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Topic :Intro to Organic Chemistry – hydrocarbons

Topic :Intro to Organic Chemistry – hydrocarbons. Do Now: read – amazing carbon . Organic chemistry = carbon compounds (except oxides, carbides (C + element that is less electronegative), & carbonates). Bonding Capacity . H can form only 1 bond

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Topic :Intro to Organic Chemistry – hydrocarbons

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  1. Topic :Intro to Organic Chemistry – hydrocarbons Do Now: read – amazing carbon

  2. Organic chemistry = carbon compounds (except oxides, carbides (C + element that is less electronegative), & carbonates)

  3. Bonding Capacity • H can form only 1 bond • The halogens (F, Cl, Br, I) form only 1 bond • O and S like to form 2 bonds • N and P form 3 bonds • C form 4 bonds

  4. Why so many C compounds? • Carbon atoms can bond with other carbon atoms in chains, rings, and networks • Bonds are covalent

  5. Lewis Diagram of C • • C • • Carbon has 4 unpaired electrons so it can form 4 covalent bonds

  6. We will be looking at 3 Homologous Series of Hydrocarbons (all are covalent molecules)AlkanesAlkenesAlkynes • Hydrocarbons: organic compounds containing only C and H • Homologous series = group of compounds with related structures &properties • molecules have fixed, numerical relationship among # of atoms See table Q

  7. Alkanes • Homologous series of saturated hydrocarbons • Release energy when burned • CnH2n+2 – all have this general formula Saturated hydrocarbons: organic compounds containing only Single bonds – can’t add any more Hydrogens

  8. Alkenes • homologous series of unsaturated hydrocarbons (can add more H by breaking the bond) • Each member contains at least one double covalent bond between C atoms • General formula = CnH2n

  9. Alkynes • Homologous series of unsaturated hydrocarbons • Each member contains at least one C≡C bond • General formula = CnH2n-2

  10. Properties of Covalent Substances(also called molecular substances) • Low melting points, low boiling points • Poor conductors of heat & electricity • May be soft or brittle • Generally nonpolar • van der Waals forces • Tend to dissolve in nonpolar solvents • React more slowly than ionic compounds

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