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hydrogen bonding
Opposite ends of water molecules attract one another. It is what gives water such a high boiling point.
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Crystal lattice
crystals of ionic compounds that contain an orderly 3-D arrangement of positive and negative ions
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Why are some things insoluble in water?
Because the pull of the water molecules is not strong enough to overcome the attractions among ions in the crystal lattice.
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Why are some things soluble in water?
Because the pull of molecules is strong enough to overcome the attractions among the ions and will start to pull the crystal apart.
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Strong electrolytes
- Dissociate in water, producing positive and negative ions
- conduct an electric current in water
- in equations show the formation of ions in aqueous solutions
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Weak electrolytes
- dissociates only slightly in water
- in water forms a solution of a few ions and mostly undissociated molecules
- associated with the equilibrium sign
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Nonelectrolytes
- dissolve as molecules in water
- do not produce ions in water
- form solutions that do not conduct electric current
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Metathesis reaction
- AKA double replacement reactions
- involve a trading of ion partners
- are driven by A) the formation of precipitates B) the formation of a molecular liquid or C) the formation of a molecular gas
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Precipitation reactions
Metathesis reactions that result in the formation of an insoluble solid
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Solubility
A physical property describing how readily a substance will dissolve in a given solvent
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Molecular equation
When ionic compounds are shown with cations and anions together to form neutral units in a chemical equation
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Ionic equation
- AKA total ionic equation or complete ionic equation
- Show soluble ionic compounds and strong acids separated into the ions that they contain
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Spectator ions
- Ions that do not change in a reaction
- In net ionic equations, the spectator ions are removed
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Arrhenius acids
- Produce H+ ions in water
- are electrolytes
- have a sour taste
- turn litmus red
- neutralize bases
- corrosive to metals and skin
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7 Strong Acids by name
- hydrochloric acid
- hydrobromic acid
- hydroiodic acid
- nitric acid
- sulfuric acid
- perchloric acid
- chloric acid
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Formula for hydrochloric acid
HCl
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Formula for hydrobromic acid
HBr
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Formula for hyroiodic acid
HI
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Formula for nitric acid
HNO3
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Formula for sulfuric acid
H2SO4
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Formula for perchloric acid
HClO4
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Formula for chloric acid
HClO3
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Arrhenius bases
- Produce OH- ions in water
- taste bitter or chalky
- are electrolytes
- feel soapy or slippery
- neutralize acids
- caustic (corrosive)
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8 Strong Bases by name
- Lithium hydroxide
- Sodium hydroxide
- Potassium hydroxide
- Rubidium hydroxide
- Cesium hydroxide
- Calcium hydroxide
- Strontium hydroxide
- Barium hydroxide
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Calcium hydroxide
Ca(OH)2
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Strontium hydroxide
Sr(OH)2
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Salt
Any ionic compound that is not a hydroxide or oxide, produced when acids and bases neutralize each other
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Oxidation reactions
- AKA redox reactions
- involve a transfer of electrons
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Oxidation numbers
- AKA oxidation state
- numbers assigned to atoms to help keep track of electrons lost or gained during a redox reaction
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Oxidation
Increase in oxidation number or loss of electrons
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Reduction
Reduction in oxidation number or gain of electrons
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Oxidising agent or oxidant
the reactant that causes another reactant to be oxidized; steals electrons; oxidants get reduced in the reaction
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Reducing agent or reductant
the reactant that causes another reactant to be reduced; gives away electrons; reductants get oxidized in the reaction
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Solubility
- the maximum amount of solute that dissolves in a specific amount of solvent
- expressed as grams of solute in 100 grams of solvent
- of most solids, increases as temperature increases
- of most gases, decreases as temperature increases
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Concentration of a solution
- Amount of solute dissolved in a specific amount of solution.
- amount of solute/amount of solution
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Mass percent equation
mass percent = g of solute/(g of solute + g of solvent) x100
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Dilution
- water is added
- volume increases
- concentration decreases
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Percent concentration equation
C1V1 = C2V2
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Molarity equation (in dilution)
M1V1 = M2V2
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Titration
techniques used to find an unknown concentration using a standard solution that reacts with the solute in the test solution
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Standard solution
A solution in a titration that has a known concentration
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Indicator
A substance that changes color in the presence of an acid or base
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Equivalence point
point in a titration when a stoichiometrically equivalent amount of base has been added to an acid (or acid to a base)
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End point
point in a titration at which the indicator changes color
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