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DAY 1 > Chemistry for Engineers > Flashcards

Chemistry for Engineers Flashcards

1
Q

Empirical Formula of the human DNA

A

C39H50O22N15P3

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2
Q

Most suitable in creating the most effective bulletproof vest

A

Polyethylene Fiber (Ultra High Molecular Weight Polyethylene, UHMWP)

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3
Q

Common material of construction for radiation protection

A

plexiglass

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4
Q

Production of plexiglass

A

polymethacrylate fiber

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5
Q

for bulletproof windows

A

polycarbonate fiber

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6
Q

previous answer for a bulletproof vest

A

polyamide fiber (Kevlar)

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7
Q

relationship of boiling point to atmospheric pressure

A

directly proportional
(high BP, high Patm)

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8
Q

relationship of atmospheric pressure to elevation

A

inversely proportional
(high Patm, low elevation)

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9
Q

relationship of cooking time to boiling point

A

inversely proportional
(low cooking time, high BP)

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10
Q

relationship of cooking time to elevation

A

directly proportional
(low cooking time, low elevation)

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11
Q

The pressure that a gas will exert in a container assuming it was alone

A

partial pressure

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12
Q

laughing gas

A

N2O (nitrous/ nitrogen oxide)

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13
Q

Cleveite

A

UO2 (Uranium dioxide)

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14
Q

nitroglycerin

A

C3H5N3O9

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15
Q

chlorophyll

A

C55H72MgN4O5

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16
Q

Baking soda

A

NaHCO3 (sodium bicarbonate)

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17
Q

It denotes the relative amount of bonds formed between the atoms of a molecule

A

Empirical Formula

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18
Q

It denotes the actual number of each atom in a molecule

A

Molecular Formula

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19
Q

Balancing redox reactions:
If the medium is acidic, __ is used to balance O

A

H2O(l)

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20
Q

Balancing redox reactions:
If the medium is acidic, __ is used to balance H

A

H+

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21
Q

Balancing redox reactions:
If the medium is a base, __ is used to balance O

A

OH-

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22
Q

Balancing redox reactions:
If the medium is a base, __ is used to balance H

A

H2O

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23
Q

Matter cannot be created nor destroyed but only change from one form into another

A

Law of Conservation of Mass

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24
Q

Law of Conservation of Mass by

A

Antoine Lavoisier

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25
Q

Regardless of the extensive amount, the percent content of an atom in a molecule must remain constant

A

Law of Definite Composition

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26
Q

Law of Definite Composition by

A

Joseph Louis Proust

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27
Q

Atoms have the tendency to bond with one another into appreciable whole number integers, each one being a distinct species.

A

Law of Multiple Proportions

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28
Q

Law of Multiple Proportions by

A

John Dalton

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29
Q

discovered by Joseph John Thomson

A

electron

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30
Q

The term electron is coined by

A

George Stoney

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31
Q

Model used by JJ Thomson

A

Plum Pudding Model

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32
Q

the charge/mass ratio of an electron was determined through __ by JJ Thomson

A

Cathode Ray Experiment

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33
Q

Oil Drop experiment was conducted by __. He precisely determined the magnitude of the electron’s charge for about 5 significant figures.

A

Robert Millikan

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34
Q

Discovered proton

A

Ernest Rutherford

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35
Q

Ernest Rutherford’s experiment

A

Geiger-Marsden Experiment (Gold Foil Experiment)

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36
Q

Model used by Ernest Rutherford. (electrons are randomly scattered)

A

Atomic Model

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37
Q

Discovered neutron

A

James Chadwick

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38
Q

___ is the model where electrons are revolving around the nucleus by ___

A

Bohr Model; Niels Bohr

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39
Q

Platinichloride Salt formula

A

B2H2PtCl6
(B = sample)

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40
Q

Chloroplatinic Acid

A

H2PtCl6

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41
Q

Commonly used in identifying the molecular mass (actual mass) of a compound

A

Platinichloride Method

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42
Q

Ratio of a sample to chloroplatinic acid

A

2:1

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43
Q

He proposed that Energy, like matter, is discontinuous (Quantum Theory)

A

Max Planck

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44
Q

First spectroscopy (they discovered two alkali metals, cesium and rubidium, with the aid of the spectroscope they had invented the year before)

