Chem Flashcards
1
Q
Boyle’s Law in terms of Length
A
P1L1 = P2L2
2
Q
Boyle’s Law other name
A
Mariotte’s Law
3
Q
Atmospheric Pressure relationship to Elevation, Boiling Point, and Time of Boiling
A
Elevation (Inverse)
Boiling point (Direct)
Boiling Time (Inverse)
4
Q
Other term for atmospheric pressure and instrument used
A
Barometric Pressure; Barometer
5
Q
Other term for gage pressure; instrument used
A
Manometric pressure; manometer
6
Q
Atmospheric pressure with respect to altitude
A
dP/dz = - rho*g
Note: rho for gas
Remember to derive
7
Q
Average molecular weight (gases)
A
MWave = yaMWa + ybMWb +…
ya and yb are mol frac
8
Q
Average molecular weight (solids and iquids)
A
1/MWave = xa/MWa + xb/MWb + …
xa and xb are weight frac
9
Q
Chlorophyll
A
C55H72MgN4O5
10
Q
Empirical Formula definition
A
denotes number of bonds between atoms
(basically, ratios ng atoms lang sya and doesn’t concern the quantity of atom)
11
Q
Molecular Formula definition
A
denotes actual number of atoms in a molecule
12
Q
Effective Bulletproof Vest
A
Polyethylene Fiber (UHMWPE: Ultra High Molecular Weight Polyethylene)
13
Q
Old material for bulletproof vest
A
polyamide fibers (kevlar)
14
Q
acrylics; for production of plexiglass and lucites
A
polymethacrylate fiber
15
Q
for bulletproof windows
A
Polycarbonate Fiber
monomer: diethyl carbonate
catalyst: bisphenol-A
16
Q
Law of Conservation of Mass proponent
A
Antoine Lavoisier
17
Q
Law of Definite Composition proponent
A
Joseph Louis Proust
18
Q
Law of Definite Composition states that
A
regardless of the amount, % of its components is constant
19
Q
Law of Multiple Proportion Proponent and statement
A
John Dalton; each combination of atoms in whole number integer is distinct
20
Q
Molecular Formula
(formula)
A
(empirical formula)(constant)
constant = molecular mass / empirical mass
21
Q
Who discovered electron
A
J.J Thomson
Cathode Ray Experiment
(also identified mass/charge ratio)
22
Q
coined the term “electron”
A
George Stoney
23
Q
identified the charge of electron up to 5 significant figures
A
Robert Millikan
Oil Drop Experiment
24
Q
Plum-Pudding Model
A
atom is made up of empty spaces where electrons are spread all over
25
who discovered proton
Ernest Rutherford
26
experiment that led to discovery of proton
Geiger Marsden Experiment
Pinapatamaan yung zinc sulfide ng alpha particle
27
Atomic Model by Rutherford
There is nucleus in the center made up of positively-charged proton
28
who discovered neutron
James Chadwick
29
Bohr Atomic Model
Neils Bohr
There is particular order of electrons and it revolves around nucleus
30
energy is discontinuous
Max Planck
31
first spectroscope
Robert Bunsen and Gustav Kirchoff
(used to discover Rubidium and Cesium)
32
Classical Physics
system can possess infinite amt of energy (macro scale)
33
Quantum Theory and the one who proposed
system may possess finite and discrete amt of energy
Max Planck
34
Planck's Equation
E = hf
E = energy of electromagnetic radiation, J
h = Planck's Constant, J*s
f = frequency, Hz
E is also energy of photon, and we can equate it with eqn of photoelectric effect
35
speed of light formula
c=vf
c = 3x10^8 m/s
v = wavelength
36
Planck's Constant in Calcu
6.626x-34 J*s
Constant 06
It can be per photon
37
who discovered photoelectric effect
Heinrich Hertz
38
Threshold Frequency
minimum frequency that light must possess to initiate photoelectric effect
39
Importance of Photoelectric effect
proved Quantum Theory by Max Planck
40
Light as a particle
photon
41
light can behave as a wave or particle
Wave Particle Duality
Albert Einstein
42
Photoelectric Effect Formula
E = WF + KE
E = energy of photon
WF = work func
KE = kinetic energy of electron
43
Mass of Electron
9.109x10^-31 kg
Constant 03
44
Work Function
Energy that binds the electron to the surface of metal
45
de Broglie's wavelength
Y = h/(m*v)
m and v is mass and velocity of macro particle
h = Planck's constant
46
ym to m
1 ym = 10^-24 m
47
Intramolecular forces
bonds between atoms of molecule
48
intermolecular forces
bonds or interaction between molecules
49
intramolecular forces is __ intermolecular forces
>>>>>>>>>>
50
Other term for van der waals
Dispersion Forces, london forces, instantaneous dopole-induced dipole interactions
51
Polarizability
Tendency to undergo electron redistribution
52
Dipole Dipole force only exists in
polar molecules
53
Dipole-Dipole force requirement
