearranging of atoms to form partial positive and partial negative.
The tendency of molecules to generate induced electric dipole moments when subjected to an electric field
polarizability
87
An intermolecular force stronger than the Van der Waals forces.
It is defined as the alignment of partial positive pole of a polar molecule to the partial negative pole of a different polar molecule
Dipole-dipole forces
88
TRUE OR FALSE:
Dipole-dipole forces only occur between polar molecules.
TRUE
89
Pulls/ attracts electrons within its vicinity;
Produces partial positive and partial negative
electronegative atoms
90
The strongest intermolecular force
Hydrogen Bonding (not exclusive to H2O)
91
Requirements of Hydrogen Bonding
(a) one molecule must have an H atom covalently bonded to an electronegative atom (ex. O, N, F)
(b) the other molecule must have a LONE PAIR in its electronegative atom (ex. O, N, F)
92
TRUE OR FALSE:
Hydrogen bonding can occur between two molecules which can be identical or not.
TRUE
93
Relationship of Polarizability to atomic radius (AR)
directly proportional
(high AR, high polarizability)
94
Periodic Table trend for increasing atomic radius
right to left, top to bottom
95
Relationship of Polarizability to molecular weight (MW)
directly proportional
(high MW, high polarizability)
96
TRUE OR FALSE:
The molecular weight is not directly involved in the phenomena of polarizability. It simply follows the same trend as the atomic radius
TRUE
97
Properties rel. to polarizability
↑ polarizability:
↑ boiling pt
↑ melting pt
↑ surface tension
↑ viscosity
↓ vapor pressure
98
occurs on the molecules on the surface of a liquid due to the unbalanced distribution of forces
Surface tension
99
friction to flow
viscosity
100
pressure induced by vapor
vapor pressure
101
A thermodynamic property that measures the various ways in which a systems' energy can be distributed among its components
Entropy
102
He discovered entropy and explained its behavior.
Rudolf Clausius
103
He defined entropy 27 years after its discovery
Ludwig Boltzmann
104
High energy
↑ microstate
↑ S
↑ mobility
↑ # of energy levels
105
It increases the entropy of the universe (ex. boiling of water L→V)
Spontaneous process
106
Common processes that increase the entropy
1 increasing the temperature
2 phase transitions: S→L, S→G, L→V
3 dissolution of a solute in a solvent
4 amount of gaseous species increases after a chemical reaction
5 mixing gases
107
TRUE OR FALSE
Increasing the temperature increases the total energy
TRUE
108
TRUE OR FALSE
In phase transitions, the intermolecular forces weakens providing more mobility.
TRUE
109
A spontaneous process causes an increase in the entropy of the universe
Second Law of Thermodynamics
110
The process involves the addition of infinitesimal amounts of heat to a system that causes incremental changes in its properties
reversible
111
Criterion for spontaneity:
ΔSuniv < 0
ΔGsys > 0
non-spontaneous
112
Criterion for spontaneity:
ΔSuniv = 0
ΔGsys = 0
reversible, equilibrium
113
Criterion for spontaneity:
ΔSuniv > 0
ΔGsys < 0
spontaneous
114
TRUE OR FALSE
A process wherein two ideal gases in separate bulbs, both at a pressure of 1 bar, are connected and allowed to expand into the total volume, exhibits a positive change in entropy
TRUE
115
Which among the following relationships fully encapsulates the idea of the Second Law of Thermodynamics
A: delta S_system < 0
B: delta S_universe > delta S_system +
delta S_surrounding
C: delta S_universe > 0
D: delta S_system
C: delta S_universe > 0
116
A measure for the maximum available energy for non-PV work
Gibbs Free energy
117
Properties of a solution that depends only on the concentration of the solute
Colligative properties
118
Common Kb and Kf values:
H2O
Kb = 0.512 °C/m
Kf = 1.858 °C/m
119
Common Kb and Kf values:
Benzene (C6H6)
Kb = 2.61°C/m
Kf = 5.065 °C/m
120
Common Kb and Kf values:
Camphor (C10H16O)
Kf = 40 °C/m
121
Common Kb and Kf values:
Ethanol (C2H5OH)
Kb = 1.07 °C/m
122
___ is a phenomena of solvent flow through a semipermeable membrane (from dilute → concentrated) to equalize the concentration on both sides. It is dictated by the ____. (The solvent provides mobility for the concentrated side.)
