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ChE LE Flashcards > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

1
Q

Molecular / Empirical Formulas:
Chloroform

A

CH Cl3

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2
Q

Molecular / Empirical Formulas:
Phenylalanine

A

C9 H11 N O2

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3
Q

Molecular / Empirical Formulas:
Arginine

A

C6 H14 N4 O2

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4
Q

Molecular / Empirical Formulas:
Monazite

A

PO4SiO4

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5
Q

Molecular / Empirical Formulas:
Cleveite

A

UO2

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6
Q

Molecular / Empirical Formulas:
Cupric oleate

A

C36 H66 Cu O4

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7
Q

Molecular / Empirical Formulas:
Aquamarine

A

Be3 Al2 (Si16 O18)

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8
Q

Molecular / Empirical Formulas:
Emerald

A

Be3 Al2 Si O6

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9
Q

Molecular / Empirical Formulas:
Lapis lazuli

A

Na4 S Si3 Al2 O12

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10
Q

Molecular / Empirical Formulas:
Prussian Blue

A

Fe7(CN)18

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11
Q

Molecular / Empirical Formulas:
Acrylonitrite

A

C3 H3 N

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12
Q

Molecular / Empirical Formulas:
Kernite

A

Na2B4O7 x 4 H2O

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13
Q

Molecular / Empirical Formulas:
Freon

A

C Cl2 F2

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14
Q

Molecular / Empirical Formulas:
DNA

A

C15 H31 N3 O13 P2

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15
Q

Molecular / Empirical Formulas:
Chlorophyll

A

C5 H72 O5 N4 Mg

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16
Q

Molecular / Empirical Formulas:
Chalcopyrite

A

CuFeS2

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17
Q

Molecular / Empirical Formulas:
Nitroglycerine

A

C3 H5 N3 O9

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18
Q

Molecular / Empirical Formulas:
Olvanil (not in Perry’s)

A

C26 H43 N O3

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19
Q

Molecular / Empirical Formulas:
Alar (not in Perry’s)

A

C6 H12 N2 O3

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20
Q

Molecular / Empirical Formulas:
Rochelle Salt (not in Perry’s)

A

K Na C4 H4 O6 * 4H2O

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21
Q

Molecular / Empirical Formulas:
Taurine (not in Perry’s)

A

C2H7NO3S

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22
Q

Molecular / Empirical Formulas:
Angelic Acid (not in Perry’s)

A

C5H8O2

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23
Q

The nonstick coating on cookware is made from what chemical formula?

A

CF2=CF2
Teflon

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24
Q

Number of double bonds in Geraniol

A

Two

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25
Q

Elemental Abundance:
Universe

A

Universe:
H > He > O > Others

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26
Q

Elemental Abundance:
Human Body

A

Human Body (by mass)
O - 65%
C - 18.5%
H - 9.5%
N - 3.2%
Others…..

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27
Q

Elemental Abundance:
Earth’s Crust

A

Earth’s Crust (by mass)
O – 47%
Si – 28%
Al – 8%
Fe – 4.5%
Ca – 3.5%
Other – 9%

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28
Q

Petroleum Products: (# of C’s and Phase)

a) Petroleum Gas
b) Gasoline
c) Kerosene
d) Fuel Oil
e) Lubricating Oil
f) Residue

A

a) Petroleum Gas: C1 to C4
Gas
b) Gasoline (naphtha): C5 to C12
Liquid
c) Kerosene: C12 to C16
Liquid
d) Fuel Oil: C15 to C18
Liquid
e) Lubricating Oil: C15 to C18
Liquid
f) Residue (asphalt): > C18
Solid

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29
Q

Scientists awarded the Nobel Prize in Chemistry in 1995 for their work on ozone depletion

A

Paul Crutzen, Sherwood Roland, Mario Molina

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30
Q

Coined the term ‘radioactivity’

A

Marie Curie

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31
Q

Definition of Radioactivity

A

emission of ionizing radiation cause by disintegration of atomic nuclei

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32
Q

First transmutated atom

A

P-30

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33
Q

Radioisotope for carbon dating

A

C-14 (Carbon-14)

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34
Q

Carbon-14 half life

A

5730 years

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35
Q

N0 (Initial amount of C-14)

A

15.3 disintegrations C-14/(min*g C-12)

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36
Q

Who discovered carbon dating?

A

Willard Libby

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37
Q

How Carbon-14 dating works?

A

Use C-12/C-14 ratio
After organism dies, C-12 is constant while C-14 decays to N-15

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38
Q

Father of nuclear chemistry and discovered proof of nuclear fission.

A

Otto Hann

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39
Q

Chemical “beacon” emitting radiation that signals the presence of the substance.

A

Radioactive tracer

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40
Q

Radioisotope for uranium-lead dating

A

U-238 (Uranium-238)

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41
Q

Radioisotope for determining the ages of rocks

A

U-238 (Uranium-238)

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42
Q

Radioisotope for nuclear power generation

A

U-235 (Uranium-235)

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43
Q

Radioisotope for measure water content in the body

A

H-3 (Tritium)

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44
Q

Discovered deuterium

A

Harold C. Urey

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45
Q

Radioisotope used as pacemaker during heart surgery

A

Plutonium 238

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46
Q

Radioisotope for cancer treatment

A

Co-60 (Cobalt-60)

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47
Q

Radioisotope for diagnosis of thyroid effect

A

I-131 (Iodine-131)

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48
Q

Discovered Iodine-131

A

Glenn Seaborg

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49
Q

Radioisotope for locating brain tumors

A

Ar-74 (Arsenic-74)

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50
Q

Radioisotope for pancreas scan

A

Se-75 (Selenium-75)

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51
Q

Radioisotope for heart scan/ heart function during exercise

A

Tl-201 (Thallium-201)

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52
Q

Radioisotope for brain, liver, kidney scans

A

Tc-99m (Tectonium-99m)

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53
Q

Radioisotope for kidney scans

A

Hg-197 (Mercury-197)

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54
Q

Nuclei of the stable hydrogen isotope deuterium

A

Deuterons H-2

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55
Q

Heaviest naturally occuring element

A

Uranium

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56
Q

Radioisotope for eye treatments

A

Strontium 90

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57
Q

Radioisotope for smoke detectors

A

Americium 241

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58
Q

Radioactive nuclide often bombarded with the various isotopes of lead to produce most of the new superheavy elements?

