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  • Home / Ask Me Stuff
  • Free Lessons
    • Thermodynamics >
      • Thermochemistry Worksheet + Answers
      • First Law of Thermodynamics
      • Pressure-Volume Work
      • Enthalpy
      • Hess' Law
      • Enthalpy of Formation
      • Heat Capacity
      • Calorimetry
      • Entropy
      • Third Law of Thermodynamics
      • Spontaneity: Gibbs Free Energy
      • Second Law of Thermodynamics
      • Spontaneity at Different Temperatures
    • Electrochemistry >
      • Redox Reactions
      • Introduction to Half-Reactions
      • Calculating Oxidation Number
      • Has a Redox Reaction Occurred?
      • How to Balance Redox Reactions (Acidic Solution)
      • How to Balance Redox Reactions (Basic Solution)
      • Galvanic Cells
      • Standard Reduction Potentials
      • Electrolytic Cells
      • Nernst Equation
    • Kinetics >
      • Introduction
      • Relative Rates of Reaction
      • Rate Laws
      • Zero-Order Reactions
      • First-Order Reactions
      • Second-Order Reactions
      • Half-Life Expressions
      • Arrhenius Equation
      • How Long will it Take to Decay?
      • What Order is this Reaction?
      • Find the Rate Constant
    • Gases >
      • Pressure, Volume, Temperature
      • Ideal Gas Law
      • Density of Gases
      • Ideal Gas Law and Changes in P, V, T
      • Kinetic Molecular Theory
      • van der Waals' Equation for Non-Ideal Gases
      • Partial Pressures
      • Kinetic Energy and Temperature
    • Equilibrium >
      • Writing Equilibrium Expressions
      • Le Chatelier's Principle
    • Acids and Bases >
      • Acids and Bases Worksheet + Answers
      • Arrhenius vs Bronsted-Lowry vs Lewis Acids
      • Solve Titration Questions
    • Intermolecular Forces >
      • Phase Diagrams
      • Phase Changes
      • Intermolecular Forces
      • Effects of Intermolecular Forces
      • Ranking by Boiling/Melting Point
      • Clausius-Clapeyron Equation
      • Heating Curves
    • Solids >
      • Ionic/Metallic/Covalent
      • Symmetry of Solids
      • Simple Cubic, fcc and bcc
      • How to Find Edge Length
    • Organic Reactions >
      • Br2 + Alkene (Adding across a double bond)
      • HCl + Alkene (Adding across a double bond)
      • Reaction of OH with Alkyl Halide
      • What is Regioselectivity?
      • Stability of Carbocations
    • Moles and Mass >
      • Average Atomic Mass
      • Solve for Isotopic Abundance
      • Limiting Reagents
      • Percent Yield
      • Actual Yield and Percentage Yield
      • Percent Composition
    • Atomic Structure >
      • What's in an Atom?
      • Quantum Numbers
      • Pauli, Aufbau, Hund
      • Light: E h ν λ
      • Energy Levels of Hydrogen
      • Energy Levels of Non-Hydrogen Atoms
    • Organic Naming >
      • Naming Organic Molecules
      • How to Name Amines
      • How to Name Amides
    • Lewis Structures
  • Privacy Policy
  • Free Help on Discord

The Four Types of Solids


Covalent Networks (Wikipedia Link)
  • Atoms are connected in long chains by covalent bonds.
  • Recall: Covalent bonds occur when two atoms share electrons and are very strong.
  • Because it takes a lot of energy to break covalent bonds, these solids have very high melting points (Ever see a diamond melt?)
  • Examples of covalent networks include diamond, graphite and quartz.
Picture

Metals (Wikipedia Link)
  • Metals are considered to have a different structure: Atoms arranged symmetrically, with a sea of electrons floating around them.
  • We assume the electrons are mobile around the atoms because metals conduct electricity so well.
  • Because there is no polarity or direction to the solid, it's easier to melt (the metal mercury (Hg) is a liquid at rom temperature!) and usually ductile (easily made into wire).
  • Examples are obvious: aluminum, copper, gold, sodium...
Picture

Ionic Solids (Wikipedia Link)
  • Positive and negative ions are held together by ionic bonds - the attraction between positively- and negatively-charged ions.
  • These bonds are tough to break as well, so ionic solids have high melting points and low vapour pressures.
  • Because the electrons are held tightly by the negative ions, these solids do not conduct electricity.
  • They are soluble because they are made of ions, and so are easily dissolved by polar water molecules.
  • Examples include sodium chloride (table salt) and calcium carbonate (chalk).
Picture

Covalent Solids (aka Molecular Solids) (Wikipedia Link)
  • These are solids formed when individual covalent (molecular) molecules freeze.
  • Water, methane, carbon dioxide, sugar (glucose, sucrose), and octane molecules have a distinct chemical formula and are made of individual molecules, which form a "covalent (molecular) solid" when frozen.
  • These solids are held together by Intermolecular Forces (dipole-dipole forces, London dispersion forces, hydrogen bonds)
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