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Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
Unit 4    Bonding
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Unit 4 Bonding

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  • 1. UNIT 4 - Bonding (Ch. 6 & 7) Let’s get molecular!!!!
  • 2. Why do elements form compounds?
    • What’s the attraction?
    • Molecules - made up of 2 or more atoms to form ONE unit or compound
    • Molecular compounds are usually gases or liquids
      • Consist of 2 or more nonmetals
        • (Where are nonmetals located on P.T?)
  • 3. Examples
    • Water….. H 2 O
      • 2 molecules of hydrogen
      • 1 molecule of oxygen
    • Sucrose (sugar)…. C 6 H 12 O 6
      • 6 molecules of Carbon
      • 12 molecules of Hydrogen
      • 6 molecules of Oxygen
  • 4. Properties of Covalent Bonding (molecular bonding)
    • Share electrons
    • Low melting point
    • Do not conduct electricity when dissolved
    • Bond with 2 or more NONMETALS ONLY
  • 5. Diatomic Elements (molecules)
    • KNOW THESE!!!!!
      • H 2 , N 2 , O 2 , F 2 , Cl 2 , Br 2 , I 2
    • These 7 elements exist in nature as DIATOMIC!!!
      • Want a stable octet soooooo badly they will bond with themselves!
  • 6. Single vs. Double vs. Triple bonds
    • Draw Lewis Dot structure for:
      • H N O Cl
    • How many electrons will each element need to “share” to be “HAPPY?”
  • 7.
    • Single bond – one pair of electrons shared
    • Double bond – two pairs of e- are shared
    • Triple bond – three pairs of e- are shared
    • Which bond would be the strongest? Weakest?
    Single vs. Double vs. Triple bonds
  • 8. Single vs. Double vs. Triple Bonds
    • Which diatomic molecules will form a single bond? Double? Triple?
  • 9. Writing/Naming Covalent
    • Know your Prefixes
      • 1 – mono
      • 2 – di
      • 3 – tri
      • 4 – tetr(a)
      • 5 – pent(a)
    • (Table 9.4)
      • 6 – hex(a)
      • 7 – hept(a)
      • 8 – oct(a)
      • 9 – non(a)
      • 10 – dec(a)
  • 10. Rule 1: Ex. N 2 O
    • If the 1 st nonmetal has MORE than ONE molecule, use the prefix.
    • Always use prefix when naming 2 nd nonmetal
    • Change ending to “ide”
    • (oxygen….oxide)
    • diNitrogen monoxide
  • 11. Rule 2: Ex. PCl 3
    • If the 1 st nonmetal has only ONE molecule, do NOT use prefix.
    • Always use prefix when naming 2 nd nonmetal
    • Change ending to “ide”
      • (Chlorine…..Chloride)
    • Phosphorous trichloride
  • 12. Your Turn:
    • Name the following:
      • SO 3
      • N 2 O 4
      • P 2 O 5
      • CO
      • NH 3
  • 13. More Practice
    • Write the formula for the following covalent compounds:
      • Carbon disulfide
      • Disulfur dichloride
      • Oxygen trifluoride
      • Tetraphosphorous decoxide
  • 14. Welcome to Ionic Bonding You better learn your Polyatomic Ions!!
  • 15. IONIC BONDING
    • Properties:
      • Bond btwn Metal and Nonmetal
        • Cations/Anions????
      • Transfer electrons
      • Strong bond b/c of opposite charges
      • Forms Crystal Lattice structure
      • High melting pt.
      • Conduct electricity when dissolved in water
        • Breaks bonds apart so only “ions” remain
  • 16. Review Ion formation
    • Cations:
    • Na
      • Na +1
    • Mg
      • Mg +2
    • Naming:
    • Name of metal
      • Na +1 …sodium
      • Mg +2 …magnesium
    • Anions:
    • Cl
      • Cl -1
    • O
      • O -2
    • Naming:
    • Change ending to “-ide”
      • Cl -1 …chloride
      • O -2 …oxide
  • 17. Writing Binary Ionic Formulas
    • Total “charge” of formula must equal ZERO
    • Always write Metal FIRST!
      • Ex. Sodium Chloride
      • Ex. Calcium Chloride
      • Ex. Potassium Sulfide
  • 18. Naming Binary Ionic
    • DO NOT use PREFIXES!!! (covalent only)
    • Write name of cation FIRST, then change ending of anion to “-ide”
      • Ex. LiBr
      • Ex. MgCl 2
      • Ex. Sr 3 N 2
  • 19. Naming using Roman Numerals
    • Use R.N for ALL metals EXCEPT groups IA, IIA, Al, Zn, Ag
      • Ex. Copper(II) = Cu 2+
      • Ex. Lead(IV) = Pb 4+
      • Ex. Chromium(III) = ???
  • 20. Naming using Roman Numerals
    • First Ask, do I need to use a roman numeral?
    • What does the R.N tell me?
      • Ex. CuCl 2
      • Ex. PbS

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