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May 2023 ChELE > Chem > Flashcards

Chem Flashcards

1
Q

Boyle’s Law in terms of Length

A

P1L1 = P2L2

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2
Q

Boyle’s Law other name

A

Mariotte’s Law

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3
Q

Atmospheric Pressure relationship to Elevation, Boiling Point, and Time of Boiling

A

Elevation (Inverse)
Boiling point (Direct)
Boiling Time (Inverse)

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4
Q

Other term for atmospheric pressure and instrument used

A

Barometric Pressure; Barometer

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5
Q

Other term for gage pressure; instrument used

A

Manometric pressure; manometer

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6
Q

Atmospheric pressure with respect to altitude

A

dP/dz = - rho*g
Note: rho for gas
Remember to derive

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7
Q

Average molecular weight (gases)

A

MWave = yaMWa + ybMWb +…
ya and yb are mol frac

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8
Q

Average molecular weight (solids and iquids)

A

1/MWave = xa/MWa + xb/MWb + …
xa and xb are weight frac

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9
Q

Chlorophyll

A

C55H72MgN4O5

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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)

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11
Q

Molecular Formula definition

A

denotes actual number of atoms in a molecule

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12
Q

Effective Bulletproof Vest

A

Polyethylene Fiber (UHMWPE: Ultra High Molecular Weight Polyethylene)

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13
Q

Old material for bulletproof vest

A

polyamide fibers (kevlar)

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14
Q

acrylics; for production of plexiglass and lucites

A

polymethacrylate fiber

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15
Q

for bulletproof windows

A

Polycarbonate Fiber
monomer: diethyl carbonate
catalyst: bisphenol-A

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16
Q

Law of Conservation of Mass proponent

A

Antoine Lavoisier

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17
Q

Law of Definite Composition proponent

A

Joseph Louis Proust

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18
Q

Law of Definite Composition states that

A

regardless of the amount, % of its components is constant

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19
Q

Law of Multiple Proportion Proponent and statement

A

John Dalton; each combination of atoms in whole number integer is distinct

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20
Q

Molecular Formula
(formula)

A

(empirical formula)(constant)
constant = molecular mass / empirical mass

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21
Q

Who discovered electron

A

J.J Thomson
Cathode Ray Experiment
(also identified mass/charge ratio)

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22
Q

coined the term “electron”

A

George Stoney

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23
Q

identified the charge of electron up to 5 significant figures

A

Robert Millikan
Oil Drop Experiment

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24
Q

Plum-Pudding Model

A

atom is made up of empty spaces where electrons are spread all over

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25
Q

who discovered proton

A

Ernest Rutherford

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26
Q

experiment that led to discovery of proton

A

Geiger Marsden Experiment
Pinapatamaan yung zinc sulfide ng alpha particle

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27
Q

Atomic Model by Rutherford

A

There is nucleus in the center made up of positively-charged proton

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28
Q

who discovered neutron

A

James Chadwick

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29
Q

Bohr Atomic Model

A

Neils Bohr
There is particular order of electrons and it revolves around nucleus

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30
Q

energy is discontinuous

A

Max Planck

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31
Q

first spectroscope

A

Robert Bunsen and Gustav Kirchoff
(used to discover Rubidium and Cesium)

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32
Q

Classical Physics

A

system can possess infinite amt of energy (macro scale)

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33
Q

Quantum Theory and the one who proposed

A

system may possess finite and discrete amt of energy
Max Planck

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34
Q

Planck’s Equation

A

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

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35
Q

speed of light formula

A

c=vf
c = 3x10^8 m/s
v = wavelength

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36
Q

Planck’s Constant in Calcu

A

6.626x-34 J*s
Constant 06
It can be per photon

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37
Q

who discovered photoelectric effect

A

Heinrich Hertz

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38
Q

Threshold Frequency

A

minimum frequency that light must possess to initiate photoelectric effect

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39
Q

Importance of Photoelectric effect

A

proved Quantum Theory by Max Planck

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40
Q

Light as a particle

A

photon

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41
Q

light can behave as a wave or particle

A

Wave Particle Duality
Albert Einstein

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42
Q

Photoelectric Effect Formula

A

E = WF + KE
E = energy of photon
WF = work func
KE = kinetic energy of electron

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43
Q

Mass of Electron

A

9.109x10^-31 kg
Constant 03

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44
Q

Work Function

A

Energy that binds the electron to the surface of metal

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45
Q

de Broglie’s wavelength

A

Y = h/(m*v)
m and v is mass and velocity of macro particle
h = Planck’s constant

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46
Q

ym to m

A

1 ym = 10^-24 m

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47
Q

Intramolecular forces

A

bonds between atoms of molecule

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48
Q

intermolecular forces

A

bonds or interaction between molecules

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49
Q

intramolecular forces is __ intermolecular forces

A

> > > > > > > > > >

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50
Q

Other term for van der waals

A

Dispersion Forces, london forces, instantaneous dopole-induced dipole interactions

