If cation is a group one metal or NH4+ If anion is NO3- ; ClO3- ; ClO4- ; or CH3COO-

-2 ; Exceptions: Bound to F ; In H2O2 (-1)

If anion is Cl- ; Br- ; or I- except with Ag+ ; Hg+ ; or Pb2+ If anion is SO42- except with Ba2+ ; Ca2+ ; Sr2+ ; or Pb2+

If anion is PO43- ; CO32- ; C2O42- ; OH- ; S2- EXCEPT GROUP 1/AMMONIUM

Things to memorize forever Flashcards by Tanya Sharma

Hydrogen’s oxidation number

+1 ; Exception: hydrides (-1)

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The amount of product actually obtained

Actual yield

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An element is a product (redox reactions) Only compounds form (non-redox reactions)

Decomposition reactions

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The ratio of stoichiometric coefficients in a balanced chemical equation

Mole ratio

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Always Soluble

If cation is a group one metal or NH₄⁺

If anion is NO₃^- ; ClO₃^- ; ClO₄^- ; or CH₃COO^-

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Hydrochloric acid

HCl ; strong acid

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Phosphorus’s molecular formula and physical state

P₄ ;Solid

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Bromine’s molecular formula and physical state

Br₂ ;Liquid

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Potassium hydroxide

KOH ; strong base

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Two or more substances react to give a single product

Combination

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Oxygen

-2 ; Exceptions: Bound to F ; In H₂O₂ (-1)

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Usually soluble

If anion is Cl^- ; Br^- ; or I^- except with Ag⁺ ; Hg⁺ ; or Pb²⁺
If anion is SO₄^2- except with Ba²⁺ ; Ca²⁺ ; Sr²⁺ ; or Pb²⁺

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Chlorine’s molecular formula and physical state

Cl₂ ;Gas

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Hydroiodic acid

HI ; strong acid

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Alkali metals

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Lab procedure that can determine the concentration of an analyte in solution; stoichiometry of a reaction; number of electrons gained in a redox reaction; and solubility products

Titrations

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Metals’ physical state

Solid

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Methylamine

CH₃NH₂ ; weak base

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Nitric acid

HNO₃ ; strong acid

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Use the ______ to know when the titration is complete due to a color change

Indicator

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Fluorine’s molecular formula and physical state

F₂ ;Gas

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Compounds that increase the concentration of H+ (aq)

Acids

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The relative amounts of reactants needed to leave no excess reactants

Stoichiometric amounts

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Gain of electrons

Reduction; substance is reduced when oxidation number decreases

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Insoluble

If anion is PO₄^3- ; CO₃^2- ; C₂O₄^2- ; OH^- ; S^2- EXCEPT GROUP 1/AMMONIUM

Sodium hydroxide

NaOH ; strong base

Acetic acid

CH₃COOH; weak acid

Compounds that dissolve in completely

Strong electrolytes

The oxidation number for an atom in its elemental form is

Zero (H₂ ; Cr ; S₈)

\_\_\_\_\_\_\_\_ _______ are never redox reactions

Exchange reactions

The chemical equation that includes only the ions in solution or compounds that undergo change

Net ionic equation

Nitrogen's molecular formula and physical state

N₂ ;Gas

Adding solvent to a solution

dilution

An insoluble solid formed from an aqueous solution

Percipitate

Compounds that dissolve only partially

Weak electrolytes

Halogens other than F

-1 ; Exceptions: Bound to O or F

Loss of electrons

Oxidation; a substance is oxidized when oxidation number increases

Alkaline metals

Perchloric acid

HClO₄ ; strong acid

Formic acid

HCOOH ; weak acid

The sum of the oxidation numbers of the atoms in a compound is

Zero

The amount of solute dissolved in a given volume of solvent

Concentration

Compounds that increase the concentration of OH- (aq)

Bases

Sulfur's molecular formula and physical state

S⁸ ;Solid

Chloric acid

HClO₃ ; strong acid

The maximum amount of product that a reaction should give

Theoretical yield

Calcium hydroxide

Ca(OH)₂ ; strong base

Oxygen's molecular formula and physical state

O₂ ;Gas

A molecule that allows us to observe the end point of a titration

Indicator

Barium hydroxide

Ba(OH)₂ ; strong base

Two compounds interchange ions to give two new compounds

Exchange

Hydrobromic acid

HBr ; strong acid

The point at which the titration is actually complete and the indicator changes color

End point

A single substance decomposes to give two or more products

Decomposition

Iodine

I₂ ;Solid

The number of moles of solute per liter of solution M = moles/liter

Molarity

Solution of known concentration that is added to a solution of unknown concentration

Titrant ; analyte

The medium into which the solute is dissolved to form a solution

Solvent

An element reacts with a compound to give a new compound and possibly a different element

Displacement

A compound reacts with O₂; when the compound is a hydrocarbon, the products are always CO₂ and H₂O; Are either displacement or combination reactions

Combustion

The oxidation number for a monatomic ion is the

Same as the charge ( O^2- = -2 ; Fe²⁺ = +2 ; Al³⁺ = +3)

All _________ \_\_\_\_\_\_\_\_ are redox reactions

Displacement reactions

Carbon's molecular formula and physical state

C ;Solid

Compounds that dissolve in water to give ions

Electrolytes

Ions that do not participate in the reaction

Spectator ions

Sulfuric acid

H₂SO₄ ; strong acid

Benzoic acid

C₆H₅COOH ; weak acid

The chemical equation with the ions in solution from soluble compounds written separately

Total ionic equation

Inorganic acids that are electrolytes

HCl ; HF ; HNO₃ ; HClO₄

An element is a reactant (redox reactions) Only compounds combine (non-redox reactions)

Combination reactions

The point in a titration where the indicator should change color (equal amounts of both substances)

Equivalence point

Carbonic acid

H₂CO₃ ; weak acid

Hypothetical charge on an atom if all of its bonds were completely ionic

Oxidation number

The substance dissolved in a solution

Solute

Rubidium hydroxide

RbOH ; strong base

Soluble ionic compounds that are electrolytes

NaCl ; LiF ; NH₄Br ; CuSO₄ ; AgNO₃

Reactants that determine how far a reaction can go

Limiting reactants

The sum of the oxidation numbers of the atoms in a polyatomic ion must equal the charge on the ion

Polyatomic ion

Hydrocyanic acid

HCN ; weak acid

Hydrogen's molecular formula and physical state

H₂ ;Gas

Strontium hydroxide

Sr(OH)₂ ; strong base

Fluorine

-1

Ammonia

NH₃ ; Weak base

The maximum amount of solute that will dissolve in a given volume of solvent at a given temperature

Solubility

Lithium hydroxide

LiOH ; strong base

A solution of known or determinable concentration that has already been prepared

Stock solution

Organic acids that are electrolytes

CH₃COOH ; C₆H₅COOH

Phosphoric acid

H₃PO₄ ; weak acid

Things to memorize forever Flashcards

(88 cards)