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72 Cards in this Set
- Front
- Back
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Length
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1m = 100cm(exact)
1cm3 + 1cc = 1mL |
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Volume
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1L = 1000mL(exact)
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Mass
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1kg = 1000g(exact)
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Temperature
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F = 1.8(C)+32
K = C+273 |
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Density
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mass of substance/volume of substance
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Significant figures
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.0004 = 1
.075 = 2 85000 = 2 25.0 = 3 5.082 = 4 |
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Desired Quantity
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Given Quantity x one or more conversion factors
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Specific gravity
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density of sample/density of water
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significant figures of multiplication/division
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same number of SFs as the measurement with the fewest SFs
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Energy
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the ability to do work
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Potential energy
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stored energy
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Kinetic energy
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energy of motion
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Heat
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energy that flows from a warmer object to a coller one
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Joule
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small amount of energy
1Cal = 4.184 kJ(exact) = 4184 J 1 kcal = 1000 cal = 1 Cal 1 kJ = 1000 J |
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Specific Heat
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Heat/grams x change in temperature
cal(or J)/1g x 1 C |
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Heat
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mass x change in temperature x specific heat
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Pure substances
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definite composition
Elements and compounds (two or more elements bonded together) |
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Mixtures
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physically mixed, not chemically combined
Homogeneous (uniform, ex: salt water) and Heterogeneous (not uniformed) |
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Chemical properties
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ability of substance to change into a new substance
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physical change
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state or appearance will change but its composition remains the same
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Heat of fusion for H2O
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334J/1 g of H2O
80. cal/1 g of H2O |
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Pure substances
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definite composition
Elements and compounds (two or more elements bonded together) |
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Mixtures
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physically mixed, not chemically combined
Homogeneous (uniform, ex: salt water) and Heterogeneous (not uniformed) |
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Chemical properties
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ability of substance to change into a new substance
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physical change
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state or appearance will change but its composition remains the same
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Heat of fusion for H2O
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334J/1 g of H2O
80. cal/1 g of H2O |
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Heat (HoF)
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mass x heat of fusion
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sublimation
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solid to gas
2590J/1 g of H2O 620.cal/1 g of H2O |
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deposition
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gas to solid
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Heat of vaporization
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Energy that must be added to vaporize one gram of water
2260J/1 g H2O 540cal/1 g H2O |
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Period
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Horizontal
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Groups (family)
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vertical
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Representative elements
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Groups 1A, 2A, 3A-8A
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Alkali Metals
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1A soft, shiny, good conductors or heat/electricity, low melting points
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Alkaline Metals
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2A not as reactive as the Alkali Metals, shiny, good conductors, low melting points
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Halogens
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7A highly reactive and form compounds with most of the elements
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Noble Gases
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unreactive, seldom found in combination with other elements
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Transition elements
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3B-12B
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Metals
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shiny solids, ductile, malleable, good conductors, melt at hight temperatures then nonmetals
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Nonmetals
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poor conductors
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metalloids
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exhibit some properties of both metals and nonmetals
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Atom
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the smallest particle of an element that retains the characteristics of that element
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Subatomic particle
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electrons, protons, neutrons
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electrons
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symbol: e-
Charge 1- Mass: 0.0005 or 1/2000 outside nucleus |
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protons
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symbol: p or p+
charge: 1+ Mass: 1 Nucleus |
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neutrons
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symbol: n
charge: 0 Mass: 1 nucleus |
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Atomic number
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number of protons in an atom
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Mass number
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number of protons + number of neutrons
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Isotopes
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atoms of the same element that have different number of neutrons
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Atomic Mass
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weighted average of the mass of all of the naturally occuring isotopes of that element
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electromagnetic radiation
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emits energy articles called photons
Low energy to high energy big waves to short skinny waves Radiowaves, Radar, Microwaves, Infared, Visible light (red --> violet) Ultraviolet, X rays, Gamma rays, Cosmic rays |
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atomic spectrum
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lines of different colors separated by dark areas
lines in the atomic spectra are changes in energy levels (n=1, n=2...) lower the levels, the closer it is to the nucleus Principal quantum number (n) 1<2<3<4<5<6<7 energy of electrons increased |
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within each energy level there are sublevels
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s, p, d, and f
low energy --> high energy |
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orbitals
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a region in an atom where there is the highest probability of finding an electron.
Max of 2 electrons in an orbital |
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electron configuration
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1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10...
s = group 1, 2 d = transition metals p = group 3A-8A f = everything else |
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valence electrons
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outer-most elevtrons (shell)
Mg = 3s2 2 dots |
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Ionization energy
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the energy needed to remove the least tightly bound electron from an atom in the gaseous state.
energy increases as you move right energy decreases as you move down |
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atomic size
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increase radius as you go down
decrease radius as you move to the right |
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An unstable nucleus is radioactive
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spontaneously emits particles of energy called radiation
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radiation
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alpha, beta, positron, gamma
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alpha
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4/2He
mass: 4 charge: 2+ |
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beta
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(B) 0/-1e
mass: 0 charge: 1- |
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postitron
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(B+) 0/+1e
mass: 0 charge: 1+ |
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gamma
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0/0 y
mass: 0 charge: 0 |
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proton
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(p) 1/1 H
mass: 1 charge: 1+ |
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neutron
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(n) 1/0n
mass: 1 charge: 0 |
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radioactive decay
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Radioactive nucleus--> new nucleus + radiation (beta, alpha, gamma, positron)
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Curie (Ci)
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Activity, becquere (Bq)
1 Ci = 3.7 x 10^10Bq |
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rad
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Absorbed dose, gray (gy)
1 gy = 100 rad |
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rem
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Diological damage, sievert (sv)
1 sv = 100 rem 25 rem = can't be detected 100 rem = temporary dec. in number of with blood cells 300 rem = White blood cell count is 0 500 rem = 50% death 600 rem = 100% death |
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fission
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spliting
1/0n + 235/92U --> 91/36Kr + 142/56Ba + 3 1/0n + energy results in a chain reaction |
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fusion
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two small nuclei combine to from a larger nucleus
3/1H + 2/1H --> 4/2He + 1/0n + energy |
