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Covalent Bonding

Covalent Bonding. Ms. Keller WTHS Chemistry. General Covalent- ness. Covalent bond - bond that results from the sharing of valence electrons. Diatomic molecule: elements that are bonded to itself in nature Br I N Cl H O F. General Covalent stuff con’t. Types of bonds:

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Covalent Bonding

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  1. Covalent Bonding Ms. Keller WTHS Chemistry

  2. General Covalent-ness • Covalent bond- bond that results from the sharing of valence electrons Diatomic molecule: elements that are bonded to itself in nature Br I N Cl H O F

  3. General Covalent stuff con’t • Types of bonds: • Single = sigma bond • Double = sigma bond + pi bond • Triple = sigma bond + 2 pi bonds Lone pair • Bonds are electron pairs that are being shared • Lone Pairs- unshared pairs of electrons

  4. Bond Lengths • Bond Length-distance between the nuclei of the 2 atoms that are bonded when they are the most attracted to one another • Determined by: • Size of the atoms • How many electron pairs are shared (how many bonds there are) • As # of bonds , the bond length 

  5. Energy and Bonds • Bond dissociation energy- amount of energy needed to break a specific covalent bond • Breaking bonds ALWAYS requires the addition of energy • Endothermic vs. Exothermic

  6. Naming Binary Molecular Compounds! • 1st element + 2nd element with the ending -ide • Use the following prefixes to indicate the number of the atoms of each element present: 1. mono 6. hexa 2. di 7. hepta 3. tri 8. octa 4. tetra 9. nona 5. penta 10. deca

  7. Naming Acids! • Binary method: • 1. prefix = hydro (to represent hydrogen) • 2. root of 2nd element • Change ending to –ic acid • Ex) HF = hydrofluoric acid

  8. Naming Acids! • Oxyacids: Acids that contain oxygen • Don’t put Hydro in for hydrogen! • If the group ends in –ate, it changes to –ic • If the group ends in –ite, it changes to –ous • ATE –IC, ITE –OUS • Throw acid on the end • Ex) H2SO4 = Sulfuric Acid • Ex) H2SO3 = Sulfurous Acid

  9. Let’s Practice Naming… • C2O4 • NO2 • C4H10 • SO3 • N2O5 • HCl • HBr • H3PO4 • HClO2

  10. Writing Formulas • Just read the name! • The prefix tells you how many of each element you have – this is your subscript! • Ex) carbon tetrafluoride = CF4 • Because tetra=4 and it’s attached to fluorine, it becomes the subscript

  11. How to Draw Lewis Structures for Covalent Bonding • Add up all valence electrons • Add up all octets that need to be filled (octet=2 for H) • Subtract step 1 from step 2 • Divide value from step 3 by 2 to get how many bonds are in the molecule Ex) CH4

  12. How to Draw Lewis Structures for Covalent Bonding Some hints for how they fit together: • Element closest to the left is usually the central atom • Hydrogen is always terminal (on the end)

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