A

Calcium-48 and Nickel-64

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59
Q

Decay product of Radon-222 that produces harmful effects

A

Polonium-218 and Polonium-214 (Po-218 &Po-214)

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60
Q

Radioisotope used in diagnosing the pathology of the spleen

A

Chromium-51 (Cr-51)

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61
Q

Radioisotope used as control rods in nuclear reactors. This nucleus absorbs a neutron and then emits an alpha particle.

A

Boron-10 (B-10)

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62
Q

Radioisotope used in atomic bomb in Hiroshima and Nagasaki, respectively

A

Hiroshima: Uranium 235
Nagasaki: Platinum 239

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63
Q

Device used to generate electricity through controlled nuclear chain reactions

A

Nuclear reactors

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64
Q

Device used to induce nuclear transmutations

A

Particle accelerator

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65
Q

Invented the cyclotron

A

Ernest O. Lawrence

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66
Q

Across the three most notorious accidents regarding nuclear power plants: Three Mile Island, Chernobyl and Fukushima, what is the most common failure that led to several environmental problems?

A

Loss of proper cooling and/or moderator

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67
Q

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

A

boron-10
check n/p hehe

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68
Q

In which among the following can a Cherenkov radiation be observed?
a) In the water surrounding the core of the 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 solar eclipse

A

a) In the water surrounding the core of the nuclear reactor

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69
Q

A noble gas derived from an ore of uranium (cleviete)

A

helium

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70
Q

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

A

absorb neutrons generated in the fission process.

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71
Q

Electron charged particles cause transparent medium to turn blue

A

Cherenkov radiation

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72
Q

Self-sustaining sequence of nuclear fission reactions

A

Nuclear chain reaction

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73
Q

Minimum mass of fissionable material required to generate a self-sustaining nuclear chain reaction.

A

Critical mass

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74
Q

Type of nuclear reaction happening at high temperatures (100 million degC)

A

Thermonuclear Reactions

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75
Q

Main advantage of nuclear fusion to fission

A

No radioactive wastes, more energy efficient

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76
Q

Radioisotopes used to trace the path of the atoms of an element in a chemical or biological process.

A

Tracers

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77
Q

Radioactive application to sterilize food of bacteria

A

Food irradiation

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78
Q

What was Melvin Calvin was known for his study of?

A

photosynthesis

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79
Q

Molecular fragments having one or more unpaired electrons; they are usually short-lived and highly reactive

A

Radicals

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80
Q

The difference between the mass of an atom and the sum of the masses of its protons, neutrons, and electrons

A

Mass defect

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81
Q

Chemical for smell and taste

A

Rhodopsin

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82
Q
A

gamma-rays < 10-12 m
x-rays 1 nm - 1 pm
ultraviolet 400 nm - 1 nm
visible 750 nm - 400 nm
near-infrared2.5 μm - 750 nm
infrared 1013 - 1014 25 μm - 2.5 μm
microwaves 31011 - 1013 1 mm - 25 μm
radio waves < 31011 > 1 mm

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83
Q

What is the wavelength of the various colors?

A

*Tip: start from 700, 50 nm each:
R 650-700 nm
O 600-650 nm
Y 550-600 nm
G 500-550 nm
B 450-500 nm
V 390-450 nm

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84
Q

Property that differentiates types electromagnetic radiation

A

energy

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85
Q

Differentiate Empirical and Molecular Formula

A

Molecular Formula: actual number of each atoms in a molecule
Empirical Formula: relative amounts of bonds formed in a molecule

Example:
Benzene: MF- C6H6 EF - CH
Acetylene: MF - C2H2 EF - CH

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86
Q

When do certain radioactive decay occur?

A

a) None - magic # (2, 8, 20, 28, 82, 20, 50, 126)
b) Alpha decay: proton > 83
c) Spontaneous fission: [p > 89 OR m > 200]
c) Beta decay - n/p > 1.0
d) Positron emission - n/p < 1.0 but smaller atoms (p = 1 to 40)
e) Electron capture: n/p < 1.0 but bigger atoms (p = 41 to 82)
f) Gamma Decay: to stabilize metastable nuclides

https://www.geigercounter.org/radioactivity/table-of-nuclides.gif

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87
Q

Describe band of stability

A

Region in which stable nuclides lie in n vs p plot.

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88
Q

Enumerate Mass and Charge:
Alpha Decay
Beta Decay
Gamma Emission
Positron Emission
Electron Capture

A

—Alpha Decay (He)
Mass: 4 Charge: +2
—Beta Decay (e- in product)
Mass: 0 Charge: -1
—Positron Emission
Mass: 0 Charge: +1
—Electron Capture (e- in reactant)
Mass: 0 Charge: -1
—Gamma Decay
Mass: 0 Charge: 0

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89
Q

What is the effect of alpha, beta and gamma particles to mass number?

A

(4,0,0)

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90
Q

Resulted from the decay of a neutron into an electron and a proton

A

beta decay

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91
Q

Resulted from the conversion of a proton into a neutron

A

Positron emission and electron capture

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92
Q

Decay that resulted from almost all other types of radioactive decay

A

Gamma emission

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93
Q

Describe and Rank Penetration and Biological Effects of Alpha, Beta and Gamma

A

alpha particles: lowest penetration, highest biological effect (only upon ingestion and inhalation)

beta particles: middle penetration and biological effect. Require specialized metal clothing. Very painful

gamma rays: highest penetration, lowest biological effect. External gamma source very dangerous

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94
Q

Why alpha particle have highest biological effect and gamma radiation have highest penetration?

A

Alpha particles are massive and highly charged, which means that they interact with matter most strongly
Gamma radiation is neutral and massless thus interact least with matter but penetrate most.

