Chemistry

• Éditeur: QuickStudy Reference Guides
• Année: 2009
• ISBN:
  9781423212553
• Sujet: Physical Sciences
• Sous-sujet: Chemistry

Best-selling guide for over 20 years and an essential companion for students taking chemistry courses of any level, this laminated six page guide is a must-have for reference throughout science courses as a serious study tool and quick refresher for the core concepts, terms, equations and periodic elements. Author and Harvard PhD, Mark D. Jackson, a scientist and university chemistry professor expertly streamlined the complicated subject of chemistry selecting the need-to-know answers for students in our easy QuickStudy outline format with helpful diagrams, graphs, tables, chemical problems, and practical applications. At this low price and durably laminated to last a lifetime, this guide has boosted test scores and grades for students for over 25 years and is guaranteed to do the same for you or your student. This guide is revised as needed and is up-to-date.
6 page laminated guide includes:

• Periodic Table of the Elements
• Atomic Structure
• Atomic Quantum Numbers & Orbitals
• Types of Matter
• Reactions
• Physical Processes
• Hints for Balancing Equations
• Nomenclature
• Stoichiometry: Mole Mass Relationships
• Chemical Interactions
• Formal Bonding Models
• Molecular Properties: Geometry
• Valence Bond Theory
• Hybrid Orbitals
• Chemical Bonding & Quantum Mechanics
• Behavior of Gases
• Molecular Orbital Theory
• Mixtures & Solutions
• Solids
• Oxidation-Reduction Reactions
• Properties of Inorganic Salts
• Acid-Base Reactions
• Thermodynamics
• Equilibrium
• Kinetics
• Nuclear Chemistry
• Measurements & Units

Nomenclature

Chemical Names

• Start with the cation name, followed by the anion name; use prefixes to clarify any ambiguity
• Anion and cation names are derived from element names
• Organic compounds: Names are based on a separate nomenclature system; many compounds have common nonsystematic names

Chemical Formulas

• Cation symbol followed by anion
• Subscripts denote relative composition
• Enclose polyatomic ions or molecules in parentheses
• Molecular formula: Discrete molecule
• Empirical formula: Relative molar ratio of elements for solids or molecules

ferric, Fe (III)	ferrous, Fe (II)
stannic, Sn (IV)	stannous, Sn (II)
plumbic, Pb (IV)	plumbous, Pb (II)
cupric, Cu (II)	cuprous, Cu (I)
mercuric, Hg (II)	mercurous, Hg (I)

Metal Cations

• Alkali metal (+1); alkaline earth (+2)
• Transition metal: Valence varies; give the valence in the name and formula; -ous or -ic ending; roman numerals are less confusing, more general

+1Polyatomic Cations

ammonium, NH₄⁺

hydronium, H₃O⁺; active form of acid in water

Monatomic Anions

–4carbide, C^4–; silicide, Si^4–

–3nitride, N^3–; phosphide, P^3–; arsenide, As^3–

–2oxide, O^2–; sulfide, S^2–; selenide, Se^2–; telluride, Te^2–

–1hydride, H^–; halides: fluoride, F^–; chloride, Cl^–; bromide, Br^–; iodide, I^–; acids: hydro -fluoric, -chloric, -bromic, -iodic

Polyatomic Anions (& Respective Acids)

–1
acetate, C2H3O2^–	acetic acid, C2H4O2
nitrate, NO3^–	nitric acid, HNO3
nitrite, NO2^–	nitrous acid, HNO2
hypochlorite, ClO^–	hypochlorous acid, HClO
chlorite, ClO2^–	chlorous acid, HClO2
chlorate, ClO3^–	chloric acid, HClO3
perchlorate, ClO4^–	perchloric acid, HClO4
cyanide, CN^–	hydrocyanic acid, HCN
hydroxide, OH^–	formed by bases in water
bicarbonate or hydrogen carbonate, HCO3^–
bisulfate or hydrogen sulfate, HSO4^–
dihydrogen phosphate, H2PO4^–
permanganate, MnO4^–
–2
carbonate, CO3^2–	carbonic acid, H2CO3
sulfate, SO4^2–	sulfuric acid, H2SO4
sulfite, SO3^2–	sulfurous acid, H2SO3
chromate, CrO4^2–	chromic acid, H2CrO4
peroxide, O2^2–
biphosphate or hydrogen phosphate, HPO4^2–
dichromate, Cr2O7^2–
thiosulfate, S2O3^2–	(thio: S substituted for O atom)
disulfide, S2^2–
–3
phosphate, PO4^3–	phosphoric acid, H3PO4
–4
silicate, SiO4^4–	silicic acid, H4SiO4

Stoichiometry: Mole-Mass Relationships

• A reaction equation is a molecular equation; the masses of individual molecules are too small for routine use; ...