CH 1 Bonding and Molecular Structure Flashcards
organic chemistry
the chemistry of compounds that contain the element carbon
chemistry
the study of matter and energy associated with its physical and chemical changes
valence electron
an electron in the outer shell of an atom which can combine with other atoms to form molecules
octet rule
the tendency of atoms to prefer to have eight electrons in the valence shell.
resonance theory
a theory by which the actual normal state of a molecule is represented not by a single valence-bond structure but by a combination of several alternative distinct structures
orbital
a particle description of the quantum state of an electron (or other particle) orbiting the nucleus of an atom; no more that 2 electrons can coexist in a single orbital because of the Pauli exclusion principle
Pauli Exclusion Principle
states no two electrons can have the identical quantum mechanical state in the same atom
Hesenberg Uncertainty Principle
the scientific principle stating that it is impossible to determine with perfect accuracy both the position and momentum of a particle at any given point in time
VSERP Model (valence shell electron pair repulsion)
a model used to predict the geometry of molecules based on minimizind the electrostatic repulsion of a molecule’s valencs electrons around a central atom
structure theory
the atoms in organic compounds can form a fixed number of bonds using their outer most shell (valence) electrons
isomers
different compounds that have the same molecular formula
constitutional isomers
different compounds that have the same molecular formula but differ in their connectivity
ionic bond
a attractive force between oppositely charged ions usually involving a metal and a nonmetal
covalent bonds
form by sharing electrons usually involving nonmetals; they melt lower than ionic compounds; some covalent bonds have ionic tendencies
molecules
are composed of atome joined exclusively or predominantly by covalent bonds
atomic orbital
the region of space where one or two electrons of an isolated atom are likely to be found
molecular orbital (MO)
represents the region of space where one or two electrons of a molecule are likely to be found
cis-trans isomerism
diastereomers that differ in their stereochemistry at adjacent atoms of a double bond or on different atoms of a ring; cis groups are on the same side of a double bond or ring; trans groups are on opposite sides of a double bond or ring
dash structural formulas
indicate tha way in which the atoms are attached to each other and are not representations of the actual shapes of the molecule
condensed structural formulas
all of the hydrogen atoms that are attached to a particular carbon are usually written immediately after the carbon
bond-line formula
shows the carbon skeleton of a molecule with lines