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95
Q

in general, the penetrating power is ____ proportional to the mass, charge, and energy of the emission

A

inversely proportional

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96
Q

By far the most dangerous and harmful form of radiation

A

Gamma rays

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97
Q

What is the difference between an alpha particle and a proton?

A

A proton is a positively charged species found in the nucleus of the atom.
An alpha particle is a positively charged helium ion.

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98
Q

What are Transuranium elements

A

p > 92
- artificial elements synthesized via nuclear transmutation

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99
Q

A parent nuclide may undergo a series of decay steps before a stable daughter nuclide forms.

A

Decay Series or
Disintegration series

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100
Q

Explain how to determine Decay Series given a nuclide specie.

A

Main Formula: (M,parent - M,given)/4
Pick which series yields a whole number

Decay Series–Parent–Daughter
Uranium——–U-238 Pb-206
Actinium——–U-235 Pb-207
Thorium———Th-232 Pb-208
Neptunium—–Np-237 Tl-205
Plutonium——Pu-239 U-235

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101
Q

Parent, Last Daughter, Natural?
Uranium series

A

U-238 to Pb-206, natural

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102
Q

Parent, Last Daughter, Natural?
Actinium series

A

U-235 to Pb-207, natural

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103
Q

Parent, Last Daughter, Natural?
Thorium series

A

Th-232 to Pb-208, natural

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104
Q

Parent, Last Daughter, Natural?
Neptunium series

A

Np-237 to Tl-205, artificial

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105
Q

Parent, Last Daughter, Natural?
Plutonium series

A

Pu-239 to U-235, artificial

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106
Q

Who discovered positron?

A

Carl David Anderson

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107
Q

Strong nuclear force

A

A force of attraction present between nucleons (proton and neutrons) over and extremely short distance of about 10^-15 m

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108
Q

It overcomes electromagnetic forces over short distances

A

Strong nuclear force

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109
Q

It serves as a nuclear binder of neighboring protons despite the electric repulsion of positive charges but only over short distances

A

Neutrons

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110
Q

Instrument to measure radiation

A

Geiger counter and chamber

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111
Q

What does the Geiger counter count and what compound does it use?

A

a) count alpha particles; with argon
b) count neutrons; with BF3

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112
Q

How is the Sun and Nuclear Fusion connected?

A

H2 atoms combine into heavier elements

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113
Q

A sequence in which one radioactive nucleus decays to a second, and so forth.

A

Radioactive Decay Series

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114
Q

Explain Transmutation

A

-Ernest Rutherford
- The nuclei of an atom will undergo transformation when bombarded with a nuclear species

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115
Q

Nucleus in an excited state with a lifetime of at least one nanosecond

A

Metastable nucleus

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116
Q

Ionization counter that count particles emitted by radioactive nuclei, consists of a metal tube filled with gas, such as argon.

A

Geiger counter

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117
Q

Device that detects nuclear radiation from flashes of light generated in a material by the radiation.

A

scintillation counter

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118
Q

What is a phosphor?

A

Part of scintillation counter
Substance that emits flashes of light when struck by radiation

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119
Q

What does the scintillation counter count and what chemical does it use?

A

a) count alpha particles; with zinc sulfide (ZnSO4)
b) count gamma particles; with Sodium Iodide (NaI) w/ Thallium Iodide (Th(I)I2)

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120
Q

Emission spectrum of hydrogen when an electron jumps to or from “n” energy level

A

Hydrogen Spectral Series

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121
Q

Enumerate Hydrogen Spectral Series

A

LandBank of the Philippines, BRo Pasabay Ha
(1)Lyman-UV,
(2)Balmer-visible light,
(3)Paschen-infrared,
(4)Brackett,
(5)Pfund,
(6)Humphreys

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122
Q

The fundamental number of hydrogen.

A

Balmer constant
3645.6 Angstrom

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123
Q

1 Angstrom is equal to __ meters

A

1 A = 1*10^-10 m

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124
Q

Made a mathematical model explaining the observed frequencies for Hydrogen Spectral Lines

A

Johannes Balmer

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125
Q

Describe Ground and Excited state

A

-Ground state – most stable energy level of electron

-Excited state – energy level in which electrons emit photons

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126
Q

Roentgen (R)

A

The amount of radiation delivered from a radiation source

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127
Q

Defined as one disintegration per second

A

becquerel (Bq)

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128
Q

Curie (Ci)

A

-Disintegration rate og 1 gram of Radium
Unit of activity equal to 3.7* 10^10 disintegrations per second.
1 Ci = 3.7* 10^10 Bq

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129
Q

Describe Gy (Gray)

A

Dosage of radiation that deposits 1 J/kg absorbing material
“Radiation dose with equal biological effect to 1 Gray of gamma radiation”

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130
Q

Dosage of radiation that deposits 0.01 J/kg tissue.

A

rad
(from Radiation Absorbed Dose)

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131
Q

Relationship of Gray and rad

A

1 Gy = 100 rad

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132
Q

Unit of radiation dosage used to relate radiation in terms of biological effects.

A

rem
(roentgen equivalent for man)

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133
Q

Sievert

A

1 Sv = 100 rem

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134
Q

Relation between rad and rem

A

rem = rad * RBE
where RBE = relative biological effectiveness

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135
Q

Why most stable radionuclide is approximately at Atomic number=60?

A

It has highest binding energy per nucleon = most stable

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136
Q

Relative Biological Effectiveness (RBE) Values

A

RBE
1 = x-ray, gamma, beta
3 = slow neutron
10 = fast neutron, proton
20 = alpha

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137
Q

Explain Ionizing Radiation

A

Energetic α, β, and γ particles that dislodged e- from atoms or molecules, forming free radicals, that can be highly damaging to cells

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138
Q

What is Avogadro’s Number?

