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216 Cards in this Set
- Front
- Back
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physical properties
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describes the physical characteristics of a substance
ex: mass, volume,color, ability to conduct electricity |
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chemical properties
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enable a substance to change and describes how a substance reacts with other substances
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0.946 liter
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1 quart
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454 grams
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1 pound
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2.54 centimeters
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1 inch
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SI system
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a worldwide measurement system based on the metric system with minor differences
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heterogeneous mixture
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a mixture whose composition varies from position to position
ex: sand in water |
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homogenous mixture
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also known as a solution
relatively uniform in composition, every portion of the mixture is like the other ex: sugar dissolved in water |
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mixtures
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physical combinations of pure substances that have no definite or constant composition
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compound
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composed of two or more elements in specific ratio
ex: H2O |
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atom
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the smallest particle of an element that still has the properties of the element
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element
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composed of a single kind of atom, are the building blocks of matter
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pure substance
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has a definite and constant composition or makeup
ex: salt, sugar |
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deposition
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going directly from a gaseous state to a solid state
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sublimation
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the process of going directly from the solid state to the gaseous state without ever becoming a liquid
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freezing
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going from a liquid to a solid
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condensation
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going from a gas to a liquid
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gas
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no definite shape or volume, particles are relatively independent of each other
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liquid
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no definite shape, but does have a definite volume, particles are farther apart and move more than in a solid
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solid
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has a definite shape and volume, molecules are close together and move very little
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3 states of matter
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solid, liquid, and gas
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extensive properties
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properties that depend on the amount of matter present
ex: mass and volume |
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intensive properties
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don't depend on the amount of matter present
ex: color |
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density
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the ratio of mass to the volume of a substance
d=m/v mass is in grams and volume in mL |
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specific gravity
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the ratio of the density of water at the same temperature
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Archimedes Principle
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the volume of an object is equal to the volume of water it displaces
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energy
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the ability to do work
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kinetic energy
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the energy of motion
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The Law of Conservation of Energy
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energy is neither created or destroyed, only transferred
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potential energy
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stored energy
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chemical bonds
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the forces that hold atoms together in compounds
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Kelvin temperature
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take the Celsius measurement and add 273
K = C+273 |
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Fahrenheit to Celsius
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C = 5/9 (F-32)
F + 9/5 (C)+32 |
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heat
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a measure of the total amount of energy a substance possesses
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1 calorie
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4.184 Joules, measures heat
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3 major subatomic particles
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proton, neutron, electron
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ions
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atoms that gain a positive or negative charge
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nucleus
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a dense central core in the middle of an atom
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mass number
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the sum of the protons and neutrons in an atom, also known as the atomic weight, listed in atomic mass units (amu)
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atomic number
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number of protons in an atom
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Element on the periodic table - symbols
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A - mass #
X - atomic symbol Z - atomic # |
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ground state
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the amount of energy an electron normally occupies
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excited state
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higher-energy, less stable state that an electron would be in if it absorbs more energy and moved to another shell
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electromagnetic spectrum
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the range of wavelengths of energy
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Bohr model
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came up with the shells model for an atom and the different energy levels for an electron
L1: 2 electrons L2: 8 electrons |
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quantum theory
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matter also has properties associated with waves
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momentum
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speed and direction
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Uncertainty Principle
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it is impossible to know both the position and momentum of an electron at the same time
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orbitals or electron clouds
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volumes of space in which there is likely to be an electron
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quantum numbers
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n - Principal quantum number, describes the orbital energy, only in positive integers
l - angular momentum quantum number, describes orbital shape, in integers from 0 to n-1 m(subscript l) - magnetic quantum number, describes orientation, only between -1 to 0 to +1 m(subscript s) - spin quantum number, describes the electron spin, either -1/2 or +1/2 |
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subshells
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orbitals that have the same value of n but different values of l
l values letter 0 s 1 p 2 d 3 f 4 g |
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Ac
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Actinium
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Al
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Aluminum
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Am
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Americium
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Sb
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Antimony
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Ar
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Argon
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As
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Arsenic
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At
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Astatine
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Ba
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Barium
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Bk
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Berkelium
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Be
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Beryllium
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Bi
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Bismuth
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Bh
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Bohrium
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B
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Boron
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Br
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Bromine
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Cd
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Cadmium
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Ca
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Calcium
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Cf
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Californium
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C
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Carbon
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Ce
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Cerium
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Cs
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Cesium
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Cl
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Chlorine
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Cr
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Chromium
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Co
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Cobalt
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Cu
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Copper
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Cm
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Curium
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Db
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Dubnium
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Dy
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Dysprosium
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Es
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Einsteinium
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Er
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Erbium
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Eu
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Europium
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Fm
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Fermium
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F
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Fluorine
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Fr
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Francium
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Gd
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Gadolinium
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Ga
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Gallium
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Ge
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Germanium
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Au
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Gold
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Hf
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Hafnium
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Hs
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Hassium
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He
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Helium
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Ho
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Holmfum
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H
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Hydrogen
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In
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Indium
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I
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Iodine
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Ir
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Iridium
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Fe
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Iron
