chapter 8 notes mr nelson 2010. chemical bonds three basic types of bonds –ionic electrostatic...
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Chapter 8 Notes
Mr Nelson 2010
Chemical Bonds• Three basic types of bonds
– Ionic• Electrostatic attraction between
ions
– Covalent• Sharing of electrons
– Metallic• Metal atoms bonded to several
other atoms
Ionic Compounds – Review
• Made up of ions– Cations (+) & Anions (-)– Metals & Nonmetals (or polyatomic ions)
• Exchange of electrons
• Charges Balance
Molecular Compounds – Intro
• No ions– Charges will not balance– Composed of two nonmetals
• Sharing of electrons– Covalent bonding
• Naming is based on prefixes
Nomenclature of Binary Compounds
• If both elements are nonmetals we must use prefixes.
• The 1st element only gets a prefix if it is greater than 1.
• 2nd element always gets a prefix and change the ending to -ide
Nomenclature of Binary Compounds
• Example of a molecular comp:
• CO2
• CO
• CCl4
Practice
• PCl5 dihydrogen monoxide
• SF6 carbon trichloride
• N2O disulfur hexoxide
• NO2 nitrogen triiodide
Naming Acids
• An acid is any compound that starts with a hydrogen
• When naming an acid:– 1st locate the anion (- charge)
Acid Nomenclature
• If the anion in the acid ends in –ide (not PI)
• change the ending to -ic acid and add the prefix hydro-
hydro________ic acid
– HCl
Acid Nomenclature
• If the anion in the acid ends in –ate (all PI’s)
• change the ending to -ic acid.
___________ic acid
– HClO3
Acid Nomenclature• If the anion in the acid ends in –ite (all PI’s) • change the ending to -ous acid.
_________ous acid
– HClO2
Acids – Finishing Up• If you have the name and need to find the formula
– Example: Acetic Acid– Cross off the –ic and add at –ate
– Acetate! = C2H3O2-
• Finish by adding the correct # of H’s (1 for every negative)
• HC2H3O2 is acetic acid
Warm Up
• HBr Chlorous Acid
• FeS Copper(I) fluoride
• PBr5 dinitrogen dioxide
• K2SO4 nitrogen monoxide
• CCl4 hydroiodic acid
• HNO3 potassium nitrate
• LiCl phosphoric acid
Covalent Bonding• Covalent bond – atoms share electrons.
• There are several electrostatic interactions in these bonds:– Attractions between electrons and nuclei
– Repulsions between electrons
– Repulsions between nuclei
Lewis Dot Structures
• ONLY Valence (outer) electrons are involved.
• Lewis dot structures can be drawn for:– atoms – molecules
• Lewis dot structures show structure of a molecule, and help predict shape.
Steps to Writing Lewis Structures1. Find the sum of valence
electrons of all atoms in the polyatomic ion or molecule.
PCl3
5 + 3(7) = 26
Writing Lewis Structures
2. Arrange element symbols to show how atoms are connected – show electrons as dots.
Draw in the valence electrons of each of the atoms
Keep track of the electrons:
Writing Lewis Structures
3. Connect the lines to form single bonds. 1 line = 2 electrons
Keep track of the electrons:
Writing Lewis Structures
4. Finish by checking for octets. Hydrogen only needs
2 electrons to be happy
Keep track of the electrons:
Writing Lewis Structures
5. If the central atom does not have an octet…
…form multiple bonds until it does. Example: HCN
Exceptions!
• Boron and Aluminum are okay with only 6 e- around them– BF3
Exceptions
• If the Lewis Dot Structure you are drawing is an ion: – Use [] and specify the charge– Add or subtract electrons
• Positive charges take away electrons
• Negative charges add electrons
• Example: Br-
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