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Chemistry: a QuickStudy Laminated Reference Guide
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About this ebook
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:
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
LanguageEnglish
PublisherBarCharts, Inc.
Release dateNov 30, 2009
ISBN9781423212553
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Reviews for Chemistry
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Book preview
Chemistry - BarCharts Publishing, Inc.
CHEMISTRYPeriodic TableorbitalsCHEMISTRY
Periodic Table of Elements
Elemental forms:
Monatomic: Noble gases: helium, neon, argon, krypton, xenon, and radon; nonreactive
Diatomic: Gases: fluorine, chlorine, hydrogen, oxygen, and nitrogen; Liquid: bromine; Solid: iodine
Molecular solids: Sulfur
Covalent solids: Carbon (diamond, graphite)
Metals: Most common type of element; high coordination numbers; very dense
Types of compounds: Large variety due to ionic, covalent, and metallic bonding options
Ionic: Electron exchange
Covalent: Shared electrons
Polar covalent: Unequal sharing
Ion complex: Central ion + Solvent
Transition metal compounds:
Coordination compound: Nonbonding ligands
Organometallic: Metal-C bond
Complex minerals: Metal oxides and silicates
Periodicity: The chemical properties of an element depend on valence electrons
Family of elements: Column in periodic table
The addition of d-orbitals produces an expanded octet
Periodic Trends
Chemistry determined by the behavior of valence electrons
Atoms or ions get larger as you go down the column; electron shells are added
Cation and anions (same charge) decrease in size as the atomic number (Z) increases
Ionization energies: Noble gases are the most stable; alkali metals are the easiest to ionize; electron screening lessens Z-effect on orbital energy
Atomic and ionic radii: Not real properties; derive from structural data; divide bond into radii using a consistent scheme
Ionic radius: Depends on charge, counter ion, and coordination (crystal type)
Atomic radius: Based on diatomic gas data or metallic solid structural data
Development of the Periodic Table
Missing elements were predicted using periodicity
Column 1: Alkali metals
Column 2: Alkaline earth metals
First transition series: Titanium– Copper
Column 17: Halogens: fluorine, chlorine, bromine, iodine, and astatine
Column 18: Rare gases: helium, neon, argon, krypton, xenon, and radon
Actinides: Z = 90 or above; radioactive
Lanthanides: f-subshell elements; starts with Z
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