Osmosis; Second Law of Thermodynamics
123
The amount of pressure necessary to impede the phenomena of osmosis
osmotic pressure
124
Formula for osmotic pressure
ℼ = MRT
ℼ → osmotic pressure
M → molarity (mol/L)
R → ideal gas constant
T → absolute temperature
125
Colligative properties
Vapor pressure lowering
Boiling point elevation
Freezing point depression
Osmotic pressure
126
Kb
ebullioscopic constant of a solvent
127
Kf
cryoscopic constant of a solvent
128
Boiling point elevation formula
ΔTb = mKb
m → molality of the solute (mol solute/ kg solvent)
Kb → ebullioscopic constant
129
Freezing point depression formula
ΔTf = mKf
m → molality of the solute (mol solute/ kg solvent)
Kf → cryoscopic constant
130
Vapor pressure lowering formula
ΔP = XsoluteP°solvent
P°solvent → pure vapor pressure of solvent
Xsolute → mole fraction of solute
131
He discovered the noble gases
William Ramsay
132
William Ramsay along with Lord Rayleigh discovered __
Argon
133
Which among the following is the
third gas that William Ramsay isolated
with Morris Travers?
A: Argon B: Neon
C: Krypton D: Xenon
D. Xenon
134
How many carbon atoms are there in one molecule of “buckyball”?
60
135
Ramsay discovered ___ from an ore of uranium (cleveite)
Helium
136
Ramsay alongside Morris Travers discovered ____________ by liquefying air and further distillation (fractional).
Neon → Krypton → Xenon
137
Ramsay working along with Frederick Soddy discovered ___, short for ___.
Radon; Radium Emanation
138
The emission of ionizing radiation by some of the heavier elements to become stable.
Radioactivity
139
"Radioactive" means
unstable
140
Which among the following scientists discovered radioactivity?
A: Marie Curie
B: Henri Becquerel
C: Otto Hahn
D: Ernest Rutherford
B: Henri Becquerel
141
___ particles have the lowest penetration, while ___ particles have the highest.
alpha; gamma
142
Alpha particles have the _____ biological destruction, while gamma particles have the ____.
highest; lowest
143
Which among the following is affected by magnetic/ electric field?
I. Alpha particle
II. Beta particle
III. Gamma particle
A. I only
B. II only
C. I, II and III
D. I and II
D. I and II
144
Discovered Polonium and Radium.
Explained the phenomena of radiation
Marie Curie
145
Father of Nuclear Chemistry
Otto Hahn
146
Nuclear fission is from ____ to ____, while nuclear fusion is from ____ to ____.
heavier, lighter;
lighter, heavier
147
Transmutation by___, the nuclei of an atom will undergo transformation when bombarded with a nuclear species.
Ernest Rutherford
148
The first artificial transmutation. _____ into _____ using ____ particles.
N14 --> O17
alpha particles
149
Synthesized the first synthetic transmuted atom
Irene Joliot Curie
150
The synthetic transmuted atom by Irene Joliot Curie
P30
151
The number of protons and neutrons in a nuclide that dictate stability
Magic numbers
152
Magic numbers of a proton
2
8
20
28
50
82
153
Magic numbers of a neutron
2
8
20
28
50
82
126
154
uses phosphor
detects presence of light
Scintillation counter
155
produces light when it interacts with radioactive substance
phosphor
156
quantifying the magnitude
Geiger counter
157
In which among the following can a Cherenkov Radiation be observed?
A: In the Water surrounding the core of a Nuclear Reactor
B: In the Mushroom Cloud produced after a Hydrogen Bomb Explosion
C: In a particle accelerator after the bombardment of two nuclides
D: In the Sun’s Corona during a Solar Eclipse
A: In the Water surrounding the core of a Nuclear Reactor
158
Across the three most notorious accidents regarding nuclear power plants: Three Mile Island, Chernobyl, and Fukushima, what is the most common cause for their failure that led to
several environmental problems?
A: A leak in the fuel rods initiating an explosion
B: Bursting of reactor due to uncontrolled pressurized steam
C: Loss of proper cooling and/or moderator
D: Run-off chain reactions of the fissile material
C: Loss of proper cooling and/or moderator
159
Radiocarbon dating formula
ln(No/N) = kt
160
half-life formula
t1/2 = ln2/k
161
half-life of C-14
5730 years
162
No of C-14
15.3 disintegrations of C14 per minute per gram of C12
163
1 Ci (Curie) = ____ Bq (Becquerel)
3.7 x 10^10
164
1 Ci (Curie) = _____ disentegration/s
3.7x10^10
165
1 Bq = ____ disintegrations/ decay per second (dps)
1
166
The amount of a substance that disintegrate per unit time
Activity
167
The amount of radiation that deposits 0.01J of energy per kg of matter
rad
168
What is the meaning of rad?
radiation absorbed dose
169
1 rad = ____ Gray (Gy)
0.01
170
Relates various kinds of radiation based on their biological destruction
rem
171
What is the meaning of rem?
roentgen equivalent man
172
Formula for rem
rad x Q
173
Relative Biological Effectiveness of:
X-ray, Y-ray and Beta particles
Q = 1
174
Relative Biological Effectiveness of:
slow neutrons
Q = 3
175
Relative Biological Effectiveness of:
fast neutrons, protons
Q = 10
176
Relative Biological Effectiveness of:
alpha particles
Q = 20
