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Exploring Chemical Bonding: Metallic, Ionic, Network, and Covalent Bonds

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bviola
24 diapositives · 264 Views · Jan 06, 2020

Learn about the different types of chemical bonds - metallic, ionic, network, and covalent - and their properties, structures, and examples. Understand the concepts of sharing electrons, transferring electrons, and how bonds impact material properties.

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  1. Warm Up: • Draw Lewis dot diagrams for sodium and chlorine.

  2. BONDING

  3. Chemical bond: mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

  4. Intramolecular Bonds • Bonds between atoms in a compound

  5. Making a bond releases energy (exothermic) • Breaking a bond requires energy (endothermic)

  6. Different types of bonds… • Metallic • Ionic • Network • Covalent

  7. 1. Metallic • Type of bond between typical metals like copper, iron, sodium, zinc, etc. • Recall metals have 1, 2 or 3 valence electrons Sea of mobile electrons

  8. Kernel: part of the atom which excludes valence electrons • kernels are packed next to each other in a regular pattern • valence electrons of all the atoms spread out over the outer surfaces of the metal

  9. Metallic Properties • Because valence electrons are not bound to any particular atom, they can move about on the surface quite easily • Good electrical and heat conductivity • Malleable • Ductile • luster

  10. 2. Ionic (Electrovalent) • Results from the electrical attraction between cations and anions • Transfer of electrons [ ] [ ]

  11. Alkali Hydrides • Are considered ionic • NaH, LiH

  12. Ionic Structure • Crystal lattice • Orderly arrangement of ions

  13. Properties of Ionic Substances • Solid at STP • High melting points • Hard and brittle • Poor conductors of heat • Poor conductors of electricity in solid phase but good conductors in liquid or aqueous phase

  14. Warm Up: • What type of bonding has a kernel surrounded by a sea of mobile electrons? • What type of bonding transfers electrons?

  15. 3. Network Bonding • Characterized by sharing of valence electrons of each atom with each neighboring atom • Forms a network throughout entire sample • Diamond, graphite, silicon carbide (SiC), silicon dioxide (SiO2)

  16. Characteristics of Network Solids • Solid at STP • High melting points • Hard and brittle • Poor conductors of heat and electricity • Orderly arrangements of atoms in network structure

  17. 4. Covalent • Results from the sharing of electron pairs between 2 atoms • Nonpolar Covlalent: bonding electrons are shared equally • Polar Covalent: bonded atoms have an unequal attraction for the shared electrons • Coordinate covalent- formed when both electrons of the shared pair are provided by the same atom

  18. Nonpolar Polar Methane (CH4)

  19. Coordinate Covalent Ammonia (NH3)

  20. Coordinate Covalent Hydronium ion (H3O+)

  21. Covalent Structure • Molecule

  22. To determine which type of bond… • Calculate the difference in electronegativities Non-polar covalent Polar Covalent Ionic 0.3 1.7 Increasing ionic character

  23. Identify these as ionic, polar covalent, nonpolar covalent, metallic, network solid • Cl2 • H2O • CH4 (methane) • HCl • Al • SiO2