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CSU - CHEM 111 - Class Notes - Week 7

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CSU - CHEM 111 - Class Notes - Week 7

School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Tags:
Name: Chem 111 week 7
Description: - Naming compounds (ionic and molecular) - Lewis structures - Octet rule - Bonding framework - Formal charges - Exceptions to octet rule
Uploaded: 03/19/2018
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background image 4.3 Nomenclature: Naming ionic compounds Write the name of the cation followed by the name of the anion, which ends in -ide *Do not specify the number of atoms because the charge is implied* Ex: NaCl: Sodium chloride Ba₃N₂: Barium nitride If the cation has more than one possible charge, write the charge as roman 
numerals in parentheses
*This is for most transition metals* Ex: FeCl₂: Iron (II) chloride Fe₂Cl₃: Iron (III) chloride For polyatomic ions use the polyatomic name (do not put -ide on the end of the 
name)
Naming binary molecular compounds The first element retains its name The second element end in -ide Prefixes denote the number of atoms of each element *Mono is emitted from the first element* *If the prefix ends in a vowel and the element starts with a vowel remove the  ending prefix vowel (except for di and tri)* Ex: CO: Carbon monoxide CO₂: Carbon dioxide Mono- 1 Di- 2 Tri- 3 Tetra- 4 Penta- 5 Hexa- 6 Hepta- 7
Octa-
8 Nona- 9 Deca- 1
0
background image CCl₄: Carbon tetrachloride N₂O₅: Dinitrogen pentoxide IF₇: Iodine heptafluoride 4.3 Lewis Symbols and Structures Symbols indicate the number of valence electrons an atom has (1 dot represents 1 
valence electron)
We can predict the number of bonds that an atom typically forms from its valence 
electrons and position on the periodic table
Shared pair of electrons (covalent bonds) are shown as lines Lone pairs of electrons (unbounded) are shows as a pair of dots The octet rule Atoms lose, gain, or share electrons in order to take on the same number of  electrons as their nearest noble gas neighbor (typically 8 except for H which is 2) F needs 1 more electron to have a full octet (8 electrons) so it likes to  form 1 bond O needs 2 more electrons to have a full octet so it likes to form 2 bonds N needs 3 more electrons for a full octet so it likes to form 3 bonds C needs 4 more electrons to have a full octet so it likes to form 4 bonds Lewis symbols for binary ionic compounds Electrons are completely transferred, not shared (so there are no lines shown) this is shown by the [box] around each element and the charge it has
background image Multiple bonds Double bond- two electron pairs are being shared O+C+O Triple bond- three electron pairs are being shared N+N Bonding framework Outer atoms bond to only one other atom Usually a low bonding capacity Hydrogen is always outer Inner atoms bond to more than one other atom Usually a higher bonding capacity Usually a lower electronegativity Carbon is always inner Drawing Lewis structures

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School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Tags:
Name: Chem 111 week 7
Description: - Naming compounds (ionic and molecular) - Lewis structures - Octet rule - Bonding framework - Formal charges - Exceptions to octet rule
Uploaded: 03/19/2018
11 Pages 89 Views 71 Unlocks
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  • Notes, Study Guides, Flashcards + More!
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