Chemistry Test 5

Opposite ends of water molecules attract one another. It is what gives water such a high boiling point.

crystals of ionic compounds that contain an orderly 3-D arrangement of positive and negative ions

Because the pull of the water molecules is not strong enough to overcome the attractions among ions in the crystal lattice.

Because the pull of molecules is strong enough to overcome the attractions among the ions and will start to pull the crystal apart.

• Dissociate in water, producing positive and negative ions
• conduct an electric current in water
• in equations show the formation of ions in aqueous solutions

• dissociates only slightly in water
• in water forms a solution of a few ions and mostly undissociated molecules
• associated with the equilibrium sign

• dissolve as molecules in water
• do not produce ions in water
• form solutions that do not conduct electric current

• 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

Metathesis reactions that result in the formation of an insoluble solid

A physical property describing how readily a substance will dissolve in a given solvent

When ionic compounds are shown with cations and anions together to form neutral units in a chemical equation

• AKA total ionic equation or complete ionic equation
• Show soluble ionic compounds and strong acids separated into the ions that they contain

• Ions that do not change in a reaction
• In net ionic equations, the spectator ions are removed

• Produce H+ ions in water
• are electrolytes
• have a sour taste
• turn litmus red
• neutralize bases
• corrosive to metals and skin

• hydrochloric acid
• hydrobromic acid
• hydroiodic acid
• nitric acid
• sulfuric acid
• perchloric acid
• chloric acid

HCl

HBr

HI

HNO₃

H₂SO₄

HClO₄

HClO₃

• Produce OH- ions in water
• taste bitter or chalky
• are electrolytes
• feel soapy or slippery
• neutralize acids
• caustic (corrosive)

• Lithium hydroxide
• Sodium hydroxide
• Potassium hydroxide
• Rubidium hydroxide
• Cesium hydroxide
• Calcium hydroxide
• Strontium hydroxide
• Barium hydroxide

LiOH

NaOH

KOH

RbOH

CsOH

Ca(OH)₂

Sr(OH)₂

Ba(OH)₂

Any ionic compound that is not a hydroxide or oxide, produced when acids and bases neutralize each other

• AKA redox reactions
• involve a transfer of electrons

• AKA oxidation state
• numbers assigned to atoms to help keep track of electrons lost or gained during a redox reaction

Increase in oxidation number or loss of electrons

Reduction in oxidation number or gain of electrons

the reactant that causes another reactant to be oxidized; steals electrons; oxidants get reduced in the reaction

the reactant that causes another reactant to be reduced; gives away electrons; reductants get oxidized in the reaction

• 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

• Amount of solute dissolved in a specific amount of solution.
• amount of solute/amount of solution

mass percent = g of solute/(g of solute + g of solvent)  x100

• water is added
• volume increases
• concentration decreases

C1V1 = C2V2

M1V1 = M2V2

techniques used to find an unknown concentration using a standard solution that reacts with the solute in the test solution

A solution in a titration that has a known concentration

A substance that changes color in the presence of an acid or base

point in a titration when a stoichiometrically equivalent amount of base has been added to an acid (or acid to a base)

point in a titration at which the indicator changes color