Chemistry Concepts (Inorganic, Nuclear) Flashcards
Material used in acrylic glass (plexiglass, Lucite, Altuglas)
Polymethacrylate Fiber
Material for bulletproof windows
Polycarbonate Fiber
Material used in the production of Kevlar
Polyamide Fiber
Catalyst used in the production of polyamide fiber
1,4-Diaminobenzene
Material for bulletproof vests
Polyethylene Fiber
Monomer of polyamide fiber
Terephthalic Acid
Catalyst used in the production of polycarbonate fiber
Bisphenol A
Monomer of polycarbonate fiber
Diethyl carbonate
Etymology of Cesium
Latin caesius meaning “sky blue”
Etymology of Rubidium
Latin rubidius meaning “deep red”
Helium was named after _____
Helios, the Greek god of the sun
Element called eka-boron by Dimitri Mendeleev prior to its discovery
Scandium
Element called eka-aluminum by Dimitri Mendeleev prior to its discovery
Gallium
Element called eka-silicon by Dimitri Mendeleev prior to its discovery
Germanium
How many elements in the periodic table are naturally occurring?
88
Four elements that play a major role in the functioning of the human body
C, H, O, N
Element that strengthens bones and aids in blood clotting
Calcium
Most abundant element (by mass) in the human body
Oxygen
Most abundant element (by moles) in the human body
Hydrogen
Two most abundant elements (by mass) in Earth’s crust
Oxygen, Silicon
Element that causes Itai-Itai disease
Cadmium
Element that causes Minamata disease
Mercury
Components of brass alloy
Copper + Zinc
Components of bronze alloy
Copper + Tin
Components of pewter alloy
Tin + Antimony + Lead
What element is called the “metal from heaven” for its presence in meteoroids?
Iron
The only non-metal that can conduct electricity
Graphite
Age of the Solar System
4.6 E9 years old
Unit defined as the electric charge freed by radiation in a specified volume of air divided by the mass of that air
Roentgen (R)
It is the ratio between radiation absorbed by a tissue and radiation delivered to the tissue
Radiation Absorbed Dose (rad)
It is the ratio between the tissue damage caused by a rad of radiation and the type of radiation
Roentgen Equivalent for Man (rem)
Number of isotopes of iodine
37 (I-108 to I-144)
Radioactive nucleus responsible for thyroid cancer
Iodine-131
Radioactive isotope used for kidney scanning
Mercury-197
Radioactive isotope used for heart scans in exercise
Thallium-201
Radioactive isotope used in smoke detectors
Americium-241
Radioactive isotope for cancer therapy
Cobalt-60
Decay product of Radon-222 that produces harmful effects
Polonium-218
Uranium Decay Series
U-238 to Pb-206, Natural
Actinium Decay Series
U-235 to Pb-207, Natural
Thorium Decay Series
Th-232 to Pb-208, Natural
Neptunium Decay Series
Np-237 to Tl-206, Artificial
Plutonium Decay Series
Pu-241 to U-235, Artificial
Radiotracer used in the medical imaging modality positron emission tomography (PET)
18-Fluorodeoxyglycose (FDG)
Ionization counter that uses Argon gas to detect alpha particles
Geiger Counter
What compound is added to the Geiger counter in order to detect neutrons?
Boron Trifluoride (BF₃)
Ionization counter which detects nuclear radiation from flashes of light
Scintillation Counter
Phosphor used in the Scintillation counter to detect alpha particles
Zinc Sulfide
Phosphor used in the Scintillation counter to detect gamma radiation
NaI crystals with TiI₂
Amount of energy deposited by 1 rad per kilogram of matter
1E-2 J energy per kg matter
Material to impede alpha particles
Any material
Material to impede beta particles
0.25 cm Al
Material to impede strong beta particles
6-12 mm Lucite or Plexiglass
Material to impede fast neutrons
Water, paraffin, concrete
Material to impede slow neutrons
Cadmium
Material to impede gamma particles
Thick layer of lead
The only radioation known to have a higher frequency than gamma rays
Cosmic rays
Ghost particle
Neutrino
The unit Curie (Ci) is defined as the amount of decays per second that occur in 1 gram of what radioactive isotope?
Radium-286
Form of energy perceived as a blue glow emitted when electrically charged particles move at speeds faster than that of light in a specific medium
Cherenkov Radiation
Radiation given off by free electrons that are deflected (i.e., decelerated) in a strong electric field particularly when hitting a metal target such as aluminum
Bremsstrahlung (German: “braking radiation”)
Glass tube with 2 metal plates connected to a high-voltage source which emits a ray drawn from the negative plate towards the positive plate
CRT or Geissler Tube
Color of light released in a cathode ray
Green
Phenomenon in which momentum transferred from a photon to an electron accelerates the latter to a new velocity
Compton Effect
Caused by the uneven distribution of intermolecular force around the molecules at the surface of a liquid
Surface Tension
When dissolving organic molecules in a polar solvent, how many carbon atoms can be taken into account by a functional group containing an electronegative atom (i.e., oxygen and nitrogen)?