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51
Q

Polarizability

A

Tendency to undergo electron redistribution

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52
Q

Dipole Dipole force only exists in

A

polar molecules

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53
Q

Dipole-Dipole force requirement

A

there must be an electronegative atom in the molecule

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54
Q

electronegative atom

A

ability to attract electrons toward itself

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55
Q

Hydrogen Bonding requirement

A

(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

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56
Q

Rank intermolecular forces

A

VDW<DDF<HB
weakest to strongest

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57
Q

Polarizabily relationships

A

van der waals (direct)
atomic radius (direct)
molecular weight (direct)

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58
Q

Atomic Radius in Periodic Table

A

Increasing from right to left
Increasing from top to bottom

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59
Q

Properties relative to intermolecular forces and its relationships

A

Direct: Boiling point, melting point, surface tension, viscosity
Inverse: vapor pressure

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60
Q

internal energy

A

sum of energy of every particle making up the system

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61
Q

introduced the concept of entropy

A

Rudolf Clausius

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62
Q

defined the concept of entropy

A

Ludwig Boltzmann

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63
Q

Entropy formula

A

S = Kb*ln(W)
Kb = Boltzmann Constant
W = microstate

64
Q

delta S universe

A

< 0 : nonspontaneous
= 0 : reversible, spontaneous
> 0 : spontaneous

Remember: delta G :opposite in terms of the process

65
Q

who discovered Argon

A

Willian Ramsay and Lord Rayleigh

66
Q

who discovered helium

A

William Ramsay

67
Q

William Ramsay and Morris Travers discovery in order

A
  1. neon
  2. krypton
  3. xenon
68
Q

who discovered Radon

A

William Ramsay and Frederick Soddy

69
Q

Buckyball

A

C60
buckmisterfullrene

70
Q

alpha particle
-notation
-charge

A

alpha, 4, 2
helium 4, 2
positive
(exponent, subscript)

71
Q

mass number

A

proton + neutron

72
Q

atomic number

A

= proton = electron

73
Q

beta particle

A

beta 0, -1
e 0, -1
(exponent, subscript)

74
Q

Gamma Ray

A

Y 0, 0
(exponent, subscript)

75
Q

Arrange forms of radioactivity in terms of penetration

A

alpha < beta < gamma
lowest to highest

76
Q

Arrange forms of radioactivity in terms of biological destruction

A

gamma < beta < alpha

77
Q

Positron notation

A

beta 0, +1
positive electron

78
Q

neutron notation

A

n 1, 0

79
Q

discovered Po and Ra

A

Marie Curie

80
Q

Father of Nuclear Chemistry

A

Otto Hahn

81
Q

Nuclear Fission

A

Decay from heavy to lighter nuclide

82
Q

Transmutation

A

converting one atom into another by bombarding nucleus with different particle

83
Q

Transmutation by Ernest Rutherford

A

N-14 to O-7

84
Q

transmutation producing first artificial nuclude

A

Irene Joliot and Frederick Joliot
P-30

85
Q

Nuclide

A

atom with particular mass and atomic number

86
Q

Nuclear Reaction

A

P a,z —> D, a, z
P is parent nuclide
Z is daughter nuclide

87
Q

Positron Emission

A

kinukuha nung nucleus yung electron and nirereact nya yun sa proton to produce neutron
(lighter nuclide)

88
Q

Electron Capture

A

same with positron emission, but electron is sourced externally
(heavier nuclide)

89
Q

Uranium Series

A

U-238 to Pb-206
(naturally occurring)

90
Q

Actinium Series

A

U-235 to Pb-207
(naturally occurring)

91
Q

Thorium Series

A

Th-232 to Pb-208
(naturally occurring)

92
Q

Neptunium Series

A

Np-237 to Tl-205
(man-made)

93
Q

Plutonium Series

A

Pu-241 to U-235
(man-made)

94
Q

Final daughter of naturally occurring decay series

A

Pb

95
Q

formula for decay series identification

A

(mass no. of parent nuclide - mass no. of suspected nuclide) / 4
Yung divisible sa 4 yung magiging decay series

96
Q

Magic Number definition

A

values of proton and neutron that signifies stability
ginagamit din if nag iidentify pag nagcocompare ng stability ng mga nuclide

97
Q

Magic Numbers: Proton

A

2 8 20 28 50 82

98
Q

Magic Numbers: Proton

A

2 8 20 28 50 82

99
Q

Activity conversion

A

1 Curie (Ci) = 3.7x10^10 Becquerel (Bq) or disintegrations per sec
disintegration can be particles, proton, photon, etc

100
Q

Activity Formula

A

Activity = kN
k = decay constant (based on half life) = ln2/t
Follows first order. alam mo na yun

101
Q

rad conversion

A

1 rad = 0.01 Gray (Gy) = 0.01 J of energy per kg matter
radiation absorbed dose

102
Q

rem conversion

A

1 Sievert (Sv) =100 rem

103
Q

rem formula

A

rem = rad*Q
Q = relative biological effectiveness (RBE)