A

Amedeo Avogadro
const 24
- number of molecules in 12 grams of Carbon-12

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139
Q

Enumerate Periodic Trends

A

INCREASE DOWN-LEFT:
Atomic Radius, Reactivity, Metallic Property
DECREASE DOWN-LEFT:
Ionization Energy, Electron Affinity, Electronegativity

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140
Q

Explain Atomic Radius

A

-Average distance between the nucleus and the valence electron

  • or! one-half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule .
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141
Q

Describe Ionic Radius (with behavior)

A

-radius of cation or anion
-add electron: increased repulsion enlarges electron cloud
-remove electron: electron cloud shrinks or remain the same

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142
Q

Explain Ionization Energy

A

-Energy required to remove an electron from a gaseous atom in its ground state

-higher ionization energy: harder to form positive ions

143
Q

Explain Electron Affinity

A

-Negative of energy change when gaseous element accepts an electron

HOW WELL ATOM CAN KEEP ITS ELECTRONS

-NONMETALS: higher electron affinity: negative ion more stable

-accept electron: negative electron affinity
-emit electron: positive electron affinity

144
Q

Explain Electronegativity

A

-Ability of an atom to attract bonding electron towards itself
-high electronegativity atoms tend to attract low electronegativity atoms (eg. Na+ and Cl-)

145
Q

Measured the Electronegativities of elements

A

Linus Pauling
(Pauling Scale)

146
Q

Calculator Constant:
Rydberg constant, R

A

const 16

147
Q

Calculator Constant:
Lightspeed, C0

A

const 28

148
Q

Calculator Constant:
Plank’s constant, h

A

const 06

149
Q

Calculator Constant:
Finite-Structure constant

A

const 10

150
Q

How is boiling point of liquids affected by elevation?

A

-dP/dz = density*g
higher elevation = lower external pressure = lower boiling point

151
Q

Most effective bulletproof vest

A

Polyethylene Fiber
or Ultra-High Molecular Weight Polyethylene (UHMWPE)

152
Q

Used in bulletproof vest (2nd choice)

A

Polyamide Fibers
or Kevlar

153
Q

Used in bulletproof windows.

A

Polycarbonate Fibers

154
Q

Used as construction material for radiation protection.

A

Polymethacrylate Fiber

155
Q

Material that Impede:
Alpha particles

A

any material

156
Q

Material that Impede:
Beta particles

A

> 0.25 mm aluminum

157
Q

Material that Impede:
strong Beta Particles

A

6-12mm Lucite or Plexi Glass

158
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 out portions of the room housing the fuel rods. If the radiation coming from the fuel rods would be a strong beta emission, which material should be utilized?

A

8.0 mm Lucite

159
Q

Radiation produced after beta particle struck high atomic number materials, such as metals

A

Bremsstrahlung radiation

160
Q

Material that Impede:
Fast neutron

A

water, paraffin (alkane/ sat’d hydrocarbon), concrete

161
Q

Material that Impede:
Gamma radiation

A

Lead

162
Q

Material that Impede:
Slow neutron

A

Cadmium

163
Q

Geochronological Methods:
Enumerate Dating Pairs

A

a) K-40 and Ar-40
b) Th-232 and Pb-208
c) U-238 and Pb-206

164
Q

“Matter is composed of indivisible particles called atoms”

A

Democritus

165
Q

Explain Dalton’s Atomic Theory

A
  1. Matter made of indivisible “atoms”
  2. Same element = Same properties.
  3. Compounds = combination of atoms
  4. Molecules =tightly bound combination of atoms
166
Q

Law of Conservation of Mass

A

Antoine Lavoisier
Matter cannot be created nor destroyed, only transformed

167
Q

Law of Definite Composition

A

Joseph Louis Proust
regardless of extensive amount, the %composition of compounds is constant

168
Q

Law of Multiple Proportions

A

John Dalton
Atoms tend to form bonds in whole number integers

169
Q

Used to identify molecular mass (actual MW) of compounds.

A

Platinichloride Method
2B + H2PtCl6 (Chloroplatinic acid) –> B2H2PtCl6 (Platinichloride salt)

170
Q

Contributions of JJ Thomson

A

-Discovered electrons by analyzing cathode rays
-Plum pudding model

171
Q

Cathode Ray Experiment

A

JJ Thomson
determined the electron mass to charge ratio

172
Q

Color of light from cathode ray experiment

A

Green

173
Q

Named the “electron”

A

George Stoney

174
Q

Oil-drop Experiment

A

Robert Millikan
Determined charge of an electron up to 5 significant sigures

175
Q

Discovered x-ray

A

Wilhelm Conrad Roentgen

176
Q

Ernest Rutherford Contributions

A

Discovered the nucleus
Atomic Model
Transmutation

177
Q

Contribution of James Chadwick

A

Discovered NEUTRON
-Bombarding beryllium atom with alpha particles to produce a neutral particle with mass slightly greater than proton

178
Q

Planetary Model

A

AKA Bohr Model
e- revolves around the nucleus

179
Q

Catalyzed the discovery of the proton

A

Geiger-Marsden Experiment or Golden Foil Experiment

180
Q

Father of Quantum Theory

A

Max Planck

181
Q

Differentiate Classical Physics vs Quantum Mechanics

A

Classical Physics - system may possess infinite energy
Quantum Mechanics - system may only possess only finite and definite amounts of energy

182
Q

Contribution of Henry Gwyn-Jeffreys Moseley

A

Relationship between atomic number and the frequency of X-Rays generated by bombarding the element with high energy electrons.

183
Q

Explained the photoelectric effect by treating light as a stream of particles called photons

A

Einstein

184
Q

What is the Photoelectric Effect?

A

The ejection of electrons from the surface of a metal or from another material when light shines on it

185
Q

Explain Wave-Particle Duality

A

Light acts as wave when in transit
Light as a particle (photon) when hitting subatomic particles

186
Q

Explain Work Function

A

Energy that binds e- to a metal surface

187
Q

Define Threshold Frequency

A

Minimum frequency of light required to initiate photoelectric effect

188
Q

Explain effect of light hitting a metal surface at differing frequencies

A

Photoelectric effect happens if light frequency is equal (but V=0) or more than threshold frequency (where electron gets knocked out of surface)

189
Q

What is de Broglie’s Wavelength?

