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Lewis Dot Molecular Structures

Lewis Dot Molecular Structures. Introduction. To this point we have studied the three main types of bonds Ionic Covalent Metallic

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Lewis Dot Molecular Structures

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  1. Lewis Dot Molecular Structures Introduction • To this point we have studied the three main types of bonds • Ionic • Covalent • Metallic • We have examined how these bonds form, how to predict what type of bond a pair of atoms will form, and the characteristics of the substances that possess these bond types. • For the rest of this unit, we are going to focus our study on covalently bonded substances.....molecules • Today, we will explore their structures

  2. Lewis Dot Molecular Structures A Little Review Which electrons appear in Lewis Dot Structures? Valence electrons How many dots can there be? 8 What sublevels do these electrons occupy? Highest s and/or p How are these 8 electrons distributed in the sublevels? 2 in the s, 6 in the p How many orbitals do these 8 electrons occupy? 1 s orbital and 3 p orbitals Define the octet rule.... When atoms bond, they are most stable when they have a complete octet of 8 valence electrons

  3. Lewis Dot Molecular Structures Lewis Dot Structures: Structural formulas • Structural formula: a model that shows how atoms are arrange in molecules • Around each element’s symbol, draw a dot for each valence e- N O H Hydrogen Nitrogen Oxygen Spread out the electrons as much as possible Cl C C Chlorine Carbon

  4. Lewis Dot Molecular Structures Putting them Together(Begin taking notes here) • These Lewis Dot structures can then be put together, like puzzle pieces, to form molecules O H Bonding Sites H

  5. Lewis Dot Molecular Structures Putting them Together Non-bonding (lone) electron pairs O H Bonding (shared) electron pairs H

  6. Lewis Dot Molecular Structures • Helpful Hints: • Put all the atoms “on paper” - single bonding them together • Often the bonding order is given in the name • Carbon is often in the middle • Halogens and Hydrogen won’t be in the middle

  7. Lewis Dot Molecular Structures • Helpful Hints: • Count all the valence electrons for every atom, watch ions! • Spread the valence electrons evenly around the molecule • Check and fill octets by multiple bonding if necessary

  8. Lewis Dot Molecular Structures • Helpful Hints: • Draw the LDMS for the following molecules and count the shared and lone pairs of electrons around the central atom • C2H6 • C2H4 • NH4+ • CO2 • N2

  9. Lewis Dot Molecular Structures • Helpful Hints: • Draw the LDMS for the following molecules and count the shared and lone pairs of electrons around the central atom • C2H6 • H • H • H • C • C • H • H • H

  10. Lewis Dot Molecular Structures • More examples: • C2H4 • NH4+ + ] [ • H • H • H • C • C • H • N • H • H • H • H Double bond! Check total electrons for ions

  11. Lewis Dot Molecular Structures • More examples: • CO2 • N2 • O • C • O • N • N Double bonds! Triple bond!

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