A

Robert Bunsen and Gustav Kirchhoff

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45
Q

Color of Caesium (Latin: Caesius)

A

sky blue

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46
Q

color of rubidium (Latin: Rubidius)

A

deep red

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47
Q

Greek: Helios, which means ___

A

Helium; the Sun

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48
Q

It places no limitation (infinite) on the amount of energy

A

Classical Physics

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49
Q

A system may only possess a finite (limited), discrete (absolute) amount of energy

A

Quantum Theory

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50
Q

the smallest discrete unit of a phenomenon

A

quanta

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51
Q

TRUE OR FALSE:
The energy of a quantum of electromagnetic radiation is proportional to the frequency of the radiation

A

TRUE

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52
Q

Planck’s Equation

A

E = hf = hc/λ

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53
Q

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.

A

Photoelectric effect

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54
Q

Photoelectric effect was discovered by

A

Heinrich Hertz

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55
Q

Light particle conceived by Einstein

A

photon

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56
Q

ejected electron in the photoelectric effect

A

photoelectrons

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57
Q

Energy that binds an electron to a metal surface. It is constant for every particular metal.

A

Work Function

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58
Q

light can behave as a wave or as a particle (photon)

A

Wave-Particle Duality
(Albert Einstein)

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59
Q

The minimum frequency that a light must possess in order to initiate the photoelectric effect

A

threshold frequency, fo

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60
Q

the energy of an object because of its motion

A

kinetic energy (KE = 1/2 mv^2)

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61
Q

De Broglie’s Wavelength

A

λ = h/mv

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62
Q

fl < fo

A

no photoelectric effect

E < WF + KE

WF = work function
KE = kinetic energy

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63
Q

fl = fo

A

photoelectric effect, but Ve = 0

E = WF; KE = 0

WF = work function
KE = kinetic energy

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64
Q

fl > fo

A

photoelectric effect (electrons are moving away)

E > WF + KE
Ve > 0

WF = work function
KE = kinetic energy

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65
Q

fl > fo

A

photoelectric effect (electrons are moving away)

E > WF + KE
Ve > 0

WF = work function
KE = kinetic energy

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66
Q

Cumulative energy that each particle of a system possesses

A

internal energy

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67
Q

examples of internal energy

A

translational
rotational
vibrational

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68
Q

How many water molecules can attach to methanol via hydrogen bonding?

A

3

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69
Q

TRUE OR FALSE:
Heat and work can be conserved in a system by distributing it evenly amongst the systems constituents.

A

False

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70
Q

Energies in transit; Exists only as energy being transferred between 2 bodies/ systems

A

heat (Q) and work (W)

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71
Q

TRUE OR FALSE:
delta U being equal to the summation of heat and work is an interpretation of the First Law of Thermodynamics

A

True

72
Q

TRUE OR FALSE:
delta H can be interpreted as the heat transferred under constant volume conditions.

A

False

73
Q

Bonds that occur between atoms to form a compound

A

Intramolecular forces

74
Q

Examples of intramolecular forces

A

ionic bond
covalent bond
metallic bond

75
Q

TRUE OR FALSE:
Intramolecular forces need high temperature to break the bond

A

True

76
Q

The minimum temperature to break intramolecular forces is __, while for intermolecular forces is ___.

A

600°C; 100°C

77
Q

transfer of electrons between metals and non-metals

A

Ionic bond

78
Q

sharing of electrons (non-metals)

A

Covalent Bond

79
Q

Metal atoms lose their outermost electron to form positively charged ions (metals)

A

Metallic bond

80
Q

TRUE OR FALSE:
Intramolecular forces are weaker than intermolecular forces

A

FALSE

81
Q

Bonds that occur between molecules, identical or not.

A

Intermolecular Forces

82
Q

Examples of intermolecular forces

A

Van der Waals Forces
Dipole-dipole forces
Hydrogen bonding

83
Q

Weakest intermolecular force. Its relative strength depends on the molecules’ polarizability

A

Van der Waals forces

84
Q

TRUE OR FALSE:
Van der Waals forces occur in every compound/ molecule

A

True

85
Q

Van der Waals is also known as

A

dispersion forces
london forces
instantaneous-induced dipole interaction

86
Q

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

A

polarizability

87
Q

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

A

Dipole-dipole forces

88
Q

TRUE OR FALSE:
Dipole-dipole forces only occur between polar molecules.

