Chemistry400 – Flashcards

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Element
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Substance that cannot be
chemically broken down into simpler substances.
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Sulfate Ion
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SO4, 2- Charge, Oxyanion
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Nitrate Ion
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NO3, 1- Charge, Oxyanion
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Phosphate Ion
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PO4 3- Charge, Oxyanion
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Calcium
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Ca, 2+ Charge
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Sodium
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Na, 1+ Charge
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Potassium
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K, 1+ Charge
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Lithium
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Li, 1+ Charge
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Rubidium
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Rb, 1+ Charge
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Beryllium
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Be, 2+ Charge
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Magnesium
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Mg, 2+ Charge
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Strontium
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Sr, 2+ Charge
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Barium
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Ba, 2+ Charge
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Flourine
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F, 1- Charge, Diatomic Gas
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Chlorine
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Cl, 1- Charge, Diatomic Gas
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Bromine
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Br, 1- Charge, Diatomic Gas
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Hydrogen
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H, 1+ Charge, Diatomic
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Oxygen
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O, 2- Charge, Diatomic
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Nitrogen
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N, 3- Charge, Diatomic
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Phosphourus
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P, 3- Charge,
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Sulfur
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S, 2- Charge, Diatomic
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Bromine
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Br, 1- Charge, Diatomic
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Iodine
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I, 1- Charge, Diatomic
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Significant Figures
Multiplication and Division Rule
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The result carries the
same number of significant figures as the factor with the fewest significant figures.
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Significant Figures
Adding and Subtracting Rule
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The result carries the same number of decimal places as the quantity with the fewest decimal places.
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Accuracy
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refers to how close the
measured value is to the actual value.
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Precision
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refers to how close a series of measurements are to one another or how reproducible they are
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Chemical Formula
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Formula with its elements and shows the number of each element
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Empirical Formula
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Formula of a chemical with the lowest ratio of each element
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Ionic Bond
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Between Metal and Nonmetal
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Covalent Bond
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Bond between two or more nonmetals, also called a Molecule
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Molecular Element
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Molecule of a single type of atom
O=O or H-H
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Compound
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Molecular or Ionic, H2O or NACL
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Atomic Elements
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Exist in nature with single atom as their basic units
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Covalent Compound
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Consists of two or more covalently bonded nonmetals, H2O CO2, PO3
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Ionic Compound
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Composed of cation and anion bound together by Ionic bonds
NaCl, CaCl2, Al2O3
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Molecular Compound and how to name them
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Made from two or more nonmetals that are covalently bonded
Name first element with number prefix, and name second element with prefix and end with "ide"
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Metal Ions and naming them
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Monoatomic cations, and named simply by their name, followed by "ion"
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Nonmetal Ions and naming them
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Normally form monoatomic anions
Name the element, and end it with "ide"
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Iron (FE) Oxidation states
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+2 and +3 or II and III
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Lead (PB) Oxidation states
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+2 and +4, II and IV
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Binary Acid and naming them
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Compounds composed of H with another nonmetal
Hydro followed by the name of the element ending with "ic" and the word "acid"
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Acid
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Substance that produces Hydrogen ions (H+) when dissolved in water
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Oxyacid and names
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Contain Oxygen in addition to Hydrogen and another nonmetal
Starting = ___ic
one O more = per__ic
one O less = ___ous
two O less = hypo__ous
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Oxyanions names
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Contain oxygen with nonmetal, but without a hydrogen
Starting = ___ate
one O more = per__ate
one O less = ___ite
two O less = hypo___ite
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Polyprotic Acids
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Acids that produce multiple protons (H+)
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Hydrate
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written in the formula as H2O, with the prefix number
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Writing Ionic compounds containing a polyatomic ion
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Write the unmodified name of the cation, then write the name of the ion, DO NOT USE PREFIXES
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Carbonate Ion
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CO3 2- Charge, Oxyanion
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Sulfite Ion
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SO3 2- Charge, Oxyanion
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Nitrite Ion
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NO2 1- Charge, Oxyanion
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Hydroxide Ion
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OH 1- Charge, Oxyanion
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Hydrogen Carbonate Ion
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HCO3 1- Charge, Acid Anion
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Hydrogen Sulfide Ion
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HS 1- Charge, Acid Anion
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Hydrogen Sulfate Ion
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HSO4 1- Charge, Acid Anion
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Hydrogen Sulfite Ion
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HSO3 1- Charge, Acid Anion
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Dihydrogen Phosphate Ion
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H2PO4 1- Charge, Acid Anion
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Chromium(II) Ion
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Cr 2+
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Manganese(II) Ion
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Mn 2+
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Nickel(II) Ion
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Ni 2+
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Copper(II) Ion
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Cu 2+
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Zinc Ion
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Zn 2+
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Cadmium Ion
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Cd 2+
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Mercury(I) Ion
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Hg_2 2+
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Mercury(II) Ion
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Hg 2+
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Formula Mass/Molecular Mass
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Sum of all individual masses making up the formula unit
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Molar Mass
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The mass in grams of 1 mol of its molecules or formula units
Numerically equivalent to its formula mass with the unit being -gram per mole- rather than amu
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Mass percent of a formula's element
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x (molar mass of element)
= -------------------------- X 100
(molar mass of formula)
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