1 / 24

Warm Up:

Warm Up:. Draw Lewis dot diagrams for sodium and chlorine. BONDING. Chemical bond: mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together. Intramolecular Bonds. Bonds between atoms in a compound.

bviola
Download Presentation

Warm Up:

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related