5 carbon atoms
Extensive property that indicates the quantity of heat needed to raise the temperature of a substance by 1°C
Heat Capacity (C)
Intensive property that indicates the amount of heat required to raise the temperature of 1 gram of substance by 1°C
Specific Heat Capacity (c)
Intensive property that indicates the amount of heat required to raise the temperature of 1 mole of substance by 1°C
Molar Heat Capacity
An inorganic mineral present in human bone and teeth that plays a role in the structural strength of bone and in bone repair and regeneration
Hydroxyapatite Ca₁₀(PO₄)₆(OH)₂
Component in willow trees that are active ingredients in aspirin
Salicin
Chemical for smell and taste
Rhodopsin
Chemical for sight
Retinal
Component of belladonna plants that treats nerve agent and pesticide poisoning
Atropine
Common name of Vitamin A
Retinol
Common name of Vitamin B12
Cobalamin
How many atoms are present in the buckyball?
60 carbon atoms
(12 pentagons, 20 hexagons)
Solid made of giant molecules which can be crystalline, semicrystalline, or amorphous
Polymeric
Solid made of a very large number of atoms connected by covalent bonds
Network
Solid made of randomly arranged atoms or molecules
Amorphous
Examples of polymeric solids
Rubber, plastics, proteins
Examples of network solids
Diamond, quartz
Examples of amorphous solids
Soot, tar, glass
Increase in temperature of the body of water causes a decrease in the sollubility of oxygen leading to the death of aquatic life
Thermal pollution
Formation of nitrogen gas bubbles in the blood as a result of high pressures
Bends
Why is water a good solvent?
Polarity
Hydrogen bonding capacity
Light passing through and scattered by a colloid viewed at a right angle
Tyndall Effect
A system, such as fat in milk, consisting of a liquid with or without an emulsifying agent in an immisible liquid, usually as droplets of larger than colloidal size
Emulsion
Motion of any colloidal particle suspended in a solvent
Brownian Motion
Passage of solvent molecules from dilute solution to a more concentrated solution across a semipermeable membrane
Osmosis
The amount of external pressure applied to the more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane
Osmotic Pressure
Pressure greater than the osmotic pressure is applied to the more concentrated solution so solvent flows from the concentrated solution to the dilute solution
Reverse Osmosis
Process of artificially fixing nitrogen gas from air into ammonia
Haber Process
Process that combines rubber and sulfur at high temperature
Vulcanization
Energy released when one mole of a formula unit is produced by bonding together multiple gas atoms
Crystal Lattice Energy
Method of determining lattice energy
Born-Haber cycle
Effect of uncommon ions in a solution that increases solubility
Salt effect
Effect of a second substance that contains the same ions that can participate in equilibrium
Common ion effect
Effect when Q < Kc
System shifts towards product side
Effect when Q > Kc
System shifts towards reactant side
Theory that states bonds are formed when electrons in the bonding molecular orbital is greater than the electrons in the non-bonding molecular orbital
Molecular Orbital Theory
Theory that states the formation of bond is due to overlap of orbitals
Valence Bond Theory
Gap between the s and p energy bands
Forbidden Zone
Chemical species consumed in an elementary step and produced in another
Intermediate
Hypothetical species between reactants and products
Activated complex
Reaction step with rate law that corresponds to molecularity of reaction
Elementary reaction
Acidity trend along a column in the periodic table
Longer bond = stronger acid
Acidity trend across a row in the periodic table
More polar = stronger acid
TRUE or FALSE: For all adiabatic processes, the entropy change of the system must be zero
False
TRUE or FALSE: For one component systems, it is possible for two phases in equilibrium to have different chemical potentials
False
TRUE or FALSE: The change in Gibb’s free energy can be negative for a cyclic process
False
TRUE or FALSE: A condition for equilibrium is that
(ΔA) T, F = 0
False
TRUE or FALSE: Carbon-14 is continually generated in the upper atmosphere by the production and decay of nitrogen 14
True
TRUE or FALSE: Carbon-14 incorporated into carbon dioxide and the other compounds are distributed worldwide as part of the carbon cycle
True
TRUE or FALSE: The continual formation of carbon-14; transfer of isotope within the oceans, atmospheres and biosphere; and the decay of living matter keep the supply constant
True
What is the common contaminant in the BTEx process?
Sulfur
Chemical used as a plant hormone for ripening of fruits
Ethylene
Other name for lecithin
Phosphatidylcholine
Compound extracted from capsicum
Capsaicin
Other name for alar
Daminozide
Gives crimson red color in flame test
Sr
Gives silver white color in flame test
Al
Gives blue color in flame test
As
Gives bright green color in flame test
B
Gives bright orange color in flame test
C
Gives brick red color in flame test
Ca
Gives blue-green color in flame test
Cu
