M1

• Organic compounds are derived from or produced by living organisms and have carbon-hydrogen covalent bonds.
• Inorganic compounds are derived from nonliving components, and generally have ionic bonds, lack carbon-hydrogen bonds, and rarely, if ever, contain any carbon atoms.
• Carbon -" King of all Elements"

  Group IV, Period ll
• Carbon Allotropes:

  Graphite - softest allotrope of C

  Diamond - hardest allotrope of C

  Activated Charcoal -pure carbon
• Carbon is Tetravalent
• Hybridization - Mixing of 2 or more non-equivalent atomic to form a new set of equivalent hybrid orbitals.
• SP3 HYBRIDIZATION OF CARBON

  • When the carbon atom is bonded to four other atoms the hybridization is said to be sp' type. Here 1 s orbital and 3 p orbitals in the same shell of an atom combine to form four new equivalent orbitals. The arrangement is tetrahedral with a bond angle of 109.5 °.
  • Example: Hybridization of CH, (Methane)
• SP2 HYBRIDIZATION OF CARBON

  • A carbon atom is sp2 hybridized when bonding takes place between 1 s-orbital with two p orbitals. There is a formation of two single bonds and one double bond between three atoms. The hybrid orbitals are placed in a triangular arrangement with 120* angles between bonds.
  • Example: Hybridization of graphite
• SP HYBRIDIZATION OF CARBON

  • Carbon can have an sp hybridization when it is bound to two other atoms with the help of two double bonds or one single and one triple bond. When the hybridization occurs the molecules have a linear arrangement of the atoms with a bond angle of 180 °.
  • Example: CO2
• CATENATION

  • Ability to form bond with itself
  • Ability to form open-ended (straight) chain and close ended (ring) chain.
• Stereochemistry

  • the 'chemistry of space', that is
  • deals with the spatial arrangements of atoms and groups in a molecule.
• FORCES OF ATTRACTION

  • When the molecules interact, both repulsive and attractive forces operate in equilibrium for the stability of the molecule.
  • necessary for the molecules and atoms to cohere, whereas repulsive forces act to prevent molecules from interpenetrating and annihilating each other.
  • Repulsion increases exponentially as the distance between atoms or molecules.
• TWO TYPES OF FORCES OF ATTRACTION

  INTRAMOLECULAR FORCES

  • Forces that hold atoms together within a molecule
  • lonic, covalent, metallic bond

  2. INTERMOLECULAR FORCES

  • forces that hold molecules together as they exist as aggregates. van der Waals, ion- dipole, ion-induced dipole, hydrogen bonding
• INTRA: inside the molecule

  INTER: between 2 molecules
• INTRAMOLECULAR FORCES

  IONIC BOND

  • complete transfer of valence electron between atoms; occurs between metal and a nonmetal.

  COVALENT BOND

  • sharing of pair of electrons by atoms to gain more stability; occurs between nonmetals.

  METALLIC BOND

  • sharing of free electrons among a structure of positively charged ions; occurs between m
• INTRAMOLECULAR FORCES: COVALENT

  BONDS

  Polar covalent bond

  • shared electronsbetween atoms are not equally shared.

  Nonpolar covalent bond

  • Equal sharing of electrons between atoms.
• INTERMOLCULAR FORCES

  van der Waals Forces

  Keesom

  • attraction between 2 permanent dipoles
  • alignment or orientation effect
  • when one dipole interacts with another dipole, the partially positive side of the one molecule interacts with and orients the partially negative side of another molecule.
• INTERMOLCULAR FORCES

  van der Waals Forces

  DEBYE

  • attraction between a permanent dipole and transient dipole
  • induction effect
  • a permanent dipole can induce polarizability of a nonpolar molecule by disturbing the even distribution of charge. The partially positive side of a permanent dipole will attract the electrons of a nonpolar molecule to induce a dipole
• INTERMOLCULAR FORCES

  van der Waals Forces

  LONDON

  • temporary attraction between 2 induced or transient dipoles
  • dispersion effect
  • there are instances when electrons of a nonpolar molecule will accumulate to one side of the molecule thereby inducing a dipole. Surrounding nonpolar molecules are then influenced by the induced dipole.
• van der Waals Forces

  • LONDON
  • DEBYE
  • Keesom
• INTERMOLCULAR FORCES

  ION-DIPOLE FORCE

  • attraction of polar molecules to positively and/or negatively charged ions
• Ion-dipole Forces Examples

  Sodium Chloride (NaCl) Dissolved in Water (H,°)
• INTERMOLCULAR FORCES

  ION-INDUCED DIPOLE FORCE

  • attraction of nopolar molecules to positively and/or negatively charged ions. The charged ions will disturb the distribution of charge in a nonpolar compound thereby inducing a temporary dipole.
• INTERMOLCULAR FORCES

  HYDROGEN BONDING

  • electrostatic attraction of H with highly electronegative atoms (F, O, N). Hydrogen bonds are formed between polar molecules