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47 Cards in this Set
- Front
- Back
Ionic
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Held together by electrostatic attraction
1 cation and 1 anion |
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covalent
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held together by sharing of electrons
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empirical formula
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simplest whole # ratios for atoms in a compound
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molecular formula:
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represents the # and type of atoms in a molecule, provides little structural information
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acetate
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C2H3O2-
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carbonate
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Co3-2
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hydrogen carbonate
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HCO3-1
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Hydroxide
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OH-
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Nitrate
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NO3-
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Nitrite
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NO2-
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Chromate
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CrO4-2
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Dichromate
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Cr2O7-2
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Phosphate
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PO4-3
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Hydrogen Phosphate
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HPO4-2
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Ammonium
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NH4+
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Hydrogen Sulfite
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HSO3-
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Hydrogen Sulfate
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HSO4-
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Peroxide
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O2-2
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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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Perchlorate
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ClO4-
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Permanganate
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MnO4-
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Sulfate
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SO4-2
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Sulfite
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SO3-2
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Cyanide
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CN-
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electronegativity
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ability of an atom in a bond to attract electrons to itself
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Mole
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# atoms present in exactly 12 g of C12
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% Comp
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Fraction of the total mass of a given compound that is made due to a single element
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Chemical Reaction Evidence:
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1) color change
2) formation of a solid 3) emission of light 4) emission of heat |
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Homogenous
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completely dissolved
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Heterogenous
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not entirely dissolved
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Electrolytes
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compounds whose solutions conduct electricity
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Always Soluble:
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Li+, Na+, K+, NH4+, NO3-, C2H3O2-
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Soluble unless paired with Ag+, Hg2+2, Pb+2
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Cl-, Br-, I-
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SO4-2 always soluble unless paired with
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Sr+2, Ba+2, Pb+2, Ca+2
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OH- always insoluble unless paired with
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Li+, Na+, K+, NH4+
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S-2 always insoluble unless paired with:
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Li+, Na+, K+, NH4+, Ca+2, Sr+2, Ba+2
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Co3-2, PO4-3 always insoluble unless paired withL
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Li+, K+, Na+, NH4+
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Spectator Ions:
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Do not undergo a change in a chemical reaction
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Acid:
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substance that causes an increase in H+ concentration
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Base
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Substance that causes an increase in OH- concentration
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Strong Acids:
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HCl, HBr, HI, HNO3, HClO4, H2SO4, LiOH, NaOH, KOH
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Weak Acids:
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CH3COOH
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Strong Bases:
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Alkaline Metals (ex. NaOH)
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Diatomic Molecules:
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H2, O2, N2, F2, Br2, I2
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Oxidation:
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Process of losing an electron
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