Compound H (C8H6O3) gives a precipitate when treated with hydroxylamine inaqueous

CH 2230 CHAPTER 1 9/9/2017  How Single Bonds are Formed in Organic Compounds (1.7) o To be able to form four bonds, carbon must promote an electron from an s orbital to an empty p orbital o Carbon forms bonds using hybrid orbitals o Bonding pairs and lone-pair electrons around an atom stay as far apart as possible o All single bonds in organic compounds are σ bonds  How Double Bonds are Formed: Bonds in Ethene 2 o A double bond consists of one σ bond and π bond; the doubly bonded carbon is sp hybridized  How Triple Bonds are Formed: Bonds in Ethyne (1.9) o A triple bond consists of one σ bond and two π bonds; the triply bonded carbon is sp hybridized  Bonds in the Methyl Cation, the Methyl Radical, and the Methyl Anion o Carbocations and carbon radicals form bonds using sp orbitals; carbanions form bonds using 3 sp orbitals  Bonds in Ammonia and in the Ammonium Ion(1.11) o The nitrogen in NH3 forms three covalent bonds and has one lone pair o The bond angles in a molecule indicate which orbitals are used in bond formation o Nitrogen hybridizes four orbitals b/c it forms three bonds and has one lone pair o All bond angles are 109.5 o  Bonds in Water o Oxygen in water forms two covalent bonds and has two lone pairs o Experimentally observed bond angle in H O is 104.5