there must be an electronegative atom in the molecule
54
electronegative atom
ability to attract electrons toward itself
55
Hydrogen Bonding requirement
(1) one molecule must have H atom bonded to an electronegative atom
(2) other molecule must have a lone pair in its electronegative atom
electronegative atom: O, N, F
56
Rank intermolecular forces
VDW
57
Polarizabily relationships
van der waals (direct)
atomic radius (direct)
molecular weight (direct)
58
Atomic Radius in Periodic Table
Increasing from right to left
Increasing from top to bottom
59
Properties relative to intermolecular forces and its relationships
Direct: Boiling point, melting point, surface tension, viscosity
Inverse: vapor pressure
60
internal energy
sum of energy of every particle making up the system
61
introduced the concept of entropy
Rudolf Clausius
62
defined the concept of entropy
Ludwig Boltzmann
63
Entropy formula
S = Kb*ln(W)
Kb = Boltzmann Constant
W = microstate
64
delta S universe
< 0 : nonspontaneous
= 0 : reversible, spontaneous
> 0 : spontaneous
Remember: delta G :opposite in terms of the process
65
who discovered Argon
Willian Ramsay and Lord Rayleigh
66
who discovered helium
William Ramsay
67
William Ramsay and Morris Travers discovery in order
1. neon
2. krypton
3. xenon
68
who discovered Radon
William Ramsay and Frederick Soddy
69
Buckyball
C60
buckmisterfullrene
70
alpha particle
-notation
-charge
alpha, 4, 2
helium 4, 2
positive
(exponent, subscript)
71
mass number
proton + neutron
72
atomic number
= proton = electron
73
beta particle
beta 0, -1
e 0, -1
(exponent, subscript)
74
Gamma Ray
Y 0, 0
(exponent, subscript)
75
Arrange forms of radioactivity in terms of penetration
alpha < beta < gamma
lowest to highest
76
Arrange forms of radioactivity in terms of biological destruction
gamma < beta < alpha
77
Positron notation
beta 0, +1
positive electron
78
neutron notation
n 1, 0
79
discovered Po and Ra
Marie Curie
80
Father of Nuclear Chemistry
Otto Hahn
81
Nuclear Fission
Decay from heavy to lighter nuclide
82
Transmutation
converting one atom into another by bombarding nucleus with different particle
83
Transmutation by Ernest Rutherford
N-14 to O-7
84
transmutation producing first artificial nuclude
Irene Joliot and Frederick Joliot
P-30
85
Nuclide
atom with particular mass and atomic number
86
Nuclear Reaction
P a,z ---> D, a, z
P is parent nuclide
Z is daughter nuclide
87
Positron Emission
kinukuha nung nucleus yung electron and nirereact nya yun sa proton to produce neutron
(lighter nuclide)
88
Electron Capture
same with positron emission, but electron is sourced externally
(heavier nuclide)
89
Uranium Series
U-238 to Pb-206
(naturally occurring)
90
Actinium Series
U-235 to Pb-207
(naturally occurring)
91
Thorium Series
Th-232 to Pb-208
(naturally occurring)
92
Neptunium Series
Np-237 to Tl-205
(man-made)
93
Plutonium Series
Pu-241 to U-235
(man-made)
94
Final daughter of naturally occurring decay series
Pb
95
formula for decay series identification
(mass no. of parent nuclide - mass no. of suspected nuclide) / 4
Yung divisible sa 4 yung magiging decay series
96
Magic Number definition
values of proton and neutron that signifies stability
ginagamit din if nag iidentify pag nagcocompare ng stability ng mga nuclide
97
Magic Numbers: Proton
2 8 20 28 50 82
98
Magic Numbers: Proton
2 8 20 28 50 82
99
Activity conversion
1 Curie (Ci) = 3.7x10^10 Becquerel (Bq) or disintegrations per sec
disintegration can be particles, proton, photon, etc
100
Activity Formula
Activity = kN
k = decay constant (based on half life) = ln2/t
Follows first order. alam mo na yun
101
rad conversion
1 rad = 0.01 Gray (Gy) = 0.01 J of energy per kg matter
radiation absorbed dose
102
rem conversion
1 Sievert (Sv) =100 rem
103
rem formula
rem = rad*Q
Q = relative biological effectiveness (RBE)
104
Q=1
RBE
x-ray, gamma ray, beta particle
105
Q=3
RBE
slow neutron
106
Q=10
RBE
fast neutrons, protons
107
Q=20
RBE
alpha particles
108
Empirical formula of human DNA
C39H50O22N15P3
109
photoelectron
Ejected electron in photoelectric effect
110
Instantaneous Dipole
redistribution of electrons due to the proximity to a magnetic field
111
Induced Dipole
electron distribution due to shear proximity to an instantaneous dipole
112
Entropy (definition by Ludwig Boltzmann)
thermodynamic property that measures the various ways in which a system distributes its energy among its components.