A

lambda = h/mv
-wavelength of any particle of mass, m
-“matter behaves as though it moves in a wave.”

190
Q

Electron beams were diffracted by these crystals which proved de Broigle’s idea

A

NaCl (Sodium chloride) crystals

191
Q

Common Velocities:
alpha particles
beta particles
gamma rays

A

alpha particles: 1/20 C
beta particles: 9/10 C
gamma rays: C

192
Q

Define Internal Energy

A

cumulative energy that each particle of a system possess

193
Q

What is the relationship of Internal Energy to Heat and Work?

A

dU = Q+W
Q and W exists in transit
U is the energy after the transfer of Q and W

194
Q

Discovered ten transuranium elements

A

Glenn Seaborg

195
Q

Arranged elements in triads

A

Johann Wolfgang Dobereiner

196
Q

“Every 8 element has similar properties”

A

Law of Octaves
John AR Newlands

197
Q

Father of Periodic Table

A

Dmitri Mendeleev

198
Q

What was the basis for Mendeleev classification of elements?

A

Atomic weight

199
Q

Differentiate Atomic weight, Formula Weight and Molecular Weight

A

Atomic: average mass based on abundance of isotopes
AW = sum(x*m,isotope)
Formula: for both ionic and covalent
Molecular: for covalent only

200
Q

Proposed to arrange the elements by their atomic masses, independent of the work of Dmitri Mendeleev

A

Lothar Meyer

201
Q

What kind of elements occupy maximum in the Lothar Meyer curve?

A

Alkali metals

202
Q

Most abundant element in the Earth’s crust, waters and atmosphere

A

Oxygen

203
Q

Most abundant element in the universe

A

Hydrogen

204
Q

Metals that melt on the palm of the hand due to its melting point

A

Gallium and Cesium

205
Q

Metal with the highest melting point

A

Tungsten

206
Q

Metallic elements are often obtained from ores. Name the metallic element which is produced from the ore Bauxite.

A

Aluminum

207
Q

The noble gases have low boiling points because ____

A

Only weak Van der Waals forces hold the atoms together

208
Q

Produced urea from ammonium cyanate

A

Friedrich Wohler

209
Q

Produced soaps from various fatty acids and alkalis this he was able to demonstrate a chemical change w/o the vital force

A

Michel Chevreul

210
Q

Produced acetic acid from carbon disulfide

A

Adolf Wilhelm Hermann Kolbe

211
Q

Discovered the structure of benzene

A

Friedrich August Kekule

212
Q

“Carbon is tetravalent”

A

Friedrich August Kekule & Archibald Scott

213
Q

“Carbon is tetrahedral”

A

Jacobus van’t Hoff

214
Q

Octet Rule

A

-Gilbert Lewis
-tendency of atoms to prefer to have 8 electrons in the valance shell

215
Q

Heisenberg uncertainty principle

A

Werner Heisenberg
“It is impossible to determine simultaneously both the position and velocity of an electron or any other particle.”

216
Q

Contributions of Erwin Schrodinger

A

Developed a mathematical model for WAVE FUNCTION, for particles exhibiting wave-like properties

217
Q

Aufbau Principle
Exceptions

A
  • Building-up Principle
  • Electron fill lowest energy orbitals first before higher ones
  • EXCEPTION: Cr and Cu
218
Q

Pauli Exclusion Principles

A

Wolfgang Pauli
“No two electrons have the same values of quantum numbers”

219
Q

Describe Paramagnetic and Diamagnetic substances

A

-Paramagnetic substances contain net unpaired spins and are attracted by a magnet.
-Diamagnetic substances do not contain net unpaired spins and are slightly repelled by a magnet.

220
Q

Enumerate Linus Pauling’s contributions

A

Postulated important concepts:
-Hybridization
-Molecular Orbital Theory
-Nature of chemical bonds
-Resonance

221
Q

Describe Resonance, Resonance Hybrid and Contributing Resonance

A

Resonance: the use of two or more Lewis structures to represent a particular molecule. (eg. Benzene)
Resonance Hybrid: composite of several contributing structures
Contributing Resonance: resonance stuctures that differ in distribution of valance electrons

222
Q

Represents the various ways a molecule can be drawn

A

Lewis structures

223
Q

Represents the true structure of the molecule

A

Resonance hybrid

224
Q

Describe Hybrid Orbitals and Hybridization

A

Hybrid Orbitals: atomic orbitals obtained when two or more nonequivalent orbitals (eg, s and p orbitals becomes sp, sp2, etc) of the same atom combine in preparation for covalent bond formation.

Hybridization: mixing of atomic orbitals in an atom (usually a central atom) to generate a set of hybrid orbitals.

225
Q

Why radicals are very reactive?

A

-Radicals tend to UNPREDICTABLY form covalent bond with another radical

226
Q

Valence Bond Theory

A
  • Bond formation is due to the overlap of two atomic orbitals
  • Bond length to minimize the electrons and nuclei repulsion, while satisfying attractive forces.
  • Energy released when bond formed, absorbed when bonds break.
227
Q

Describe Molecular Orbital Theory

A

-Linus Pauling
- Bonding molecular orbital: region where e- are in between two nuclei
- Antibonding molecular orbital: region where e- are away from either nuclei. Adding e- here will make bonds more unstable.

228
Q

According to Molecular Orbital Theory, placing electrons in a bonding molecular orbital yields ___ whereas placing electrons in an antibonding molecular orbital results in ___

A

Bonding: Yields stable covalent bonds
Antibonding: unstable bond

229
Q

Relate Bond Order, Strength, Energy

A

Higher order = More bonds = Higher strength = More energy required to break

230
Q

___ Rule of Multiplicity

A

-Hund’s Rule
-lowest energy (MOST STABLE) electron arrangement is one with highest number of parallel spin (=up-down spin)
- minimize repulsions of electrons

231
Q

Hund’s Rule:
Describe Paramagnetic and Diamagnetic substances

A

Paramagnetic - has unpaired electron spin/s. Attracted by magnets.
Diamagnetic - all electrons are paired. Slightly repelled by magnets.

