Chemistry: a QuickStudy Laminated Reference Guide
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About this ebook
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
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Chemistry - BarCharts, Inc.
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