A

TRUE

89
Q

Pulls/ attracts electrons within its vicinity;
Produces partial positive and partial negative

A

electronegative atoms

90
Q

The strongest intermolecular force

A

Hydrogen Bonding (not exclusive to H2O)

91
Q

Requirements of Hydrogen Bonding

A

(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
Q

TRUE OR FALSE:
Hydrogen bonding can occur between two molecules which can be identical or not.

A

TRUE

93
Q

Relationship of Polarizability to atomic radius (AR)

A

directly proportional
(high AR, high polarizability)

94
Q

Periodic Table trend for increasing atomic radius

A

right to left, top to bottom

95
Q

Relationship of Polarizability to molecular weight (MW)

A

directly proportional
(high MW, high polarizability)

96
Q

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

A

TRUE

97
Q

Properties rel. to polarizability

A

↑ polarizability:

↑ boiling pt
↑ melting pt
↑ surface tension
↑ viscosity
↓ vapor pressure

98
Q

occurs on the molecules on the surface of a liquid due to the unbalanced distribution of forces

A

Surface tension

99
Q

friction to flow

A

viscosity

100
Q

pressure induced by vapor

A

vapor pressure

101
Q

A thermodynamic property that measures the various ways in which a systems’ energy can be distributed among its components

A

Entropy

102
Q

He discovered entropy and explained its behavior.

A

Rudolf Clausius

103
Q

He defined entropy 27 years after its discovery

A

Ludwig Boltzmann

104
Q

High energy

A

↑ microstate
↑ S
↑ mobility
↑ # of energy levels

105
Q

It increases the entropy of the universe (ex. boiling of water L→V)

A

Spontaneous process

106
Q

Common processes that increase the entropy

A

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
Q

TRUE OR FALSE
Increasing the temperature increases the total energy

A

TRUE

108
Q

TRUE OR FALSE
In phase transitions, the intermolecular forces weakens providing more mobility.

A

TRUE

109
Q

A spontaneous process causes an increase in the entropy of the universe

A

Second Law of Thermodynamics

110
Q

The process involves the addition of infinitesimal amounts of heat to a system that causes incremental changes in its properties

A

reversible

111
Q

Criterion for spontaneity:
ΔSuniv < 0
ΔGsys > 0

A

non-spontaneous

112
Q

Criterion for spontaneity:
ΔSuniv = 0
ΔGsys = 0

A

reversible, equilibrium

113
Q

Criterion for spontaneity:
ΔSuniv > 0
ΔGsys < 0

A

spontaneous

114
Q

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

A

TRUE

115
Q

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 <deltaS_surrounding

A

C: delta S_universe > 0

116
Q

A measure for the maximum available energy for non-PV work

A

Gibbs Free energy

117
Q

Properties of a solution that depends only on the concentration of the solute

A

Colligative properties

118
Q

Common Kb and Kf values:
H2O

A

Kb = 0.512 °C/m
Kf = 1.858 °C/m

119
Q

Common Kb and Kf values:
Benzene (C6H6)

A

Kb = 2.61°C/m
Kf = 5.065 °C/m

120
Q

Common Kb and Kf values:
Camphor (C10H16O)

A

Kf = 40 °C/m

121
Q

Common Kb and Kf values:
Ethanol (C2H5OH)

A

Kb = 1.07 °C/m

122
Q

___ 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.)

A

Osmosis; Second Law of Thermodynamics

123
Q

The amount of pressure necessary to impede the phenomena of osmosis

A

osmotic pressure

124
Q

Formula for osmotic pressure

A

ℼ = MRT

ℼ → osmotic pressure
M → molarity (mol/L)
R → ideal gas constant
T → absolute temperature

125
Q

Colligative properties

A

Vapor pressure lowering
Boiling point elevation
Freezing point depression
Osmotic pressure

126
Q

Kb

A

ebullioscopic constant of a solvent

127
Q

Kf

A

cryoscopic constant of a solvent

128
Q

Boiling point elevation formula

A

ΔTb = mKb

m → molality of the solute (mol solute/ kg solvent)
Kb → ebullioscopic constant

129
Q

Freezing point depression formula

A

ΔTf = mKf

m → molality of the solute (mol solute/ kg solvent)
Kf → cryoscopic constant

130
Q

Vapor pressure lowering formula

A

ΔP = XsoluteP°solvent

P°solvent → pure vapor pressure of solvent
Xsolute → mole fraction of solute

131
Q

He discovered the noble gases

A

William Ramsay

132
Q

William Ramsay along with Lord Rayleigh discovered __

A

Argon

133
Q

Which among the following is the
third gas that William Ramsay isolated
with Morris Travers?

