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Covalent Bonds

Covalent Bonds. Bonding Atoms - Review. Why do atoms bond? Each atom wants a full outermost energy level How do they do this? By gaining, losing, or sharing valence electrons to achieve octet rule aka: “being happy or stable”

michael-beard
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Covalent Bonds

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  1. Covalent Bonds

  2. Bonding Atoms - Review • Why do atoms bond? • Each atom wants a full outermost energy level • How do they do this? • By gaining, losing, or sharing valence electrons to achieve octet rule aka: “being happy or stable” • Gives each atom an electron configuration similar to that of a noble gas

  3. Types of Bonding • Ionic Bond • Gives / Takes Electrons • One atom will give an electron to another atom • Covalent Bond • Share electrons • Two elements will share electrons between them so they are both “happy” / stable • Polar Bond • We aren’t going to cover

  4. Covalent Bonds • A chemical bond in which two atoms share a pair of valence electrons • Always formed between nonmetals

  5. Steps to Covalent Bonds • Step 1: Draw the Bohr Model OR the Lewis Dot Diagram • Step 2: Put circles around the electrons that are being shared • Step 3: Redraw the diagrams replacing the circled dots with lines • Step 4: Write the compound

  6. Step by Step Covalent Example • Hydrogen and Hydrogen • Step 1: Draw the Bohr/ Lewis Dot Diagram • Step 2: Put a circle around the shared electrons • Step 3: Replace the circle with a solid line • Step 4: Write the completed compound H2

  7. Practice Problem • Hydrogen and Oxygen • Hydrogen needs 1 additional electron to fill its outer shell • It only have 1 to share • THEY MUST SHARE EQUAL NUMBERS • Oxygen needs 2 more electrons to fill its outer shell • ** This tells us that one hydrogen isn’t enough

  8. Hydrogen and Oxygen • Step 1/2: • Step 3: • Step 4:

  9. Covalent Bonds • Single Bonds • One electron is shared between 2 elements • Double Bonds • Two electrons are shared between 2 elements • Triple Bonds • Three electrons are shared between 2 elements

  10. Double Bond Example • Oxygen and Oxygen • Both have 6 electrons and NEED 2 more • They can both share 2 • Step 1/2 • Step 3 • Step 4

  11. Two Types of Covalent Bonds • Diatomic • Two of the same elements are bonded • Aren’t found alone. Always found together or bonded to other elements • ONLY the following • H O N Cl Br I F • Polytomic • More than 2 elements are bonded together

  12. https://www.youtube.com/watch?v=QIfTT-_-xLo

  13. Characteristics of covalent compounds • Low melting and boiling points • Solubility and electrical conductivity • Do NOT dissolve well in water. • At room temperature covalent substances are gases, or liquids or low melting point solids.

  14. Naming Covalent Compounds • Look at the 1st Element • If only 1 – just use the element name • If more than 1 – use the correct prefix • Look at the 2nd Element • If its an element use the chart above • If it’s a compound use the compound chart

  15. Naming Covalent Compounds • Prefix System prefix # of atoms mono (1) di (2) tri (3) tetra (4) penta (5) hexa (6) hepta (7) octa (8) nona (9) deca (10)

  16. Polyatomic Ions Cont. • Common Polyatomic Ions

  17. Name the following compounds 1. SiO2 2. PBr3 3. CI4 4. N2O3

  18. Naming Covalent Compounds Cont. Naming covalent compounds from formula 1. SiO2 = Silicon dioxide 2. PBr3 =Phosphorus tribromide 3. CI4 = Carbon tetraiodide 4. N2O3 = Dinitrogen trioxide

  19. Writing Formulas for Covalent Compunds Writing formulas from names • Carbon Dioxide CO2 • DinitrogenPentoxide N2O5 3. Triphosphorusmonosulfide P3S 4. Sulfur MonobromideSBr

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