Organic Chemistry

Fundamental particles of nature that cannot be broken down or destroyed.  Displayed on periodic table of elements.

Smallest amount of an element that can exist.

• Protons - p+ (in the nucleus)
• Neutrons - n⁰ (in the nucleus)
• Electrons e-

model for the atom.  shows electrons occupying different energy levels within the atom.  These different energy levels are called shells.

Hold between zero to two electrons.  have a shell # and subshell designation

Ex: 2s, 3p, 5d orbitals

region where occupying electrons fall into 's' type orbitals

region where occupying electrons fall into 'p' type orbitals

shows electrons occupying subshells at various possible energy levels.

• Ground state carbon: 1s²2s²2p²
• Ground state sodium: 1s²2s²2p⁶3s¹

electrons existing within the top energy shell on an atom

shows valence electrons as dots about an element.

elements lying to the left of the metalloids on the periodic table

elements lying to the right of the metalloids on the periodic table

charged particles.  formed by either gaining or losing electrons to become negatively or positively charged particles

positive ions

negative ions

a bond between cations and anions formed by an electrostatic attraction between particles of opposite charge.

a compound held together through only ionic bonds.

Ex: NaCl

a bond formed between atoms through the overlapping of orbitals to share valence electrons

a compound held together through only covalent bonds.

Ex: CO2

a method to predict the shapes of molecules and bond angles formed with designation of three atoms.

a bonding atom or lone pair of electrons used in VSEPR theory

the ability of an atom to attract electrons to itself in a chemical bond.  scale runs 0-4.0

a bond formed through the uneven sharing of electrons resulting in a positive and negative region between bonding atoms.

a bond formed through the even sharing of electrons with no resulting positive or negative regions between bonding atoms.

a molecule that is electrically unsymmetrical causing it to be oppositely charged in different regions

a molecule that is electrically symmetrical.  the centers of positive and negative charge will coincide.

a mathematical method to assign charge to atoms in covalent compounds.

valence electrons - 1/2 shared electrons - electrons in lone pairs

add multipliers to chemicals in equations to show the ratios in which they are consumed and produced.  balanced equations will have conservation of mass.

a compound that acts as a proton donor. (H+ donor)

a compound that acts as a proton acceptor (H+ acceptor)

living things (biological origin: flora, forna, food, us)

an indefinable characteristic that separated living organisms and materials derived from living organisms from inanimate inorganic matter

geological origin: minerals, rock, sea, air

huge field of chemistry.  more than 30 million compounds to date

carbon atoms can bond strongly to almost all other elements in the periodic table.

carbon atoms can form long carbon - carbon chains or rings with itself to give a stable carbon skeleton.  a single carbon skeleton gives rise to many possible organic compounds.

compounds made only from the elements carbon and hydrogen

Ex: CH₄, C₂H₆, C₂H₂

compounds that contain the maximum number of hydrogen atoms per the number of carbon present.

C_nH_2n+2

Ex: C₂H₆

compounds that do not contain the maximum number of hydrogen atoms per the number of carbon present.  will have a double or triple bond.

Ex: C₂H₂

saturated hydrocarbons which contain only carbon-carbon single bonds

shows all atoms and bonds present in the molecule

shows groups of atoms about each carbon in an individual chain

shows individual carbon atoms as intersections or endpoints of line segments.  all hydrogen atoms are assumed in a line-bond structure

• 1. odorless or mild odor, colorless and tasteless.
• 2. non-polar molecules
• 3. for liquids, density range is from 0.6-0.8 (g/mL)
• 4. not water soluble. (like dissolves like)
• 5. attracted to each other through London Dispersion Forces
• 6. as molecular weight increases, their melting and boiling points also increase
• 7. flammable (combustion reaction)
• 8. limited reactivity

an intermolecular forces of attraction caused by the formation of temporary dipoles

physical properties resemble that of fats and oils (saturated and big)

different compounds with the same formula

molecules with the same formula and connectivity of atoms but different spatial arrangement allowed through free rotation.  (alkanes possess free rotation along their carbon - carbon axis)

molecules with the same formula but a different connectivity of atoms or bonding arrangement.  (cannot simply rotate into each other as with conformational isomers)

molecules with the same formula but different connectivity of their carbon framework

different bonding groups of atoms attached along a carbon backbone.

molecules with the same formula and connectivity of atoms but different spatial arrangement which are locked or permanent.  (this arrangement cannot be changed without breaking chemical bonds)

non-superimposable mirror image molecules which contain chiral center

a molecule that is electrically unsymmetrical causing it to be oppositely charged at two points.  only applies to convalently bonded atoms.

CH₄

CH₃CH₃

CH₃CH₂CH₃

CH₃CH₂CH₂CH₃

CH₃CH₂CH₂CH₂CH₃

CH₃CH₂CH₂CH₂CH₂CH₃

CH₃CH₂CH₂CH₂CH₂CH₂CH₃

CH₃CH₂CH₂CH₂CH₂CH₂CH₂CH₃

CH₃CH₂CH₂CH₂CH₂CH₂CH₂CH₂CH₃

CH₃CH₂CH₂CH₂CH₂CH₂CH₂CH₂CH₂CH₃

a class of organic compound where one or more alkane-hydrogen atoms has been replaced with a group 7A halogen.  Halogens can be: F, Cl, Br, or I.

• 1. moderately polar
• 2. good solvents and aerosol propellants
• 3. CFC's (used in refrigerator and air conditioner)
• 4. non-toxic, non-flammable, non-corrosive
• 5. can damage earth's ozone layer