A: Argon B: Neon
C: Krypton D: Xenon

A

D. Xenon

134
Q

How many carbon atoms are there in one molecule of “buckyball”?

A

60

135
Q

Ramsay discovered ___ from an ore of uranium (cleveite)

A

Helium

136
Q

Ramsay alongside Morris Travers discovered ____________ by liquefying air and further distillation (fractional).

A

Neon → Krypton → Xenon

137
Q

Ramsay working along with Frederick Soddy discovered ___, short for ___.

A

Radon; Radium Emanation

138
Q

The emission of ionizing radiation by some of the heavier elements to become stable.

A

Radioactivity

139
Q

“Radioactive” means

A

unstable

140
Q

Which among the following scientists discovered radioactivity?
A: Marie Curie
B: Henri Becquerel
C: Otto Hahn
D: Ernest Rutherford

A

B: Henri Becquerel

141
Q

___ particles have the lowest penetration, while ___ particles have the highest.

A

alpha; gamma

142
Q

Alpha particles have the _____ biological destruction, while gamma particles have the ____.

A

highest; lowest

143
Q

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

A

D. I and II

144
Q

Discovered Polonium and Radium.
Explained the phenomena of radiation

A

Marie Curie

145
Q

Father of Nuclear Chemistry

A

Otto Hahn

146
Q

Nuclear fission is from ____ to ____, while nuclear fusion is from ____ to ____.

A

heavier, lighter;
lighter, heavier

147
Q

Transmutation by___, the nuclei of an atom will undergo transformation when bombarded with a nuclear species.

A

Ernest Rutherford

148
Q

The first artificial transmutation. _____ into _____ using ____ particles.

A

N14 –> O17
alpha particles

149
Q

Synthesized the first synthetic transmuted atom

A

Irene Joliot Curie

150
Q

The synthetic transmuted atom by Irene Joliot Curie

A

P30

151
Q

The number of protons and neutrons in a nuclide that dictate stability

A

Magic numbers

152
Q

Magic numbers of a proton

A

2
8
20
28
50
82

153
Q

Magic numbers of a neutron

A

2
8
20
28
50
82
126

154
Q

uses phosphor
detects presence of light

A

Scintillation counter

155
Q

produces light when it interacts with radioactive substance

A

phosphor

156
Q

quantifying the magnitude

A

Geiger counter

157
Q

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

A: In the Water surrounding the core of a Nuclear Reactor

158
Q

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

A

C: Loss of proper cooling and/or moderator

159
Q

Radiocarbon dating formula

A

ln(No/N) = kt

160
Q

half-life formula

A

t1/2 = ln2/k

161
Q

half-life of C-14

A

5730 years

162
Q

No of C-14

A

15.3 disintegrations of C14 per minute per gram of C12

163
Q

1 Ci (Curie) = ____ Bq (Becquerel)

A

3.7 x 10^10

164
Q

1 Ci (Curie) = _____ disentegration/s

A

3.7x10^10

165
Q

1 Bq = ____ disintegrations/ decay per second (dps)

A

1

166
Q

The amount of a substance that disintegrate per unit time

A

Activity

167
Q

The amount of radiation that deposits 0.01J of energy per kg of matter

A

rad

168
Q

What is the meaning of rad?

A

radiation absorbed dose

169
Q

1 rad = ____ Gray (Gy)

A

0.01

170
Q

Relates various kinds of radiation based on their biological destruction

A

rem

171
Q

What is the meaning of rem?

A

roentgen equivalent man

172
Q

Formula for rem

A

rad x Q

173
Q

Relative Biological Effectiveness of:
X-ray, Y-ray and Beta particles

A

Q = 1

174
Q

Relative Biological Effectiveness of:
slow neutrons

A

Q = 3

175
Q

Relative Biological Effectiveness of:
fast neutrons, protons

A

Q = 10

176
Q

Relative Biological Effectiveness of:
alpha particles

A

Q = 20

DAY 1 (1 decks)

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