Lewis Structures. Lewis Structures. Lewis Structures. Lewis Structures. What pattern do you see? What pattern do you see?

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1 Look at the following chart: IA IIA IIIA IVA VA VIA VIIA VIIIA 2s1 2s2 2s22p1 2s22p2 2s22p3 2s22p4 2s22p5 2s22p6 The Roman Numerals are the Group numbers from the Periodic Table, Beneath them is the outer electronic structure of the elements in the 2nd row (Period) of the Periodic Table. What pattern do you see? IA IIA IIIA IVA VA VIA VIIA VIIIA 2s1 2s2 2s22p1 2s22p2 2s22p3 2s22p4 2s22p5 2s22p6 The Group Numbers tell you the number of outer electrons. These are called Valence electrons. One way of showing these valence electrons is by Dot- Diagrams IA IIA IIIA IVA VA VIA VIIA VIIIA 2s 1 2s 2 2s 2 2p 1 2s 2 2p 2 2s 2 2p 3 2s 2 2p 4 2s 2 2p 5 2s 2 2p 6 Li Be B C N O F Ne What pattern do you see? The Group Number becomes the number of dots you put around the element s symbol.

2 What are the four types of chemical bonds that you studied last semester? This pattern works for all the periods. Between metals: Between same element: Between different elements: Between far apart elements: Metallic Covalent Polar Covalent Ionic You can use these dot-diagrams to show how atoms bond together in POLAR COVALENT or COVALENT molecules (NOT IONIC molecules!). You can use these dot-diagrams to show how atoms bond together in POLAR COVALENT or COVALENT molecules (NOT IONIC molecules!). This: : When you do this, you are using Lewis Diagrams. Here are some examples: Not this: To show how the atoms bond together, you pair-up each atoms single electrons.

3 We are next going to use the Lewis Dot Symbols for the main group elements to represent the bonding and structure for various species, molecules, compounds and polyatomic ions. Diatomic Elements: H 2 Cl 2 N 2 O 2 all valence electrons for every atom will be included all shared pairs of e s will be indicated by a dash all unshared pairs of e s will be indicated by a dot We will use the octet rule as our guiding principle. Chlorine, Cl 2 (same for Br 2, F 2, I 2 ) N 2, Nitrogen: Check octets! NO OCTET STILL NO OCTET

4 Covalent triple bond OXYGEN ACTS LIKE THIS* CORRECT LEWIS STRUCTURE, Covalent double bond *Required whole new bonding theory to explain... Now it s time to Practice! Rules for Drawing Decide which atoms are bonded. Count ALL valence electrons. Place two electrons in each bond. Lewis Symbols and Structures - 1 Complete the octets of the atoms attached to the central atom by adding e- in pairs. Place any remaining electrons on the central atom in pairs. If the central atom does not have an octet, form double bonds or triple bonds.

5 Decide which atoms are bonded. Count ALL valence electrons. Decide on arrangement of atoms. For most species, the element written first in the molecule or ion is the central atom and the remainder of the atoms are grouped around it. Add up all available valence electrons. If species is cation, subtract positive charge from total. If species is anion, add negative charge to total. Hydrogen is a problem in oxo acids where it is written first in the formula. Ignore H, start with the next atom in formula and place the H or H s on the O or O s. Place two electrons in each bond. Step 1 Step 2 Place a pair of electrons between each pair of bonded atoms to represent a single bond (use either a pair of dots or dash!) Step 3

6 Complete the octets of the atoms attached to the central atom by adding e- in pairs. If the central atom does not have an octet, form double bonds or triple bonds. Step 4 Examine central atom to determine if a double or triple bond is required to achieve the central atom s octet. Do so using unshared pairs, IF central atom is: C, N, P, O, S No Step 5 needed N, octet Rules for Drawing Decide which atoms are bonded. Count ALL valence electrons. Place two electrons in each bond. Complete the octets of the atoms attached to the central atom by adding e- in pairs. Place any remaining electrons on the central atom in pairs. Writing for Ionic Compounds is even easier. Since each atom gains or loses electrons to reach its nearest nobel gas configuration, all you have to do is to locate each element in the Periodic Table and determine the number of electrons it must gain or lose. If the central atom does not have an octet, form double bonds or triple bonds.

7 For example: Sodium and chlorine combined: Na + + Cl Lithium and oxygen combined: 2Li + + O 2- Potassium and sulfur combined: 2K + + S 2- Now it s time to Practice! Lewis Symbols and Structures - 2

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