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Understanding Ionic, Covalent, and Metallic Compounds in Chemistry

Learn about the properties, structures, and bonding in ionic, covalent, and metallic compounds. Explore how atoms form different types of bonds and arrange themselves in crystalline solids.

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Understanding Ionic, Covalent, and Metallic Compounds in Chemistry

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  1. Chapter 7: Properties of Ionic Covalent and Metal Materials

  2. Types of Atoms Ionic Compounds: Ions (Cations & Anions) Covalent (Molecular Compounds): Two or more nonmetal atoms Metallic Solids: Only metal atoms

  3. Bond formation Bond formation Ionic Compounds: Transfer of electrons Form Ionic bonds Covalent (Molecular Compounds): Sharing of electrons Form Covalent bonds Metallic Solids: Free moving valence electrons

  4. Properties Ionic Compounds: • At room temperature they are a crystalline solid. • Hard & Brittle, High melting point Covalent (Molecular Compounds): • At room temperature they can be a low-melting pt solid, liquid or gas. • Usually soft & low melting point

  5. Properties Metallic Solids: • Soft to very hard solids Why? Strength increases with an increase in # of e- available for bonding. • Low to very high melting points • Ductile: Metal can be drawn into thin wires • Malleable: Metal can be hammered into different shapes

  6. Compound Arrangement Ionic Compound • Three dimensional pattern How is the 3D pattern created? • Opposite charged ions form close-packed layers. • Layers stack together to make a regular repeating 3D pattern called a: Unit cell • Closely packed layers will keep stacking to form a: Crystal

  7. Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ An Ion Coordination Number Is the # of opposite- charged ions that surround an ion in a crystal How many Na+ surround Cl-?

  8. Compound Arrangement Molecular Compound • Consist of atoms (nonmetals) which form molecules. • The bonds between molecules are weak forces. Weak forces Water molecules

  9. vs. Ionic Compounds Molecular Compounds

  10. Compound Arrangement Metallic Solid • Consist of closely packed cations. How are metallic bonds formed? • They are formed from the attraction of free-moving valence electrons for the cations • These electrons bind the cations together to create a metallic solid.

  11. Electron cloud e- e- Form a bond

  12. Strength Type of Bond Force & Strength Ionic Compounds: Electrostatic forces Very Strong Covalent (Molecular Compounds): Intermolecular forces Weak Dispersion forces, Dipole-dipole, H-bonding Metallic Solids: A “sea” of Valence Electrons Strong

  13. Conductors Conductors Ionic Compounds: Good conductors of electricity(dissolved ionic compounds are electrolytes) Two ways ionic compounds conduct electricity: • Conduct an electric current in the melted state. • Conduct electricity when the compound is dissolved in water.

  14. Conductors Ionic Compounds cont… How do ionic compounds conduct electricity? • Bonds break (melt) or dissociate (dissolve). • The ions separate and are free tomove around. The ion movement produces a flow of electricity! • Apply voltage allowing the cations move to one electrode & the anions to the other.

  15. Conductors Molecular Compounds: Poor conductors Why? • Intermolecular bonds will break easily, but notformions.Covalent bonds (holding the molecule together) do not break easily. • Molecular compounds do not readily disassociate in water. • Molecular compounds do not contain ions that can conduct electricity.

  16. Conductors Metallic Solids: Good conductors of electricity Why? • Free-moving valence electrons Good conductors of heat Why? • Free-moving valence electrons

  17. Goodconductors of heat& electricity.

  18. Network Solids Network Solid • Consist of atoms held together by large network of covalent bonds. • Each atom is covalently bonded in a largechain or network. • There are NO moleculesin a network solid, onlyatoms bonded together. • Bonds are very strong. Example: Diamond

  19. Metallic solids can arrange its bonds to form 3 orderly patterns: Body-centered cubic Face-centered cubic

  20. Hexagonal close-packed Why are metallic solids the simplest crystalline solid?

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