Module 1 Flashcards
IUPAC
International Union of Pure and Applied Chemistry. The world’s head on everything regarding chemistry formatting ex. naming, units, values, etc. International Federation. Makes sure chemistry is universal.
CAS
Chemical Abstract Services. A database containing information about elements’ properities.
Alkali Metals
Group 1
Alkaline Earth Metals
Group 2
Transition Metals
Groups 3 - 12
Halogens
Group 17
Noble Gases
Group 18
Lanthanoids
Top row of the bottom two rows.
Actinoids
Bottom row of the bottom two rows.
Synthesis
A + B —> C OR A + B —> C + D
Decomposition
A —> B + C
Single Displacement
AB + C —> BC + A
Double Displacement
AB + CD —> AC + BD
Combustion
CxHy + O2 —> CO2 + H2O
Acid-Base
Acid + Base —> Salt + Water
Solution
A homogeneous mixture in which one or more solutes are dissolved in a solvent.
Aqueous Solutions
Have water as the solvent.
Ionic Compounds
Consist in positive and negative ions in a crystal lattice. Ions are bonded by ionic bonds. Ex. NaCl.
Molecular Compounds
Stable, neutral molecules held by covalent bonds. Ex. H2O, CCl4, CO2.
Precipitation Reactions
The ions in the solution form a solid, ie. a precipitate.
Gravimetric/Gravitational Analysis
The amount of substance in a sample is concluded by the mass of the precipitate that is formed, ie. how much product was formed.
Solubility Guidelines for Ionic Compounds Rule 1
Salts of alkali metals, group 1, are soluble. Ex. NaCl, KNO3.
Solubility Guidelines for Ionic Compounds Rule 2
Ammonium, NH4+, salts are soluble. Ex. NH4Cl, (NH4)2SO4.
Solubility Guidelines for Ionic Compounds Rule 3
Nitrates, NO3-, are soluble. Ex. AgNO3, Zn(NO3)2.
Solubility Guidelines for Ionic Compounds Rule 4
Chlorides, Cl-, bromides, Br-, and iodides, I-, are soluble except when paired with lead, Pb^2+, mercury, Hg+ and Hg2^2+, and silver, Ag+. Ex. ZnCl2 is soluble but PbCl2 is not soluble.
Solubility Guidelines for Ionic Compounds Rule 5
Sulfates, SO4^2-, are soluble except when paired with calcium, Ca^2+, strontium, Sr^2+, barium, Ba^2+, silver, Ag2+, mercury, Hg2+ and Hg^2+, and lead, Pb^2+. Ex. Na2SO4 is soluble but CaSO4 is not.
Solubility Guidelines for Ionic Compounds Rule 6
Carbonates, CO3^2-, phosphates, PO4^3-, and sulfides, S^2-, are insoluble expect when paired with:
i) alkalis (Rule 1)
ii) ammonium (Rule 2)
Solubility Guidelines for Ionic Compounds Rule 7
Hydroxides, OH-, are insoluble/slightly soluble expect when paired with alkalis (Rule 1). Note: the hydroxides of group 2, alkaline earth metals, are slightly soluble.
Full Molecular Equation
The full balanced chemical equation.
Net Ionic Equation
The balanced chemical equation not including the spectator ions.
Brønsted-Lowry Acid-Base
The acid is a proton (H+) donor and the base is a proton (H+) acceptor. The proton is transferred from the acid to the base.
Protonated
An acid produces H3O+ ions when dissolved in water.
De-protonated
A base produces OH- ions when dissolved in water.
Strong Acids
Completely ionizes in water.
Strong Bases
Completely ionizes in water.
Common Strong Acids
HCl - hydrochloric acid
HBr - hydrobromic acid
HI - hydroiodic acid
HClO4 - perchloric acid
HBrO4 - perbromic acid
HIO4 - periodic acid
HNO3 - nitric acid
H2SO4 - sulfuric acid
Common Strong Bases
Group 1 + 2 hydroxides
Hydride, H-, ions
Oxide, O^2-, ions
Diprotic
Ionizes twice. Ex. H2SO4.
Mole (mol)
The SI unit for the amount of substance.
Avogadro’s Number
1 mol = 6.022 x 10^23 particles
Molar Mass (Mr)
The mass in g of 1.0 mol of a substance.
Molecular Formula
Mr molecular = x(Mr empirical)
Theoretical Yield
The maximum amount of products that can be produced.
Limiting Reactant/Reagent
The species that limits the amount of product that can form (the one that “runs out” first).
% Yield
% Yield = (actual yield/theoretical yield) x 100%
Consecutive Reactions
A series of reactions that occur sequentially. The products from one reaction are consumed as reactants in a subsequent reaction. Can add the reactions together to obtain the overall reaction.
Simultaneous Reactions
Reactions that are independent and occur at the same time. Are used in the analysis of chemical mixtures. Can’t add together.
Intermediate
A species produced in one step and consumed in a subsequent step. Never appears in the overall equation. May need to be multiplied by a coefficient to cancel it out.
Green Chemistry
An approach to chemistry that is intentionally focused on not only the efficient use of atoms (and energy) but also chemical methods that reduce or eliminate reagents, products, solvents, by-products, wastes, etc. that are hazardous to human health or the environment.
% Atom Economy
(stoichiometric mass of the desired product/sum of the stoichiometric mass of the reactants) x 100%
Stoichiometric Mass
stoichiometric coefficients x molar mass
E-factor (Environmental Factor)
mass of waste produce (minus water)/mass of product obtained
