Organic Chemistry

• Alcohols contain an OH group attached to a carbon atom.
• Alkanes are saturated hydrocarbons, while alkenes have double bonds between two carbons.
• The number of isomers increases with the length of the carbon chain.
• Esters have a COOR functional group on both ends of their molecules.
• An atom consists of a single, central, massive, positively charged nucleus surrounded by electrons.
• Covalent bonding occurs when atoms share pairs of electrons.
• Atoms can be represented as spherical balls or as dots arranged around a circle representing the nucleus.
• A molecule is made up of atoms joined together chemically
• Ionic bonding involves electrostatic attraction between oppositely charged ions.
• Metals tend to lose electrons to form positive ions (cations), while non-metals gain electrons to form negative ions (anions).
• Molecular geometry refers to the arrangement of atoms around a central atom in a molecule or polyatomic ion.
• Metals lose electrons to form cations (positive ions), while non-metals gain electrons to form anions (negative ions).
• Ionic compounds consist of positive and negative ions held together by electrostatic forces.
• Molecular formulae show the relative numbers of different types of atoms present in a compound.
• Molecular geometry refers to how atoms are arranged relative to one another within a molecule.
• Ionic bonds occur between oppositely charged ions (atoms).
• The number of protons determines an element's identity, while the number of neutrons does not affect it.
• Lewis structures show how valence electrons are shared among atoms in a molecule or ion.
• The number of valence electrons determines whether an element will act as a metal, non-metal, or metalloid.
• Covalent bonds are formed when two atoms share one or more pairs of electrons.
• Organic Chemistry

  The Chemistry of the Compounds of Carbon
• An understanding of organic chemistry must begin with an understanding of molecular structure
• Atom

  Consists of a single, central, massive, positively charged nucleus surrounded by electrons
• Atomic Number (Z)

  The number of protons in the nucleus
• Proton

  Positively Charged
• Electron

  Carries an equal but opposite negative charge
• Positively Charged Nucleus

  • Surrounded by electrons arranged in concentric Shells or Energy Levels
  • The maximum no. Of electrons each shell can accommodate is equal to 2n^2
• Subshell

  Substructure within the major shell; region of space within an electron shell that contains electrons that have the same energy
• Types of Subshells

  • Subshell s = 2 electrons
  • Subshell p = 6 electrons
  • Subshell d = 10 electrons
  • Subshell f = 14 electrons
• Electron Orbitals

  Region of space within an electron shell that contains electrons that have the same energy
• Pauli Exclusion Principle

  Two electrons may occupy the same orbital only when they have opposite, or "paired", spins
• S Orbital

  • Spherically symmetrical
  • Boundary Surface – A surface that captures a high proportion of the electron density
• P Orbital

  • Double-lobed, with a region of high electron density on each side of the nucleus
• D Orbital

  • Has its lobes arranged in a slightly more complicated pattern and labeled accordingly
• Electronic Configuration

  The arrangement of electrons in the orbitals of an atom
• Valence Shell/Electron

  Outermost shell of electrons; determines the chemical behaviour of an atom
• The Group VIIIA possess 8 electrons in their valence shell; they are said to have a complete octet of electrons. These elements are known as Noble Gases. They are characterized by an extremely stable "closed-shell" electron configuration and are very unreactive
• Chemical Bond

  Attractive force between atoms in a compound
• Ionic Bond

  • One type of a chemical bond, is the force of electrostatic attraction between oppositely charged species (ions)
  • Electrons are transferred from one atom to another
  • Very common in inorganic compounds, but rare in organic ones
• Cations

  Ions that are positively charged