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Kr
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Krypton
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La
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Lanthanum
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Lr
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Lawrencium
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Pb
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Lead
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Li
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Lithium
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Lu
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Lutetium
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Mg
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Magnesium
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Mn
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Manganese
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Mt
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Meitnerium
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Md
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Mendelevium
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Hg
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Mercury
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Mo
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Molybdenum
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Nd
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Neodymium
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Ne
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Neon
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Np
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Neptunium
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Ni
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Nickel
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Nb
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Niobium
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N
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Nitrogen
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No
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Nobelium
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Os
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Osmium
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O
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Oxygen
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Pd
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Palladium
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P
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Phosphorus
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Pt
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Platinum
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Pu
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Plutonium
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Po
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Polonium
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K
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Potassium
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Pr
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Praseodymium
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Pm
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Promethium
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Pa
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Protactinium
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Ra
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Radium
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Rn
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Radon
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Re
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Rhenium
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Rh
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Rhodium
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Rb
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Rubidium
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Ru
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Ruthenium
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Rf
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Rutherfordium
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Sm
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Samarium
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Sc
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Scandium
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Sg
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Seaborgium
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Se
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Selenium
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Si
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Silicon
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Ag
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Silver
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Na
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Sodium
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Sr
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Strontium
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S
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Sulfur
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Ta
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Tantalum
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Tc
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Technetium
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Te
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Tellurium
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Tb
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Terbium
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Tl
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Thallium
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Th
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Thorium
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Tm
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Thulium
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Sn
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Tin
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Ti
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Titanium
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W
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Tungsten
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U
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Uranium
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V
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Vanadium
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Xe
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Xenon
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Y
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Ytterbium
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Zn
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Zinc
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Zr
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Zirconium
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electron configuration
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a shorthand notation to show the information that an energy level diagram shows
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Valence electron
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an electron that is on the outermost energy level
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ions
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atoms in which there are unequal numbers of protons and electrons
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cations
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ions with a positive charge
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isoelectronic
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when two chemical species have the same electron configurations
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anion
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an ion with a negative charge
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electrolyte
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a substance that conducts electricity when melted or dissolved with water
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1
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H - Hydrogen
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2
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He- Helium
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3
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Li - Lithium
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4
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Be - Beryllium
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5
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B - Boron
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6
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C - Carbon
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7
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N - Nitrogen
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8
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O - Oxygen
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9
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F - Fluorine
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10
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Ne - Neon
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11
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Na - Sodium
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12
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Mg - Magnesium
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13
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Al - Aluminum
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14
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Si - Silicon
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15
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P - Phosphorus
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16
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S - Sulfur
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17
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Cl - Chlorine
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18
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Ar - Argon
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19
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K - Potassium
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20
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Ca - Calcium
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21
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Sc - Scandium
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22
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Ti - Titanium
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23
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V - Vanadium
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24
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Cr - Chromium
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25
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Mn - Manganese
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26
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Fe - Iron
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27
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Co - Cobalt
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28
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Ni - Nickel
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29
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Cu - Copper
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30
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Zn - Zinc
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31
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Ga - Gallium
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32
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Ge - Germanium
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33
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As - Arsenic
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34
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Se - Selenium
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35
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Br- Bromine
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periods
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the horizontal rows on the table of elements
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groups or families
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the vertical columns on the table of elements
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Alkali metals
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IA Family, tend to lose 1 electron
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Alkaline earth metals
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IIA Family, tend to lose 2 electrons
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Halogens
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VIIA Family, tend to gain 1 electron
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noble gases
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VIIIA Family, unreactive except in special circumstances, all 8 valence electrons are full which makes them very stable
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transition metals
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the families that have a B instead of an A with their roman numeral
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isotopes
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atoms of the same element with a different amount of neutrons
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sulfate
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SO₄²⁺
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sulfite
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SO₃²⁻
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nitrate
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NO₃⁻
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nitrite
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NO₂⁻
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hypochlorite
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ClO⁻
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Chlorite
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ClO₂⁻
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Chlorate
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ClO₃⁻
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