104
Q

Q=1
RBE

A

x-ray, gamma ray, beta particle

105
Q

Q=3
RBE

A

slow neutron

106
Q

Q=10
RBE

A

fast neutrons, protons

107
Q

Q=20
RBE

A

alpha particles

108
Q

Empirical formula of human DNA

A

C39H50O22N15P3

109
Q

photoelectron

A

Ejected electron in photoelectric effect

110
Q

Instantaneous Dipole

A

redistribution of electrons due to the proximity to a magnetic field

111
Q

Induced Dipole

A

electron distribution due to shear proximity to an instantaneous dipole

112
Q

Entropy (definition by Ludwig Boltzmann)

A

thermodynamic property that measures the various ways in which a system distributes its energy among its components.

113
Q

discovered radioactivity

A

Henri Becquerel

114
Q

metastate

A

substances that are only stable for a short period of time

115
Q

List the Decay Series

A

Uranium
Actinium
Thorium
Neptunium
Plutonium

116
Q

Thyroid cancer

A

I-131

117
Q

Perchloroethylene
Does this molecule have polar bonds? Is it a polar molecule? Does it have a dipole?

A

yes, non-polar, none

118
Q

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?

A

manganese, calcium chloride, sodium acetate

119
Q

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

A

potential, kinetic, potential, kinetic, kinetic

120
Q

Who invented the Carbon-14 dating method?

A

Williard Libby

121
Q

Process of breaking down a large isotope into smaller isotopes.

A

nuclear fission

122
Q

How does alpha, beta and gamma particle affect the mass number of an atom?

A

4, 0, 0

123
Q

What was Melvin Calvin was known for his study of?

A

photosynthesis

124
Q

Iodine vapor forms iodine crystals when it touches a cold surface. What is the reverse of the process being described?

A

sublimation

125
Q

Which of the following has a larger ionic nucleus? Na+ or Na?

A

Na

126
Q

The purpose of control rods in a fission reactor is to:

A

absorb neutrons generated in the fission process.

127
Q

Which bond is the least polar? C-C, C-N, C-Cl, C-F, C-O?

A

C-C < C-Cl < C-N < C-O < C-F

128
Q

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?

A

Group 2 A

129
Q

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.

A

HCl < HI < HBr

130
Q

Which isotope of boron is the most stable: boron-8, boron-10, or boron-12?

A

boron-10

131
Q

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.

A

only (2)

132
Q

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

A

homogeneous, heterogeneous, colloidal, heterogeneous, colloidal, colloidal

133
Q

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?

A

No, Yes, No

134
Q

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

A

1.0% soln. of NaCl

135
Q

Human Chorionic Gonadotropin or hCG is a hormone that is primarily detected by which among the following tests?

A

Pregnancy Test

136
Q

Human Chorionic Gonadotropin or hCG is a hormone that is primarily detected by which among the following tests?

A

Pregnancy Test

137
Q

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

A Geiger Counter containing Argon
and Boron trifluoride

138
Q

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

A

C: NaI Crystals containing Thallium (II) Iodide

139
Q
  1. 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

140
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

Loss of proper cooling and/or
moderator

141
Q

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

A

C: 8.0 mm of Lucite

142
Q

Intensity of Radiation and Distance from Source Relationship

A

(I1)(d1)^2 = (I2)(d^2)^2
inverse
Intensity can be activity

143
Q

most stable isotope have

A

equal no. of protons and neutrons

144
Q

proton notation in nuclear reaction

A

H-1

145
Q

no. of half lives elapsed

A

t/(t1/2)

146
Q

3.25 What kind of emission does not result in
transmutation?

A

Gamma emission does not result in transmutation.

147
Q

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?

A

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
Q

3.48 What is the product of the fusion of hydrogen-2 and hydrogen-3 nuclei?

A

He-4 + n-1 + 5.3x10^-8 kcal/mol

149
Q

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?

A

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
Q

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

a bit more than 0.1 (or 10%) of the half-life of carbon-14
if 2012 is assumed year

151
Q

3.67 Which radiation will cause more ionization, Xrays
or radar?

A

X rays will cause more ionization than radar waves
because X rays have higher energy than radar waves.

152
Q

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?

A

One sievert is 100 rem. This dose is sufficient to cause radiation sickness but not certain death

153
Q

3.75 Oxygen-16 is the stable, nonradioactive isotope. Do the half-lives indicate anything about the stability of the other oxygen isotopes?

A

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
Q

number of beta particles emitted

A

atomic no. of parent - atomic no. of suspected -2a
a = alpha particles emitted

155
Q

degree of deprotonation

A

pH = pKa + log [deprotonation / protonation ]
pH = pKa + log [x / 1-x]

156
Q

identifying compounds having covalent bonds

A

delta electronegativity = right - left
if delta electronegativity > .4, polar

May 2023 ChELE (11 decks)

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