Organic Chemistry Lecture

• Carbon - is known to form a seemingly unlimited number of compounds
• vital force theory: organic compounds are only found in living organisms and could not be synthesized from inorganic material.
• Jons Jacob Berzelius - made the vital force theory
• Frederich wohler - proved that organic compounds can be synthesized
• organic compounds comprise almost 90% of all known compunds
• catenation - tetravalency of carbon, tendency to form multiple bonds and isomerism
• Catenation - self-linking of atoms of an element to create chains and rings.
• isomerism - the existence of molecules that have the same numbers of the same kinds of atoms but differ in chemical and physical properties.
• isomerism - the existence of molecules that have the same numbers of the same kinds of atoms but differ in chemical and physical properties.
• organic compounds are characterized by the presence of carbon atoms while inorganic doesn't have any.
• organic compounds exist in the form of solid, liquids, and gases while inorganic compounds exist as solids
• inorganic compounds are soluble in water while organic compounds are insoluble
• organic compounds form covalent bonds while inorganic compounds form ionic bonds
• inorganic compounds are good conductors of heat and electricity while organic compounds are poor conductors
• organic compounds cannot make salts while inorganic can make salts
• inorganic compounds have high rate of reaction while organic compounds have slow rate of reaction
• ionic bond - formed through electrostatic attraction between two oppositely charged ions
• ionic bond - formed between a cation and an anion
• covalent bond - bond in which one or more pairs of electrons are shared by two atoms
• covalent compounds - compounds that are held together mainly by covalent bonds
• nonpolar covalent - the bonding electrons are shared equally between the two bonding atoms
• polar covalent - the electrons are shared between two bonding atoms, but unequally, with the electrons spending more time around the more electronegative atom
• single bond - two atoms share one electron pair
• double bond - two atoms share two electron pair
• triple bond - two atoms share three electron pair
• metallic bond - in metals, all atoms lose their valence electrons which form electronic cloud, which attracts the nucleus of neighboring atoms
• hydrogen bonding - electrostatic force of attraction between highly electronegative atom and partially positive hydrogen atom
• Covalent bond - the number of bonds that an atom can form can often be predicted from the number of electrons needed to reach an octet (eight valence electrons)
• valence electrons - the electrons in the outermost shell of an atom
• hydrogen is an element that is an exception to the octet rule.
• electronegativity - a measure of the tendency of an atom to attract electrons towards itself.
• flourine - element with the highest electronegativity with a value of 4.0
• ionic forces - strong electrostatic forces of attraction between oppositely charged ions
• ionic interaction by Colombus law - the force increases with charge and decreases as the distance between ions increases.
• hydrogen bonding - occurs in molecules containing the highly electronegative elements (F, O, or N) directly bond to hydrogen
• van der waals dipole-dipole interactions - other groups beside can be involved in polar covalent bonding with strongly electronegative atoms
• van der waals dispersion forces -the weakest intermoelcular forces of all. these represent the attraction between instantaneous dipoles in a molecule
• polarizability - term used to describe how readily atoms can form these instantaneous dipoles.
• Lewis structure - a representation of covalent bonding in which shared electron pairs are shown either as lines or as pairs of dots between two atoms, and lone pairs are shown as pairs of dots on individual atoms
• octet rule - an atom other than hydrogen tends to form bonds until it is sorrounded by eight valence electrons