232
Q

The region in space where an electron is most likely to be found is called ______

A

orbital

233
Q

Define bond order

A

number of bonds between atoms

234
Q

VSEPR

A
  • Ronald Nyholm
  • Valance Shel Electron Pair Repulsion
  • “Atoms achieve geometry that minimizes repulsion between electrons in valence shell”
235
Q

Fajan’s Rule

A
  • Kazimerz Fajans
  • Predicts whether a bond is covalent or ionic based on ionic & atomic radii
  • Covalent: high positive charge, small cation, large anion (very polarizable)
  • Ionic: low positive charge, large cation (very polarizable), small anion
236
Q

Predict bond type using electronegativity difference
Non-polar covalent
Polar Covalent
Ionic

A

Non-polar covalent: Less than 0.5
Polar Covalent: 0.5 to 1.9
Ionic: Greater than 1.9

237
Q

The compound formed by the combination of positive and negative ions

A

ionic compound

238
Q

The most common occurrence of this bond occurs between two nonmetals or between a nonmetal and a metalloid.

A

covalent bonds

239
Q

A bond in which electrons are shared between elements having a difference in electronegativity of between 0.5 and ~2.0

A

polar covalent bond

240
Q

Covalent bond in which the bonding electrons are not shared equally

A

polar covalent bond

241
Q

Covalent bond in which the bonding electrons are shared equally

A

nonpolar covalent bond

242
Q

Define Bonding electrons

A

Bonding electrons: shared valance electrons involved in covalent bond formation

243
Q

Define Nonbonding electrons

A

Valence electrons not involved in forming covalent bonds; that is, unshared electrons

244
Q

Electrostatic force that holds ions together in an ionic compound.

A

Ionic bond

245
Q

Energy required to completely separate one mole of a solid ionic compound into gaseous ions

A

Lattice energy

246
Q

Measure of the stability of an ionic solid.

A

Lattice energy

247
Q

Lattice energy is dependent on ___ and ___

A

Coulomb’s Law
Pot. Energy (E) = kQ1Q2/r
Force (F) = kQ1Q2/r^2

  1. Charge of ions (Q1, Q2)
  2. Distance between ions (r)
248
Q

Predict Molecular Shapes based on # Regions of Electron Density Around Central Atom:
-Tetrahedral
-Trigonal Planar
-Linear
*Also predict their bond angles

A

*Tetrahedral: 4, 109.5 deg
*Trigonal Planar: 4, 120 deg
*Linear: 4, 180 deg

249
Q

Differential Metals, Nonmetals, and Metalloids

A

Metal: solid that is shiny, conducts electricity, is ductile and malleable, and forms alloys. Tend to loose electrons
Nonmetal: does not have metallic properties. Tend to accept electrons
Metalloids: display some properties of metals and nonmetals

250
Q

Combination of two or more atomic orbitals to form the same number of hybrid orbitals each having the same shape & energy

A

Hybridization

251
Q

The pull of electron density through sigma bonds caused by electronegativity differences of atoms

A

Inductive Effects

252
Q

Atom or group of atoms responsible for the characteristics of organic compounds.

A

Functional Groups

253
Q

Dictate the 3 Water Solubility Rules

A
  1. ALWAYS SOLUBLE:
    AANG
    (Acetate, Ammonium, Nitrates, Group 1 cations)
  2. INSOLUBLE HALIDES:
    PuMaSa
    (Pb2+, Mercury, Silver)
  3. INSOLUBLE SULFATE: BA-CA SR. PoliceMan Siya (Ba2+, Ca+2, Sr2+, Pb2+, Mercury, Silver) (BaCaSrPMS)
  4. SOLUBLE OH-:
    Group 1 cations, and Ba,2+
  5. SOLUBLE CARBONATE, PHOSPHATE, CHROMATES, SULFIDES: (CarPho ChromSu):
    Group 1 cations, and ammonium (NH4+)
254
Q

Given combination of solution Ag2CO3 and CaCl2, NaCl2 and PbSO4. Which of the ff. will form precipitate?

A

Ag2CO3

255
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

(1) Physiological saline solution : homo
(2) Orange juice : hetero
(3) A cloud : colloidal
(4) Wet sand : hetero
(5) Suds : colloidal
(6) Milk : colloidal

256
Q

Homogeneous mixtures of
solids

A

alloys

257
Q

The chemical nature of an element is independent of _____

A

the number of neutrons present in it.

258
Q

Gases diffuse faster compared to liquids because of the reason that the liquid molecules are ____

A

are held together by stronger inter-molecular forces.

259
Q

Atoms of the same element, but of different masses are called

A

isotopes

260
Q

Describe Kirchhoff’s law

A

Temperature dependence of a reaction enthalpy
Cp = sum (vCp,m)
dH,r = Cp,rdT

261
Q

Describe Hess’ Law

A

“The standard reaction enthalpy is the sum of the values for the individual reactions into which the overall reaction may be divided.”

dH,r = sum (v*dH,f)

262
Q

Redox reactions in which the compounds or mixtures that are burned are oxidized by oxygen.