113
discovered radioactivity
Henri Becquerel
114
metastate
substances that are only stable for a short period of time
115
List the Decay Series
Uranium
Actinium
Thorium
Neptunium
Plutonium
116
Thyroid cancer
I-131
117
Perchloroethylene
Does this molecule have polar bonds? Is it a polar molecule? Does it have a dipole?
yes, non-polar, none
118
You place manganese, calcium chloride and sodium acetate in a liquid, in which they are not soluble. The liquid has a density of 2.15 g/ml. Which will sink to the bottom, which will stay on the top, and which will stay in the middle of the liquid?
manganese, calcium chloride, sodium acetate
119
Classify these as kinetic or potential energy (1) Water held by a dam (2) A speeding train (3) A book on its edge before falling (4) A falling book (5) Electric current in a light bulb
potential, kinetic, potential, kinetic, kinetic
120
Who invented the Carbon-14 dating method?
Williard Libby
121
Process of breaking down a large isotope into smaller isotopes.
nuclear fission
122
How does alpha, beta and gamma particle affect the mass number of an atom?
4, 0, 0
123
What was Melvin Calvin was known for his study of?
photosynthesis
124
Iodine vapor forms iodine crystals when it touches a cold surface. What is the reverse of the process being described?
sublimation
125
Which of the following has a larger ionic nucleus? Na+ or Na?
Na
126
The purpose of control rods in a fission reactor is to:
absorb neutrons generated in the fission process.
127
Which bond is the least polar? C-C, C-N, C-Cl, C-F, C-O?
C-C < C-Cl < C-N < C-O < C-F
128
You are presented with a Lewis dot structure of element X as X:. To which two groups in the Periodic Table might this element belong?
Group 2 A
129
The normal boiling point of a substance depends on both the mass of the molecule and the attractive forces between molecules. Arrange the compounds in each set in order of increasing boiling point: (1) HCl, (2) HBr and (3) HI.
HCl < HI < HBr
130
Which isotope of boron is the most stable: boron-8, boron-10, or boron-12?
boron-10
131
Write an equation for the reaction of HCl with each compound. Which are acid–base reactions? Which are redox reactions? (1) Na2CO3 (2) Mg (3) NaOH (4) NH3 (5) Fe2O3 (6) CH3NH2 (7) NaHCO3.
only (2)
132
Classify the following systems as homogeneous, heterogeneous, or colloidal mixtures. (1) Physiological saline solution (2) Orange juice (3) A cloud (4) Wet sand (5) Suds (6) Milk
homogeneous, heterogeneous, colloidal, heterogeneous, colloidal, colloidal
133
By nature, sulfur molecules can exist in various conditions such as S8, S2, and S. (1) Is the mass of one mole of each of these molecules the same? (2) Is the number of molecules in one mole of each of these molecules the same? (3) Is the number of atoms of sulfur in one mole of each of these molecules the same?
No, Yes, No
134
Which among the following has the highest boiling point?
1.0% soln. of (NH2)2CO
1.0% soln. of NaCl
1.0% soln. of ZnSO4
1.0% soln. of C6H12O6
1.0% soln. of NaCl
135
Human Chorionic Gonadotropin or hCG is a hormone that is primarily detected by which among the following tests?
