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Recognizing Oxidation and Reduction Reactions
- A substance is oxidized when its oxidation number is increased in a reaction.
- A substance is reduced when its oxidation number is decreased in a reaction.
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Molecule
Independent structure consisting of 2 or more atoms chemically bound together.
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Compound
Matter composed of 2 or more elements that are chemically bound.
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Law of Mass Conservation
- Total mass of substances does not change during chemical reaction.
- Matter cannot be created or destroyed.
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Law of Definite Composition
- Compounds are composed of the same element in the same part (fractions) by mass.
- Divide mass of each element by total mass of compound.
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Bionary Ionic Compound
2 elements (typically 1 metal, 1 nonmetal) where each metal loses an electron and the nonmetal gains an electron.
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Monatomic Ion
Cation or Anion derived from a single atom
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Coulumb's Law
- The energy of attraction/ repulsion btwn 2 particles is directly proportional to the product of charges and inversely proportional to distance btwn them.
- 1. Ions w/ higher charges attract/ repel more strongly than lower charges
- 2. Smaller ions attract/ repel more strongly b/c the disance btwn charges is shorter
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Diatomic Molecules
Pairs of atoms that are chemically bound and behave as an independent unit.
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Polyatomic Ions
2 or more atoms bonded covalently and have a net positive or negative charge.
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Empirical Formula
- 1) Convert percentages to grams
- 2) Do ratios for grames to moles
- 3) Divide by smallest #
- 4) Write formula with subscripts
- 5) All subscripts must be integers- adjust as necessary
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Molecular Formula
- 1) Convert % to grams
- 2) divide grams by element's amu
- 3) convert from grams to mole (no math)
- 4) divide each answer by smallest
- 5) add amus of empirical formula
- 6) divide molecular weight/ amus
- 7) multiply empirical formula by total from #6
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Structural Formula
Shows number of atoms and bonds between them.
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-ium
cation ending for metal names
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-ide
anion ending for nonmetal
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Naming Binary Ionic Compound
- 1) Cation name first
- 2) add -ide to nonmetal
- 3) place anion last
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Subscript
- Refers to element preceding it
- the subscript '1' is implied from symbol
- The charge of one ion becomes he superscript of the other
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Oxoan-ions
- Those in which an elment, usually nonmetal, is bonded to one or more oxygen atoms.
- More 0 atoms- ate
- Less O atoms - ite
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HPO4-2
Hydrogen Phosphate
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Molecular Mass
Sum of Atomic Masses
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Reactants
- Substances that react during change.
- Placed to LEFT of arrow
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Products
- All substances produced.
- Placed to RIGHT of arrow.
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Group 1A
Bonds with Group 7AMakes a salt
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Group 2A
Bonds with group 6AForms a salt
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Isimers
Molecules with same chemical formul but different structural formulas
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Soluable
I would rather be surrounded by water.
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Must have to find Formula Weight and Molecular Weight
Chemical formula and Periodic table
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To find Molecular Formula
- 1) Find % Composition then Empirical Formula2) Molecualr Weight or
- molar Mass
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Spectator Ion
No Change even with mixutre
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Oxidation
- 1) Gain in Oxygen
- 2) Loss of
- 3) Loss of Electrons
LEO
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Reduction
- 1) Loss of Oxygen
- 2) Gain of Hydrogen
- 3) Gain of Electrons
GER
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To write compounds
- 1) write compounds largest to smallest moving across table
- 2) go from top to bottom in case of a tie
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Molecular Formula
- 1) Convert % to grams
- 2) Divide gramst by element's amu
- 3) Convert from g to mole (no math)
- 4) Divide each answer by smallest
- 5) Add amus of Empirical Formula
- 6) Divide Molecular Weight/ amus
- 7) Multiply empirical formula by total from #6
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Metals
- Lose electrons easily
- positive ions
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Nonmetals
gain electrons, for negative ions
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Charge of Monatomic Ions
- IA-IIIA= +1-+3 respectively, electrons lost = to group number
- IB-IIB= electrons lost = group #
- IIIB-VIIIB= +2 or +3
- Max # of electons gained by nonmetals- 8-group #
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Molecule Mass
Sum of the masses of the atoms
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Nonelectrolytes
- Do not produce ions in solution and do not yield conducting solutions
- Alcohol, sugar, water
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Strong Electrolyes
- Dissociate or ionize 100% in aqueous solution
- Yield very conducting solutions at reasonable concentrations.
- Salts, strong acids, strong bases
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Dissociate
Ions already exist, water allows them to 'drift apart
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Ionize
Ions don't already exist. polar compounds have 'tendency to form ions
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Oxidation numbers
- All have a number of 0
- For single atom, O.N. is = to charge of ion
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Oxidation Number of H
- H+
- Unless in metal hydride (NaH-, CaH2-), then it is -1
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Oxidation number of O
- -2
- Unluss O is peroxide (H2O2, NA2O2), Then it is -1
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Radioactive Element
- Atomic Nuclei are unstable
- Nucleus is not balanced and there is continuous change
- Usually rare metals
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