A

Combustion

263
Q

Breathed oxygen oxidizes carbon containing compounds to produce CO2 and H2O

A

Respiration

264
Q

Oxidation of iron

A

Rusting

265
Q

Bleaches are very strong ____ agents

A

Oxidizing agents

266
Q

Process that converts nitrogen in atmospheric air into ammonia for fertilizers

A

Haber process

267
Q

Kb and Kf of Water

A

Kb = 0.52 C/m
Kf = 1.86 C/m

268
Q

Kb and Kf of Benzene

A

Kb = 2.53 C/m
Kf = 5.12 C/m

new values…
Kb = 2.61 C/m
Kf = 5.07 C/m

269
Q

Kb and Kf of Ethanol

A

Kb = 1.22 C/m
Kf = 1.99 C/m

270
Q

Kb and Kf of Acetic Acid

A

Kb = 2.93 C/m
Kf = 3.90 C/m

271
Q

Kb and Kf of Cyclohexane

A

Kb = 2.79 C/m
Kf = 20 C/m

272
Q

Kb and Kf of Camphor

A

Kb = ~
Kf = 40 C/m

273
Q

Constant volume calorimeter

A

Bomb calorimeter

274
Q

Constant pressure calorimeter

A

Adiabatic flame calorimeter

275
Q

The observation that real gases at the same reduced volume and reduced temperature exert the same reduced pressure

A

Principle of Corresponding States

276
Q

Gives the fraction of molecules that have speeds in a specified range.

A

Maxwell–Boltzmann distribution of speeds

277
Q

Known as limiting gas laws (lim P–>0)

A

Boyle’s and Charles’ laws

278
Q

To increase the life of an incandescent lamp, it is ______

A

filled with argon gas

279
Q

Time to develop antibodies for foreign substance

A

1 to 2 weeks

280
Q

If the entropy of a system decreases, the entropy of its surroundings must _____

A

Must always increase
(for dS,univ>0)

281
Q

The enzyme capsaicin is commonly found in ____

A

Capsacium

282
Q

When does the ff IMFA exist:
Van der Waals
Dipole-Dipole
Hydrogen Bonding

A

Assume multiple of the given molecule exists
VdW: every time
DD: molecule capable of having + and - poles. Check if forces cancel (eg: CCl4)
H-Bond:
a) one molecule have H atom bounded to N,O,F
b) the other molecule have one lone pair in its N,O,F

283
Q

What is Polarizability?

A

Tendency of atom to redistribute its electrons in the presence of a positive pole

284
Q

Factors that Affect Polarizability

A

-Atomic Radii - directly proportional. Left Down the PT
-Atomic Mass - if radii not in the choices
-Surface Area - directly proportional

285
Q

Affected by Polarizability

A

Directly proportional to: boil pt, melt pt, surface tension, viscosity
Inversely proportional to: vapor pressure

286
Q

How to compare molecule properties using IMFA?

A
  1. Determine strongest IMFA
  2. If diff strongest: compare using them
  3. If same strongest: use Polarizability, if failed then compare the remaining IMFA
287
Q

Entropy

A

-discovered and explained by Rudolf Clausius
-defined by Boltzmann

288
Q

Entropy Definition

A

-defined by Ludwig Boltzmann
-thermodynamics property that measures the number of meta-states of system energy
-used to determine spontaneity of process using the UNIVERSE

289
Q

Process that Increase Entropy

A

INCREASED TOTAL ENERGY
-Increase Temperature
INCREASES MOBILITY
-Phase Transition (to less dense phase)
-Dissolution of solute
-dn=(c+d)-(a+b) : change in moles of gas after reaction
-Mixing of gasses: mix will increase the space each species can occupy

290
Q

Gibbs Free Energy

A

G=H-TS
-Josiah Willard Gibbs
-used to determine spontaneity of process using SYSTEM ALONE

291
Q

Define the Colligative Propeties

A

Colligative Props: change in solvent properties depending only on solution concentration and solvent nature

BPE/FPD: increase/decrease in BP/FP

Osmosis: selective passage of solvent molecules through porous membrane from dilute to more concentration part. Levels of each compartment will be unequal

292
Q

Explain Osmotic pressure

A

External pressure applied to the more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane.
- external pressure to equal the levels of each compartment

293
Q

When we apply pressures greater than the osmotic pressure to the more concentrated solution, solvent flows from the more dilute solution to the more concentrated solution

A

reverse osmosis

294
Q

Describe Effusion and Graham’s Law

A

-Thomas Graham
-Effusion: process by which a gas under pressure escapes from one compartment to another through a small opening
- rate inversely prop. to sqrt(MW)

295
Q

Explain Kinetic Molecular Theory

A
  1. KE proportional to Temp
  2. Perfectly elastic collisions (momentum conserved).
  3. IMFA negligible
  4. Gas molecules negligible compared to distances between other molecules
  5. Pressure is from collision of gas molecules to container walls
296
Q

Following are pH ranges for several human biological materials. From the pH at the midpoint of each range, calculate the corresponding [H3O -]. Which materials are acidic?
(1) Milk, pH 6.6–7.6
(2) Gastric contents, pH 1.0–3.0
(3) Spinal fluid, pH 7.3–7.5
(4) Saliva, pH 6.5–7.5
(5) Urine, pH 4.8–8.4
(6) Blood plasma, pH 7.35–7.45
(7) Feces, pH 4.6–8.4
(8) Bile, pH 6.8–7.0

A

Acidic materials (pH <7.0 based on midpoint):
(2) Gastric contents: pH=2
(5) Urine: pH=6.6
(7) Feces: pH=6.5
(8) Bile: pH=6.9

297
Q

Water on heating from 1 to 4°C

A

contracts

298
Q

This law explains why aerosol cans carry the warning “Do not
incinerate”.

A

Gay-Lussac Law

Can —> involves pressure
Incinerate –> involves temperature

299
Q

Laughing Gas

A

NO, Nitric Oxide

300
Q

Important element to prevent tooth decay

A

Fluoride

301
Q

The instrument used to measure blood pressure

A

sphygmomanometer

302
Q

Binds to hemoglobin so that O2 cannot be taken up to the lungs

A

CO, carbon monoxide

303
Q

Aims to imitate the same filtration function as kidneys

A

Hemodialysis

304
Q

Happens for diver when they ascend too rapidly, dissolved N2 creates bubble

A

Nitrogen Narcosis

305
Q

pH of normal rain and acid acid

A

normal rain: 5 to 5.5
acid rain: 4.0

306
Q

Typical human blood pH range

A

7.35 to 7.45

307
Q

Typical pH of gastric juices

A

1.0 - 2.0

308
Q

Condition when blood pH is below 7.35 to 7.45 that leads to depression of the nervous system.