Pregnancy Test
136
Human Chorionic Gonadotropin or hCG is a hormone that is primarily detected by which among the following tests?
Pregnancy Test
137
Which among the following can
detect the neutrons produced by U-235
undergoing nuclear fission?
A. A Geiger Counter containing Fluorine Gas
B. A Scintillation Counter containing Zinc Sulfide and Xenon
C: A Geiger Counter containing Argon and Boron trifluoride
D: A Scintillation Counter containing
Tungsten Carbide
A Geiger Counter containing Argon
and Boron trifluoride
138
Which among the following is the
phosphor of a scintillation counter
intended for the detection of gamma
radiation?
A: Zinc Sulfide
B: Metastable Technetium-99
C: NaI Crystals containing Thallium (II) Iodide
D: Buckminsterfullerene
C: NaI Crystals containing Thallium (II) Iodide
139
38. 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
In the Water surrounding the core
of a Nuclear Reactor
140
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
Loss of proper cooling and/or
moderator
141
The Bataan Nuclear Power Plant is
planned to be retrofitted in hopes of
using it for the first time. One point
of concern is the material that would
be used in the outer portions of the
room housing the fuel rods. If the
radiation coming from the fuel rods
would be a strong beta emission, which
material among the following should be
utilized?
A: 1.00 cm of Aluminum
B: 7.50 m of Concrete
C: 8.0 mm of Lucite
D: 35.0 m of Lead
C: 8.0 mm of Lucite
142
Intensity of Radiation and Distance from Source Relationship
(I1)(d1)^2 = (I2)(d^2)^2
inverse
Intensity can be activity
143
most stable isotope have
equal no. of protons and neutrons
144
proton notation in nuclear reaction
H-1
145
no. of half lives elapsed
t/(t1/2)
146
3.25 What kind of emission does not result in
transmutation?
Gamma emission does not result in transmutation.
147
3.31 The element radium is extremely radioactive. If you converted a piece of radium metal to radium chloride (with the weight of the radium remaining the same), would it become less radioactive?
No, the conversion of Ra to Ra2+ involves loss of
valence electrons, which is not a nuclear process and, therefore, does not involve a change in radioactivity.
148
3.48 What is the product of the fusion of hydrogen-2 and hydrogen-3 nuclei?
He-4 + n-1 + 5.3x10^-8 kcal/mol
149
3.53 (Chemical Connections 3A) Why is it accurate to
assume that the carbon-14 to carbon-12 ratio in a
living plant remains constant over the lifetime of
the plant?
The assumption of a constant carbon-14 to carbon-12 ratio rests on two assumptions: (1) that carbon-14 is continually generated in the upper atmosphere by the production and decay of nitrogen-14, and (2) that carbon-14 is incorporated into carbon dioxide,
CO2, and other carbon compounds are then distributed worldwide as part of the carbon cycle. The continual formation of carbon-14; transfer of the isotope within the oceans, atmosphere, and biosphere; and the decay of living matter keep the supply of carbon-14 constant.
150
3.55 (Chemical Connections 3A) Carbon-14 dating of them Shroud of Turin indicated that the plant from which the shroud was made was alive around AD 1350. To how many half-lives does this correspond?
a bit more than 0.1 (or 10%) of the half-life of carbon-14
if 2012 is assumed year
151
3.67 Which radiation will cause more ionization, Xrays
or radar?
X rays will cause more ionization than radar waves
because X rays have higher energy than radar waves.
152
3.71 A patient is reported to have been irradiated by
a dose of 1 sievert in a nuclear accident. Is he in
mortal danger?
One sievert is 100 rem. This dose is sufficient to cause radiation sickness but not certain death
153
3.75 Oxygen-16 is the stable, nonradioactive isotope. Do the half-lives indicate anything about the stability of the other oxygen isotopes?
Oxygen-16 is stable because it has an equal number of protons and neutrons. The other isotopes are unstable because the numbers of protons and neutrons are unequal. In this case, the greater the neutron/proton ratio, the shorter the half-life of the isotope.
154
number of beta particles emitted
atomic no. of parent - atomic no. of suspected -2a
a = alpha particles emitted
155
degree of deprotonation
pH = pKa + log [deprotonation / protonation ]
pH = pKa + log [x / 1-x]
156
identifying compounds having covalent bonds
delta electronegativity = right - left
if delta electronegativity > .4, polar
