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Bonding and Molecular Structure
A set of flashcards that help students review terms and content on Bonding and the Molecular Structure of compounds.
41
Organic Chemistry
Undergraduate 2
01/15/2013

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Term
anion
Definition
a negatively charged ion; an ion that contains more electrons than protons
Term
antibonding molecular orbital
Definition
results when two orbitals of the opposite phase overlap
Term
atomic orbital
Definition
the region of space where one or two electrons of an isolated atom are likely to be found
Term
aufbau principle
Definition
rule for electron configurations that states orbitals should be filled starting with the lowest energy orbital first
Term
bonding molecular orbital
Definition
results when two orbitals of the same phase overlap; a molecular orbital that usually contains the bonding electrons
Term
bond-line formula
Definition
a forumla that shows the carbon skeleton of a molecule with lines; the number of hydrogens used to complete each carbon's valence shell are assumed, but not depicted; other atoms (O, Cl, N, etc.) and hydrogens bonded to those atoms are written
Term
cation
Definition
a positively charged ion; an ion that contains more protons than electrons
Term
condensed structural formulas
Definition
a depiction of a molecule where the hydrogens attached to a carbon are written immediately after that carbon, all covalent bonds are usually omitted but atoms are written in the order of bonding to depict connectivity
Term
constitutional isomers
Definition
different compound that have the same molecular formula, but differ in the sequence in which their atoms are bonded
Term
covalent bonds
Definition
bond formed by the sharing of electrons by two atoms with similar electronegativities
Term
curved arrows
Definition
arrows used to show the movement of electrons pairs
Term
dash structural formulas
Definition
structual depiction in which atoms symbols are drawn and a line or "dash" represents pairs of bonding electrons; show connectivity but do not show geometry
Term
degenerate orbitals
Definition
orbitals of equal energy; such as the three 2p orbitals
Term
electron
Definition
negatively charged atomic particle; resides outside of the nucleus
Term
electronegativity
Definition
a measure of the ability of an atom to attract electrons
Term
formal charge
Definition
the difference between the number of electrons assigned to an atom in a molecule and the number of electrons it has in its non-bonded state.
Term
Heisenberg uncertainty principle
Definition
a principle that states we cannot simultaneously know both the position and momentum of an electron
Term
Hund's rule
Definition
when filling orbitals of equal energy, add one electron to each orbital with their spins unpaired until each orbital contains one electron. Then add additional electrons to fill the orbitals so that spins are paired.
Term
ionic bond
Definition
an attractive force between oppositely charged ions
Term
isomers
Definition
different compound that have the same molecular formula
Term
isotope
Definition
atoms that have the same atomic number, but differ in the number of neutrons in the nucleus
Term
lewis structure
Definition
a structural formula that displays bonded electrons between two atoms as a line, and nonbonding electrons as dots
Term
molecular orbital
Definition
represents the region of space where one or two electrons of a molecule are likely to be found; the number of molecular orbitals always equals the number of atomic orbitals that were combined
Term
molecules
Definition
compounds whose atoms are joined primarily or exclusively by covalent bonds
Term
neutron
Definition
neutral atomic particle; resides in the nucleus of an atom
Term
octet rule
Definition
the tendancy of an atom to achieve a configuration where its valence shell contains eight electrons
Term
orbital
Definition
region of space where the probability of finding an electron is high
Term
orbital hybridization
Definition
approach that involves combining individual atomic orbitals (s and p) to obtain new orbitals to use for bonding; new orbitals have, in varying proportions, the properties of the original orbitals taken separately
Term
Pauli exclusion Principle
Definition
a maximum of two electrons may be placed in each orbital, but only when the spins of the electrons are paired
Term
pi bond
Definition
a bond formed when the electrons occupy a bonding pi molecular orbital; electron density of the pi bond is centered above and below the sigma bond axis; only occur when there are two or more bonds between the same two atoms
Term
pi molecular orbital
Definition
a molecular orbital formed when parallel p orbitals on adjacent atoms overlap
Term
proton
Definition
positively charged atomic particle; resides in the nucleus of an atom
Term
resonance contributor
Definition
(resonance structure) lewis structures that differ from each other only in the position of electrons
Term
resonance theory
Definition
whenever a molecule can be depicted by two or more valid lewis structures that differ only in the placement of electrons
Term
salts
Definition
ionic compounds
Term
sigma bond
Definition
a single bond between two atoms; bond formed when eletrons occupy the bonding sigma orbital formed by the end-to-end overlap of atomic (or hybrid) orbitals on adjacent atoms; has circular symmetry when viewed along the bond axis
Term
sigma orbital
Definition
molecular orbital formed by the end-on overlap of orbitals (or lobes of orbitals) on adjacent atoms
Term
three-dimensional forumla
Definition
depicts the correct geometry of an sp3 hybridized atom using dash and wedge bonds to show perspective
Term
valence
Definition
the number of times an atom commonly bonds in a molecule to give a formal charge of 0 for that element
Term
valence electrons
Definition
electrons that reside in the valence shell; involved in bonding
Term
valence shell
Definition
the outermost electron shell
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