A

Acidosis

309
Q

Condition when blood pH is higher than 7.45 that leads to overstimulation of the nervous
system, muscle cramps, dizziness, and convulsions.

A

Alkalosis

310
Q

Scientists that theorized that CFCs destroy the atmospheric ozone

A

Paul Crutzen, Sherwood Rowland and Mario Molina

311
Q

What happened when we lower our diaphragm during breathing?

A

BOYLE’S LAW
*Lower Diaphragm: Increased volume = Lower pressure = Air tends to enter the lungs
*Raise Diaphragm: decreased volume = increased pressure = exhale

312
Q

Also known as Boyle’s Law

A

Mariotte’s Law

313
Q

Which gas law explains hot air balloon? How?

A

CHARLES’ LAW
*Increased Temp = Increased volume = Decreased air density = LIFT!

314
Q

What is Proof? (alcohol concentration)

A

Proof = 2* (%v/v alcohol content)

315
Q

Invented Vulcanized Rubber

A

Charles Goodyear

316
Q

Sound travels faster during the day or night?

A

Night

317
Q

Number of Carbon atoms in Olvanil

A

26

318
Q

Primary use of ethylene

A

ripening of fruits

319
Q

What is Ozoloysis

A

Alkenes, alkynes and azo compounds are cleaved with ozone

320
Q

Solid Part of the Earth

A

Lithosphere

321
Q

What is Nujol Mull?

A

A way to obtain infrared spectra of solids

322
Q

Discovered zeolites

A

Cronstedt

323
Q

The Nobel Prize for radioactivity discovery was shared between Curie and Roentgen. Who coined the word “Serendipity” in 1754?

A

Horace Walpole

324
Q

Contribution of Adolf von Baeyer

A

Phenolphthalein and Barbituric Acid

325
Q

Discovered EDTA

A

Ferdinand Munz

326
Q

Use of EDTA

A

Bind metal ions in Chelation therapy
Treating Hg and Pb poisoning

327
Q

Process on how to differentiate alkane, alkenes and alkynes

A

Reaction with Br2

328
Q

Other name for taurine

A

2-AminoEthylSulfonic Acid
2-AminoEthane Sulfonic Acid

329
Q

_____ is an organic compound that is widely distributed in animal tissues. It is a major constituent of bile and can be found in the large intestine, and accounts for up to 0.1% of total human body weight. It was first isolated from ox bile in 1827 by German scientists Friedrich Tiedemann and Leopold Gmelin.

A

Taurine or 2-aminoethanesulfonic acid

330
Q

Component of sunblock that helps reflect light

A

Zinc Oxide

331
Q

Temperature of the moon at day and night

A

Day: 127C
Night: -173C

332
Q

What makes plastics or polymers biodegradable?

A

Hydrophilicity

333
Q

*Shale oil is a high-quality ______ that lies between layers of shale rock, impermeable mudstone, or siltstone. Oil companies produce shale oil by fracturing the layers of rock that contain the layers of oil.
*____ is rock suffused with kerogen, a precursor to oil. In some cases, shale oil describes oil that’s been converted from kerogen in shale rocks.

A

crude oil, oil shale

334
Q

Brix scale is the hydrometer scale for ______

A

sugar solution

335
Q

Is a brand of mineral oil by Plough, Inc. CAS number 8012-95-1, and density 0.838 g/mL at 25 C, used in IR spectroscopy. It is a heavy paraffin oil so it is chemically inert and has a relatively uncomplicated IR spectrum, with major peaks between 2950-2800, 1465-1450, and 1360-1300 cm^-1.

A

Nujol Mull

336
Q

Liquid part of the blood that remains after removal of the cellular particulates and fibrinogen.

A

Blood serum

337
Q

Most oxidized form of nitrogen

A

Nitrates

338
Q

The distance of the Earth to the most remote normal galaxy is calculated to be:

A

2x10^22 m
(yung choice puro 2)

339
Q

Which do float?
balsa wood
ethylene glycol
table salt
ethanol

A

balsa wood

340
Q

Which is a synthetic dye?
alizatrin
melanin
carotenoid

A

Carotenois

341
Q

What is the polymer used for printing and coating?

A

Acrylic and Styrene
Acrylic Emulsion

342
Q

Example of pseudo plastic fluid
apple sauce
rubber latex
tap water
sewage sludge

A

apple sauce

343
Q

Product of distillation of coal tar

A

phenol

344
Q

What is the chemical formula and molesular weight of 11-tetradecenyl acetate?

A

C16 H30 O2

345
Q

What is the common contaminant in the BTEX process?

A

benzene, toluene, ethylbenzene and xylene

346
Q

Chouse the common method in the removal of fine particle in how airstream common in cement production

A

Venturi Scrubber

347
Q

What is the meathod that Wohler do to break the vital force theory in nature?

A

Heating of NH4CL with AgCN to from Urea

348
Q

What happens to the pH of carbonated brinks if it open in atmospheric condition?

A

Increase (more basic)

349
Q

Range of melting point of fatty acids
(Saturated, Unsaturated

A

Saturated Fatty Acids: 100-110C
Unsaturated: 70-85C

350
Q

What is the cost common form of nitro-glycerol?

A

Nitroglycerin

351
Q

In stem cell studies, a chemical known as telomeres is attached to the chromosome to promote longer life. How would you apply this as a chemical engineering in the field of agriculture and food?

A

Geneticallyu enhance plants to prolong shelf life

352
Q

Liquid nitrogen is placed in an Erlenmeyer flask. Hardboiled egg is then place on top of the opening, what will happen?

A

Egg will get sucked in
Note: the liquid nitrogen being extremely cold would lower the pressure in the Erlenmeyer, creating a vacuum for the egg to be suctioned in.

353
Q

You are an environmental engineer sent to a place with the cholera epidemic. What is the best thing to do?

A

Treat water supply

354
Q

When will a pine tree grow in Alaska?

A

Not in a million years

ChE LE Flashcards (20 decks)

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